{"id":141059,"date":"2022-03-16T13:36:07","date_gmt":"2022-03-16T08:06:07","guid":{"rendered":"https:\/\/infinitylearn.com\/surge\/?p=141059"},"modified":"2024-12-18T17:09:55","modified_gmt":"2024-12-18T11:39:55","slug":"blog-iit-jee-hydration-enthalpy","status":"publish","type":"post","link":"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/","title":{"rendered":"Hydration Enthalpy"},"content":{"rendered":"<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_37 counter-hierarchy ez-toc-counter ez-toc-grey ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title\">Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" style=\"display: none;\"><label for=\"item\" aria-label=\"Table of Content\"><span style=\"display: flex;align-items: center;width: 35px;height: 30px;justify-content: center;\"><svg style=\"fill: #999;color:#999\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #999;color:#999\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/label><input type=\"checkbox\" id=\"item\"><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1' style='display:block'><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Solution_Enthalpy_Change\" title=\"Solution Enthalpy Change\">Solution Enthalpy Change<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Factors_Influencing_Hydration_Enthalpy_Size\" title=\"Factors Influencing Hydration Enthalpy Size\">Factors Influencing Hydration Enthalpy Size<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Why_does_the_groups_hydration_enthalpy_decrease\" title=\"Why does the group&#8217;s hydration enthalpy decrease?\">Why does the group&#8217;s hydration enthalpy decrease?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Factors_Affecting_Hydration_Enthalpy\" title=\"Factors Affecting Hydration Enthalpy\">Factors Affecting Hydration Enthalpy<\/a><ul class='ez-toc-list-level-3'><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Ionic_Radius\" title=\"Ionic Radius\">Ionic Radius<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Ionic_charge\" title=\"Ionic charge\">Ionic charge<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-7\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Hydration_Enthalpy_Application\" title=\"Hydration Enthalpy Application\">Hydration Enthalpy Application<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Importance_of_the_topic_Hydration_Enthalpy_for_JEE_CBSE_Exam\" title=\"Importance of the topic Hydration Enthalpy for JEE  &amp; CBSE Exam\">Importance of the topic Hydration Enthalpy for JEE  &amp; CBSE Exam<\/a><ul class='ez-toc-list-level-4'><li class='ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-9\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#FAQs\" title=\"FAQ\u2019s\">FAQ\u2019s<\/a><ul class='ez-toc-list-level-5'><li class='ez-toc-heading-level-5'><a class=\"ez-toc-link ez-toc-heading-10\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Is_the_enthalpy_of_hydration_positive_or_negative\" title=\"Is the enthalpy of hydration positive or negative?\">Is the enthalpy of hydration positive or negative?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-5'><a class=\"ez-toc-link ez-toc-heading-11\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#What_is_the_link_between_the_enthalpy_of_hydration_and_solubility\" title=\"What is the link between the enthalpy of hydration and solubility?\">What is the link between the enthalpy of hydration and solubility?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-5'><a class=\"ez-toc-link ez-toc-heading-12\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/#Is_Hydration_Absorbing_or_Releasing_Energy\" title=\"Is Hydration Absorbing or Releasing Energy?\">Is Hydration Absorbing or Releasing Energy?<\/a><\/li><\/ul><\/li><\/ul><\/li><\/ul><\/li><\/ul><\/nav><\/div>\n<p><img loading=\"lazy\" class=\"aligncenter wp-image-141063\" src=\"https:\/\/infinitylearn.com\/surge\/wp-content\/uploads\/2022\/03\/download-2-5.png\" alt=\"Hydration Enthalpy\" width=\"893\" height=\"516\" \/><\/p>\n<p><span style=\"font-weight: 400;\">Hydration energy, also known as hydration enthalpy, is the energy generated when one mole of ions undergo hydration, a kind of solvation. It is a type of dissolution of energy in which the solvent is water.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">When we dissolve salt in water, the outermost ions (those at the lattice&#8217;s border) travel away from the lattice and become covered by nearby water molecules. The salt is known to be water-soluble if the hydration energy is equal to or greater than the lattice energy. Solvation happens with a release of energy in the form of heat in salts where the hydration energy is known to be greater than the lattice energy. When CaCl<sub>2<\/sub> (anhydrous calcium chloride) dissolves, it warms the water. The hexahydrate, CaCl<sub>2.<\/sub>6H2O, on the other hand, cools the water upon dissolution. The latter occurs because the hydration energy does not entirely overcome the lattice energy, and the remainder must be extracted from the water to compensate for the energy loss.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">The enthalpy of hydration, H<sub>hyd<\/sub>, is the amount of energy released when a mole of an ion dissolves in a vast volume of water, generating an infinitely dilute solution in the process, Az<sup>+<\/sup>(g) + aH<sub>2<\/sub>O \u2192 Az<sup>+<\/sup>(aq), where Az<sup>+<\/sup>(aq) represents ions surrounded by water molecules and scattered throughout the solution. The estimated hydration energies of several common ions are shown below. According to the table, when the atomic number increases, the ionic size reduces, resulting in a drop in absolute enthalpy of hydration values.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Solution_Enthalpy_Change\"><\/span><span style=\"color: #000000; font-size: 18pt;\">Solution Enthalpy Change<\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400;\">The enthalpy change of solution is defined as the enthalpy change that occurs when one mole of an ionic compound dissolves in water to form an infinitely diluted solution. The solution&#8217;s enthalpies might be either negative or positive. In other words, certain ionic compounds dissolve endothermically (for example, NaCl), whereas others dissolve exothermically (for example, NaOH).<\/span><\/p>\n<p><span style=\"font-weight: 400;\">An endlessly dilute solution is one in which there is such a massive surplus of water that adding more causes no more heat to be absorbed or generated. As a result, when 1 mole of sodium chloride crystals is dissolved in excess water, the enthalpy change of solution is +3.9 kJ mol<sup>-1<\/sup>. The transition is slightly endothermic. As a result, the temperature of the solution will be somewhat lower than the temperature of the original water.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Factors_Influencing_Hydration_Enthalpy_Size\"><\/span><span style=\"color: #0000ff;\"><span style=\"color: #000000;\">Factors Influencing Hydration Enthalpy Size<\/span><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400;\"><span style=\"color: #0000ff;\">Enthalpy<\/span> of hydration: Hydration enthalpy is the amount of energy generated when positive or negative ions form attractions with water molecules. There may be loose ion-dipole interactions between the &#8211; oxygen atoms in the water molecules and the positive ions when there are positive ions, or there may be formal dative covalent (coordinate covalent) connections. Ion-dipole attractions arise between the negative ions and the + hydrogens in water molecules when negative ions are present. The degree of attraction between the ions and the water molecules generally governs the magnitude of the hydration enthalpy. Smaller ions have higher attractions in general. For example, as we move down the Periodic Table, the hydration enthalpies decrease.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Why_does_the_groups_hydration_enthalpy_decrease\"><\/span><span style=\"color: #000000;\">Why does the group&#8217;s hydration enthalpy decrease?<\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400;\">The greater the hydration enthalpy, the smaller the ion since smaller atoms can accommodate many water molecules surrounding them and get hydrated. The hydration enthalpy falls as one moves down the group, but the atom&#8217;s size grows owing to the addition of more valence shells.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">In addition, when cation size grows, the hydration enthalpy falls. On the other hand, lattice enthalpy drops quicker than hydration enthalpy owing to the square factor. As a result, the solubility of Group 2 hydroxides rises as one moves down the group.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Factors_Affecting_Hydration_Enthalpy\"><\/span><span style=\"color: #000000;\">Factors Affecting Hydration Enthalpy<\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400;\">The quantity the ions are attracted to the water molecules affects the typical enthalpy change of hydration (H<sub>hyd<\/sub>).<\/span><\/p>\n<p><span style=\"font-weight: 400;\">The ionic charge and radius are two parameters that influence this attraction.<\/span><\/p>\n<h3><span class=\"ez-toc-section\" id=\"Ionic_Radius\"><\/span><span style=\"color: #0000ff;\">Ionic Radius<\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p><span style=\"font-weight: 400;\">With decreasing ionic radii, ionic radius H<sub>hyd<\/sub> becomes increasingly exothermic.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Smaller ions have a higher charge density, which results in stronger ion-dipole attractions between the water molecules and the ions in the solution.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">As a result, they release more energy as they get hydrated, and H<sub>hyd<\/sub> becomes more exothermic.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">For example, the hydrogen sulphate (H<sub>hyd<\/sub>) of magnesium sulphate (MgSO<sub>4<\/sub>) is more exothermic than the hydrogen sulphate (H<sub>hyd<\/sub>) of barium sulphate (BaSO<sub>4<\/sub>)<\/span><\/p>\n<ul>\n<li><span style=\"font-weight: 400;\">Because both compounds include a sulphate ion, the difference in H<sub>hyd<\/sub> must be attributed to the magnesium ion in MgSO<sub>4<\/sub> and the barium ion in BaSO4.<\/span><\/li>\n<li>Magnesium is a Group 2 element and a Period 3 element. Barium is a Group 2 element and a Period 6 element.<\/li>\n<li>This implies that the Mg<sup>2+<\/sup> ion is less massive than the Ba<sup>2+<\/sup> ion.<\/li>\n<li>As a result, the attraction for the Mg<sup>2+<\/sup> ion is substantially greater.<\/li>\n<li>As a result, MgSO4&#8217;s typical enthalpy of hydration is more exothermic than BaSO4&#8217;s.<\/li>\n<\/ul>\n<h3><span class=\"ez-toc-section\" id=\"Ionic_charge\"><\/span><span style=\"color: #000000;\">Ionic charge<\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<ul>\n<li><span style=\"font-weight: 400;\">For ions with higher ionic charges, H<sub>hyd<\/sub> is more exothermic.<\/span><\/li>\n<li>Ions with significant ionic charges have a higher charge density, resulting in stronger ion-dipole interactions between water molecules and ions in solution.<\/li>\n<li>As a result, they release more energy as they get hydrated, and H<sub>hyd<\/sub> becomes more exothermic.<\/li>\n<li>The H<sub>hyd<\/sub> of calcium oxide (CaO), for example, is more exothermic than the H<sub>hyd<\/sub> of potassium chloride (KCl).<\/li>\n<\/ul>\n<h3><span class=\"ez-toc-section\" id=\"Hydration_Enthalpy_Application\"><\/span><span style=\"color: #000000;\">Hydration Enthalpy Application<\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p><span style=\"font-weight: 400;\">The reaction of cement with water is one use of enthalpy of hydration. Because the process is exothermic, it generates a lot of heat. This heat generated becomes substantial in large-scale projects such as dams and other buildings. Large amounts of cement are utilized in the building of enormous concrete blocks.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">Heat is emitted during the setting process. The exterior surfaces of the block cool comparatively quicker than the interior, creating a thermal gradient in the block and potentially initiating fractures that lead to structural collapse.<\/span><\/p>\n<p><span style=\"font-weight: 400;\">To prevent this difficulty, low heat cement is favoured for large-scale buildings, as is cement containing pozzolanic admixtures such as fly ash or slag, and ice instead of water to produce concrete.<\/span><\/p>\n<h3><span style=\"color: #0000ff;\">Importance of the topic Hydration Enthalpy for JEE  &amp; CBSE Exam<\/span><\/h3>\n<p>Hydration Enthalpy is an important topic for <span style=\"color: #0000ff;\"><a style=\"color: #0000ff;\" href=\"https:\/\/infinitylearn.com\/jee\" target=\"_blank\" rel=\"noopener\">JEE Exam Preparation<\/a><\/span>. Students can score better marks by developing an understanding of this topic.<\/p>\n<h4><span class=\"ez-toc-section\" id=\"FAQs\"><\/span><span style=\"color: #000000; font-size: 14pt;\"><strong>FAQ\u2019s<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n\t\t<section class=\"sc_fs_faq sc_card \">\n\t\t\t<div>\n\t\t\t\t<h5><span class=\"ez-toc-section\" id=\"Is_the_enthalpy_of_hydration_positive_or_negative\"><\/span>Is the enthalpy of hydration positive or negative?<span class=\"ez-toc-section-end\"><\/span><\/h5>\t\t\t\t<div>\n\t\t\t\t\t\t\t\t\t\t<p>\n\t\t\t\t\t\tThe enthalpies of hydration are always negative. Hydration enthalpy is the amount of energy generated when positive or negative ions attach water molecules.\t\t\t\t\t<\/p>\n\t\t\t\t<\/div>\n\t\t\t<\/div>\n\t\t<\/section>\n\t\t\t\t<section class=\"sc_fs_faq sc_card \">\n\t\t\t<div>\n\t\t\t\t<h5><span class=\"ez-toc-section\" id=\"What_is_the_link_between_the_enthalpy_of_hydration_and_solubility\"><\/span>What is the link between the enthalpy of hydration and solubility?<span class=\"ez-toc-section-end\"><\/span><\/h5>\t\t\t\t<div>\n\t\t\t\t\t\t\t\t\t\t<p>\n\t\t\t\t\t\tWhen the hydration enthalpy is large, the chemical is very soluble in water.\t\t\t\t\t<\/p>\n\t\t\t\t<\/div>\n\t\t\t<\/div>\n\t\t<\/section>\n\t\t\t\t<section class=\"sc_fs_faq sc_card \">\n\t\t\t<div>\n\t\t\t\t<h5><span class=\"ez-toc-section\" id=\"Is_Hydration_Absorbing_or_Releasing_Energy\"><\/span>Is Hydration Absorbing or Releasing Energy?<span class=\"ez-toc-section-end\"><\/span><\/h5>\t\t\t\t<div>\n\t\t\t\t\t\t\t\t\t\t<p>\n\t\t\t\t\t\tHydration enthalpy, also known as Hydration energy, is the amount of energy released during the hydration of a single ion-molecule. Drainage capacity is one component of the solution volume analysis. It is a unique water condition.\t\t\t\t\t<\/p>\n\t\t\t\t<\/div>\n\t\t\t<\/div>\n\t\t<\/section>\n\t\t\n<script type=\"application\/ld+json\">\n\t{\n\t\t\"@context\": \"https:\/\/schema.org\",\n\t\t\"@type\": \"FAQPage\",\n\t\t\"mainEntity\": [\n\t\t\t\t\t{\n\t\t\t\t\"@type\": \"Question\",\n\t\t\t\t\"name\": \"Is the enthalpy of hydration positive or negative?\",\n\t\t\t\t\"acceptedAnswer\": {\n\t\t\t\t\t\"@type\": \"Answer\",\n\t\t\t\t\t\"text\": \"The enthalpies of hydration are always negative. Hydration enthalpy is the amount of energy generated when positive or negative ions attach water molecules.\"\n\t\t\t\t\t\t\t\t\t}\n\t\t\t}\n\t\t\t,\t\t\t\t{\n\t\t\t\t\"@type\": \"Question\",\n\t\t\t\t\"name\": \"What is the link between the enthalpy of hydration and solubility?\",\n\t\t\t\t\"acceptedAnswer\": {\n\t\t\t\t\t\"@type\": \"Answer\",\n\t\t\t\t\t\"text\": \"When the hydration enthalpy is large, the chemical is very soluble in water.\"\n\t\t\t\t\t\t\t\t\t}\n\t\t\t}\n\t\t\t,\t\t\t\t{\n\t\t\t\t\"@type\": \"Question\",\n\t\t\t\t\"name\": \"Is Hydration Absorbing or Releasing Energy?\",\n\t\t\t\t\"acceptedAnswer\": {\n\t\t\t\t\t\"@type\": \"Answer\",\n\t\t\t\t\t\"text\": \"Hydration enthalpy, also known as Hydration energy, is the amount of energy released during the hydration of a single ion-molecule. Drainage capacity is one component of the solution volume analysis. It is a unique water condition.\"\n\t\t\t\t\t\t\t\t\t}\n\t\t\t}\n\t\t\t\t\t\t]\n\t}\n<\/script>\n\n","protected":false},"excerpt":{"rendered":"<p>Hydration energy, also known as hydration enthalpy, is the energy generated when one mole of ions undergo hydration, a kind [&hellip;]<\/p>\n","protected":false},"author":7,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_yoast_wpseo_focuskw":"Hydration Enthalpy","_yoast_wpseo_title":"","_yoast_wpseo_metadesc":"Hydration energy, also known as hydration enthalpy, is the amount of energy generated when one mole of ions undergo hydration, which is a kind of salvation.","custom_permalink":"blog\/iit-jee\/hydration-enthalpy\/"},"categories":[53,57],"tags":[],"table_tags":[],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v17.9 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Hydration Enthalpy - Infinity Learn by Sri Chaitanya<\/title>\n<meta name=\"description\" content=\"Hydration energy, also known as hydration enthalpy, is the amount of energy generated when one mole of ions undergo hydration, which is a kind of salvation.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/iit-jee\/hydration-enthalpy\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Hydration Enthalpy - 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