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Inorganic and Applied Chemistry
[Pb2+] 0 = 0 M
[I-] 0 = 3.33 · 10-2 M
The end concentrations is found on the basis of the reaction scheme:
PbI 2 (s) Pb2+(aq) + 2 I-(aq)
[Pb2+] = x
[I-] = 3.33 · 10-2 M + 2x
And by insertion into the expression for Ksp in the equation we achieve:
Ksp = 1.4 · 10-8 M^3 = [Pb2+] · [I-] = x · (3.33 · 10-2 M + 2x)^2
x = 1.3 · 10-5 M
Thus, the equilibrium concentrations become:
[Pb2+]equilibrium = 1.3 · 10-5 M
[I-] equilibrium = 3.33 · 10-2 M + 2x 3.33 · 10-2 M
Thereby we have determined the equilibrium concentrations of lead and iodine ions in a solution that is
prepared by mixing solutions of sodium iodine and lead.
Equilibrium