{"id":269005,"date":"2025-07-24T10:16:56","date_gmt":"2025-07-24T10:16:56","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=269005"},"modified":"2025-07-24T10:16:58","modified_gmt":"2025-07-24T10:16:58","slug":"write-equations-which-represent-the-dissociation-of-each-of-these-acids-or-bases-in-aqueous-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/24\/write-equations-which-represent-the-dissociation-of-each-of-these-acids-or-bases-in-aqueous-solution\/","title":{"rendered":"Write equations which represent the dissociation of each of these acids or bases in aqueous solution"},"content":{"rendered":"\n

Write equations which represent the dissociation of each of these acids or bases in aqueous solution. Use a single arrow in the case of a strong acid or base, and a double arrow to represent the equilibrium condition that exists in the solution of a weak acid or base. a) KOH b) HClO4 c) HCN d) C6H5NH2 (a weak base)<\/p>\n\n\n\n

The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Dissociation Equations:<\/h3>\n\n\n\n
    \n
  1. KOH (Strong Base)<\/strong>
    Equation<\/strong>: KOH(aq)\u2192K+(aq)+OH\u2212(aq)\\text{KOH} (aq) \\rightarrow \\text{K}^+ (aq) + \\text{OH}^- (aq) Explanation<\/strong>: Potassium hydroxide (KOH) is a strong base, meaning it dissociates completely in aqueous solution. The potassium ion (K\u207a) and hydroxide ion (OH\u207b) are produced in a 1:1 ratio.<\/li>\n\n\n\n
  2. HClO\u2084 (Strong Acid)<\/strong>
    Equation<\/strong>: HClO4(aq)\u2192H+(aq)+ClO4\u2212(aq)\\text{HClO}_4 (aq) \\rightarrow \\text{H}^+ (aq) + \\text{ClO}_4^- (aq) Explanation<\/strong>: Perchloric acid (HClO\u2084) is a strong acid and dissociates completely in water, releasing hydrogen ions (H\u207a) and perchlorate ions (ClO\u2084\u207b). The dissociation happens without equilibrium, meaning no reversible reaction occurs.<\/li>\n\n\n\n
  3. HCN (Weak Acid)<\/strong>
    Equation<\/strong>: HCN(aq)\u21ccH+(aq)+CN\u2212(aq)\\text{HCN} (aq) \\rightleftharpoons \\text{H}^+ (aq) + \\text{CN}^- (aq) Explanation<\/strong>: Hydrocyanic acid (HCN) is a weak acid, meaning it only partially dissociates in aqueous solution. The reaction reaches an equilibrium where both HCN and its dissociation products (H\u207a and CN\u207b) exist in the solution.<\/li>\n\n\n\n
  4. C\u2086H\u2085NH\u2082 (Weak Base)<\/strong>
    Equation<\/strong>: C6H5NH2(aq)+H2O(l)\u21ccC6H5NH3+(aq)+OH\u2212(aq)\\text{C}_6\\text{H}_5\\text{NH}_2 (aq) + \\text{H}_2\\text{O} (l) \\rightleftharpoons \\text{C}_6\\text{H}_5\\text{NH}_3^+ (aq) + \\text{OH}^- (aq) Explanation<\/strong>: Aniline (C\u2086H\u2085NH\u2082) is a weak base, so it reacts partially with water. The reaction is reversible, producing aniline hydrochloride (C\u2086H\u2085NH\u2083\u207a) and hydroxide ions (OH\u207b), and the system reaches an equilibrium.<\/li>\n<\/ol>\n\n\n\n

    Summary:<\/h3>\n\n\n\n
      \n
    • Strong acids and bases<\/strong> like HClO\u2084 and KOH dissociate completely in solution, represented by a single arrow.<\/li>\n\n\n\n
    • Weak acids and bases<\/strong> like HCN and C\u2086H\u2085NH\u2082 dissociate partially, represented by a double arrow to indicate equilibrium. The concentration of the undissociated acid or base remains significant, and the products are in equilibrium with each other.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

      Write equations which represent the dissociation of each of these acids or bases in aqueous solution. Use a single arrow in the case of a strong acid or base, and a double arrow to represent the equilibrium condition that exists in the solution of a weak acid or base. a) KOH b) HClO4 c) HCN […]<\/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-269005","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/269005","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=269005"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/269005\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=269005"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=269005"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=269005"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}