{"id":221414,"date":"2025-05-29T13:25:04","date_gmt":"2025-05-29T13:25:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221414"},"modified":"2025-05-29T13:25:12","modified_gmt":"2025-05-29T13:25:12","slug":"use-the-solubility-interactive-to-complete-the-solubility-table","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/use-the-solubility-interactive-to-complete-the-solubility-table\/","title":{"rendered":"Use the solubility interactive to complete the solubility table."},"content":{"rendered":"\n

Use the solubility interactive to complete the solubility table. co; SO? – s2 Pb2+ Ni2+ Ba? + Answer Bank soluble insoluble For the chemical reaction Na,Co, + Ca(NO3)2 +CaCO3 +2 NaNO, how many moles of calcium carbonate (CaCO3) are produced from 8.0 mol of sodium carbonat<\/p>\n\n\n\n

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

Answer:<\/strong><\/p>\n\n\n\n

For the reaction:<\/p>\n\n\n\n

Na\u2082CO\u2083 + Ca(NO\u2083)\u2082 \u2192 CaCO\u2083 + 2 NaNO\u2083<\/strong><\/p>\n\n\n\n

From the balanced chemical equation, 1 mole of sodium carbonate (Na\u2082CO\u2083)<\/strong> reacts with 1 mole of calcium nitrate (Ca(NO\u2083)\u2082)<\/strong> to produce 1 mole of calcium carbonate (CaCO\u2083)<\/strong>.<\/p>\n\n\n\n

So, 8.0 moles of Na\u2082CO\u2083<\/strong> will produce 8.0 moles of CaCO\u2083<\/strong>, provided there is at least 8.0 moles of Ca(NO\u2083)\u2082 available.<\/p>\n\n\n\n

\n

\u2705 Answer: 8.0 moles of CaCO\u2083 are produced.<\/strong><\/p>\n<\/blockquote>\n\n\n\n

\n\n\n\n

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

This problem involves a double displacement reaction<\/strong> between sodium carbonate (Na\u2082CO\u2083)<\/strong> and calcium nitrate (Ca(NO\u2083)\u2082)<\/strong>. The balanced chemical reaction is:<\/p>\n\n\n\n

Na\u2082CO\u2083 + Ca(NO\u2083)\u2082 \u2192 CaCO\u2083 \u2193 + 2 NaNO\u2083<\/strong><\/p>\n\n\n\n

This equation shows a 1:1 molar ratio<\/strong> between sodium carbonate and calcium carbonate. That means for every 1 mole of Na\u2082CO\u2083 that reacts, 1 mole of CaCO\u2083 is produced, assuming calcium nitrate is present in excess or in an equimolar amount.<\/p>\n\n\n\n

In this case, if we are given 8.0 moles of sodium carbonate and no limiting information about calcium nitrate, we assume it is in sufficient quantity<\/strong>. Therefore, using the molar ratio:<\/p>\n\n\n\n

    \n
  • 1 mol Na\u2082CO\u2083 : 1 mol CaCO\u2083<\/li>\n\n\n\n
  • 8.0 mol Na\u2082CO\u2083 : 8.0 mol CaCO\u2083<\/li>\n<\/ul>\n\n\n\n

    This reaction is also used in qualitative analysis to test for calcium ions. Calcium carbonate is insoluble in water<\/strong>, and it precipitates out<\/strong> as a solid. That\u2019s why it appears as a white precipitate<\/strong> in lab settings.<\/p>\n\n\n\n

    Solubility rules tell us:<\/p>\n\n\n\n

      \n
    • Most carbonate salts (CO\u2083\u00b2\u207b) are insoluble<\/strong>, except those with Group 1 cations (e.g., Na\u207a, K\u207a)<\/strong> and ammonium (NH\u2084\u207a)<\/strong>.<\/li>\n\n\n\n
    • Calcium carbonate (CaCO\u2083)<\/strong> is insoluble<\/strong>, so it forms a precipitate.<\/li>\n\n\n\n
    • Sodium nitrate (NaNO\u2083)<\/strong> is soluble<\/strong> and remains dissolved in the solution.<\/li>\n<\/ul>\n\n\n\n

      This simple stoichiometry calculation highlights key chemical concepts: molar ratios<\/strong>, limiting reactants<\/strong>, and solubility rules<\/strong>, which are fundamental in predicting the outcomes of chemical reactions.<\/p>\n\n\n\n

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

      Use the solubility interactive to complete the solubility table. co; SO? – s2 Pb2+ Ni2+ Ba? + Answer Bank soluble insoluble For the chemical reaction Na,Co, + Ca(NO3)2 +CaCO3 +2 NaNO, how many moles of calcium carbonate (CaCO3) are produced from 8.0 mol of sodium carbonat The Correct Answer and Explanation is: Answer: For 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-221414","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221414","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=221414"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221414\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221414"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221414"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221414"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}