{"id":187774,"date":"2025-02-06T06:31:48","date_gmt":"2025-02-06T06:31:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187774"},"modified":"2025-02-06T06:31:50","modified_gmt":"2025-02-06T06:31:50","slug":"what-are-the-net-ionic-equations-for-the-hydrolysis-of-the-the-following","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/06\/what-are-the-net-ionic-equations-for-the-hydrolysis-of-the-the-following\/","title":{"rendered":"What are the net ionic equations for the hydrolysis of the the following"},"content":{"rendered":"\n<p>What are the net ionic equations for the hydrolysis of the the following:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>NaC2H3O2 2. Na2CO3 3. NH4CL 4.ZnCl2 5.KAl (SO4)2 6.KAl(SO4)2 for 5 &amp; 6 there are supposed to be 2 different hydrolysis reactions occurring Also determine if each is Ka or Kb<\/li>\n<\/ol>\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<h3 class=\"wp-block-heading\">Net Ionic Equations for Hydrolysis Reactions<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Sodium Acetate (NaC\u2082H\u2083O\u2082)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reaction:<\/strong><br>[<br>C_2H_3O_2^- + H_2O \\rightleftharpoons HC_2H_3O_2 + OH^-<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Base hydrolysis (( K_b )), since acetate (( C_2H_3O_2^- )) is the conjugate base of a weak acid (acetic acid, ( HC_2H_3O_2 )).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Sodium Carbonate (Na\u2082CO\u2083)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reactions:<\/strong> (Stepwise hydrolysis of carbonate)<br>[<br>CO_3^{2-} + H_2O \\rightleftharpoons HCO_3^- + OH^-<br>]<br>[<br>HCO_3^- + H_2O \\rightleftharpoons H_2CO_3 + OH^-<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Base hydrolysis (( K_b )), since carbonate acts as a weak base.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Ammonium Chloride (NH\u2084Cl)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reaction:<\/strong><br>[<br>NH_4^+ + H_2O \\rightleftharpoons NH_3 + H_3O^+<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Acid hydrolysis (( K_a )), since ammonium (( NH_4^+ )) is the conjugate acid of ammonia.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Zinc Chloride (ZnCl\u2082)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reaction:<\/strong><br>[<br>Zn^{2+} + 2H_2O \\rightleftharpoons Zn(OH)_2 + 2H^+<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Acid hydrolysis (( K_a )), since ( Zn^{2+} ) hydrolyzes to release ( H^+ ), making the solution acidic.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Potassium Aluminum Sulfate (KAl(SO\u2084)\u2082)<\/strong> &#8211; First Hydrolysis<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reaction:<\/strong><br>[<br>Al^{3+} + 3H_2O \\rightleftharpoons Al(OH)_3 + 3H^+<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Acid hydrolysis (( K_a )), since ( Al^{3+} ) hydrolyzes and produces ( H^+ ).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Potassium Aluminum Sulfate (KAl(SO\u2084)\u2082)<\/strong> &#8211; Second Hydrolysis<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reaction:<\/strong><br>[<br>SO_4^{2-} + H_2O \\rightleftharpoons HSO_4^- + OH^-<br>]<\/li>\n\n\n\n<li><strong>Type:<\/strong> Base hydrolysis (( K_b )), since sulfate acts as a weak base.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (300 Words)<\/h3>\n\n\n\n<p>Hydrolysis occurs when ions from a salt react with water to form acidic or basic solutions. The determining factor is whether the salt&#8217;s cation or anion originates from a strong or weak acid or base.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sodium acetate (NaC\u2082H\u2083O\u2082)<\/strong> hydrolyzes because acetate (( C_2H_3O_2^- )) is the conjugate base of a weak acid (acetic acid). It reacts with water to produce hydroxide ions (( OH^- )), making the solution basic (( K_b )).<\/li>\n\n\n\n<li><strong>Sodium carbonate (Na\u2082CO\u2083)<\/strong> undergoes stepwise hydrolysis. The carbonate ion (( CO_3^{2-} )) is a strong base and reacts with water to form bicarbonate (( HCO_3^- )) and hydroxide ions (( OH^- )), increasing the pH (( K_b )).<\/li>\n\n\n\n<li><strong>Ammonium chloride (NH\u2084Cl)<\/strong> contains ammonium (( NH_4^+ )), the conjugate acid of ammonia. It donates a proton to water, forming hydronium (( H_3O^+ )), making the solution acidic (( K_a )).<\/li>\n\n\n\n<li><strong>Zinc chloride (ZnCl\u2082)<\/strong> undergoes hydrolysis because ( Zn^{2+} ) is a small, highly charged metal ion. It interacts with water, forming zinc hydroxide and releasing protons, thus decreasing the pH (( K_a )).<\/li>\n\n\n\n<li><strong>Potassium aluminum sulfate (KAl(SO\u2084)\u2082)<\/strong> has two hydrolysis reactions:<\/li>\n\n\n\n<li><strong>Aluminum ion (( Al^{3+} ))<\/strong> hydrolyzes, producing ( H^+ ), making the solution acidic (( K_a )).<\/li>\n\n\n\n<li><strong>Sulfate ion (( SO_4^{2-} ))<\/strong> hydrolyzes weakly, producing ( OH^- ), contributing to basicity (( K_b )).<\/li>\n<\/ul>\n\n\n\n<p>The net effect of these hydrolysis reactions determines whether the salt solution is acidic or basic, impacting real-world applications like buffer solutions and industrial chemistry.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What are the net ionic equations for the hydrolysis of the the following: The Correct Answer and Explanation is : Net Ionic Equations for Hydrolysis Reactions Explanation (300 Words) Hydrolysis occurs when ions from a salt react with water to form acidic or basic solutions. The determining factor is whether the salt&#8217;s cation or anion [&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-187774","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187774","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=187774"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187774\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187774"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187774"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187774"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}