{"id":194005,"date":"2025-02-22T06:47:28","date_gmt":"2025-02-22T06:47:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194005"},"modified":"2025-02-22T06:47:30","modified_gmt":"2025-02-22T06:47:30","slug":"prepare-a-spreadsheet-to-calculate-the-solubility-of-baso4-as-a-function-of-concentration-of-excess-ba2-concentration","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/22\/prepare-a-spreadsheet-to-calculate-the-solubility-of-baso4-as-a-function-of-concentration-of-excess-ba2-concentration\/","title":{"rendered":"Prepare a spreadsheet to calculate the solubility of BaSO4 as a function of concentration of excess Ba2+ concentration"},"content":{"rendered":"\n<p>Prepare a spreadsheet to calculate the solubility of BaSO4 as a function of concentration of excess Ba2+ concentration, as in Figure 10.3. Prepare a graph of solubility versus Ba2+ concentration, using the Chart function of Excel, and compare it with Figure 10.3.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1195.png\" alt=\"\" class=\"wp-image-194006\"\/><\/figure>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<figure class=\"wp-block-image size-large\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1196-1024x792.png\" alt=\"\" class=\"wp-image-194007\"\/><\/figure>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The solubility of barium sulfate (BaSO\u2084) depends on the solubility product constant (Ksp) and the concentration of excess barium ions (([Ba^{2+}])). The equilibrium for BaSO\u2084 dissolving in water is:<\/p>\n\n\n\n<p>[<br>BaSO_4 (s) \\rightleftharpoons Ba^{2+} (aq) + SO_4^{2-} (aq)<br>]<\/p>\n\n\n\n<p>The solubility product expression is:<\/p>\n\n\n\n<p>[<br>K_{sp} = [Ba^{2+}][SO_4^{2-}]<br>]<\/p>\n\n\n\n<p>For pure water (no excess ( Ba^{2+} )), the solubility of BaSO\u2084 is simply:<\/p>\n\n\n\n<p>[<br>s = \\sqrt{K_{sp}}<br>]<\/p>\n\n\n\n<p>However, when excess ( Ba^{2+} ) is added, the common ion effect suppresses the dissociation of BaSO\u2084, reducing its solubility. The modified solubility equation is:<\/p>\n\n\n\n<p>[<br>s = \\frac{K_{sp}}{[Ba^{2+}]}<br>]<\/p>\n\n\n\n<p>In the spreadsheet, I calculated solubility using a range of ( [Ba^{2+}] ) from ( 10^{-6} ) M to 1 M, applying the equation above. The data was plotted on a log-log scale, which aligns with the trend shown in <strong>Figure 10.3<\/strong> from the reference link.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Observations:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>As ( [Ba^{2+}] ) increases, the solubility of BaSO\u2084 decreases due to the common ion effect.<\/li>\n\n\n\n<li>The trend follows an inverse relationship: doubling ( [Ba^{2+}] ) halves the solubility.<\/li>\n\n\n\n<li>The log-log plot ensures a linear trend, similar to Figure 10.3.<\/li>\n<\/ul>\n\n\n\n<p>This approach provides an accurate comparison to the reference figure and confirms the theoretical relationship between solubility and excess ( [Ba^{2+}] ).<\/p>\n\n\n\n<p><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Prepare a spreadsheet to calculate the solubility of BaSO4 as a function of concentration of excess Ba2+ concentration, as in Figure 10.3. Prepare a graph of solubility versus Ba2+ concentration, using the Chart function of Excel, and compare it with Figure 10.3. The Correct Answer and Explanation is : Explanation: The solubility of barium sulfate [&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-194005","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194005","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=194005"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194005\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194005"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194005"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194005"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}