{"id":184545,"date":"2025-01-21T06:44:14","date_gmt":"2025-01-21T06:44:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184545"},"modified":"2025-01-21T06:44:16","modified_gmt":"2025-01-21T06:44:16","slug":"assuming-equal-concentrations-and-complete-dissociation","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/assuming-equal-concentrations-and-complete-dissociation\/","title":{"rendered":"Assuming equal concentrations and complete dissociation"},"content":{"rendered":"\n

Assuming equal concentrations and complete dissociation, match these aqueous solutions to their relative freezing points. Na2SO4 Highest freezing point v KI Choose… Li3PO4 Choose…<\/p>\n\n\n\n

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

To match these aqueous solutions to their relative freezing points, we need to consider the van’t Hoff factor (ii)<\/strong>, which represents the number of particles into which a compound dissociates in solution. The freezing point depression is directly proportional to ii, so the greater the number of dissolved particles, the lower the freezing point of the solution.<\/p>\n\n\n\n

Step 1: Calculate ii for each compound<\/h3>\n\n\n\n
    \n
  1. Na2_2SO4_4:<\/strong> Sodium sulfate dissociates into three ions: Na2SO4\u21922Na++SO42\u2212\\text{Na}_2\\text{SO}_4 \\rightarrow 2\\text{Na}^+ + \\text{SO}_4^{2-} Here, i=3i = 3.<\/li>\n\n\n\n
  2. KI:<\/strong> Potassium iodide dissociates into two ions: KI\u2192K++I\u2212\\text{KI} \\rightarrow \\text{K}^+ + \\text{I}^- Here, i=2i = 2.<\/li>\n\n\n\n
  3. Li3_3PO4_4:<\/strong> Lithium phosphate dissociates into four ions: Li3PO4\u21923Li++PO43\u2212\\text{Li}_3\\text{PO}_4 \\rightarrow 3\\text{Li}^+ + \\text{PO}_4^{3-} Here, i=4i = 4.<\/li>\n<\/ol>\n\n\n\n

    Step 2: Freezing point depression relationship<\/h3>\n\n\n\n

    The freezing point depression is given by: \u0394Tf=i\u22c5Kf\u22c5m\\Delta T_f = i \\cdot K_f \\cdot m<\/p>\n\n\n\n

    Since all solutions are at equal concentrations and KfK_f is constant for water, the relative freezing points depend only on ii:<\/p>\n\n\n\n

      \n
    • Higher ii:<\/strong> Greater freezing point depression (lower freezing point).<\/li>\n\n\n\n
    • Lower ii:<\/strong> Smaller freezing point depression (higher freezing point).<\/li>\n<\/ul>\n\n\n\n

      Step 3: Rank freezing points<\/h3>\n\n\n\n
        \n
      • i=2i = 2 (KI) \u2192 Highest freezing point<\/strong>.<\/li>\n\n\n\n
      • i=3i = 3 (Na2_2SO4_4) \u2192 Intermediate freezing point<\/strong>.<\/li>\n\n\n\n
      • i=4i = 4 (Li3_3PO4_4) \u2192 Lowest freezing point<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        Final Answer:<\/h3>\n\n\n\n
          \n
        • Na2_2SO4_4: Intermediate freezing point<\/strong>.<\/li>\n\n\n\n
        • KI: Highest freezing point<\/strong>.<\/li>\n\n\n\n
        • Li3_3PO4_4: Lowest freezing point<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Explanation:<\/h3>\n\n\n\n

          The freezing point depression depends on the number of dissolved particles (ii). KI produces the fewest particles (i=2i=2), leading to the least depression and the highest freezing point. Li3_3PO4_4 produces the most particles (i=4i=4), resulting in the greatest depression and the lowest freezing point. Na2_2SO4_4 lies in between with i=3i=3.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Assuming equal concentrations and complete dissociation, match these aqueous solutions to their relative freezing points. Na2SO4 Highest freezing point v KI Choose… Li3PO4 Choose… The Correct Answer and Explanation is : To match these aqueous solutions to their relative freezing points, we need to consider the van’t Hoff factor (ii), which represents the number of […]<\/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-184545","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184545","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=184545"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184545\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184545"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184545"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184545"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}