{"id":186576,"date":"2025-01-25T09:33:59","date_gmt":"2025-01-25T09:33:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186576"},"modified":"2025-01-25T09:34:04","modified_gmt":"2025-01-25T09:34:04","slug":"strontium-sulfate-srso4-would-be-the-least-soluble-in-which-following-solutions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/25\/strontium-sulfate-srso4-would-be-the-least-soluble-in-which-following-solutions\/","title":{"rendered":"Strontium sulfate, SrSO4, would be the least soluble in which following solutions"},"content":{"rendered":"\n<p>Strontium sulfate, SrSO4, would be the least soluble in which following solutions?<\/p>\n\n\n\n<p>a) 0.1 M HCl<br>b) 0.1 M NaF<br>c) 0.1 M Na2SO4<br>d) 0.1 M NaOH<br>e) 0.1 M NaCl<\/p>\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<p>The correct answer is <strong>(c) 0.1 M Na\u2082SO\u2084<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Strontium sulfate (SrSO\u2084) is an ionic compound, and its solubility is affected by the presence of common ions in solution. This is due to the <strong>common ion effect<\/strong>, which reduces the solubility of a salt when a common ion is added to the solution. The solubility product constant (Ksp) for SrSO\u2084 is very small, indicating that it is poorly soluble in water.<\/p>\n\n\n\n<p>The solubility of SrSO\u2084 is governed by the equilibrium: SrSO\u2084&nbsp;(s)\u21ccSr2+(aq)+SO\u20842\u2212(aq)\\text{SrSO\u2084 (s)} \\rightleftharpoons \\text{Sr}^{2+} (aq) + \\text{SO\u2084}^{2-} (aq)<\/p>\n\n\n\n<p>Now, let&#8217;s analyze each solution:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>0.1 M HCl (a):<\/strong> Hydrochloric acid dissociates into H\u207a and Cl\u207b ions. The chloride ion (Cl\u207b) does not share a common ion with SrSO\u2084, so the solubility of SrSO\u2084 would not be significantly affected by the presence of HCl. Therefore, SrSO\u2084 would have moderate solubility in this solution.<\/li>\n\n\n\n<li><strong>0.1 M NaF (b):<\/strong> Sodium fluoride dissociates into Na\u207a and F\u207b ions. Neither of these ions is a common ion to SrSO\u2084. Thus, the solubility of SrSO\u2084 would not be strongly affected by NaF.<\/li>\n\n\n\n<li><strong>0.1 M Na\u2082SO\u2084 (c):<\/strong> Sodium sulfate dissociates into Na\u207a and SO\u2084\u00b2\u207b ions. The sulfate ion (SO\u2084\u00b2\u207b) is a common ion with SrSO\u2084. According to the common ion effect, the presence of additional sulfate ions in solution would shift the equilibrium to the left, reducing the solubility of SrSO\u2084. Hence, SrSO\u2084 would be the least soluble in this solution.<\/li>\n\n\n\n<li><strong>0.1 M NaOH (d):<\/strong> Sodium hydroxide dissociates into Na\u207a and OH\u207b ions. Neither Na\u207a nor OH\u207b ions are common to SrSO\u2084, so SrSO\u2084&#8217;s solubility would not be greatly affected by NaOH.<\/li>\n\n\n\n<li><strong>0.1 M NaCl (e):<\/strong> Sodium chloride dissociates into Na\u207a and Cl\u207b ions. Again, neither of these ions is a common ion to SrSO\u2084, so its solubility would not be significantly affected by NaCl.<\/li>\n<\/ol>\n\n\n\n<p>Therefore, the presence of the sulfate ion in <strong>0.1 M Na\u2082SO\u2084<\/strong> will have the greatest effect in reducing the solubility of SrSO\u2084, making it the least soluble in this solution.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Strontium sulfate, SrSO4, would be the least soluble in which following solutions? a) 0.1 M HClb) 0.1 M NaFc) 0.1 M Na2SO4d) 0.1 M NaOHe) 0.1 M NaCl The Correct Answer and Explanation is : The correct answer is (c) 0.1 M Na\u2082SO\u2084. Explanation: Strontium sulfate (SrSO\u2084) is an ionic compound, and its solubility is [&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-186576","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186576","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=186576"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186576\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186576"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186576"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186576"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}