Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 Cl (aq) Suppose you add 0.2460 g of PbCl, (s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb (aq) is 0.0159 M and the concentration of Cl (ag) is 0.0318 M. What is the value of the equilibrium constant, K, for the dissolution of PbCl2 ?
Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 Cl (aq) Suppose you add 0.2460 g of PbCl, (s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb (aq) is 0.0159 M and the concentration of Cl (ag) is 0.0318 M. What is the value of the equilibrium constant, K, 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
Section12.5: Using Equilibrium Constants
Problem 12.6PSP
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