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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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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