A voltaic cell is constructed by immersing a strip of copper metal in 1.0 M CuSO 4 solution and a strip of aluminum in 0.50 M Al 2(SO 4) 3 solution. A wire and a salt bridge complete the circuit. The aluminum strip loses mass, and the concentration of aluminum ions in the solution increases. The copper electrode gains mass, and the concentration of copper ions decreases. What is the cell potential?
To determine the cell potential, we need to know the reduction potentials of the half-reactions involved in the voltaic cell.
Firstly, let's write out the balanced half-reactions that occur at each electrode:
At the copper electrode: Cu^2+ + 2e^- -> Cu
At the aluminum electrode: 2Al -> 2Al^3+ + 6e^-
The standard reduction potential for the copper half-reaction is +0.34 V, and for the aluminum half-reaction, it is -1.66 V.
To find the overall cell potential, we subtract the reduction potential of the anode (aluminum) from the reduction potential of the cathode (copper):
Cell Potential = Reduction Potential (cathode) - Reduction Potential (anode)
= 0.34 V - (-1.66 V)
= 0.34 V + 1.66 V
= 2.00 V
So, the cell potential is 2.00 V in this voltaic cell.