A copper,(Cu(s) , electrode is immersed in a solution that is 1.00 M in ammonia,NH3 , and 1.00M in tetraamminecopper(II),[Cu(NH3)4]^2+ . If a standard hydrogen electrode is used as the cathode, the cell potential,Ecell , is found to be 0.074V at 298K .
Based on the cell potential, what is the concentration of \rm Cu^{2+} in this solution?
Additional data..
Use the standard reduction potentials shown here to answer the questions.
Reduction half-reaction
0.337 V Cu^2+(aq) + 2e- ------->Cu(s)
0.000V 2H^+(aq) +2e- ------->H2(g)