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 H₂EDTA²^-, resulting in the reaction: H₂EDTA²^- + V²⁺ VEDTA²^- + 2H⁺ The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred when 500.0 mL of H₂EDTA²^- solution was added. At the stoichiometric point, E_cell was 1.98 V. The solution was buffered at pH 10.00.

Question

Quizplus · Accepted Answer

The Answer of 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 H₂EDTA²^-, resulting in the reaction: H₂EDTA²^- + V²⁺ VEDTA²^- + 2H⁺ The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred when 500.0 mL of H₂EDTA²^- solution was added. At the stoichiometric point, E_cell was 1.98 V. The solution was buffered at pH 10.00.

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

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