{"id":220095,"date":"2025-05-27T13:32:07","date_gmt":"2025-05-27T13:32:07","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=220095"},"modified":"2025-05-27T13:32:09","modified_gmt":"2025-05-27T13:32:09","slug":"mgclo42-dissolved-in-water-acidic-basic-or-neutral","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/27\/mgclo42-dissolved-in-water-acidic-basic-or-neutral\/","title":{"rendered":"Mg(CLO4)2 dissolved in water acidic, basic, or neutral"},"content":{"rendered":"\n

Mg(CLO4)2 dissolved in water acidic, basic, or neutral? and why?<\/p>\n\n\n\n

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

When magnesium perchlorate (Mg(ClO\u2084)\u2082)<\/strong> dissolves in water, the resulting solution is slightly acidic<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Explanation <\/strong><\/h3>\n\n\n\n

Magnesium perchlorate (Mg(ClO\u2084)\u2082) is a salt formed from the reaction of magnesium hydroxide (Mg(OH)\u2082)<\/strong>, a weak base<\/strong>, and perchloric acid (HClO\u2084)<\/strong>, a strong acid<\/strong>. To determine the nature of its aqueous solution\u2014acidic, basic, or neutral\u2014we analyze the behavior of its constituent ions when dissolved in water.<\/p>\n\n\n\n

Upon dissolution, Mg(ClO\u2084)\u2082 dissociates into its ions: Mg(ClO\u2084)\u2082 (s)\u2192Mg2+(aq)+2ClO\u2084\u2212(aq)\\text{Mg(ClO\u2084)\u2082 (s)} \\rightarrow \\text{Mg}^{2+} (aq) + 2 \\text{ClO\u2084}^- (aq)<\/p>\n\n\n\n

    \n
  • ClO\u2084\u207b (perchlorate ion)<\/strong>: This is the conjugate base of a strong acid (HClO\u2084), so it is extremely weak<\/strong> and does not hydrolyze<\/strong> in water. It has no significant effect on the pH.<\/li>\n\n\n\n
  • Mg\u00b2\u207a (magnesium ion)<\/strong>: This is a small, highly charged cation (a 2+ charge<\/strong>) and can undergo hydrolysis<\/strong>. It interacts with water molecules to form a hydrated ion like [Mg(H\u2082O)\u2086]\u00b2\u207a. The positive charge on Mg\u00b2\u207a polarizes the water molecules in its hydration shell, making them more likely to donate protons (H\u207a). This results in the release of hydrogen ions (H\u207a), causing a slight acidification<\/strong> of the solution:<\/li>\n<\/ul>\n\n\n\n

    [Mg(H\u2082O)\u2086]2+\u21cc[Mg(H\u2082O)\u2085OH]++H+\\text{[Mg(H\u2082O)\u2086]}^{2+} \\rightleftharpoons \\text{[Mg(H\u2082O)\u2085OH]}^{+} + \\text{H}^{+}<\/p>\n\n\n\n

    Thus, the presence of Mg\u00b2\u207a contributes to a slight increase in hydrogen ion concentration, lowering the pH and making the solution slightly acidic<\/strong>.<\/p>\n\n\n\n

    In summary, Mg(ClO\u2084)\u2082 yields a slightly acidic solution because the magnesium ion hydrolyzes<\/strong>, while the perchlorate ion remains inert<\/strong>. The overall result is a solution with a pH just below 7, typically around 5.5\u20136.5<\/strong>, depending on concentration.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    Mg(CLO4)2 dissolved in water acidic, basic, or neutral? and why? The Correct Answer and Explanation is: When magnesium perchlorate (Mg(ClO\u2084)\u2082) dissolves in water, the resulting solution is slightly acidic. Explanation Magnesium perchlorate (Mg(ClO\u2084)\u2082) is a salt formed from the reaction of magnesium hydroxide (Mg(OH)\u2082), a weak base, and perchloric acid (HClO\u2084), a strong acid. To […]<\/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-220095","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220095","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=220095"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220095\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=220095"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=220095"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=220095"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}