{"id":184153,"date":"2025-01-19T11:09:38","date_gmt":"2025-01-19T11:09:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184153"},"modified":"2025-01-19T11:09:40","modified_gmt":"2025-01-19T11:09:40","slug":"calculate-the-molar-mass-of-phosphoric-acid-h3po4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/19\/calculate-the-molar-mass-of-phosphoric-acid-h3po4\/","title":{"rendered":"Calculate the molar mass of phosphoric acid H3PO4"},"content":{"rendered":"\n

Calculate the molar mass of phosphoric acid H3PO4.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n
\"\"<\/figure>\n\n\n\n

The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Molar Mass of Phosphoric Acid (H\u2083PO\u2084)<\/h3>\n\n\n\n

The molar mass of phosphoric acid is calculated by summing the atomic masses of its constituent atoms. The chemical formula H3PO4H_3PO_4 indicates it contains:<\/p>\n\n\n\n

    \n
  • Hydrogen (H):<\/strong> 3 atoms<\/li>\n\n\n\n
  • Phosphorus (P):<\/strong> 1 atom<\/li>\n\n\n\n
  • Oxygen (O):<\/strong> 4 atoms<\/li>\n<\/ul>\n\n\n\n

    Using the periodic table:<\/p>\n\n\n\n

      \n
    • Atomic mass of H = 1.01 g\/mol<\/li>\n\n\n\n
    • Atomic mass of P = 30.97 g\/mol<\/li>\n\n\n\n
    • Atomic mass of O = 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n

      Calculation:<\/h4>\n\n\n\n

      Molar mass=(3\u00d71.01)+(1\u00d730.97)+(4\u00d716.00)\\text{Molar mass} = (3 \\times 1.01) + (1 \\times 30.97) + (4 \\times 16.00) Molar mass=3.03+30.97+64.00=98.00\u2009g\/mol\\text{Molar mass} = 3.03 + 30.97 + 64.00 = 98.00 \\, \\text{g\/mol}<\/p>\n\n\n\n

      Thus, the molar mass of phosphoric acid (H3PO4H_3PO_4) is 98.00 g\/mol<\/strong>.<\/p>\n\n\n\n

      \n\n\n\n

      Explanation:<\/h3>\n\n\n\n

      Molar mass is the mass of one mole of a chemical compound, expressed in grams per mole (g\/molg\/mol). It is a crucial property in chemistry for understanding the quantities of substances involved in chemical reactions.<\/p>\n\n\n\n

      Steps:<\/h4>\n\n\n\n
        \n
      1. Understand the Formula<\/strong>: The formula H3PO4H_3PO_4 shows the ratio of atoms in the compound: 3 hydrogens, 1 phosphorus, and 4 oxygens.<\/li>\n\n\n\n
      2. Find Atomic Masses<\/strong>: Atomic masses of individual elements are obtained from the periodic table. These values reflect the average mass of an atom, accounting for isotopes.<\/li>\n\n\n\n
      3. Multiply by Number of Atoms<\/strong>: For each element, multiply its atomic mass by the number of atoms in the compound.\n
          \n
        • For hydrogen: 3\u00d71.01\u2009g\/mol3 \\times 1.01 \\, \\text{g\/mol}<\/li>\n\n\n\n
        • For phosphorus: 1\u00d730.97\u2009g\/mol1 \\times 30.97 \\, \\text{g\/mol}<\/li>\n\n\n\n
        • For oxygen: 4\u00d716.00\u2009g\/mol4 \\times 16.00 \\, \\text{g\/mol}.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Sum the Results<\/strong>: Adding these contributions gives the total molar mass.<\/li>\n<\/ol>\n\n\n\n

          Phosphoric acid is a triprotic acid widely used in fertilizers, food flavoring, and rust removal. Understanding its molar mass allows chemists to measure precise quantities for reactions, ensuring accurate stoichiometric calculations.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Calculate the molar mass of phosphoric acid H3PO4. The correct answer and explanation is: Molar Mass of Phosphoric Acid (H\u2083PO\u2084) The molar mass of phosphoric acid is calculated by summing the atomic masses of its constituent atoms. The chemical formula H3PO4H_3PO_4 indicates it contains: Using the periodic table: Calculation: Molar mass=(3\u00d71.01)+(1\u00d730.97)+(4\u00d716.00)\\text{Molar mass} = (3 \\times 1.01) […]<\/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-184153","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184153","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=184153"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184153\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184153"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184153"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184153"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}