{"id":267647,"date":"2025-07-23T15:51:41","date_gmt":"2025-07-23T15:51:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267647"},"modified":"2025-07-23T15:51:44","modified_gmt":"2025-07-23T15:51:44","slug":"when-mixed-solutions-of-silver-nitrate-agno3-and-sodium-sulfate-na2so4-form-a-precipitate-of-silver-sulfate-ag2so4-3","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-ag2so4-3\/","title":{"rendered":"When mixed, solutions of silver nitrate, AgNO3, and sodium sulfate, Na2SO4, form a precipitate of silver sulfate, Ag2SO4."},"content":{"rendered":"\n

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

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

To calculate the amount of silver sulfate (Ag2SO4) formed when mixing solutions of silver nitrate (AgNO3) and sodium sulfate (Na2SO4), follow these steps:<\/p>\n\n\n\n

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

The balanced chemical equation is:2AgNO3(aq)+Na2SO4(aq)\u2192Ag2SO4(s)+2NaNO3(aq)2AgNO3(aq) + Na2SO4(aq) \\rightarrow Ag2SO4(s) + 2NaNO3(aq)2AgNO3(aq)+Na2SO4(aq)\u2192Ag2SO4(s)+2NaNO3(aq)<\/p>\n\n\n\n

Step 2: Determine the limiting reagent<\/h3>\n\n\n\n

First, let’s look at the stoichiometric coefficients of the equation:<\/p>\n\n\n\n

    \n
  • 2 moles of AgNO3 react with 1 mole of Na2SO4 to produce 1 mole of Ag2SO4.<\/li>\n<\/ul>\n\n\n\n

    You are given:<\/p>\n\n\n\n

      \n
    • 0.50 mol of AgNO3<\/li>\n\n\n\n
    • 0.30 mol of Na2SO4<\/li>\n<\/ul>\n\n\n\n

      Now, compare the mole ratios:<\/p>\n\n\n\n

        \n
      • According to the equation, 2 moles of AgNO3 need 1 mole of Na2SO4.<\/li>\n\n\n\n
      • To fully react with 0.50 mol of AgNO3, we would need 0.502=0.25\\frac{0.50}{2} = 0.2520.50\u200b=0.25 mol of Na2SO4.<\/li>\n<\/ul>\n\n\n\n

        Since we have 0.30 mol of Na2SO4 available, and only 0.25 mol is needed, Na2SO4 is in excess<\/strong>, and AgNO3 is the limiting reagent<\/strong>.<\/p>\n\n\n\n

        Step 3: Calculate the amount of Ag2SO4 formed<\/h3>\n\n\n\n

        Since AgNO3 is the limiting reagent, use its amount to calculate the amount of Ag2SO4:<\/p>\n\n\n\n

          \n
        • From the balanced equation, 2 moles of AgNO3 produce 1 mole of Ag2SO4.<\/li>\n\n\n\n
        • Therefore, 0.50 mol of AgNO3 will produce 0.502=0.25\\frac{0.50}{2} = 0.2520.50\u200b=0.25 mol of Ag2SO4.<\/li>\n<\/ul>\n\n\n\n

          Step 4: Convert moles of Ag2SO4 to grams<\/h3>\n\n\n\n

          Now, calculate the mass of Ag2SO4 formed. The molar mass of Ag2SO4 is:Molar mass of Ag2SO4=2(107.87\u2009g\/mol)+32.07\u2009g\/mol+4(16.00\u2009g\/mol)=311.87\u2009g\/mol\\text{Molar mass of Ag2SO4} = 2(107.87 \\, \\text{g\/mol}) + 32.07 \\, \\text{g\/mol} + 4(16.00 \\, \\text{g\/mol}) = 311.87 \\, \\text{g\/mol}Molar mass of Ag2SO4=2(107.87g\/mol)+32.07g\/mol+4(16.00g\/mol)=311.87g\/mol<\/p>\n\n\n\n

          Thus, the mass of Ag2SO4 formed is:Mass of Ag2SO4=0.25\u2009mol\u00d7311.87\u2009g\/mol=77.97\u2009g\\text{Mass of Ag2SO4} = 0.25 \\, \\text{mol} \\times 311.87 \\, \\text{g\/mol} = 77.97 \\, \\text{g}Mass of Ag2SO4=0.25mol\u00d7311.87g\/mol=77.97g<\/p>\n\n\n\n

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

          The mass of silver sulfate (Ag2SO4) expected to form is 77.97 g<\/strong>.<\/p>\n\n\n\n

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

          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 The Correct […]<\/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-267647","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267647","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=267647"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267647\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267647"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267647"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267647"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}