{"id":200065,"date":"2025-03-13T07:14:33","date_gmt":"2025-03-13T07:14:33","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=200065"},"modified":"2025-03-13T07:14:35","modified_gmt":"2025-03-13T07:14:35","slug":"assuming-100-dissociation","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/13\/assuming-100-dissociation\/","title":{"rendered":"Assuming 100% dissociation"},"content":{"rendered":"\n<p>Assuming 100% dissociation, calculate the freezing point (f) and boiling point (?b) of 3.29 ? AgNO3(aq).<\/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 determine the freezing point (Tf) and boiling point (Tb) of a 3.29 m AgNO\u2083(aq) solution, assuming 100% dissociation, we can apply the principles of colligative properties. These properties depend on the number of solute particles in a given amount of solvent, irrespective of the nature of the solute particles.<\/p>\n\n\n\n<p><strong>Step 1: Understanding the Dissociation of AgNO\u2083<\/strong><\/p>\n\n\n\n<p>Silver nitrate (AgNO\u2083) dissociates completely in water into silver ions (Ag\u207a) and nitrate ions (NO\u2083\u207b):<\/p>\n\n\n\n<p>[ \\text{AgNO\u2083} \\rightarrow \\text{Ag}^+ + \\text{NO}_3^- ]<\/p>\n\n\n\n<p>This dissociation results in two particles per formula unit, giving a van&#8217;t Hoff factor (i) of 2.<\/p>\n\n\n\n<p><strong>Step 2: Calculating Freezing Point Depression (\u0394Tf)<\/strong><\/p>\n\n\n\n<p>The freezing point depression is given by the formula:<\/p>\n\n\n\n<p>[ \\Delta T_f = i \\times K_f \\times m ]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( i ) is the van&#8217;t Hoff factor (2 for AgNO\u2083),<\/li>\n\n\n\n<li>( K_f ) is the cryoscopic constant (freezing point depression constant) for water, approximately 1.86 \u00b0C\u00b7kg\/mol,<\/li>\n\n\n\n<li>( m ) is the molality of the solution (3.29 mol\/kg).<\/li>\n<\/ul>\n\n\n\n<p>Plugging in the values:<\/p>\n\n\n\n<p>[ \\Delta T_f = 2 \\times 1.86\\,^\\circ\\text{C} \\cdot \\text{kg\/mol} \\times 3.29\\,\\text{mol\/kg} ]<br>[ \\Delta T_f = 12.22\\,^\\circ\\text{C} ]<\/p>\n\n\n\n<p>Therefore, the freezing point of the solution is:<\/p>\n\n\n\n<p>[ T_f = 0\\,^\\circ\\text{C} &#8211; 12.22\\,^\\circ\\text{C} = -12.22\\,^\\circ\\text{C} ]<\/p>\n\n\n\n<p><strong>Step 3: Calculating Boiling Point Elevation (\u0394Tb)<\/strong><\/p>\n\n\n\n<p>The boiling point elevation is calculated using:<\/p>\n\n\n\n<p>[ \\Delta T_b = i \\times K_b \\times m ]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_b ) is the ebullioscopic constant (boiling point elevation constant) for water, approximately 0.512 \u00b0C\u00b7kg\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Calculating:<\/p>\n\n\n\n<p>[ \\Delta T_b = 2 \\times 0.512\\,^\\circ\\text{C} \\cdot \\text{kg\/mol} \\times 3.29\\,\\text{mol\/kg} ]<br>[ \\Delta T_b = 3.37\\,^\\circ\\text{C} ]<\/p>\n\n\n\n<p>Thus, the boiling point of the solution is:<\/p>\n\n\n\n<p>[ T_b = 100\\,^\\circ\\text{C} + 3.37\\,^\\circ\\text{C} = 103.37\\,^\\circ\\text{C} ]<\/p>\n\n\n\n<p><strong>Conclusion<\/strong><\/p>\n\n\n\n<p>For a 3.29 m AgNO\u2083(aq) solution, assuming complete dissociation:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The freezing point is approximately -12.22\u202f\u00b0C.<\/li>\n\n\n\n<li>The boiling point is approximately 103.37\u202f\u00b0C.<\/li>\n<\/ul>\n\n\n\n<p>These changes are due to the presence of solute particles disrupting the formation of the solid lattice in freezing and affecting the vapor pressure in boiling.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Assuming 100% dissociation, calculate the freezing point (f) and boiling point (?b) of 3.29 ? AgNO3(aq). The correct answer and explanation is : To determine the freezing point (Tf) and boiling point (Tb) of a 3.29 m AgNO\u2083(aq) solution, assuming 100% dissociation, we can apply the principles of colligative properties. These properties depend on 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-200065","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/200065","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=200065"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/200065\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=200065"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=200065"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=200065"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}