{"id":267525,"date":"2025-07-23T14:44:27","date_gmt":"2025-07-23T14:44:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267525"},"modified":"2025-07-23T14:44:29","modified_gmt":"2025-07-23T14:44:29","slug":"when-mixed-solutions-of-silver-nitrate-agno3-and-sodium-sulfate-na2so4-form-a-precipitate-of-silver-sulfate-ag2so4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/when-mixed-solutions-of-silver-nitrate-agno3-and-sodium-sulfate-na2so4-form-a-precipitate-of-silver-sulfate-ag2so4\/","title":{"rendered":"When mixed, solutions of silver nitrate, AgNO3, and sodium sulfate, Na2SO4, form a precipitate of silver sulfate, Ag2SO4"},"content":{"rendered":"\n<p>When mixed, solutions of silver nitrate, AgNO3, and sodium sulfate, Na2SO4, form a precipitate of silver sulfate, Ag2SO4. The balanced equation is: 2AgNO3(aq) + Na2SO4(aq) \u2192 Ag2SO4(s) + 2NaNO3(aq) How many grams of silver sulfate are expected when a solution containing 0.50 mol AgNO3 is mixed with a solution containing 0.30 mol Na2SO4?<br>When mixed, solutions of silver nitrate, AgNO3, and sodium sulfate, Na2SO4, form a precipitate of silver sulfate, Ag2SO4. The balanced equation is: 2AgNO3(aq) + Na2SO4(aq) \u2192 Ag2SO4(s) + 2NaNO3(aq) How many grams of silver sulfate are expected when a solution containing 0.50 mol AgNO3 is mixed with a solution containing 0.30 mol Na2SO4?<\/p>\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<p>To solve this problem, we need to determine the amount of silver sulfate (Ag2SO4) produced in the reaction when mixing 0.50 mol of AgNO3 and 0.30 mol of Na2SO4. We&#8217;ll do this step by step, considering the stoichiometry of the reaction.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Write the balanced chemical equation<\/h3>\n\n\n\n<p>The balanced equation for the reaction is:2AgNO3(aq)+Na2SO4(aq)\u2192Ag2SO4(s)+2NaNO3(aq)2AgNO_3(aq) + Na_2SO_4(aq) \\rightarrow Ag_2SO_4(s) + 2NaNO_3(aq)2AgNO3\u200b(aq)+Na2\u200bSO4\u200b(aq)\u2192Ag2\u200bSO4\u200b(s)+2NaNO3\u200b(aq)<\/p>\n\n\n\n<p>From this equation, we see that:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>2 moles of AgNO3 react with 1 mole of Na2SO4 to produce 1 mole of Ag2SO4.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Identify the limiting reactant<\/h3>\n\n\n\n<p>We are given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>0.50 mol of AgNO3<\/li>\n\n\n\n<li>0.30 mol of Na2SO4<\/li>\n<\/ul>\n\n\n\n<p>From the equation, we need 2 moles of AgNO3 for every 1 mole of Na2SO4. Let\u2019s check how much AgNO3 is needed for 0.30 mol of Na2SO4:0.30\u2009mol&nbsp;Na2SO4\u00d72\u2009mol&nbsp;AgNO31\u2009mol&nbsp;Na2SO4=0.60\u2009mol&nbsp;AgNO30.30 \\, \\text{mol Na}_2\\text{SO}_4 \\times \\frac{2 \\, \\text{mol AgNO}_3}{1 \\, \\text{mol Na}_2\\text{SO}_4} = 0.60 \\, \\text{mol AgNO}_30.30mol&nbsp;Na2\u200bSO4\u200b\u00d71mol&nbsp;Na2\u200bSO4\u200b2mol&nbsp;AgNO3\u200b\u200b=0.60mol&nbsp;AgNO3\u200b<\/p>\n\n\n\n<p>We have 0.50 mol of AgNO3, but we need 0.60 mol to completely react with 0.30 mol of Na2SO4. Therefore, <strong>AgNO3<\/strong> is the <strong>limiting reactant<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculate the amount of silver sulfate produced<\/h3>\n\n\n\n<p>From the balanced equation, 2 moles of AgNO3 produce 1 mole of Ag2SO4. Since AgNO3 is limiting, we can calculate how many moles of Ag2SO4 are produced from 0.50 mol of AgNO3:0.50\u2009mol&nbsp;AgNO3\u00d71\u2009mol&nbsp;Ag2SO42\u2009mol&nbsp;AgNO3=0.25\u2009mol&nbsp;Ag2SO40.50 \\, \\text{mol AgNO}_3 \\times \\frac{1 \\, \\text{mol Ag}_2\\text{SO}_4}{2 \\, \\text{mol AgNO}_3} = 0.25 \\, \\text{mol Ag}_2\\text{SO}_40.50mol&nbsp;AgNO3\u200b\u00d72mol&nbsp;AgNO3\u200b1mol&nbsp;Ag2\u200bSO4\u200b\u200b=0.25mol&nbsp;Ag2\u200bSO4\u200b<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Convert moles of Ag2SO4 to grams<\/h3>\n\n\n\n<p>Next, we need to convert the moles of Ag2SO4 to grams. The molar mass of Ag2SO4 is calculated as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Silver (Ag): 107.87\u2009g\/mol107.87 \\, \\text{g\/mol}107.87g\/mol<\/li>\n\n\n\n<li>Sulfur (S): 32.07\u2009g\/mol32.07 \\, \\text{g\/mol}32.07g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 16.00\u2009g\/mol16.00 \\, \\text{g\/mol}16.00g\/mol<\/li>\n<\/ul>\n\n\n\n<p>The molar mass of Ag2SO4 is:(2\u00d7107.87)+32.07+(4\u00d716.00)=215.74+32.07+64.00=311.81\u2009g\/mol(2 \\times 107.87) + 32.07 + (4 \\times 16.00) = 215.74 + 32.07 + 64.00 = 311.81 \\, \\text{g\/mol}(2\u00d7107.87)+32.07+(4\u00d716.00)=215.74+32.07+64.00=311.81g\/mol<\/p>\n\n\n\n<p>Now, calculate the mass of Ag2SO4 produced:0.25\u2009mol&nbsp;Ag2SO4\u00d7311.81\u2009g\/mol=77.95\u2009g&nbsp;Ag2SO40.25 \\, \\text{mol Ag}_2\\text{SO}_4 \\times 311.81 \\, \\text{g\/mol} = 77.95 \\, \\text{g Ag}_2\\text{SO}_40.25mol&nbsp;Ag2\u200bSO4\u200b\u00d7311.81g\/mol=77.95g&nbsp;Ag2\u200bSO4\u200b<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The mass of silver sulfate (Ag2SO4) produced is <strong>77.95 grams<\/strong>.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1694.jpeg\" alt=\"\" class=\"wp-image-267550\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>When mixed, solutions of silver nitrate, AgNO3, and sodium sulfate, Na2SO4, form a precipitate of silver sulfate, Ag2SO4. The balanced equation is: 2AgNO3(aq) + Na2SO4(aq) \u2192 Ag2SO4(s) + 2NaNO3(aq) How many grams of silver sulfate are expected when a solution containing 0.50 mol AgNO3 is mixed with a solution containing 0.30 mol Na2SO4?When mixed, solutions [&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-267525","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267525","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=267525"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267525\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267525"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267525"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267525"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}