A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e Ag(s) + CI (aq) E°red = 0.2223 V %3D And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red%3D 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V. Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549, what is the concentration of chloride ions in the solution?
A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e Ag(s) + CI (aq) E°red = 0.2223 V %3D And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red%3D 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V. Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549, what is the concentration of chloride ions in the solution?
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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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![**Determining Chloride Ion Concentration Using a Galvanic Cell**
A student aims to determine the chloride ion concentration in a water sample at 25°C using a galvanic cell constructed with a graphite electrode and a half-cell of:
\[ \text{AgCl(s)} + \text{e}^- \rightarrow \text{Ag(s)} + \text{Cl}^-(\text{aq}) \quad E^\circ_{\text{red}} = 0.2223 \, \text{V} \]
And a copper electrode with 0.500 M Cu²⁺ as the second half-cell:
\[ \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Cu(s)} \quad E^\circ_{\text{red}} = 0.337 \, \text{V} \]
The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V.
Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549 V, what is the concentration of chloride ions in the solution?
**Feedback and Notes:**
- Incorrect, 3 attempts remaining
- Your submitted answer contains too many significant figures.
**Your Submission:**
- 0.2322 M
**Feedback:**
- Use the Nernst equation to solve for the concentration of chloride ions based on the cell potential given. Consider how the reaction quotient is calculated.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeef920a-b7fc-42c4-a405-16f92aebf3b1%2F3d82821a-293c-4ea8-841b-2d9996ab02a5%2Fvajent_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Determining Chloride Ion Concentration Using a Galvanic Cell**
A student aims to determine the chloride ion concentration in a water sample at 25°C using a galvanic cell constructed with a graphite electrode and a half-cell of:
\[ \text{AgCl(s)} + \text{e}^- \rightarrow \text{Ag(s)} + \text{Cl}^-(\text{aq}) \quad E^\circ_{\text{red}} = 0.2223 \, \text{V} \]
And a copper electrode with 0.500 M Cu²⁺ as the second half-cell:
\[ \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Cu(s)} \quad E^\circ_{\text{red}} = 0.337 \, \text{V} \]
The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V.
Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549 V, what is the concentration of chloride ions in the solution?
**Feedback and Notes:**
- Incorrect, 3 attempts remaining
- Your submitted answer contains too many significant figures.
**Your Submission:**
- 0.2322 M
**Feedback:**
- Use the Nernst equation to solve for the concentration of chloride ions based on the cell potential given. Consider how the reaction quotient is calculated.
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