{"id":191509,"date":"2025-02-15T07:32:23","date_gmt":"2025-02-15T07:32:23","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191509"},"modified":"2025-02-15T07:32:25","modified_gmt":"2025-02-15T07:32:25","slug":"the-ka-of-h2co3-is-4-3-x-10-7","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/15\/the-ka-of-h2co3-is-4-3-x-10-7\/","title":{"rendered":"The Ka of H2CO3 is 4.3 x 10-7"},"content":{"rendered":"\n<p>The Ka of H2CO3 is 4.3 x 10-7. What is the Kb for its conjugate Base HCO3?<br>Hint: for acid-base conjugate pairs:<br>Ka. Kb Kw Kw 1&#215;10-14<br>Pka+Pkb-14<br>2.3 x 108<br>6.3 x 10-8<br>53&#215;108<br>45&#215;108<\/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 Kb of the conjugate base HCO3^- for the acid H2CO3, we can use the relationship between the acid dissociation constant (Ka) and the base dissociation constant (Kb) for conjugate acid-base pairs. The equation we will use is:<\/p>\n\n\n\n<p>[<br>K_a \\times K_b = K_w<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_a ) is the acid dissociation constant for H2CO3.<\/li>\n\n\n\n<li>( K_b ) is the base dissociation constant for the conjugate base HCO3^-.<\/li>\n\n\n\n<li>( K_w ) is the ionization constant for water, which is ( 1 \\times 10^{-14} ) at 25\u00b0C.<\/li>\n<\/ul>\n\n\n\n<p>Given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_a = 4.3 \\times 10^{-7} )<\/li>\n\n\n\n<li>( K_w = 1 \\times 10^{-14} )<\/li>\n<\/ul>\n\n\n\n<p>To solve for ( K_b ):<\/p>\n\n\n\n<p>[<br>K_b = \\frac{K_w}{K_a} = \\frac{1 \\times 10^{-14}}{4.3 \\times 10^{-7}}<br>]<\/p>\n\n\n\n<p>Now let&#8217;s calculate it.<\/p>\n\n\n\n<p>[<br>K_b = 2.33 \\times 10^{-8}<br>]<\/p>\n\n\n\n<p>Thus, the ( K_b ) for the conjugate base HCO3^- is ( 2.3 \\times 10^{-8} ).<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>The relationship between the acid dissociation constant (Ka) and the base dissociation constant (Kb) for a conjugate acid-base pair is an important concept in acid-base chemistry. When an acid dissociates in water, it produces hydronium ions (H3O+), and its conjugate base can accept protons to form the original acid. In the case of H2CO3, the bicarbonate ion (HCO3-) is the conjugate base.<\/p>\n\n\n\n<p>Using the equation ( K_a \\times K_b = K_w ), we know that the product of the acid dissociation constant and the base dissociation constant for a conjugate pair must always equal the ionization constant of water, ( K_w = 1 \\times 10^{-14} ). Therefore, by rearranging this equation and solving for ( K_b ), we can determine the base dissociation constant for the conjugate base HCO3^-.<\/p>\n\n\n\n<p>The value of ( K_b = 2.3 \\times 10^{-8} ) indicates that HCO3^- is a weak base, meaning it does not strongly accept protons.<\/p>\n\n\n\n<p>Let me generate a visual to represent this calculation.<\/p>\n\n\n\n<p>Here is the diagram that visually represents the relationship between ( K_a ), ( K_b ), and ( K_w ) for conjugate acid-base pairs, showing the calculation for ( K_b ) of HCO3^-.<\/p>\n\n\n\n<p>Let me know if you need any more clarifications or additional help with this!<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-579.png\" alt=\"\" class=\"wp-image-191510\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The Ka of H2CO3 is 4.3 x 10-7. What is the Kb for its conjugate Base HCO3?Hint: for acid-base conjugate pairs:Ka. Kb Kw Kw 1&#215;10-14Pka+Pkb-142.3 x 1086.3 x 10-853&#215;10845&#215;108 The Correct Answer and Explanation is : To calculate the Kb of the conjugate base HCO3^- for the acid H2CO3, we can use the relationship between [&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-191509","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191509","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=191509"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191509\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191509"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191509"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191509"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}