Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

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


The equilibrium would favor the reactants, producing more $PbCl_2(s)$.

Work Step by Step

This is the equilibrium reaction: $PbCl_2(s) \lt -- \gt Pb^{2+} (aq) + 2Cl^-(aq)$ When we add $Pb(NO_3)_2$, the common ion effect (because it has $Pb^{2+}$ ions) will act, and the reaction will be more reactant-favored. That follows the Le Chatelier's principle. Since we are raising the concentration of one of the products, the equilibrium will try to reduce this concentration, to reduce the change.
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