A solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10.
(A) Assuming that the hydroxide is 1.0 x 10^-2 M, calculate the concentration of Fe2+ ions in the solution.
(B) A battery is prepared using the above solution with an iron wire dipping into it as one half-cell. The other half-cell is the standard nickel electrode. Write the balanced net ionic equation for the cell reaction.
(c) use the nerst equation to calculate the potential of the above cell.
I don't know how to do B & C
For (A) i got 8.0*10^-6M. if not please help
Thank You!
Ni2+(aq) +2e- --> Ni(s) -0.28V
Fe2+(aq) + 2e- --> Fe(s) -0.440V
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