In a cell containing copper and Hydrogen electrode, Copper will be the cathode and Hydrogen electrode will be the anode.
A.
At anode, H2 (g) ------->2H+ + 2e-
At Cathode, Cu2+(aq) +2e- ---> Cu (s)
Cell reaction Cu2+(aq) + H2 (g) --------> 2H+ + Cu (s)
[Cu2+] = 3.8 x 10-4M (given)
E0 = 0.34V
Nernst equation is given by
E = E0- (0.0592/n) log {[H+]2/[Cu2+]}
E = 0.34 – (0.0592/2) Log{1/3.8 x 10-4M}
E = 0.23876 V
B.
E = E0- (0.0592/2) log {[H+]2/[Cu2+]}
E = 0.206 V (given)
0.206 = 0.34 + 0.0296 log[Cu2+]
log[Cu2+] = -4.4966
[Cu2+] = 3.186 x 10-5 M
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