{"id":179917,"date":"2025-01-03T00:38:06","date_gmt":"2025-01-03T00:38:06","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=179917"},"modified":"2025-01-03T00:38:09","modified_gmt":"2025-01-03T00:38:09","slug":"solvent-for-each-solute","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/03\/solvent-for-each-solute\/","title":{"rendered":"solvent For each solute"},"content":{"rendered":"\n

solvent<\/p>\n\n\n\n

For each solute, identify the better solvent: water or carbon\u00c3\u201a\u00c2 tetrachloride.<\/p>\n\n\n\n

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

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

When deciding whether water or carbon tetrachloride (CCl4CCl_4) is a better solvent for a given solute, the key factors are the polarity of the solute and the principle of “like dissolves like.” Below is the detailed explanation for each solvent:<\/p>\n\n\n\n

\n\n\n\n

Water<\/strong><\/h3>\n\n\n\n

Water is a highly polar solvent due to its significant dipole moment and hydrogen-bonding capability. It is particularly effective at dissolving:<\/p>\n\n\n\n

    \n
  • Ionic compounds<\/strong>: These dissociate into ions, which interact strongly with the partial charges in water molecules.<\/li>\n\n\n\n
  • Polar covalent molecules<\/strong>: Compounds with permanent dipoles (e.g., alcohols, sugars, and acids) readily form hydrogen bonds or dipole-dipole interactions with water.<\/li>\n<\/ul>\n\n\n\n

    Examples of solutes better dissolved in water<\/strong>:<\/p>\n\n\n\n

      \n
    1. Sodium chloride (NaCl)<\/strong>: An ionic compound that dissociates into Na+Na^+ and Cl\u2212Cl^-, which are stabilized by water molecules.<\/li>\n\n\n\n
    2. Ethanol (C2H5OHC_2H_5OH)<\/strong>: Its hydroxyl group interacts with water through hydrogen bonding.<\/li>\n\n\n\n
    3. Glucose (C6H12O6C_6H_{12}O_6)<\/strong>: Highly polar and forms hydrogen bonds with water.<\/li>\n<\/ol>\n\n\n\n
      \n\n\n\n

      Carbon Tetrachloride (CCl4CCl_4)<\/strong><\/h3>\n\n\n\n

      Carbon tetrachloride is a nonpolar solvent due to its symmetric tetrahedral structure and the absence of a net dipole moment. It is effective for dissolving:<\/p>\n\n\n\n

        \n
      • Nonpolar molecules<\/strong>: These include hydrocarbons and other substances without significant polarity or hydrogen-bonding capability.<\/li>\n\n\n\n
      • Lipophilic compounds<\/strong>: Compounds that are soluble in nonpolar environments.<\/li>\n<\/ul>\n\n\n\n

        Examples of solutes better dissolved in CCl4CCl_4<\/strong>:<\/p>\n\n\n\n

          \n
        1. Iodine (I2I_2)<\/strong>: A nonpolar molecule that dissolves well in CCl4CCl_4 through London dispersion forces.<\/li>\n\n\n\n
        2. Hexane (C6H14C_6H_{14})<\/strong>: A hydrocarbon that is miscible with CCl4CCl_4 due to similar nonpolar characteristics.<\/li>\n\n\n\n
        3. Chloroform (CHCl3CHCl_3)<\/strong>: While slightly polar, it is more soluble in CCl4CCl_4 due to weak intermolecular interactions.<\/li>\n<\/ol>\n\n\n\n
          \n\n\n\n

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

          Water is better for ionic and polar compounds due to its high polarity and hydrogen-bonding ability, whereas CCl4CCl_4 excels at dissolving nonpolar substances due to its symmetry and lack of polarity.<\/p>\n","protected":false},"excerpt":{"rendered":"

          solvent For each solute, identify the better solvent: water or carbon\u00c3\u201a\u00c2 tetrachloride. The correct answer and explanation is: When deciding whether water or carbon tetrachloride (CCl4CCl_4) is a better solvent for a given solute, the key factors are the polarity of the solute and the principle of “like dissolves like.” Below is the detailed explanation for […]<\/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-179917","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/179917","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=179917"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/179917\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=179917"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=179917"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=179917"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}