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class="vector-toc-link" href="#Solvents_and_intermolecular_interactions"> <div class="vector-toc-text"> <span class="vector-toc-numb">2</span> <span>Solvents and intermolecular interactions</span> </div> </a> <ul id="toc-Solvents_and_intermolecular_interactions-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Solvation_energy_and_thermodynamic_considerations" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Solvation_energy_and_thermodynamic_considerations"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Solvation energy and thermodynamic considerations</span> </div> </a> <ul id="toc-Solvation_energy_and_thermodynamic_considerations-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Macromolecules_and_assemblies" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Macromolecules_and_assemblies"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Macromolecules and assemblies</span> </div> </a> <ul id="toc-Macromolecules_and_assemblies-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Importance_of_solvation_in_computer_simulations" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Importance_of_solvation_in_computer_simulations"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Importance of solvation in computer simulations</span> </div> </a> <ul id="toc-Importance_of_solvation_in_computer_simulations-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>See also</span> </div> </a> <ul id="toc-See_also-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>References</span> </div> </a> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Further_reading" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Further_reading"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>Further reading</span> </div> </a> <ul id="toc-Further_reading-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>External links</span> </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" > <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" ><span class="vector-icon mw-ui-icon-listBullet mw-ui-icon-wikimedia-listBullet"></span> <span class="vector-dropdown-label-text">Toggle the table of contents</span> </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"><span class="mw-page-title-main">Solvation</span></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. 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href="https://be.wikipedia.org/wiki/%D0%A1%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D1%8B%D1%8F" title="Сальватацыя – Belarusian" lang="be" hreflang="be" data-title="Сальватацыя" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target"><span>Беларуская</span></a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Solvataci%C3%B3" title="Solvatació – Catalan" lang="ca" hreflang="ca" data-title="Solvatació" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target"><span>Català</span></a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Solvatisierung" title="Solvatisierung – German" lang="de" hreflang="de" data-title="Solvatisierung" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target"><span>Deutsch</span></a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Solvatatsioon" title="Solvatatsioon – Estonian" lang="et" hreflang="et" data-title="Solvatatsioon" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target"><span>Eesti</span></a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Solvataci%C3%B3n" title="Solvatación – Spanish" lang="es" hreflang="es" data-title="Solvatación" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target"><span>Español</span></a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Solbatazio" title="Solbatazio – Basque" lang="eu" hreflang="eu" data-title="Solbatazio" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target"><span>Euskara</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D8%AD%D9%84%D8%A7%D9%84%E2%80%8C%D9%BE%D9%88%D8%B4%DB%8C" title="حلال‌پوشی – Persian" lang="fa" hreflang="fa" data-title="حلال‌پوشی" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target"><span>فارسی</span></a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Solvatation" title="Solvatation – French" lang="fr" hreflang="fr" data-title="Solvatation" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EC%9A%A9%ED%95%B4" title="용해 – Korean" lang="ko" hreflang="ko" data-title="용해" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target"><span>한국어</span></a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%BC%D5%B8%D6%82%D5%AE%D5%B8%D6%82%D5%B4" title="Լուծում – Armenian" lang="hy" hreflang="hy" data-title="Լուծում" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target"><span>Հայերեն</span></a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Solvatacija" title="Solvatacija – Croatian" lang="hr" hreflang="hr" data-title="Solvatacija" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Solvasi" title="Solvasi – Indonesian" lang="id" hreflang="id" data-title="Solvasi" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target"><span>Bahasa Indonesia</span></a></li><li class="interlanguage-link interwiki-xh mw-list-item"><a href="https://xh.wikipedia.org/wiki/I-solvation" title="I-solvation – Xhosa" lang="xh" hreflang="xh" data-title="I-solvation" data-language-autonym="IsiXhosa" data-language-local-name="Xhosa" class="interlanguage-link-target"><span>IsiXhosa</span></a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Solvatazione" title="Solvatazione – Italian" lang="it" hreflang="it" data-title="Solvatazione" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target"><span>Italiano</span></a></li><li class="interlanguage-link interwiki-he badge-Q70894304 mw-list-item" title=""><a href="https://he.wikipedia.org/wiki/%D7%94%D7%9E%D7%A1%D7%94" title="המסה – Hebrew" lang="he" hreflang="he" data-title="המסה" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target"><span>עברית</span></a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BB%D1%8C%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D0%B8%D1%8F" title="Сольватация – Kazakh" lang="kk" hreflang="kk" data-title="Сольватация" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target"><span>Қазақша</span></a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BB%D1%8C%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D0%B8%D1%8F" title="Сольватация – Kyrgyz" lang="ky" hreflang="ky" data-title="Сольватация" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target"><span>Кыргызча</span></a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Szolvat%C3%A1ci%C3%B3" title="Szolvatáció – Hungarian" lang="hu" hreflang="hu" data-title="Szolvatáció" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target"><span>Magyar</span></a></li><li class="interlanguage-link interwiki-mdf mw-list-item"><a href="https://mdf.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BB%D1%8C%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D0%B8%D1%8F%D1%81%D1%8C" title="Сольватациясь – Moksha" lang="mdf" hreflang="mdf" data-title="Сольватациясь" data-language-autonym="Мокшень" data-language-local-name="Moksha" class="interlanguage-link-target"><span>Мокшень</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Solvatatie" title="Solvatatie – Dutch" lang="nl" hreflang="nl" data-title="Solvatatie" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target"><span>Nederlands</span></a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E6%BA%B6%E5%AA%92%E5%92%8C" title="溶媒和 – Japanese" lang="ja" hreflang="ja" data-title="溶媒和" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target"><span>日本語</span></a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Solvatisering" title="Solvatisering – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Solvatisering" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target"><span>Norsk nynorsk</span></a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Solwatacja" title="Solwatacja – Polish" lang="pl" hreflang="pl" data-title="Solwatacja" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target"><span>Polski</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Solvata%C3%A7%C3%A3o" title="Solvatação – Portuguese" lang="pt" hreflang="pt" data-title="Solvatação" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target"><span>Português</span></a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Solvatare" title="Solvatare – Romanian" lang="ro" hreflang="ro" data-title="Solvatare" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BB%D1%8C%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D0%B8%D1%8F" title="Сольватация – Russian" lang="ru" hreflang="ru" data-title="Сольватация" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target"><span>Русский</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Solvation" title="Solvation – Simple English" lang="en-simple" hreflang="en-simple" data-title="Solvation" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target"><span>Simple English</span></a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Solvat%C3%A1cia" title="Solvatácia – Slovak" lang="sk" hreflang="sk" data-title="Solvatácia" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target"><span>Slovenčina</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BB%D0%B2%D0%B0%D1%82%D0%B0%D1%86%D0%B8%D1%98%D0%B0" title="Солватација – Serbian" lang="sr" hreflang="sr" data-title="Солватација" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target"><span>Српски / srpski</span></a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Solvatacija" title="Solvatacija – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Solvatacija" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target"><span>Srpskohrvatski / српскохрватски</span></a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Solvatisering" title="Solvatisering – Swedish" lang="sv" hreflang="sv" data-title="Solvatisering" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target"><span>Svenska</span></a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/%C3%87%C3%B6z%C3%BClme" title="Çözülme – Turkish" lang="tr" hreflang="tr" data-title="Çözülme" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target"><span>Türkçe</span></a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a 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style="display:none">Association of molecules of a solvent with molecules or ions of a solute</div> <style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">Not to be confused with <a href="/wiki/Salvation" title="Salvation">salvation</a>.</div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Na%2BH2O.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/67/Na%2BH2O.svg/260px-Na%2BH2O.svg.png" decoding="async" width="260" height="260" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/67/Na%2BH2O.svg/390px-Na%2BH2O.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/67/Na%2BH2O.svg/520px-Na%2BH2O.svg.png 2x" data-file-width="512" data-file-height="512" /></a><figcaption>A sodium ion solvated by water molecules</figcaption></figure> <p><b>Solvation</b> describes the interaction of a <a href="/wiki/Solvent" title="Solvent">solvent</a> with <a href="/wiki/Solution_(chemistry)" title="Solution (chemistry)">dissolved</a> molecules. Both <a href="/wiki/Ion" title="Ion">ionized</a> and uncharged <a href="/wiki/Molecule" title="Molecule">molecules</a> interact strongly with a solvent, and the strength and nature of this interaction influence many properties of the solute, including solubility, reactivity, and color, as well as influencing the properties of the solvent such as its viscosity and density.<sup id="cite_ref-article-1_1-0" class="reference"><a href="#cite_note-article-1-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> If the attractive forces between the solvent and solute particles are greater than the attractive forces holding the solute particles together, the solvent particles pull the solute particles apart and surround them. The surrounded solute particles then move away from the solid solute and out into the solution. Ions are surrounded by a <a href="/wiki/Solvation_shell" title="Solvation shell">concentric shell of solvent</a>. Solvation is the process of reorganizing solvent and solute molecules into solvation complexes and involves bond formation, <a href="/wiki/Hydrogen_bonding" class="mw-redirect" title="Hydrogen bonding">hydrogen bonding</a>, and <a href="/wiki/Van_der_Waals_force" title="Van der Waals force">van der Waals forces</a>. Solvation of a solute by water is called hydration.<sup id="cite_ref-2" class="reference"><a href="#cite_note-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> </p><p>Solubility of <a href="/wiki/Solid" title="Solid">solid</a> compounds depends on a competition between <a href="/wiki/Lattice_energy" title="Lattice energy">lattice energy</a> and solvation, including entropy effects related to changes in the solvent structure.<sup id="cite_ref-3" class="reference"><a href="#cite_note-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Distinction_from_solubility">Distinction from solubility</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=1" title="Edit section: Distinction from solubility"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>By an <a href="/wiki/International_Union_of_Pure_and_Applied_Chemistry" title="International Union of Pure and Applied Chemistry">IUPAC</a> definition,<sup id="cite_ref-4" class="reference"><a href="#cite_note-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup> solvation is an interaction of a solute with the <a href="/wiki/Solvent" title="Solvent">solvent</a>, which leads to stabilization of the solute species in the <a href="/wiki/Solution_(chemistry)" title="Solution (chemistry)">solution</a>. In the solvated state, an ion or molecule in a solution is surrounded or <a href="/wiki/Complex_(chemistry)" class="mw-redirect" title="Complex (chemistry)">complexed</a> by solvent molecules. Solvated species can often be described by <a href="/wiki/Coordination_number" title="Coordination number">coordination number</a>, and the complex <a href="/wiki/Equilibrium_constant" title="Equilibrium constant">stability constants</a>. The concept of the solvation interaction can also be applied to an insoluble material, for example, solvation of functional groups on a surface of <a href="/wiki/Ion-exchange_resin" title="Ion-exchange resin">ion-exchange resin</a>. </p><p>Solvation is, in concept, distinct from <a href="/wiki/Solubility" title="Solubility">solubility</a>. Solvation or dissolution is a <a href="/wiki/Chemical_kinetics" title="Chemical kinetics">kinetic</a> process and is quantified by its rate. Solubility quantifies the <a href="/wiki/Dynamic_equilibrium" title="Dynamic equilibrium">dynamic equilibrium</a> state achieved when the rate of dissolution equals the rate of <a href="/wiki/Precipitation_(chemistry)" title="Precipitation (chemistry)">precipitation</a>. The consideration of the units makes the distinction clearer. The typical unit for dissolution rate is mol/s. The units for solubility express a concentration: mass per volume (mg/mL), molarity (mol/L), etc.<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (August 2022)">citation needed</span></a></i>]</sup> </p> <div class="mw-heading mw-heading2"><h2 id="Solvents_and_intermolecular_interactions">Solvents and intermolecular interactions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=2" title="Edit section: Solvents and intermolecular interactions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Solvation involves different types of intermolecular interactions: </p> <ul><li>Hydrogen bonding</li> <li>Ion–dipole interactions</li> <li>The van der Waals forces, which consist of dipole–dipole, dipole–induced dipole, and induced dipole–induced dipole interactions.</li></ul> <p>Which of these forces are at play depends on the molecular structure and properties of the solvent and solute. The similarity or complementary character of these properties between solvent and solute determines how well a solute can be solvated by a particular solvent. </p> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Nile_red_01.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Nile_red_01.jpg/220px-Nile_red_01.jpg" decoding="async" width="220" height="145" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Nile_red_01.jpg/330px-Nile_red_01.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/96/Nile_red_01.jpg/440px-Nile_red_01.jpg 2x" data-file-width="2900" data-file-height="1913" /></a><figcaption><a href="/wiki/Nile_red" title="Nile red">Nile red</a> at daylight (top row) and UV-light (second row) in different solvents. From left to right: 1. Water, 2. Methanol, 3. Ethanol, 4. Acetonitrile, 5. Dimethylformamide, 6. Acetone, 7. Ethylacetate, 8. Dichlormethane 9. n-Hexane, 10. Methyl-tert-Butylether, 11. Cyclohexane, 12. Toluene. Photographer: Armin Kübelbeck, CC-BY-SA, Wikimedia Commons</figcaption></figure> <p>Solvent <a href="/wiki/Chemical_polarity" title="Chemical polarity">polarity</a> is the most important factor in determining how well it solvates a particular solute. Polar solvents have molecular dipoles, meaning that part of the solvent molecule has more electron density than another part of the molecule. The part with more electron density will experience a partial negative charge while the part with less electron density will experience a partial positive charge. Polar solvent molecules can solvate polar solutes and ions because they can orient the appropriate partially charged portion of the molecule towards the solute through electrostatic attraction. This stabilizes the system and creates a <a href="/wiki/Solvation_shell" title="Solvation shell">solvation shell</a> (or hydration shell in the case of water) around each particle of solute. The solvent molecules in the immediate vicinity of a solute particle often have a much different ordering than the rest of the solvent, and this area of differently ordered solvent molecules is called the cybotactic region.<sup id="cite_ref-Anslyn_&_Dougherty_5-0" class="reference"><a href="#cite_note-Anslyn_&_Dougherty-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> Water is the most common and well-studied polar solvent, but others exist, such as <a href="/wiki/Ethanol" title="Ethanol">ethanol</a>, <a href="/wiki/Methanol" title="Methanol">methanol</a>, <a href="/wiki/Acetone" title="Acetone">acetone</a>, <a href="/wiki/Acetonitrile" title="Acetonitrile">acetonitrile</a>, and <a href="/wiki/Dimethyl_sulfoxide" title="Dimethyl sulfoxide">dimethyl sulfoxide</a>. Polar solvents are often found to have a high <a href="/wiki/Dielectric_constant" class="mw-redirect" title="Dielectric constant">dielectric constant</a>, although other solvent scales are also used to classify solvent polarity. Polar solvents can be used to dissolve inorganic or ionic compounds such as salts. The <a href="/wiki/Electrical_resistivity_and_conductivity" title="Electrical resistivity and conductivity">conductivity</a> of a solution depends on the solvation of its ions. Nonpolar solvents cannot solvate ions, and ions will be found as ion pairs. </p><p>Hydrogen bonding among solvent and solute molecules depends on the ability of each to accept H-bonds, donate H-bonds, or both. Solvents that can donate H-bonds are referred to as protic, while solvents that do not contain a polarized bond to a hydrogen atom and cannot donate a hydrogen bond are called aprotic. H-bond donor ability is classified on a scale (α).<sup id="cite_ref-6" class="reference"><a href="#cite_note-6"><span class="cite-bracket">[</span>6<span class="cite-bracket">]</span></a></sup> Protic solvents can solvate solutes that can accept hydrogen bonds. Similarly, solvents that can accept a hydrogen bond can solvate H-bond-donating solutes. The hydrogen bond acceptor ability of a solvent is classified on a scale (β).<sup id="cite_ref-7" class="reference"><a href="#cite_note-7"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup> Solvents such as water can both donate and accept hydrogen bonds, making them excellent at solvating solutes that can donate or accept (or both) H-bonds. </p><p>Some chemical compounds experience <a href="/wiki/Solvatochromism" title="Solvatochromism">solvatochromism</a>, which is a change in color due to solvent polarity. This phenomenon illustrates how different solvents interact differently with the same solute. Other <a href="/wiki/Solvent_effects" title="Solvent effects">solvent effects</a> include conformational or isomeric preferences and changes in the acidity of a solute. </p> <div class="mw-heading mw-heading2"><h2 id="Solvation_energy_and_thermodynamic_considerations">Solvation energy and thermodynamic considerations</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=3" title="Edit section: Solvation energy and thermodynamic considerations"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The solvation process will be thermodynamically favored only if the overall <a href="/wiki/Gibbs_energy" class="mw-redirect" title="Gibbs energy">Gibbs energy</a> of the solution is decreased, compared to the Gibbs energy of the separated solvent and solid (or gas or liquid). This means that the change in <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> minus the change in <a href="/wiki/Entropy" title="Entropy">entropy</a> (multiplied by the absolute temperature) is a negative value, or that the Gibbs energy of the system decreases. A negative Gibbs energy indicates a spontaneous process but does not provide information about the rate of dissolution. </p><p>Solvation involves multiple steps with different energy consequences. First, a cavity must form in the solvent to make space for a solute. This is both entropically and enthalpically unfavorable, as solvent ordering increases and solvent-solvent interactions decrease. Stronger interactions among solvent molecules leads to a greater enthalpic penalty for cavity formation. Next, a particle of solute must separate from the bulk. This is enthalpically unfavorable since solute-solute interactions decrease, but when the solute particle enters the cavity, the resulting solvent-solute interactions are enthalpically favorable. Finally, as solute mixes into solvent, there is an entropy gain.<sup id="cite_ref-Anslyn_&_Dougherty_5-1" class="reference"><a href="#cite_note-Anslyn_&_Dougherty-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p><p><span typeof="mw:File"><a href="/wiki/File:Effect_of_solvent_on_solubility.png" class="mw-file-description" title="Solvation of a solute by solvent"><img alt="Solvation of a solute by solvent" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Effect_of_solvent_on_solubility.png/600px-Effect_of_solvent_on_solubility.png" decoding="async" width="600" height="91" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Effect_of_solvent_on_solubility.png/900px-Effect_of_solvent_on_solubility.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Effect_of_solvent_on_solubility.png/1200px-Effect_of_solvent_on_solubility.png 2x" data-file-width="1277" data-file-height="194" /></a></span> </p><p>The <a href="/wiki/Enthalpy_of_solution" class="mw-redirect" title="Enthalpy of solution">enthalpy of solution</a> is the solution enthalpy minus the enthalpy of the separate systems, whereas the entropy of solution is the corresponding difference in <a href="/wiki/Entropy" title="Entropy">entropy</a>. The solvation energy (change in <a href="/wiki/Gibbs_free_energy" title="Gibbs free energy">Gibbs free energy</a>) is the change in enthalpy minus the product of temperature (in <a href="/wiki/Kelvin" title="Kelvin">Kelvin</a>) times the change in entropy. Gases have a negative entropy of solution, due to the decrease in gaseous volume as gas dissolves. Since their enthalpy of solution does not decrease too much with temperature, and their entropy of solution is negative and does not vary appreciably with temperature, most gases are less soluble at higher temperatures. </p><p>Enthalpy of solvation can help explain why solvation occurs with some ionic lattices but not with others. The difference in energy between that which is necessary to release an ion from its lattice and the energy given off when it combines with a solvent molecule is called the <a href="/wiki/Enthalpy_change_of_solution" title="Enthalpy change of solution">enthalpy change of solution</a>. A <a href="/wiki/Negative_number" title="Negative number">negative</a> value for the enthalpy change of solution corresponds to an ion that is likely to dissolve, whereas a high <a href="/wiki/Positive_number" class="mw-redirect" title="Positive number">positive</a> value means that solvation will not occur. It is possible that an ion will dissolve even if it has a positive enthalpy value. The extra energy required comes from the increase in <a href="/wiki/Entropy" title="Entropy">entropy</a> that results when the ion dissolves. The introduction of entropy makes it harder to determine by calculation alone whether a substance will dissolve or not. A quantitative measure for solvation power of solvents is given by <a href="/wiki/Donor_number" title="Donor number">donor numbers</a>.<sup id="cite_ref-8" class="reference"><a href="#cite_note-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup> </p><p>Although early thinking was that a higher ratio of a cation's ion charge to <a href="/wiki/Ionic_radius" title="Ionic radius">ionic radius</a>, or the charge density, resulted in more solvation, this does not stand up to scrutiny for ions like iron(III) or <a href="/wiki/Lanthanide" title="Lanthanide">lanthanides</a> and <a href="/wiki/Actinide" title="Actinide">actinides</a>, which are readily hydrolyzed to form insoluble (hydrous) oxides. As these are solids, it is apparent that they are not solvated. </p><p>Strong solvent–solute interactions make the process of solvation more favorable. One way to compare how favorable the dissolution of a solute is in different solvents is to consider the free energy of transfer. The free energy of transfer quantifies the free energy difference between dilute solutions of a solute in two different solvents. This value essentially allows for comparison of solvation energies without including solute-solute interactions.<sup id="cite_ref-Anslyn_&_Dougherty_5-2" class="reference"><a href="#cite_note-Anslyn_&_Dougherty-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p><p>In general, thermodynamic analysis of solutions is done by modeling them as reactions. For example, if you add sodium chloride to water, the salt will dissociate into the ions sodium(+aq) and chloride(-aq). The <a href="/wiki/Equilibrium_constant" title="Equilibrium constant">equilibrium constant</a> for this dissociation can be predicted by the change in Gibbs energy of this reaction. </p><p>The <a href="/wiki/Born_equation" title="Born equation">Born equation</a> is used to estimate Gibbs free energy of solvation of a gaseous ion. </p><p>Recent simulation studies have shown that the variation in solvation energy between the ions and the surrounding water molecules underlies the mechanism of the <a href="/wiki/Hofmeister_series" title="Hofmeister series">Hofmeister series</a>.<sup id="cite_ref-9" class="reference"><a href="#cite_note-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-article-1_1-1" class="reference"><a href="#cite_note-article-1-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Macromolecules_and_assemblies">Macromolecules and assemblies</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=4" title="Edit section: Macromolecules and assemblies"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Solvation (specifically, <a href="/wiki/Hydrate" title="Hydrate">hydration</a>) is important for many biological structures and processes. For instance, solvation of ions and/or of charged macromolecules, like <a href="/wiki/DNA" title="DNA">DNA</a> and proteins, in aqueous solutions influences the formation of heterogeneous assemblies, which may be responsible for biological function.<sup id="cite_ref-10" class="reference"><a href="#cite_note-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> As another example, <a href="/wiki/Protein_folding" title="Protein folding">protein folding</a> occurs spontaneously, in part because of a favorable change in the interactions between the protein and the surrounding water molecules. Folded proteins are stabilized by 5-10 kcal/mol relative to the <a href="/wiki/Random_coil" title="Random coil">unfolded state</a> due to a combination of solvation and the <a href="/wiki/Enthalpy_of_fusion" title="Enthalpy of fusion">stronger intramolecular interactions in the folded protein structure</a>, including <a href="/wiki/H-bonds" class="mw-redirect" title="H-bonds">hydrogen bonding</a>.<sup id="cite_ref-11" class="reference"><a href="#cite_note-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> Minimizing the number of <a href="/wiki/Hydrophobic" class="mw-redirect" title="Hydrophobic">hydrophobic</a> side chains exposed to water by burying them in the center of a folded protein is a driving force related to solvation. </p><p>Solvation also affects <a href="/wiki/Host%E2%80%93guest_chemistry" title="Host–guest chemistry">host–guest complexation</a>. Many host molecules have a hydrophobic pore that readily encapsulates a hydrophobic guest. These interactions can be used in applications such as drug delivery, such that a hydrophobic drug molecule can be delivered in a biological system without needing to covalently modify the drug in order to solubilize it. Binding constants for <a href="/wiki/Inclusion_compound" class="mw-redirect" title="Inclusion compound">host–guest complexes</a> depend on the polarity of the solvent.<sup id="cite_ref-12" class="reference"><a href="#cite_note-12"><span class="cite-bracket">[</span>12<span class="cite-bracket">]</span></a></sup> </p><p>Hydration affects electronic and vibrational properties of biomolecules.<sup id="cite_ref-13" class="reference"><a href="#cite_note-13"><span class="cite-bracket">[</span>13<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-14" class="reference"><a href="#cite_note-14"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Importance_of_solvation_in_computer_simulations">Importance of solvation in computer simulations</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=5" title="Edit section: Importance of solvation in computer simulations"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Due to the importance of the effects of solvation on the structure of macromolecules, early computer simulations which attempted to model their behaviors without including the effects of solvent (<i>in vacuo</i>) could yield poor results when compared with experimental data obtained in solution. Small molecules may also adopt more compact conformations when simulated <i>in vacuo</i>; this is due to favorable <a href="/wiki/Van_der_Waals_force" title="Van der Waals force">van der Waals interactions</a> and intramolecular electrostatic interactions which would be dampened in the presence of a solvent. </p><p>As computer power increased, it became possible to try and incorporate the effects of solvation within a simulation and the simplest way to do this is to surround the molecule being simulated with a "skin" of solvent molecules, akin to simulating the molecule within a drop of solvent if the skin is sufficiently deep.<sup id="cite_ref-15" class="reference"><a href="#cite_note-15"><span class="cite-bracket">[</span>15<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=6" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1184024115">.mw-parser-output .div-col{margin-top:0.3em;column-width:30em}.mw-parser-output .div-col-small{font-size:90%}.mw-parser-output .div-col-rules{column-rule:1px solid #aaa}.mw-parser-output .div-col dl,.mw-parser-output .div-col ol,.mw-parser-output .div-col ul{margin-top:0}.mw-parser-output .div-col li,.mw-parser-output .div-col dd{page-break-inside:avoid;break-inside:avoid-column}</style><div class="div-col" style="column-width: 15em;"> <ul><li><a href="/wiki/Born_equation" title="Born equation">Born equation</a></li> <li><a href="/wiki/Saturated_solution" class="mw-redirect" title="Saturated solution">Saturated solution</a></li> <li><a href="/wiki/Solubility_equilibrium" title="Solubility equilibrium">Solubility equilibrium</a></li> <li><a href="/wiki/Solvent_models" class="mw-redirect" title="Solvent models">Solvent models</a></li> <li><a href="/wiki/Supersaturation" title="Supersaturation">Supersaturation</a></li> <li><a href="/wiki/Water_model" title="Water model">Water model</a></li></ul> </div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=7" title="Edit section: References"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-article-1-1"><span class="mw-cite-backlink">^ <a href="#cite_ref-article-1_1-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-article-1_1-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><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 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.id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite 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B</i>. <b>121</b> (34): 8195–8202. <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%2Facs.jpcb.7b04297">10.1021/acs.jpcb.7b04297</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/28816050">28816050</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Phys.+Chem.+B&rft.atitle=Coarse-Grained+Model+of+the+Dynamics+of+Electrolyte+Solutions&rft.volume=121&rft.issue=34&rft.pages=8195-8202&rft.date=2017&rft_id=info%3Adoi%2F10.1021%2Facs.jpcb.7b04297&rft_id=info%3Apmid%2F28816050&rft.au=M.+Andreev&rft.au=A.+Chremos&rft.au=J.+de+Pablo&rft.au=J.+F.+Douglas&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> <li id="cite_note-10"><span class="mw-cite-backlink"><b><a href="#cite_ref-10">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFA._ChremosJ._F._Douglas2018" class="citation journal cs1">A. 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Douglas (2018). <a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC6217855">"Polyelectrolyte association and solvation"</a>. <i>The Journal of Chemical Physics</i>. <b>149</b> (16): 163305. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/2018JChPh.149p3305C">2018JChPh.149p3305C</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1063%2F1.5030530">10.1063/1.5030530</a>. <a href="/wiki/PMC_(identifier)" class="mw-redirect" title="PMC (identifier)">PMC</a> <span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC6217855">6217855</a></span>. <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/30384680">30384680</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=The+Journal+of+Chemical+Physics&rft.atitle=Polyelectrolyte+association+and+solvation&rft.volume=149&rft.issue=16&rft.pages=163305&rft.date=2018&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC6217855%23id-name%3DPMC&rft_id=info%3Apmid%2F30384680&rft_id=info%3Adoi%2F10.1063%2F1.5030530&rft_id=info%3Abibcode%2F2018JChPh.149p3305C&rft.au=A.+Chremos&rft.au=J.+F.+Douglas&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC6217855&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> <li id="cite_note-11"><span class="mw-cite-backlink"><b><a href="#cite_ref-11">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFPaceShirleyMcNuttGajiwala1996" class="citation journal cs1">Pace, CN; Shirley, BA; McNutt, M; Gajiwala, K (1996). <a rel="nofollow" class="external text" href="https://doi.org/10.1096%2Ffasebj.10.1.8566551">"Forces contributing to the conformational stability of proteins"</a>. <i>FASEB Journal</i>. <b>10</b> (1): 75–83. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://doi.org/10.1096%2Ffasebj.10.1.8566551">10.1096/fasebj.10.1.8566551</a></span>. <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/8566551">8566551</a>. <a href="/wiki/S2CID_(identifier)" class="mw-redirect" title="S2CID (identifier)">S2CID</a> <a rel="nofollow" class="external text" href="https://api.semanticscholar.org/CorpusID:20021399">20021399</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=FASEB+Journal&rft.atitle=Forces+contributing+to+the+conformational+stability+of+proteins&rft.volume=10&rft.issue=1&rft.pages=75-83&rft.date=1996&rft_id=https%3A%2F%2Fapi.semanticscholar.org%2FCorpusID%3A20021399%23id-name%3DS2CID&rft_id=info%3Apmid%2F8566551&rft_id=info%3Adoi%2F10.1096%2Ffasebj.10.1.8566551&rft.aulast=Pace&rft.aufirst=CN&rft.au=Shirley%2C+BA&rft.au=McNutt%2C+M&rft.au=Gajiwala%2C+K&rft_id=https%3A%2F%2Fdoi.org%2F10.1096%252Ffasebj.10.1.8566551&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> <li id="cite_note-12"><span class="mw-cite-backlink"><b><a href="#cite_ref-12">^</a></b></span> <span class="reference-text">Steed, J. W. and Atwood, J. L. (2013) Supramolecular Chemistry. 2nd ed. Wiley. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/1118681509" title="Special:BookSources/1118681509">1118681509</a>, 9781118681503.</span> </li> <li id="cite_note-13"><span class="mw-cite-backlink"><b><a href="#cite_ref-13">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMashaghi_Alireza2012" class="citation journal cs1">Mashaghi Alireza; et al. (2012). <a rel="nofollow" class="external text" href="https://doi.org/10.1063%2F1.3694280">"Hydration strongly affects the molecular and electronic structure of membrane phospholipids"</a>. <i>J. Chem. Phys</i>. <b>136</b> (11): 114709. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/2012JChPh.136k4709M">2012JChPh.136k4709M</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://doi.org/10.1063%2F1.3694280">10.1063/1.3694280</a></span>. <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/22443792">22443792</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Chem.+Phys.&rft.atitle=Hydration+strongly+affects+the+molecular+and+electronic+structure+of+membrane+phospholipids&rft.volume=136&rft.issue=11&rft.pages=114709&rft.date=2012&rft_id=info%3Apmid%2F22443792&rft_id=info%3Adoi%2F10.1063%2F1.3694280&rft_id=info%3Abibcode%2F2012JChPh.136k4709M&rft.au=Mashaghi+Alireza&rft_id=https%3A%2F%2Fdoi.org%2F10.1063%252F1.3694280&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> <li id="cite_note-14"><span class="mw-cite-backlink"><b><a href="#cite_ref-14">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBonn_Mischa2012" class="citation journal cs1">Bonn Mischa; et al. (2012). "Interfacial Water Facilitates Energy Transfer by Inducing Extended Vibrations in Membrane Lipids". <i>J Phys Chem</i>. <b>116</b> (22): 6455–6460. <a href="/wiki/CiteSeerX_(identifier)" class="mw-redirect" title="CiteSeerX (identifier)">CiteSeerX</a> <span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://citeseerx.ist.psu.edu/viewdoc/summary?doi=10.1.1.709.5345">10.1.1.709.5345</a></span>. <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%2Fjp302478a">10.1021/jp302478a</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/22594454">22594454</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J+Phys+Chem&rft.atitle=Interfacial+Water+Facilitates+Energy+Transfer+by+Inducing+Extended+Vibrations+in+Membrane+Lipids&rft.volume=116&rft.issue=22&rft.pages=6455-6460&rft.date=2012&rft_id=https%3A%2F%2Fciteseerx.ist.psu.edu%2Fviewdoc%2Fsummary%3Fdoi%3D10.1.1.709.5345%23id-name%3DCiteSeerX&rft_id=info%3Apmid%2F22594454&rft_id=info%3Adoi%2F10.1021%2Fjp302478a&rft.au=Bonn+Mischa&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> <li id="cite_note-15"><span class="mw-cite-backlink"><b><a href="#cite_ref-15">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLeach2001" class="citation book cs1">Leach, Andrew R. (2001). <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/45008511"><i>Molecular modelling : principles and applications</i></a> (2nd ed.). Harlow, England: Prentice Hall. p. 320. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-582-38210-6" title="Special:BookSources/0-582-38210-6"><bdi>0-582-38210-6</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/45008511">45008511</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Molecular+modelling+%3A+principles+and+applications&rft.place=Harlow%2C+England&rft.pages=320&rft.edition=2nd&rft.pub=Prentice+Hall&rft.date=2001&rft_id=info%3Aoclcnum%2F45008511&rft.isbn=0-582-38210-6&rft.aulast=Leach&rft.aufirst=Andrew+R.&rft_id=https%3A%2F%2Fwww.worldcat.org%2Foclc%2F45008511&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></span> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="Further_reading">Further reading</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=8" title="Edit section: Further reading"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFDogonadze1985–88" class="citation book cs1 cs1-prop-year-range-abbreviated"><a href="/wiki/Revaz_Dogonadze" title="Revaz Dogonadze">Dogonadze, Revaz</a>; et al., eds. (1985–88). <i>The Chemical Physics of Solvation</i> (3 vol. ed.). Amsterdam: Elsevier.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Chemical+Physics+of+Solvation&rft.place=Amsterdam&rft.edition=3+vol.&rft.pub=Elsevier&rft.date=1985%2F1988&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-444-42551-9" title="Special:BookSources/0-444-42551-9">0-444-42551-9</a> (part A), <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-444-42674-4" title="Special:BookSources/0-444-42674-4">0-444-42674-4</a> (part B), <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-444-42984-0" title="Special:BookSources/0-444-42984-0">0-444-42984-0</a> (Chemistry).</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFJiang_D.Urakawa_A.Yulikov_M.Mallat_T.2009" class="citation journal cs1">Jiang D.; Urakawa A.; Yulikov M.; Mallat T.; Jeschke G.; Baiker A. (2009). "Size selectivity of a copper metal-organic framework and origin of catalytic activity in epoxide alcoholysis". <i>Chemistry: A European Journal</i>. <b>15</b> (45): 12255–62. <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%2Fchem.200901510">10.1002/chem.200901510</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/19806616">19806616</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chemistry%3A+A+European+Journal&rft.atitle=Size+selectivity+of+a+copper+metal-organic+framework+and+origin+of+catalytic+activity+in+epoxide+alcoholysis&rft.volume=15&rft.issue=45&rft.pages=12255-62&rft.date=2009&rft_id=info%3Adoi%2F10.1002%2Fchem.200901510&rft_id=info%3Apmid%2F19806616&rft.au=Jiang+D.&rft.au=Urakawa+A.&rft.au=Yulikov+M.&rft.au=Mallat+T.&rft.au=Jeschke+G.&rft.au=Baiker+A.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span> One example of a solvated MOF, where partial dissolution is described.</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSerafin2003" class="citation journal cs1">Serafin, J.M. (October 2003). <span class="id-lock-subscription" title="Paid subscription required"><a rel="nofollow" class="external text" href="http://pubs.acs.org/doi/pdf/10.1021/ed080p1194">"Transfer Free Energy and the Hydrophobic Effect"</a></span>. <i>J. Chem. Educ</i>. <b>80</b> (10): 1194–1196. <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%2Fed080p1194">10.1021/ed080p1194</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Chem.+Educ.&rft.atitle=Transfer+Free+Energy+and+the+Hydrophobic+Effect&rft.volume=80&rft.issue=10&rft.pages=1194-1196&rft.date=2003-10&rft_id=info%3Adoi%2F10.1021%2Fed080p1194&rft.aulast=Serafin&rft.aufirst=J.M.&rft_id=http%3A%2F%2Fpubs.acs.org%2Fdoi%2Fpdf%2F10.1021%2Fed080p1194&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASolvation" class="Z3988"></span></li></ul> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Solvation&action=edit&section=9" title="Edit section: External links"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1235681985">.mw-parser-output .side-box{margin:4px 0;box-sizing:border-box;border:1px solid #aaa;font-size:88%;line-height:1.25em;background-color:var(--background-color-interactive-subtle,#f8f9fa);display:flow-root}.mw-parser-output .side-box-abovebelow,.mw-parser-output .side-box-text{padding:0.25em 0.9em}.mw-parser-output .side-box-image{padding:2px 0 2px 0.9em;text-align:center}.mw-parser-output .side-box-imageright{padding:2px 0.9em 2px 0;text-align:center}@media(min-width:500px){.mw-parser-output .side-box-flex{display:flex;align-items:center}.mw-parser-output .side-box-text{flex:1;min-width:0}}@media(min-width:720px){.mw-parser-output .side-box{width:238px}.mw-parser-output .side-box-right{clear:right;float:right;margin-left:1em}.mw-parser-output .side-box-left{margin-right:1em}}</style><style data-mw-deduplicate="TemplateStyles:r1237033735">@media print{body.ns-0 .mw-parser-output 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