10. Electrochemical cells, E° values and the Nernst Equation. Given the following diagram for a galvanic cell, Cu | CuSO4(0.010 M)||AgNO3(0.30 M)| Ag a) Prepare a sketch of the cell. b) Write balanced equations for the half-cell reactions and for the over-all reaction that occurs when the copper and silver wires are connected c) Calculate E°cell and show on your diagram the direction of flow of electrons between the half cells. d) Use the Nernst equation to calculate Ecel from E°cell and the concentrations of the electrolytes. 11. Potentiometric titration with electrochemical monitoring. The cell described in 10 can be used to monitor the concentration of Ag* ion in the titration of a soluble chloride or bromide with AGNO3. The potential of a silver wire immersed in the chloride solution, measured relative to a Cu|CUSO4(1 M) reference electrode which makes contact with the analyte solution through a porous thread (see sketch), is given by E(volts) = 0.46 - 0.059 pAg where pAg = -log[Ag*]. a) Derive the above equation from the Nernst equation and the E° values of the Cu2*|Cu and Ag*|Ag half-cells (question 10). b) Calculate the potential of the cell at the equivalence point in the precipitation titration of a soluble chloride with silver nitrate.
10. Electrochemical cells, E° values and the Nernst Equation. Given the following diagram for a galvanic cell, Cu | CuSO4(0.010 M)||AgNO3(0.30 M)| Ag a) Prepare a sketch of the cell. b) Write balanced equations for the half-cell reactions and for the over-all reaction that occurs when the copper and silver wires are connected c) Calculate E°cell and show on your diagram the direction of flow of electrons between the half cells. d) Use the Nernst equation to calculate Ecel from E°cell and the concentrations of the electrolytes. 11. Potentiometric titration with electrochemical monitoring. The cell described in 10 can be used to monitor the concentration of Ag* ion in the titration of a soluble chloride or bromide with AGNO3. The potential of a silver wire immersed in the chloride solution, measured relative to a Cu|CUSO4(1 M) reference electrode which makes contact with the analyte solution through a porous thread (see sketch), is given by E(volts) = 0.46 - 0.059 pAg where pAg = -log[Ag*]. a) Derive the above equation from the Nernst equation and the E° values of the Cu2*|Cu and Ag*|Ag half-cells (question 10). b) Calculate the potential of the cell at the equivalence point in the precipitation titration of a soluble chloride with silver nitrate.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![10. Electrochemical cells, E° values and the Nernst Equation. Given the following diagram for a
galvanic cell,
Cu | CuSO4(0.010 M)||AgNO3(0.30 M)| Ag
a) Prepare a sketch of the cell.
b) Write balanced equations for the half-cell reactions and for the over-all reaction that occurs when
the copper and silver wires are connected
c) Calculate E°cell and show on your diagram the direction of flow of electrons between the half cells.
d) Use the Nernst equation to calculate Ecel from E°cell and the concentrations of the electrolytes.
11. Potentiometric titration with electrochemical monitoring. The cell described in 10 can be used
to monitor the concentration of Ag* ion in the titration of a soluble chloride or bromide with AGNO3.
The potential of a silver wire immersed in the chloride solution, measured relative to a Cu|CUSO4(1
M) reference electrode which makes contact with the analyte solution through a porous thread (see
sketch), is given by
E(volts) = 0.46 - 0.059 pAg
where pAg = -log[Ag*].
a) Derive the above equation from the Nernst equation and the E° values of the Cu2*|Cu and Ag*|Ag
half-cells (question 10).
b) Calculate the potential of the cell at the equivalence point in the precipitation titration of a soluble
chloride with silver nitrate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fef0f8725-cbe2-4b3a-903c-3a49204031c7%2F35d4de9c-3790-4481-89ad-e577d2a7f0e4%2Fbjn0bk.jpeg&w=3840&q=75)
Transcribed Image Text:10. Electrochemical cells, E° values and the Nernst Equation. Given the following diagram for a
galvanic cell,
Cu | CuSO4(0.010 M)||AgNO3(0.30 M)| Ag
a) Prepare a sketch of the cell.
b) Write balanced equations for the half-cell reactions and for the over-all reaction that occurs when
the copper and silver wires are connected
c) Calculate E°cell and show on your diagram the direction of flow of electrons between the half cells.
d) Use the Nernst equation to calculate Ecel from E°cell and the concentrations of the electrolytes.
11. Potentiometric titration with electrochemical monitoring. The cell described in 10 can be used
to monitor the concentration of Ag* ion in the titration of a soluble chloride or bromide with AGNO3.
The potential of a silver wire immersed in the chloride solution, measured relative to a Cu|CUSO4(1
M) reference electrode which makes contact with the analyte solution through a porous thread (see
sketch), is given by
E(volts) = 0.46 - 0.059 pAg
where pAg = -log[Ag*].
a) Derive the above equation from the Nernst equation and the E° values of the Cu2*|Cu and Ag*|Ag
half-cells (question 10).
b) Calculate the potential of the cell at the equivalence point in the precipitation titration of a soluble
chloride with silver nitrate.
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