{"id":257078,"date":"2025-07-16T17:57:09","date_gmt":"2025-07-16T17:57:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=257078"},"modified":"2025-07-16T17:57:11","modified_gmt":"2025-07-16T17:57:11","slug":"the-freezing-point-depression-constant-kf-of-benzene-is-5-12-k-kg-mol-1-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/16\/the-freezing-point-depression-constant-kf-of-benzene-is-5-12-k-kg-mol-1-2\/","title":{"rendered":"The freezing point depression constant (Kf) of benzene is 5.12 K kg mol-1."},"content":{"rendered":"\n<p>The freezing point depression constant (Kf) of benzene is 5.12 K kg mol-1. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off to two decimal places):<\/p>\n\n\n\n<p><em><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/em><\/p>\n\n\n\n<p>To calculate the freezing point depression (\u0394Tf\\Delta T_f\u0394Tf\u200b) of a solution, we use the formula:\u0394Tf=Kf\u00d7m\\Delta T_f = K_f \\times m\u0394Tf\u200b=Kf\u200b\u00d7m<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u0394Tf\\Delta T_f\u0394Tf\u200b is the freezing point depression,<\/li>\n\n\n\n<li>KfK_fKf\u200b is the freezing point depression constant,<\/li>\n\n\n\n<li>mmm is the molality of the solution.<\/li>\n<\/ul>\n\n\n\n<p>Given data:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The freezing point depression constant (KfK_fKf\u200b) for benzene is 5.12 K kg\/mol.<\/li>\n\n\n\n<li>The molality (mmm) of the solution is 0.078 m (mol of solute per kg of solvent).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Calculation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Substitute the given values into the formula<\/strong>: \u0394Tf=5.12\u2009K\u00a0kg\/mol\u00d70.078\u2009mol\/kg\\Delta T_f = 5.12 \\, \\text{K kg\/mol} \\times 0.078 \\, \\text{mol\/kg}\u0394Tf\u200b=5.12K\u00a0kg\/mol\u00d70.078mol\/kg<\/li>\n\n\n\n<li><strong>Perform the multiplication<\/strong>: \u0394Tf=0.39936\u2009K\\Delta T_f = 0.39936 \\, \\text{K}\u0394Tf\u200b=0.39936K<\/li>\n\n\n\n<li><strong>Round to two decimal places<\/strong>: \u0394Tf\u22480.40\u2009K\\Delta T_f \\approx 0.40 \\, \\text{K}\u0394Tf\u200b\u22480.40K<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The freezing point depression measures how much the freezing point of the solvent is lowered by the presence of a solute. In this case, benzene is the solvent, and the presence of a non-electrolyte solute lowers its freezing point by 0.40 K.<\/p>\n\n\n\n<p>Since the solute is non-electrolyte, it does not dissociate into ions in solution, meaning the molality directly contributes to the freezing point depression without any additional factors from ionization.<\/p>\n\n\n\n<p>This depression can help us understand the behavior of the solvent in the presence of a solute. It is important for understanding colligative properties, which depend on the number of solute particles present, rather than their specific identity.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-694.jpeg\" alt=\"\" class=\"wp-image-257079\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The freezing point depression constant (Kf) of benzene is 5.12 K kg mol-1. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off to two decimal places): The Correct Answer and Explanation is: To calculate the freezing point depression (\u0394Tf\\Delta T_f\u0394Tf\u200b) of a solution, we [&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-257078","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257078","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=257078"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257078\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=257078"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=257078"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=257078"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}