The conjugate base of an acid is the species that remains after the acid donates a proton (H\u207a). This principle follows the Br\u00f8nsted-Lowry definition of acids and bases. Now, let\u2019s analyze each given acid and identify its conjugate base.<\/p>\n\n\n\n
- \n
- Hypochlorous acid (HOCl):<\/strong> HOCl is a weak acid, and it donates a proton to form its conjugate base. The removal of a proton leaves behind hypochlorite (OCl\u207b<\/strong>), as shown in the equation:<\/li>\n<\/ol>\n\n\n\n
HOCl\u2192OCl\u207b+H\u207a\\text{HOCl} \\rightarrow \\text{OCl\u207b} + \\text{H\u207a}<\/p>\n\n\n\n
- \n
- Sulfuric acid (H\u2082SO\u2084):<\/strong> H\u2082SO\u2084 is a strong acid and undergoes complete ionization in water. When it loses one proton, the resulting species is bisulfate (HSO\u2084\u207b<\/strong>). Further loss of another proton results in sulfate (SO\u2084\u00b2\u207b<\/strong>). The first dissociation is:<\/li>\n<\/ol>\n\n\n\n
H\u2082SO\u2084\u2192HSO\u2084\u207b+H\u207a\\text{H\u2082SO\u2084} \\rightarrow \\text{HSO\u2084\u207b} + \\text{H\u207a}<\/p>\n\n\n\n
The second dissociation is:<\/p>\n\n\n\n
HSO\u2084\u207b\u2192SO\u2084\u00b2\u207b+H\u207a\\text{HSO\u2084\u207b} \\rightarrow \\text{SO\u2084\u00b2\u207b} + \\text{H\u207a}<\/p>\n\n\n\n
- \n
- Pyridinium ion (H\u2085C\u2085NH\u2082\u207a):<\/strong> The pyridinium ion is the protonated form of pyridine (C\u2085H\u2085N). When it donates a proton, the resulting conjugate base is pyridine (C\u2085H\u2085N<\/strong>), as represented by:<\/li>\n<\/ol>\n\n\n\n
H\u2085C\u2085NH\u2082\u207a\u2192C\u2085H\u2085N+H\u207a\\text{H\u2085C\u2085NH\u2082\u207a} \\rightarrow \\text{C\u2085H\u2085N} + \\text{H\u207a}<\/p>\n\n\n\n
Explanation<\/h3>\n\n\n\n
The concept of conjugate acid-base pairs is fundamental in acid-base chemistry. Acids donate protons and transform into their conjugate bases, while bases accept protons and turn into their conjugate acids.<\/p>\n\n\n\n
For HOCl, the loss of an H\u207a results in hypochlorite (OCl\u207b), which can act as a weak base in aqueous solutions. The equilibrium between HOCl and OCl\u207b plays an important role in disinfection and water treatment.<\/p>\n\n\n\n
Sulfuric acid, being diprotic, has two conjugate bases. HSO\u2084\u207b is relatively acidic, allowing it to donate another proton to form SO\u2084\u00b2\u207b. The sulfate ion is highly stable and commonly found in salts such as sodium sulfate (Na\u2082SO\u2084).<\/p>\n\n\n\n
The pyridinium ion originates from pyridine, a widely used organic compound in pharmaceuticals and catalysts. Its conjugate base, pyridine (C\u2085H\u2085N), is a weak base due to the nitrogen\u2019s ability to accept a proton.<\/p>\n\n\n\n
Understanding these conjugate bases is essential for predicting acid-base behavior, equilibrium reactions, and buffer systems in various chemical applications.<\/p>\n\n\n\n
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<\/figure>\n","protected":false},"excerpt":{"rendered":"What is the conjugate base of the following acids: HOCl H2SO4 H5C5NH2+ The Correct Answer and Explanation is: The conjugate base of an acid is the species that remains after the acid donates a proton (H\u207a). This principle follows the Br\u00f8nsted-Lowry definition of acids and bases. Now, let\u2019s analyze each given acid and identify its […]<\/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-231443","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231443","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=231443"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231443\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231443"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231443"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231443"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- Pyridinium ion (H\u2085C\u2085NH\u2082\u207a):<\/strong> The pyridinium ion is the protonated form of pyridine (C\u2085H\u2085N). When it donates a proton, the resulting conjugate base is pyridine (C\u2085H\u2085N<\/strong>), as represented by:<\/li>\n<\/ol>\n\n\n\n
- Sulfuric acid (H\u2082SO\u2084):<\/strong> H\u2082SO\u2084 is a strong acid and undergoes complete ionization in water. When it loses one proton, the resulting species is bisulfate (HSO\u2084\u207b<\/strong>). Further loss of another proton results in sulfate (SO\u2084\u00b2\u207b<\/strong>). The first dissociation is:<\/li>\n<\/ol>\n\n\n\n