{"id":184730,"date":"2025-01-21T10:46:53","date_gmt":"2025-01-21T10:46:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184730"},"modified":"2025-01-21T10:46:55","modified_gmt":"2025-01-21T10:46:55","slug":"what-is-the-molar-solubility-of-calcium-fluoride-caf2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/what-is-the-molar-solubility-of-calcium-fluoride-caf2\/","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 solution? Ksp for calcium fluoride is 3.45 x 10-11. \u00c3\u201a\u00c2<br>What is the molar solubility of calcium fluoride, CaF2, in a solution of 0.25 M calcium nitrate, Ca(NO3)2<br>solution?<\/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 ( \\text{CaF}_2 ) in a solution of ( 0.25 \\, \\text{M} ) calcium nitrate (( \\text{Ca(NO}_3)_2 )), we need to account for the common ion effect caused by the ( \\text{Ca}^{2+} ) ions already present in the solution.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Write the dissociation equation 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 (( K_{sp} )) expression is:<br>[<br>K_{sp} = [\\text{Ca}^{2+}] [\\text{F}^-]^2<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Define the concentrations<\/h3>\n\n\n\n<p>Let the molar solubility of ( \\text{CaF}_2 ) be ( s ) (in moles per liter).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The concentration of ( \\text{Ca}^{2+} ) from ( \\text{CaF}_2 ) is ( s ), but there is already ( 0.25 \\, \\text{M} ) ( \\text{Ca}^{2+} ) from ( \\text{Ca(NO}_3)_2 ).<br>[<br>[\\text{Ca}^{2+}] = 0.25 + s<br>]<\/li>\n\n\n\n<li>The concentration of ( \\text{F}^- ) from ( \\text{CaF}_2 ) is ( 2s ).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Substitute into ( K_{sp} )<\/h3>\n\n\n\n<p>Given ( K_{sp} = 3.45 \\times 10^{-11} ),<br>[<br>3.45 \\times 10^{-11} = (0.25 + s)(2s)^2<br>]<\/p>\n\n\n\n<p>For small ( s ), ( 0.25 + s \\approx 0.25 ). Thus:<br>[<br>3.45 \\times 10^{-11} = (0.25)(4s^2)<br>]<\/p>\n\n\n\n<p>[<br>3.45 \\times 10^{-11} = 1.0s^2<br>]<\/p>\n\n\n\n<p>[<br>s^2 = 3.45 \\times 10^{-11}<br>]<\/p>\n\n\n\n<p>[<br>s = \\sqrt{3.45 \\times 10^{-11}} = 5.88 \\times 10^{-6} \\, \\text{M}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Interpretation<\/h3>\n\n\n\n<p>The molar solubility of ( \\text{CaF}_2 ) in a ( 0.25 \\, \\text{M} ) calcium nitrate solution is approximately ( 5.88 \\times 10^{-6} \\, \\text{M} ). The ( 0.25 \\, \\text{M} ) ( \\text{Ca}^{2+} ) suppresses the solubility significantly compared to pure water due to the common ion effect, which shifts the equilibrium toward the solid ( \\text{CaF}_2 ).<\/p>\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)2 solution? Ksp for calcium fluoride is 3.45 x 10-11. \u00c3\u201a\u00c2What is the molar solubility of calcium fluoride, CaF2, in a solution of 0.25 M calcium nitrate, Ca(NO3)2solution? The Correct Answer and Explanation is : To calculate the [&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-184730","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184730","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=184730"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184730\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184730"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184730"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184730"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}