{"id":187458,"date":"2025-02-05T03:32:44","date_gmt":"2025-02-05T03:32:44","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187458"},"modified":"2025-02-05T03:32:46","modified_gmt":"2025-02-05T03:32:46","slug":"using-the-kas-for-hc2h3o2-and-hco3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/05\/using-the-kas-for-hc2h3o2-and-hco3\/","title":{"rendered":"Using the Ka&#8217;s for HC2H3O2 and HCO3"},"content":{"rendered":"\n<p>Using the Ka&#8217;s for HC2H3O2 and HCO3- calculate the Kb&#8217;s for the C2H3O2- and CO3-2 ions.<\/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>To calculate the base dissociation constant (( K_b )) for the conjugate bases of acetic acid (( \\text{HC}_2\\text{H}_3\\text{O}_2 )) and bicarbonate (( \\text{HCO}_3^- )), we use the relationship:<\/p>\n\n\n\n<p>[<br>K_w = K_a \\times K_b<br>]<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_w ) is the ionization constant of water (( 1.0 \\times 10^{-14} ) at 25\u00b0C),<\/li>\n\n\n\n<li>( K_a ) is the acid dissociation constant,<\/li>\n\n\n\n<li>( K_b ) is the base dissociation constant.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Given ( K_a ) values:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_a ) for acetic acid (( \\text{HC}_2\\text{H}_3\\text{O}_2 )) = ( 1.8 \\times 10^{-5} )<\/li>\n\n\n\n<li>( K_a ) for bicarbonate (( \\text{HCO}_3^- )) = ( 4.8 \\times 10^{-11} )<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Calculating ( K_b ):<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>For the acetate ion (( \\text{C}_2\\text{H}_3\\text{O}_2^- ))<\/strong>:<br>[<br>K_b = \\frac{K_w}{K_a} = \\frac{1.0 \\times 10^{-14}}{1.8 \\times 10^{-5}}<br>]<br>[<br>K_b = 5.56 \\times 10^{-10}<br>]<\/li>\n\n\n\n<li><strong>For the carbonate ion (( \\text{CO}_3^{2-} ))<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_a ) for bicarbonate (( \\text{HCO}_3^- )) corresponds to the second dissociation step of carbonic acid.<\/li>\n\n\n\n<li>The conjugate base of bicarbonate is carbonate (( \\text{CO}_3^{2-} )). [<br>K_b = \\frac{K_w}{K_a} = \\frac{1.0 \\times 10^{-14}}{4.8 \\times 10^{-11}}<br>] [<br>K_b = 2.08 \\times 10^{-4}<br>]<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The ( K_b ) values represent the strength of the conjugate bases. Since acetate (( \\text{C}_2\\text{H}_3\\text{O}_2^- )) is derived from a weak acid (acetic acid), it has a low ( K_b ), making it a weak base. On the other hand, carbonate (( \\text{CO}_3^{2-} )) is derived from bicarbonate, which is a much weaker acid, leading to a higher ( K_b ), making carbonate a stronger base.<\/p>\n\n\n\n<p>This calculation is crucial in acid-base chemistry to understand the behavior of conjugate acid-base pairs in aqueous solutions.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Using the Ka&#8217;s for HC2H3O2 and HCO3- calculate the Kb&#8217;s for the C2H3O2- and CO3-2 ions. The Correct Answer and Explanation is : To calculate the base dissociation constant (( K_b )) for the conjugate bases of acetic acid (( \\text{HC}_2\\text{H}_3\\text{O}_2 )) and bicarbonate (( \\text{HCO}_3^- )), we use the relationship: [K_w = K_a \\times [&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-187458","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187458","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=187458"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187458\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187458"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187458"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187458"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}