We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cell is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G°

We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cell is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G°

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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