{"id":199798,"date":"2025-03-12T15:54:57","date_gmt":"2025-03-12T15:54:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199798"},"modified":"2025-03-12T15:54:59","modified_gmt":"2025-03-12T15:54:59","slug":"magnesium-carbonate-magnesium-oxide-and-magnesium-hydroxide-are-all-white-solids-that-react-with-acidic-solutions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/12\/magnesium-carbonate-magnesium-oxide-and-magnesium-hydroxide-are-all-white-solids-that-react-with-acidic-solutions\/","title":{"rendered":"Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions"},"content":{"rendered":"\n

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. <\/p>\n\n\n\n

(a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. <\/p>\n\n\n\n

(b) By observing the reactions in part (a) could you distinguish any of the three magnesium substances from the other two? If so how? <\/p>\n\n\n\n

(c) If excess HCl(aq) is added, would the clear solutions left behind after the reaction is complete contain the same or different ions in each case?<\/p>\n\n\n\n

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

(a) Balanced Molecular and Net Ionic Equations<\/h3>\n\n\n\n
    \n
  1. Magnesium carbonate (MgCO\u2083) with HCl:<\/strong>
    Molecular Equation:<\/strong>
    [
    MgCO\u2083 (s) + 2HCl (aq) \\rightarrow MgCl\u2082 (aq) + CO\u2082 (g) + H\u2082O (l)
    ]
    Net Ionic Equation:<\/strong>
    [
    CO\u2083^{2-} (s) + 2H\u207a (aq) \\rightarrow CO\u2082 (g) + H\u2082O (l)
    ]<\/li>\n\n\n\n
  2. Magnesium oxide (MgO) with HCl:<\/strong>
    Molecular Equation:<\/strong>
    [
    MgO (s) + 2HCl (aq) \\rightarrow MgCl\u2082 (aq) + H\u2082O (l)
    ]
    Net Ionic Equation:<\/strong>
    [
    O^{2-} (s) + 2H\u207a (aq) \\rightarrow H\u2082O (l)
    ]<\/li>\n\n\n\n
  3. Magnesium hydroxide (Mg(OH)\u2082) with HCl:<\/strong>
    Molecular Equation:<\/strong>
    [
    Mg(OH)\u2082 (s) + 2HCl (aq) \\rightarrow MgCl\u2082 (aq) + 2H\u2082O (l)
    ]
    Net Ionic Equation:<\/strong>
    [
    OH\u207b (s) + H\u207a (aq) \\rightarrow H\u2082O (l)
    ]<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    (b) Distinguishing the Three Magnesium Compounds<\/h3>\n\n\n\n

    Yes, these substances can be distinguished based on their reaction observations:<\/p>\n\n\n\n

      \n
    • Magnesium carbonate (MgCO\u2083):<\/strong> Produces bubbles of CO\u2082 gas (effervescence) when reacting with HCl, which is a visible indicator.<\/li>\n\n\n\n
    • Magnesium oxide (MgO):<\/strong> Reacts with HCl but does not produce gas, just dissolves while forming a clear solution.<\/li>\n\n\n\n
    • Magnesium hydroxide (Mg(OH)\u2082):<\/strong> Reacts similarly to MgO but dissolves more slowly since it is only sparingly soluble in water. No gas formation occurs.<\/li>\n<\/ul>\n\n\n\n

      Thus, MgCO\u2083 can be distinguished from the other two<\/strong> due to gas evolution<\/strong>. MgO and Mg(OH)\u2082 could be harder to differentiate without additional tests, though Mg(OH)\u2082 may be distinguished by its slower dissolution in acid.<\/p>\n\n\n\n

      \n\n\n\n

      (c) Ionic Composition of Final Solution<\/h3>\n\n\n\n

      After the reaction, the solution will contain the same ions<\/strong> in all cases. The excess HCl will react with all solid reactants<\/strong>, forming magnesium chloride (MgCl\u2082) and water<\/strong> in each case. Since MgCl\u2082 is a soluble salt, the final solution will contain Mg\u00b2\u207a and Cl\u207b ions<\/strong> regardless of which solid was initially used. Therefore, the solution will be identical in ionic composition across all three cases.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a) could you distinguish any of the […]<\/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-199798","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199798","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=199798"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199798\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199798"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199798"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199798"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}