A galvanic cell is based on the following half reactions: Cu 2+ + 2e - Cu(s) o = 0.34 V V 2+ +

A galvanic cell is based on the following half reactions:

Cu²⁺ + 2e^-  →  Cu(s) ϐ^o = 0.34 V

V²⁺ + 2e^- → V(s) ϐ^o = 21.20 V

In this cell the copper compartment contains a copper electrode and [Cu²⁺] = 1.00 M, and 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-(aq) + V²⁺(aq) ⇌ VEDTA^2-(aq) + 2H⁺(aq) K = ? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL of H₂EDTA^2- solution added. At the stoichiometric point, ϐ cell was observed to be 1.98 V. The solution was buffered at a pH of 10.00.

a. Calculate ϐ cell before the titration was carried out.

b. Calculate the value of the equilibrium constant K for the titration reaction.

c. Calculate ϐ cell at the halfway point in the titration.