{"id":164161,"date":"2024-11-09T14:01:58","date_gmt":"2024-11-09T14:01:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=164161"},"modified":"2024-11-09T14:02:00","modified_gmt":"2024-11-09T14:02:00","slug":"calculate-the-vant-hoff-factor-of-a-0-0500-m-formic-acid-solution-hco2h-which-begins-to-freeze-at-0-0984c","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/09\/calculate-the-vant-hoff-factor-of-a-0-0500-m-formic-acid-solution-hco2h-which-begins-to-freeze-at-0-0984c\/","title":{"rendered":"Calculate the van&#8217;t Hoff factor of a 0.0500 m formic acid solution (HCO2H) which begins to freeze at -0.0984\u00b0C"},"content":{"rendered":"\n<p>Calculate the van&#8217;t Hoff factor of a 0.0500 m formic acid solution (HCO2H) which begins to freeze at -0.0984\u00b0C. *\u0394Tf = KfCmi, Kf = -1.86 \u00b0C\/m<\/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 van\u2019t Hoff factor (i) for the given solution, we need to use the freezing point depression formula:<\/p>\n\n\n\n<p>[<br>\\Delta T_f = K_f \\cdot C_m \\cdot i<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(\\Delta T_f) is the freezing point depression (change in freezing point),<\/li>\n\n\n\n<li>(K_f) is the cryoscopic constant (given as -1.86 \u00b0C\/m),<\/li>\n\n\n\n<li>(C_m) is the molality of the solution (given as 0.0500 m),<\/li>\n\n\n\n<li>(i) is the van\u2019t Hoff factor (the number of particles into which a solute dissociates in solution).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Calculate the freezing point depression (\\Delta T_f)<\/h3>\n\n\n\n<p>The normal freezing point of water is 0.00\u00b0C. The solution begins to freeze at -0.0984\u00b0C, so the freezing point depression is:<\/p>\n\n\n\n<p>[<br>\\Delta T_f = 0.00\u00b0C &#8211; (-0.0984\u00b0C) = 0.0984\u00b0C<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Rearrange the freezing point depression equation to solve for (i)<\/h3>\n\n\n\n<p>The equation we have is:<\/p>\n\n\n\n<p>[<br>\\Delta T_f = K_f \\cdot C_m \\cdot i<br>]<\/p>\n\n\n\n<p>Rearranging to solve for (i):<\/p>\n\n\n\n<p>[<br>i = \\frac{\\Delta T_f}{K_f \\cdot C_m}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Plug in the known values<\/h3>\n\n\n\n<p>Now, substitute the values into the equation:<\/p>\n\n\n\n<p>[<br>i = \\frac{0.0984\u00b0C}{(-1.86\u00b0C\/m) \\cdot (0.0500 m)}<br>]<\/p>\n\n\n\n<p>[<br>i = \\frac{0.0984}{-0.093}<br>]<\/p>\n\n\n\n<p>[<br>i \\approx 1.06<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Interpretation of the result<\/h3>\n\n\n\n<p>The van\u2019t Hoff factor (i) is approximately 1.06. This suggests that formic acid (HCO2H) dissociates very slightly in solution, but not completely. A value of 1 would indicate no dissociation, while a value greater than 1 (like 1.06) suggests a small amount of dissociation into ions or particles.<\/p>\n\n\n\n<p>In the case of formic acid, it is a weak acid, so it partially dissociates into H\u207a and HCO\u2082\u207b ions. This result reflects the fact that the dissociation is minimal but contributes to the observed freezing point depression.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the van&#8217;t Hoff factor of a 0.0500 m formic acid solution (HCO2H) which begins to freeze at -0.0984\u00b0C. *\u0394Tf = KfCmi, Kf = -1.86 \u00b0C\/m The Correct Answer and Explanation is : To calculate the van\u2019t Hoff factor (i) for the given solution, we need to use the freezing point depression formula: [\\Delta T_f [&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-164161","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164161","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=164161"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164161\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=164161"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=164161"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=164161"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}