{"id":267194,"date":"2025-07-23T10:25:59","date_gmt":"2025-07-23T10:25:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267194"},"modified":"2025-07-23T10:26:01","modified_gmt":"2025-07-23T10:26:01","slug":"consider-the-acid-base-nature-of-calcium-chloride-cacl","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/consider-the-acid-base-nature-of-calcium-chloride-cacl\/","title":{"rendered":"Consider the acid-base nature of calcium chloride, CaCl"},"content":{"rendered":"\n

Consider the acid-base nature of calcium chloride, CaCl
, when it is dissolved in water. (1) What are the acid-base properties of the cation? (2) What are the acid-base properties of the anion? (3) Would an aqueous solution of calcium chloride be acidic, basic or neutral?<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

When calcium chloride (CaCl2) dissolves in water, it dissociates into calcium ions (Ca\u00b2\u207a) and chloride ions (Cl\u207b). Let’s analyze the acid-base properties of each ion:<\/p>\n\n\n\n

    \n
  1. Acid-Base Properties of the Cation (Ca\u00b2\u207a):<\/strong>
    The calcium ion (Ca\u00b2\u207a) is a highly charged metal ion and can interact with water molecules. It tends to polarize water molecules, making the hydrogen atoms more likely to dissociate into protons (H\u207a). This creates a slightly acidic environment, as Ca\u00b2\u207a can lead to the production of H\u207a ions by the following reaction: \\text{Ca}^{2+} + 6H_2O \\rightarrow \\text{[Ca(H2O)6]}^{2+} \\rightarrow \\text{[Ca(H2O)5]^{2+}} + H_2O \\rightarrow H^+ + OH^- Although calcium ions do not directly release protons themselves, they can increase the concentration of protons (H\u207a) through this interaction with water, making the solution weakly acidic. However, since this is not a strong acid-base reaction, the acidity is relatively low.<\/li>\n\n\n\n
  2. Acid-Base Properties of the Anion (Cl\u207b):<\/strong>
    The chloride ion (Cl\u207b) is the conjugate base of a strong acid (HCl). As a result, it does not readily react with water to produce OH\u207b ions, meaning it has no significant basicity. Chloride ions are neutral in solution and do not affect the pH of the solution.<\/li>\n\n\n\n
  3. Acid-Base Nature of the Aqueous Solution of Calcium Chloride:<\/strong>
    In an aqueous solution, the calcium cation (Ca\u00b2\u207a) is slightly acidic, while the chloride anion (Cl\u207b) is neutral. As a result, the overall solution of calcium chloride will be slightly acidic but not strongly so. The contribution of Ca\u00b2\u207a is small compared to other acids, so the solution will be nearly neutral with a slight tendency to lower the pH.<\/li>\n<\/ol>\n\n\n\n

    Conclusion:<\/h3>\n\n\n\n

    An aqueous solution of calcium chloride (CaCl2) is typically neutral to slightly acidic<\/strong> due to the weakly acidic nature of Ca\u00b2\u207a.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    Consider the acid-base nature of calcium chloride, CaCl, when it is dissolved in water. (1) What are the acid-base properties of the cation? (2) What are the acid-base properties of the anion? (3) Would an aqueous solution of calcium chloride be acidic, basic or neutral? The Correct Answer and Explanation is: When calcium chloride (CaCl2) […]<\/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-267194","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267194","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=267194"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267194\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267194"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267194"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267194"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}