{"id":206927,"date":"2025-04-17T09:34:26","date_gmt":"2025-04-17T09:34:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=206927"},"modified":"2025-04-17T09:34:28","modified_gmt":"2025-04-17T09:34:28","slug":"the-heat-of-solution-with-copper-i-sulfate-is-exothermic","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/17\/the-heat-of-solution-with-copper-i-sulfate-is-exothermic\/","title":{"rendered":"The heat of solution with copper (I) sulfate is exothermic"},"content":{"rendered":"\n

The heat of solution with copper (I) sulfate is exothermic. What will happen to the temperature of the container\/flask when copper (II) sulfate is added to water in the container\/flask? What is the sign of the enthalpy?<\/p>\n\n\n\n

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

When copper (II) sulfate<\/strong> (CuSO\u2084) is added to water, the temperature of the container will increase<\/strong>, indicating that heat is released into the surroundings. This means the process is exothermic<\/strong>, and the sign of the enthalpy change (\u0394H) is negative<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Explanation (Approx. 300 words):<\/h3>\n\n\n\n

When a substance dissolves in water, the process is called dissolution<\/strong>, and the associated heat change is known as the enthalpy of solution<\/strong> (\u0394H_solution). This process involves two main steps:<\/p>\n\n\n\n

    \n
  1. Breaking the lattice structure<\/strong> of the solute (in this case, solid CuSO\u2084), which requires energy (endothermic).<\/li>\n\n\n\n
  2. Hydration of ions<\/strong>, where water molecules surround and stabilize the separated ions, releasing energy (exothermic).<\/li>\n<\/ol>\n\n\n\n

    For copper (II) sulfate<\/strong>, when it dissolves in water, it dissociates into Cu\u00b2\u207a and SO\u2084\u00b2\u207b ions<\/strong>. The hydration of these highly charged ions releases a significant amount of energy\u2014more than what is needed to break apart the ionic crystal structure of solid CuSO\u2084. As a result, the overall dissolution process releases more energy than it consumes<\/strong>, making it exothermic<\/strong>.<\/p>\n\n\n\n

    An exothermic reaction causes a temperature rise<\/strong> in the surroundings. In this case, the water in the container will absorb the heat released from the dissolving CuSO\u2084, resulting in a noticeable increase in water temperature.<\/p>\n\n\n\n

    The sign of enthalpy change (\u0394H)<\/strong> for an exothermic process is negative (\u2013\u0394H)<\/strong> because energy is lost from the system (the dissolving substance) to the surroundings (the water).<\/p>\n\n\n\n

    It is important not to confuse copper (I) sulfate<\/strong> and copper (II) sulfate<\/strong>, though both may have exothermic heats of solution. The key idea remains the same: if the heat of solution is exothermic, the temperature of the solution increases, and \u0394H is negative.<\/p>\n\n\n\n

    \n\n\n\n

    Answer:<\/strong><\/p>\n\n\n\n

      \n
    • Temperature change:<\/strong> Increases<\/li>\n\n\n\n
    • Sign of enthalpy (\u0394H):<\/strong> Negative<\/li>\n<\/ul>\n\n\n\n
      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

      The heat of solution with copper (I) sulfate is exothermic. What will happen to the temperature of the container\/flask when copper (II) sulfate is added to water in the container\/flask? What is the sign of the enthalpy? The correct answer and explanation is : When copper (II) sulfate (CuSO\u2084) is added to water, the temperature […]<\/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-206927","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206927","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=206927"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206927\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206927"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206927"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206927"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}