{"id":42666,"date":"2025-06-29T08:07:40","date_gmt":"2025-06-29T08:07:40","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=42666"},"modified":"2025-06-29T08:07:41","modified_gmt":"2025-06-29T08:07:41","slug":"what-is-the-net-ionic-equation-for-the-reaction-between-lead-nitrate-and-potassium-chloride","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/what-is-the-net-ionic-equation-for-the-reaction-between-lead-nitrate-and-potassium-chloride\/","title":{"rendered":"What is the net ionic equation for the reaction between lead nitrate and potassium chloride"},"content":{"rendered":"\n

What is the net ionic equation for the reaction between lead nitrate and potassium chloride<\/p>\n\n\n\n

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

To write the net ionic equation for the reaction between lead(II) nitrate and potassium chloride, we first need to understand the reaction itself and the relevant steps involved.<\/p>\n\n\n\n

Step 1: Write the balanced molecular equation<\/h3>\n\n\n\n

The reactants are lead(II) nitrate (Pb(NO\u2083)\u2082) and potassium chloride (KCl). These two compounds react in an aqueous solution, and when mixed, they undergo a double displacement reaction.<\/p>\n\n\n\n

The molecular equation for the reaction is:Pb(NO3)2(aq)+2KCl(aq)\u2192PbCl2(s)+2KNO3(aq)\\text{Pb(NO}_3\\text{)}_2(aq) + 2\\text{KCl}(aq) \\rightarrow \\text{PbCl}_2(s) + 2\\text{KNO}_3(aq)Pb(NO3\u200b)2\u200b(aq)+2KCl(aq)\u2192PbCl2\u200b(s)+2KNO3\u200b(aq)<\/p>\n\n\n\n

In this reaction, lead(II) chloride (PbCl\u2082) is formed as a solid precipitate, while potassium nitrate (KNO\u2083) remains dissolved in the aqueous solution.<\/p>\n\n\n\n

Step 2: Write the full ionic equation<\/h3>\n\n\n\n

When compounds are dissolved in water, they dissociate into their respective ions. So, we need to break up the soluble ionic compounds into ions.Pb2+(aq)+2NO3\u2212(aq)+2K+(aq)+2Cl\u2212(aq)\u2192PbCl2(s)+2K+(aq)+2NO3\u2212(aq)\\text{Pb}^{2+}(aq) + 2\\text{NO}_3^-(aq) + 2\\text{K}^+(aq) + 2\\text{Cl}^-(aq) \\rightarrow \\text{PbCl}_2(s) + 2\\text{K}^+(aq) + 2\\text{NO}_3^-(aq)Pb2+(aq)+2NO3\u2212\u200b(aq)+2K+(aq)+2Cl\u2212(aq)\u2192PbCl2\u200b(s)+2K+(aq)+2NO3\u2212\u200b(aq)<\/p>\n\n\n\n

Step 3: Identify the spectator ions<\/h3>\n\n\n\n

Spectator ions are ions that do not participate in the reaction and remain unchanged on both sides of the equation. In this case, the potassium ions (K+\\text{K}^+K+) and nitrate ions (NO3\u2212\\text{NO}_3^-NO3\u2212\u200b) are spectator ions.<\/p>\n\n\n\n

Step 4: Write the net ionic equation<\/h3>\n\n\n\n

After canceling the spectator ions, we are left with the following net ionic equation:Pb2+(aq)+2Cl\u2212(aq)\u2192PbCl2(s)\\text{Pb}^{2+}(aq) + 2\\text{Cl}^-(aq) \\rightarrow \\text{PbCl}_2(s)Pb2+(aq)+2Cl\u2212(aq)\u2192PbCl2\u200b(s)<\/p>\n\n\n\n

This equation shows that lead(II) ions (Pb2+\\text{Pb}^{2+}Pb2+) and chloride ions (Cl\u2212\\text{Cl}^-Cl\u2212) combine to form solid lead(II) chloride (PbCl\u2082), which precipitates out of the solution.<\/p>\n\n\n\n

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

The net ionic equation represents only the ions involved in the formation of the precipitate. In this case, the lead(II) ion and chloride ion come together to form PbCl\u2082 as a solid, with the other ions (K\u207a and NO\u2083\u207b) remaining in solution as spectator ions.<\/p>\n\n\n\n

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

What is the net ionic equation for the reaction between lead nitrate and potassium chloride The Correct Answer and Explanation is: To write the net ionic equation for the reaction between lead(II) nitrate and potassium chloride, we first need to understand the reaction itself and the relevant steps involved. Step 1: Write the balanced molecular […]<\/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-42666","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/42666","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=42666"}],"version-history":[{"count":2,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/42666\/revisions"}],"predecessor-version":[{"id":42669,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/42666\/revisions\/42669"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=42666"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=42666"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=42666"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}