{"id":190992,"date":"2025-02-14T04:47:58","date_gmt":"2025-02-14T04:47:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=190992"},"modified":"2025-02-14T04:48:00","modified_gmt":"2025-02-14T04:48:00","slug":"this-is-the-net-ionic-equation-for-the-neutralization-of-a-hydrochloric-acid-with-sodium-hydroxide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/this-is-the-net-ionic-equation-for-the-neutralization-of-a-hydrochloric-acid-with-sodium-hydroxide\/","title":{"rendered":"This is the net ionic equation for the neutralization of a hydrochloric acid with sodium hydroxide"},"content":{"rendered":"\n<p>This is the net ionic equation for the neutralization of a hydrochloric acid with sodium hydroxide:<br>NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)<br>Na (aq) + Cl (aq) NaCl (aq)<br>OH (aq) + H+ (aq) \u2192 H2O (1)<br>NaOH (aq) + HCl (aq) \u2192 H2O (I) + NaCl (aq)<br>Na (aq) + H+(aq) \u2192 NaH (aq)<br>Question 3 (1 point)<br>This is the net ionic equation for the complete neutralization of a generic diprotic acid with sodium hydroxide:<br>H2A (aq) + 2 NaOH (aq) 2 H2O (I) + Na2A (aq)<br>OH (aq) + H+ (aq) \u2192 H2O (1)<br>2 Na (aq) + A2-(aq) \u2192 Na2Cl (s)<br>2 OH (aq) + 2 H* (aq) \u2192 2H2O (1)<\/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<h3 class=\"wp-block-heading\">Correct Net Ionic Equation:<\/h3>\n\n\n\n<p>For the complete neutralization of a <strong>generic diprotic acid<\/strong> (H\u2082A) with <strong>sodium hydroxide<\/strong> (NaOH), the correct net ionic equation is:<\/p>\n\n\n\n<p>[<br>H_2A (aq) + 2 OH^- (aq) \\rightarrow 2 H_2O (l) + A^{2-} (aq)<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (300 Words):<\/h3>\n\n\n\n<p>A <strong>diprotic acid<\/strong> is an acid that can donate two protons (H\u207a) per molecule. The general formula for a diprotic acid is <strong>H\u2082A<\/strong>, where &#8220;A&#8221; represents the conjugate base after losing both protons. Common examples of diprotic acids include <strong>sulfuric acid (H\u2082SO\u2084), carbonic acid (H\u2082CO\u2083), and oxalic acid (H\u2082C\u2082O\u2084)<\/strong>.<\/p>\n\n\n\n<p>When a diprotic acid reacts with <strong>sodium hydroxide (NaOH),<\/strong> a <strong>strong base<\/strong>, neutralization occurs in two steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>First Proton Donation:<\/strong><br>[<br>H_2A (aq) + OH^- (aq) \\rightarrow H_2O (l) + HA^- (aq)<br>]<br>The first hydroxide ion removes one proton from H\u2082A, forming the intermediate conjugate base <strong>HA\u207b<\/strong>.<\/li>\n\n\n\n<li><strong>Second Proton Donation:<\/strong><br>[<br>HA^- (aq) + OH^- (aq) \\rightarrow H_2O (l) + A^{2-} (aq)<br>]<br>The second hydroxide ion removes another proton from HA\u207b, leaving the final conjugate base <strong>A\u00b2\u207b<\/strong>.<\/li>\n<\/ol>\n\n\n\n<p>Since sodium hydroxide fully dissociates in water, Na\u207a ions are spectator ions and do not participate in the actual reaction. The final net ionic equation simplifies to:<\/p>\n\n\n\n<p>[<br>H_2A (aq) + 2 OH^- (aq) \\rightarrow 2 H_2O (l) + A^{2-} (aq)<br>]<\/p>\n\n\n\n<p>This equation represents the neutralization process for any diprotic acid reacting with a strong base. The reaction is essential in titration calculations, buffer solutions, and various industrial applications like wastewater treatment and pharmaceutical formulations.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>This is the net ionic equation for the neutralization of a hydrochloric acid with sodium hydroxide:NaOH (aq) + HCl (aq) H2O (l) + NaCl (aq)Na (aq) + Cl (aq) NaCl (aq)OH (aq) + H+ (aq) \u2192 H2O (1)NaOH (aq) + HCl (aq) \u2192 H2O (I) + NaCl (aq)Na (aq) + H+(aq) \u2192 NaH (aq)Question 3 [&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-190992","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190992","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=190992"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190992\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=190992"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=190992"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=190992"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}