Consider the reversible dissolution of lead(II) chloride. PbCl₂ (s) Pb²+ (aq) + 2Cl- (aq) Suppose you add 0.2425 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, Ksp, for the dissolution of PbCl₂ ? (Note that the equilibrium constant associated with sparingly soluble salts is called the solubility product constant, Ksp.) Type answer:
Consider the reversible dissolution of lead(II) chloride. PbCl₂ (s) Pb²+ (aq) + 2Cl- (aq) Suppose you add 0.2425 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, Ksp, for the dissolution of PbCl₂ ? (Note that the equilibrium constant associated with sparingly soluble salts is called the solubility product constant, Ksp.) Type answer:
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 30P
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