{"id":220782,"date":"2025-05-28T19:09:04","date_gmt":"2025-05-28T19:09:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=220782"},"modified":"2025-05-28T19:09:08","modified_gmt":"2025-05-28T19:09:08","slug":"refer-to-the-precipitation-reaction-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/28\/refer-to-the-precipitation-reaction-below\/","title":{"rendered":"Refer To The Precipitation Reaction Below"},"content":{"rendered":"\n

Refer To The Precipitation Reaction Below. BaCl2 (Aq) + H2SO4 (Aq) \u2013 BaSO4 (S) + 2HCl (Aq) How Much 0.22 M H2SO4 Solution In Liters Will Completely Precipitate The Ba\u00b2? Ion In 1.2 L Of 0.19 M BaCl2 Solution? Do Not Include Units In Your Answer, And Round To Two Significant Figures.<\/p>\n\n\n\n

Refer to the precipitation reaction below. BaCl2 (aq) + H2SO4 (aq) \u2013 BaSO4 (s) + 2HCl (aq) How much 0.22 M H2SO4 solution in<\/p>\n\n\n\n

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

Answer:<\/strong> 1.0<\/code><\/p>\n\n\n\n

\n\n\n\n

Step-by-Step Solution and Explanation<\/strong><\/h3>\n\n\n\n

We are given the balanced chemical reaction:<\/p>\n\n\n\n

BaCl\u2082 (aq) + H\u2082SO\u2084 (aq) \u2192 BaSO\u2084 (s) + 2HCl (aq)<\/strong><\/p>\n\n\n\n

This shows a 1:1 molar ratio<\/strong> between BaCl\u2082<\/strong> and H\u2082SO\u2084<\/strong>, meaning one mole of sulfuric acid reacts with one mole of barium chloride to form one mole of barium sulfate precipitate.<\/p>\n\n\n\n

\n\n\n\n

Step 1: Calculate moles of Ba\u00b2\u207a in BaCl\u2082 solution<\/strong><\/h3>\n\n\n\n

We are told:<\/p>\n\n\n\n

    \n
  • Volume of BaCl\u2082 = 1.2 L<\/strong><\/li>\n\n\n\n
  • Molarity of BaCl\u2082 = 0.19 M<\/strong><\/li>\n<\/ul>\n\n\n\n

    Moles of BaCl2=Molarity\u00d7Volume=0.19 mol\/L\u00d71.2 L=0.228 mol\\text{Moles of BaCl}_2 = Molarity \\times Volume = 0.19\\ \\text{mol\/L} \\times 1.2\\ \\text{L} = 0.228\\ \\text{mol}<\/p>\n\n\n\n

    Since each BaCl\u2082 provides one Ba\u00b2\u207a ion, moles of Ba\u00b2\u207a = 0.228 mol<\/strong>.<\/p>\n\n\n\n

    \n\n\n\n

    Step 2: Use stoichiometry to find moles of H\u2082SO\u2084 needed<\/strong><\/h3>\n\n\n\n

    From the balanced equation:<\/p>\n\n\n\n

      \n
    • 1 mole of H\u2082SO\u2084 reacts with 1 mole of Ba\u00b2\u207a.<\/li>\n\n\n\n
    • So, moles of H\u2082SO\u2084 needed = 0.228 mol<\/strong><\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      Step 3: Use molarity of H\u2082SO\u2084 to find required volume<\/strong><\/h3>\n\n\n\n

      We are told:<\/p>\n\n\n\n

        \n
      • Molarity of H\u2082SO\u2084 = 0.22 M<\/strong><\/li>\n<\/ul>\n\n\n\n

        Volume of H2SO4=MolesMolarity=0.228 mol0.22 mol\/L=1.036 L\\text{Volume of H}_2\\text{SO}_4 = \\frac{\\text{Moles}}{\\text{Molarity}} = \\frac{0.228\\ \\text{mol}}{0.22\\ \\text{mol\/L}} = 1.036\\ \\text{L}<\/p>\n\n\n\n

        \n\n\n\n

        Step 4: Round the final answer<\/strong><\/h3>\n\n\n\n

        Rounded to two significant figures<\/strong>, the answer is: 1.0\\boxed{1.0}<\/p>\n\n\n\n

        \n\n\n\n

        Final Explanation:<\/strong><\/h3>\n\n\n\n

        To completely precipitate all the Ba\u00b2\u207a ions from a 1.2 L solution of 0.19 M BaCl\u2082, you need the same number of moles of H\u2082SO\u2084 because the reaction has a 1:1 molar ratio. You calculated the moles of Ba\u00b2\u207a present, matched it to the moles of H\u2082SO\u2084 needed, and then used the molarity of H\u2082SO\u2084 to find the required volume. Rounding gives a final answer of 1.0 liters<\/strong>.<\/p>\n\n\n\n

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

        Refer To The Precipitation Reaction Below. BaCl2 (Aq) + H2SO4 (Aq) \u2013 BaSO4 (S) + 2HCl (Aq) How Much 0.22 M H2SO4 Solution In Liters Will Completely Precipitate The Ba\u00b2? Ion In 1.2 L Of 0.19 M BaCl2 Solution? Do Not Include Units In Your Answer, And Round To Two Significant Figures. Refer to the […]<\/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-220782","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220782","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=220782"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220782\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=220782"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=220782"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=220782"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}