The following data were measured using a nickel electrode as the standard.
Cu2+ (aq) + 2e- ? Cu (s) + 0.62
Ni2+ (aq) + 2e- ? Ni (s) + 0.00
Fe2+ (aq) + 2e- ?Fe (s) - 0.15
Al3+ (aq) + 3e- ? Al (s) - 1.38
1. which ion is most easily reduced?
2. which metal is most easily oxidized?
3. the copper and aluminum electrodes are connected in a battery.
a) which is the anode?
b) Which is oxidized?
c) What will the battery voltage be?
d) Write a balanced net ionic equation for the reaction that takes place.
4. A solution is prepared in which a slight 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 of Fe(OH)2 = 8.0 x 10-10.
a. Assuming that the hydroxide ion concentration is 1.0 x 10-2 M, calculate the concentration of Fe2+ in the solution.
b. A battery is prepared in which the above solution with an iron wire dipping into it is 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 Nernst equation to calculate the potential of the above cell.