{"id":182700,"date":"2025-01-14T17:40:50","date_gmt":"2025-01-14T17:40:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182700"},"modified":"2025-01-14T17:40:58","modified_gmt":"2025-01-14T17:40:58","slug":"solid-potassium-permanganate-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/14\/solid-potassium-permanganate-2\/","title":{"rendered":"Solid, potassium permanganate"},"content":{"rendered":"\n

Solid, potassium permanganate, KMnO4, is much more soluble in water than in CH2Cl2 (a non-polar solvent). Which of the following intermolecular forces is primarily responsible for the greater solubility of KMnO4 in water than in CH2Cl2? O dipole-dipole forces London dispersion forces hydrogen bonding ion-dipole forces ionic bonding<\/p>\n\n\n\n

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

The correct answer is ion-dipole forces<\/strong>.<\/p>\n\n\n\n

Explanation:<\/strong>
Potassium permanganate (KMnO\u2084) is an ionic compound, consisting of potassium ions (K\u207a) and permanganate ions (MnO\u2084\u207b). The solubility of ionic compounds like KMnO\u2084 in solvents depends on the interactions between the ions in the compound and the solvent molecules.<\/p>\n\n\n\n

    \n
  1. Water as a solvent<\/strong>: Water is a highly polar solvent, with a strong ability to form hydrogen bonds due to the electronegativity of oxygen. When KMnO\u2084 is added to water, the polar water molecules surround the K\u207a and MnO\u2084\u207b ions, forming ion-dipole interactions. The positively charged potassium ion is attracted to the partial negative charge of the oxygen in water molecules, and the negatively charged permanganate ion is attracted to the partial positive charge of the hydrogen atoms in water. These ion-dipole forces are strong and effectively break the ionic bonds in KMnO\u2084, allowing the compound to dissolve.<\/li>\n\n\n\n
  2. CH\u2082Cl\u2082 (dichloromethane) as a solvent<\/strong>: CH\u2082Cl\u2082 is a non-polar solvent, which has weaker intermolecular forces compared to water. It primarily experiences London dispersion forces, which are much weaker than ion-dipole forces. Non-polar solvents cannot effectively interact with the K\u207a and MnO\u2084\u207b ions in KMnO\u2084, meaning that KMnO\u2084 will not dissolve well in CH\u2082Cl\u2082.<\/li>\n<\/ol>\n\n\n\n

    Conclusion<\/strong>: The greater solubility of KMnO\u2084 in water compared to CH\u2082Cl\u2082 is due to the strong ion-dipole interactions between the ions of KMnO\u2084 and the polar water molecules. These interactions are significantly stronger than the London dispersion forces that would operate in CH\u2082Cl\u2082, leading to a greater solubility in water.<\/p>\n","protected":false},"excerpt":{"rendered":"

    Solid, potassium permanganate, KMnO4, is much more soluble in water than in CH2Cl2 (a non-polar solvent). Which of the following intermolecular forces is primarily responsible for the greater solubility of KMnO4 in water than in CH2Cl2? O dipole-dipole forces London dispersion forces hydrogen bonding ion-dipole forces ionic bonding The Correct Answer and Explanation is : […]<\/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-182700","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182700","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=182700"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182700\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182700"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182700"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182700"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}