Consider the reversible dissolution of lead(II) chloride. PbCl2(s)−⇀↽−Pb2+(aq)+2Cl−(aq) Suppose you add 0.2296 g of PbCl2(s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+(aq) is 0.0159 M and the concentration of Cl−(aq) is 0.0318 M. What is the value of the equilibrium constant, Kc, for the dissolution of PbCl2?
Consider the reversible dissolution of lead(II) chloride. PbCl2(s)−⇀↽−Pb2+(aq)+2Cl−(aq) Suppose you add 0.2296 g of PbCl2(s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+(aq) is 0.0159 M and the concentration of Cl−(aq) is 0.0318 M. What is the value of the equilibrium constant, Kc, for the dissolution of PbCl2?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 61QRT
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Consider the reversible dissolution of lead(II) chloride.
PbCl2(s)−⇀↽−Pb2+(aq)+2Cl−(aq)
Suppose you add 0.2296 g of PbCl2(s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+(aq) is 0.0159 M and the concentration of Cl−(aq) is 0.0318 M. What is the value of the equilibrium constant, Kc, for the dissolution of PbCl2?
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