Consider the reversible dissolution of lead(11) chloride. PbCl₂ (s) Pb²+ (aq) + 2Cl(aq) Suppose you add 0.2310 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.)
Consider the reversible dissolution of lead(11) chloride. PbCl₂ (s) Pb²+ (aq) + 2Cl(aq) Suppose you add 0.2310 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.)
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.6: Equilibria Involving Complex Ions
Problem 1.4ACP: Silver undergoes similar reactions as those shown for gold. Both metals react with cyanide ion in...
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