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class="vector-toc-text"> 3.1 Alkali metals </div> </a> <ul id="toc-Alkali_metals-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Alkaline_earth_metals" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Alkaline_earth_metals"> <div class="vector-toc-text"> 3.2 Alkaline earth metals </div> </a> <ul id="toc-Alkaline_earth_metals-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Boron_group_elements" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Boron_group_elements"> <div class="vector-toc-text"> 3.3 Boron group elements </div> </a> <ul id="toc-Boron_group_elements-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Carbon_group_elements" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Carbon_group_elements"> <div class="vector-toc-text"> 3.4 Carbon group elements </div> </a> <ul id="toc-Carbon_group_elements-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_main-group_elements" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Other_main-group_elements"> <div class="vector-toc-text"> 3.5 Other main-group elements </div> </a> <ul id="toc-Other_main-group_elements-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Transition_and_post-transition_metals" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Transition_and_post-transition_metals"> <div class="vector-toc-text"> 3.6 Transition and post-transition metals </div> </a> <ul id="toc-Transition_and_post-transition_metals-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Basic_salts_containing_hydroxide" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Basic_salts_containing_hydroxide"> <div class="vector-toc-text"> 4 Basic salts containing hydroxide </div> </a> <ul id="toc-Basic_salts_containing_hydroxide-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Structural_chemistry" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Structural_chemistry"> <div class="vector-toc-text"> 5 Structural chemistry </div> </a> <ul id="toc-Structural_chemistry-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organic_reactions" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Organic_reactions"> <div class="vector-toc-text"> 6 Organic reactions </div> </a> <button aria-controls="toc-Organic_reactions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Organic reactions subsection </button> <ul id="toc-Organic_reactions-sublist" class="vector-toc-list"> <li id="toc-Base_catalysis" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Base_catalysis"> <div class="vector-toc-text"> 6.1 Base catalysis </div> </a> <ul id="toc-Base_catalysis-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-As_a_nucleophilic_reagent" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#As_a_nucleophilic_reagent"> <div class="vector-toc-text"> 6.2 As a nucleophilic reagent </div> </a> <ul id="toc-As_a_nucleophilic_reagent-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Notes" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Notes"> <div class="vector-toc-text"> 7 Notes </div> </a> <ul id="toc-Notes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> 8 References </div> </a> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Bibliography" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Bibliography"> <div class="vector-toc-text"> 9 Bibliography </div> </a> <ul id="toc-Bibliography-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">Hydroxide</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 61 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-61" aria-hidden="true" > 61 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/Hidroksied" title="Hidroksied – Afrikaans" lang="af" hreflang="af" data-title="Hidroksied" 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%87%D9%8A%D8%AF%D8%B1%D9%88%D9%83%D8%B3%D9%8A%D8%AF" title="هيدروكسيد – Arabic" lang="ar" hreflang="ar" data-title="هيدروكسيد" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target">العربية</a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Hidr%C3%B3xidu" title="Hidróxidu – Asturian" lang="ast" hreflang="ast" data-title="Hidróxidu" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target">Asturianu</a></li><li class="interlanguage-link interwiki-azb mw-list-item"><a href="https://azb.wikipedia.org/wiki/%D9%87%DB%8C%D8%AF%D8%B1%D9%88%DA%A9%D8%B3%DB%8C%D8%AF" title="هیدروکسید – South Azerbaijani" lang="azb" hreflang="azb" data-title="هیدروکسید" 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%B9%E0%A6%BE%E0%A6%87%E0%A6%A1%E0%A7%8D%E0%A6%B0%E0%A7%8B%E0%A6%95%E0%A7%8D%E0%A6%B8%E0%A6%BE%E0%A6%87%E0%A6%A1" title="হাইড্রোক্সাইড – Bangla" lang="bn" hreflang="bn" data-title="হাইড্রোক্সাইড" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target">বাংলা</a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%93%D1%96%D0%B4%D1%80%D0%B0%D0%BA%D1%81%D1%96%D0%B4%D1%8B" title="Гідраксіды – Belarusian" lang="be" hreflang="be" data-title="Гідраксіды" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target">Беларуская</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%A5%D0%B8%D0%B4%D1%80%D0%BE%D0%BA%D1%81%D0%B8%D0%B4" title="Хидроксид – Bulgarian" lang="bg" hreflang="bg" data-title="Хидроксид" 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/Hidroksid" title="Hidroksid – Bosnian" lang="bs" hreflang="bs" data-title="Hidroksid" 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/Hidr%C3%B2xid" title="Hidròxid – Catalan" lang="ca" hreflang="ca" data-title="Hidròxid" 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/Hydroxidy" title="Hydroxidy – Czech" lang="cs" hreflang="cs" data-title="Hydroxidy" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target">Čeština</a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Hydroxid" title="Hydroxid – Danish" lang="da" hreflang="da" data-title="Hydroxid" 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/Hydroxide" title="Hydroxide – German" lang="de" hreflang="de" data-title="Hydroxide" 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/H%C3%BCdroksiidid" title="Hüdroksiidid – Estonian" lang="et" hreflang="et" data-title="Hüdroksiidid" 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%A5%CE%B4%CF%81%CE%BF%CE%BE%CE%B5%CE%AF%CE%B4%CE%B9%CE%BF" title="Υδροξείδιο – Greek" lang="el" hreflang="el" data-title="Υδροξείδιο" 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/Hidr%C3%B3xido" title="Hidróxido – Spanish" lang="es" hreflang="es" data-title="Hidróxido" 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/Hidroksido" title="Hidroksido – Esperanto" lang="eo" hreflang="eo" data-title="Hidroksido" 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/Hidroxido" title="Hidroxido – Basque" lang="eu" hreflang="eu" data-title="Hidroxido" 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/%D9%87%DB%8C%D8%AF%D8%B1%D9%88%DA%A9%D8%B3%DB%8C%D8%AF" title="هیدروکسید – Persian" lang="fa" hreflang="fa" data-title="هیدروکسید" 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/Hydroxyde" title="Hydroxyde – French" lang="fr" hreflang="fr" data-title="Hydroxyde" 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/Hiodrocsa%C3%ADd" title="Hiodrocsaíd – Irish" lang="ga" hreflang="ga" data-title="Hiodrocsaíd" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target">Gaeilge</a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Hidr%C3%B3xido" title="Hidróxido – Galician" lang="gl" hreflang="gl" data-title="Hidróxido" 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/%EC%88%98%EC%82%B0%ED%99%94%EB%AC%BC" title="수산화물 – Korean" lang="ko" hreflang="ko" data-title="수산화물" 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/%D5%80%D5%AB%D5%A4%D6%80%D6%85%D6%84%D5%BD%D5%AB%D5%A4%D5%B6%D5%A5%D6%80" title="Հիդրօքսիդներ – Armenian" lang="hy" hreflang="hy" data-title="Հիդրօքսիդներ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target">Հայերեն</a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Hidroksidi" title="Hidroksidi – Croatian" lang="hr" hreflang="hr" data-title="Hidroksidi" 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/Hidroksida" title="Hidroksida – Indonesian" lang="id" hreflang="id" data-title="Hidroksida" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target">Bahasa Indonesia</a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Idrossido" title="Idrossido – Italian" lang="it" hreflang="it" data-title="Idrossido" 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%94%D7%99%D7%93%D7%A8%D7%95%D7%A7%D7%A1%D7%99%D7%93" title="הידרוקסיד – Hebrew" lang="he" hreflang="he" data-title="הידרוקסיד" 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/Hidroksida" title="Hidroksida – Javanese" lang="jv" hreflang="jv" data-title="Hidroksida" data-language-autonym="Jawa" data-language-local-name="Javanese" class="interlanguage-link-target">Jawa</a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%B0%E1%83%98%E1%83%93%E1%83%A0%E1%83%9D%E1%83%A5%E1%83%A1%E1%83%98%E1%83%93%E1%83%98" title="ჰიდროქსიდი – Georgian" lang="ka" hreflang="ka" data-title="ჰიდროქსიდი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target">ქართული</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%93%D0%B8%D0%B4%D1%80%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D1%82%D0%B5%D1%80" title="Гидроксидтер – Kazakh" lang="kk" hreflang="kk" data-title="Гидроксидтер" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target">Қазақша</a></li><li class="interlanguage-link interwiki-la mw-list-item"><a href="https://la.wikipedia.org/wiki/Hydroxidum" title="Hydroxidum – Latin" lang="la" hreflang="la" data-title="Hydroxidum" 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/Hidroks%C4%ABdi" title="Hidroksīdi – Latvian" lang="lv" hreflang="lv" data-title="Hidroksīdi" 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/Hidroksidas" title="Hidroksidas – Lithuanian" lang="lt" hreflang="lt" data-title="Hidroksidas" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target">Lietuvių</a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%A5%D0%B8%D0%B4%D1%80%D0%BE%D0%BA%D1%81%D0%B8%D0%B4" title="Хидроксид – Macedonian" lang="mk" hreflang="mk" data-title="Хидроксид" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target">Македонски</a></li><li class="interlanguage-link interwiki-mg mw-list-item"><a href="https://mg.wikipedia.org/wiki/Hidr%C3%B4ksida" title="Hidrôksida – Malagasy" lang="mg" hreflang="mg" data-title="Hidrôksida" data-language-autonym="Malagasy" data-language-local-name="Malagasy" class="interlanguage-link-target">Malagasy</a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Hidroksida" title="Hidroksida – Malay" lang="ms" hreflang="ms" data-title="Hidroksida" 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/Hydroxide" title="Hydroxide – Dutch" lang="nl" hreflang="nl" data-title="Hydroxide" 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/%E6%B0%B4%E9%85%B8%E5%8C%96%E7%89%A9" title="水酸化物 – Japanese" lang="ja" hreflang="ja" data-title="水酸化物" 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/H%C3%BCdroksiid" title="Hüdroksiid – Northern Frisian" lang="frr" hreflang="frr" data-title="Hüdroksiid" 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/Hydroksid" title="Hydroksid – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Hydroksid" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target">Norsk bokmål</a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Gidroksidlar" title="Gidroksidlar – Uzbek" lang="uz" hreflang="uz" data-title="Gidroksidlar" 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/Wodorotlenki" title="Wodorotlenki – Polish" lang="pl" hreflang="pl" data-title="Wodorotlenki" 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/Hidr%C3%B3xido" title="Hidróxido – Portuguese" lang="pt" hreflang="pt" data-title="Hidróxido" 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/Hidroxid" title="Hidroxid – Romanian" lang="ro" hreflang="ro" data-title="Hidroxid" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target">Română</a></li><li class="interlanguage-link interwiki-qu mw-list-item"><a href="https://qu.wikipedia.org/wiki/Yakumuksi" title="Yakumuksi – Quechua" lang="qu" hreflang="qu" data-title="Yakumuksi" data-language-autonym="Runa Simi" data-language-local-name="Quechua" class="interlanguage-link-target">Runa Simi</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%93%D0%B8%D0%B4%D1%80%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D1%8B" title="Гидроксиды – Russian" lang="ru" hreflang="ru" data-title="Гидроксиды" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target">Русский</a></li><li class="interlanguage-link interwiki-sco mw-list-item"><a href="https://sco.wikipedia.org/wiki/Hydroxide" title="Hydroxide – Scots" lang="sco" hreflang="sco" data-title="Hydroxide" data-language-autonym="Scots" data-language-local-name="Scots" class="interlanguage-link-target">Scots</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Hydroxide" title="Hydroxide – Simple English" lang="en-simple" hreflang="en-simple" data-title="Hydroxide" data-language-autonym="Simple English" 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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>Hydroxide </caption> <tbody><tr> <td colspan="2" style="text-align:center; padding:2px;"><figure class="mw-halign-center skin-invert-image" typeof="mw:File"><a href="/wiki/File:Hydroxide_lone_pairs-2D.svg" class="mw-file-description"><img alt="Lewis structure of the hydroxide ion showing three lone pairs on the oxygen atom" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b0/Hydroxide_lone_pairs-2D.svg/250px-Hydroxide_lone_pairs-2D.svg.png" decoding="async" width="170" height="80" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b0/Hydroxide_lone_pairs-2D.svg/330px-Hydroxide_lone_pairs-2D.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b0/Hydroxide_lone_pairs-2D.svg/340px-Hydroxide_lone_pairs-2D.svg.png 2x" data-file-width="340" data-file-height="160" /></a><figcaption></figcaption></figure> </td></tr> <tr> <td colspan="2" class="borderless" style="text-align:center"> <table border="0" style="width:100%;display:inline-table;"> <tbody><tr> <td style="border-right:1px solid #aaa; width:50%;"><figure class="mw-halign-center bg-transparent" typeof="mw:File"><a href="/wiki/File:Hydroxide-3D-vdW.png" class="mw-file-description"><img alt="Space-filling representation of the hydroxide ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5a/Hydroxide-3D-vdW.png/120px-Hydroxide-3D-vdW.png" decoding="async" width="110" height="90" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5a/Hydroxide-3D-vdW.png/250px-Hydroxide-3D-vdW.png 1.5x" data-file-width="1100" data-file-height="904" /></a><figcaption></figcaption></figure> </td> <td style="width:50%;"><figure class="mw-halign-center bg-transparent" typeof="mw:File"><a href="/wiki/File:Hydroxide-3D-balls.png" class="mw-file-description"><img alt="Ball-and-stick model of the hydroxide ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/07/Hydroxide-3D-balls.png/110px-Hydroxide-3D-balls.png" decoding="async" width="110" height="67" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/07/Hydroxide-3D-balls.png/165px-Hydroxide-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/07/Hydroxide-3D-balls.png/220px-Hydroxide-3D-balls.png 2x" data-file-width="1100" data-file-height="673" /></a><figcaption></figcaption></figure> </td></tr></tbody></table> </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;">Hydroxide</div> </td></tr> <tr> <td colspan="2" style="text-align:left;"><a href="/wiki/Chemical_nomenclature#Systematic_name" title="Chemical nomenclature">Systematic IUPAC name</a> <div style="max-width:22em; word-wrap:break-word; padding-left:1.7em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0; max-width:22em;">Oxidanide (not recommended)</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><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 rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=14280-30-9">14280-30-9</a></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=%5BOH-%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=16234">CHEBI:16234</a></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.936.html">936</a></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/961">961</a></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/9159UV381P">9159UV381P</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/H2O/h1H2/p-1</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%;">[OH-]</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>OH− </td></tr> <tr> <td><a href="/wiki/Molar_mass" title="Molar mass">Molar mass</a> </td> <td>17.007 g·mol−1 </td></tr> <tr> <td><a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">Basicity</a> (pKb) </td> <td>0.0 <a href="#cite_note-1">[1]</a> </td></tr> <tr> <td><a href="/wiki/Conjugate_acid" class="mw-redirect" title="Conjugate acid">Conjugate acid</a> </td> <td><a href="/wiki/Properties_of_water" title="Properties of water">Water</a> </td></tr> <tr> <td><a href="/wiki/Conjugate_base" class="mw-redirect" title="Conjugate base">Conjugate base</a> </td> <td><a href="/wiki/Oxide_anion" class="mw-redirect" title="Oxide anion">Oxide anion</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;">Related compounds</div> </td> <td><a href="/wiki/Dioxidanylium" title="Dioxidanylium">O2H+</a> <a href="/wiki/Hydroxyl_radical" title="Hydroxyl radical">OH•</a> <a href="/wiki/Peroxide" title="Peroxide">O22−</a> <a href="/wiki/Water" title="Water">H2O</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> <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> Hydroxide is a <a href="/wiki/Polyatomic_ion" title="Polyatomic ion">diatomic anion</a> with <a href="/wiki/Chemical_formula" title="Chemical formula">chemical formula</a> OH−. It consists of an <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and <a href="/wiki/Hydrogen" title="Hydrogen">hydrogen</a> <a href="/wiki/Atom" title="Atom">atom</a> held together by a single <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bond</a>, and carries a negative <a href="/wiki/Electric_charge" title="Electric charge">electric charge</a>. It is an important but usually <a href="/wiki/Self-ionization_of_water" title="Self-ionization of water">minor constituent of water</a>. It functions as a <a href="/wiki/Base_(chemistry)" title="Base (chemistry)">base</a>, a <a href="/wiki/Ligand" title="Ligand">ligand</a>, a <a href="/wiki/Nucleophile" title="Nucleophile">nucleophile</a>, and a <a href="/wiki/Catalyst" class="mw-redirect" title="Catalyst">catalyst</a>. The hydroxide ion forms <a href="/wiki/Salt_(chemistry)" title="Salt (chemistry)">salts</a>, some of which <a href="/wiki/Dissociation_(chemistry)" title="Dissociation (chemistry)">dissociate</a> in aqueous solution, liberating solvated hydroxide ions. <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">Sodium hydroxide</a> is a multi-million-ton per annum <a href="/wiki/Commodity_chemicals" title="Commodity chemicals">commodity chemical</a>. The corresponding <a href="/wiki/Electrically_neutral" class="mw-redirect" title="Electrically neutral">electrically neutral</a> compound HO• is the <a href="/wiki/Hydroxyl_radical" title="Hydroxyl radical">hydroxyl radical</a>. The corresponding <a href="/wiki/Covalent_bond" title="Covalent bond">covalently</a> bound <a href="/wiki/Functional_group" title="Functional group">group</a> <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>−OH of atoms is the <a href="/wiki/Hydroxy_group" title="Hydroxy group">hydroxy group</a>. Both the hydroxide ion and hydroxy group are <a href="/wiki/Nucleophile" title="Nucleophile">nucleophiles</a> and can act as catalysts in <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>. Many <a href="/wiki/Inorganic" class="mw-redirect" title="Inorganic">inorganic</a> substances which bear the word hydroxide in their names are not <a href="/wiki/Ionic_compound" class="mw-redirect" title="Ionic compound">ionic compounds</a> of the hydroxide ion, but covalent compounds which contain <a href="/wiki/Hydroxy_group" title="Hydroxy group">hydroxy groups</a>. <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Hydroxide_ion">Hydroxide ion</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=1" title="Edit section: Hydroxide ion">edit</a>]</div> The hydroxide ion is naturally produced from <a href="/wiki/Water" title="Water">water</a> by the <a href="/wiki/Self-ionization_of_water" title="Self-ionization of water">self-ionization</a> reaction:<a href="#cite_note-2">[2]</a> <dl><dd><a href="/wiki/Hydronium" title="Hydronium">H3O+</a> + OH− ⇌ 2H2O</dd></dl> The <a href="/wiki/Equilibrium_constant" title="Equilibrium constant">equilibrium constant</a> for this reaction, defined as <dl><dd>Kw = [H+][OH−]<a href="#cite_note-3">[note 1]</a></dd></dl> has a value close to 10−14 at 25 °C, so the <a href="/wiki/Concentration" title="Concentration">concentration</a> of hydroxide ions in pure water is close to 10−7 mol∙dm−3, to satisfy the equal charge constraint. The <a href="/wiki/PH" title="PH">pH</a> of a solution is equal to the decimal <a href="/wiki/Cologarithm" class="mw-redirect" title="Cologarithm">cologarithm</a> of the <a href="/wiki/Hydron_(chemistry)" title="Hydron (chemistry)">hydrogen cation</a> concentration;<a href="#cite_note-4">[note 2]</a> the pH of pure water is close to 7 at ambient temperatures. The concentration of hydroxide ions can be expressed in terms of <a href="/wiki/PH#pOH" title="PH">pOH</a>, which is close to (14 − pH),<a href="#cite_note-5">[note 3]</a> so the pOH of pure water is also close to 7. Addition of a base to water will reduce the hydrogen cation concentration and therefore increase the hydroxide ion concentration (decrease pH, increase pOH) even if the base does not itself contain hydroxide. For example, <a href="/wiki/Ammonia" title="Ammonia">ammonia</a> solutions have a pH greater than 7 due to the reaction NH3 + H+ ⇌ NH+ 4, which decreases the hydrogen cation concentration, which increases the hydroxide ion concentration. pOH can be kept at a nearly constant value with various <a href="/wiki/Buffer_solution" title="Buffer solution">buffer solutions</a>. <figure typeof="mw:File/Thumb"><a href="/wiki/File:Bihydoxide.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/81/Bihydoxide.png/150px-Bihydoxide.png" decoding="async" width="150" height="187" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/8/81/Bihydoxide.png 1.5x" data-file-width="176" data-file-height="219" /></a><figcaption>Schematic representation of the bihydroxide ion<a href="#cite_note-ARF-6">[3]</a></figcaption></figure> In an <a href="/wiki/Aqueous_solution" title="Aqueous solution">aqueous solution</a><a href="#cite_note-7">[4]</a> the hydroxide ion is a <a href="/wiki/Base_(chemistry)" title="Base (chemistry)">base</a> in the <a href="/wiki/Br%C3%B8nsted%E2%80%93Lowry_acid%E2%80%93base_theory" title="Brønsted–Lowry acid–base theory">Brønsted–Lowry</a> sense as it can accept a proton<a href="#cite_note-8">[note 4]</a> from a Brønsted–Lowry acid to form a water molecule. It can also act as a <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis base</a> by donating a pair of electrons to a Lewis acid. In aqueous solution both hydrogen ions and hydroxide ions are strongly solvated, with <a href="/wiki/Hydrogen_bond" title="Hydrogen bond">hydrogen bonds</a> between oxygen and hydrogen atoms. Indeed, the bihydroxide ion H 3O− 2 has been characterized in the solid state. This compound is centrosymmetric and has a very short hydrogen bond (114.5 <a href="/wiki/Picometre" title="Picometre">pm</a>) that is similar to the length in the <a href="/wiki/Bifluoride" title="Bifluoride">bifluoride</a> ion HF− 2 (114 pm).<a href="#cite_note-ARF-6">[3]</a> In aqueous solution the hydroxide ion forms strong hydrogen bonds with water molecules. A consequence of this is that concentrated solutions of sodium hydroxide have high <a href="/wiki/Viscosity" title="Viscosity">viscosity</a> due to the formation of an extended network of hydrogen bonds as in <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a> solutions. In solution, exposed to air, the hydroxide ion reacts rapidly with atmospheric <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a>, which acts as a lewis acid, to form, initially, the <a href="/wiki/Bicarbonate" title="Bicarbonate">bicarbonate</a> ion. <dl><dd>OH− + CO2 ⇌ HCO− 3</dd></dl> The <a href="/wiki/Equilibrium_constant" title="Equilibrium constant">equilibrium constant</a> for this reaction can be specified either as a reaction with dissolved carbon dioxide or as a reaction with carbon dioxide gas (see <a href="/wiki/Carbonic_acid" title="Carbonic acid">Carbonic acid</a> for values and details). At neutral or acid pH, the reaction is slow, but is catalyzed by the <a href="/wiki/Enzyme" title="Enzyme">enzyme</a> <a href="/wiki/Carbonic_anhydrase" title="Carbonic anhydrase">carbonic anhydrase</a>, which effectively creates hydroxide ions at the active site. Solutions containing the hydroxide ion attack <a href="/wiki/Glass" title="Glass">glass</a>. In this case, the <a href="/wiki/Silicate" title="Silicate">silicates</a> in glass are acting as acids. Basic hydroxides, whether solids or in solution, are stored in <a href="/wiki/Airtight" class="mw-redirect" title="Airtight">airtight</a> plastic containers. The hydroxide ion can function as a typical electron-pair donor <a href="/wiki/Ligand" title="Ligand">ligand</a>, forming such complexes as tetrahydroxoaluminate/tetrahydroxido<a href="/wiki/Aluminate" title="Aluminate">aluminate</a> [Al(OH)4]−. It is also often found in mixed-ligand complexes of the type [MLx(OH)y]z+, where L is a ligand. The hydroxide ion often serves as a <a href="/wiki/Bridging_ligand" title="Bridging ligand">bridging ligand</a>, donating one pair of electrons to each of the atoms being bridged. As illustrated by [Pb2(OH)]3+, metal hydroxides are often written in a simplified format. It can even act as a 3-electron-pair donor, as in the tetramer [PtMe3(OH)]4.<a href="#cite_note-9">[5]</a> When bound to a strongly electron-withdrawing metal centre, hydroxide ligands tend to <a href="/wiki/Dissociation_(chemistry)" title="Dissociation (chemistry)">ionise</a> into oxide ligands. For example, the bichromate ion [HCrO4]− dissociates according to <dl><dd>[O3CrO–H]− ⇌ [CrO4]2− + H+</dd></dl> with a pKa of about 5.9.<a href="#cite_note-scdb-10">[6]</a> <div class="mw-heading mw-heading3"><h3 id="Vibrational_spectra">Vibrational spectra</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=2" title="Edit section: Vibrational spectra">edit</a>]</div> The <a href="/wiki/Infrared_spectrum" class="mw-redirect" title="Infrared spectrum">infrared spectra</a> of compounds containing the OH <a href="/wiki/Functional_group" title="Functional group">functional group</a> have strong <a href="/wiki/Spectral_line" title="Spectral line">absorption bands</a> in the region centered around 3500 cm−1.<a href="#cite_note-nakamoto-11">[7]</a> The high frequency of <a href="/wiki/Molecular_vibration" title="Molecular vibration">molecular vibration</a> is a consequence of the small mass of the hydrogen atom as compared to the mass of the oxygen atom, and this makes detection of hydroxyl groups by <a href="/wiki/Infrared_spectroscopy" title="Infrared spectroscopy">infrared spectroscopy</a> relatively easy. A band due to an OH group tends to be sharp. However, the <a href="/wiki/Spectral_linewidth" class="mw-redirect" title="Spectral linewidth">band width</a> increases when the OH group is involved in hydrogen bonding. A water molecule has an HOH bending mode at about 1600 cm−1, so the absence of this band can be used to distinguish an OH group from a water molecule. When the OH group is bound to a metal ion in a <a href="/wiki/Coordination_complex" title="Coordination complex">coordination complex</a>, an M−OH bending mode can be observed. For example, in [Sn(OH)6]2− it occurs at 1065 cm−1. The bending mode for a bridging hydroxide tends to be at a lower frequency as in [(<a href="/wiki/Bipyridine" title="Bipyridine">bipyridine</a>)Cu(OH)2Cu(<a href="/wiki/Bipyridine" title="Bipyridine">bipyridine</a>)]2+ (955 cm−1).<a href="#cite_note-12">[8]</a> M−OH stretching vibrations occur below about 600 cm−1. For example, the <a href="/wiki/Tetrahedron" title="Tetrahedron">tetrahedral</a> ion [Zn(OH)4]2− has bands at 470 cm−1 (<a href="/wiki/Raman_spectroscopy" title="Raman spectroscopy">Raman</a>-active, polarized) and 420 cm−1 (infrared). The same ion has a (HO)–Zn–(OH) bending vibration at 300 cm−1.<a href="#cite_note-13">[9]</a> <div class="mw-heading mw-heading2"><h2 id="Applications">Applications</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=3" title="Edit section: Applications">edit</a>]</div> <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">Sodium hydroxide</a> solutions, also known as <a href="/wiki/Lye" title="Lye">lye</a> and caustic soda, are used in the manufacture of <a href="/wiki/Wood_pulp" class="mw-redirect" title="Wood pulp">pulp</a> and <a href="/wiki/Paper" title="Paper">paper</a>, <a href="/wiki/Textile" title="Textile">textiles</a>, <a href="/wiki/Drinking_water" title="Drinking water">drinking water</a>, <a href="/wiki/Soap" title="Soap">soaps</a> and <a href="/wiki/Detergent" title="Detergent">detergents</a>, and as a <a href="/wiki/Drain_cleaner" title="Drain cleaner">drain cleaner</a>. Worldwide production in 2004 was approximately 60 million <a href="/wiki/Tonne" title="Tonne">tonnes</a>.<a href="#cite_note-Ullmann-14">[10]</a> The principal method of manufacture is the <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a>. Solutions containing the hydroxide ion are generated when a salt of a <a href="/wiki/Weak_acid" class="mw-redirect" title="Weak acid">weak acid</a> is dissolved in water. <a href="/wiki/Sodium_carbonate" title="Sodium carbonate">Sodium carbonate</a> is used as an alkali, for example, by virtue of the <a href="/wiki/Hydrolysis" title="Hydrolysis">hydrolysis</a> reaction <dl><dd>CO2− 3 + H2O ⇌ HCO− 3 + OH−       (<a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">pKa2</a> = 10.33 at 25 °C and zero <a href="/wiki/Ionic_strength" title="Ionic strength">ionic strength</a>)</dd></dl> An example of the use of sodium carbonate as an alkali is when <a href="/wiki/Washing_soda" class="mw-redirect" title="Washing soda">washing soda</a> (another name for sodium carbonate) acts on insoluble <a href="/wiki/Ester" title="Ester">esters</a>, such as <a href="/wiki/Triglyceride" title="Triglyceride">triglycerides</a>, commonly known as fats, to hydrolyze them and make them soluble. <a href="/wiki/Bauxite" title="Bauxite">Bauxite</a>, a basic hydroxide of <a href="/wiki/Aluminium" title="Aluminium">aluminium</a>, is the principal ore from which the metal is manufactured.<a href="#cite_note-15">[11]</a> Similarly, <a href="/wiki/Goethite" title="Goethite">goethite</a> (α-FeO(OH)) and <a href="/wiki/Lepidocrocite" title="Lepidocrocite">lepidocrocite</a> (γ-FeO(OH)), basic hydroxides of <a href="/wiki/Iron" title="Iron">iron</a>, are among the principal ores used for the manufacture of metallic iron.<a href="#cite_note-16">[12]</a> <div class="mw-heading mw-heading2"><h2 id="Inorganic_hydroxides">Inorganic hydroxides</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=4" title="Edit section: Inorganic hydroxides">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Alkali_metals">Alkali metals</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=5" title="Edit section: Alkali metals">edit</a>]</div> Aside from NaOH and KOH, which enjoy very large scale applications, the hydroxides of the other alkali metals also are useful. <a href="/wiki/Lithium_hydroxide" title="Lithium hydroxide">Lithium hydroxide</a> (LiOH) is used in <a href="/wiki/Breathing_gas" title="Breathing gas">breathing gas</a> purification systems for <a href="/wiki/Spacecraft" title="Spacecraft">spacecraft</a>, <a href="/wiki/Submarine" title="Submarine">submarines</a>, and <a href="/wiki/Rebreather" title="Rebreather">rebreathers</a> to remove <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> from exhaled gas.<a href="#cite_note-17">[13]</a> <dl><dd>2 LiOH + CO2 → Li2CO3 + H2O</dd></dl> The hydroxide of lithium is preferred to that of sodium because of its lower mass. <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">Sodium hydroxide</a>, <a href="/wiki/Potassium_hydroxide" title="Potassium hydroxide">potassium hydroxide</a>, and the hydroxides of the other <a href="/wiki/Alkali_metal" title="Alkali metal">alkali metals</a> are also <a href="/wiki/Strong_base" class="mw-redirect" title="Strong base">strong bases</a>.<a href="#cite_note-18">[14]</a> <div class="mw-heading mw-heading3"><h3 id="Alkaline_earth_metals">Alkaline earth metals</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=6" title="Edit section: Alkaline earth metals">edit</a>]</div> <figure class="mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Beryllium_trimer.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Beryllium_trimer.svg/130px-Beryllium_trimer.svg.png" decoding="async" width="130" height="144" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Beryllium_trimer.svg/195px-Beryllium_trimer.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Beryllium_trimer.svg/260px-Beryllium_trimer.svg.png 2x" data-file-width="91" data-file-height="101" /></a><figcaption>Trimeric hydrolysis product of beryllium dication<a href="#cite_note-19">[note 5]</a></figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:BeHydrolysis.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1f/BeHydrolysis.png/250px-BeHydrolysis.png" decoding="async" width="220" height="218" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/1/1f/BeHydrolysis.png 1.5x" data-file-width="282" data-file-height="280" /></a><figcaption>Beryllium hydrolysis as a function of pH. Water molecules attached to Be are omitted.</figcaption></figure> <a href="/wiki/Beryllium_hydroxide" title="Beryllium hydroxide">Beryllium hydroxide</a> Be(OH)2 is <a href="/wiki/Amphoteric" class="mw-redirect" title="Amphoteric">amphoteric</a>.<a href="#cite_note-amph-20">[15]</a> The hydroxide itself is <a href="/wiki/Insoluble" class="mw-redirect" title="Insoluble">insoluble</a> in water, with a <a href="/wiki/Solubility_product" class="mw-redirect" title="Solubility product">solubility product</a> log K*sp of −11.7. Addition of acid gives soluble <a href="/wiki/Hydrolysis" title="Hydrolysis">hydrolysis</a> products, including the trimeric ion [Be3(OH)3(H2O)6]3+, which has OH groups bridging between pairs of beryllium ions making a 6-membered ring.<a href="#cite_note-21">[16]</a> At very low pH the <a href="/wiki/Metal_ions_in_aqueous_solution" title="Metal ions in aqueous solution">aqua ion</a> [Be(H2O)4]2+ is formed. Addition of hydroxide to Be(OH)2 gives the soluble tetrahydroxoberyllate or tetrahydroxido<a href="/wiki/Beryllate" title="Beryllate">beryllate</a> anion, [Be(OH)4]2−. The solubility in water of the other hydroxides in this group increases with increasing <a href="/wiki/Atomic_number" title="Atomic number">atomic number</a>.<a href="#cite_note-22">[17]</a> <a href="/wiki/Magnesium_hydroxide" title="Magnesium hydroxide">Magnesium hydroxide</a> Mg(OH)2 is a strong base (up to the limit of its solubility, which is very low in pure water), as are the hydroxides of the heavier alkaline earths: <a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">calcium hydroxide</a>, <a href="/wiki/Strontium_hydroxide" title="Strontium hydroxide">strontium hydroxide</a>, and <a href="/wiki/Barium_hydroxide" title="Barium hydroxide">barium hydroxide</a>. A solution or suspension of calcium hydroxide is known as <a href="/wiki/Limewater" class="mw-redirect" title="Limewater">limewater</a> and can be used to test for the <a href="/wiki/Weak_acid" class="mw-redirect" title="Weak acid">weak acid</a> carbon dioxide. The reaction Ca(OH)2 + CO2 ⇌ Ca2+ + HCO− 3 + OH− illustrates the basicity of calcium hydroxide. <a href="/wiki/Soda_lime" title="Soda lime">Soda lime</a>, which is a mixture of the strong bases NaOH and KOH with Ca(OH)2, is used as a CO2 absorbent. <div class="mw-heading mw-heading3"><h3 id="Boron_group_elements">Boron group elements</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=7" title="Edit section: Boron group elements">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:AlHydrolysis.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/83/AlHydrolysis.png/220px-AlHydrolysis.png" decoding="async" width="220" height="222" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/8/83/AlHydrolysis.png 1.5x" data-file-width="278" data-file-height="281" /></a><figcaption>Aluminium hydrolysis as a function of pH. Water molecules attached to Al are omitted</figcaption></figure> The simplest hydroxide of boron B(OH)3, known as <a href="/wiki/Boric_acid" title="Boric acid">boric acid</a>, is an acid. Unlike the hydroxides of the alkali and alkaline earth hydroxides, it does not dissociate in aqueous solution. Instead, it reacts with water molecules acting as a Lewis acid, releasing protons. <dl><dd>B(OH)3 + H2O ⇌ <a href="/wiki/Tetrahydroxyborate" title="Tetrahydroxyborate">B(OH)− 4</a> + H+</dd></dl> A variety of <a href="/wiki/Oxyanion" title="Oxyanion">oxyanions</a> of boron are known, which, in the protonated form, contain hydroxide groups.<a href="#cite_note-23">[18]</a> <figure class="mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Tetrahydroxoaluminate_ion.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/9d/Tetrahydroxoaluminate_ion.svg/120px-Tetrahydroxoaluminate_ion.svg.png" decoding="async" width="100" height="68" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/9d/Tetrahydroxoaluminate_ion.svg/150px-Tetrahydroxoaluminate_ion.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/9d/Tetrahydroxoaluminate_ion.svg/200px-Tetrahydroxoaluminate_ion.svg.png 2x" data-file-width="205" data-file-height="140" /></a><figcaption>Tetrahydroxo- aluminate(III) ion</figcaption></figure> <a href="/wiki/Aluminium_hydroxide" title="Aluminium hydroxide">Aluminium hydroxide</a> Al(OH)3 is amphoteric and dissolves in alkaline solution.<a href="#cite_note-amph-20">[15]</a> <dl><dd>Al(OH)3 (solid) + OH− (aq) ⇌ <a href="/wiki/Aluminate" title="Aluminate">Al(OH)− 4</a> (aq)</dd></dl> In the <a href="/wiki/Bayer_process" title="Bayer process">Bayer process</a><a href="#cite_note-24">[19]</a> for the production of pure aluminium oxide from <a href="/wiki/Bauxite" title="Bauxite">bauxite</a> minerals this equilibrium is manipulated by careful control of temperature and alkali concentration. In the first phase, aluminium dissolves in hot alkaline solution as Al(OH)− 4, but other hydroxides usually present in the mineral, such as iron hydroxides, do not dissolve because they are not amphoteric. After removal of the insolubles, the so-called <a href="/wiki/Red_mud" title="Red mud">red mud</a>, pure aluminium hydroxide is made to precipitate by reducing the temperature and adding water to the extract, which, by diluting the alkali, lowers the pH of the solution. Basic aluminium hydroxide AlO(OH), which may be present in bauxite, is also amphoteric. In mildly acidic solutions, the hydroxo/hydroxido complexes formed by aluminium are somewhat different from those of boron, reflecting the greater size of Al(III) vs. B(III). The concentration of the species [Al13(OH)32]7+ is very dependent on the total aluminium concentration. Various other hydroxo complexes are found in crystalline compounds. Perhaps the most important is the basic hydroxide AlO(OH), a polymeric material known by the names of the mineral forms <a href="/wiki/Boehmite" title="Boehmite">boehmite</a> or <a href="/wiki/Diaspore" title="Diaspore">diaspore</a>, depending on crystal structure. <a href="/wiki/Gallium_hydroxide" class="mw-redirect" title="Gallium hydroxide">Gallium hydroxide</a>,<a href="#cite_note-amph-20">[15]</a> <a href="/wiki/Indium_hydroxide" class="mw-redirect" title="Indium hydroxide">indium hydroxide</a>, and <a href="/wiki/Thallium(III)_hydroxide" title="Thallium(III) hydroxide">thallium(III) hydroxide</a> are also amphoteric. <a href="/wiki/Thallium(I)_hydroxide" title="Thallium(I) hydroxide">Thallium(I) hydroxide</a> is a strong base.<a href="#cite_note-25">[20]</a> <div class="mw-heading mw-heading3"><h3 id="Carbon_group_elements">Carbon group elements</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=8" title="Edit section: Carbon group elements">edit</a>]</div> Carbon forms no simple hydroxides. The <a href="/wiki/Hypothetical_compound" class="mw-redirect" title="Hypothetical compound">hypothetical compound</a> C(OH)4 (<a href="/wiki/Orthocarbonic_acid" title="Orthocarbonic acid">orthocarbonic acid</a> or methanetetrol) is unstable in aqueous solution:<a href="#cite_note-26">[21]</a> <dl><dd>C(OH)4 → HCO− 3 + H3O+</dd> <dd>HCO− 3 + H+ ⇌ H2CO3</dd></dl> <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">Carbon dioxide</a> is also known as carbonic anhydride, meaning that it forms by dehydration of <a href="/wiki/Carbonic_acid" title="Carbonic acid">carbonic acid</a> H2CO3 (OC(OH)2).<a href="#cite_note-27">[22]</a> <a href="/wiki/Silicic_acid" title="Silicic acid">Silicic acid</a> is the name given to a variety of compounds with a generic formula [SiOx(OH)4−2x]n.<a href="#cite_note-28">[23]</a><a href="#cite_note-29">[24]</a> Orthosilicic acid has been identified in very dilute aqueous solution. It is a weak acid with pKa1 = 9.84, pKa2 = 13.2 at 25 °C. It is usually written as H4SiO4, but the formula Si(OH)4 is generally accepted.<a href="#cite_note-scdb-10">[6]</a>[<a href="/wiki/Wikipedia:Accuracy_dispute#Disputed_statement" title="Wikipedia:Accuracy dispute">dubious</a> – <a href="/wiki/Talk:Hydroxide#discuss" title="Talk:Hydroxide">discuss</a>] Other silicic acids such as metasilicic acid (H2SiO3), disilicic acid (H2Si2O5), and pyrosilicic acid (H6Si2O7) have been characterized. These acids also have hydroxide groups attached to the silicon; the formulas suggest that these acids are protonated forms of poly<a href="/wiki/Oxyanion" title="Oxyanion">oxyanions</a>. Few hydroxo complexes of <a href="/wiki/Germanium" title="Germanium">germanium</a> have been characterized. <a href="/wiki/Tin(II)_hydroxide" title="Tin(II) hydroxide">Tin(II) hydroxide</a> Sn(OH)2 was prepared in anhydrous media. When <a href="/wiki/Tin(II)_oxide" title="Tin(II) oxide">tin(II) oxide</a> is treated with alkali the pyramidal hydroxo complex Sn(OH)− 3 is formed. When solutions containing this ion are acidified, the ion [Sn3(OH)4]2+ is formed together with some basic hydroxo complexes. The structure of [Sn3(OH)4]2+ has a triangle of tin atoms connected by bridging hydroxide groups.<a href="#cite_note-30">[25]</a> Tin(IV) hydroxide is unknown but can be regarded as the hypothetical acid from which <a href="/wiki/Stannate" title="Stannate">stannates</a>, with a formula [Sn(OH)6]2−, are derived by reaction with the (Lewis) basic hydroxide ion.<a href="#cite_note-31">[26]</a> Hydrolysis of Pb2+ in aqueous solution is accompanied by the formation of various hydroxo-containing complexes, some of which are insoluble. The basic hydroxo complex [Pb6O(OH)6]4+ is a cluster of six lead centres with metal–metal bonds surrounding a central oxide ion. The six hydroxide groups lie on the faces of the two external Pb4 tetrahedra. In strongly alkaline solutions soluble <a href="/wiki/Plumbate" title="Plumbate">plumbate</a> ions are formed, including [Pb(OH)6]2−.<a href="#cite_note-32">[27]</a> <div class="mw-heading mw-heading3"><h3 id="Other_main-group_elements">Other main-group elements</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=9" title="Edit section: Other main-group elements">edit</a>]</div> <table class="wikitable" style="text-align:center"> <tbody><tr> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Phosphonic-acid-2D-dimensions-vector.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e3/Phosphonic-acid-2D-dimensions-vector.svg/250px-Phosphonic-acid-2D-dimensions-vector.svg.png" decoding="async" width="150" height="131" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e3/Phosphonic-acid-2D-dimensions-vector.svg/330px-Phosphonic-acid-2D-dimensions-vector.svg.png 2x" data-file-width="1100" data-file-height="959" /></a><figcaption></figcaption></figure> </td> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Phosphoric-acid-2D-dimensions.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/98/Phosphoric-acid-2D-dimensions.svg/250px-Phosphoric-acid-2D-dimensions.svg.png" decoding="async" width="180" height="125" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/98/Phosphoric-acid-2D-dimensions.svg/330px-Phosphoric-acid-2D-dimensions.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/98/Phosphoric-acid-2D-dimensions.svg/500px-Phosphoric-acid-2D-dimensions.svg.png 2x" data-file-width="1100" data-file-height="765" /></a><figcaption></figcaption></figure> </td> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Sulfuric-acid-2D-dimensions.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/8b/Sulfuric-acid-2D-dimensions.svg/180px-Sulfuric-acid-2D-dimensions.svg.png" decoding="async" width="180" height="120" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/8b/Sulfuric-acid-2D-dimensions.svg/270px-Sulfuric-acid-2D-dimensions.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/8b/Sulfuric-acid-2D-dimensions.svg/360px-Sulfuric-acid-2D-dimensions.svg.png 2x" data-file-width="228" data-file-height="152" /></a><figcaption></figcaption></figure> </td> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Telluric_acid.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fc/Telluric_acid.svg/250px-Telluric_acid.svg.png" decoding="async" width="150" height="114" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fc/Telluric_acid.svg/330px-Telluric_acid.svg.png 2x" data-file-width="620" data-file-height="471" /></a><figcaption></figcaption></figure> </td> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Ortho-Periods%C3%A4ure.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Ortho-Periods%C3%A4ure.svg/150px-Ortho-Periods%C3%A4ure.svg.png" decoding="async" width="150" height="123" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Ortho-Periods%C3%A4ure.svg/225px-Ortho-Periods%C3%A4ure.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/96/Ortho-Periods%C3%A4ure.svg/300px-Ortho-Periods%C3%A4ure.svg.png 2x" data-file-width="118" data-file-height="97" /></a><figcaption></figcaption></figure> </td> <td><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Xenic_acid.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/66/Xenic_acid.png/150px-Xenic_acid.png" decoding="async" width="150" height="110" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/66/Xenic_acid.png/225px-Xenic_acid.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/66/Xenic_acid.png/300px-Xenic_acid.png 2x" data-file-width="2000" data-file-height="1467" /></a><figcaption></figcaption></figure> </td></tr> <tr> <td><a href="/wiki/Phosphorous_acid" title="Phosphorous acid">Phosphorous acid</a> </td> <td><a href="/wiki/Phosphoric_acid" title="Phosphoric acid">Phosphoric acid</a> </td> <td><a href="/wiki/Sulfuric_acid" title="Sulfuric acid">Sulfuric acid</a> </td> <td><a href="/wiki/Telluric_acid" title="Telluric acid">Telluric acid</a> </td> <td><a href="/wiki/Orthoperiodic_acid" class="mw-redirect" title="Orthoperiodic acid">Orthoperiodic acid</a> </td> <td><a href="/wiki/Xenic_acid" title="Xenic acid">Xenic acid</a> </td></tr></tbody></table> In the higher oxidation states of the <a href="/wiki/Pnictogen" title="Pnictogen">pnictogens</a>, <a href="/wiki/Chalcogen" title="Chalcogen">chalcogens</a>, <a href="/wiki/Halogen" title="Halogen">halogens</a>, and <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a> there are oxoacids in which the central atom is attached to oxide ions and hydroxide ions. Examples include <a href="/wiki/Phosphoric_acid" title="Phosphoric acid">phosphoric acid</a> H3PO4, and <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> H2SO4. In these compounds one or more hydroxide groups can <a href="/wiki/Dissociation_(chemistry)" title="Dissociation (chemistry)">dissociate</a> with the liberation of hydrogen cations as in a standard <a href="/wiki/Br%C3%B8nsted%E2%80%93Lowry_acid%E2%80%93base_theory" title="Brønsted–Lowry acid–base theory">Brønsted–Lowry</a> acid. Many oxoacids of sulfur are known and all feature OH groups that can dissociate.<a href="#cite_note-33">[28]</a> <a href="/wiki/Telluric_acid" title="Telluric acid">Telluric acid</a> is often written with the formula H2TeO4·2H2O but is better described structurally as Te(OH)6.<a href="#cite_note-34">[29]</a> Orthoperiodic acid<a href="#cite_note-35">[note 6]</a> can lose all its protons, eventually forming the periodate ion [IO4]−. It can also be protonated in strongly acidic conditions to give the octahedral ion [I(OH)6]+, completing the <a href="/wiki/Isoelectronic" class="mw-redirect" title="Isoelectronic">isoelectronic</a> series, [E(OH)6]z, E = Sn, Sb, Te, I; z = −2, −1, 0, +1. Other acids of iodine(VII) that contain hydroxide groups are known, in particular in salts such as the mesoperiodate ion that occurs in K4[I2O8(OH)2]·8H2O.<a href="#cite_note-36">[30]</a> As is common outside of the alkali metals, hydroxides of the elements in lower oxidation states are complicated. For example, <a href="/wiki/Phosphorous_acid" title="Phosphorous acid">phosphorous acid</a> H3PO3 predominantly has the structure OP(H)(OH)2, in equilibrium with a small amount of P(OH)3.<a href="#cite_note-37">[31]</a><a href="#cite_note-38">[32]</a> The oxoacids of <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>, <a href="/wiki/Bromine" title="Bromine">bromine</a>, and <a href="/wiki/Iodine" title="Iodine">iodine</a> have the formula O<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>⁠n−1/2⁠A(OH), where n is the <a href="/wiki/Oxidation_number" class="mw-redirect" title="Oxidation number">oxidation number</a>: +1, +3, +5, or +7, and A = Cl, Br, or I. The only oxoacid of <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> is F(OH), <a href="/wiki/Hypofluorous_acid" title="Hypofluorous acid">hypofluorous acid</a>. When these acids are neutralized the hydrogen atom is removed from the hydroxide group.<a href="#cite_note-39">[33]</a> <div class="mw-heading mw-heading3"><h3 id="Transition_and_post-transition_metals">Transition and post-transition metals</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=10" title="Edit section: Transition and post-transition metals">edit</a>]</div> The hydroxides of the <a href="/wiki/Transition_metal" title="Transition metal">transition metals</a> and <a href="/wiki/Post-transition_metal" title="Post-transition metal">post-transition metals</a> usually have the metal in the +2 (M = Mn, Fe, Co, Ni, Cu, Zn) or +3 (M = Fe, Ru, Rh, Ir) oxidation state. None are soluble in water, and many are poorly defined. One complicating feature of the hydroxides is their tendency to undergo further condensation to the oxides, a process called <a href="/wiki/Olation" title="Olation">olation</a>. Hydroxides of metals in the +1 oxidation state are also poorly defined or unstable. For example, <a href="/wiki/Silver_hydroxide" class="mw-redirect" title="Silver hydroxide">silver hydroxide</a> Ag(OH) decomposes spontaneously to the oxide (Ag2O). Copper(I) and gold(I) hydroxides are also unstable, although stable adducts of CuOH and AuOH are known.<a href="#cite_note-40">[34]</a> The polymeric compounds M(OH)2 and M(OH)3 are in general prepared by increasing the pH of an aqueous solution of the corresponding metal cation until the hydroxide <a href="/wiki/Precipitate" class="mw-redirect" title="Precipitate">precipitates</a> out of solution. On the converse, the hydroxides dissolve in acidic solution. <a href="/wiki/Zinc_hydroxide" title="Zinc hydroxide">Zinc hydroxide</a> Zn(OH)2 is amphoteric, forming the tetrahydroxido<a href="/wiki/Zincate" title="Zincate">zincate</a> ion Zn(OH)2− 4 in strongly alkaline solution.<a href="#cite_note-amph-20">[15]</a> Numerous mixed ligand complexes of these metals with the hydroxide ion exist. In fact, these are in general better defined than the simpler derivatives. Many can be made by deprotonation of the corresponding <a href="/wiki/Metal_aquo_complex" title="Metal aquo complex">metal aquo complex</a>. <dl><dd>LnM(OH2) + B ⇌ LnM(OH)– + BH+ (L = ligand, B = base)</dd></dl> <a href="/wiki/Vanadic_acid" class="mw-redirect" title="Vanadic acid">Vanadic acid</a> H3VO4 <a href="/wiki/Acid_dissociation_constant#Polyprotic_acids" title="Acid dissociation constant">shows similarities</a> with phosphoric acid H3PO4 though it has a much more complex <a href="/wiki/Vanadate" title="Vanadate">vanadate</a> oxoanion chemistry. <a href="/wiki/Chromic_acid" title="Chromic acid">Chromic acid</a> H2CrO4, has similarities with sulfuric acid H2SO4; for example, both form <a href="/wiki/Acid_salt" title="Acid salt">acid salts</a> A+[HMO4]−. Some metals, e.g. V, Cr, Nb, Ta, Mo, W, tend to exist in high oxidation states. Rather than forming hydroxides in aqueous solution, they convert to oxo clusters by the process of <a href="/wiki/Olation" title="Olation">olation</a>, forming <a href="/wiki/Polyoxometalate" title="Polyoxometalate">polyoxometalates</a>.<a href="#cite_note-41">[35]</a> <div class="mw-heading mw-heading2"><h2 id="Basic_salts_containing_hydroxide">Basic salts containing hydroxide</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=11" title="Edit section: Basic salts containing hydroxide">edit</a>]</div> In some cases, the products of partial hydrolysis of metal ion, described above, can be found in crystalline compounds. A striking example is found with <a href="/wiki/Zirconium" title="Zirconium">zirconium</a>(IV). Because of the high oxidation state, salts of Zr4+ are extensively hydrolyzed in water even at low pH. The compound originally formulated as ZrOCl2·8H2O was found to be the chloride salt of a <a href="/wiki/Tetrameric" class="mw-redirect" title="Tetrameric">tetrameric</a> cation [Zr4(OH)8(H2O)16]8+ in which there is a square of Zr4+ ions with two hydroxide groups bridging between Zr atoms on each side of the square and with four water molecules attached to each Zr atom.<a href="#cite_note-wells561-42">[36]</a> The mineral <a href="/wiki/Malachite" title="Malachite">malachite</a> is a typical example of a basic carbonate. The formula, Cu2CO3(OH)2 shows that it is halfway between <a href="/wiki/Basic_copper_carbonate" title="Basic copper carbonate">copper carbonate</a> and <a href="/wiki/Copper_hydroxide" class="mw-redirect" title="Copper hydroxide">copper hydroxide</a>. Indeed, in the past the formula was written as CuCO3·Cu(OH)2. The <a href="/wiki/Crystal_structure" title="Crystal structure">crystal structure</a> is made up of copper, carbonate and hydroxide ions.<a href="#cite_note-wells561-42">[36]</a> The mineral <a href="/wiki/Atacamite" title="Atacamite">atacamite</a> is an example of a basic chloride. It has the formula Cu2Cl(OH)3. In this case the composition is nearer to that of the hydroxide than that of the chloride: CuCl2·3Cu(OH)2.<a href="#cite_note-43">[37]</a> Copper forms hydroxyphosphate (<a href="/wiki/Libethenite" title="Libethenite">libethenite</a>), arsenate (<a href="/wiki/Olivenite" title="Olivenite">olivenite</a>), sulfate (<a href="/wiki/Brochantite" title="Brochantite">brochantite</a>), and nitrate compounds. <a href="/wiki/White_lead" title="White lead">White lead</a> is a basic <a href="/wiki/Lead" title="Lead">lead</a> carbonate, (PbCO3)2·Pb(OH)2, which has been used as a white <a href="/wiki/Pigment" title="Pigment">pigment</a> because of its opaque quality, though its use is now restricted because it can be a source for <a href="/wiki/Lead_poisoning" title="Lead poisoning">lead poisoning</a>.<a href="#cite_note-wells561-42">[36]</a> <div class="mw-heading mw-heading2"><h2 id="Structural_chemistry">Structural chemistry</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=12" title="Edit section: Structural chemistry">edit</a>]</div> The hydroxide ion appears to rotate freely in crystals of the heavier alkali metal hydroxides at higher temperatures so as to present itself as a spherical ion, with an effective <a href="/wiki/Ionic_radius" title="Ionic radius">ionic radius</a> of about 153 pm.<a href="#cite_note-wells548-44">[38]</a> Thus, the high-temperature forms of KOH and NaOH have the <a href="/wiki/Sodium_chloride#Crystal_structure" title="Sodium chloride">sodium chloride</a> structure,<a href="#cite_note-45">[39]</a> which gradually freezes in a monoclinically distorted sodium chloride structure at temperatures below about 300 °C. The OH groups still rotate even at room temperature around their symmetry axes and, therefore, cannot be detected by <a href="/wiki/X-ray_diffraction" title="X-ray diffraction">X-ray diffraction</a>.<a href="#cite_note-46">[40]</a> The room-temperature form of NaOH has the <a href="/wiki/Thallium(I)_iodide" title="Thallium(I) iodide">thallium iodide</a> structure. LiOH, however, has a layered structure, made up of tetrahedral Li(OH)4 and (OH)Li4 units.<a href="#cite_note-wells548-44">[38]</a> This is consistent with the weakly basic character of LiOH in solution, indicating that the Li–OH bond has much covalent character. The hydroxide ion displays cylindrical symmetry in hydroxides of divalent metals Ca, Cd, Mn, Fe, and Co. For example, magnesium hydroxide Mg(OH)2 (<a href="/wiki/Brucite" title="Brucite">brucite</a>) crystallizes with the <a href="/wiki/Cadmium_iodide" title="Cadmium iodide">cadmium iodide</a> layer structure, with a kind of close-packing of magnesium and hydroxide ions.<a href="#cite_note-wells548-44">[38]</a><a href="#cite_note-47">[41]</a> The <a href="/wiki/Amphoterism" title="Amphoterism">amphoteric</a> hydroxide Al(OH)3 has four major crystalline forms: <a href="/wiki/Gibbsite" title="Gibbsite">gibbsite</a> (most stable), <a href="/wiki/Bayerite" class="mw-redirect" title="Bayerite">bayerite</a>, <a href="/w/index.php?title=Nordstrandite&action=edit&redlink=1" class="new" title="Nordstrandite (page does not exist)">nordstrandite</a>, and <a href="/wiki/Doyleite" title="Doyleite">doyleite</a>.<a href="#cite_note-48">[note 7]</a> All these <a href="/wiki/Polymorphism_(materials_science)" class="mw-redirect" title="Polymorphism (materials science)">polymorphs</a> are built up of double layers of hydroxide ions—the aluminium atoms on two-thirds of the octahedral holes between the two layers—and differ only in the stacking sequence of the layers.<a href="#cite_note-49">[42]</a> The structures are similar to the brucite structure. However, whereas the brucite structure can be described as a close-packed structure, in gibbsite the OH groups on the underside of one layer rest on the groups of the layer below. This arrangement led to the suggestion that there are directional bonds between OH groups in adjacent layers.<a href="#cite_note-50">[43]</a> This is an unusual form of <a href="/wiki/Hydrogen_bond" title="Hydrogen bond">hydrogen bonding</a> since the two hydroxide ions involved would be expected to point away from each other. The hydrogen atoms have been located by <a href="/wiki/Neutron_diffraction" title="Neutron diffraction">neutron diffraction</a> experiments on α-AlO(OH) (<a href="/wiki/Diaspore" title="Diaspore">diaspore</a>). The O–H–O distance is very short, at 265 pm; the hydrogen is not equidistant between the oxygen atoms and the short OH bond makes an angle of 12° with the O–O line.<a href="#cite_note-51">[44]</a> A similar type of hydrogen bond has been proposed for other amphoteric hydroxides, including Be(OH)2, Zn(OH)2, and Fe(OH)3.<a href="#cite_note-wells548-44">[38]</a> A number of mixed hydroxides are known with stoichiometry A3MIII(OH)6, A2MIV(OH)6, and AMV(OH)6. As the formula suggests these substances contain M(OH)6 octahedral structural units.<a href="#cite_note-52">[45]</a> <a href="/wiki/Layered_double_hydroxides" title="Layered double hydroxides">Layered double hydroxides</a> may be represented by the formula [Mz+ 1−xM3+ x(OH) 2]q+(Xn−) <style data-mw-deduplicate="TemplateStyles:r1154941027">.mw-parser-output .frac{white-space:nowrap}.mw-parser-output .frac .num,.mw-parser-output .frac .den{font-size:80%;line-height:0;vertical-align:super}.mw-parser-output .frac .den{vertical-align:sub}.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>q⁄n·yH 2O. Most commonly, z = 2, and M2+ = Ca2+, Mg2+, Mn2+, Fe2+, Co2+, Ni2+, Cu2+, or Zn2+; hence q = x. <div class="mw-heading mw-heading2"><h2 id="Organic_reactions">Organic reactions</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=13" title="Edit section: Organic reactions">edit</a>]</div> <a href="/wiki/Potassium_hydroxide" title="Potassium hydroxide">Potassium hydroxide</a> and <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a> are two well-known <a href="/wiki/Reagent" title="Reagent">reagents</a> in <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>. <div class="mw-heading mw-heading3"><h3 id="Base_catalysis">Base catalysis</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=14" title="Edit section: Base catalysis">edit</a>]</div> The hydroxide ion may act as a <a href="/wiki/Base_catalyst" class="mw-redirect" title="Base catalyst">base catalyst</a>.<a href="#cite_note-53">[46]</a> The base abstracts a proton from a weak acid to give an intermediate that goes on to react with another reagent. Common substrates for proton abstraction are <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohols</a>, <a href="/wiki/Phenol" title="Phenol">phenols</a>, <a href="/wiki/Amine" title="Amine">amines</a>, and <a href="/wiki/Carbon_acid" class="mw-redirect" title="Carbon acid">carbon acids</a>. The <a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">pKa</a> value for dissociation of a C–H bond is extremely high, but the pKa <a href="/wiki/Alpha_hydrogen" class="mw-redirect" title="Alpha hydrogen">alpha hydrogens</a> of a carbonyl compound are about 3 log units lower. Typical pKa values are 16.7 for <a href="/wiki/Acetaldehyde" title="Acetaldehyde">acetaldehyde</a> and 19 for <a href="/wiki/Acetone" title="Acetone">acetone</a>.<a href="#cite_note-54">[47]</a> Dissociation can occur in the presence of a suitable base. <dl><dd>RC(O)CH2R' + B ⇌ RC(O)CH−R' + BH+</dd></dl> The base should have a pKa value not less than about 4 log units smaller, or the equilibrium will lie almost completely to the left. The hydroxide ion by itself is not a strong enough base, but it can be converted to one by adding sodium hydroxide to <a href="/wiki/Ethanol" title="Ethanol">ethanol</a> <dl><dd>OH− + EtOH ⇌ EtO− + H2O</dd></dl> to produce the <a href="/wiki/Ethoxide" class="mw-redirect" title="Ethoxide">ethoxide</a> ion. The <a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">pKa</a> for self-dissociation of ethanol is about 16, so the alkoxide ion is a strong enough base.<a href="#cite_note-55">[48]</a> The addition of an alcohol to an <a href="/wiki/Aldehyde" title="Aldehyde">aldehyde</a> to form a <a href="/wiki/Hemiacetal" title="Hemiacetal">hemiacetal</a> is an example of a reaction that can be catalyzed by the presence of hydroxide. Hydroxide can also act as a Lewis-base catalyst.<a href="#cite_note-56">[49]</a> <div class="mw-heading mw-heading3"><h3 id="As_a_nucleophilic_reagent">As a nucleophilic reagent</h3>[<a href="/w/index.php?title=Hydroxide&action=edit&section=15" title="Edit section: As a nucleophilic reagent">edit</a>]</div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:AcylSubstitution.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f6/AcylSubstitution.svg/330px-AcylSubstitution.svg.png" decoding="async" width="300" height="98" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f6/AcylSubstitution.svg/450px-AcylSubstitution.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f6/AcylSubstitution.svg/600px-AcylSubstitution.svg.png 2x" data-file-width="351" data-file-height="115" /></a><figcaption>Nucleophilic acyl substitution with an anionic <a href="/wiki/Nucleophile" title="Nucleophile">nucleophile</a> (Nu−) and <a href="/wiki/Leaving_group" title="Leaving group">leaving group</a> (L−)</figcaption></figure> The hydroxide ion is intermediate in <a href="/wiki/Nucleophilicity" class="mw-redirect" title="Nucleophilicity">nucleophilicity</a> between the <a href="/wiki/Fluoride" title="Fluoride">fluoride</a> ion F−, and the <a href="/wiki/Azanide" title="Azanide">amide</a> ion NH− 2.<a href="#cite_note-57">[50]</a> <a href="/wiki/Ester_hydrolysis" title="Ester hydrolysis">Ester hydrolysis</a> under alkaline conditions (also known as <a href="/wiki/Base_hydrolysis" class="mw-redirect" title="Base hydrolysis">base hydrolysis</a>) <dl><dd>R1C(O)OR2 + OH− ⇌ R1CO(O)H + −OR2 ⇌ R1CO2− + HOR2</dd></dl> is an example of a hydroxide ion serving as a nucleophile.<a href="#cite_note-Hardinger-58">[51]</a> Early methods for <a href="/wiki/Saponification" title="Saponification">manufacturing soap</a> treated <a href="/wiki/Triglyceride" title="Triglyceride">triglycerides</a> from animal fat (the ester) with <a href="/wiki/Lye" title="Lye">lye</a>. Other cases where hydroxide can act as a nucleophilic reagent are <a href="/wiki/Amide" title="Amide">amide</a> hydrolysis, the <a href="/wiki/Cannizzaro_reaction" title="Cannizzaro reaction">Cannizzaro reaction</a>, <a href="/wiki/Nucleophilic_aliphatic_substitution" class="mw-redirect" title="Nucleophilic aliphatic substitution">nucleophilic aliphatic substitution</a>, <a href="/wiki/Nucleophilic_aromatic_substitution" title="Nucleophilic aromatic substitution">nucleophilic aromatic substitution</a>, and in <a href="/wiki/Elimination_reaction" title="Elimination reaction">elimination reactions</a>. The reaction medium for KOH and NaOH is usually water but with a <a href="/wiki/Phase-transfer_catalyst" title="Phase-transfer catalyst">phase-transfer catalyst</a> the hydroxide anion can be shuttled into an organic solvent as well, for example in the generation of the reactive intermediate <a href="/wiki/Dichlorocarbene" title="Dichlorocarbene">dichlorocarbene</a>. <div class="mw-heading mw-heading2"><h2 id="Notes">Notes</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=16" title="Edit section: Notes">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"><ol class="references"> <li id="cite_note-3"><a href="#cite_ref-3">^</a> [H+] denotes the concentration of <a href="/wiki/Hydron_(chemistry)" title="Hydron (chemistry)">hydrogen cations</a> and [OH−] the concentration of hydroxide ions </li> <li id="cite_note-4"><a href="#cite_ref-4">^</a> Strictly speaking pH is the cologarithm of the hydrogen cation <a href="/wiki/Activity_(chemistry)" class="mw-redirect" title="Activity (chemistry)">activity</a> </li> <li id="cite_note-5"><a href="#cite_ref-5">^</a> pOH signifies the negative logarithm to base 10 of [OH−], alternatively the logarithm of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035" />⁠1/[OH−]⁠ </li> <li id="cite_note-8"><a href="#cite_ref-8">^</a> In this context proton is the term used for a solvated hydrogen cation </li> <li id="cite_note-19"><a href="#cite_ref-19">^</a> In aqueous solution the ligands L are water molecules, but they may be replaced by other ligands </li> <li id="cite_note-35"><a href="#cite_ref-35">^</a> The name is not derived from "period", but from "iodine": periodic acid (compare <a href="/wiki/Iodic_acid" title="Iodic acid">iodic acid</a>, <a href="/wiki/Perchloric_acid" title="Perchloric acid">perchloric acid</a>), and it is thus pronounced per-iodic <a href="/wiki/Help:IPA/English" title="Help:IPA/English">/ˌpɜːraɪˈɒdɪk/</a> <a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key">PUR-eye-OD-ik</a>, and not as <a href="/wiki/Help:IPA/English" title="Help:IPA/English">/ˌpɪərɪ-/</a> <a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key">PEER-ee-</a>. </li> <li id="cite_note-48"><a href="#cite_ref-48">^</a> Crystal structures are illustrated at Web mineral: <a rel="nofollow" class="external text" href="http://webmineral.com/data/Gibbsite.shtml">Gibbsite</a>, <a rel="nofollow" class="external text" href="http://webmineral.com/data/Bayerite.shtml">Bayerite</a>, <a rel="nofollow" class="external text" href="http://webmineral.com/data/Nordstrandite.shtml">Norstrandite</a> and <a rel="nofollow" class="external text" href="http://webmineral.com/data/Doyleite.shtml">Doyleite</a> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=17" title="Edit section: References">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239543626" /><div class="reflist reflist-columns references-column-width" style="column-width: 30em;"> <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 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(2010). "Aqueous Basic Solutions: Hydroxide Solvation, Structural Diffusion, and Comparison to the Hydrated Proton". Chem. Rev. 110 (4): 2174–2216. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fcr900233f">10.1021/cr900233f</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/20170203">20170203</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chem.+Rev.&rft.atitle=Aqueous+Basic+Solutions%3A+Hydroxide+Solvation%2C+Structural+Diffusion%2C+and+Comparison+to+the+Hydrated+Proton&rft.volume=110&rft.issue=4&rft.pages=%3Cspan+class%3D%22nowrap%22%3E2174-%3C%2Fspan%3E2216&rft.date=2010&rft_id=info%3Adoi%2F10.1021%2Fcr900233f&rft_id=info%3Apmid%2F20170203&rft.aulast=Marx&rft.aufirst=D.&rft.au=Chandra%2C+A&rft.au=Tuckerman%2C+M.E.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> <li id="cite_note-9"><a href="#cite_ref-9">^</a> Greenwood, p. 1168 </li> <li id="cite_note-scdb-10">^ <a href="#cite_ref-scdb_10-0">a</a> <a href="#cite_ref-scdb_10-1">b</a> <a rel="nofollow" class="external text" href="http://www.acadsoft.co.uk/scdbase/scdbase.htm">IUPAC SC-Database</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20170619235720/http://www.acadsoft.co.uk/scdbase/scdbase.htm">Archived</a> 2017-06-19 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> A comprehensive database of published data on equilibrium constants of metal complexes and ligands </li> <li id="cite_note-nakamoto-11"><a href="#cite_ref-nakamoto_11-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFNakamoto1997" class="citation book cs1">Nakamoto, K. (1997). Infrared and Raman spectra of Inorganic and Coordination compounds. Part A (5th ed.). Wiley. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-471-16394-7" title="Special:BookSources/978-0-471-16394-7"><bdi>978-0-471-16394-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Infrared+and+Raman+spectra+of+Inorganic+and+Coordination+compounds&rft.series=Part+A&rft.edition=5th&rft.pub=Wiley&rft.date=1997&rft.isbn=978-0-471-16394-7&rft.aulast=Nakamoto&rft.aufirst=K.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> <li id="cite_note-12"><a href="#cite_ref-12">^</a> Nakamoto, Part B, p. 57 </li> <li id="cite_note-13"><a href="#cite_ref-13">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFAdams1967" class="citation book cs1">Adams, D.M. (1967). Metal–Ligand and Related Vibrations. London: Edward Arnold.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Metal%E2%80%93Ligand+and+Related+Vibrations&rft.place=London&rft.pub=Edward+Arnold&rft.date=1967&rft.aulast=Adams&rft.aufirst=D.M.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> Chapter 5. </li> <li id="cite_note-Ullmann-14"><a href="#cite_ref-Ullmann_14-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFCetin_Kurt,_Jürgen_Bittner" class="citation encyclopaedia cs1">Cetin Kurt, Jürgen Bittner. "Sodium Hydroxide". <a href="/wiki/Ullmann%27s_Encyclopedia_of_Industrial_Chemistry" title="Ullmann's Encyclopedia of Industrial Chemistry">Ullmann's Encyclopedia of Industrial Chemistry</a>. Weinheim: Wiley-VCH. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F14356007.a24_345.pub2">10.1002/14356007.a24_345.pub2</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3-527-30673-2" title="Special:BookSources/978-3-527-30673-2"><bdi>978-3-527-30673-2</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Sodium+Hydroxide&rft.btitle=Ullmann%27s+Encyclopedia+of+Industrial+Chemistry&rft.place=Weinheim&rft.pub=Wiley-VCH&rft_id=info%3Adoi%2F10.1002%2F14356007.a24_345.pub2&rft.isbn=978-3-527-30673-2&rft.au=Cetin+Kurt%2C+J%C3%BCrgen+Bittner&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> <li id="cite_note-15"><a href="#cite_ref-15">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFEmsley2001" class="citation book cs1">Emsley, John (2001). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=j-Xu07p3cKwC&pg=PA24">"Aluminium"</a>. <a rel="nofollow" class="external text" href="https://archive.org/details/naturesbuildingb0000emsl/page/24">Nature's Building Blocks: An A–Z Guide to the Elements</a>. Oxford, UK: Oxford University Press. p. <a rel="nofollow" class="external text" href="https://archive.org/details/naturesbuildingb0000emsl/page/24">24</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-19-850340-8" title="Special:BookSources/978-0-19-850340-8"><bdi>978-0-19-850340-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Aluminium&rft.btitle=Nature%27s+Building+Blocks%3A+An+A%E2%80%93Z+Guide+to+the+Elements&rft.place=Oxford%2C+UK&rft.pages=24&rft.pub=Oxford+University+Press&rft.date=2001&rft.isbn=978-0-19-850340-8&rft.aulast=Emsley&rft.aufirst=John&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3Dj-Xu07p3cKwC%26pg%3DPA24&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> <li id="cite_note-16"><a href="#cite_ref-16">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFEmsley2001" class="citation book cs1">Emsley, John (2001). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=j-Xu07p3cKwC&pg=PA209">"Aluminium"</a>. <a rel="nofollow" class="external text" href="https://archive.org/details/naturesbuildingb0000emsl/page/209">Nature's Building Blocks: An A–Z Guide to the Elements</a>. Oxford, UK: Oxford University Press. p. <a rel="nofollow" class="external text" href="https://archive.org/details/naturesbuildingb0000emsl/page/209">209</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-19-850340-8" title="Special:BookSources/978-0-19-850340-8"><bdi>978-0-19-850340-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Aluminium&rft.btitle=Nature%27s+Building+Blocks%3A+An+A%E2%80%93Z+Guide+to+the+Elements&rft.place=Oxford%2C+UK&rft.pages=209&rft.pub=Oxford+University+Press&rft.date=2001&rft.isbn=978-0-19-850340-8&rft.aulast=Emsley&rft.aufirst=John&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3Dj-Xu07p3cKwC%26pg%3DPA209&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> <li id="cite_note-17"><a href="#cite_ref-17">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFJaunsen1989" class="citation journal cs1 cs1-prop-long-vol cs1-prop-unfit">Jaunsen, JR (1989). <a rel="nofollow" class="external text" href="https://web.archive.org/web/20090824104846/http://archive.rubicon-foundation.org/4998">"The Behavior and Capabilities of Lithium Hydroxide Carbon Dioxide Scrubbers in a Deep Sea Environment"</a>. 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(2017). <a rel="nofollow" class="external text" href="http://www.chem.ucla.edu/~harding/IGOC/S/saponification.html">"Illustrated Glossary of Organic Chemistry: Saponification"</a>. <a href="/wiki/UCLA_College_of_Letters_and_Science" title="UCLA College of Letters and Science">Department of Chemistry & Biochemistry, UCLA</a>. Retrieved April 10, 2023.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Illustrated+Glossary+of+Organic+Chemistry%3A+Saponification&rft.pub=Department+of+Chemistry+%26+Biochemistry%2C+UCLA&rft.date=2017&rft.aulast=Hardinger&rft.aufirst=Steven+A.&rft_id=http%3A%2F%2Fwww.chem.ucla.edu%2F~harding%2FIGOC%2FS%2Fsaponification.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"> </li> </ol></div> <div class="mw-heading mw-heading2"><h2 id="Bibliography">Bibliography</h2>[<a href="/w/index.php?title=Hydroxide&action=edit&section=18" title="Edit section: Bibliography">edit</a>]</div> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFHollemanWibergWiberg2001" class="citation book cs1">Holleman, A.F.; Wiberg, E.; Wiberg, N. (2001). Inorganic Chemistry. Academic press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-12-352651-9" title="Special:BookSources/978-0-12-352651-9"><bdi>978-0-12-352651-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Inorganic+Chemistry&rft.pub=Academic+press&rft.date=2001&rft.isbn=978-0-12-352651-9&rft.aulast=Holleman&rft.aufirst=A.F.&rft.au=Wiberg%2C+E.&rft.au=Wiberg%2C+N.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFHousecroftSharpe2008" class="citation book cs1">Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-13-175553-6" title="Special:BookSources/978-0-13-175553-6"><bdi>978-0-13-175553-6</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Inorganic+Chemistry&rft.edition=3rd&rft.pub=Prentice+Hall&rft.date=2008&rft.isbn=978-0-13-175553-6&rft.aulast=Housecroft&rft.aufirst=C.+E.&rft.au=Sharpe%2C+A.+G.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="/wiki/Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-08-037941-8" title="Special:BookSources/978-0-08-037941-8"><bdi>978-0-08-037941-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry+of+the+Elements&rft.edition=2nd&rft.pub=Butterworth-Heinemann&rft.date=1997&rft.isbn=978-0-08-037941-8&rft.aulast=Greenwood&rft.aufirst=Norman+N.&rft.au=Earnshaw%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFShriverAtkins1999" class="citation book cs1">Shriver, D.F; Atkins, P.W (1999). Inorganic Chemistry (3rd ed.). Oxford: Oxford University Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-19-850330-9" title="Special:BookSources/978-0-19-850330-9"><bdi>978-0-19-850330-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Inorganic+Chemistry&rft.place=Oxford&rft.edition=3rd&rft.pub=Oxford+University+Press&rft.date=1999&rft.isbn=978-0-19-850330-9&rft.aulast=Shriver&rft.aufirst=D.F&rft.au=Atkins%2C+P.W&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFWells1962" class="citation book cs1">Wells, A.F (1962). Structural Inorganic Chemistry (3rd. ed.). Oxford: Clarendon Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-19-855125-6" title="Special:BookSources/978-0-19-855125-6"><bdi>978-0-19-855125-6</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Structural+Inorganic+Chemistry&rft.place=Oxford&rft.edition=3rd.&rft.pub=Clarendon+Press&rft.date=1962&rft.isbn=978-0-19-855125-6&rft.aulast=Wells&rft.aufirst=A.F&rfr_id=info%3Asid%2Fen.wikipedia.org%3AHydroxide" class="Z3988"></li></ul> <div class="navbox-styles"><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline 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href="/wiki/Template:Hydroxides" title="Template:Hydroxides"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Hydroxides" title="Template talk:Hydroxides"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Hydroxides" title="Special:EditPage/Template:Hydroxides"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Hydroxides88" style="font-size:114%;margin:0 4em"><a class="mw-selflink selflink">Hydroxides</a></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/Properties_of_water" title="Properties of water">HOH</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_hydroxide" title="Lithium hydroxide">LiOH</a> </td> <td><a href="/wiki/Beryllium_hydroxide" title="Beryllium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Be(OH)2</a> </td> <td><a href="/wiki/Boric_acid" title="Boric acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />B(OH)3</a> </td> <td><a href="/wiki/Orthocarbonic_acid" title="Orthocarbonic acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />C(OH)4</a> </td> <td><a href="/w/index.php?title=Azorous_acid&action=edit&redlink=1" class="new" title="Azorous acid (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />N(OH)3</a> <a href="/wiki/Ammonium_hydroxide" class="mw-redirect" title="Ammonium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />[NH4]+OH−</a> </td> <td><a href="/wiki/Trioxidane" title="Trioxidane"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />O(OH)2</a> </td> <td><a href="/wiki/Hypofluorous_acid" title="Hypofluorous acid">FOH</a> </td> <td>Ne </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">NaOH</a> </td> <td><a href="/wiki/Magnesium_hydroxide" title="Magnesium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Mg(OH)2</a> </td> <td><a href="/wiki/Aluminium_hydroxide" title="Aluminium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Al(OH)3</a> </td> <td><a href="/wiki/Orthosilicic_acid" title="Orthosilicic acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Si(OH)4</a> </td> <td><a href="/wiki/Phosphorous_acid" title="Phosphorous acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />P(OH)3</a> </td> <td><a href="/wiki/Sulfur_dihydroxide" class="mw-redirect" title="Sulfur dihydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />S(OH)2</a> </td> <td><a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">ClOH</a> </td> <td>Ar </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Potassium_hydroxide" title="Potassium hydroxide">KOH</a> </td> <td><a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ca(OH)2</a> </td> <td style="background-color:white;color:inherit;border:none"> </td> <td><a href="/wiki/Scandium(III)_hydroxide" title="Scandium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sc(OH)3</a> </td> <td><a href="/w/index.php?title=Titanium(II)_hydroxide&action=edit&redlink=1" class="new" title="Titanium(II) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ti(OH)2</a> <a href="/w/index.php?title=Titanium(III)_hydroxide&action=edit&redlink=1" class="new" title="Titanium(III) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ti(OH)3</a> <a href="/wiki/Titanium(IV)_hydroxide" class="mw-redirect" title="Titanium(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ti(OH)4</a> </td> <td><a href="/w/index.php?title=Vanadium(II)_hydroxide&action=edit&redlink=1" class="new" title="Vanadium(II) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />V(OH)2</a> <a href="/w/index.php?title=Vanadium(III)_hydroxide&action=edit&redlink=1" class="new" title="Vanadium(III) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />V(OH)3</a> </td> <td><a href="/w/index.php?title=Chromium(II)_hydroxide&action=edit&redlink=1" class="new" title="Chromium(II) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Cr(OH)2</a> <a href="/wiki/Chromium(III)_hydroxide" title="Chromium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Cr(OH)3</a> </td> <td><a href="/wiki/Manganese(II)_hydroxide" title="Manganese(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Mn(OH)2</a> </td> <td><a href="/wiki/Iron(II)_hydroxide" title="Iron(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Fe(OH)2</a> <a href="/wiki/Iron(III)_hydroxide" class="mw-redirect" title="Iron(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Fe(OH)3</a> </td> <td><a href="/wiki/Cobalt(II)_hydroxide" title="Cobalt(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Co(OH)2</a> </td> <td><a href="/wiki/Nickel(II)_hydroxide" title="Nickel(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ni(OH)2</a> </td> <td><a href="/wiki/Copper(I)_hydroxide" title="Copper(I) hydroxide">CuOH</a> <a href="/wiki/Copper(II)_hydroxide" title="Copper(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Cu(OH)2</a> </td> <td><a href="/wiki/Zinc_hydroxide" title="Zinc hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Zn(OH)2</a> </td> <td><a href="/wiki/Gallium(III)_hydroxide" title="Gallium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ga(OH)3</a> </td> <td><a href="/wiki/Germanium(II)_hydroxide" title="Germanium(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ge(OH)2</a> </td> <td><a href="/wiki/Arsenous_acid" title="Arsenous acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />As(OH)3</a> </td> <td>Se </td> <td><a href="/wiki/Hypobromous_acid" title="Hypobromous acid">BrOH</a> </td> <td>Kr </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Rubidium_hydroxide" title="Rubidium hydroxide">RbOH</a> </td> <td><a href="/wiki/Strontium_hydroxide" title="Strontium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sr(OH)2</a> </td> <td style="background-color:white;color:inherit;border:none"> </td> <td><a href="/wiki/Yttrium_hydroxide" title="Yttrium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Y(OH)3</a> </td> <td><a href="/wiki/Zirconium(IV)_hydroxide" title="Zirconium(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Zr(OH)4</a> </td> <td>Nb </td> <td>Mo </td> <td><a href="/wiki/Technetium(IV)_hydroxide" class="mw-redirect" title="Technetium(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Tc(OH)4</a> </td> <td>Ru </td> <td><a href="/wiki/Rhodium(III)_hydroxide" title="Rhodium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Rh(OH)3</a> </td> <td>Pd </td> <td><a href="/wiki/Silver_hydroxide" class="mw-redirect" title="Silver hydroxide">AgOH</a> </td> <td><a href="/wiki/Cadmium_hydroxide" title="Cadmium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Cd(OH)2</a> </td> <td><a href="/wiki/Indium(III)_hydroxide" title="Indium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />In(OH)3</a> </td> <td><a href="/wiki/Tin(II)_hydroxide" title="Tin(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sn(OH)2</a> <a href="/wiki/Tin(IV)_hydroxide" class="mw-redirect" title="Tin(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sn(OH)4</a> </td> <td><a href="/w/index.php?title=Antimonous_acid&action=edit&redlink=1" class="new" title="Antimonous acid (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sb(OH)3</a> </td> <td><a href="/wiki/Telluric_acid" title="Telluric acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Te(OH)6</a> </td> <td><a href="/wiki/Hypoiodous_acid" title="Hypoiodous acid">IOH</a> </td> <td>Xe </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Caesium_hydroxide" title="Caesium hydroxide">CsOH</a> </td> <td><a href="/wiki/Barium_hydroxide" title="Barium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ba(OH)2</a> </td> <td style="background-color:white;color:inherit;border:none">* </td> <td><a href="/wiki/Lutetium(III)_hydroxide" title="Lutetium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Lu(OH)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><a href="/wiki/Gold(III)_hydroxide" title="Gold(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Au(OH)3</a> </td> <td><a href="/wiki/Mercury(II)_hydroxide" title="Mercury(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Hg(OH)2</a> </td> <td><a href="/wiki/Thallium(I)_hydroxide" title="Thallium(I) hydroxide">TlOH</a> <a href="/wiki/Thallium(III)_hydroxide" title="Thallium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Tl(OH)3</a> </td> <td><a href="/wiki/Lead(II)_hydroxide" title="Lead(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pb(OH)2</a> <a href="/w/index.php?title=Lead(IV)_hydroxide&action=edit&redlink=1" class="new" title="Lead(IV) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pb(OH)4</a> </td> <td><a href="/wiki/Bismuth_hydroxide" title="Bismuth hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Bi(OH)3</a> </td> <td>Po </td> <td>At </td> <td>Rn </td></tr> <tr style="background-color:mistyrose;color:black;"> <td><a href="/wiki/Francium_hydroxide" title="Francium hydroxide">FrOH</a> </td> <td><a href="/wiki/Radium_hydroxide" title="Radium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ra(OH)2</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_hydroxide" title="Lanthanum hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />La(OH)3</a> </td> <td><a href="/wiki/Cerium(III)_hydroxide" title="Cerium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ce(OH)3</a> <a href="/wiki/Cerium(IV)_hydroxide" title="Cerium(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ce(OH)4</a> </td> <td><a href="/wiki/Praseodymium(III)_hydroxide" title="Praseodymium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pr(OH)3</a> </td> <td><a href="/wiki/Neodymium(III)_hydroxide" title="Neodymium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Nd(OH)3</a> </td> <td><a href="/wiki/Promethium(III)_hydroxide" title="Promethium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pm(OH)3</a> </td> <td><a href="/wiki/Samarium(III)_hydroxide" title="Samarium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Sm(OH)3</a> </td> <td><a href="/wiki/Europium(II)_hydroxide" title="Europium(II) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Eu(OH)2</a> <a href="/wiki/Europium(III)_hydroxide" title="Europium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Eu(OH)3</a> </td> <td><a href="/wiki/Gadolinium(III)_hydroxide" title="Gadolinium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Gd(OH)3</a> </td> <td><a href="/wiki/Terbium(III)_hydroxide" title="Terbium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Tb(OH)3</a> </td> <td><a href="/wiki/Dysprosium(III)_hydroxide" title="Dysprosium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Dy(OH)3</a> </td> <td><a href="/wiki/Holmium(III)_hydroxide" title="Holmium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ho(OH)3</a> </td> <td><a href="/wiki/Erbium(III)_hydroxide" title="Erbium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Er(OH)3</a> </td> <td><a href="/wiki/Thulium(III)_hydroxide" title="Thulium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Tm(OH)3</a> </td> <td><a href="/wiki/Ytterbium(III)_hydroxide" title="Ytterbium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Yb(OH)3</a> </td></tr> <tr style="background-color:mistyrose;color:black;"> <td style="background-color:white;color:inherit;border:none">** </td> <td><a href="/wiki/Actinium(III)_hydroxide" title="Actinium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Ac(OH)3</a> </td> <td><a href="/wiki/Thorium(IV)_hydroxide" title="Thorium(IV) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Th(OH)4</a> </td> <td>Pa </td> <td><a href="/w/index.php?title=Uranium(II)_hydroxide&action=edit&redlink=1" class="new" title="Uranium(II) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />U(OH)2</a> <a href="/w/index.php?title=Uranium(III)_hydroxide&action=edit&redlink=1" class="new" title="Uranium(III) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />U(OH)3</a> <a href="/wiki/Uranyl_hydroxide" title="Uranyl hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />UO2(OH)2</a> </td> <td><a href="/w/index.php?title=Neptunium(III)_hydroxide&action=edit&redlink=1" class="new" title="Neptunium(III) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Np(OH)3</a> <a href="/w/index.php?title=Neptunium(IV)_hydroxide&action=edit&redlink=1" class="new" title="Neptunium(IV) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Np(OH)4</a> <a href="/wiki/Neptunium(VII)_oxide-hydroxide" title="Neptunium(VII) oxide-hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />NpO2(OH)3</a> </td> <td><a href="/w/index.php?title=Plutonium(III)_hydroxide&action=edit&redlink=1" class="new" title="Plutonium(III) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pu(OH)3</a> <a href="/w/index.php?title=Plutonium(IV)_hydroxide&action=edit&redlink=1" class="new" title="Plutonium(IV) hydroxide (page does not exist)"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Pu(OH)4</a> </td> <td><a href="/wiki/Americium(III)_hydroxide" title="Americium(III) hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Am(OH)3</a> </td> <td><a href="/wiki/Curium_hydroxide" class="mw-redirect" title="Curium hydroxide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410" />Cm(OH)3</a> </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 authority-control" aria-label="Navbox711" style="padding:3px"><table class="nowraplinks hlist navbox-inner" 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