{"id":248344,"date":"2025-07-08T10:14:53","date_gmt":"2025-07-08T10:14:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=248344"},"modified":"2025-07-08T10:14:54","modified_gmt":"2025-07-08T10:14:54","slug":"a-solution-of-h2so4-with-a-molal-concentration-of-5-25m-has-a-density-of-1-266-g-ml-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/08\/a-solution-of-h2so4-with-a-molal-concentration-of-5-25m-has-a-density-of-1-266-g-ml-2\/","title":{"rendered":"A solution of H2SO4 with a molal concentration of 5.25m has a density of 1.266 g\/ml."},"content":{"rendered":"\n<p>A solution of H2SO4 with a molal concentration of 5.25m has a density of 1.266 g\/ml. what is the molar concentration of this solution?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the molar concentration (molarity) of a solution from its molality, we need to use the relationship between molality, molarity, and density.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Given:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molality (m) = 5.25 mol\/kg<\/li>\n\n\n\n<li>Density (d) = 1.266 g\/mL<\/li>\n\n\n\n<li>The molar mass of H2SO4 = 98.08 g\/mol<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Convert density from g\/mL to g\/L<\/h3>\n\n\n\n<p>The density is given in g\/mL, but we need it in g\/L to match the molarity units (mol\/L). Since there are 1000 mL in 1 L, we multiply the density by 1000:Density&nbsp;(g\/L)=1.266\u2009g\/mL\u00d71000=1266\u2009g\/L\\text{Density (g\/L)} = 1.266 \\, \\text{g\/mL} \\times 1000 = 1266 \\, \\text{g\/L}Density&nbsp;(g\/L)=1.266g\/mL\u00d71000=1266g\/L<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Convert molality to moles of solute per kilogram of solvent<\/h3>\n\n\n\n<p>Molality is defined as moles of solute per kilogram of solvent. We know that:Molality=moles&nbsp;of&nbsp;solutemass&nbsp;of&nbsp;solvent&nbsp;(kg)\\text{Molality} = \\frac{\\text{moles of solute}}{\\text{mass of solvent (kg)}}Molality=mass&nbsp;of&nbsp;solvent&nbsp;(kg)moles&nbsp;of&nbsp;solute\u200b<\/p>\n\n\n\n<p>This gives us the number of moles of H2SO4 per kilogram of water.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Convert mass of solution from g to kg<\/h3>\n\n\n\n<p>The mass of the solution can be calculated by the density and volume. Assuming 1 L of solution:Mass&nbsp;of&nbsp;solution=1266\u2009g\u2009(since&nbsp;we&nbsp;are&nbsp;considering&nbsp;1&nbsp;L&nbsp;of&nbsp;solution)\\text{Mass of solution} = 1266 \\, \\text{g} \\, \\text{(since we are considering 1 L of solution)}Mass&nbsp;of&nbsp;solution=1266g(since&nbsp;we&nbsp;are&nbsp;considering&nbsp;1&nbsp;L&nbsp;of&nbsp;solution)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Calculate the mass of the solvent (water)<\/h3>\n\n\n\n<p>The mass of the solvent (water) can be found by subtracting the mass of the solute (H2SO4) from the total mass of the solution.<\/p>\n\n\n\n<p>First, calculate the moles of H2SO4 in the solution:moles&nbsp;of&nbsp;H2SO4=5.25\u2009mol\/kg\u00d71\u2009kg=5.25\u2009mol\\text{moles of H2SO4} = 5.25 \\, \\text{mol\/kg} \\times 1 \\, \\text{kg} = 5.25 \\, \\text{mol}moles&nbsp;of&nbsp;H2SO4=5.25mol\/kg\u00d71kg=5.25mol<\/p>\n\n\n\n<p>Then, calculate the mass of H2SO4:Mass&nbsp;of&nbsp;H2SO4=5.25\u2009mol\u00d798.08\u2009g\/mol=514.92\u2009g\\text{Mass of H2SO4} = 5.25 \\, \\text{mol} \\times 98.08 \\, \\text{g\/mol} = 514.92 \\, \\text{g}Mass&nbsp;of&nbsp;H2SO4=5.25mol\u00d798.08g\/mol=514.92g<\/p>\n\n\n\n<p>Now, the mass of the solvent (water) is:Mass&nbsp;of&nbsp;water=1266\u2009g\u2212514.92\u2009g=751.08\u2009g=0.751\u2009kg\\text{Mass of water} = 1266 \\, \\text{g} &#8211; 514.92 \\, \\text{g} = 751.08 \\, \\text{g} = 0.751 \\, \\text{kg}Mass&nbsp;of&nbsp;water=1266g\u2212514.92g=751.08g=0.751kg<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 5: Calculate molarity (M)<\/h3>\n\n\n\n<p>Molarity is defined as moles of solute per liter of solution. We already know the number of moles of H2SO4 (5.25 mol) and the volume of the solution (1 L):Molarity=moles&nbsp;of&nbsp;H2SO4volume&nbsp;of&nbsp;solution&nbsp;(L)=5.25\u2009mol1\u2009L=5.25\u2009M\\text{Molarity} = \\frac{\\text{moles of H2SO4}}{\\text{volume of solution (L)}} = \\frac{5.25 \\, \\text{mol}}{1 \\, \\text{L}} = 5.25 \\, \\text{M}Molarity=volume&nbsp;of&nbsp;solution&nbsp;(L)moles&nbsp;of&nbsp;H2SO4\u200b=1L5.25mol\u200b=5.25M<\/p>\n\n\n\n<p>Thus, the molar concentration of the H2SO4 solution is <strong>5.25 M<\/strong>.<\/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-banner8-208.jpeg\" alt=\"\" class=\"wp-image-248345\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>A solution of H2SO4 with a molal concentration of 5.25m has a density of 1.266 g\/ml. what is the molar concentration of this solution? The Correct Answer and Explanation is: To find the molar concentration (molarity) of a solution from its molality, we need to use the relationship between molality, molarity, and density. Given: Step [&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-248344","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248344","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=248344"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248344\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=248344"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=248344"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=248344"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}