## Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning

# Chapter 15 - Additional Aqueous Equilibria - Questions for Review and Thought - Topical Questions - Page 693c: 64b

#### Answer

The equilibrium would favor the products, dissolving more of the $PbCl_2(s)$ into $Pb^{2+}$ and $Cl^-$ ions. ** The solid $PbCl_2$ would lose some concentration, but $AgCl(s)$ would be formed.

#### Work Step by Step

This is the equilibrium reaction: $PbCl_2(s) \lt -- \gt Pb^{2+} (aq) + 2Cl^-(aq)$ When we add $AgNO_3$, the $Ag^+$ ions will react with the $Cl^-$ ions, producing $AgCl$ (which will precipitate). Following the Le Chatelier's principle, since we are reducing the concentration of one of the products, the equilibrium will try to raise this concentration, to reduce the change. Therefore, the salt will start to dissolve, because the equilibrium moved to the right.

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