{"id":186731,"date":"2025-01-26T06:43:03","date_gmt":"2025-01-26T06:43:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186731"},"modified":"2025-01-26T06:43:05","modified_gmt":"2025-01-26T06:43:05","slug":"the-exothermic-dissolution-of-mgoh2-solid-in-water-is-represented-by-the-equation-above","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/26\/the-exothermic-dissolution-of-mgoh2-solid-in-water-is-represented-by-the-equation-above\/","title":{"rendered":"The exothermic dissolution of Mg(OH)2 (solid) in water is represented by the equation above"},"content":{"rendered":"\n<p>The exothermic dissolution of Mg(OH)2 (solid) in water is represented by the equation above. The Ksp of Mg(OH)2 is 1.8 x 10-11. Why will decreasing the pH increase the solubility of Mg(OH)2 in an aqueous solution?<\/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 solubility of magnesium hydroxide (Mg(OH)\u2082) in water is governed by the equilibrium:<\/p>\n\n\n\n<p>[<br>\\text{Mg(OH)}_2 (s) \\rightleftharpoons \\text{Mg}^{2+} (aq) + 2\\text{OH}^- (aq)<br>]<\/p>\n\n\n\n<p>The solubility product constant (Ksp) for this reaction is (1.8 \\times 10^{-11}), which represents the equilibrium between solid magnesium hydroxide and its ions in solution.<\/p>\n\n\n\n<p>The reason why decreasing the pH will increase the solubility of Mg(OH)\u2082 is because of the common ion effect, specifically involving the concentration of hydroxide ions ((OH^-)).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>When the pH decreases (which means the concentration of hydrogen ions ([H^+]) increases), the equilibrium is shifted to the right due to Le Chatelier\u2019s Principle.<\/li>\n\n\n\n<li>In an acidic environment, the increase in ([H^+]) reacts with ([OH^-]) to form water, effectively reducing the concentration of (OH^-) ions in the solution.<\/li>\n\n\n\n<li>To restore equilibrium, the dissolution of Mg(OH)\u2082 increases, producing more (OH^-) and (Mg^{2+}), thus increasing the solubility of Mg(OH)\u2082.<\/li>\n<\/ul>\n\n\n\n<p>In summary, when the pH is decreased (i.e., more acidic), the concentration of (OH^-) ions decreases, shifting the equilibrium to the right, which increases the solubility of magnesium hydroxide.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The exothermic dissolution of Mg(OH)2 (solid) in water is represented by the equation above. The Ksp of Mg(OH)2 is 1.8 x 10-11. Why will decreasing the pH increase the solubility of Mg(OH)2 in an aqueous solution? The Correct Answer and Explanation is : The solubility of magnesium hydroxide (Mg(OH)\u2082) in water is governed by the [&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-186731","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186731","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=186731"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186731\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186731"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186731"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186731"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}