Question 4Since E can be used to determine Q and vice versa, if you know the Ksp of a salt, youcan 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 Ag3PO4 and the other half-cell isa silver electrode in a 0.5 M solution of AgNO3.We start with determining the concentration of Ag+ in the saturated solution. TheKsp of silver phosphate is 1.8 x 10-18.What is the solubility of silver phosphate?What is the concentration of Ag+?Now we can use the Nernst equation to find E for our cell:Ag(s) Aga) (saturated conc.A/AIn the Nernst equation, what value will we have for E?AAA/Now we can use the Nernst equation to find E for our cell:Ag(s) Ag(aq) (saturated conc. .) || Agaq) (0.5 M) | Ag(s)In the Nernst equation, what value will we have for Eº?nc.) || Agaq) (0.5 M) |In the Nernst equation, what value will we have for n?AAg(s)Given the concentration you found, what is the value for Q? (If you couldn't solve the first part, use 1.0x 103 M as the concentration you needed to find so you can solve for Q and continue the problem).A/Now solve for E. What is this value? Use 298 K as the temperature and 96485 C/s for F

Answered: Image /qna-images/answer/6a2f94d1-eaf9-4d95-8e3a-5f928bf33048.jpg

Since E can be used to determine Q and vice versa, 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 Ag3PO4 and the other half-cell is a silver electrode in a 0.5 M solution of AgNO3. We start with determining the concentration of Ag+ in the saturated solution. The Ksp of silver phosphate is 1.8 x 10-18 What is the solubility of silver phosphate? What is the concentration of Ag+? Now we can use the Nernst equation to find E for our cell: Ag(s) Agaq) (saturated conc. c.) || Ag(aq) (0.5 M) | A A In the Nernst equation, what value will we have for E*? A/ A Now we can use the Nernst equation to find E for our cell: Ag(s) Ag(aq) saturated conc. ) || Ag) (0.5 M)| Ag(s) In the Nernst equation, what value will we have for Eº? A In the Nernst equation, what value will we have for n? A/ Ag(s) Given the concentration you found, what is the value for Q? (If you couldn't solve the first part, use 1.0 x 103 M as the concentration you needed to find so you can solve for Q and continue the problem). A Now solve for E. What is this value? Use 298 K as the temperature and 96485 C/s for F

Since E can be used to determine Q and vice versa, 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 Ag3PO4 and the other half-cell is a silver electrode in a 0.5 M solution of AgNO3. We start with determining the concentration of Ag+ in the saturated solution. The Ksp of silver phosphate is 1.8 x 10-18 What is the solubility of silver phosphate? What is the concentration of Ag+? Now we can use the Nernst equation to find E for our cell: Ag(s) Agaq) (saturated conc. c.) || Ag(aq) (0.5 M) | A A In the Nernst equation, what value will we have for E*? A/ A Now we can use the Nernst equation to find E for our cell: Ag(s) Ag(aq) saturated conc. ) || Ag) (0.5 M)| Ag(s) In the Nernst equation, what value will we have for Eº? A In the Nernst equation, what value will we have for n? A/ Ag(s) Given the concentration you found, what is the value for Q? (If you couldn't solve the first part, use 1.0 x 103 M as the concentration you needed to find so you can solve for Q and continue the problem). A Now solve for E. What is this value? Use 298 K as the temperature and 96485 C/s for F

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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