{"id":207109,"date":"2025-04-18T10:32:26","date_gmt":"2025-04-18T10:32:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=207109"},"modified":"2025-04-18T10:32:35","modified_gmt":"2025-04-18T10:32:35","slug":"the-molar-mass-of-ascorbic-acid-vitamin-c-c6h8o6-is-176-12-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/18\/the-molar-mass-of-ascorbic-acid-vitamin-c-c6h8o6-is-176-12-g-mol\/","title":{"rendered":"The molar mass of Ascorbic acid (vitamin C, C6H8O6) is 176.12 g\/mol"},"content":{"rendered":"\n<p>The molar mass of Ascorbic acid (vitamin C, C6H8O6) is 176.12 g\/mol. If you have 704.48 g of Ascorbic acid, how many moles Ascorbic acid would that be?<br>2 mole<br>4 mole<br>1 mole<br>3 mole<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate how many <strong>moles<\/strong> of Ascorbic acid (Vitamin C, <strong>C\u2086H\u2088O\u2086<\/strong>) are present in <strong>704.48 grams<\/strong>, we use the following formula:<\/p>\n\n\n\n<p>[<br>\\text{Moles} = \\frac{\\text{Mass (g)}}{\\text{Molar Mass (g\/mol)}}<br>]<\/p>\n\n\n\n<p>We are given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Mass<\/strong> = 704.48 g<\/li>\n\n\n\n<li><strong>Molar Mass of Ascorbic acid<\/strong> = 176.12 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Now apply the formula:<\/p>\n\n\n\n<p>[<br>\\text{Moles} = \\frac{704.48}{176.12} = 4.0 \\text{ moles}<br>]<\/p>\n\n\n\n<p>\u2705 <strong>Correct Answer: 4 mole<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (300 words):<\/h3>\n\n\n\n<p>In chemistry, the concept of the <strong>mole<\/strong> is a fundamental way of expressing the amount of a substance. One mole of any substance contains <strong>Avogadro&#8217;s number<\/strong> of particles (6.022 \u00d7 10\u00b2\u00b3). However, for practical laboratory purposes, chemists often need to convert between the <strong>mass of a substance (in grams)<\/strong> and <strong>moles<\/strong>, which is where the <strong>molar mass<\/strong> becomes essential.<\/p>\n\n\n\n<p>The <strong>molar mass<\/strong> of a compound is the mass of one mole of its molecules, expressed in grams per mole (g\/mol). For Ascorbic acid (Vitamin C), with the molecular formula <strong>C\u2086H\u2088O\u2086<\/strong>, the molar mass is <strong>176.12 g\/mol<\/strong>. This means that one mole of ascorbic acid weighs 176.12 grams.<\/p>\n\n\n\n<p>To determine how many moles are present in a given mass of the substance, we divide the total mass by the molar mass. In this case, dividing 704.48 grams by 176.12 g\/mol gives exactly 4 moles.<\/p>\n\n\n\n<p>Understanding this calculation is critical in fields such as pharmaceuticals, nutrition, and chemical engineering. For example, in dietary science, knowing how many moles of Vitamin C are present helps determine dosage and nutritional value. Similarly, in a lab setting, chemists use mole calculations to prepare solutions and reactants accurately.<\/p>\n\n\n\n<p>This calculation also highlights the elegance and simplicity of stoichiometry\u2014using relationships between quantities in chemical reactions. Whether making a vitamin supplement or conducting an experiment, the mole concept ensures precision and consistency in chemical measurements.<\/p>\n\n\n\n<p>Thus, 704.48 grams of ascorbic acid equals <strong>4 moles<\/strong>, making &#8220;4 mole&#8221; the correct and most scientifically accurate answer.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/04\/image-158.png\" alt=\"\" class=\"wp-image-207110\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molar mass of Ascorbic acid (vitamin C, C6H8O6) is 176.12 g\/mol. If you have 704.48 g of Ascorbic acid, how many moles Ascorbic acid would that be?2 mole4 mole1 mole3 mole The correct answer and explanation is : To calculate how many moles of Ascorbic acid (Vitamin C, C\u2086H\u2088O\u2086) are present in 704.48 grams, [&hellip;]<\/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-207109","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207109","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=207109"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207109\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=207109"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=207109"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=207109"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}