Equilibria Involving Sparingly Soluble Salts<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n \ue203When a sparingly soluble salt is added to water, it establishes an equilibrium between its solid form and its constituent ions in solution.\ue204 For example, consider the dissolution of silver chloride (AgCl):\ue206<\/p>\n\n\n\n \ue203AgCl (s)\u21ccAg+(aq)+Cl\u2212(aq)\\text{AgCl (s)} \\rightleftharpoons \\text{Ag}^+ (\\text{aq}) + \\text{Cl}^- (\\text{aq})\ue204\ue206<\/p>\n\n\n\n \ue203The solubility product constant (K\u209b\u209a) for AgCl at 25\u00b0C is 1.8 \u00d7 10\u207b\u00b9\u2070, indicating its limited solubility in water.\ue204 \ue200cite\ue202turn0search2\ue201\ue206<\/p>\n\n\n\n 1. Account for your observations.<\/strong><\/p>\n\n\n\n \ue203Upon adding a sparingly soluble salt like AgCl to water, it partially dissolves, releasing its ions into the solution until the concentration of these ions reaches a point where the rate of dissolution equals the rate of precipitation. This dynamic equilibrium results in a saturated solution where the concentration of dissolved ions remains constant.\ue204\ue206<\/p>\n\n\n\n 2. Did the precipitated salt dissolve? Explain.<\/strong><\/p>\n\n\n\n \ue203Yes, the precipitated salt did dissolve to some extent. The extent of dissolution depends on the salt’s K\u209b\u209a value. For AgCl, with a K\u209b\u209a of 1.8 \u00d7 10\u207b\u00b9\u2070, only a small amount dissolves, leading to a low concentration of Ag\u207a and Cl\u207b ions in the solution.\ue204\ue206<\/p>\n\n\n\n 3. What effect did the addition of a common ion have on the contents of the test tube? Explain.<\/strong><\/p>\n\n\n\n \ue203Adding a common ion, such as NaCl, to the solution introduces additional Cl\u207b ions. According to Le Ch\u00e2telier’s principle, the system will adjust to counteract this change by shifting the equilibrium to the left, favoring the formation of more solid AgCl. This results in increased precipitation of AgCl, thereby decreasing its solubility in the solution. This phenomenon is known as the common-ion effect.\ue204 \ue200cite\ue202turn0search21\ue201\ue206<\/p>\n\n\n\n \ue203In summary, the dissolution of sparingly soluble salts is governed by their K\u209b\u209a values, and the addition of a common ion decreases their solubility by shifting the dissolution equilibrium toward the solid phase.\ue204<\/p>\n","protected":false},"excerpt":{"rendered":" Equilibria Involving Sparingly Soluble Salts The Correct Answer and Explanation is : \ue203When a sparingly soluble salt is added to water, it establishes an equilibrium between its solid form and its constituent ions in solution.\ue204 For example, consider the dissolution of silver chloride (AgCl):\ue206 \ue203AgCl (s)\u21ccAg+(aq)+Cl\u2212(aq)\\text{AgCl (s)} \\rightleftharpoons \\text{Ag}^+ (\\text{aq}) + \\text{Cl}^- (\\text{aq})\ue204\ue206 \ue203The solubility product […]<\/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-180929","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/180929","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=180929"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/180929\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=180929"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=180929"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=180929"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}