Cu²⁺ + 2e^- $\rightarrow$ Cu(s) E° = 0 $\rightarrow$ V(s) E° = -1

question 70

Short Answer

Cu²⁺ + 2e^- $\rightarrow$ Cu(s) E° = 0.34 V
V²⁺ + 2e^- $\rightarrow$ V(s) E° = -1.20 V
In a galvanic cell, the copper compartment contains a copper electrode and [Cu²⁺] = 1.00 M. The vanadium compartment contains a vanadium electrode and V²⁺ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H₂EDTA^2-, resulting in the reaction:
H₂EDTA^2- + V²⁺ VEDTA^2- + 2H⁺
The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred when 500.0 mL of H₂EDTA^2- solution was added. At the stoichiometric point, E_cell was 1.98 V. The solution was buffered at pH 10.00.
A) Calculate E_cell before titration was carried out.
B) Calculate the equilibrium constant K for the titration reaction.
C) Calculate E_cell at the halfway point of titration.

• A) Calculate E_cell before titration was carried out.
• B) Calculate the equilibrium constant K for the titration reaction.
• C) Calculate E_cell at the halfway point of titration.

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