{"id":260883,"date":"2025-07-19T17:25:20","date_gmt":"2025-07-19T17:25:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=260883"},"modified":"2025-07-19T17:25:21","modified_gmt":"2025-07-19T17:25:21","slug":"what-reagent-would-distinguish-between-ba2-and-pb2-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/19\/what-reagent-would-distinguish-between-ba2-and-pb2-2\/","title":{"rendered":"What reagent would distinguish between Ba2+ and Pb2+"},"content":{"rendered":"\n

What reagent would distinguish between Ba2+ and Pb2+? A) KCl B) Li2S2O3 C) K2SO4 D) LiNO3<\/p>\n\n\n\n

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

The correct reagent to distinguish between Ba\u00b2\u207a and Pb\u00b2\u207a is C) K\u2082SO\u2084<\/strong>.<\/p>\n\n\n\n

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

Both Ba\u00b2\u207a (barium ion) and Pb\u00b2\u207a (lead ion) are common cations found in aqueous solutions, and distinguishing between them is important in various analytical chemistry applications. The key to distinguishing between these two ions lies in their different solubilities in certain salts, particularly sulfate salts.<\/p>\n\n\n\n

    \n
  1. Barium Ion (Ba\u00b2\u207a)<\/strong>:\n
      \n
    • When K\u2082SO\u2084 (potassium sulfate)<\/strong> is added to a solution containing Ba\u00b2\u207a ions, barium sulfate (BaSO\u2084)<\/strong> forms as a white precipitate. This is because barium sulfate has an extremely low solubility in water (it is nearly insoluble).<\/li>\n\n\n\n
    • The precipitation of BaSO\u2084 is a distinctive reaction that allows you to identify the presence of Ba\u00b2\u207a.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Lead Ion (Pb\u00b2\u207a)<\/strong>:\n
        \n
      • Lead(II) sulfate (PbSO\u2084) also forms when K\u2082SO\u2084<\/strong> is added to a solution containing Pb\u00b2\u207a. However, PbSO\u2084<\/strong> is only sparingly soluble in water, meaning that the precipitate might not form as readily or might appear much less than that of BaSO\u2084. The solubility product (Ksp) of PbSO\u2084 is higher than that of BaSO\u2084, so under certain conditions (such as lower concentrations), Pb\u00b2\u207a may stay in solution, though it would still precipitate to some extent.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

        Therefore, while both ions react with K\u2082SO\u2084 to form a sulfate precipitate, the key difference<\/strong> is that Ba\u00b2\u207a<\/strong> will always<\/strong> form a precipitate of BaSO\u2084, while Pb\u00b2\u207a<\/strong> might not form a precipitate as readily or will form a much less dense precipitate due to its higher solubility.<\/p>\n\n\n\n

        The other reagents (A) KCl, (B) Li\u2082S\u2082O\u2083, and (D) LiNO\u2083 do not effectively distinguish between Ba\u00b2\u207a and Pb\u00b2\u207a in a straightforward way through precipitation reactions.<\/p>\n\n\n\n

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

        What reagent would distinguish between Ba2+ and Pb2+? A) KCl B) Li2S2O3 C) K2SO4 D) LiNO3 The Correct Answer and Explanation is: The correct reagent to distinguish between Ba\u00b2\u207a and Pb\u00b2\u207a is C) K\u2082SO\u2084. Explanation: Both Ba\u00b2\u207a (barium ion) and Pb\u00b2\u207a (lead ion) are common cations found in aqueous solutions, and distinguishing between them is […]<\/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-260883","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260883","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=260883"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260883\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=260883"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=260883"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=260883"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}