{"id":253114,"date":"2025-07-11T21:43:29","date_gmt":"2025-07-11T21:43:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=253114"},"modified":"2025-07-11T21:43:32","modified_gmt":"2025-07-11T21:43:32","slug":"write-a-balanced-net-ionic-equation-for-the-reaction-of-aqueous-solutions-of-hydrochloric-acid-hcl-and-sodium-carbonate-na2co3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/11\/write-a-balanced-net-ionic-equation-for-the-reaction-of-aqueous-solutions-of-hydrochloric-acid-hcl-and-sodium-carbonate-na2co3\/","title":{"rendered":"Write a balanced, net-ionic equation for the reaction of aqueous solutions of hydrochloric acid (HCl) and sodium carbonate (Na2CO3)."},"content":{"rendered":"\n

Write a balanced, net-ionic equation for the reaction of aqueous solutions of hydrochloric acid (HCl) and sodium carbonate (Na2CO3). a. 2 HCl(aq) + Na2CO3(aq) \u2192 H2CO3(aq) + 2 NaCl(aq) b. 2 H+(aq) + CO32-(aq) \u2192 H2CO3(aq) c. H+(aq) + NaCO3-(aq) \u2192 NaHCO3(s) d. 2 H+(aq) + CO32-(aq) \u2192 H2O + CO2(g) e. Cl-(aq) + Na+(aq) \u2192 NaCl(aq)<\/p>\n\n\n\n

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

To determine the correct net ionic equation for the reaction of aqueous solutions of hydrochloric acid (HCl) and sodium carbonate (Na2CO3), we need to consider the chemical interactions between the ions in solution.<\/p>\n\n\n\n

Step-by-step analysis:<\/h3>\n\n\n\n
    \n
  1. Write the full ionic equation<\/strong>:
    • When HCl dissociates in water, it breaks into H\u207a (aq) and Cl\u207b (aq).<\/li>
    • Sodium carbonate (Na\u2082CO\u2083) dissociates into 2 Na\u207a (aq) and CO\u2083\u00b2\u207b (aq).<\/li>
    • The reaction between H\u207a and CO\u2083\u00b2\u207b (carbonate ion) forms carbonic acid (H\u2082CO\u2083), which is unstable and rapidly decomposes into water (H\u2082O) and carbon dioxide (CO\u2082) gas.<\/li><\/ul>So, the full ionic equation<\/strong> would be: 2H+(aq)+CO32\u2212(aq)\u2192H2CO3(aq)2 H^+(aq) + CO_3^{2-}(aq) \\rightarrow H_2CO_3(aq)2H+(aq)+CO32\u2212\u200b(aq)\u2192H2\u200bCO3\u200b(aq) Carbonic acid (H\u2082CO\u2083) decomposes to form water and carbon dioxide: H2CO3(aq)\u2192H2O(l)+CO2(g)H_2CO_3(aq) \\rightarrow H_2O(l) + CO_2(g)H2\u200bCO3\u200b(aq)\u2192H2\u200bO(l)+CO2\u200b(g)<\/li>\n\n\n\n
    • Write the net ionic equation<\/strong>:
      The full ionic equation includes spectator ions like Na\u207a and Cl\u207b, which do not participate in the reaction. We remove them to get the net ionic equation. The final net ionic equation<\/strong> becomes: 2H+(aq)+CO32\u2212(aq)\u2192H2O(l)+CO2(g)2 H^+(aq) + CO_3^{2-}(aq) \\rightarrow H_2O(l) + CO_2(g)2H+(aq)+CO32\u2212\u200b(aq)\u2192H2\u200bO(l)+CO2\u200b(g) This shows that the hydrogen ions from hydrochloric acid react with the carbonate ions from sodium carbonate to form water and carbon dioxide gas.<\/li>\n<\/ol>\n\n\n\n

      Option analysis:<\/h3>\n\n\n\n
        \n
      • Option a (2 HCl(aq) + Na\u2082CO\u2083(aq) \u2192 H\u2082CO\u2083(aq) + 2 NaCl(aq))<\/strong>: This is the molecular equation but does not show the actual ionization and reaction of the acid with the carbonate.<\/li>\n\n\n\n
      • Option b (2 H\u207a(aq) + CO\u2083\u00b2\u207b(aq) \u2192 H\u2082CO\u2083(aq))<\/strong>: This is part of the reaction but neglects the decomposition of carbonic acid into water and carbon dioxide.<\/li>\n\n\n\n
      • Option c (H\u207a(aq) + NaCO\u2083\u207b(aq) \u2192 NaHCO\u2083(s))<\/strong>: This does not represent the carbonate ion properly and incorrectly implies the formation of sodium bicarbonate (NaHCO\u2083) instead of CO\u2082.<\/li>\n\n\n\n
      • Option d (2 H\u207a(aq) + CO\u2083\u00b2\u207b(aq) \u2192 H\u2082O + CO\u2082(g))<\/strong>: This is the correct net ionic equation, as it properly shows the complete reaction where carbonic acid decomposes.<\/li>\n\n\n\n
      • Option e (Cl\u207b(aq) + Na\u207a(aq) \u2192 NaCl(aq))<\/strong>: This shows the spectator ions, which do not participate in the reaction and are thus not part of the net ionic equation.<\/li>\n<\/ul>\n\n\n\n

        Conclusion:<\/h3>\n\n\n\n

        The correct answer is Option d<\/strong>: 2H+(aq)+CO32\u2212(aq)\u2192H2O(l)+CO2(g)2 H^+(aq) + CO_3^{2-}(aq) \\rightarrow H_2O(l) + CO_2(g)2H+(aq)+CO32\u2212\u200b(aq)\u2192H2\u200bO(l)+CO2\u200b(g)<\/p>\n\n\n\n

        This equation reflects the neutralization of carbonate ions with hydrogen ions to produce water and carbon dioxide.<\/p>\n\n\n\n

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

        Write a balanced, net-ionic equation for the reaction of aqueous solutions of hydrochloric acid (HCl) and sodium carbonate (Na2CO3). a. 2 HCl(aq) + Na2CO3(aq) \u2192 H2CO3(aq) + 2 NaCl(aq) b. 2 H+(aq) + CO32-(aq) \u2192 H2CO3(aq) c. H+(aq) + NaCO3-(aq) \u2192 NaHCO3(s) d. 2 H+(aq) + CO32-(aq) \u2192 H2O + CO2(g) e. Cl-(aq) + Na+(aq) […]<\/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-253114","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253114","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=253114"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253114\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=253114"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=253114"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=253114"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}