{"id":248292,"date":"2025-07-08T09:36:47","date_gmt":"2025-07-08T09:36:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=248292"},"modified":"2025-07-08T09:36:49","modified_gmt":"2025-07-08T09:36:49","slug":"a-solution-of-h2so4aq-with-a-molal-concentration-of-3-97-m-has-a-density-of-1-216-g-ml","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/08\/a-solution-of-h2so4aq-with-a-molal-concentration-of-3-97-m-has-a-density-of-1-216-g-ml\/","title":{"rendered":"A solution of\u00a0H2SO4(aq)\u00a0with a molal concentration of\u00a03.97\u00a0m\u00a0has a density of\u00a01.216\u00a0g\/mL."},"content":{"rendered":"\n
A solution of H2SO4(aq) with a molal concentration of 3.97 m has a density of 1.216 g\/mL.<\/pre>\n\n\n\n
\"\"<\/figure>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
3.47 M<\/strong><\/p>\n\n\n\n
To determine the molar concentration (molarity) from the molal concentration (molality), we need to find the number of moles of solute in one liter of the solution. The key difference between these two concentration units is their denominator: molarity uses the volume of the solution, while molality uses the mass of the solvent.<\/p>\n\n\n\n
Here is the step by step conversion:<\/p>\n\n\n\n
    \n
  1. Assume a Basis:<\/strong>\u00a0To make the calculation straightforward, we will assume we have a sample of the solution that contains exactly 1 kg (1000 g) of solvent (water).<\/li>\n\n\n\n
  2. Find Moles of Solute:<\/strong>\u00a0The given molality is 3.97 m, which means there are 3.97 moles of H\u2082SO\u2084 for every 1 kg of water. So, our assumed sample contains 3.97 moles of H\u2082SO\u2084.<\/li>\n\n\n\n
  3. Find Mass of Solute:<\/strong>\u00a0We need to calculate the mass of 3.97 moles of H\u2082SO\u2084. First, we find the molar mass of H\u2082SO\u2084:\n
      \n
    • H: 2 \u00d7 1.008\u00a0g\/mol\u00a0= 2.016\u00a0g\/mol<\/li>\n\n\n\n
    • S: 1 \u00d7 32.06\u00a0g\/mol\u00a0= 32.06\u00a0g\/mol<\/li>\n\n\n\n
    • O: 4 \u00d7 16.00\u00a0g\/mol\u00a0= 64.00\u00a0g\/mol<\/li>\n\n\n\n
    • Molar Mass = 98.076\u00a0g\/mol
      Now, calculate the mass of the solute:
      Mass of H\u2082SO\u2084 = 3.97 mol \u00d7 98.076\u00a0g\/mol\u00a0= 389.36 g<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Find Total Mass of Solution:<\/strong>\u00a0The total mass of the solution is the sum of the mass of the solvent and the mass of the solute.
      Total Mass = 1000 g (solvent) + 389.36 g (solute) = 1389.36 g<\/li>\n\n\n\n
    • Find Volume of Solution:<\/strong>\u00a0Using the given density of the solution (1.216 g\/mL), we can find the volume.
      Volume = Mass \/ Density = 1389.36 g \/ 1.216 g\/mL = 1142.56 mL
      To calculate molarity, this volume must be in liters:
      Volume = 1142.56 mL \/ 1000 mL\/L = 1.14256 L<\/li>\n\n\n\n
    • Calculate Molarity:<\/strong>\u00a0Molarity is moles of solute divided by liters of solution.
      Molarity (M) = 3.97 mol \/ 1.14256 L = 3.474 M<\/li>\n<\/ol>\n\n\n\n
      Rounding to three significant figures, which is consistent with the given molality, the molar concentration is 3.47 M.<\/p>\n\n\n\n
      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
      A solution of H2SO4(aq) with a molal concentration of 3.97 m has a density of 1.216 g\/mL. The Correct Answer and Explanation is: 3.47 M To determine the molar concentration (molarity) from the molal concentration (molality), we need to find the number of moles of solute in one liter of the solution. The key difference between these two concentration units is their […]<\/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-248292","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248292","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=248292"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248292\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=248292"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=248292"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=248292"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}