{"id":198156,"date":"2025-03-08T12:34:20","date_gmt":"2025-03-08T12:34:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198156"},"modified":"2025-03-08T12:34:22","modified_gmt":"2025-03-08T12:34:22","slug":"calculate-the-boiling-and-freezing-points-of-water-solutions-that-are-1-15-m-in-the-following-solutes","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/08\/calculate-the-boiling-and-freezing-points-of-water-solutions-that-are-1-15-m-in-the-following-solutes\/","title":{"rendered":"Calculate the boiling and freezing points of water solutions that are 1.15 M in the following solutes"},"content":{"rendered":"\n

Calculate the boiling and freezing points of water solutions that are 1.15 M in the following solutes:<\/p>\n\n\n\n

a. KBr, a strong electrolyte<\/p>\n\n\n\n

b. ethylene glycol, a nonelectrolyte<\/p>\n\n\n\n

c. (NH4)2CO3, a strong electrolyte<\/p>\n\n\n\n

d. Al2(SO4)3, a strong electrolyte<\/p>\n\n\n\n

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

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

The boiling and freezing points of water solutions depend on the colligative properties of the solute, specifically the van’t Hoff factor (i), which reflects how many particles a solute dissociates into. Here’s how to calculate the changes for the solutions provided:<\/p>\n\n\n\n

Constants and Formula:<\/h3>\n\n\n\n
    \n
  • Freezing Point Depression<\/strong>: (\\Delta T_f = i \\times K_f \\times M)<\/li>\n\n\n\n
  • Boiling Point Elevation<\/strong>: (\\Delta T_b = i \\times K_b \\times M)<\/li>\n<\/ul>\n\n\n\n

    Where:<\/p>\n\n\n\n

      \n
    • (i) is the van’t Hoff factor (number of particles the solute dissociates into),<\/li>\n\n\n\n
    • (K_f = 1.86 \\, \\text{\u00b0C\u00b7kg\/mol}) is the cryoscopic constant for water,<\/li>\n\n\n\n
    • (K_b = 0.512 \\, \\text{\u00b0C\u00b7kg\/mol}) is the ebullioscopic constant for water,<\/li>\n\n\n\n
    • (M = 1.15 \\, \\text{mol\/L}) is the molarity of the solution.<\/li>\n<\/ul>\n\n\n\n

      Breakdown of Solutes:<\/h3>\n\n\n\n
        \n
      1. KBr (Strong Electrolyte)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
          \n
        • Dissociates into 2 particles: (K^+) and (Br^-) (i = 2).<\/li>\n\n\n\n
        • Boiling Point: (100\u00b0C + \\Delta T_b)<\/li>\n\n\n\n
        • Freezing Point: (0\u00b0C – \\Delta T_f)<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Ethylene Glycol (Nonelectrolyte)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
              \n
            • Does not dissociate (i = 1).<\/li>\n\n\n\n
            • Boiling Point: (100\u00b0C + \\Delta T_b)<\/li>\n\n\n\n
            • Freezing Point: (0\u00b0C – \\Delta T_f)<\/li>\n<\/ul>\n\n\n\n
                \n
              1. (NH4)2CO3 (Strong Electrolyte)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                  \n
                • Dissociates into 3 particles: (2 \\, NH_4^+) and (CO_3^{2-}) (i = 3).<\/li>\n\n\n\n
                • Boiling Point: (100\u00b0C + \\Delta T_b)<\/li>\n\n\n\n
                • Freezing Point: (0\u00b0C – \\Delta T_f)<\/li>\n<\/ul>\n\n\n\n
                    \n
                  1. Al2(SO4)3 (Strong Electrolyte)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                      \n
                    • Dissociates into 5 particles: (2 \\, Al^{3+}) and (3 \\, SO_4^{2-}) (i = 5).<\/li>\n\n\n\n
                    • Boiling Point: (100\u00b0C + \\Delta T_b)<\/li>\n\n\n\n
                    • Freezing Point: (0\u00b0C – \\Delta T_f)<\/li>\n<\/ul>\n\n\n\n

                      Results:<\/h3>\n\n\n\n
                        \n
                      • Boiling Points<\/strong>: The more the solute dissociates, the higher the boiling point, with Al2(SO4)3 raising the boiling point the most.<\/li>\n\n\n\n
                      • Freezing Points<\/strong>: Similarly, the more dissociation, the greater the depression in the freezing point.<\/li>\n<\/ul>\n\n\n\n

                        The provided plot illustrates these changes for each solute, showing that Al2(SO4)3 has the highest boiling point and the greatest freezing point depression, while ethylene glycol, a nonelectrolyte, has the least impact on both.<\/p>\n","protected":false},"excerpt":{"rendered":"

                        Calculate the boiling and freezing points of water solutions that are 1.15 M in the following solutes: a. KBr, a strong electrolyte b. ethylene glycol, a nonelectrolyte c. (NH4)2CO3, a strong electrolyte d. Al2(SO4)3, a strong electrolyte The correct answer and explanation is : The boiling and freezing points of water solutions depend on 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-198156","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198156","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=198156"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198156\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198156"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198156"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198156"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}