{"id":189596,"date":"2025-02-10T05:36:54","date_gmt":"2025-02-10T05:36:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189596"},"modified":"2025-02-10T05:36:56","modified_gmt":"2025-02-10T05:36:56","slug":"construct-the-expression-for-ksp-for-solid-zns-in-aqueous-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/10\/construct-the-expression-for-ksp-for-solid-zns-in-aqueous-solution\/","title":{"rendered":"Construct the expression for Ksp for solid ZnS in aqueous solution"},"content":{"rendered":"\n

Construct the expression for Ksp for solid ZnS in aqueous solution. ZnS(s) = Zn\u00b2+ (aq) + S\u00b2-(aq) Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile.. [ZnS] [Zn\u00b2+1\u00b2 2[ZnS] [S-] Ksp [ZnS]\u00b2 2[S] = [Zn+] [S-1\u00b2 2[Zn+] [S\u00b2-] [Zn+]\u00b2 2[S\u00b2] [Zn\u00b2+] [S\u00b2-1\u00b2 RESET 2[Zn\u00b2+]<\/p>\n\n\n\n

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

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

The solubility product constant, (K_{sp}), is an equilibrium constant that describes the solubility of a sparingly soluble salt in water. The general dissociation reaction of zinc sulfide (ZnS) in water is:<\/p>\n\n\n\n

[
\\text{ZnS(s)} \\rightleftharpoons \\text{Zn}^{2+} (aq) + \\text{S}^{2-} (aq)
]<\/p>\n\n\n\n

To construct the expression for (K_{sp}), we use the concentrations of the ions in the solution at equilibrium. The solubility product, (K_{sp}), is the product of the concentrations of the ions in solution, each raised to the power of their respective coefficients from the balanced dissociation equation.<\/p>\n\n\n\n

    \n
  1. Write the dissociation equation:<\/strong>
    [
    \\text{ZnS(s)} \\rightleftharpoons \\text{Zn}^{2+} (aq) + \\text{S}^{2-} (aq)
    ]<\/li>\n\n\n\n
  2. The equilibrium expression for (K_{sp}):<\/strong>
    The concentration of the solid ZnS does not appear in the expression because it is a solid, and the concentration of a pure solid is considered to be 1. The equilibrium expression will only include the aqueous ions: [
    K_{sp} = [\\text{Zn}^{2+}][\\text{S}^{2-}]
    ] Here, ([Zn^{2+}]) is the concentration of zinc ions, and ([S^{2-}]) is the concentration of sulfide ions in the solution at equilibrium.<\/li>\n\n\n\n
  3. Explanation of (K_{sp}):<\/strong>
    The solubility product constant ((K_{sp})) reflects the extent to which ZnS dissociates in water. Since ZnS is a sparingly soluble salt, only a small amount of it will dissolve in water, meaning the concentrations of (Zn^{2+}) and (S^{2-}) will be relatively low at equilibrium. However, these concentrations are essential to determine the solubility of the salt. The value of (K_{sp}) is specific to the temperature at which the equilibrium is established, and it allows you to calculate the solubility of ZnS in water. If the concentrations of (\\text{Zn}^{2+}) and (\\text{S}^{2-}) are known, you can substitute them into the (K_{sp}) expression to solve for the solubility of ZnS. Conversely, knowing the (K_{sp}) value allows you to predict the concentrations of the ions at equilibrium given the solubility of ZnS.<\/li>\n<\/ol>\n\n\n\n

    In summary, the expression for the solubility product of ZnS is:<\/p>\n\n\n\n

    [
    K_{sp} = [\\text{Zn}^{2+}][\\text{S}^{2-}]
    ]<\/p>\n\n\n\n

    This expression allows for the calculation of the solubility of ZnS in aqueous solution based on the concentrations of its dissociated ions.<\/p>\n","protected":false},"excerpt":{"rendered":"

    Construct the expression for Ksp for solid ZnS in aqueous solution. ZnS(s) = Zn\u00b2+ (aq) + S\u00b2-(aq) Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile.. [ZnS] [Zn\u00b2+1\u00b2 2[ZnS] [S-] Ksp [ZnS]\u00b2 2[S] = […]<\/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-189596","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189596","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=189596"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189596\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189596"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189596"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189596"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}