{"id":183584,"date":"2025-01-16T17:16:24","date_gmt":"2025-01-16T17:16:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183584"},"modified":"2025-01-16T17:16:26","modified_gmt":"2025-01-16T17:16:26","slug":"a-lewis-electron-dot-diagram-of-the-oxalate-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/16\/a-lewis-electron-dot-diagram-of-the-oxalate-ion\/","title":{"rendered":"A Lewis electron-dot diagram of the oxalate ion"},"content":{"rendered":"\n

A Lewis electron-dot diagram of the oxalate ion, C_{2}O_{4} ^ 2- is shown. (a) Identify the hybridization of the valence orbitals of either carbon atom in the oxalate ion. (b) Silver oxalate, A<\/em>g_{2}C_{2}<\/em>O_{4}(s) is slightly soluble in water. The value of K sp for Ag_{2}<\/em>C_{2}*O_{4} is 5.4 * 10 ^ – 12 (i) Write the expression for the solubility-product constant, K sp for Ag_{2}<\/em>C_{2}O_{4} (ii) Calculate the molar solubility of A<\/em>g_{2}C_{2}<\/em>O_{4} in neutral distilled water.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

(a) Hybridization of Carbon in Oxalate Ion (C\u2082O\u2084\u00b2\u207b):<\/h3>\n\n\n\n

In the oxalate ion (C\u2082O\u2084\u00b2\u207b), each carbon atom is bonded to two oxygen atoms through single bonds and one oxygen atom through a double bond. This leads to the formation of a planar structure with resonance between the two possible structures (where the double bond shifts between the two carbon-oxygen bonds).<\/p>\n\n\n\n

Each carbon atom in the oxalate ion forms three sigma bonds: two with oxygen atoms and one with the other carbon atom. The carbon-carbon bond is a sigma bond, and the carbon-oxygen bonds include a sigma bond and a pi bond (for the double-bonded oxygen). This configuration implies that the carbon atoms are involved in three bonding regions, suggesting sp\u00b2 hybridization<\/strong> for each carbon atom.<\/p>\n\n\n\n

(b) Silver Oxalate Solubility:<\/h3>\n\n\n\n

(i) Expression for the Solubility-Product Constant (Ksp) of Ag\u2082C\u2082O\u2084:<\/h4>\n\n\n\n

The dissolution of silver oxalate (Ag\u2082C\u2082O\u2084) in water can be represented by the following equilibrium equation:<\/p>\n\n\n\n

[
\\text{Ag}_2\\text{C}_2\\text{O}_4 (s) \\rightleftharpoons 2 \\text{Ag}^+ (aq) + \\text{C}_2\\text{O}_4^{2-} (aq)
]<\/p>\n\n\n\n

The solubility product constant expression is:<\/p>\n\n\n\n

[
K_{sp} = [\\text{Ag}^+]^2 [\\text{C}_2\\text{O}_4^{2-}]
]<\/p>\n\n\n\n

where:<\/p>\n\n\n\n

    \n
  • ([\\text{Ag}^+]) is the concentration of silver ions,<\/li>\n\n\n\n
  • ([\\text{C}_2\\text{O}_4^{2-}]) is the concentration of oxalate ions.<\/li>\n<\/ul>\n\n\n\n

    (ii) Calculation of Molar Solubility:<\/h4>\n\n\n\n

    Let the molar solubility of Ag\u2082C\u2082O\u2084 in water be represented by (s). According to the dissolution reaction:<\/p>\n\n\n\n

      \n
    • For every 1 mole of Ag\u2082C\u2082O\u2084 that dissolves, 2 moles of Ag\u207a are produced, and 1 mole of C\u2082O\u2084\u00b2\u207b is produced.<\/li>\n<\/ul>\n\n\n\n

      Thus, at equilibrium:<\/p>\n\n\n\n

        \n
      • The concentration of Ag\u207a will be (2s),<\/li>\n\n\n\n
      • The concentration of C\u2082O\u2084\u00b2\u207b will be (s).<\/li>\n<\/ul>\n\n\n\n

        Substituting these concentrations into the Ksp expression:<\/p>\n\n\n\n

        [
        K_{sp} = (2s)^2 (s) = 4s^3
        ]<\/p>\n\n\n\n

        Given that the Ksp value is (5.4 \\times 10^{-12}), we can solve for (s):<\/p>\n\n\n\n

        [
        4s^3 = 5.4 \\times 10^{-12}
        ]<\/p>\n\n\n\n

        [
        s^3 = \\frac{5.4 \\times 10^{-12}}{4} = 1.35 \\times 10^{-12}
        ]<\/p>\n\n\n\n

        [
        s = \\sqrt[3]{1.35 \\times 10^{-12}} \\approx 1.1 \\times 10^{-4} \\, \\text{M}
        ]<\/p>\n\n\n\n

        Thus, the molar solubility of Ag\u2082C\u2082O\u2084 in neutral distilled water is approximately (1.1 \\times 10^{-4} \\, \\text{M}).<\/p>\n\n\n\n

        Explanation:<\/h3>\n\n\n\n
          \n
        1. Hybridization of Carbon<\/strong>: The carbon atoms in oxalate ion are sp\u00b2 hybridized because they are involved in three regions of bonding (two sigma bonds with oxygen and one with the other carbon atom), and the structure of oxalate is planar due to resonance.<\/li>\n\n\n\n
        2. Solubility of Silver Oxalate<\/strong>: The solubility product (Ksp) provides a way to quantify how much of a slightly soluble salt (like Ag\u2082C\u2082O\u2084) dissolves in water. The concentration of ions at equilibrium is calculated based on the dissociation of the compound into its ions. By solving for the molar solubility, we find the concentration of silver oxalate that will dissolve in water to be approximately (1.1 \\times 10^{-4} \\, \\text{M}).<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

          A Lewis electron-dot diagram of the oxalate ion, C_{2}O_{4} ^ 2- is shown. (a) Identify the hybridization of the valence orbitals of either carbon atom in the oxalate ion. (b) Silver oxalate, Ag_{2}C_{2}O_{4}(s) is slightly soluble in water. The value of K sp for Ag_{2}C_{2}*O_{4} is 5.4 * 10 ^ – 12 (i) Write the […]<\/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-183584","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183584","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=183584"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183584\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183584"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183584"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183584"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}