Problem: A Cu/Cu2+ concentration cell has a voltage of 0.21V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.6. What is the concentration of Cu2+ in the other half-cell?

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Cu2+ (aq) + Cu (s) → Cu2+ (aq) + Cu (s) 

↓ E° → oxidation → anode

↑ E° → reduction → cathode


E°cell=E°cathode-E°anode  

E°cell = 0 V


Calculate Ecell.

Ecell =E°cell- (0.0592n)log[Cu2+] anode[Cu2+] cathode0.21=0- (0.05922)log[Cu2+] anode[Cu2+] cathode 

[Cu2+] anode must be less than [Cu2+] cathode to have a positive Ecell

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A Cu/Cu2+ concentration cell has a voltage of 0.21V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.6. What is the concentration of Cu2+ in the other half-cell?

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