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id="toc-Biological_sources" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Biological_sources"> <div class="vector-toc-text"> 5.2 Biological sources </div> </a> <ul id="toc-Biological_sources-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Extraterrestrial" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Extraterrestrial"> <div class="vector-toc-text"> 5.3 Extraterrestrial </div> </a> <ul id="toc-Extraterrestrial-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Geology" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Geology"> <div class="vector-toc-text"> 6 Geology </div> </a> <button aria-controls="toc-Geology-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Geology subsection </button> <ul id="toc-Geology-sublist" class="vector-toc-list"> <li id="toc-Carbonate_compensation_depth" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Carbonate_compensation_depth"> <div class="vector-toc-text"> 6.1 Carbonate compensation depth </div> </a> <ul id="toc-Carbonate_compensation_depth-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Role_in_taphonomy" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Role_in_taphonomy"> <div class="vector-toc-text"> 6.2 Role in taphonomy </div> </a> <ul id="toc-Role_in_taphonomy-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Uses" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Uses"> <div class="vector-toc-text"> 7 Uses </div> </a> <button aria-controls="toc-Uses-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Uses subsection </button> <ul id="toc-Uses-sublist" class="vector-toc-list"> <li id="toc-Construction" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Construction"> <div class="vector-toc-text"> 7.1 Construction </div> </a> <ul id="toc-Construction-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Health_and_diet" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Health_and_diet"> <div class="vector-toc-text"> 7.2 Health and diet </div> </a> <ul id="toc-Health_and_diet-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Agriculture_and_aquaculture" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Agriculture_and_aquaculture"> <div class="vector-toc-text"> 7.3 Agriculture and aquaculture </div> </a> <ul id="toc-Agriculture_and_aquaculture-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Household_cleaning" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Household_cleaning"> <div class="vector-toc-text"> 7.4 Household cleaning </div> </a> <ul id="toc-Household_cleaning-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Pollution_mitigation" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Pollution_mitigation"> <div class="vector-toc-text"> 7.5 Pollution mitigation </div> </a> <ul id="toc-Pollution_mitigation-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Plastics" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Plastics"> <div class="vector-toc-text"> 7.6 Plastics </div> </a> <ul id="toc-Plastics-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Calcination_equilibrium" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Calcination_equilibrium"> <div class="vector-toc-text"> 8 Calcination equilibrium </div> </a> <ul id="toc-Calcination_equilibrium-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Solubility" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Solubility"> <div class="vector-toc-text"> 9 Solubility </div> </a> <button aria-controls="toc-Solubility-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Solubility subsection </button> <ul id="toc-Solubility-sublist" class="vector-toc-list"> <li id="toc-With_varying_CO2_pressure" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#With_varying_CO2_pressure"> <div class="vector-toc-text"> 9.1 With varying CO2 pressure </div> </a> <ul id="toc-With_varying_CO2_pressure-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-With_varying_pH,_temperature_and_salinity:_CaCO3_scaling_in_swimming_pools" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#With_varying_pH,_temperature_and_salinity:_CaCO3_scaling_in_swimming_pools"> <div class="vector-toc-text"> 9.2 With varying pH, temperature and salinity: CaCO3 scaling in swimming pools </div> </a> <ul id="toc-With_varying_pH,_temperature_and_salinity:_CaCO3_scaling_in_swimming_pools-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Solubility_in_a_strong_or_weak_acid_solution" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Solubility_in_a_strong_or_weak_acid_solution"> <div class="vector-toc-text"> 9.3 Solubility in a strong or weak acid solution </div> </a> <ul id="toc-Solubility_in_a_strong_or_weak_acid_solution-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> 10 See also </div> </a> <ul id="toc-See_also-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> 11 References </div> </a> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> 12 External links </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" title="Table of Contents" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" > Toggle the table of contents </label> <div class="vector-dropdown-content"> <div id="vector-page-titlebar-toc-unpinned-container" class="vector-unpinned-container"> </div> </div> </div> </nav> <h1 id="firstHeading" class="firstHeading mw-first-heading">Calcium carbonate</h1> <div id="p-lang-btn" class="vector-dropdown mw-portlet mw-portlet-lang" > <input type="checkbox" id="p-lang-btn-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-p-lang-btn" class="vector-dropdown-checkbox mw-interlanguage-selector" aria-label="Go to an article in another language. Available in 77 languages" > <label id="p-lang-btn-label" for="p-lang-btn-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--action-progressive mw-portlet-lang-heading-77" aria-hidden="true" > 77 languages </label> <div class="vector-dropdown-content"> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li class="interlanguage-link interwiki-af mw-list-item"><a href="https://af.wikipedia.org/wiki/Kalsiumkarbonaat" title="Kalsiumkarbonaat – Afrikaans" lang="af" hreflang="af" data-title="Kalsiumkarbonaat" data-language-autonym="Afrikaans" data-language-local-name="Afrikaans" class="interlanguage-link-target">Afrikaans</a></li><li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D9%83%D8%B1%D8%A8%D9%88%D9%86%D8%A7%D8%AA_%D8%A7%D9%84%D9%83%D8%A7%D9%84%D8%B3%D9%8A%D9%88%D9%85" title="كربونات الكالسيوم – Arabic" lang="ar" hreflang="ar" data-title="كربونات الكالسيوم" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target">العربية</a></li><li class="interlanguage-link interwiki-an mw-list-item"><a href="https://an.wikipedia.org/wiki/Carbonato_calcico" title="Carbonato calcico – Aragonese" lang="an" hreflang="an" data-title="Carbonato calcico" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target">Aragonés</a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Carbonatu_de_calciu" title="Carbonatu de calciu – Asturian" lang="ast" hreflang="ast" data-title="Carbonatu de calciu" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target">Asturianu</a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/Kalsium_karbonat" title="Kalsium karbonat – Azerbaijani" lang="az" hreflang="az" data-title="Kalsium karbonat" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target">Azərbaycanca</a></li><li class="interlanguage-link interwiki-azb mw-list-item"><a href="https://azb.wikipedia.org/wiki/%DA%A9%D9%84%D8%B3%DB%8C%D9%88%D9%85_%DA%A9%D8%B1%D8%A8%D9%88%D9%86%D8%A7%D8%AA" title="کلسیوم کربونات – South Azerbaijani" lang="azb" hreflang="azb" data-title="کلسیوم کربونات" data-language-autonym="تۆرکجه" data-language-local-name="South Azerbaijani" class="interlanguage-link-target">تۆرکجه</a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%95%E0%A7%8D%E0%A6%AF%E0%A6%BE%E0%A6%B2%E0%A6%B8%E0%A6%BF%E0%A6%AF%E0%A6%BC%E0%A6%BE%E0%A6%AE_%E0%A6%95%E0%A6%BE%E0%A6%B0%E0%A7%8D%E0%A6%AC%E0%A6%A8%E0%A7%87%E0%A6%9F" title="ক্যালসিয়াম কার্বনেট – Bangla" lang="bn" hreflang="bn" data-title="ক্যালসিয়াম কার্বনেট" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target">বাংলা</a></li><li class="interlanguage-link interwiki-zh-min-nan mw-list-item"><a href="https://zh-min-nan.wikipedia.org/wiki/Tho%C3%A0%E2%81%BF-sng_kh%C4%81-l%C3%BA-si%C3%BAm" title="Thoàⁿ-sng khā-lú-siúm – Minnan" lang="nan" hreflang="nan" data-title="Thoàⁿ-sng khā-lú-siúm" data-language-autonym="閩南語 / Bân-lâm-gú" data-language-local-name="Minnan" class="interlanguage-link-target">閩南語 / Bân-lâm-gú</a></li><li class="interlanguage-link interwiki-ba mw-list-item"><a href="https://ba.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%8C%D1%86%D0%B8%D0%B9_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82%D1%8B" title="Кальций карбонаты – Bashkir" lang="ba" hreflang="ba" data-title="Кальций карбонаты" data-language-autonym="Башҡортса" data-language-local-name="Bashkir" class="interlanguage-link-target">Башҡортса</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%86%D0%B8%D0%B5%D0%B2_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82" title="Калциев карбонат – Bulgarian" lang="bg" hreflang="bg" data-title="Калциев карбонат" data-language-autonym="Български" data-language-local-name="Bulgarian" class="interlanguage-link-target">Български</a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Kalcij-karbonat" title="Kalcij-karbonat – Bosnian" lang="bs" hreflang="bs" data-title="Kalcij-karbonat" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target">Bosanski</a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Carbonat_de_calci" title="Carbonat de calci – Catalan" lang="ca" hreflang="ca" data-title="Carbonat de calci" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target">Català</a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/Uhli%C4%8Ditan_v%C3%A1penat%C3%BD" title="Uhličitan vápenatý – Czech" lang="cs" hreflang="cs" data-title="Uhličitan vápenatý" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target">Čeština</a></li><li class="interlanguage-link interwiki-cy mw-list-item"><a href="https://cy.wikipedia.org/wiki/Calsiwm_carbonad" title="Calsiwm carbonad – Welsh" lang="cy" hreflang="cy" data-title="Calsiwm carbonad" data-language-autonym="Cymraeg" data-language-local-name="Welsh" class="interlanguage-link-target">Cymraeg</a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Calciumcarbonat" title="Calciumcarbonat – Danish" lang="da" hreflang="da" data-title="Calciumcarbonat" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target">Dansk</a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Calciumcarbonat" title="Calciumcarbonat – German" lang="de" hreflang="de" data-title="Calciumcarbonat" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target">Deutsch</a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Kaltsiumkarbonaat" title="Kaltsiumkarbonaat – Estonian" lang="et" hreflang="et" data-title="Kaltsiumkarbonaat" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target">Eesti</a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%91%CE%BD%CE%B8%CF%81%CE%B1%CE%BA%CE%B9%CE%BA%CF%8C_%CE%B1%CF%83%CE%B2%CE%AD%CF%83%CF%84%CE%B9%CE%BF" title="Ανθρακικό ασβέστιο – Greek" lang="el" hreflang="el" data-title="Ανθρακικό ασβέστιο" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target">Ελληνικά</a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Carbonato_de_calcio" title="Carbonato de calcio – Spanish" lang="es" hreflang="es" data-title="Carbonato de calcio" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target">Español</a></li><li class="interlanguage-link interwiki-eo mw-list-item"><a href="https://eo.wikipedia.org/wiki/Kalcia_karbonato" title="Kalcia karbonato – Esperanto" lang="eo" hreflang="eo" data-title="Kalcia karbonato" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target">Esperanto</a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Kaltzio_karbonato" title="Kaltzio karbonato – Basque" lang="eu" hreflang="eu" data-title="Kaltzio karbonato" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target">Euskara</a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%DA%A9%D9%84%D8%B3%DB%8C%D9%85_%DA%A9%D8%B1%D8%A8%D9%86%D8%A7%D8%AA" title="کلسیم کربنات – Persian" lang="fa" hreflang="fa" data-title="کلسیم کربنات" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target">فارسی</a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Carbonate_de_calcium" title="Carbonate de calcium – French" lang="fr" hreflang="fr" data-title="Carbonate de calcium" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target">Français</a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Carb%C3%B3n%C3%A1it_chailciam" title="Carbónáit chailciam – Irish" lang="ga" hreflang="ga" data-title="Carbónáit chailciam" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target">Gaeilge</a></li><li class="interlanguage-link interwiki-gv mw-list-item"><a href="https://gv.wikipedia.org/wiki/Carbonaid_chelkium" title="Carbonaid chelkium – Manx" lang="gv" hreflang="gv" data-title="Carbonaid chelkium" data-language-autonym="Gaelg" data-language-local-name="Manx" class="interlanguage-link-target">Gaelg</a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Carbonato_de_calcio" title="Carbonato de calcio – Galician" lang="gl" hreflang="gl" data-title="Carbonato de calcio" data-language-autonym="Galego" data-language-local-name="Galician" class="interlanguage-link-target">Galego</a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%ED%83%84%EC%82%B0_%EC%B9%BC%EC%8A%98" title="탄산 칼슘 – Korean" lang="ko" hreflang="ko" data-title="탄산 칼슘" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%BF%D5%A1%D5%AC%D6%81%D5%AB%D5%B8%D6%82%D5%B4%D5%AB_%D5%AF%D5%A1%D6%80%D5%A2%D5%B8%D5%B6%D5%A1%D5%BF" title="Կալցիումի կարբոնատ – Armenian" lang="hy" hreflang="hy" data-title="Կալցիումի կարբոնատ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target">Հայերեն</a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%95%E0%A5%88%E0%A4%B2%E0%A5%8D%E0%A4%B8%E0%A4%BF%E0%A4%AF%E0%A4%AE_%E0%A4%95%E0%A4%BE%E0%A4%B0%E0%A5%8D%E0%A4%AC%E0%A5%8B%E0%A4%A8%E0%A5%87%E0%A4%9F" title="कैल्सियम कार्बोनेट – Hindi" lang="hi" hreflang="hi" data-title="कैल्सियम कार्बोनेट" data-language-autonym="हिन्दी" data-language-local-name="Hindi" class="interlanguage-link-target">हिन्दी</a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Kalcijev_karbonat" title="Kalcijev karbonat – Croatian" lang="hr" hreflang="hr" data-title="Kalcijev karbonat" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target">Hrvatski</a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Kalsium_karbonat" title="Kalsium karbonat – Indonesian" lang="id" hreflang="id" data-title="Kalsium karbonat" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target">Bahasa Indonesia</a></li><li class="interlanguage-link interwiki-is mw-list-item"><a href="https://is.wikipedia.org/wiki/Kals%C3%ADumkarb%C3%B3nat" title="Kalsíumkarbónat – Icelandic" lang="is" hreflang="is" data-title="Kalsíumkarbónat" data-language-autonym="Íslenska" data-language-local-name="Icelandic" class="interlanguage-link-target">Íslenska</a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Carbonato_di_calcio" title="Carbonato di calcio – Italian" lang="it" hreflang="it" data-title="Carbonato di calcio" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target">Italiano</a></li><li class="interlanguage-link interwiki-he mw-list-item"><a href="https://he.wikipedia.org/wiki/%D7%A1%D7%99%D7%93%D7%9F_%D7%A4%D7%97%D7%9E%D7%AA%D7%99" title="סידן פחמתי – Hebrew" lang="he" hreflang="he" data-title="סידן פחמתי" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target">עברית</a></li><li class="interlanguage-link interwiki-jv mw-list-item"><a href="https://jv.wikipedia.org/wiki/Kalsium_karbonat" title="Kalsium karbonat – Javanese" lang="jv" hreflang="jv" data-title="Kalsium karbonat" data-language-autonym="Jawa" data-language-local-name="Javanese" class="interlanguage-link-target">Jawa</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%8C%D1%86%D0%B8%D0%B9_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82%D1%8B" title="Кальций карбонаты – Kazakh" lang="kk" hreflang="kk" data-title="Кальций карбонаты" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target">Қазақша</a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%8C%D1%86%D0%B8%D0%B9_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82%D1%8B" title="Кальций карбонаты – Kyrgyz" lang="ky" hreflang="ky" data-title="Кальций карбонаты" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target">Кыргызча</a></li><li class="interlanguage-link interwiki-la mw-list-item"><a href="https://la.wikipedia.org/wiki/Carbonatum_calcii" title="Carbonatum calcii – Latin" lang="la" hreflang="la" data-title="Carbonatum calcii" data-language-autonym="Latina" data-language-local-name="Latin" class="interlanguage-link-target">Latina</a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Kalcija_karbon%C4%81ts" title="Kalcija karbonāts – Latvian" lang="lv" hreflang="lv" data-title="Kalcija karbonāts" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target">Latviešu</a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Kalcio_karbonatas" title="Kalcio karbonatas – Lithuanian" lang="lt" hreflang="lt" data-title="Kalcio karbonatas" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target">Lietuvių</a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Kalcium-karbon%C3%A1t" title="Kalcium-karbonát – Hungarian" lang="hu" hreflang="hu" data-title="Kalcium-karbonát" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target">Magyar</a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%86%D0%B8%D1%83%D0%BC_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82" title="Калциум карбонат – Macedonian" lang="mk" hreflang="mk" data-title="Калциум карбонат" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target">Македонски</a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%95%E0%B4%BE%E0%B5%BD%E0%B4%B8%E0%B5%8D%E0%B4%AF%E0%B4%82_%E0%B4%95%E0%B4%BE%E0%B5%BC%E0%B4%AC%E0%B4%A3%E0%B5%87%E0%B4%B1%E0%B5%8D%E0%B4%B1%E0%B5%8D" title="കാൽസ്യം കാർബണേറ്റ് – Malayalam" lang="ml" hreflang="ml" data-title="കാൽസ്യം കാർബണേറ്റ്" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target">മലയാളം</a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%95%E0%A5%85%E0%A4%B2%E0%A5%8D%E0%A4%B6%E0%A4%BF%E0%A4%AF%E0%A4%AE_%E0%A4%95%E0%A4%BE%E0%A4%B0%E0%A5%8D%E0%A4%AC%E0%A5%8B%E0%A4%A8%E0%A5%87%E0%A4%9F" title="कॅल्शियम कार्बोनेट – Marathi" lang="mr" hreflang="mr" data-title="कॅल्शियम कार्बोनेट" data-language-autonym="मराठी" data-language-local-name="Marathi" class="interlanguage-link-target">मराठी</a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Kalsium_karbonat" title="Kalsium karbonat – Malay" lang="ms" hreflang="ms" data-title="Kalsium karbonat" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target">Bahasa Melayu</a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Calciumcarbonaat" title="Calciumcarbonaat – Dutch" lang="nl" hreflang="nl" data-title="Calciumcarbonaat" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target">Nederlands</a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E7%82%AD%E9%85%B8%E3%82%AB%E3%83%AB%E3%82%B7%E3%82%A6%E3%83%A0" title="炭酸カルシウム – Japanese" lang="ja" hreflang="ja" data-title="炭酸カルシウム" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target">日本語</a></li><li class="interlanguage-link interwiki-frr mw-list-item"><a href="https://frr.wikipedia.org/wiki/Kaltsiumkarbonaat" title="Kaltsiumkarbonaat – Northern Frisian" lang="frr" hreflang="frr" data-title="Kaltsiumkarbonaat" data-language-autonym="Nordfriisk" data-language-local-name="Northern Frisian" class="interlanguage-link-target">Nordfriisk</a></li><li class="interlanguage-link interwiki-no mw-list-item"><a href="https://no.wikipedia.org/wiki/Kalsiumkarbonat" title="Kalsiumkarbonat – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Kalsiumkarbonat" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target">Norsk bokmål</a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Kalsiumkarbonat" title="Kalsiumkarbonat – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Kalsiumkarbonat" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target">Norsk nynorsk</a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/Carbonat_de_calci" title="Carbonat de calci – Occitan" lang="oc" hreflang="oc" data-title="Carbonat de calci" data-language-autonym="Occitan" data-language-local-name="Occitan" class="interlanguage-link-target">Occitan</a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Kalsiy_karbonat" title="Kalsiy karbonat – Uzbek" lang="uz" hreflang="uz" data-title="Kalsiy karbonat" data-language-autonym="Oʻzbekcha / ўзбекча" data-language-local-name="Uzbek" class="interlanguage-link-target">Oʻzbekcha / ўзбекча</a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/W%C4%99glan_wapnia" title="Węglan wapnia – Polish" lang="pl" hreflang="pl" data-title="Węglan wapnia" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target">Polski</a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Carbonato_de_c%C3%A1lcio" title="Carbonato de cálcio – Portuguese" lang="pt" hreflang="pt" data-title="Carbonato de cálcio" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Carbonat_de_calciu" title="Carbonat de calciu – Romanian" lang="ro" hreflang="ro" data-title="Carbonat de calciu" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target">Română</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%9A%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82_%D0%BA%D0%B0%D0%BB%D1%8C%D1%86%D0%B8%D1%8F" title="Карбонат кальция – Russian" lang="ru" hreflang="ru" data-title="Карбонат кальция" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target">Русский</a></li><li class="interlanguage-link interwiki-sah mw-list-item"><a href="https://sah.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%8C%D1%86%D0%B8%D0%B9_%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D0%B0%D1%82%D0%B0" title="Кальций карбонаата – Yakut" lang="sah" hreflang="sah" data-title="Кальций карбонаата" data-language-autonym="Саха тыла" data-language-local-name="Yakut" class="interlanguage-link-target">Саха тыла</a></li><li class="interlanguage-link interwiki-sco mw-list-item"><a href="https://sco.wikipedia.org/wiki/Calcium_carbonate" title="Calcium carbonate – Scots" lang="sco" hreflang="sco" data-title="Calcium carbonate" data-language-autonym="Scots" data-language-local-name="Scots" class="interlanguage-link-target">Scots</a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B6%9A%E0%B7%90%E0%B6%BD%E0%B7%8A%E0%B7%83%E0%B7%92%E0%B6%BA%E0%B6%B8%E0%B7%8A_%E0%B6%9A%E0%B7%8F%E0%B6%B6%E0%B6%B1%E0%B7%9A%E0%B6%A7%E0%B7%8A" title="කැල්සියම් කාබනේට් – Sinhala" lang="si" hreflang="si" data-title="කැල්සියම් කාබනේට්" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target">සිංහල</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Calcium_carbonate" title="Calcium carbonate – Simple English" lang="en-simple" hreflang="en-simple" data-title="Calcium carbonate" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target">Simple English</a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Uhli%C4%8Ditan_v%C3%A1penat%C3%BD" title="Uhličitan vápenatý – Slovak" lang="sk" hreflang="sk" data-title="Uhličitan vápenatý" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target">Slovenčina</a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/Kalcijev_karbonat" title="Kalcijev karbonat – Slovenian" lang="sl" hreflang="sl" data-title="Kalcijev karbonat" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target">Slovenščina</a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%9A%D0%B0%D0%BB%D1%86%D0%B8%D1%98%D1%83%D0%BC-%D0%BA%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82" title="Калцијум-карбонат – Serbian" lang="sr" hreflang="sr" data-title="Калцијум-карбонат" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target">Српски / srpski</a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Kalcijum_karbonat" title="Kalcijum karbonat – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Kalcijum karbonat" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target">Srpskohrvatski / српскохрватски</a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Kalsiumkarbonaatti" title="Kalsiumkarbonaatti – Finnish" lang="fi" hreflang="fi" data-title="Kalsiumkarbonaatti" data-language-autonym="Suomi" data-language-local-name="Finnish" class="interlanguage-link-target">Suomi</a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Kalciumkarbonat" title="Kalciumkarbonat – Swedish" lang="sv" hreflang="sv" data-title="Kalciumkarbonat" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target">Svenska</a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%95%E0%AE%BE%E0%AE%B2%E0%AF%8D%E0%AE%9A%E0%AE%BF%E0%AE%AF%E0%AE%AE%E0%AF%8D_%E0%AE%95%E0%AE%BE%E0%AE%B0%E0%AF%8D%E0%AE%AA%E0%AE%A9%E0%AF%87%E0%AE%9F%E0%AF%8D%E0%AE%9F%E0%AF%81" title="கால்சியம் கார்பனேட்டு – Tamil" lang="ta" hreflang="ta" data-title="கால்சியம் கார்பனேட்டு" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target">தமிழ்</a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B9%81%E0%B8%84%E0%B8%A5%E0%B9%80%E0%B8%8B%E0%B8%B5%E0%B8%A2%E0%B8%A1%E0%B8%84%E0%B8%B2%E0%B8%A3%E0%B9%8C%E0%B8%9A%E0%B8%AD%E0%B9%80%E0%B8%99%E0%B8%95" title="แคลเซียมคาร์บอเนต – Thai" lang="th" hreflang="th" data-title="แคลเซียมคาร์บอเนต" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target">ไทย</a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/Kalsiyum_karbonat" title="Kalsiyum karbonat – Turkish" lang="tr" hreflang="tr" data-title="Kalsiyum karbonat" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target">Türkçe</a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%9A%D0%B0%D1%80%D0%B1%D0%BE%D0%BD%D0%B0%D1%82_%D0%BA%D0%B0%D0%BB%D1%8C%D1%86%D1%96%D1%8E" title="Карбонат кальцію – Ukrainian" lang="uk" hreflang="uk" data-title="Карбонат кальцію" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target">Українська</a></li><li class="interlanguage-link interwiki-ur mw-list-item"><a href="https://ur.wikipedia.org/wiki/%DA%A9%DB%8C%D9%84%D8%B4%DB%8C%D9%85_%DA%A9%D8%A7%D8%B1%D8%A8%D9%86%DB%8C%D9%B9" title="کیلشیم کاربنیٹ – Urdu" lang="ur" hreflang="ur" data-title="کیلشیم کاربنیٹ" data-language-autonym="اردو" data-language-local-name="Urdu" class="interlanguage-link-target">اردو</a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Calci_carbonat" title="Calci carbonat – Vietnamese" lang="vi" hreflang="vi" data-title="Calci carbonat" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target">Tiếng Việt</a></li><li class="interlanguage-link interwiki-zh-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E7%A2%B3%E9%85%B8%E9%88%A3" title="碳酸鈣 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="碳酸鈣" data-language-autonym="文言" data-language-local-name="Literary Chinese" class="interlanguage-link-target">文言</a></li><li class="interlanguage-link interwiki-war mw-list-item"><a href="https://war.wikipedia.org/wiki/Calcium_carbonate" title="Calcium carbonate – Waray" lang="war" hreflang="war" data-title="Calcium carbonate" data-language-autonym="Winaray" data-language-local-name="Waray" class="interlanguage-link-target">Winaray</a></li><li class="interlanguage-link interwiki-wuu mw-list-item"><a href="https://wuu.wikipedia.org/wiki/%E7%A2%B3%E9%85%B8%E9%92%99" title="碳酸钙 – Wu" lang="wuu" hreflang="wuu" data-title="碳酸钙" data-language-autonym="吴语" data-language-local-name="Wu" class="interlanguage-link-target">吴语</a></li><li class="interlanguage-link interwiki-zh-yue mw-list-item"><a href="https://zh-yue.wikipedia.org/wiki/%E7%A2%B3%E9%85%B8%E9%88%A3" title="碳酸鈣 – Cantonese" lang="yue" hreflang="yue" data-title="碳酸鈣" data-language-autonym="粵語" data-language-local-name="Cantonese" class="interlanguage-link-target">粵語</a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a 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dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> <style data-mw-deduplicate="TemplateStyles:r1268415487">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}</style> <table class="infobox ib-chembox"> <caption>Calcium carbonate </caption> <tbody><tr> <td colspan="2" style="text-align:center; padding:2px;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Calcium_carbonate.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d3/Calcium_carbonate.png/220px-Calcium_carbonate.png" decoding="async" width="220" height="103" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d3/Calcium_carbonate.png/330px-Calcium_carbonate.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d3/Calcium_carbonate.png/440px-Calcium_carbonate.png 2x" data-file-width="1554" data-file-height="729" /></a><figcaption></figcaption></figure> </td></tr> <tr> <td colspan="2" style="text-align:center; padding:2px;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Calcium_carbonate.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Calcium_carbonate.jpg/220px-Calcium_carbonate.jpg" decoding="async" width="220" height="214" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Calcium_carbonate.jpg/330px-Calcium_carbonate.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/0/04/Calcium_carbonate.jpg 2x" data-file-width="401" data-file-height="390" /></a><figcaption></figcaption></figure> </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Names </th></tr> <tr> <td colspan="2" style="text-align:left;"><a href="/wiki/Chemical_nomenclature" title="Chemical nomenclature">IUPAC name</a> <div style="max-width:22em; word-wrap:break-word; padding-left:1.7em;">Calcium carbonate</div> </td></tr> <tr> <td colspan="2" style="text-align:left;">Other names <div style="max-width:22em; word-wrap:break-word; padding-left:1.7em;"><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style><div class="plainlist"><ul><li><a href="/wiki/Aragonite" title="Aragonite">Aragonite</a></li><li><a href="/wiki/Calcite" title="Calcite">Calcite</a></li><li><a href="/wiki/Chalk" title="Chalk">Chalk</a></li><li><a href="/wiki/Lime_(material)" title="Lime (material)">Lime</a></li><li><a href="/wiki/Limestone" title="Limestone">Limestone</a></li><li><a href="/wiki/Marble" title="Marble">Marble</a></li><li><a href="/wiki/Oyster" title="Oyster">Oystershell</a></li><li><a href="/wiki/Pearl" title="Pearl">Pearl</a></li></ul></div></div> </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Identifiers </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/CAS_Registry_Number" title="CAS Registry Number">CAS Number</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=471-34-1">471-34-1</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">3D model (<a href="/wiki/JSmol" class="mw-redirect" title="JSmol">JSmol</a>)</div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://chemapps.stolaf.edu/jmol/jmol.php?model=%5BCa%2B2%5D.%5BO-%5DC%28%5BO-%5D%29%3DO">Interactive image</a></li><li><a rel="nofollow" class="external text" href="https://chemapps.stolaf.edu/jmol/jmol.php?model=C%28%3DO%29%28%5BO-%5D%29%5BO-%5D.%5BCa%2B2%5D">Interactive image</a></li></ul></div> </td></tr> <tr> <td><a href="/wiki/ChEBI" title="ChEBI">ChEBI</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chebi/searchId.do?chebiId=3311">CHEBI:3311</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</li></ul></div> </td></tr> <tr> <td><a href="/wiki/ChEMBL" title="ChEMBL">ChEMBL</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chembl/explore/compound/ChEMBL1200539">ChEMBL1200539</a> <img alt="☒" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" />N</li></ul></div> </td></tr> <tr> <td><a href="/wiki/ChemSpider" title="ChemSpider">ChemSpider</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://www.chemspider.com/Chemical-Structure.9708.html">9708</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</li></ul></div> </td></tr> <tr> <td><a href="/wiki/DrugBank" title="DrugBank">DrugBank</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://www.drugbank.ca/drugs/DB06724">DB06724</a></li></ul></div> </td></tr> <tr> <td><a href="/wiki/ECHA_InfoCard" class="mw-redirect" title="ECHA InfoCard">ECHA InfoCard</a> </td> <td><a rel="nofollow" class="external text" href="https://echa.europa.eu/substance-information/-/substanceinfo/100.006.765">100.006.765</a> <a href="https://www.wikidata.org/wiki/Q23767#P2566" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a> </td></tr> <tr> <td><a href="/wiki/European_Community_number" title="European Community number">EC Number</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>207-439-9</li></ul></div> </td></tr> <tr> <td><a href="/wiki/E_number" title="E number">E number</a> </td> <td>E170 <a href="/wiki/E_number#E100–E199" title="E number">(colours)</a> </td></tr> <tr> <td><a href="/wiki/KEGG" title="KEGG">KEGG</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://www.kegg.jp/entry/D00932">D00932</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/PubChem" title="PubChem">PubChem</a> <abbr title="Compound ID">CID</abbr></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://pubchem.ncbi.nlm.nih.gov/compound/10112">10112</a></li></ul></div> </td></tr> <tr> <td><a href="/wiki/RTECS" class="mw-redirect" title="RTECS">RTECS number</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>FF9335000</li></ul></div> </td></tr> <tr> <td><a href="/wiki/Unique_Ingredient_Identifier" title="Unique Ingredient Identifier">UNII</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://precision.fda.gov/uniisearch/srs/unii/H0G9379FGK">H0G9379FGK</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/CompTox_Chemicals_Dashboard" title="CompTox Chemicals Dashboard">CompTox Dashboard</a> (<abbr title="U.S. Environmental Protection Agency">EPA</abbr>)</div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a rel="nofollow" class="external text" href="https://comptox.epa.gov/dashboard/chemical/details/DTXSID3036238">DTXSID3036238</a> <a href="https://www.wikidata.org/wiki/Q23767#P3117" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></li></ul></div> </td></tr> <tr> <td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;"> <div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal;"><div><a href="/wiki/International_Chemical_Identifier" title="International Chemical Identifier">InChI</a></div></div> <ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1S/CH2O3.Ca/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: VTYYLEPIZMXCLO-UHFFFAOYSA-L <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y</div></div></li><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1/CH2O3.Ca/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2</div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: VTYYLEPIZMXCLO-NUQVWONBAS</div></div></li></ul> </div> </td></tr> <tr> <td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;"> <div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal;"><div><a href="/wiki/Simplified_molecular-input_line-entry_system" class="mw-redirect" title="Simplified molecular-input line-entry system">SMILES</a></div></div> <ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.6em; word-wrap:break-word; text-indent:-1.5em; text-align:left; font-size:97%; line-height:120%;">[Ca+2].[O-]C([O-])=O</div></li><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.6em; word-wrap:break-word; text-indent:-1.5em; text-align:left; font-size:97%; line-height:120%;">C(=O)([O-])[O-].[Ca+2]</div></li></ul> </div> </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Properties </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Chemical_formula" title="Chemical formula">Chemical formula</a></div> </td> <td><style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style>CaCO3 </td></tr> <tr> <td><a href="/wiki/Molar_mass" title="Molar mass">Molar mass</a> </td> <td>100.0869 g/mol </td></tr> <tr> <td>Appearance </td> <td>Fine white powder or colorless crystals; chalky taste </td></tr> <tr> <td><a href="/wiki/Odor" title="Odor">Odor</a> </td> <td>odorless </td></tr> <tr> <td><a href="/wiki/Density" title="Density">Density</a> </td> <td>2.711 g/cm3 (<a href="/wiki/Calcite" title="Calcite">calcite</a>) 2.83 g/cm3 (<a href="/wiki/Aragonite" title="Aragonite">aragonite</a>) </td></tr> <tr> <td><a href="/wiki/Melting_point" title="Melting point">Melting point</a> </td> <td>1,339 °C (2,442 °F; 1,612 K) (calcite) 825 °C (1,517 °F; 1,098 K) (aragonite)<a href="#cite_note-4">[4]</a><a href="#cite_note-5">[5]</a> </td></tr> <tr> <td><a href="/wiki/Boiling_point" title="Boiling point">Boiling point</a> </td> <td><a href="/wiki/Chemical_decomposition" title="Chemical decomposition">decomposes</a> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Aqueous_solution" title="Aqueous solution">Solubility in water</a></div> </td> <td>0.013 g/L (25 °C)<a href="#cite_note-1">[1]</a><a href="#cite_note-2">[2]</a> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Solubility_equilibrium" title="Solubility equilibrium">Solubility product</a> (Ksp) </div> </td> <td>3.3×10−9<a href="#cite_note-3">[3]</a> </td></tr> <tr> <td><a href="/wiki/Solubility" title="Solubility">Solubility</a> in dilute acids </td> <td>soluble </td></tr> <tr> <td><a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">Acidity</a> (pKa) </td> <td>9.0 </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Magnetic_susceptibility" title="Magnetic susceptibility">Magnetic susceptibility</a> (χ)</div> </td> <td>−3.82×10−5 cm3/mol </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Refractive_index" title="Refractive index">Refractive index</a> (nD)</div> </td> <td>1.59 </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Structure </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Crystal_structure" title="Crystal structure">Crystal structure</a></div> </td> <td>Trigonal </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Space_group" title="Space group">Space group</a></div> </td> <td>32/m </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Thermochemistry </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Standard_molar_entropy" title="Standard molar entropy">Std molar entropy</a> (S⦵298)</div> </td> <td>93 J/(mol·K)<a href="#cite_note-b1-6">[6]</a> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Standard_enthalpy_change_of_formation" class="mw-redirect" title="Standard enthalpy change of formation">Std enthalpy of formation</a> (ΔfH⦵298)</div> </td> <td>−1207 kJ/mol<a href="#cite_note-b1-6">[6]</a> </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Pharmacology </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Anatomical_Therapeutic_Chemical_Classification_System" title="Anatomical Therapeutic Chemical Classification System">ATC code</a></div> </td> <td><a href="/wiki/ATC_code_A02" title="ATC code A02">A02AC01</a> (<a rel="nofollow" class="external text" href="https://www.whocc.no/atc_ddd_index/?code=A02AC01">WHO</a>) <a href="/wiki/ATC_code_A12" title="ATC code A12">A12AA04</a> (<a rel="nofollow" class="external text" href="https://www.whocc.no/atc_ddd_index/?code=A12AA04">WHO</a>) </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Hazards </th></tr> <tr> <td><a href="/wiki/NFPA_704" title="NFPA 704">NFPA 704</a> (fire diamond) </td> <td><style data-mw-deduplicate="TemplateStyles:r1170367383">.mw-parser-output .nfpa-704-diamond-ref{float:right;padding:1px;text-align:right}.mw-parser-output .nfpa-704-diamond-container{width:82px;font-family:sans-serif;margin:0 auto}.mw-parser-output .nfpa-704-diamond-container-ref{float:left;margin-left:1em}.mw-parser-output .nfpa-704-diamond-images{float:left;font-size:20px;text-align:center;position:relative;height:80px;width:80px;padding:1px}.mw-parser-output .nfpa-704-diamond-map{position:absolute;height:80px;width:80px}.mw-parser-output .nfpa-704-diamond .noresize{margin:0 auto}.mw-parser-output .nfpa-704-diamond-code{line-height:1em;text-align:center;position:absolute}.mw-parser-output .nfpa-704-diamond-code>a{color:black}.mw-parser-output .nfpa-704-diamond-blue{width:13px;top:31px;left:15px}.mw-parser-output .nfpa-704-diamond-red{width:12px;top:12px;left:35px}.mw-parser-output .nfpa-704-diamond-yellow{width:13px;top:31px;left:54px}.mw-parser-output .nfpa-704-diamond-white-image{position:relative;top:51px;left:0}.mw-parser-output .nfpa-704-diamond-white-text{vertical-align:middle;text-align:center;line-height:80%;position:absolute;top:52px}.mw-parser-output .nfpa-704-diamond-white-text a>span{position:absolute;color:black}.mw-parser-output .nfpa-704-diamond-white-wors{font-size:15px;width:23px;left:29px}.mw-parser-output .nfpa-704-diamond-white-wox{font-size:15px;font-stretch:condensed;width:21px;line-height:80%;top:-4px;left:29px}.mw-parser-output .nfpa-704-diamond-white-abcp{font-size:13.5px;font-stretch:condensed;width:28px;left:26px}.mw-parser-output .nfpa-704-diamond-white-ac{font-size:10px;width:30px;left:25px}.mw-parser-output .nfpa-704-diamond-white-strike{text-decoration:line-through}</style><div class="nfpa-704-diamond notheme"><div class="nfpa-704-diamond-container"><div class="nfpa-704-diamond-images nounderlines"> <div class="nfpa-704-diamond-map"><figure class="noresize" typeof="mw:File"><img alt="NFPA 704 four-colored diamond" src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/80px-NFPA_704.svg.png" decoding="async" width="80" height="80" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/120px-NFPA_704.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/160px-NFPA_704.svg.png 2x" data-file-width="512" data-file-height="512" usemap="#ImageMap_fbee98d65da2341e" /><map name="ImageMap_fbee98d65da2341e"><area href="/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chloride" title="Health 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chloride" /><area href="/wiki/NFPA_704#Red" shape="poly" coords="47,0,70,23,47,47,23,23" alt="Flammability 0: Will not burn. E.g. water" title="Flammability 0: Will not burn. E.g. water" /><area href="/wiki/NFPA_704#Yellow" shape="poly" coords="70,23,94,47,70,70,47,47" alt="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" /><area href="/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazards (white): no code" title="Special hazards (white): no code" /></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue"> <a href="/wiki/NFPA_704#Blue" title="NFPA 704">0</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-red"> <a href="/wiki/NFPA_704#Red" title="NFPA 704">0</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-yellow"> <a href="/wiki/NFPA_704#Yellow" title="NFPA 704">0</a></div></div></div></div> </td></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;color:inherit;">Lethal dose or concentration (LD, LC): </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">LD50 (<a href="/wiki/Lethal_dose#LD50" title="Lethal dose">median dose</a>)</div> </td> <td>6450 mg/kg (oral, rat) </td></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;color:inherit;"><a href="/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health">NIOSH</a> (US health exposure limits): </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Permissible_exposure_limit" title="Permissible exposure limit">PEL</a> (Permissible)</div> </td> <td>TWA 15 mg/m3 (total) TWA 5 mg/m3 (resp)<a href="#cite_note-7">[7]</a> </td></tr> <tr> <td><a href="/wiki/Safety_data_sheet" title="Safety data sheet">Safety data sheet</a> (SDS) </td> <td><a rel="nofollow" class="external text" href="http://www.inchem.org/documents/icsc/icsc/eics1193.htm">ICSC 1193</a> </td></tr> <tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Related compounds </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Other <a href="/wiki/Ion" title="Ion">anions</a></div> </td> <td><a href="/wiki/Calcium_bicarbonate" title="Calcium bicarbonate">Calcium bicarbonate</a> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Other <a href="/wiki/Ion" title="Ion">cations</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a href="/wiki/Beryllium_carbonate" title="Beryllium carbonate">Beryllium carbonate</a></li><li><a href="/wiki/Magnesium_carbonate" title="Magnesium carbonate">Magnesium carbonate</a></li><li><a href="/wiki/Strontium_carbonate" title="Strontium carbonate">Strontium carbonate</a></li><li><a href="/wiki/Barium_carbonate" title="Barium carbonate">Barium carbonate</a></li><li><a href="/wiki/Radium_carbonate" title="Radium carbonate">Radium carbonate</a></li><li><a href="/wiki/Zinc_carbonate" title="Zinc carbonate">Zinc carbonate</a></li><li><a href="/wiki/Otavite" title="Otavite">Cadmium carbonate</a></li><li><a href="/wiki/Lead(II)_carbonate" class="mw-redirect" title="Lead(II) carbonate">Lead(II) carbonate</a></li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Related compounds</div> </td> <td><a href="/wiki/Calcium_sulfate" title="Calcium sulfate">Calcium sulfate</a> </td></tr> <tr> <td colspan="2" style="text-align:left; background:#f8eaba; color:inherit; border:1px solid #a2a9b1;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Except where otherwise noted, data are given for materials in their <a href="/wiki/Standard_state" title="Standard state">standard state</a> (at 25 °C [77 °F], 100 kPa).</div> <div style="margin-top: 0.3em;"><div style="text-align:center;"><img alt="☒" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/12px-X_mark.svg.png" decoding="async" width="12" height="14" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/18px-X_mark.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/24px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" />N <a class="external text" href="https://en.wikipedia.org/w/index.php?title=Special:ComparePages&rev1=477003420&page2=Calcium+carbonate">verify</a> (<a href="/wiki/Wikipedia:WikiProject_Chemicals/Chembox_validation" title="Wikipedia:WikiProject Chemicals/Chembox validation">what is</a> <img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" />Y<img alt="☒" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" />N ?) </div></div> <div style="margin-top: 0.3em; text-align: center;"><a href="/wiki/Wikipedia:Chemical_infobox#References" title="Wikipedia:Chemical infobox">Infobox references</a></div> </td></tr> </tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Calcite.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/97/Calcite.png/220px-Calcite.png" decoding="async" width="220" height="269" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/97/Calcite.png/330px-Calcite.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/97/Calcite.png/440px-Calcite.png 2x" data-file-width="546" data-file-height="668" /></a><figcaption>Crystal structure of calcite</figcaption></figure> Calcium carbonate is a <a href="/wiki/Chemical_compound" title="Chemical compound">chemical compound</a> with the <a href="/wiki/Chemical_formula" title="Chemical formula">chemical formula</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Calcium" title="Calcium">Ca</a><a href="/wiki/Carbonate" title="Carbonate">CO3</a>. It is a common substance found in <a href="/wiki/Rock_(geology)" title="Rock (geology)">rocks</a> as the <a href="/wiki/Mineral" title="Mineral">minerals</a> <a href="/wiki/Calcite" title="Calcite">calcite</a> and <a href="/wiki/Aragonite" title="Aragonite">aragonite</a>, most notably in <a href="/wiki/Chalk" title="Chalk">chalk</a> and <a href="/wiki/Limestone" title="Limestone">limestone</a>, <a href="/wiki/Eggshell" title="Eggshell">eggshells</a>, <a href="/wiki/Gastropod_shell" title="Gastropod shell">gastropod shells</a>, <a href="/wiki/Shellfish" title="Shellfish">shellfish</a> skeletons and <a href="/wiki/Pearl" title="Pearl">pearls</a>. Materials containing much calcium carbonate or resembling it are described as <a href="/wiki/Calcareous" title="Calcareous">calcareous</a>. Calcium carbonate is the active ingredient in <a href="/wiki/Agricultural_lime" title="Agricultural lime">agricultural lime</a> and is produced when calcium <a href="/wiki/Ion" title="Ion">ions</a> in <a href="/wiki/Hard_water" title="Hard water">hard water</a> react with <a href="/wiki/Carbonate_ion" class="mw-redirect" title="Carbonate ion">carbonate ions</a> to form <a href="/wiki/Limescale" title="Limescale">limescale</a>. It has medical use as a <a href="/wiki/Calcium" title="Calcium">calcium</a> supplement or as an <a href="/wiki/Antacid" title="Antacid">antacid</a>, but excessive consumption can be hazardous and cause <a href="/wiki/Hypercalcemia" class="mw-redirect" title="Hypercalcemia">hypercalcemia</a> and digestive issues.<a href="#cite_note-jer15-8">[8]</a> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Chemistry">Chemistry</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=1" title="Edit section: Chemistry">edit</a>]</div> Calcium carbonate shares the typical properties of other <a href="/wiki/Carbonate" title="Carbonate">carbonates</a>. Notably it <ul><li>reacts with <a href="/wiki/Acid" title="Acid">acids</a>, releasing <a href="/wiki/Carbonic_acid" title="Carbonic acid">carbonic acid</a> which quickly disintegrates into <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> and <a href="/wiki/Water" title="Water">water</a>:</li></ul> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3(s) + 2 H+(aq) → Ca2+(aq) + CO2(g) + H2O(l)</dd></dl> <ul><li>releases carbon dioxide upon heating, called a <a href="/wiki/Thermal_decomposition" title="Thermal decomposition">thermal decomposition</a> reaction, or <a href="/wiki/Calcination" title="Calcination">calcination</a> (to above 840 °C in the case of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3), to form <a href="/wiki/Calcium_oxide" title="Calcium oxide">calcium oxide</a>, CaO, commonly called <a href="/wiki/Quicklime" class="mw-redirect" title="Quicklime">quicklime</a>, with reaction <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> 178 kJ/mol:</li></ul> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3(s) → CaO(s) + CO2(g)</dd></dl> <ul><li>reacts with gaseous hydrogen to form methane and water vapor plus solid calcium oxide or calcium hydroxide depending on temperature and product gas composition. Various metals including palladium and nickel are catalysts for the reaction.</li></ul> Calcium carbonate reacts with water that is saturated with carbon dioxide to form the soluble <a href="/wiki/Calcium_bicarbonate" title="Calcium bicarbonate">calcium bicarbonate</a>. <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3(s) + CO2(g) + H2O(l) → Ca(HCO3)2(aq)</dd></dl> This reaction is important in the <a href="/wiki/Erosion" title="Erosion">erosion</a> of <a href="/wiki/Carbonate_rock" title="Carbonate rock">carbonate rock</a>, forming <a href="/wiki/Cavern" class="mw-redirect" title="Cavern">caverns</a>, and leads to <a href="/wiki/Hard_water" title="Hard water">hard water</a> in many regions. An unusual form of calcium carbonate is the hexahydrate <a href="/wiki/Ikaite" title="Ikaite">ikaite</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3·6H2O. Ikaite is stable only below 8 °C. <div class="mw-heading mw-heading2"><h2 id="Preparation">Preparation</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=2" title="Edit section: Preparation">edit</a>]</div> The vast majority of calcium carbonate used in industry is extracted by mining or quarrying. Pure calcium carbonate (such as for food or pharmaceutical use), can be produced from a pure quarried source (usually <a href="/wiki/Marble" title="Marble">marble</a>). Alternatively, calcium carbonate is prepared from <a href="/wiki/Calcium_oxide" title="Calcium oxide">calcium oxide</a>. Water is added to give <a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">calcium hydroxide</a> then <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> is passed through this solution to <a href="/wiki/Precipitate" class="mw-redirect" title="Precipitate">precipitate</a> the desired calcium carbonate, referred to in the industry as precipitated calcium carbonate (PCC) This process is called <a href="/wiki/Carbonatation" title="Carbonatation">carbonatation</a>:<a href="#cite_note-PCC-9">[9]</a> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaO + H2O → Ca(OH)2</dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca(OH)2 + CO2 → CaCO3 + H2O</dd></dl> In a laboratory, calcium carbonate can easily be crystallized from <a href="/wiki/Calcium_chloride" title="Calcium chloride">calcium chloride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCl2), by placing an <a href="/wiki/Aqueous_solution" title="Aqueous solution">aqueous solution</a> of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCl2 in a <a href="/wiki/Desiccator" title="Desiccator">desiccator</a> alongside <a href="/wiki/Ammonium_carbonate" title="Ammonium carbonate">ammonium carbonate</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[NH4]2CO3.<a href="#cite_note-10">[10]</a> In the desiccator, ammonium carbonate is exposed to air and decomposes into <a href="/wiki/Ammonia" title="Ammonia">ammonia</a>, carbon dioxide, and <a href="/wiki/Water" title="Water">water</a>. The carbon dioxide then diffuses into the aqueous solution of calcium chloride, reacts with the calcium ions and the water, and forms calcium carbonate. <div class="mw-heading mw-heading2"><h2 id="Structure">Structure</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=3" title="Edit section: Structure">edit</a>]</div> The thermodynamically stable form of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 under normal conditions is <a href="/wiki/Hexagonal_crystal_family" title="Hexagonal crystal family">hexagonal</a> β-<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (the mineral <a href="/wiki/Calcite" title="Calcite">calcite</a>). Other forms can be prepared, the denser (2.83 g/cm3) <a href="/wiki/Orthorhombic" class="mw-redirect" title="Orthorhombic">orthorhombic</a> λ-<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (the mineral <a href="/wiki/Aragonite" title="Aragonite">aragonite</a>) and hexagonal μ-<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3, occurring as the mineral <a href="/wiki/Vaterite" title="Vaterite">vaterite</a>. The aragonite form can be prepared by precipitation at temperatures above 85 °C; the vaterite form can be prepared by precipitation at 60 °C. Calcite contains calcium atoms coordinated by six oxygen atoms; in aragonite they are coordinated by nine oxygen atoms.[<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">citation needed</a>] The vaterite structure is not fully understood.<a href="#cite_note-DemichelisRaiteri2013-11">[11]</a> <a href="/wiki/Magnesium_carbonate" title="Magnesium carbonate">Magnesium carbonate</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">MgCO3) has the calcite structure, whereas <a href="/wiki/Strontium_carbonate" title="Strontium carbonate">strontium carbonate</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SrCO3) and <a href="/wiki/Barium_carbonate" title="Barium carbonate">barium carbonate</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BaCO3) adopt the aragonite structure, reflecting their larger <a href="/wiki/Atomic_radius" title="Atomic radius">ionic radii</a>.[<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">citation needed</a>] <div class="mw-heading mw-heading2"><h2 id="Polymorphs">Polymorphs</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=4" title="Edit section: Polymorphs">edit</a>]</div> Calcium carbonate crystallizes in three <a href="/wiki/Anhydrous" title="Anhydrous">anhydrous</a> <a href="/wiki/Polymorphism_(materials_science)" class="mw-redirect" title="Polymorphism (materials science)">polymorphs</a>,<a href="#cite_note-12">[12]</a><a href="#cite_note-13">[13]</a> of which <a href="/wiki/Calcite" title="Calcite">calcite</a> is the thermodynamically most stable at room temperature, <a href="/wiki/Aragonite" title="Aragonite">aragonite</a> is only slightly less so, and <a href="/wiki/Vaterite" title="Vaterite">vaterite</a> is the least stable.<a href="#cite_note-Nahi-2022-14">[14]</a> <div class="mw-heading mw-heading3"><h3 id="Crystal_structure">Crystal structure</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=5" title="Edit section: Crystal structure">edit</a>]</div> The <a href="/wiki/Calcite" title="Calcite">calcite</a> crystal structure is <a href="/wiki/Trigonal" class="mw-redirect" title="Trigonal">trigonal</a>, with <a href="/wiki/Space_group" title="Space group">space group</a> R3c (No. 167 in the International Tables for Crystallography<a href="#cite_note-15">[15]</a>), and <a href="/wiki/Pearson_symbol" title="Pearson symbol">Pearson symbol</a> hR10.<a href="#cite_note-16">[16]</a> <a href="/wiki/Aragonite" title="Aragonite">Aragonite</a> is <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic</a>, with space group Pmcn (No 62), and Pearson Symbol oP20.<a href="#cite_note-17">[17]</a> <a href="/wiki/Vaterite" title="Vaterite">Vaterite</a> is composed of at least two different coexisting crystallographic structures. The major structure exhibits <a href="/wiki/Hexagonal_crystal_family" title="Hexagonal crystal family">hexagonal</a> symmetry in space group P63/mmc, the minor structure is still unknown.<a href="#cite_note-18">[18]</a> <div class="mw-heading mw-heading3"><h3 id="Crystallization">Crystallization</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=6" title="Edit section: Crystallization">edit</a>]</div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Calcite%2BAragonite.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/df/Calcite%2BAragonite.png/234px-Calcite%2BAragonite.png" decoding="async" width="234" height="185" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/df/Calcite%2BAragonite.png/351px-Calcite%2BAragonite.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/df/Calcite%2BAragonite.png/468px-Calcite%2BAragonite.png 2x" data-file-width="866" data-file-height="685" /></a><figcaption>Crystal structure of calcite and aragonite</figcaption></figure> All three polymorphs crystallize simultaneously from aqueous solutions under ambient conditions.<a href="#cite_note-Nahi-2022-14">[14]</a> In additive-free aqueous solutions, calcite forms easily as the major product, while aragonite appears only as a minor product. At high saturation, vaterite is typically the first phase precipitated, which is followed by a transformation of the vaterite to calcite.<a href="#cite_note-19">[19]</a> This behavior seems to follow <a href="/wiki/Ostwald%27s_rule" title="Ostwald's rule">Ostwald's rule</a>, in which the least stable polymorph crystallizes first, followed by the crystallization of different polymorphs via a sequence of increasingly stable phases.<a href="#cite_note-20">[20]</a> However, aragonite, whose stability lies between those of vaterite and calcite, seems to be the exception to this rule, as aragonite does not form as a precursor to calcite under ambient conditions.<a href="#cite_note-Nahi-2022-14">[14]</a> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Calcite%2BVaterite.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/99/Calcite%2BVaterite.png/220px-Calcite%2BVaterite.png" decoding="async" width="220" height="143" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/99/Calcite%2BVaterite.png/330px-Calcite%2BVaterite.png 1.5x, //upload.wikimedia.org/wikipedia/commons/9/99/Calcite%2BVaterite.png 2x" data-file-width="405" data-file-height="263" /></a><figcaption>Microscopic calcite and vaterite</figcaption></figure> Aragonite occurs in majority when the reaction conditions inhibit the formation of calcite and/or promote the nucleation of aragonite. For example, the formation of aragonite is promoted by the presence of magnesium ions,<a href="#cite_note-21">[21]</a> or by using proteins and peptides derived from biological calcium carbonate.<a href="#cite_note-22">[22]</a> Some polyamines such as <a href="/wiki/Cadaverine" title="Cadaverine">cadaverine</a> and <a href="/wiki/Polyethylenimine" title="Polyethylenimine">Poly(ethylene imine)</a> have been shown to facilitate the formation of aragonite over calcite.<a href="#cite_note-Nahi-2022-14">[14]</a> <div class="mw-heading mw-heading3"><h3 id="Selection_by_organisms">Selection by organisms</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=7" title="Edit section: Selection by organisms">edit</a>]</div> Organisms, such as <a href="/wiki/Mollusca" title="Mollusca">molluscs</a> and <a href="/wiki/Arthropod" title="Arthropod">arthropods</a>, have shown the ability to grow all three crystal polymorphs of calcium carbonate, mainly as protection (shells) and muscle attachments.<a href="#cite_note-23">[23]</a> Moreover, they exhibit a remarkable capability of phase selection over calcite and aragonite, and some organisms can switch between the two polymorphs. The ability of phase selection is usually attributed to the use of specific macromolecules or combinations of macromolecules by such organisms.<a href="#cite_note-24">[24]</a><a href="#cite_note-25">[25]</a><a href="#cite_note-26">[26]</a> <div class="mw-heading mw-heading2"><h2 id="Occurrence">Occurrence</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=8" title="Edit section: Occurrence">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Silfurberg.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/14/Silfurberg.jpg/220px-Silfurberg.jpg" decoding="async" width="220" height="180" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/14/Silfurberg.jpg/330px-Silfurberg.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/14/Silfurberg.jpg/440px-Silfurberg.jpg 2x" data-file-width="3000" data-file-height="2455" /></a><figcaption><a href="/wiki/Calcite" title="Calcite">Calcite</a> is the most stable <a href="/wiki/Polymorphism_(materials_science)" class="mw-redirect" title="Polymorphism (materials science)">polymorph</a> of calcium carbonate. It is transparent to opaque. A transparent variety called <a href="/wiki/Iceland_spar" title="Iceland spar">Iceland spar</a> (shown here) was used to create <a href="/wiki/Polarized_light" class="mw-redirect" title="Polarized light">polarized light</a> in the 19th century.<a href="#cite_note-Russell2008-27">[27]</a></figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Geological_sources">Geological sources</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=9" title="Edit section: Geological sources">edit</a>]</div> <a href="/wiki/Calcite" title="Calcite">Calcite</a>, <a href="/wiki/Aragonite" title="Aragonite">aragonite</a> and <a href="/wiki/Vaterite" title="Vaterite">vaterite</a> are pure calcium carbonate minerals. Industrially important source rocks which are predominantly calcium carbonate include <a href="/wiki/Limestone" title="Limestone">limestone</a>, <a href="/wiki/Chalk" title="Chalk">chalk</a>, <a href="/wiki/Marble" title="Marble">marble</a> and <a href="/wiki/Travertine" title="Travertine">travertine</a>. <div class="mw-heading mw-heading3"><h3 id="Biological_sources">Biological sources</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=10" title="Edit section: Biological sources">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Calcium_carbonate_chunks.JPG" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/50/Calcium_carbonate_chunks.JPG/220px-Calcium_carbonate_chunks.JPG" decoding="async" width="220" height="124" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/50/Calcium_carbonate_chunks.JPG/330px-Calcium_carbonate_chunks.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/50/Calcium_carbonate_chunks.JPG/440px-Calcium_carbonate_chunks.JPG 2x" data-file-width="1068" data-file-height="601" /></a><figcaption>Calcium carbonate chunks from <a href="/wiki/Clam" title="Clam">clamshell</a></figcaption></figure> <a href="/wiki/Eggshell" title="Eggshell">Eggshells</a>, <a href="/wiki/Snail" title="Snail">snail</a> shells and most <a href="/wiki/Seashell" title="Seashell">seashells</a> are predominantly calcium carbonate and can be used as industrial sources of that chemical.<a href="#cite_note-28">[28]</a> <a href="/wiki/Oyster" title="Oyster">Oyster</a> shells have enjoyed recent recognition as a source of dietary calcium, but are also a practical industrial source.<a href="#cite_note-29">[29]</a><a href="#cite_note-30">[30]</a> Dark <a href="/wiki/Green_vegetables" class="mw-redirect" title="Green vegetables">green vegetables</a> such as <a href="/wiki/Broccoli" title="Broccoli">broccoli</a> and <a href="/wiki/Kale" title="Kale">kale</a> contain dietarily significant amounts of calcium carbonate, but they are not practical as an industrial source.<a href="#cite_note-31">[31]</a> <a href="/wiki/Annelid" title="Annelid">Annelids</a> in the family <a href="/wiki/Lumbricidae" title="Lumbricidae">Lumbricidae</a>, earthworms, possess a regionalization of the digestive track called <a href="/w/index.php?title=Calciferous_glands&action=edit&redlink=1" class="new" title="Calciferous glands (page does not exist)">calciferous glands</a>, Kalkdrüsen, or glandes de Morren, that processes calcium and <a href="/wiki/Carbon_dioxide" title="Carbon dioxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2</a> into calcium carbonate, which is later excreted into the dirt.<a href="#cite_note-32">[32]</a> The function of these glands is unknown but is believed to serve as a <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 regulation mechanism within the animals' tissues.<a href="#cite_note-33">[33]</a> This process is ecologically significant, stabilizing the <a href="/wiki/Soil_pH" title="Soil pH">pH of acid soils</a>.<a href="#cite_note-34">[34]</a> <div class="mw-heading mw-heading3"><h3 id="Extraterrestrial">Extraterrestrial</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=11" title="Edit section: Extraterrestrial">edit</a>]</div> Beyond Earth, strong evidence suggests the presence of calcium carbonate on <a href="/wiki/Mars" title="Mars">Mars</a>. Signs of calcium carbonate have been detected at more than one location (notably at <a href="/wiki/Gusev_crater" class="mw-redirect" title="Gusev crater">Gusev</a> and <a href="/wiki/Huygens_(crater)" title="Huygens (crater)">Huygens</a> craters). This provides some evidence for the past presence of liquid water.<a href="#cite_note-35">[35]</a><a href="#cite_note-Clark2007-36">[36]</a> <div class="mw-heading mw-heading2"><h2 id="Geology">Geology</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=12" title="Edit section: Geology">edit</a>]</div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Rubaksa_tufa_plug.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/49/Rubaksa_tufa_plug.jpg/220px-Rubaksa_tufa_plug.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/49/Rubaksa_tufa_plug.jpg/330px-Rubaksa_tufa_plug.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/49/Rubaksa_tufa_plug.jpg/440px-Rubaksa_tufa_plug.jpg 2x" data-file-width="4128" data-file-height="3096" /></a><figcaption>Surface precipitation of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 as <a href="/wiki/Tufa" title="Tufa">tufa</a> in <a href="/wiki/Rubaksa" class="mw-redirect" title="Rubaksa">Rubaksa</a>, Ethiopia</figcaption></figure> Carbonate is found frequently in geologic settings and constitutes an enormous <a href="/wiki/Carbon_cycle" title="Carbon cycle">carbon reservoir</a>. Calcium carbonate occurs as <a href="/wiki/Aragonite" title="Aragonite">aragonite</a>, <a href="/wiki/Calcite" title="Calcite">calcite</a> and <a href="/wiki/Dolomite_(mineral)" title="Dolomite (mineral)">dolomite</a> as significant constituents of the <a href="/wiki/Calcium_cycle" title="Calcium cycle">calcium cycle</a>. The <a href="/wiki/Carbonate_mineral" title="Carbonate mineral">carbonate minerals</a> form the rock types: <a href="/wiki/Limestone" title="Limestone">limestone</a>, <a href="/wiki/Chalk" title="Chalk">chalk</a>, <a href="/wiki/Marble" title="Marble">marble</a>, <a href="/wiki/Travertine" title="Travertine">travertine</a>, <a href="/wiki/Tufa" title="Tufa">tufa</a>, and others. <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg/220px-Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg/330px-Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/18/Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg/440px-Water-of-Five-colored-Pond_Huanglong_Sichuan_China.jpg 2x" data-file-width="1920" data-file-height="1440" /></a><figcaption><a href="/wiki/Tufa" title="Tufa">Tufa</a> at <a href="/wiki/Huanglong_Scenic_and_Historic_Interest_Area" title="Huanglong Scenic and Historic Interest Area">Huanglong</a>, <a href="/wiki/Sichuan" title="Sichuan">Sichuan</a></figcaption></figure> In warm, clear tropical waters <a href="/wiki/Coral" title="Coral">corals</a> are more abundant than towards the poles where the waters are cold. Calcium carbonate contributors, including <a href="/wiki/Plankton" title="Plankton">plankton</a> (such as <a href="/wiki/Coccolith" title="Coccolith">coccoliths</a> and planktic <a href="/wiki/Foraminifera" title="Foraminifera">foraminifera</a>), <a href="/wiki/Coralline_algae" title="Coralline algae">coralline algae</a>, <a href="/wiki/Sea_sponge" class="mw-redirect" title="Sea sponge">sponges</a>, <a href="/wiki/Brachiopod" title="Brachiopod">brachiopods</a>, <a href="/wiki/Echinoderm" title="Echinoderm">echinoderms</a>, <a href="/wiki/Bryozoa" title="Bryozoa">bryozoa</a> and <a href="/wiki/Mollusc_shell" title="Mollusc shell">mollusks</a>, are typically found in shallow water environments where sunlight and filterable food are more abundant. Cold-water carbonates do exist at higher latitudes but have a very slow growth rate. The <a href="/wiki/Calcification" title="Calcification">calcification</a> processes are changed by <a href="/wiki/Ocean_acidification" title="Ocean acidification">ocean acidification</a>. Where the <a href="/wiki/Oceanic_crust" title="Oceanic crust">oceanic crust</a> is <a href="/wiki/Subduction" title="Subduction">subducted</a> under a <a href="/wiki/Continental_plate" class="mw-redirect" title="Continental plate">continental plate</a> sediments will be carried down to warmer zones in the <a href="/wiki/Asthenosphere" title="Asthenosphere">asthenosphere</a> and <a href="/wiki/Lithosphere" title="Lithosphere">lithosphere</a>. Under these conditions calcium carbonate decomposes to produce <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> which, along with other gases, give rise to explosive <a href="/wiki/Volcano" title="Volcano">volcanic eruptions</a>. <div class="mw-heading mw-heading3"><h3 id="Carbonate_compensation_depth">Carbonate compensation depth</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=13" title="Edit section: Carbonate compensation depth">edit</a>]</div> The <a href="/wiki/Carbonate_compensation_depth" title="Carbonate compensation depth">carbonate compensation depth</a> (CCD) is the point in the ocean where the rate of precipitation of calcium carbonate is balanced by the rate of dissolution due to the conditions present. Deep in the ocean, the temperature drops and pressure increases. Increasing pressure also increases the solubility of calcium carbonate. Calcium carbonate is unusual in that its solubility increases with decreasing temperature.<a href="#cite_note-weyl1959-37">[37]</a> The carbonate compensation depth ranges from 4,000 to 6,000 meters below sea level in modern oceans, and the various polymorphs (calcite, aragonite) have different compensation depths based on their stability.<a href="#cite_note-38">[38]</a> <div class="mw-heading mw-heading3"><h3 id="Role_in_taphonomy">Role in taphonomy</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=14" title="Edit section: Role in taphonomy">edit</a>]</div> Calcium carbonate can <a href="/wiki/Taphonomy" title="Taphonomy">preserve fossils</a> through <a href="/wiki/Permineralization" title="Permineralization">permineralization</a>. Most of the vertebrate fossils of the <a href="/wiki/Two_Medicine_Formation" title="Two Medicine Formation">Two Medicine Formation</a>—a <a href="/wiki/Geologic_formation" class="mw-redirect" title="Geologic formation">geologic formation</a> known for its <a href="/wiki/Duck-billed_dinosaur" class="mw-redirect" title="Duck-billed dinosaur">duck-billed dinosaur</a> eggs—are preserved by <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 permineralization.<a href="#cite_note-twoturn-39">[39]</a> This type of preservation conserves high levels of detail, even down to the microscopic level. However, it also leaves specimens vulnerable to <a href="/wiki/Weathering" title="Weathering">weathering</a> when exposed to the surface.<a href="#cite_note-twoturn-39">[39]</a> <a href="/wiki/Trilobite" title="Trilobite">Trilobite</a> populations were once thought to have composed the majority of aquatic life during the <a href="/wiki/Cambrian" title="Cambrian">Cambrian</a>, due to the fact that their calcium carbonate-rich shells were more easily preserved than those of other species,<a href="#cite_note-40">[40]</a> which had purely <a href="/wiki/Chitin" title="Chitin">chitinous</a> shells. <div class="mw-heading mw-heading2"><h2 id="Uses">Uses</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=15" title="Edit section: Uses">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Construction">Construction</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=16" title="Edit section: Construction">edit</a>]</div> The main use of calcium carbonate is in the construction industry, either as a building material, or limestone <a href="/wiki/Construction_aggregate" title="Construction aggregate">aggregate</a> for road building, as an ingredient of <a href="/wiki/Cement" title="Cement">cement</a>, or as the starting material for the preparation of <a href="/wiki/Slaked_lime" class="mw-redirect" title="Slaked lime">builders' lime</a> by burning in a <a href="/wiki/Kiln" title="Kiln">kiln</a>. However, because of weathering mainly caused by <a href="/wiki/Acid_rain" title="Acid rain">acid rain</a>,<a href="#cite_note-41">[41]</a> calcium carbonate (in limestone form) is no longer used for building purposes on its own, but only as a raw primary substance for building materials. Calcium carbonate is also used in the purification of <a href="/wiki/Iron" title="Iron">iron</a> from <a href="/wiki/Iron_ore" title="Iron ore">iron ore</a> in a <a href="/wiki/Blast_furnace" title="Blast furnace">blast furnace</a>. The carbonate is <a href="/wiki/Calcination" title="Calcination">calcined</a> in situ to give <a href="/wiki/Calcium_oxide" title="Calcium oxide">calcium oxide</a>, which forms a <a href="/wiki/Slag" title="Slag">slag</a> with various impurities present, and separates from the purified iron.<a href="#cite_note-42">[42]</a> In the <a href="/wiki/Oil_industry" class="mw-redirect" title="Oil industry">oil industry</a>, calcium carbonate is added to <a href="/wiki/Drilling_fluid" title="Drilling fluid">drilling fluids</a> as a formation-bridging and filtercake-sealing agent; it is also a weighting material which increases the density of drilling fluids to control the downhole pressure. Calcium carbonate is added to <a href="/wiki/Swimming_pool" title="Swimming pool">swimming pools</a>, as a <a href="/wiki/PH" title="PH">pH</a> corrector for maintaining <a href="/wiki/Alkalinity" title="Alkalinity">alkalinity</a> and offsetting the acidic properties of the <a href="/wiki/Disinfectant" title="Disinfectant">disinfectant</a> agent.<a href="#cite_note-43">[43]</a> It is also used as a raw material in the <a href="/wiki/Sugar_refining" class="mw-redirect" title="Sugar refining">refining of sugar</a> from <a href="/wiki/Sugar_beet" title="Sugar beet">sugar beet</a>; it is calcined in a kiln with <a href="/wiki/Anthracite" title="Anthracite">anthracite</a> to produce calcium oxide and carbon dioxide. This burnt lime is then slaked in fresh water to produce a calcium hydroxide <a href="/wiki/Suspension_(chemistry)" title="Suspension (chemistry)">suspension</a> for the precipitation of impurities in raw juice during <a href="/wiki/Carbonatation" title="Carbonatation">carbonatation</a>.<a href="#cite_note-44">[44]</a> Calcium carbonate in the form of <a href="/wiki/Chalk" title="Chalk">chalk</a> has traditionally been a major component of <a href="/wiki/Blackboard" title="Blackboard">blackboard</a> chalk. However, modern manufactured chalk is mostly <a href="/wiki/Gypsum" title="Gypsum">gypsum</a>, hydrated <a href="/wiki/Calcium_sulfate" title="Calcium sulfate">calcium sulfate</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaSO4·2H2O. Calcium carbonate is a main source for growing <a href="/wiki/Biorock" title="Biorock">biorock</a>. Precipitated calcium carbonate (PCC), pre-dispersed in <a href="/wiki/Slurry" title="Slurry">slurry</a> form, is a common filler material for <a href="/wiki/Latex_gloves" class="mw-redirect" title="Latex gloves">latex gloves</a> with the aim of achieving maximum saving in material and production costs.<a href="#cite_note-precaco3-45">[45]</a> Fine ground calcium carbonate (GCC) is an essential ingredient in the microporous film used in <a href="/wiki/Diapers" class="mw-redirect" title="Diapers">diapers</a> and some building films, as the pores are nucleated around the calcium carbonate particles during the manufacture of the film by biaxial stretching. GCC and PCC are used as a filler in <a href="/wiki/Paper" title="Paper">paper</a> because they are cheaper than <a href="/wiki/Wood_fiber" class="mw-redirect" title="Wood fiber">wood fiber</a>. Printing and writing paper can contain 10–20% calcium carbonate. In North America, calcium carbonate has begun to replace <a href="/wiki/Kaolinite" title="Kaolinite">kaolin</a> in the production of <a href="/wiki/Glossy_paper" class="mw-redirect" title="Glossy paper">glossy paper</a>. Europe has been practicing this as alkaline <a href="/wiki/Papermaking" title="Papermaking">papermaking</a> or acid-free papermaking for some decades. PCC used for paper filling and paper coatings is precipitated and prepared in a variety of shapes and sizes having characteristic narrow particle size distributions and equivalent spherical diameters of 0.4 to 3 micrometers.[<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">citation needed</a>] Calcium carbonate is widely used as an <a href="/wiki/Extender_(ink)" title="Extender (ink)">extender</a> in <a href="/wiki/Paint" title="Paint">paints</a>,<a href="#cite_note-reade-46">[46]</a> in particular <a href="/wiki/Gloss_and_matte_paint" class="mw-redirect" title="Gloss and matte paint">matte</a> <a href="/wiki/Emulsion_paint" class="mw-redirect" title="Emulsion paint">emulsion paint</a> where typically 30% by weight of the paint is either chalk or marble. It is also a popular filler in plastics.<a href="#cite_note-reade-46">[46]</a> Some typical examples include around 15–20% loading of chalk in <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">unplasticized polyvinyl chloride</a> (uPVC) <a href="/wiki/Rain_gutter" title="Rain gutter">drainpipes</a>, 5–15% loading of <a href="/wiki/Stearic_acid" title="Stearic acid">stearate</a>-coated chalk or marble in uPVC window profile. <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">PVC</a> cables can use calcium carbonate at loadings of up to 70 phr (parts per hundred parts of resin) to improve mechanical properties (tensile strength and elongation) and electrical properties (volume resistivity).[<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">citation needed</a>] <a href="/wiki/Polypropylene" title="Polypropylene">Polypropylene</a> compounds are often filled with calcium carbonate to increase rigidity, a requirement that becomes important at high usage temperatures.<a href="#cite_note-Imerys-47">[47]</a> Here the percentage is often 20–40%. It also routinely used as a filler in <a href="/wiki/Thermosetting_plastic" class="mw-redirect" title="Thermosetting plastic">thermosetting resins</a> (sheet and bulk molding compounds)<a href="#cite_note-Imerys-47">[47]</a> and has also been mixed with <a href="/wiki/Acrylonitrile_butadiene_styrene" title="Acrylonitrile butadiene styrene">ABS</a>, and other ingredients, to form some types of compression molded "clay" <a href="/wiki/Poker_chip" class="mw-redirect" title="Poker chip">poker chips</a>.<a href="#cite_note-48">[48]</a> Precipitated calcium carbonate, made by dropping <a href="/wiki/Calcium_oxide" title="Calcium oxide">calcium oxide</a> into water, is used by itself or with additives as a white paint, known as <a href="/wiki/Whitewash" title="Whitewash">whitewashing</a>.<a href="#cite_note-49">[49]</a><a href="#cite_note-JimohEtAl2017-50">[50]</a> Calcium carbonate is added to a wide range of trade and <a href="/wiki/Do_it_yourself" title="Do it yourself">do it yourself</a> adhesives, sealants, and decorating fillers.<a href="#cite_note-reade-46">[46]</a> Ceramic tile adhesives typically contain 70% to 80% limestone. Decorating crack fillers contain similar levels of marble or dolomite. It is also mixed with putty in setting <a href="/wiki/Stained_glass" title="Stained glass">stained glass</a> windows, and as a resist to prevent glass from sticking to kiln shelves when firing glazes and paints at high temperature.<a href="#cite_note-51">[51]</a><a href="#cite_note-52">[52]</a><a href="#cite_note-53">[53]</a><a href="#cite_note-54">[54]</a> In <a href="/wiki/Ceramic_glaze" title="Ceramic glaze">ceramic glaze</a> applications, calcium carbonate is known as whiting,<a href="#cite_note-reade-46">[46]</a> and is a common ingredient for many glazes in its white powdered form. When a glaze containing this material is fired in a kiln, the whiting acts as a <a href="/wiki/Ceramic_flux" title="Ceramic flux">flux</a> material in the glaze. Ground calcium carbonate is an <a href="/wiki/Abrasive" title="Abrasive">abrasive</a> (both as scouring powder and as an ingredient of household scouring creams), in particular in its calcite form, which has the relatively low hardness level of 3 on the <a href="/wiki/Mohs_scale_of_mineral_hardness" class="mw-redirect" title="Mohs scale of mineral hardness">Mohs scale</a>, and will therefore not scratch <a href="/wiki/Glass" title="Glass">glass</a> and most other <a href="/wiki/Ceramic" title="Ceramic">ceramics</a>, <a href="/wiki/Vitreous_enamel" title="Vitreous enamel">enamel</a>, <a href="/wiki/Bronze" title="Bronze">bronze</a>, <a href="/wiki/Iron" title="Iron">iron</a>, and <a href="/wiki/Steel" title="Steel">steel</a>, and have a moderate effect on softer metals like <a href="/wiki/Aluminium" title="Aluminium">aluminium</a> and <a href="/wiki/Copper" title="Copper">copper</a>. A paste made from calcium carbonate and <a href="/wiki/Deionized_water" class="mw-redirect" title="Deionized water">deionized water</a> can be used to clean <a href="/wiki/Tarnish" title="Tarnish">tarnish</a> on <a href="/wiki/Silver" title="Silver">silver</a>.<a href="#cite_note-Make_it_Shine-55">[55]</a> <div class="mw-heading mw-heading3"><h3 id="Health_and_diet">Health and diet</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=17" title="Edit section: Health and diet">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:500_mg_calcium_supplements_with_vitamin_D.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/2f/500_mg_calcium_supplements_with_vitamin_D.jpg/220px-500_mg_calcium_supplements_with_vitamin_D.jpg" decoding="async" width="220" height="147" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/2f/500_mg_calcium_supplements_with_vitamin_D.jpg/330px-500_mg_calcium_supplements_with_vitamin_D.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/2f/500_mg_calcium_supplements_with_vitamin_D.jpg/440px-500_mg_calcium_supplements_with_vitamin_D.jpg 2x" data-file-width="3185" data-file-height="2122" /></a><figcaption>500-milligram calcium supplements made from calcium carbonate</figcaption></figure> Calcium carbonate is widely used medicinally as an inexpensive dietary calcium supplement for <a href="/wiki/Antacid" title="Antacid">gastric antacid</a><a href="#cite_note-medline-56">[56]</a> (such as <a href="/wiki/Tums" title="Tums">Tums</a> and <a href="/wiki/Eno_(drug)" title="Eno (drug)">Eno</a>). It may be used as a <a href="/wiki/Phosphate_binder" title="Phosphate binder">phosphate binder</a> for the treatment of <a href="/wiki/Hyperphosphatemia" title="Hyperphosphatemia">hyperphosphatemia</a> (primarily in patients with <a href="/wiki/Chronic_kidney_failure" class="mw-redirect" title="Chronic kidney failure">chronic kidney failure</a>). It is used in the pharmaceutical industry as an inert <a href="/wiki/Excipient" title="Excipient">filler</a> for <a href="/wiki/Tablet_(pharmacy)" title="Tablet (pharmacy)">tablets</a> and other <a href="/wiki/Pharmaceuticals" class="mw-redirect" title="Pharmaceuticals">pharmaceuticals</a>.<a href="#cite_note-57">[57]</a> Calcium carbonate is used in the production of calcium oxide as well as toothpaste and has seen a resurgence as a food preservative and color retainer, when used in or with products such as organic apples.<a href="#cite_note-58">[58]</a> Calcium carbonate is used therapeutically as phosphate binder in patients on maintenance <a href="/wiki/Haemodialysis" class="mw-redirect" title="Haemodialysis">haemodialysis</a>. It is the most common form of phosphate binder prescribed, particularly in non-dialysis chronic kidney disease. Calcium carbonate is the most commonly used phosphate binder, but clinicians are increasingly prescribing the more expensive, non-calcium-based phosphate binders, particularly <a href="/wiki/Sevelamer" title="Sevelamer">sevelamer</a>. Excess calcium from supplements, fortified food, and high-calcium diets can cause <a href="/wiki/Milk-alkali_syndrome" title="Milk-alkali syndrome">milk-alkali syndrome</a>, which has serious toxicity and can be fatal. In 1915, <a href="/wiki/Bertram_Welton_Sippy" title="Bertram Welton Sippy">Bertram Sippy</a> introduced the "Sippy regimen" of hourly ingestion of milk and cream, and the gradual addition of eggs and cooked cereal, for 10 days, combined with alkaline powders, which provided symptomatic relief for peptic ulcer disease. Over the next several decades, the Sippy regimen resulted in <a href="/wiki/Kidney_failure" title="Kidney failure">kidney failure</a>, <a href="/wiki/Alkalosis" title="Alkalosis">alkalosis</a>, and <a href="/wiki/Hypercalcaemia" title="Hypercalcaemia">hypercalcaemia</a>, mostly in men with peptic ulcer disease. These adverse effects were reversed when the regimen stopped, but it was fatal in some patients with protracted vomiting. Milk-alkali syndrome declined in men after effective treatments for <a href="/wiki/Peptic_ulcer" class="mw-redirect" title="Peptic ulcer">peptic ulcer</a> disease arose. Since the 1990s it has been most frequently reported in women taking calcium supplements above the recommended range of 1.2 to 1.5 grams daily, for prevention and treatment of osteoporosis,<a href="#cite_note-pmid17483976-59">[59]</a><a href="#cite_note-pmid16702792-60">[60]</a> and is exacerbated by <a href="/wiki/Dehydration" title="Dehydration">dehydration</a>. Calcium has been added to over-the-counter products, which contributes to inadvertent excessive intake. Excessive calcium intake can lead to hypercalcemia, complications of which include vomiting, abdominal pain and altered mental status.<a href="#cite_note-61">[61]</a> As a <a href="/wiki/Food_additive" title="Food additive">food additive</a> it is designated <a href="/wiki/E_numbers" class="mw-redirect" title="E numbers">E170</a>,<a href="#cite_note-62">[62]</a> and it has an <a href="/wiki/International_Numbering_System_for_Food_Additives" title="International Numbering System for Food Additives">INS</a> number of 170. Used as an <a href="/wiki/Acidity_regulator" title="Acidity regulator">acidity regulator</a>, <a href="/wiki/Anticaking_agent" title="Anticaking agent">anticaking agent</a>, <a href="/wiki/Stabilizer_(food)" class="mw-redirect" title="Stabilizer (food)">stabilizer</a> or <a href="/wiki/Food_coloring" title="Food coloring">color</a> it is approved for usage in the EU,<a href="#cite_note-63">[63]</a> US<a href="#cite_note-64">[64]</a> and <a href="/wiki/Australia" title="Australia">Australia</a> and <a href="/wiki/New_Zealand" title="New Zealand">New Zealand</a>.<a href="#cite_note-65">[65]</a> It is "added by law to all UK milled bread flour except wholemeal".<a href="#cite_note-lhbread-66">[66]</a><a href="#cite_note-defra13-67">[67]</a> It is used in some <a href="/wiki/Soy_milk" title="Soy milk">soy milk</a> and <a href="/wiki/Almond_milk" title="Almond milk">almond milk</a> products as a source of dietary calcium; at least one study suggests that calcium carbonate might be as <a href="/wiki/Bioavailable" class="mw-redirect" title="Bioavailable">bioavailable</a> as the calcium in <a href="/wiki/Cow%27s_milk" class="mw-redirect" title="Cow's milk">cow's milk</a>.<a href="#cite_note-68">[68]</a> Calcium carbonate is also used as a <a href="/wiki/Firming_agent" title="Firming agent">firming agent</a> in many canned and bottled vegetable products. Several calcium supplement formulations have been documented to contain the chemical element <a href="/wiki/Lead" title="Lead">lead</a>,<a href="#cite_note-Kauffman-2007-69">[69]</a> posing a <a href="/wiki/Public_health" title="Public health">public health</a> concern.<a href="#cite_note-ross20-70">[70]</a> Lead is commonly found in natural sources of calcium.<a href="#cite_note-Kauffman-2007-69">[69]</a> <div class="mw-heading mw-heading3"><h3 id="Agriculture_and_aquaculture">Agriculture and aquaculture</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=18" title="Edit section: Agriculture and aquaculture">edit</a>]</div> <a href="/wiki/Agricultural_lime" title="Agricultural lime">Agricultural lime</a>, powdered chalk or limestone, is used as a cheap method of neutralising <a href="/wiki/Soil_pH" title="Soil pH">acidic soil</a>, making it suitable for planting, also used in aquaculture industry for pH regulation of pond soil before initiating culture.<a href="#cite_note-Oates2008-71">[71]</a> There is interest in understanding whether or not it can affect pesticide adsorption and desorption in calcareous soil.<a href="#cite_note-72">[72]</a> <div class="mw-heading mw-heading3"><h3 id="Household_cleaning">Household cleaning</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=19" title="Edit section: Household cleaning">edit</a>]</div> Calcium carbonate is a key ingredient in many household cleaning powders like <a href="/wiki/Comet_(cleanser)" title="Comet (cleanser)">Comet</a> and is used as a scrubbing agent. <div class="mw-heading mw-heading3"><h3 id="Pollution_mitigation">Pollution mitigation</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=20" title="Edit section: Pollution mitigation">edit</a>]</div> In 1989, a researcher, Ken Simmons, introduced <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 into the Whetstone Brook in <a href="/wiki/Massachusetts" title="Massachusetts">Massachusetts</a>.<a href="#cite_note-New_York_Times-73">[73]</a> His hope was that the calcium carbonate would counter the acid in the stream from acid rain and save the trout that had ceased to spawn. Although his experiment was a success, it did increase the amount of aluminium ions in the area of the brook that was not treated with the limestone. This shows that <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 can be added to neutralize the effects of acid rain in <a href="/wiki/River" title="River">river</a> ecosystems. Currently calcium carbonate is used to neutralize acidic conditions in both soil and water.<a href="#cite_note-env-74">[74]</a><a href="#cite_note-Schreiber-1988-75">[75]</a><a href="#cite_note-Kircheis-2006-76">[76]</a> Since the 1970s, such liming has been practiced on a large scale in Sweden to mitigate acidification and several thousand lakes and streams are limed repeatedly.<a href="#cite_note-Guhrén-2006-77">[77]</a> Calcium carbonate is also used in <a href="/wiki/Flue-gas_desulfurization" title="Flue-gas desulfurization">flue-gas desulfurization</a> applications eliminating harmful <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SO2 and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">NO2 emissions from coal and other fossil fuels burnt in large fossil fuel power stations.<a href="#cite_note-env-74">[74]</a> <div class="mw-heading mw-heading3"><h3 id="Plastics">Plastics</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=21" title="Edit section: Plastics">edit</a>]</div> Calcium carbonate is commonly used in the plastic industry as a filler. When it is incorporated in a plastic material, it can improve the hardness, stiffness, dimensional stability and processability of the material.<a href="#cite_note-78">[78]</a> <div class="mw-heading mw-heading2"><h2 id="Calcination_equilibrium">Calcination equilibrium</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=22" title="Edit section: Calcination equilibrium">edit</a>]</div> <a href="/wiki/Calcination" title="Calcination">Calcination</a> of <a href="/wiki/Limestone" title="Limestone">limestone</a> using <a href="/wiki/Charcoal" title="Charcoal">charcoal</a> fires to produce <a href="/wiki/Calcium_oxide" title="Calcium oxide">quicklime</a> has been practiced since antiquity by cultures all over the world. The temperature at which limestone yields calcium oxide is usually given as 825 °C, but stating an absolute threshold is misleading. Calcium carbonate exists in equilibrium with calcium oxide and <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> at any temperature. At each temperature there is a <a href="/wiki/Partial_pressure" title="Partial pressure">partial pressure</a> of carbon dioxide that is in equilibrium with calcium carbonate. At room temperature the equilibrium overwhelmingly favors calcium carbonate, because the equilibrium <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure is only a tiny fraction of the partial <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure in air, which is about 0.035 kPa. At temperatures above 550 °C the equilibrium <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure begins to exceed the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure in air. So above 550 °C, calcium carbonate begins to outgas <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 into air. However, in a charcoal fired kiln, the concentration of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 will be much higher than it is in air. Indeed, if all the <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> in the kiln is consumed in the fire, then the partial pressure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 in the kiln can be as high as 20 kPa.<a href="#cite_note-solvaypcc2007-79">[79]</a> The table shows that this partial pressure is not achieved until the temperature is nearly 800 °C. For the outgassing of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 from calcium carbonate to happen at an economically useful rate, the equilibrium pressure must significantly exceed the ambient pressure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2. And for it to happen rapidly, the equilibrium pressure must exceed total atmospheric pressure of 101 kPa, which happens at 898 °C.<div style="clear:right;" class=""></div> <dl><dd><table class="wikitable"> <caption>Equilibrium pressure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 over <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (P) versus temperature (T).<a href="#cite_note-crc-80">[80]</a> </caption> <tbody><tr> <th>P (kPa) </th> <td>0.055</td> <td>0.13</td> <td>0.31</td> <td>1.80</td> <td>5.9</td> <td>9.3</td> <td>14</td> <td>24</td> <td>34</td> <td>51</td> <td>72</td> <td>80</td> <td>91</td> <td>101</td> <td>179</td> <td>901</td> <td>3961 </td></tr> <tr> <th>T (°C) </th> <td>550</td> <td>587</td> <td>605</td> <td>680</td> <td>727</td> <td>748</td> <td>777</td> <td>800</td> <td>830</td> <td>852</td> <td>871</td> <td>881</td> <td>891</td> <td>898</td> <td>937</td> <td>1082</td> <td>1241 </td></tr></tbody></table></dd></dl> <div class="mw-heading mw-heading2"><h2 id="Solubility">Solubility</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=23" title="Edit section: Solubility">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="With_varying_CO2_pressure">With varying <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=24" title="Edit section: With varying CO2 pressure">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:CanarySpring.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/CanarySpring.jpg/220px-CanarySpring.jpg" decoding="async" width="220" height="141" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/CanarySpring.jpg/330px-CanarySpring.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4c/CanarySpring.jpg/440px-CanarySpring.jpg 2x" data-file-width="2321" data-file-height="1488" /></a><figcaption><a href="/wiki/Travertine" title="Travertine">Travertine</a> calcium carbonate deposits from a <a href="/wiki/Hot_spring" title="Hot spring">hot spring</a></figcaption></figure> Calcium carbonate is poorly soluble in pure water (47 mg/L at normal atmospheric <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 partial pressure as shown below). The equilibrium of its solution is given by the equation (with dissolved calcium carbonate on the right): <dl><dd><table width="500"> <tbody><tr> <td style="width:50%; height:30px;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 ⇌ Ca2+ + CO2−3 </td> <td>Ksp = 3.7×10−9 to 8.7×10−9 at 25 °C </td></tr></tbody></table></dd></dl> where the <a href="/wiki/Solubility_product" class="mw-redirect" title="Solubility product">solubility product</a> for <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+][CO2−3] is given as anywhere from Ksp = 3.7×10−9 to Ksp = 8.7×10−9 at 25 °C, depending upon the data source.<a href="#cite_note-crc-80">[80]</a><a href="#cite_note-81">[81]</a> What the equation means is that the product of molar concentration of calcium ions (<a href="/wiki/Mole_(unit)" title="Mole (unit)">moles</a> of dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+ per liter of solution) with the molar concentration of dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3 cannot exceed the value of Ksp. This seemingly simple solubility equation, however, must be taken along with the more complicated equilibrium of <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> with <a href="/wiki/Water" title="Water">water</a> (see <a href="/wiki/Carbonic_acid" title="Carbonic acid">carbonic acid</a>). Some of the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3 combines with <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+ in the solution according to <dl><dd><table width="500"> <tbody><tr> <td style="width:50%; height:25px;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 ⇌ H+ + CO2−3    </td> <td>Ka2 = 5.61×10−11 at 25 °C </td></tr></tbody></table></dd></dl> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 is known as the <a href="/wiki/Bicarbonate" title="Bicarbonate">bicarbonate</a> ion. <a href="/wiki/Calcium_bicarbonate" title="Calcium bicarbonate">Calcium bicarbonate</a> is many times more soluble in water than calcium carbonate—indeed it exists only in solution. Some of the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 combines with <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+ in solution according to <dl><dd><table> <tbody><tr> <td width="250"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2CO3 ⇌ H+ + HCO−3 </td> <td>Ka1 = 2.5×10−4 at 25 °C </td></tr></tbody></table></dd></dl> Some of the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2CO3 breaks up into water and dissolved carbon dioxide according to <dl><dd><table> <tbody><tr> <td width="250"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2O + CO2(<a href="/wiki/Aqueous" class="mw-redirect" title="Aqueous">aq</a>) ⇌ H2CO3 </td> <td>Kh = 1.70×10−3 at 25 °C </td></tr></tbody></table></dd></dl> And dissolved carbon dioxide is in equilibrium with atmospheric carbon dioxide according to <dl><dd><table> <tbody><tr> <td width="250"><style data-mw-deduplicate="TemplateStyles:r1214402035">.mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num{display:block;line-height:1em;margin:0.0em 0.1em;border-bottom:1px solid}.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0.1em 0.1em}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style>⁠P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2/<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[CO2]⁠ = <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle H_{\rm {v}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="normal">v</mi> </mrow> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle H_{\rm {v}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/802bf8887503d86c668b2f51bd054e2dee6c4f0e" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:3.031ex; height:2.509ex;" alt="{\displaystyle H_{\rm {v}}}"> </td> <td>where <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle H_{\rm {v}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="normal">v</mi> </mrow> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle H_{\rm {v}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/802bf8887503d86c668b2f51bd054e2dee6c4f0e" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:3.031ex; height:2.509ex;" alt="{\displaystyle H_{\rm {v}}}"> = 29.76 atm/(mol/L) at 25 °C (<a href="/wiki/Henry%27s_law" title="Henry's law">Henry volatility</a>), and P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 is the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 partial pressure. </td></tr></tbody></table></dd></dl> For ambient air, P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 is around 3.5×10−4 <a href="/wiki/Standard_atmosphere_(unit)" title="Standard atmosphere (unit)">atm</a> (or equivalently 35 <a href="/wiki/Pascal_(unit)" title="Pascal (unit)">Pa</a>). The last equation above fixes the concentration of dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 as a function of P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2, independent of the concentration of dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3. At atmospheric partial pressure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2, dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 concentration is 1.2×10−5 moles per liter. The equation before that fixes the concentration of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2CO3 as a function of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 concentration. For [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2] = 1.2×10−5, it results in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[H2CO3] = 2.0×10−8 moles per liter. When <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[H2CO3] is known, the remaining three equations together with <table class="wikitable floatright"> <caption>Calcium ion solubility as a function of <a href="/wiki/Carbon_dioxide" title="Carbon dioxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2</a> <a href="/wiki/Partial_pressure" title="Partial pressure">partial pressure</a> at 25 °C (Ksp = 4.47×10−9) </caption> <tbody><tr> <th>P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 (atm) </th> <th><a href="/wiki/PH" title="PH">pH</a> </th> <th><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+] (mol/L) </th></tr> <tr> <td>10−12</td> <td>12.0</td> <td>5.19×10−3 </td></tr> <tr> <td>10−10</td> <td>11.3</td> <td>1.12×10−3 </td></tr> <tr> <td>10−8</td> <td>10.7</td> <td>2.55×10−4 </td></tr> <tr> <td>10−6</td> <td>9.83</td> <td>1.20×10−4 </td></tr> <tr> <td>10−4</td> <td>8.62</td> <td>3.16×10−4 </td></tr> <tr> <td>3.5×10−4</td> <td>8.27</td> <td>4.70×10−4 </td></tr> <tr> <td>10−3</td> <td>7.96</td> <td>6.62×10−4 </td></tr> <tr> <td>10−2</td> <td>7.30</td> <td>1.42×10−3 </td></tr> <tr> <td>10−1</td> <td>6.63</td> <td>3.05×10−3 </td></tr> <tr> <td>1</td> <td>5.96</td> <td>6.58×10−3 </td></tr> <tr> <td>10</td> <td>5.30</td> <td>1.42×10−2 </td></tr></tbody></table> <dl><dd><table width="450"> <tbody><tr> <td style="width:50%; height:25px;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2O ⇌ H+ + OH− </td> <td>K = 10−14 at 25 °C </td></tr></tbody></table></dd></dl> (which is true for all aqueous solutions), and the constraint that the solution must be electrically neutral, i.e., the overall charge of dissolved positive ions <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+] + 2 [H+] must be cancelled out by the overall charge of dissolved negative ions <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[HCO−3] + [CO2−3] + [OH−], make it possible to solve simultaneously for the remaining five unknown concentrations (the previously mentioned form of the neutrality is valid only if calcium carbonate has been put in contact with pure water or with a neutral pH solution; in the case where the initial water solvent pH is not neutral, the balance is not neutral). The adjacent table shows the result for <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+] and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[H+] (in the form of pH) as a function of ambient partial pressure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 (Ksp = 4.47×10−9 has been taken for the calculation). <ul><li>At atmospheric levels of ambient <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 the table indicates that the solution will be slightly alkaline with a maximum <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 solubility of 47 mg/L.</li> <li>As ambient <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 partial pressure is reduced below atmospheric levels, the solution becomes more and more alkaline. At extremely low P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2, dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2, bicarbonate ion, and carbonate ion largely evaporate from the solution, leaving a highly alkaline solution of <a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">calcium hydroxide</a>, which is more soluble than <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3. For P<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 = 10−12 atm, the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+][OH−]2 product is still below the solubility product of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca(OH)2 (8×10−6). For still lower <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 pressure, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca(OH)2 precipitation will occur before <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 precipitation.</li> <li>As ambient <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 partial pressure increases to levels above atmospheric, pH drops, and much of the carbonate ion is converted to bicarbonate ion, which results in higher solubility of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+.</li></ul> The effect of the latter is especially evident in day-to-day life of people who have hard water. Water in aquifers underground can be exposed to levels of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 much higher than atmospheric. As such water percolates through calcium carbonate rock, the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 dissolves according to one of the trends above. When that same water then emerges from the tap, in time it comes into equilibrium with <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 levels in the air by outgassing its excess <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2. The calcium carbonate becomes less soluble as a result, and the excess precipitates as lime scale. This same process is responsible for the formation of <a href="/wiki/Stalactites" class="mw-redirect" title="Stalactites">stalactites</a> and <a href="/wiki/Stalagmite" title="Stalagmite">stalagmites</a> in limestone caves. Two hydrated phases of calcium carbonate, <a href="/wiki/Monohydrocalcite" title="Monohydrocalcite">monohydrocalcite</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3·H2O and <a href="/wiki/Ikaite" title="Ikaite">ikaite</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3·6H2O, may <a href="/wiki/Precipitate" class="mw-redirect" title="Precipitate">precipitate</a> from water at ambient conditions and persist as metastable phases. <div class="mw-heading mw-heading3"><h3 id="With_varying_pH,_temperature_and_salinity:_CaCO3_scaling_in_swimming_pools">With varying pH, temperature and salinity: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 scaling in swimming pools</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=25" title="Edit section: With varying pH, temperature and salinity: CaCO3 scaling in swimming pools">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:CaCO3-pH.gif" class="mw-file-description"><img alt="Effects of salinity and pH on the maximum calcium ion level before scaling is anticipated at 25 °C and 1 mmol/L bicarbonate concentration (e.g. in swimming pools)" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/31/CaCO3-pH.gif/220px-CaCO3-pH.gif" decoding="async" width="220" height="137" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/31/CaCO3-pH.gif/330px-CaCO3-pH.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/31/CaCO3-pH.gif/440px-CaCO3-pH.gif 2x" data-file-width="460" data-file-height="287" /></a><figcaption></figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:CaCO3-Temp.gif" class="mw-file-description"><img alt="Effects of temperature and bicarbonate concentration on the maximum calcium ion level before scaling is anticipated at pH 7 and 5,000 ppm salinity (such as in swimming pools)" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/09/CaCO3-Temp.gif/220px-CaCO3-Temp.gif" decoding="async" width="220" height="140" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/09/CaCO3-Temp.gif/330px-CaCO3-Temp.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/09/CaCO3-Temp.gif/440px-CaCO3-Temp.gif 2x" data-file-width="466" data-file-height="296" /></a><figcaption></figcaption></figure> In contrast to the open equilibrium scenario above, many swimming pools are managed by addition of <a href="/wiki/Sodium_bicarbonate" title="Sodium bicarbonate">sodium bicarbonate</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">NaHCO3) to the concentration of about 2 mmol/L as a buffer, then control of pH through use of HCl, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">NaHSO4, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Na2CO3, NaOH or chlorine formulations that are acidic or basic. In this situation, dissolved inorganic carbon (<a href="/wiki/Total_inorganic_carbon" title="Total inorganic carbon">total inorganic carbon</a>) is far from equilibrium with atmospheric <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2. Progress towards equilibrium through outgassing of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 is slowed by <div><ol><li>the slow reaction <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Carbonic_acid" title="Carbonic acid">H2CO3</a> ⇌ CO2(<a href="/wiki/Aqueous_solution" title="Aqueous solution">aq</a>) + H2O;<a href="#cite_note-82">[82]</a></dd></dl></li><li>limited aeration in a deep water column; and</li><li>periodic replenishment of bicarbonate to maintain buffer capacity (often estimated through measurement of <a href="/wiki/Alkalinity" title="Alkalinity">total alkalinity</a>).</li></ol></div> In this situation, the dissociation constants for the much faster reactions <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2CO3 ⇌ H+ + HCO−3 ⇌ 2 H+ + CO2−3</dd></dl> allow the prediction of concentrations of each dissolved inorganic carbon species in solution, from the added concentration of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 (which constitutes more than 90% of <a href="/wiki/Bjerrum_plot" title="Bjerrum plot">Bjerrum plot</a> species from pH 7 to pH 8 at 25 °C in fresh water).<a href="#cite_note-Mook_2000-83">[83]</a> Addition of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 will increase <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3 concentration at any pH. Rearranging the equations given above, we can see that <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Ca2+] = <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠Ksp/[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3]⁠, and [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3] = <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠Ka2 [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3]/[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+]⁠. Therefore, when <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3 concentration is known, the maximum concentration of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+ ions before scaling through <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 precipitation can be predicted from the formula: <dl><dd>[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+]max = <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠Ksp/Ka2⁠ × <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+]/[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3]⁠</dd></dl> The solubility product for <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (Ksp) and the dissociation constants for the dissolved inorganic carbon species (including Ka2) are all substantially affected by temperature and <a href="/wiki/Salinity" title="Salinity">salinity</a>,<a href="#cite_note-Mook_2000-83">[83]</a> with the overall effect that [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+]max increases from freshwater to saltwater, and decreases with rising temperature, pH, or added bicarbonate level, as illustrated in the accompanying graphs. The trends are illustrative for pool management, but whether scaling occurs also depends on other factors including interactions with <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Magnesium" title="Magnesium">Mg</a>2+, <a href="/wiki/Tetrahydroxyborate" title="Tetrahydroxyborate"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[B(OH)4]−</a> and other ions in the pool, as well as supersaturation effects.<a href="#cite_note-84">[84]</a><a href="#cite_note-85">[85]</a> Scaling is commonly observed in electrolytic chlorine generators, where there is a high pH near the cathode surface and scale deposition further increases temperature. This is one reason that some pool operators prefer borate over bicarbonate as the primary pH buffer, and avoid the use of pool chemicals containing calcium.<a href="#cite_note-86">[86]</a> <div class="mw-heading mw-heading3"><h3 id="Solubility_in_a_strong_or_weak_acid_solution">Solubility in a strong or weak acid solution</h3>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=26" title="Edit section: Solubility in a strong or weak acid solution">edit</a>]</div> Solutions of <a href="/wiki/Strong_acid" class="mw-redirect" title="Strong acid">strong</a> (<a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">HCl</a>), moderately strong (<a href="/wiki/Sulfamic_acid" title="Sulfamic acid">sulfamic</a>) or <a href="/wiki/Weak_acid" class="mw-redirect" title="Weak acid">weak</a> (<a href="/wiki/Acetic_acid" title="Acetic acid">acetic</a>, <a href="/wiki/Citric_acid" title="Citric acid">citric</a>, <a href="/wiki/Sorbic_acid" title="Sorbic acid">sorbic</a>, <a href="/wiki/Lactic_acid" title="Lactic acid">lactic</a>, <a href="/wiki/Phosphoric_acid" title="Phosphoric acid">phosphoric</a>) acids are commercially available. They are commonly used as <a href="/wiki/Descaling_agent" title="Descaling agent">descaling agents</a> to remove <a href="/wiki/Limescale" title="Limescale">limescale</a> deposits. The maximum amount of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 that can be "dissolved" by one liter of an acid solution can be calculated using the above equilibrium equations. <ul><li>In the case of a strong monoacid with decreasing acid concentration [A] = [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A−], we obtain (with <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 molar mass = 100 g/mol):</li></ul> <dl><dd><dl><dd><table class="wikitable"> <tbody><tr> <th>[A] (mol/L) </th> <td>1 </td> <td>10−1 </td> <td>10−2 </td> <td>10−3 </td> <td>10−4 </td> <td>10−5 </td> <td>10−6 </td> <td>10−7 </td> <td>10−10 </td></tr> <tr> <th>Initial pH </th> <td>0.00</td> <td>1.00</td> <td>2.00</td> <td>3.00</td> <td>4.00</td> <td>5.00</td> <td>6.00</td> <td>6.79</td> <td>7.00 </td></tr> <tr> <th>Final pH </th> <td>6.75</td> <td>7.25</td> <td>7.75</td> <td>8.14</td> <td>8.25</td> <td>8.26</td> <td>8.26</td> <td>8.26</td> <td>8.27 </td></tr> <tr> <th>Dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (g/L of acid) </th> <td>50.0</td> <td>5.00</td> <td>0.514</td> <td>0.0849</td> <td>0.0504</td> <td>0.0474</td> <td>0.0471</td> <td>0.0470</td> <td>0.0470 </td></tr></tbody></table></dd></dl></dd></dl> <dl><dd>where the initial state is the acid solution with no <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+ (not taking into account possible <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2 dissolution) and the final state is the solution with saturated <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+. For strong acid concentrations, all species have a negligible concentration in the final state with respect to <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A− so that the neutrality equation reduces approximately to 2[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+] = [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A−] yielding [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+] ≈ 0.5 [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A−]. When the concentration decreases, [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3] becomes non-negligible so that the preceding expression is no longer valid. For vanishing acid concentrations, one can recover the final pH and the solubility of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 in pure water.</dd></dl> <ul><li>In the case of a weak monoacid (here we take acetic acid with <a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">pKa</a> = 4.76) with decreasing total acid concentration [A] = [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A−] + [AH], we obtain:</li></ul> <dl><dd><dl><dd><table class="wikitable"> <tbody><tr> <th>[A] (mol/L) </th> <td>[<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+] ≈ 0.5 [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">A−] [<a href="/wiki/Wikipedia:Please_clarify" title="Wikipedia:Please clarify">clarification needed</a>] </td> <td>10−1 </td> <td>10−2 </td> <td>10−3 </td> <td>10−4 </td> <td>10−5 </td> <td>10−6 </td> <td>10−7 </td> <td>10−10 </td></tr> <tr> <th>Initial pH </th> <td>2.38</td> <td>2.88</td> <td>3.39</td> <td>3.91</td> <td>4.47</td> <td>5.15</td> <td>6.02</td> <td>6.79</td> <td>7.00 </td></tr> <tr> <th>Final pH </th> <td>6.75</td> <td>7.25</td> <td>7.75</td> <td>8.14</td> <td>8.25</td> <td>8.26</td> <td>8.26</td> <td>8.26</td> <td>8.27 </td></tr> <tr> <th>Dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (g/L of acid) </th> <td>49.5</td> <td>4.99</td> <td>0.513</td> <td>0.0848</td> <td>0.0504</td> <td>0.0474</td> <td>0.0471</td> <td>0.0470</td> <td>0.0470 </td></tr></tbody></table></dd></dl></dd></dl> <dl><dd>For the same total acid concentration, the initial pH of the weak acid is less acid than the one of the strong acid; however, the maximum amount of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 which can be dissolved is approximately the same. This is because in the final state, the pH is larger than the pKa, so that the weak acid is almost completely dissociated, yielding in the end as many <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+ ions as the strong acid to "dissolve" the calcium carbonate.</dd></dl> <ul><li>The calculation in the case of <a href="/wiki/Phosphoric_acid" title="Phosphoric acid">phosphoric acid</a> (which is the most widely used for domestic applications) is more complicated since the concentrations of the four dissociation states corresponding to this acid must be calculated together with [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HCO−3], [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CO2−3], [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Ca2+], [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+] and [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">OH−]. The system may be reduced to a seventh degree equation for [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H+] the numerical solution of which gives</li></ul> <dl><dd><dl><dd><table class="wikitable"> <tbody><tr> <th>[A] (mol/L) </th> <td>1 </td> <td>10−1 </td> <td>10−2 </td> <td>10−3 </td> <td>10−4 </td> <td>10−5 </td> <td>10−6 </td> <td>10−7 </td> <td>10−10 </td></tr> <tr> <th>Initial pH </th> <td>1.08</td> <td>1.62</td> <td>2.25</td> <td>3.05</td> <td>4.01</td> <td>5.00</td> <td>5.97</td> <td>6.74</td> <td>7.00 </td></tr> <tr> <th>Final pH </th> <td>6.71</td> <td>7.17</td> <td>7.63</td> <td>8.06</td> <td>8.24</td> <td>8.26</td> <td>8.26</td> <td>8.26</td> <td>8.27 </td></tr> <tr> <th>Dissolved <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CaCO3 (g/L of acid) </th> <td>62.0</td> <td>7.39</td> <td>0.874</td> <td>0.123</td> <td>0.0536</td> <td>0.0477</td> <td>0.0471</td> <td>0.0471</td> <td>0.0470 </td></tr></tbody></table></dd></dl></dd></dl> <dl><dd>where [A] = <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[H3PO4] + [H2PO−4] + [HPO2−4] + [PO3−4] is the total acid concentration. Thus phosphoric acid is more efficient than a monoacid since at the final almost neutral pH, the second dissociated state concentration [<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HPO2−4] is not negligible (see <a href="/wiki/Phosphoric_acid#pH_and_composition_of_a_phosphoric_acid_aqueous_solution" title="Phosphoric acid">phosphoric acid</a>).</dd></dl> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=27" title="Edit section: See also">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Vodn%C3%AD_k%C3%A1men.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Vodn%C3%AD_k%C3%A1men.jpg/220px-Vodn%C3%AD_k%C3%A1men.jpg" decoding="async" width="220" height="220" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Vodn%C3%AD_k%C3%A1men.jpg/330px-Vodn%C3%AD_k%C3%A1men.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Vodn%C3%AD_k%C3%A1men.jpg/440px-Vodn%C3%AD_k%C3%A1men.jpg 2x" data-file-width="1536" data-file-height="1537" /></a><figcaption>Electron micrograph of needle-like calcium carbonate crystals formed as limescale in a kettle</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Calcium-48_carbonate.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/af/Calcium-48_carbonate.png/220px-Calcium-48_carbonate.png" decoding="async" width="220" height="265" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/af/Calcium-48_carbonate.png/330px-Calcium-48_carbonate.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/af/Calcium-48_carbonate.png/440px-Calcium-48_carbonate.png 2x" data-file-width="592" data-file-height="714" /></a><figcaption>Around 2 g of calcium-48 carbonate</figcaption></figure> <style data-mw-deduplicate="TemplateStyles:r1184024115">.mw-parser-output .div-col{margin-top:0.3em;column-width:30em}.mw-parser-output .div-col-small{font-size:90%}.mw-parser-output .div-col-rules{column-rule:1px solid #aaa}.mw-parser-output .div-col dl,.mw-parser-output .div-col ol,.mw-parser-output .div-col ul{margin-top:0}.mw-parser-output .div-col li,.mw-parser-output .div-col dd{page-break-inside:avoid;break-inside:avoid-column}</style><div class="div-col" style="column-width: 22em;"> <ul><li><a href="/wiki/Cuttlebone" title="Cuttlebone">Cuttlebone</a></li> <li><a href="/wiki/Cuttlefish" title="Cuttlefish">Cuttlefish</a></li> <li><a href="/wiki/Gesso" title="Gesso">Gesso</a></li> <li><a href="/wiki/Limescale" title="Limescale">Limescale</a></li> <li><a href="/wiki/Marble" title="Marble">Marble</a></li> <li><a href="/wiki/Ocean_acidification" title="Ocean acidification">Ocean acidification</a></li> <li><a href="/wiki/Whiting_event" title="Whiting event">Whiting event</a></li> <li><a href="/wiki/List_of_climate_engineering_topics" title="List of climate engineering topics">List of climate engineering topics</a></li> <li><a href="/wiki/Lysocline" title="Lysocline">Lysocline</a></li></ul></div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2>[<a href="/w/index.php?title=Calcium_carbonate&action=edit&section=28" title="Edit section: References">edit</a>]</div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-1"><a href="#cite_ref-1">^</a> <style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite id="CITEREFAylwardFindlay2008" class="citation book cs1">Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data Book (4th ed.). John Wiley & Sons Australia. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-470-81638-7" title="Special:BookSources/978-0-470-81638-7"><bdi>978-0-470-81638-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=SI+Chemical+Data+Book&rft.edition=4th&rft.pub=John+Wiley+%26+Sons+Australia&rft.date=2008&rft.isbn=978-0-470-81638-7&rft.aulast=Aylward&rft.aufirst=Gordon&rft.au=Findlay%2C+Tristan&rfr_id=info%3Asid%2Fen.wikipedia.org%3ACalcium+carbonate" class="Z3988"> </li> <li id="cite_note-2"><a href="#cite_ref-2">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFRohlederKroker2001" class="citation book cs1">Rohleder, J.; Kroker, E. (2001). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=pbkKGa19k5QC&pg=RA1-PR2">Calcium Carbonate: From the Cretaceous Period Into the 21st Century</a>. 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Retrieved 15 December 2022.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+the+American+Chemical+Society&rft.atitle=Nacre+Protein+Fragment+Templates+Lamellar+Aragonite+Growth&rft.volume=132&rft.issue=18&rft.pages=%3Cspan+class%3D%22nowrap%22%3E6329-%3C%2Fspan%3E6334&rft.date=2010-05-12&rft.issn=0002-7863&rft_id=info%3Apmid%2F20397648&rft_id=info%3Adoi%2F10.1021%2Fja909735y&rft.aulast=Metzler&rft.aufirst=Rebecca+A.&rft.au=Evans%2C+John+Spencer&rft.au=Killian%2C+Christopher+E.&rft.au=Zhou%2C+Dong&rft.au=Churchill%2C+Tyler+H.&rft.au=Appathurai%2C+Narayana+P.&rft.au=Coppersmith%2C+Susan+N.&rft.au=Gilbert%2C+P.+U.+P.+A.&rft_id=https%3A%2F%2Fpubs.acs.org%2Fdoi%2F10.1021%2Fja909735y&rfr_id=info%3Asid%2Fen.wikipedia.org%3ACalcium+carbonate" class="Z3988"> </li> <li id="cite_note-23"><a href="#cite_ref-23">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLowenstamWeiner1989" class="citation book cs1">Lowenstam, H.A.; Weiner, S. 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Retrieved 20 April 2018.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+Geophysical+Research&rft.atitle=Evidence+for+montmorillonite+or+its+compositional+equivalent+in+Columbia+Hills%2C+Mars&rft.volume=112&rft.issue=E6&rft.pages=E06S01&rft.date=2007&rft_id=info%3Ahdl%2F1893%2F17119&rft_id=info%3Adoi%2F10.1029%2F2006JE002756&rft_id=info%3Abibcode%2F2007JGRE..112.6S01C&rft.aulast=Clark&rft.aufirst=B.+C.+III&rft.au=Arvidson%2C+R.+E.&rft.au=Gellert%2C+R.&rft.au=Morris%2C+R.+V.&rft.au=Ming%2C+D.+W.&rft.au=Richter%2C+L.&rft.au=Ruff%2C+S.+W.&rft.au=Michalski%2C+J.+R.&rft.au=Farrand%2C+W.+H.&rft.au=Yen%2C+A.&rft.au=Herkenhoff%2C+K.+E.&rft.au=Li%2C+R.&rft.au=Squyres%2C+S.+W.&rft.au=Schr%C3%B6der%2C+C.&rft.au=Klingelh%C3%B6fer%2C+G.&rft.au=Bell%2C+J.+F.&rft_id=http%3A%2F%2Fdspace.stir.ac.uk%2Fbitstream%2F1893%2F17119%2F1%2FClark2007_Evidence_for_montmorillonite_or_its_compositional_equivalent_in_Columbia_Hills_Mars.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3ACalcium+carbonate" class="Z3988"> </li> <li id="cite_note-weyl1959-37"><a href="#cite_ref-weyl1959_37-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWeyl1959" class="citation journal cs1">Weyl, P.K. 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title="PubChem">PubChem</a></li> <li><a href="/wiki/ATC_codes" class="mw-redirect" title="ATC codes">ATC codes</a>: <a href="/wiki/ATC_code_A02" title="ATC code A02">A02AC01</a> (<a rel="nofollow" class="external text" href="https://www.whocc.no/atc_ddd_index/?code=A02AC01">WHO</a>) and <a href="/wiki/ATC_code_A12" title="ATC code A12">A12AA04</a> (<a rel="nofollow" class="external text" href="https://www.whocc.no/atc_ddd_index/?code=A12AA04">WHO</a>)</li> <li><a rel="nofollow" class="external text" href="http://calcium-carbonate.org.uk/calcium-carbonate.asp">The British Calcium Carbonate Association – What is calcium carbonate</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20080524102528/http://www.calcium-carbonate.org.uk/calcium-carbonate.asp">Archived</a> 24 May 2008 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a></li> <li><a rel="nofollow" class="external text" href="https://www.cdc.gov/niosh/npg/npgd0090.html">CDC 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scope="row" class="navbox-group" style="width:1%">Hydrogen & halogens</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_hydride" title="Calcium hydride">CaH2</a></li> <li><a href="/wiki/Calcium_fluoride" title="Calcium fluoride">CaF2</a></li> <li><a href="/wiki/Calcium_chloride" title="Calcium chloride">CaCl2</a></li> <li><a href="/wiki/Calcium_hypochlorite" title="Calcium hypochlorite">Ca(ClO)2</a></li> <li><a href="/wiki/Calcium_chlorate" title="Calcium chlorate">Ca(ClO3)2</a></li> <li><a href="/wiki/Calcium_perchlorate" title="Calcium perchlorate">Ca(ClO4)2</a></li> <li><a href="/wiki/Calcium_bromide" title="Calcium bromide">CaBr2</a></li> <li><a href="/wiki/Calcium_bromate" title="Calcium bromate">Ca(BrO3)2</a></li> <li><a href="/wiki/Calcium_iodide" title="Calcium iodide">CaI2</a></li> <li><a href="/wiki/Calcium_iodate" title="Calcium iodate">Ca(IO3)2</a></li> <li><a href="/wiki/Calcium(I)_chloride" title="Calcium(I) chloride">CaICl</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Chalcogens</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_oxide" title="Calcium oxide">CaO</a></li> <li><a href="/wiki/Calcium_peroxide" title="Calcium peroxide">CaO2</a></li> <li><a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">Ca(OH)2</a></li> <li><a href="/wiki/Calcium_sulfide" title="Calcium sulfide">CaS</a></li> <li><a href="/wiki/Calcium_sulfite" title="Calcium sulfite">CaSO3</a></li> <li><a href="/wiki/Calcium_bisulfite" title="Calcium bisulfite">CaH2S2O6</a></li> <li><a href="/wiki/Calcium_sulfate" title="Calcium sulfate">CaSO4</a></li> <li><a href="/wiki/Calcium_selenide" title="Calcium selenide">CaSe</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Pnictogens</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_nitride" title="Calcium nitride">Ca3N2</a></li> <li><a href="/wiki/Calcium_azide" title="Calcium azide">CaN6</a></li> <li><a href="/wiki/Calcium_nitrite" title="Calcium nitrite">Ca(NO2)2</a></li> <li><a href="/wiki/Calcium_nitrate" title="Calcium nitrate">Ca(NO3)2</a></li> <li><a href="/wiki/Calcium_phosphide" title="Calcium phosphide">Ca3P2</a></li> <li><a href="/wiki/Calcium_monophosphide" title="Calcium monophosphide">CaP</a></li> <li><a href="/wiki/Tetracalcium_phosphate" title="Tetracalcium phosphate">Ca4(PO4)2O</a></li> <li><a href="/wiki/Tricalcium_phosphate" title="Tricalcium phosphate">Ca3(PO4)2</a></li> <li><a href="/wiki/Dicalcium_phosphate" title="Dicalcium phosphate">CaHPO4</a></li> <li><a href="/wiki/Monocalcium_phosphate" title="Monocalcium phosphate">Ca(H2PO4)2</a></li> <li><a href="/wiki/Calcium_pyrophosphate" title="Calcium pyrophosphate">Ca2P2O7</a></li> <li><a href="/wiki/Calcium_arsenide" title="Calcium arsenide">CaAs</a></li> <li><a href="/wiki/Calcium_arsenate" title="Calcium arsenate">Ca3(AsO4)2</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Group 13 & 14</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_carbide" title="Calcium carbide">CaC2</a></li> <li><a href="/wiki/Calcium_cyanide" title="Calcium cyanide">Ca(CN)2</a></li> <li><a href="/wiki/Calcium_cyanamide" title="Calcium cyanamide">CaCN2</a></li> <li><a class="mw-selflink selflink">CaCO3</a></li> <li><a href="/wiki/Calcium_bicarbonate" title="Calcium bicarbonate">Ca(HCO3)2</a></li> <li><a href="/wiki/Calcium_monosilicide" title="Calcium monosilicide">CaSi</a></li> <li><a href="/wiki/Calcium_disilicide" title="Calcium disilicide">CaSi2</a></li> <li><a href="/wiki/Calcium_silicate" title="Calcium silicate">Ca2SiO4</a></li> <li><a href="/wiki/Calcium_borate" title="Calcium borate">Ca3(BO3)2</a></li> <li><a href="/wiki/Monocalcium_aluminate" title="Monocalcium aluminate">CaAl2O4</a></li> <li><a href="/wiki/Tricalcium_aluminate" title="Tricalcium aluminate">Ca3Al2O6</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Trans metals</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_permanganate" title="Calcium permanganate">Ca(MnO4)2</a></li> <li><a href="/wiki/Calcium_chromate" title="Calcium chromate">CaCrO4</a></li> <li><a href="/wiki/Calcium_titanate" title="Calcium titanate">CaTiO3</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Organics</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Calcium_oxalate" title="Calcium oxalate">CaC2O4</a></li> <li><a href="/wiki/Calcium_formate" title="Calcium formate">Ca(HCO2)2</a></li> <li><a href="/wiki/Calcium_acetate" title="Calcium acetate">Ca(CH3CO2)2</a></li> <li><a href="/wiki/Calcium_propanoate" title="Calcium propanoate">Ca(C3H5O2)2</a></li> <li><a href="/wiki/Calcium_fumarate" title="Calcium fumarate">CaC4H2O4</a></li> <li><a href="/wiki/Calcium_citrate" title="Calcium citrate">Ca3(C6H5O7)2</a></li> <li><a href="/wiki/Calcium_glycerylphosphate" title="Calcium glycerylphosphate">C3H7CaO6P</a></li> <li><a href="/wiki/Calcium_dobesilate" title="Calcium dobesilate">Ca(C6H5O5S)2</a></li> <li><a href="/wiki/Calcium_erythorbate" title="Calcium erythorbate">Ca(C6H7O6)2</a></li> <li><a href="/wiki/Calcium_inosinate" title="Calcium inosinate">C10H11CaN4O8P</a></li> <li><a href="/wiki/Calcium_guanylate" title="Calcium guanylate">CaC10H12O4N5PO4</a></li> <li><a href="/wiki/Calcium_diglutamate" title="Calcium diglutamate">C10H16CaN2O8</a></li> <li><a href="/wiki/Calcium_gluconate" title="Calcium gluconate">C12H22CaO14</a></li> <li><a href="/wiki/Calcium_glucoheptonate" title="Calcium glucoheptonate">C14H26CaO16</a></li> <li><a href="/wiki/Calcium_glubionate" title="Calcium glubionate">C18H32CaO19</a></li> <li><a href="/wiki/Calcium_stearate" title="Calcium stearate">C36H70CaO4</a></li> <li><a href="/wiki/Calcium_fructoborate" title="Calcium fructoborate">C24H40B2CaO24</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div><div role="navigation" class="navbox" aria-labelledby="Compounds_containing_the_carbonate_group127" style="display:table;;padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit;table-layout:fixed;"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Carbonates" title="Template:Carbonates"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Carbonates" title="Template talk:Carbonates"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Carbonates" title="Special:EditPage/Template:Carbonates"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Compounds_containing_the_carbonate_group127" style="font-size:114%;margin:0 4em">Compounds containing the <a href="/wiki/Carbonate" title="Carbonate">carbonate</a> group</div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd" style="width:100%;padding:0;border-width:0;"><div style="padding:0"><div class="mw-collapsible-content" style="overflow-x:auto"> <table class="center"> <tbody><tr style="background-color:mistyrose"> <td><a href="/wiki/Carbonic_acid" title="Carbonic acid">H2CO3</a> </td> <td style="background-color:white;color:inherit;border:none"> </td> <td style="background-color:white;color:inherit;border:none" colspan="11" rowspan="3"> </td> <td style="background-color:white;color:inherit;border:none" colspan="5"> </td> <td>He </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Lithium_carbonate" title="Lithium carbonate">Li2CO3</a>, <a href="/wiki/Lithium_bicarbonate" title="Lithium bicarbonate">LiHCO3</a> </td> <td><a href="/wiki/Beryllium_carbonate" title="Beryllium carbonate">BeCO3</a> </td> <td><a href="/wiki/Borate_carbonate" title="Borate carbonate">+BO3</a> </td> <td><a href="/wiki/Carbonate_ester" title="Carbonate ester">(RO)(R'O)CO</a> <a href="/wiki/Carbonate_oxalate" title="Carbonate oxalate">+C2O4</a> </td> <td><a href="/wiki/Ammonium_carbonate" title="Ammonium carbonate">(NH4)2CO3</a>, <a href="/wiki/Ammonium_bicarbonate" title="Ammonium bicarbonate">NH4HCO3</a>, <a href="/wiki/Carbonate_nitrate" title="Carbonate nitrate">+NO3</a> </td> <td>O </td> <td><a href="/wiki/Carbonate_fluoride" class="mw-redirect" title="Carbonate fluoride">+F</a> </td> <td>Ne </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Sodium_carbonate" title="Sodium carbonate">Na2CO3</a>, <a href="/wiki/Sodium_bicarbonate" title="Sodium bicarbonate">NaHCO3</a>, <a href="/wiki/Sodium_sesquicarbonate" title="Sodium sesquicarbonate">Na3H(CO3)2</a> </td> <td><a href="/wiki/Magnesium_carbonate" title="Magnesium carbonate">MgCO3</a>, <a href="/wiki/Magnesium_bicarbonate" title="Magnesium bicarbonate">Mg(HCO3)2</a> </td> <td><a href="/wiki/Aluminium_carbonate" title="Aluminium carbonate">Al2(CO3)3</a> </td> <td><a href="/wiki/Silicon_carbonate" title="Silicon carbonate">SiCO4</a>, <a href="/wiki/Silicate_carbonate" title="Silicate carbonate">+SiO4</a> </td> <td>P </td> <td><a href="/wiki/Sulfate_carbonate" title="Sulfate carbonate">+SO4</a> </td> <td><a href="/wiki/Carbonate_chloride" title="Carbonate chloride">+Cl</a> </td> <td>Ar </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Potassium_carbonate" title="Potassium carbonate">K2CO3</a>, <a href="/wiki/Potassium_bicarbonate" title="Potassium bicarbonate">KHCO3</a> </td> <td><a class="mw-selflink selflink">CaCO3</a>, <a href="/wiki/Calcium_bicarbonate" title="Calcium bicarbonate">Ca(HCO3)2</a> </td> <td style="background-color:white;color:inherit;border:none"> </td> <td>Sc </td> <td>Ti </td> <td>V </td> <td><a href="/w/index.php?title=Chromium(II)_carbonate&action=edit&redlink=1" class="new" title="Chromium(II) carbonate (page does not exist)">CrCO3</a>, <a href="/w/index.php?title=Chromium(III)_carbonate&action=edit&redlink=1" class="new" title="Chromium(III) carbonate (page does not exist)">Cr2(CO3)3</a> </td> <td><a href="/wiki/Manganese(II)_carbonate" title="Manganese(II) carbonate">MnCO3</a> </td> <td><a href="/wiki/Iron(II)_carbonate" title="Iron(II) carbonate">FeCO3</a> </td> <td><a href="/wiki/Cobalt(II)_carbonate" title="Cobalt(II) carbonate">CoCO3</a>, <a href="/w/index.php?title=Cobalt(III)_carbonate&action=edit&redlink=1" class="new" title="Cobalt(III) carbonate (page does not exist)">Co2(CO3)3</a> </td> <td><a href="/wiki/Nickel(II)_carbonate" title="Nickel(II) carbonate">NiCO3</a> </td> <td><a href="/w/index.php?title=Copper(I)_carbonate&action=edit&redlink=1" class="new" title="Copper(I) carbonate (page does not exist)">Cu2CO3</a>, <a href="/wiki/Copper(II)_carbonate" title="Copper(II) carbonate">CuCO3</a>, <a href="/wiki/Basic_copper_carbonate" title="Basic copper carbonate">Cu2CO3(OH)2</a> </td> <td><a href="/wiki/Zinc_carbonate" title="Zinc carbonate">ZnCO3</a> </td> <td>Ga </td> <td>Ge </td> <td>As </td> <td>Se </td> <td>Br </td> <td>Kr </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Rubidium_carbonate" title="Rubidium carbonate">Rb2CO3</a> </td> <td><a href="/wiki/Strontium_carbonate" title="Strontium carbonate">SrCO3</a> </td> <td style="background-color:white;color:inherit;border:none"> </td> <td>Y </td> <td>Zr </td> <td>Nb </td> <td>Mo </td> <td>Tc </td> <td>Ru </td> <td>Rh </td> <td><a href="/w/index.php?title=Palladium(II)_carbonate&action=edit&redlink=1" class="new" title="Palladium(II) carbonate (page does not exist)">PdCO3</a> </td> <td><a href="/wiki/Silver_carbonate" title="Silver carbonate">Ag2CO3</a> </td> <td><a href="/wiki/Cadmium_carbonate" class="mw-redirect" title="Cadmium carbonate">CdCO3</a> </td> <td>In </td> <td>Sn </td> <td>Sb </td> <td>Te </td> <td>I </td> <td>Xe </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Caesium_carbonate" title="Caesium carbonate">Cs2CO3</a>, <a href="/wiki/Caesium_bicarbonate" title="Caesium bicarbonate">CsHCO3</a> </td> <td><a href="/wiki/Barium_carbonate" title="Barium carbonate">BaCO3</a> </td> <td style="background-color:white;color:inherit;border:none">* </td> <td><a href="/w/index.php?title=Lutetium(III)_carbonate&action=edit&redlink=1" class="new" title="Lutetium(III) carbonate (page does not exist)">Lu2(CO3)3</a> </td> <td>Hf </td> <td>Ta </td> <td>W </td> <td>Re </td> <td>Os </td> <td>Ir </td> <td>Pt </td> <td>Au </td> <td><a href="/w/index.php?title=Mercury(II)_carbonate&action=edit&redlink=1" class="new" title="Mercury(II) carbonate (page does not exist)">HgCO3</a> </td> <td><a href="/wiki/Thallium(I)_carbonate" title="Thallium(I) carbonate">Tl2CO3</a> </td> <td><a href="/wiki/Lead_carbonate" title="Lead carbonate">PbCO3</a> </td> <td><a href="/wiki/Bismuth_subcarbonate" title="Bismuth subcarbonate">(BiO)2CO3</a> </td> <td><a href="/w/index.php?title=Polonium(IV)_carbonate&action=edit&redlink=1" class="new" title="Polonium(IV) carbonate (page does not exist)">Po(CO3)2</a> </td> <td>At </td> <td>Rn </td></tr> <tr style="background-color:mistyrose;color:black;"> <td>Fr </td> <td><a href="/wiki/Radium_carbonate" title="Radium carbonate">RaCO3</a> </td> <td style="background-color:white;color:inherit;border:none">** </td> <td>Lr </td> <td>Rf </td> <td>Db </td> <td>Sg </td> <td>Bh </td> <td>Hs </td> <td>Mt </td> <td>Ds </td> <td>Rg </td> <td>Cn </td> <td>Nh </td> <td>Fl </td> <td>Mc </td> <td>Lv </td> <td>Ts </td> <td>Og </td></tr> <tr> <td style="background-color:white;color:inherit;border:none" colspan="2" rowspan="3"> </td> <td style="background-color:white;color:inherit;border:none" colspan="20">  </td></tr> <tr style="background-color:mistyrose;color:black;"> <td style="background-color:white;color:inherit;border:none">* </td> <td><a href="/wiki/Lanthanum_carbonate" title="Lanthanum carbonate">La2(CO3)3</a> </td> <td><a href="/wiki/Cerium(III)_carbonate" title="Cerium(III) carbonate">Ce2(CO3)3</a> </td> <td><a href="/wiki/Praseodymium(III)_carbonate" title="Praseodymium(III) carbonate">Pr2(CO3)3</a> </td> <td><a href="/wiki/Neodymium(III)_carbonate" title="Neodymium(III) carbonate">Nd2(CO3)3</a> </td> <td>Pm </td> <td><a href="/w/index.php?title=Samarium(III)_carbonate&action=edit&redlink=1" class="new" title="Samarium(III) carbonate (page does not exist)">Sm2(CO3)3</a> </td> <td><a href="/w/index.php?title=Europium(II)_carbonate&action=edit&redlink=1" class="new" title="Europium(II) carbonate (page does not exist)">EuCO3</a>, <a href="/wiki/Europium(III)_carbonate" title="Europium(III) carbonate">Eu2(CO3)3</a> </td> <td><a href="/w/index.php?title=Gadolinium(III)_carbonate&action=edit&redlink=1" class="new" title="Gadolinium(III) carbonate (page does not exist)">Gd2(CO3)3</a> </td> <td><a href="/w/index.php?title=Terbium(III)_carbonate&action=edit&redlink=1" class="new" title="Terbium(III) carbonate (page does not exist)">Tb2(CO3)3</a> </td> <td><a href="/w/index.php?title=Dysprosium(III)_carbonate&action=edit&redlink=1" class="new" title="Dysprosium(III) carbonate (page does not exist)">Dy2(CO3)3</a> </td> <td><a href="/w/index.php?title=Holmium(III)_carbonate&action=edit&redlink=1" class="new" title="Holmium(III) carbonate (page does not exist)">Ho2(CO3)3</a> </td> <td><a href="/w/index.php?title=Erbium(III)_carbonate&action=edit&redlink=1" class="new" title="Erbium(III) carbonate (page does not exist)">Er2(CO3)3</a> </td> <td><a href="/w/index.php?title=Thulium(III)_carbonate&action=edit&redlink=1" class="new" title="Thulium(III) carbonate (page does not exist)">Tm2(CO3)3</a> </td> <td><a href="/w/index.php?title=Ytterbium(III)_carbonate&action=edit&redlink=1" class="new" title="Ytterbium(III) carbonate (page does not exist)">Yb2(CO3)3</a> </td></tr> <tr style="background-color:mistyrose;color:black;"> <td style="background-color:white;color:inherit;border:none">** </td> <td>Ac </td> <td><a href="/w/index.php?title=Thorium(IV)_carbonate&action=edit&redlink=1" class="new" title="Thorium(IV) carbonate (page does not exist)">Th(CO3)2</a> </td> <td>Pa </td> <td><a href="/wiki/Uranyl_carbonate" title="Uranyl carbonate">UO2CO3</a> </td> <td>Np </td> <td>Pu </td> <td>Am </td> <td>Cm </td> <td>Bk </td> <td>Cf </td> <td>Es </td> <td>Fm </td> <td>Md </td> <td>No </td></tr></tbody></table></div> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div><div role="navigation" class="navbox" aria-labelledby="Drugs_for_acid_related_disorders:_Antacids_(A02A)231" style="padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Antacids" title="Template:Antacids"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Antacids" title="Template talk:Antacids"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Antacids" title="Special:EditPage/Template:Antacids"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Drugs_for_acid_related_disorders:_Antacids_(A02A)231" style="font-size:114%;margin:0 4em">Drugs for acid related disorders: <a href="/wiki/Antacid" title="Antacid">Antacids</a> (<a href="/wiki/ATC_code_A02#A02A" title="ATC code A02">A02A</a>)</div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Magnesium" title="Magnesium">Magnesium</a> (increases motility)</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Magnesium_carbonate" title="Magnesium carbonate">Magnesium carbonate</a></li> <li><a href="/wiki/Magnesium_oxide" title="Magnesium oxide">Magnesium oxide</a></li> <li><a href="/wiki/Magnesium_peroxide" title="Magnesium peroxide">Magnesium peroxide</a></li> <li><a href="/wiki/Magnesium_hydroxide" title="Magnesium hydroxide">Magnesium hydroxide</a></li> <li><a href="/wiki/Talc" title="Talc">Magnesium silicate</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Aluminium" title="Aluminium">Aluminium</a> (decreases motility)</th><td class="navbox-list-with-group navbox-list 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<ul><li><a class="mw-selflink selflink">Calcium carbonate</a></li> <li><a href="/wiki/Calcium_silicate" title="Calcium silicate">Calcium silicate</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Sodium" title="Sodium">Sodium</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Sodium_bicarbonate" title="Sodium bicarbonate">Sodium bicarbonate</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Combinations and complexes of aluminium, calcium and magnesium</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Almagate" title="Almagate">Almagate</a></li> <li><a href="/wiki/Almasilate" title="Almasilate">Almasilate</a></li> <li><a href="/wiki/Hydrotalcite" title="Hydrotalcite">Hydrotalcite</a></li> <li><a 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