When lead metal (Pb) is added to a 0.300 M solution of Cr+3 at room temperature, an oxidation/reduction equilibrium is established. The equation for this equilibrium appears below:
Pb (s) + 2 Cr3+ (aq) Pb2+ (aq) + 2 Cr2+ (aq) Keq = 3.2 X 10-10
When the equilibrium is reached, what are all of the concentrations in solution (this is also called the equilibrium composition)?
[Cr3+] =
[Pb2+] =
[Cr2+] =