Using the Nernst equation, determine the concetration of Cu(II) needed to produce a concentration cell, in combination with the provided 0.10 M Cu(II) solution, that will have a measured cell potential of 0.030 V.
Cu2+ +2e- > Cu
Eo for above reaction is = 0.34 V
E cell = Eo cell - (0.059/n) log (c1/c2)
0.03 = 0.34 - (0.059/2) log (c1/c2)
log (c1/c2) = 10.51
c1/c2 = 3.22*10^10
There are 2 possible possible answers depending on the avialable call of 0.1 M is used as cathode or anode.
If c1= 0.1 M then c2= 3.11*10^-12 M
If c1= 0.1 M then c2= 3.22*10^9 M
Answers are:
3.11*10^-12 M or 3.22*10^9 M
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