The two pKa values of sulfuric acid (H\u2082SO\u2084) are:<\/strong><\/p>\n\n\n\n Sulfuric acid (H\u2082SO\u2084) is a diprotic acid<\/strong>, meaning it can donate two protons (H\u207a) in aqueous solution. Each of these proton donations is associated with a specific acid dissociation constant (Ka)<\/strong>, which is commonly expressed as pKa<\/strong>, the negative logarithm of Ka. The lower the pKa value, the stronger the acid.<\/p>\n\n\n\n H2SO4\u2192H++HSO4\u2212\\text{H}_2\\text{SO}_4 \\rightarrow \\text{H}^+ + \\text{HSO}_4^-H2\u200bSO4\u200b\u2192H++HSO4\u2212\u200b<\/p>\n\n\n\n This step is a strong acid dissociation<\/strong>, meaning it occurs almost completely in water. Because of this, the first pKa is very low\u2014approximately \u20133<\/strong>. In aqueous solution, virtually all H\u2082SO\u2084 molecules dissociate to form hydrogen ions (H\u207a) and hydrogen sulfate ions (HSO\u2084\u207b), making sulfuric acid one of the strongest known mineral acids.<\/p>\n\n\n\n HSO4\u2212\u21ccH++SO42\u2212\\text{HSO}_4^- \\rightleftharpoons \\text{H}^+ + \\text{SO}_4^{2-}HSO4\u2212\u200b\u21ccH++SO42\u2212\u200b<\/p>\n\n\n\n This is a weaker acid dissociation<\/strong> compared to the first step. The hydrogen sulfate ion (HSO\u2084\u207b) is amphiprotic\u2014it can act as both an acid and a base. The equilibrium for this second dissociation lies less completely toward the right, with a pKa of approximately 1.99<\/strong>. This value indicates that HSO\u2084\u207b is still a relatively strong acid, though significantly weaker than H\u2082SO\u2084.<\/p>\n\n\n\n Understanding the two pKa values is critical in acid\u2013base chemistry, especially in titration curves, buffer systems, and industrial applications where sulfuric acid is used. In many practical contexts, only the first dissociation is considered when dealing with strong acids, because it is complete. However, in reactions where the pH is closer to neutral or in more dilute solutions, the second dissociation step becomes relevant.<\/p>\n\n\n\n List the 2 pKa’s for H2SO4 The Correct Answer and Explanation is: The two pKa values of sulfuric acid (H\u2082SO\u2084) are: Explanation: Sulfuric acid (H\u2082SO\u2084) is a diprotic acid, meaning it can donate two protons (H\u207a) in aqueous solution. Each of these proton donations is associated with a specific acid dissociation constant (Ka), which is […]<\/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-231979","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231979","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=231979"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231979\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231979"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231979"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231979"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}\n
\n\n\n\nExplanation:<\/h3>\n\n\n\n
First Dissociation:<\/h4>\n\n\n\n
Second Dissociation:<\/h4>\n\n\n\n
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<\/figure>\n","protected":false},"excerpt":{"rendered":"