Answer:
Two, KCl and PbCl₂.
Explanation:
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In this case, since the addition of chloride ions promote the following three ionic reactions:
[tex]Ag^+(aq)+Cl^-(aq)\rightleftharpoons AgCl(s)\\\\K^+(aq)+Cl^-(aq)\rightleftharpoons KCl(aq)\\\\Pb^{2+}(aq)+Cl^-(aq)\rightleftharpoons PbCl_2(s)[/tex]
We can infer that both silver chloride and lead (II) chloride are precipitated products as their Ksp are 6.56x10⁻⁴ and 1.59x10⁻⁵ respectively, which means they are merely soluble in water.
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Silver chloride (AgCl), Potassium chloride (KCl) and Lead chloride (Pb2Cl) are produced when added the solution of chlorine.
If a chloride solution is added in the container which contains aqueous mixture that comprise of Ag+ , K+ , and Pb2+ cations, three different solid precipitate will be formed. Silver chloride (AgCl), Potassium chloride (KCl) and Lead chloride (Pb2Cl) are the three solid precipitate that will formed when the chlorine in added to the solution.
The chlorine is an anion which reacts with all three Ag+, K+ and Pb2+ cations produces Silver chloride (AgCl), Potassium chloride (KCl) and Lead chloride (Pb2Cl) respectively so we can conclude that Silver chloride (AgCl), Potassium chloride (KCl) and Lead chloride (Pb2Cl) are produced when added the solution of chlorine.
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