{"id":184547,"date":"2025-01-21T06:45:50","date_gmt":"2025-01-21T06:45:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184547"},"modified":"2025-01-21T06:45:52","modified_gmt":"2025-01-21T06:45:52","slug":"assuming-equal-concentrations-and-complete-dissociation-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/assuming-equal-concentrations-and-complete-dissociation-2\/","title":{"rendered":"Assuming equal concentrations and complete dissociation"},"content":{"rendered":"\n<p>Assuming equal concentrations and complete dissociation, arrange these aqueous solutions by their freezing points. Highest freezing point<\/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>When arranging aqueous solutions by their freezing points, it&#8217;s essential to consider the <strong>colligative properties<\/strong> of solutions, specifically <strong>freezing point depression<\/strong>. This property depends on the number of solute particles in the solution, not the chemical identity of the solute.<\/p>\n\n\n\n<p>The key formula for freezing point depression is: \u0394Tf=i\u22c5Kf\u22c5m\\Delta T_f = i \\cdot K_f \\cdot m<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u0394Tf\\Delta T_f: Freezing point depression<\/li>\n\n\n\n<li>ii: Van &#8216;t Hoff factor (number of particles the solute dissociates into)<\/li>\n\n\n\n<li>KfK_f: Freezing point depression constant for the solvent<\/li>\n\n\n\n<li>mm: Molality of the solution<\/li>\n<\/ul>\n\n\n\n<p>For <strong>equal concentrations<\/strong> and assuming <strong>complete dissociation<\/strong>, the freezing point is primarily determined by the <strong>Van &#8216;t Hoff factor (ii)<\/strong>, which is the total number of particles produced when the solute dissociates.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Example Solutions:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>NaCl<\/strong>: Dissociates into 2 particles (i=2i = 2) NaCl\u2192Na++Cl\u2212\\text{NaCl} \\to \\text{Na}^+ + \\text{Cl}^-<\/li>\n\n\n\n<li><strong>K2_2SO4_4<\/strong>: Dissociates into 3 particles (i=3i = 3) K2SO4\u21922K++SO42\u2212\\text{K}_2\\text{SO}_4 \\to 2\\text{K}^+ + \\text{SO}_4^{2-}<\/li>\n\n\n\n<li><strong>CaCl2_2<\/strong>: Dissociates into 3 particles (i=3i = 3) CaCl2\u2192Ca2++2Cl\u2212\\text{CaCl}_2 \\to \\text{Ca}^{2+} + 2\\text{Cl}^-<\/li>\n\n\n\n<li><strong>Glucose (C6_6H12_{12}O6_6)<\/strong>: Does not dissociate (i=1i = 1).<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Freezing Point Order (Highest to Lowest):<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Glucose (i=1i = 1)<\/strong>: Least freezing point depression.<\/li>\n\n\n\n<li><strong>NaCl (i=2i = 2)<\/strong>.<\/li>\n\n\n\n<li><strong>K2_2SO4_4<\/strong> and <strong>CaCl2_2<\/strong> (i=3i = 3): Greatest freezing point depression (lowest freezing point).<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Glucose has the <strong>highest freezing point<\/strong> because it does not dissociate, producing only 1 particle per molecule. NaCl dissociates into 2 particles, leading to greater freezing point depression than glucose. Both K2_2SO4_4 and CaCl2_2 dissociate into 3 particles, causing the most significant freezing point depression and having the <strong>lowest freezing point<\/strong>.<\/p>\n\n\n\n<p>This demonstrates how the number of dissociated particles directly impacts the freezing point of solutions.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Assuming equal concentrations and complete dissociation, arrange these aqueous solutions by their freezing points. Highest freezing point The Correct Answer and Explanation is : When arranging aqueous solutions by their freezing points, it&#8217;s essential to consider the colligative properties of solutions, specifically freezing point depression. This property depends on the number of solute particles in [&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-184547","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184547","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=184547"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184547\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184547"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184547"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184547"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}