{"id":219711,"date":"2025-05-26T15:28:15","date_gmt":"2025-05-26T15:28:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=219711"},"modified":"2025-05-26T15:28:17","modified_gmt":"2025-05-26T15:28:17","slug":"solvi-ammonium-phosphate-nh43po4-is-an-important-ingredient-in-many-fertilizers","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/26\/solvi-ammonium-phosphate-nh43po4-is-an-important-ingredient-in-many-fertilizers\/","title":{"rendered":"Solvi Ammonium Phosphate ((NH4)3PO4) is an important ingredient in many fertilizers"},"content":{"rendered":"\n

Solvi Ammonium Phosphate ((NH4)3PO4) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4) with ammonia (NH3). What mass of ammonium phosphate is produced by the reaction of 4.6 g of phosphoric acid? Round your answer to 2 significant digits.<\/p>\n\n\n\n

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

To determine the mass of ammonium phosphate ((NH\u2084)\u2083PO\u2084)<\/strong> produced from 4.6 g of phosphoric acid (H\u2083PO\u2084)<\/strong>, we follow these steps:<\/p>\n\n\n\n

\n\n\n\n

Step 1: Write the balanced chemical equation<\/strong><\/h3>\n\n\n\n

H\u2083PO\u2084+3NH\u2083\u2192(NH\u2084)3PO\u2084\\text{H\u2083PO\u2084} + 3\\text{NH\u2083} \\rightarrow (\\text{NH\u2084})\u2083\\text{PO\u2084}<\/p>\n\n\n\n

This reaction shows that 1 mole of H\u2083PO\u2084<\/strong> reacts with 3 moles of NH\u2083<\/strong> to form 1 mole of (NH\u2084)\u2083PO\u2084<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Step 2: Calculate the molar mass of H\u2083PO\u2084<\/strong><\/h3>\n\n\n\n
    \n
  • H: 1.01 \u00d7 3 = 3.03 g\/mol<\/li>\n\n\n\n
  • P: 30.97 g\/mol<\/li>\n\n\n\n
  • O: 16.00 \u00d7 4 = 64.00 g\/mol
    Total = 3.03 + 30.97 + 64.00 = 98.00 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    Step 3: Convert 4.6 g H\u2083PO\u2084 to moles<\/strong><\/h3>\n\n\n\n

    4.6 g98.00 g\/mol=0.04694 mol\\frac{4.6 \\text{ g}}{98.00 \\text{ g\/mol}} = 0.04694 \\text{ mol}<\/p>\n\n\n\n

    \n\n\n\n

    Step 4: Use the mole ratio<\/strong><\/h3>\n\n\n\n

    From the balanced equation, 1 mol H\u2083PO\u2084 \u2192 1 mol (NH\u2084)\u2083PO\u2084<\/strong>, so: 0.04694 mol H\u2083PO\u2084\u21920.04694 mol (NH\u2084)\u2083PO\u20840.04694 \\text{ mol H\u2083PO\u2084} \u2192 0.04694 \\text{ mol (NH\u2084)\u2083PO\u2084}<\/p>\n\n\n\n

    \n\n\n\n

    Step 5: Calculate molar mass of (NH\u2084)\u2083PO\u2084<\/strong><\/h3>\n\n\n\n
      \n
    • N: 14.01 \u00d7 3 = 42.03<\/li>\n\n\n\n
    • H: 1.01 \u00d7 12 = 12.12<\/li>\n\n\n\n
    • P: 30.97<\/li>\n\n\n\n
    • O: 16.00 \u00d7 4 = 64.00
      Total = 42.03 + 12.12 + 30.97 + 64.00 = 149.12 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      Step 6: Calculate mass of (NH\u2084)\u2083PO\u2084 produced<\/strong><\/h3>\n\n\n\n

      0.04694 mol\u00d7149.12 g\/mol=6.999 g0.04694 \\text{ mol} \u00d7 149.12 \\text{ g\/mol} = 6.999 \\text{ g}<\/p>\n\n\n\n

      \n\n\n\n

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

      7.0 g\\boxed{7.0 \\text{ g}}<\/p>\n\n\n\n

      \n\n\n\n

      Explanation <\/strong><\/h3>\n\n\n\n

      The production of ammonium phosphate ((NH\u2084)\u2083PO\u2084), a widely used fertilizer component, involves a reaction between phosphoric acid (H\u2083PO\u2084) and ammonia (NH\u2083). This is an example of an acid-base reaction, where phosphoric acid donates protons to form ammonium ions, which then combine with phosphate ions.<\/p>\n\n\n\n

      To determine how much ammonium phosphate is formed from 4.6 grams of H\u2083PO\u2084, we start with the balanced chemical equation. This equation shows a 1:1 molar ratio between phosphoric acid and ammonium phosphate, meaning each mole of H\u2083PO\u2084 yields one mole of (NH\u2084)\u2083PO\u2084, assuming excess ammonia is available.<\/p>\n\n\n\n

      Next, we calculate the molar mass of H\u2083PO\u2084, which is 98.00 g\/mol. By dividing the given mass (4.6 g) by this molar mass, we find the number of moles of H\u2083PO\u2084: approximately 0.04694 mol.<\/p>\n\n\n\n

      Since the ratio is 1:1, the same number of moles of (NH\u2084)\u2083PO\u2084 will be produced. The next step is to calculate the molar mass of ammonium phosphate, which is 149.12 g\/mol. Multiplying this by the number of moles gives us the final mass: around 6.999 g. Rounding this to two significant figures (based on the initial data), we obtain 7.0 g<\/strong>.<\/p>\n\n\n\n

      This calculation is important in both academic and industrial chemistry contexts, as precise stoichiometry is critical in producing the correct amount of product while minimizing waste and ensuring cost efficiency in large-scale fertilizer production.<\/p>\n\n\n\n

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

      Solvi Ammonium Phosphate ((NH4)3PO4) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4) with ammonia (NH3). What mass of ammonium phosphate is produced by the reaction of 4.6 g of phosphoric acid? Round your answer to 2 significant digits. The Correct Answer and Explanation is: To determine the […]<\/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-219711","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219711","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=219711"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219711\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=219711"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=219711"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=219711"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}