{"id":257215,"date":"2025-07-16T19:49:40","date_gmt":"2025-07-16T19:49:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=257215"},"modified":"2025-07-16T19:49:42","modified_gmt":"2025-07-16T19:49:42","slug":"calculate-the-molar-mass-of-ammonium-sulfate-nhaasoa","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/16\/calculate-the-molar-mass-of-ammonium-sulfate-nhaasoa\/","title":{"rendered":"Calculate the molar mass of ammonium sulfate – (NH\u00e2\u201a\u201e)\u00e2\u201a\u201aSO\u00e2\u201a\u201e"},"content":{"rendered":"\n

Calculate the molar mass of ammonium sulfate – (NH\u00e2\u201a\u201e)\u00e2\u201a\u201aSO\u00e2\u201a\u201e<\/p>\n\n\n\n

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

To calculate the molar mass of ammonium sulfate, (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b, we need to sum the atomic masses of all the atoms in the formula.<\/p>\n\n\n\n

Step-by-step calculation:<\/h3>\n\n\n\n
    \n
  1. Ammonium ion (NH4)+(NH\u2084)^+(NH4\u200b)+<\/strong>:
    • The ammonium ion consists of one nitrogen atom and four hydrogen atoms.<\/li>
    • Atomic mass of nitrogen (N)<\/strong> = 14.01 g\/mol<\/li>
    • Atomic mass of hydrogen (H)<\/strong> = 1.008 g\/mol<\/li><\/ul>For (NH4)+(NH\u2084)^+(NH4\u200b)+:
      • Nitrogen: 1 \u00d7 14.01 = 14.01 g\/mol<\/li>
      • Hydrogen: 4 \u00d7 1.008 = 4.032 g\/mol<\/li><\/ul>The molar mass of (NH4)+(NH\u2084)^+(NH4\u200b)+ is: 14.01\u2009g\/mol+4.032\u2009g\/mol=18.042\u2009g\/mol14.01 \\, \\text{g\/mol} + 4.032 \\, \\text{g\/mol} = 18.042 \\, \\text{g\/mol}14.01g\/mol+4.032g\/mol=18.042g\/mol<\/li>\n\n\n\n
      • Sulfate ion SO42\u2212SO\u2084^{2-}SO42\u2212\u200b<\/strong>:
        • The sulfate ion consists of one sulfur atom and four oxygen atoms.<\/li>
        • Atomic mass of sulfur (S)<\/strong> = 32.07 g\/mol<\/li>
        • Atomic mass of oxygen (O)<\/strong> = 16.00 g\/mol<\/li><\/ul>For SO42\u2212SO\u2084^{2-}SO42\u2212\u200b:
          • Sulfur: 1 \u00d7 32.07 = 32.07 g\/mol<\/li>
          • Oxygen: 4 \u00d7 16.00 = 64.00 g\/mol<\/li><\/ul>The molar mass of SO42\u2212SO\u2084^{2-}SO42\u2212\u200b is: 32.07\u2009g\/mol+64.00\u2009g\/mol=96.07\u2009g\/mol32.07 \\, \\text{g\/mol} + 64.00 \\, \\text{g\/mol} = 96.07 \\, \\text{g\/mol}32.07g\/mol+64.00g\/mol=96.07g\/mol<\/li>\n\n\n\n
          • Molar mass of ammonium sulfate (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b<\/strong>:
            • The formula (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b indicates that there are 2 ammonium ions and 1 sulfate ion.<\/li>
            • Molar mass of 2 ammonium ions: 2\u00d718.042=36.084\u2009g\/mol2 \u00d7 18.042 = 36.084 \\, \\text{g\/mol}2\u00d718.042=36.084g\/mol<\/li>
            • Molar mass of 1 sulfate ion: 96.07\u2009g\/mol96.07 \\, \\text{g\/mol}96.07g\/mol<\/li><\/ul>So, the total molar mass is: 36.084\u2009g\/mol+96.07\u2009g\/mol=132.154\u2009g\/mol36.084 \\, \\text{g\/mol} + 96.07 \\, \\text{g\/mol} = 132.154 \\, \\text{g\/mol}36.084g\/mol+96.07g\/mol=132.154g\/mol<\/li>\n<\/ol>\n\n\n\n

              Final Answer:<\/h3>\n\n\n\n

              The molar mass of ammonium sulfate (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b is 132.154 g\/mol<\/strong>.<\/p>\n\n\n\n

              Explanation:<\/h3>\n\n\n\n
                \n
              • Molar mass is calculated by summing the masses of each atom in the compound.<\/li>\n\n\n\n
              • The periodic table provides the atomic masses, which we multiply by the number of atoms in the formula.<\/li>\n\n\n\n
              • This gives the total molar mass of the compound, which is essential for understanding stoichiometry in chemical reactions, such as when calculating how much ammonium sulfate is required for a reaction.<\/li>\n<\/ul>\n\n\n\n
                \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

                Calculate the molar mass of ammonium sulfate – (NH\u00e2\u201a\u201e)\u00e2\u201a\u201aSO\u00e2\u201a\u201e The Correct Answer and Explanation is: To calculate the molar mass of ammonium sulfate, (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b, we need to sum the atomic masses of all the atoms in the formula. Step-by-step calculation: Final Answer: The molar mass of ammonium sulfate (NH4)2SO4(NH\u2084)_2SO\u2084(NH4\u200b)2\u200bSO4\u200b is 132.154 g\/mol. Explanation:<\/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-257215","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257215","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=257215"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257215\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=257215"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=257215"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=257215"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}