Answered: The answer is (C), but why is (D)…

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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The answer is (C), but why is (D) correct? Why would the negative ions in the salt bridge have to move from "the silver half-cell" to the copper half-cell? Don't the negative ions of whatever compound is in the whole of the salt bridge move to the copper half-cell? Maybe I'm just reading this too closely, let me know. Thanks!

**Electrochemical Cells and Redox Reactions**

**Example Problem:**

A strip of copper is placed in a 1 M solution of copper nitrate and a strip of silver is placed in a 1 M solution of silver nitrate. The two metal strips are connected to a voltmeter by wires and a salt bridge connects the solutions. The following standard reduction potentials apply:

- \( \text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s) \)
- \( E^\circ_{\text{cell}} = 0.80 \, \text{V} \)
- \( \text{Cu}^{2+}(aq) + 2e^- \rightarrow \text{Cu}(s) \)
- \( E^\circ_{\text{cell}} = 0.34 \, \text{V} \)

**Which of the following statements is false?**

A) Electrons flow in the external circuit from the copper electrode to the silver electrode.

B) The silver electrode increases in mass as the cell operates.

C) There is a net general movement of silver ions through the salt bridge to the copper half-cell.

D) Negative ions pass through the salt bridge from the silver half-cell to the copper half-cell.

**Analysis and Explanation:**

- **Statement A**: This statement indicates the direction of electron flow. In an electrochemical cell, electrons flow from the electrode with a lower reduction potential to the electrode with a higher reduction potential. Here, copper has a lower reduction potential (\( 0.34 \, \text{V} \)) than silver (\( 0.80 \, \text{V} \)), so electrons will flow from copper to silver.

- **Statement B**: This statement is correct because as the cell operates, silver ions in the solution gain electrons (are reduced) and deposit as metallic silver on the silver electrode, thereby increasing its mass.

- **Statement C**: This statement involves the function of the salt bridge. The salt bridge allows ions to flow to maintain charge neutrality. Silver ions, being positively charged, will not generally flow through the salt bridge from the silver solution to the copper solution. Instead, the flow typically involves negative ions.

- **Statement D**: To maintain charge balance, anions (negative ions) will move from the silver half-cell to the copper half-cell, counteracting the flow of positive charge through the external circuit.

Expert Solution

Step 1

Since reduction potential of silver is more than the reduction potential of copper. Silver electrode will be cathode and copper electrode will be anode.

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