Cu²⁺ + 2e^- → Cu(s) E° = 0.34 V
V²⁺ + 2e^- → 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.

Question

Cu²⁺ + 2e^- → Cu(s) E° = 0.34 V
V²⁺ + 2e^- → 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⁺

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

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.

Quizplus · Accepted Answer

The Answer of Cu²⁺ + 2e^- → Cu(s) E° = 0.34 V V²⁺ + 2e^- → 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.

Cu2+ + 2e- → Cu(s) E° = 0

Cu²⁺ + 2e^- → Cu(s) E° = 0