{"id":28756,"date":"2025-06-20T15:10:11","date_gmt":"2025-06-20T15:10:11","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=28756"},"modified":"2025-06-20T15:10:12","modified_gmt":"2025-06-20T15:10:12","slug":"a-balanced-net-ionic-equation-for-the-reaction-of-agno3aq-with-kclaq","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/a-balanced-net-ionic-equation-for-the-reaction-of-agno3aq-with-kclaq\/","title":{"rendered":"A balanced net ionic equation for the reaction of AgNO3(aq) with KCl(aq)."},"content":{"rendered":"\n<p>A balanced net ionic equation for the reaction of AgNO3(aq) with KCl(aq). a. AgNO3(aq) + KCl(aq) \u00e2\u2020\u2019 AgCl(aq) + KNO3(aq) b. Ag+(aq) + Cl-(aq) \u00e2\u2020\u2019 AgCl(s) c. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) \u00e2\u2020\u2019 AgCl(s) + K+(aq) + NO3-(aq) d. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) \u00e2\u2020\u2019 Ag+(aq) + Cl-(aq) + KNO3(aq) e. K+(aq) + Cl-(aq) \u00e2\u2020\u2019 KCl(s)<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct balanced net ionic equation for the reaction of <strong>AgNO\u2083(aq)<\/strong> with <strong>KCl(aq)<\/strong> is:<\/p>\n\n\n\n<p><strong>b. Ag\u207a(aq) + Cl\u207b(aq) \u2192 AgCl(s)<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>When silver nitrate (AgNO\u2083) and potassium chloride (KCl) are mixed in aqueous solution, they undergo a <strong>double replacement reaction<\/strong>, which is a type of <strong>precipitation reaction<\/strong>. In solution, both compounds dissociate into their respective ions:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>AgNO\u2083 dissociates into Ag\u207a and NO\u2083\u207b<\/li>\n\n\n\n<li>KCl dissociates into K\u207a and Cl\u207b<\/li>\n<\/ul>\n\n\n\n<p>So, the full ionic equation is:<\/p>\n\n\n\n<p><strong>Ag\u207a(aq) + NO\u2083\u207b(aq) + K\u207a(aq) + Cl\u207b(aq) \u2192 AgCl(s) + K\u207a(aq) + NO\u2083\u207b(aq)<\/strong><\/p>\n\n\n\n<p>In this equation, we can see that <strong>K\u207a<\/strong> and <strong>NO\u2083\u207b<\/strong> ions appear on both sides of the equation without changing. These are called <strong>spectator ions<\/strong> because they do not participate directly in the chemical reaction. To focus on the actual chemical change occurring, we eliminate the spectator ions, which gives us the <strong>net ionic equation<\/strong>:<\/p>\n\n\n\n<p><strong>Ag\u207a(aq) + Cl\u207b(aq) \u2192 AgCl(s)<\/strong><\/p>\n\n\n\n<p>This shows that <strong>silver ions (Ag\u207a)<\/strong> and <strong>chloride ions (Cl\u207b)<\/strong> combine to form <strong>solid silver chloride (AgCl)<\/strong>, which precipitates out of the solution. The formation of a <strong>solid product<\/strong> (precipitate) is evidence of a chemical reaction taking place in solution.<\/p>\n\n\n\n<p>Other choices are incorrect for the following reasons:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>a<\/strong> shows the molecular form, not the net ionic equation.<\/li>\n\n\n\n<li><strong>c<\/strong> includes spectator ions and is not a net ionic equation.<\/li>\n\n\n\n<li><strong>d<\/strong> incorrectly suggests no reaction, as it shows ions on both sides unchanged.<\/li>\n\n\n\n<li><strong>e<\/strong> is a reaction that does not occur under normal aqueous conditions, as KCl is highly soluble and does not form a solid.<\/li>\n<\/ul>\n\n\n\n<p>Thus, <strong>option b<\/strong> is the correct net ionic equation.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-248.jpeg\" alt=\"\" class=\"wp-image-28759\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-248.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-248-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-248-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>A balanced net ionic equation for the reaction of AgNO3(aq) with KCl(aq). a. AgNO3(aq) + KCl(aq) \u00e2\u2020\u2019 AgCl(aq) + KNO3(aq) b. Ag+(aq) + Cl-(aq) \u00e2\u2020\u2019 AgCl(s) c. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) \u00e2\u2020\u2019 AgCl(s) + K+(aq) + NO3-(aq) d. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) \u00e2\u2020\u2019 Ag+(aq) + Cl-(aq) + KNO3(aq) e. [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-28756","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28756","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=28756"}],"version-history":[{"count":2,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28756\/revisions"}],"predecessor-version":[{"id":28762,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28756\/revisions\/28762"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=28756"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=28756"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=28756"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}