{"id":184732,"date":"2025-01-21T10:48:00","date_gmt":"2025-01-21T10:48:00","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184732"},"modified":"2025-01-21T10:48:01","modified_gmt":"2025-01-21T10:48:01","slug":"what-is-the-molar-solubility-of-calcium-fluoride-caf2-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/what-is-the-molar-solubility-of-calcium-fluoride-caf2-2\/","title":{"rendered":"What is the molar solubility of calcium fluoride, CaF2"},"content":{"rendered":"\n<p>What is the molar solubility of calcium fluoride, CaF2, in a solution of 0.25 M calcium nitrate, Ca(NO3)2<br>solution?<br>Ksp for calcium fluoride is 3.45 x 10-11.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate the molar solubility of calcium fluoride (( \\text{CaF}_2 )) in a ( 0.25 \\, \\text{M} ) calcium nitrate (( \\text{Ca(NO}_3\\text{)}_2 )) solution, we account for the common ion effect caused by ( \\text{Ca}^{2+} ) ions from ( \\text{Ca(NO}_3\\text{)}_2 ).<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Write the equilibrium expression for ( \\text{CaF}_2 ):<\/h3>\n\n\n\n<p>[<br>\\text{CaF}_2 (s) \\leftrightarrow \\text{Ca}^{2+} (aq) + 2 \\text{F}^- (aq)<br>]<\/p>\n\n\n\n<p>The solubility product constant (( K_\\text{sp} )) is:<br>[<br>K_\\text{sp} = [\\text{Ca}^{2+}][\\text{F}^-]^2<br>]<\/p>\n\n\n\n<p>Given ( K_\\text{sp} = 3.45 \\times 10^{-11} ), and the initial concentration of ( \\text{Ca}^{2+} ) from ( \\text{Ca(NO}_3\\text{)}_2 ) is ( 0.25 \\, \\text{M} ), the additional ( \\text{Ca}^{2+} ) from ( \\text{CaF}_2 ) is negligible.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Define solubility (( s )):<\/h3>\n\n\n\n<p>Let ( s ) be the molar solubility of ( \\text{CaF}_2 ) in the solution. Upon dissolution:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( [\\text{Ca}^{2+}] = 0.25 + s ) (approx. ( 0.25 \\, \\text{M} ), since ( s \\ll 0.25 ))<\/li>\n\n\n\n<li>( [\\text{F}^-] = 2s )<\/li>\n<\/ul>\n\n\n\n<p>Substituting into the ( K_\\text{sp} ) expression:<br>[<br>K_\\text{sp} = (0.25)(2s)^2<br>]<br>[<br>3.45 \\times 10^{-11} = (0.25)(4s^2)<br>]<br>[<br>s^2 = \\frac{3.45 \\times 10^{-11}}{1.0} = 3.45 \\times 10^{-11}<br>]<br>[<br>s = \\sqrt{3.45 \\times 10^{-11}} = 1.86 \\times 10^{-6} \\, \\text{M}<br>]<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The molar solubility of ( \\text{CaF}_2 ) in ( 0.25 \\, \\text{M} ) calcium nitrate solution is:<br>[<br>\\boxed{1.86 \\times 10^{-6} \\, \\text{M}}<br>]<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The ( \\text{Ca(NO}_3\\text{)}_2 ) provides a high initial ( \\text{Ca}^{2+} ) concentration, suppressing ( \\text{CaF}_2 ) dissolution due to the common ion effect.<\/li>\n\n\n\n<li>The equilibrium shifts to reduce ( \\text{F}^- ) concentration, drastically lowering the solubility.<\/li>\n\n\n\n<li>Using ( K_\\text{sp} ), we account for the interaction of ion concentrations in equilibrium.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>What is the molar solubility of calcium fluoride, CaF2, in a solution of 0.25 M calcium nitrate, Ca(NO3)2solution?Ksp for calcium fluoride is 3.45 x 10-11. The Correct Answer and Explanation is : To calculate the molar solubility of calcium fluoride (( \\text{CaF}_2 )) in a ( 0.25 \\, \\text{M} ) calcium nitrate (( \\text{Ca(NO}_3\\text{)}_2 )) [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-184732","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184732","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=184732"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184732\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184732"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184732"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184732"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}