{"id":218916,"date":"2025-05-24T16:40:04","date_gmt":"2025-05-24T16:40:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=218916"},"modified":"2025-05-24T16:40:06","modified_gmt":"2025-05-24T16:40:06","slug":"write-the-net-ionic-equation-for-the-reaction-that-occurs-when-equal-volumes-of-0-056-m-aqueous-formic-acid-and-sodiumacetate-are-mixed","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/24\/write-the-net-ionic-equation-for-the-reaction-that-occurs-when-equal-volumes-of-0-056-m-aqueous-formic-acid-and-sodiumacetate-are-mixed\/","title":{"rendered":"Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed."},"content":{"rendered":"\n<p>formic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 HCOOH acetic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 CH3COOH HCOOH\u00c3\u201a\u00c2 is a stronger acid than\u00c3\u201a\u00c2 CH3COOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion Which is the strongest base, HCOO- or CH3COO- At equilibrium will the (reactants or products) be favored. \u00c3\u201a\u00c2<br>formic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 HCOOH<br>acetic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 CH3COOH<\/p>\n\n\n\n<p>HCOOH\u00c3\u201a\u00c2 is a stronger acid than\u00c3\u201a\u00c2 CH3COOH<\/p>\n\n\n\n<p>(1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion<\/p>\n\n\n\n<p>Which is the strongest base, HCOO- or CH3COO-<\/p>\n\n\n\n<p>At equilibrium will the (reactants or products) be favored.<\/p>\n\n\n\n<p>\u00c3\u201a\u00c2<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Answer:<\/strong><\/p>\n\n\n\n<p><strong>(1) Net ionic equation:<\/strong> HCOOH+CH3COO\u2212\u21ccCH3COOH+HCOO\u2212\\text{HCOOH} + \\text{CH}_3\\text{COO}^- \\rightleftharpoons \\text{CH}_3\\text{COOH} + \\text{HCOO}^-<\/p>\n\n\n\n<p><strong>Strongest base:<\/strong><br>CH\u2083COO\u207b (acetate ion)<\/p>\n\n\n\n<p><strong>At equilibrium, the:<\/strong><br><strong>Reactants<\/strong> will be favored.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation <\/h3>\n\n\n\n<p>The reaction involves mixing formic acid (HCOOH), a weak acid, with sodium acetate (CH\u2083COONa), a salt that dissociates to produce acetate ions (CH\u2083COO\u207b), the conjugate base of acetic acid. The key process here is an <strong>acid-base reaction<\/strong> between formic acid (an acid) and acetate (a base).<\/p>\n\n\n\n<p>The <strong>net ionic equation<\/strong> focuses only on the species that change in the reaction: HCOOH+CH3COO\u2212\u21ccCH3COOH+HCOO\u2212\\text{HCOOH} + \\text{CH}_3\\text{COO}^- \\rightleftharpoons \\text{CH}_3\\text{COOH} + \\text{HCOO}^-<\/p>\n\n\n\n<p>This represents a <strong>proton transfer<\/strong>: formic acid donates a proton (H\u207a) to acetate, forming acetic acid and formate ion.<\/p>\n\n\n\n<p>To understand equilibrium direction, we compare acid strengths using their <strong>conjugate bases<\/strong>. It\u2019s stated that <strong>formic acid is stronger than acetic acid<\/strong>. That means:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>HCOOH \u21cc H\u207a + HCOO\u207b has a <strong>greater tendency to donate protons<\/strong> than<\/li>\n\n\n\n<li>CH\u2083COOH \u21cc H\u207a + CH\u2083COO\u207b<\/li>\n<\/ul>\n\n\n\n<p>Thus, <strong>HCOO\u207b is a weaker base<\/strong> than CH\u2083COO\u207b. A stronger acid has a <strong>weaker conjugate base<\/strong>.<\/p>\n\n\n\n<p>Since the stronger acid (HCOOH) reacts with the stronger base (CH\u2083COO\u207b), the system shifts <strong>toward the weaker acid-base pair<\/strong>: CH\u2083COOH and HCOO\u207b.<\/p>\n\n\n\n<p>In acid-base equilibria, the position favors the side with the <strong>weaker acid and base<\/strong>, i.e., the side that is <strong>less reactive<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>CH\u2083COO\u207b is the stronger base<\/strong>.<\/li>\n\n\n\n<li>Since the stronger acid and stronger base are on the left, <strong>the reactants are favored at equilibrium<\/strong>.<\/li>\n\n\n\n<li>This means only a small amount of product (CH\u2083COOH and HCOO\u207b) will form.<\/li>\n<\/ul>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/image-385.png\" alt=\"\" class=\"wp-image-218917\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>formic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 HCOOH acetic acid \u00c3\u201a\u00c2 = \u00c3\u201a\u00c2 CH3COOH HCOOH\u00c3\u201a\u00c2 is a stronger acid than\u00c3\u201a\u00c2 CH3COOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed. It is not necessary to include states such as (aq) or (s). [&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-218916","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218916","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=218916"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218916\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=218916"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=218916"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=218916"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}