{"id":248288,"date":"2025-07-08T09:33:33","date_gmt":"2025-07-08T09:33:33","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=248288"},"modified":"2025-07-08T09:33:35","modified_gmt":"2025-07-08T09:33:35","slug":"a-solution-of-h2so4-with-a-molal-concentration-of-8-01-mol-kg-has-a-density-of-1-354-g-ml","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/08\/a-solution-of-h2so4-with-a-molal-concentration-of-8-01-mol-kg-has-a-density-of-1-354-g-ml\/","title":{"rendered":"A solution of H2SO4 with a molal concentration of 8.01 mol\/kg has a density of 1.354 g\/mL"},"content":{"rendered":"\n

A solution of H2SO4 with a molal concentration of 8.01 mol\/kg has a density of 1.354 g\/mL. What is the molar concentration of this solution<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To find the molar concentration of the solution, we need to follow a few steps using the information provided:<\/p>\n\n\n\n

Step 1: Understand what molal concentration is<\/h3>\n\n\n\n

Molality (m) is defined as the number of moles of solute (H\u2082SO\u2084 in this case) per kilogram of solvent. You are given that the solution has a molal concentration of 8.01 mol\/kg. This means that for every 1 kg of solvent, there are 8.01 moles of H\u2082SO\u2084.<\/p>\n\n\n\n

Step 2: Use the density to convert mass into volume<\/h3>\n\n\n\n

Next, we are given the density of the solution, which is 1.354 g\/mL. The density formula is: Density=MassVolume\\text{Density} = \\frac{\\text{Mass}}{\\text{Volume}}Density=VolumeMass\u200b<\/p>\n\n\n\n

Rearranging this formula to solve for volume: Volume=MassDensity\\text{Volume} = \\frac{\\text{Mass}}{\\text{Density}}Volume=DensityMass\u200b<\/p>\n\n\n\n

Let’s say we have 1 kg of solvent (1000 g), and from the molality definition, there will be 8.01 moles of H\u2082SO\u2084. Now, calculate the mass of the solution.<\/p>\n\n\n\n

    \n
  • Mass of solution<\/strong> = Mass of solvent + Mass of solute (H\u2082SO\u2084).<\/li>\n<\/ul>\n\n\n\n

    The molar mass of H\u2082SO\u2084 is 98.079 g\/mol. So:<\/p>\n\n\n\n

      \n
    • Mass of H\u2082SO\u2084 = 8.01 mol \u00d7 98.079 g\/mol = 785.1 g.<\/li>\n<\/ul>\n\n\n\n

      Thus, the total mass of the solution is:<\/p>\n\n\n\n

        \n
      • Total mass = 1000 g (solvent) + 785.1 g (solute) = 1785.1 g.<\/li>\n<\/ul>\n\n\n\n

        Now, we can calculate the volume using the density: Volume=1785.1\u2009g1.354\u2009g\/mL=1319.8\u2009mL=1.3198\u2009L.\\text{Volume} = \\frac{1785.1 \\, \\text{g}}{1.354 \\, \\text{g\/mL}} = 1319.8 \\, \\text{mL} = 1.3198 \\, \\text{L}.Volume=1.354g\/mL1785.1g\u200b=1319.8mL=1.3198L.<\/p>\n\n\n\n

        Step 3: Calculate molar concentration<\/h3>\n\n\n\n

        Molar concentration (M) is the number of moles of solute per liter of solution. The number of moles of H\u2082SO\u2084 is 8.01 mol (as given), and the volume of the solution is 1.3198 L. Therefore, the molar concentration is: M=8.01\u2009mol1.3198\u2009L=6.07\u2009mol\/L.M = \\frac{8.01 \\, \\text{mol}}{1.3198 \\, \\text{L}} = 6.07 \\, \\text{mol\/L}.M=1.3198L8.01mol\u200b=6.07mol\/L.<\/p>\n\n\n\n

        Conclusion:<\/h3>\n\n\n\n

        The molar concentration of the solution is 6.07 mol\/L<\/strong>.<\/p>\n\n\n\n

        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        A solution of H2SO4 with a molal concentration of 8.01 mol\/kg has a density of 1.354 g\/mL. What is the molar concentration of this solution The Correct Answer and Explanation is: To find the molar concentration of the solution, we need to follow a few steps using the information provided: Step 1: Understand what molal […]<\/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-248288","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248288","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=248288"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248288\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=248288"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=248288"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=248288"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}