{"id":39507,"date":"2025-06-27T08:02:38","date_gmt":"2025-06-27T08:02:38","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=39507"},"modified":"2025-06-27T08:02:39","modified_gmt":"2025-06-27T08:02:39","slug":"the-molar-mass-of-ammonium-hydrogen-phosphate-nh4h2po4-is","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/the-molar-mass-of-ammonium-hydrogen-phosphate-nh4h2po4-is\/","title":{"rendered":"The molar mass of Ammonium Hydrogen Phosphate; (NH4H2PO4) is"},"content":{"rendered":"\n<p>The molar mass of Ammonium Hydrogen Phosphate; (NH4H2PO4) is? A. 422 g\/mole B. 132.1 g\/mole C. 164.0 g\/mole D. 130.0 g\/mole E. 264.2 g\/mole F. 123.0 g\/mole<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"700\" height=\"302\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-395.png\" alt=\"\" class=\"wp-image-39508\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-395.png 700w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-395-300x129.png 300w\" sizes=\"auto, (max-width: 700px) 100vw, 700px\" \/><\/figure>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the molar mass of ammonium hydrogen phosphate, given the correct formula <strong>(NH\u2084)\u2082HPO\u2084<\/strong>, we must add the atomic masses of all atoms present in the compound.<\/p>\n\n\n\n<p>Break the formula down into its components:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Two ammonium ions: (NH\u2084)\u2082<\/li>\n\n\n\n<li>One hydrogen phosphate ion: HPO\u2084<\/li>\n<\/ul>\n\n\n\n<p>Let\u2019s calculate each component step by step using standard atomic masses:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen (N): 14.01 g\/mol<\/li>\n\n\n\n<li>Hydrogen (H): 1.008 g\/mol<\/li>\n\n\n\n<li>Phosphorus (P): 30.97 g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p><strong>Ammonium (NH\u2084):<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>One nitrogen: 14.01 g\/mol<\/li>\n\n\n\n<li>Four hydrogens: 4 \u00d7 1.008 = 4.032 g\/mol<\/li>\n\n\n\n<li>Total for NH\u2084: 14.01 + 4.032 = 18.042 g\/mol<\/li>\n\n\n\n<li>Since there are two ammonium ions: 2 \u00d7 18.042 = 36.084 g\/mol<\/li>\n<\/ul>\n\n\n\n<p><strong>Hydrogen phosphate (HPO\u2084):<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>One hydrogen: 1.008 g\/mol<\/li>\n\n\n\n<li>One phosphorus: 30.97 g\/mol<\/li>\n\n\n\n<li>Four oxygens: 4 \u00d7 16.00 = 64.00 g\/mol<\/li>\n\n\n\n<li>Total for HPO\u2084: 1.008 + 30.97 + 64.00 = 95.978 g\/mol<\/li>\n<\/ul>\n\n\n\n<p><strong>Add everything together:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>36.084 (from ammonium)<\/li>\n\n\n\n<li>95.978 (from hydrogen phosphate)<\/li>\n\n\n\n<li>Total molar mass = 36.084 + 95.978 = <strong>132.062 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Rounded appropriately based on significant figures, the molar mass is <strong>132.1 g\/mol<\/strong>, which matches <strong>option B<\/strong>.<\/p>\n\n\n\n<p>This compound is often used in fertilizers and buffer solutions in biochemistry. The accuracy in calculating its molar mass is essential for preparing solutions with correct concentrations, especially in experiments where ionic balance and buffering capacity are critical. Proper calculation also helps in determining molarity and stoichiometric requirements during titrations or reactions involving phosphate groups.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1161.jpeg\" alt=\"\" class=\"wp-image-39509\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1161.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1161-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1161-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molar mass of Ammonium Hydrogen Phosphate; (NH4H2PO4) is? A. 422 g\/mole B. 132.1 g\/mole C. 164.0 g\/mole D. 130.0 g\/mole E. 264.2 g\/mole F. 123.0 g\/mole The Correct Answer and Explanation is: To determine the molar mass of ammonium hydrogen phosphate, given the correct formula (NH\u2084)\u2082HPO\u2084, we must add the atomic masses of all [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-39507","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39507","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=39507"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39507\/revisions"}],"predecessor-version":[{"id":39510,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39507\/revisions\/39510"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39507"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39507"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39507"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}