To calculate the solubility of barium sulfate (BaSO4) in pure water, we will use its solubility product constant (Ksp), which is given as 1.1 \u00d7 10^-10 at 25\u00b0C.<\/p>\n\n\n\n
The dissolution of BaSO4 in water can be represented by the following equilibrium equation:<\/p>\n\n\n\n
BaSO4 (s) \u21cc Ba2+ (aq) + SO4^2- (aq)<\/p>\n\n\n\n
Let the solubility of BaSO4 be S<\/em> moles per liter. At equilibrium, the concentrations of Ba2+ and SO4^2- will both be S<\/em>, since one mole of BaSO4 dissociates to give one mole of Ba2+ and one mole of SO4^2-.<\/p>\n\n\n\n The expression for the solubility product (Ksp) is:<\/p>\n\n\n\n Ksp = [Ba2+][SO4^2-]<\/p>\n\n\n\n Since both ion concentrations are equal to S<\/em>, the equation becomes:<\/p>\n\n\n\n Ksp = S\u00b2<\/p>\n\n\n\n Substituting the given Ksp value:<\/p>\n\n\n\n 1.1 \u00d7 10^-10 = S\u00b2<\/p>\n\n\n\n To find S<\/em>, take the square root of both sides:<\/p>\n\n\n\n S = \u221a(1.1 \u00d7 10^-10) Therefore, the solubility of BaSO4 in pure water is approximately 1.05 \u00d7 10^-5 moles per liter.<\/p>\n\n\n\n Now, to convert this into grams per liter, we need the molar mass of BaSO4. The molar mass of BaSO4 is:<\/p>\n\n\n\n Ba = 137.33 g\/mol Molar mass of BaSO4 = 137.33 + 32.07 + 64.00 = 233.40 g\/mol<\/p>\n\n\n\n The solubility in grams per liter is:<\/p>\n\n\n\n Solubility (g\/L) = S \u00d7 molar mass Therefore, the solubility of BaSO4 in pure water is approximately 2.45 \u00d7 10^-3 grams per liter.<\/p>\n\n\n\n BaSO4 (s) \u21cc Ba2+ (aq) + SO4^2- (aq) The Correct Answer and Explanation is: To calculate the solubility of barium sulfate (BaSO4) in pure water, we will use its solubility product constant (Ksp), which is given as 1.1 \u00d7 10^-10 at 25\u00b0C. The dissolution of BaSO4 in water can be represented by the following equilibrium […]<\/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-266400","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266400","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=266400"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266400\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266400"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266400"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266400"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
S \u2248 1.05 \u00d7 10^-5 M<\/p>\n\n\n\n
S = 32.07 g\/mol
O = 16.00 g\/mol (\u00d74 for SO4)<\/p>\n\n\n\n
Solubility \u2248 (1.05 \u00d7 10^-5 mol\/L) \u00d7 (233.40 g\/mol)
Solubility \u2248 2.45 \u00d7 10^-3 g\/L<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1591.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"