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.)

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Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.6: Equilibria Involving Complex Ions
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Consider the reversible dissolution of lead(II) 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.)
Type answer:
Transcribed Image Text:Consider the reversible dissolution of lead(II) 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.) Type answer:
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