Use the standard reduction potentials shown here to answer the
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M 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 0.073 V at 298 K.
Based on the cell potential, what is the concentration of Cu2+ in this solution?
Express your answer to one significant figure and include the appropriate units.
The H electrode to form the anode and the standard E(cell) will
be +0.337 v
now assume the [Cu(NH3)4]2+ is not directly involved in the measured cell potential only Cu2+(aq) is.
Then use the Nernst equation to find [Cu2+(aq)]
E(cell) = standard E(cell) - (0.0592/n).log Q ---------------- Formula
where in this case Q = 1/[Cu2+(aq)] and n = 2
E(cell)=0.073 V, standard E(cell)=0.337 V, n=2 calculate Cu2+=?
Put the values in formula
0.073 = 0.337 –(0.0592/2) log(1/ Cu2+)
0.073 + (0.0296) log(1/ Cu2+) = 0.337
(0.0296) log(1/ Cu2+)=0.264
log(1/ Cu2+)= 0.264/0.0296
(1/Cu2+) = 108.92
Cu2+=1.20 x 10-9 M
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