The quinone electrode was introduced in the 1920's as a means of measuring solution pH. Consider the following quinone voltaic cell: Pt (s) | 1:1 mole ratio of quinone:hydroquinone in solution of unknown pH || NaCl (ag) (0.5 M) | Hg»Cl2 (s) | Hg (1) | Pt (s) Half-reaction E° (V) quinone (ag) + 2 H* (ag) + 2 e-2 hydroquinone (aq) Hg2Cl2 (s) + 2 e- 2 2 Hg (1) + 2 Cl (aq) 0.700 0.268 a. Write a Nernst equation that describes this voltaic cell then rearrange it into the form Ecell = A + B pH, where A and B are constants. Determine the values of these constants at room temperature. b. What is the expected cell potential if the 1:1 mole ratio of quinone:hydroquinone is dissolved in a solution of pH 4.5? Assume the dissolution of the hydroquinone does not affect the solution pH. O: но HO- quinone hydroquinone

The quinone electrode was introduced in the 1920's as a means of measuring solution pH. Consider the following quinone voltaic cell: Pt (s) | 1:1 mole ratio of quinone:hydroquinone in solution of unknown pH || NaCl (ag) (0.5 M) | Hg»Cl2 (s) | Hg (1) | Pt (s) Half-reaction E° (V) quinone (ag) + 2 H* (ag) + 2 e-2 hydroquinone (aq) Hg2Cl2 (s) + 2 e- 2 2 Hg (1) + 2 Cl (aq) 0.700 0.268 a. Write a Nernst equation that describes this voltaic cell then rearrange it into the form Ecell = A + B pH, where A and B are constants. Determine the values of these constants at room temperature. b. What is the expected cell potential if the 1:1 mole ratio of quinone:hydroquinone is dissolved in a solution of pH 4.5? Assume the dissolution of the hydroquinone does not affect the solution pH. O: но HO- quinone hydroquinone

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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Question

The quinone electrode was introduced in the 1920's as a means of measuring solution pH. Consider the following quinone voltaic cell:

\[ \text{Pt (s)} \mid 1:1 \text{ mole ratio of quinone:hydroquinone in solution of unknown pH} \parallel \text{NaCl (aq) (0.5 M)} \mid \text{Hg}_2\text{Cl}_2 (s) \mid \text{Hg (l)} \mid \text{Pt (s)} \]

\[
\begin{array}{c|c}
\text{Half-reaction} & E^\circ \text{ (V)} \\
\hline
\text{quinone (aq) + 2 H}^+ \text{(aq) + 2 e}^- \leftrightarrow \text{hydroquinone (aq)} & 0.700 \\
\text{Hg}_2\text{Cl}_2 \text{(s) + 2 e}^- \leftrightarrow 2 \text{Hg (l)} + 2 \text{Cl}^- \text{(aq)} & 0.268 \\
\end{array}
\]

a. Write a Nernst equation that describes this voltaic cell then rearrange it into the form
\[ E_{\text{cell}} = A + B \cdot \text{pH} \]
where \( A \) and \( B \) are constants. Determine the values of these constants at room temperature.

b. What is the expected cell potential if the 1:1 mole ratio of quinone:hydroquinone is dissolved in a solution of pH 4.5? Assume the dissolution of the hydroquinone does not affect the solution pH.

Below is a structural depiction of quinone and hydroquinone:

- **Quinone:** A six-membered benzene ring with two carbonyl groups (C=O) at opposite positions.
- **Hydroquinone:** A six-membered benzene ring with two hydroxyl groups (OH) at opposite positions.

This diagram is essential for understanding the structures involved in the redox reactions of the quinone/hydroquinone pair.

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