{"id":232968,"date":"2025-06-12T12:04:00","date_gmt":"2025-06-12T12:04:00","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=232968"},"modified":"2025-06-12T12:04:02","modified_gmt":"2025-06-12T12:04:02","slug":"what-is-the-theoretical-yield-of-aspirin-in-your-synthesis","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/12\/what-is-the-theoretical-yield-of-aspirin-in-your-synthesis\/","title":{"rendered":"What is the theoretical yield of aspirin in your synthesis"},"content":{"rendered":"\n<pre id=\"preorder-ask-header-text\" class=\"wp-block-preformatted\">What is the theoretical yield of aspirin in your synthesis? The mole ratio is 1:1 between salicylic acid and aspirin in this reaction. The melting temperature of pure acetylsalicylic acid is 135\u00c2\u00b0C. Based on the results of the melting temperature test, do you believe that your aspirin sample is pure? Explain. Based on the results of the absorbance testing with the spectrophotometer, what is the percent purity of your sample of aspirin? Does this percent purity compare well with the results of the melting temperature test? Explain. Use your percent purity calculations to determine the percent yield of your synthesis of aspirin.<\/pre>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Theoretical Yield Calculation:<\/strong><\/h3>\n\n\n\n<p>Let\u2019s say you started with <strong>2.00 g of salicylic acid (C\u2087H\u2086O\u2083)<\/strong>. The molar mass of salicylic acid is approximately <strong>138.12 g\/mol<\/strong>.Moles&nbsp;of&nbsp;salicylic&nbsp;acid=2.00&nbsp;g138.12&nbsp;g\/mol=0.01448&nbsp;mol\\text{Moles of salicylic acid} = \\frac{2.00\\ \\text{g}}{138.12\\ \\text{g\/mol}} = 0.01448\\ \\text{mol}Moles&nbsp;of&nbsp;salicylic&nbsp;acid=138.12&nbsp;g\/mol2.00&nbsp;g\u200b=0.01448&nbsp;mol<\/p>\n\n\n\n<p>Given the 1:1 ratio, the theoretical moles of aspirin = 0.01448 mol.<br>The molar mass of aspirin (C\u2089H\u2088O\u2084) is approximately <strong>180.16 g\/mol<\/strong>:Theoretical&nbsp;yield&nbsp;of&nbsp;aspirin=0.01448&nbsp;mol\u00d7180.16&nbsp;g\/mol=2.61&nbsp;g\\text{Theoretical yield of aspirin} = 0.01448\\ \\text{mol} \\times 180.16\\ \\text{g\/mol} = 2.61\\ \\text{g}Theoretical&nbsp;yield&nbsp;of&nbsp;aspirin=0.01448&nbsp;mol\u00d7180.16&nbsp;g\/mol=2.61&nbsp;g<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Melting Point Test Interpretation:<\/strong><\/h3>\n\n\n\n<p>Pure acetylsalicylic acid has a melting point of <strong>135\u00b0C<\/strong>. If your sample melted at a <strong>lower or broader range<\/strong>, it indicates the presence of <strong>impurities<\/strong>. For example, if your sample melts between <strong>128\u2013132\u00b0C<\/strong>, the deviation suggests that the aspirin is not pure. A sharp, narrow melting range at <strong>135\u00b0C<\/strong> would indicate a high degree of purity.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Percent Purity from Spectrophotometer:<\/strong><\/h3>\n\n\n\n<p>Assume your spectrophotometer testing shows that <strong>your sample is 85% pure<\/strong>. This means that out of the total mass of recovered product, <strong>only 85% is pure aspirin<\/strong>. This aligns with the melting point result: both tests suggest <strong>some impurities<\/strong> are present.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Percent Yield Using Percent Purity:<\/strong><\/h3>\n\n\n\n<p>Let\u2019s say you isolated <strong>2.40 g<\/strong> of crude aspirin. To find <strong>actual yield of pure aspirin<\/strong>, multiply by percent purity:Pure&nbsp;aspirin=2.40&nbsp;g\u00d70.85=2.04&nbsp;g\\text{Pure aspirin} = 2.40\\ \\text{g} \\times 0.85 = 2.04\\ \\text{g}Pure&nbsp;aspirin=2.40&nbsp;g\u00d70.85=2.04&nbsp;g<\/p>\n\n\n\n<p>Then calculate <strong>percent yield<\/strong>:Percent&nbsp;yield=(2.04&nbsp;g2.61&nbsp;g)\u00d7100%=78.2%\\text{Percent yield} = \\left( \\frac{2.04\\ \\text{g}}{2.61\\ \\text{g}} \\right) \\times 100\\% = 78.2\\%Percent&nbsp;yield=(2.61&nbsp;g2.04&nbsp;g\u200b)\u00d7100%=78.2%<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Conclusion:<\/strong><\/h3>\n\n\n\n<p>Your sample\u2019s <strong>melting point and spectrophotometer results both indicate it is impure<\/strong>. The melting point is slightly lower than the pure compound, and the spectrophotometer confirms 85% purity. This moderate purity impacts the percent yield: while 2.40 g of product was collected, only 2.04 g was true aspirin, resulting in a <strong>78.2% actual yield<\/strong>. These results are typical in student lab settings, where minor impurities or incomplete reactions are common.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner5-386.jpeg\" alt=\"\" class=\"wp-image-232969\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the theoretical yield of aspirin in your synthesis? The mole ratio is 1:1 between salicylic acid and aspirin in this reaction. The melting temperature of pure acetylsalicylic acid is 135\u00c2\u00b0C. Based on the results of the melting temperature test, do you believe that your aspirin sample is pure? Explain. Based on the results [&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-232968","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232968","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=232968"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232968\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=232968"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=232968"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=232968"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}