The following acidic galvanic cell is set-up with the following overall cell reaction 14 H*(ag) + Cr207 (aq) + 6 Ag() → 6 Ag" (aq) + 2 Cr*(aq) +7 H2O() V Porous Barrier Pt Ag 0.22 M Na2Cr207 0.25 M Cr(NO3)3 0.20 M AGNO3 If the cell voltage is 0.257 V, what is the pH of the cell?
The following acidic galvanic cell is set-up with the following overall cell reaction 14 H*(ag) + Cr207 (aq) + 6 Ag() → 6 Ag" (aq) + 2 Cr*(aq) +7 H2O() V Porous Barrier Pt Ag 0.22 M Na2Cr207 0.25 M Cr(NO3)3 0.20 M AGNO3 If the cell voltage is 0.257 V, what is the pH of the cell?
Chemistry
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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
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![### Educational Resource: Galvanic Cell Chemistry
**Galvanic Cell Setup and Reaction**
The following acidic galvanic cell is set up with the overall cell reaction:
\[ 14 \text{ H}^+ (\text{aq}) + \text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 6 \text{ Ag} (\text{s}) \rightarrow 6 \text{ Ag}^+ (\text{aq}) + 2 \text{ Cr}^{3+} (\text{aq}) + 7 \text{ H}_2\text{O} (\text{l}) \]
**Diagram Explanation**
The diagram showing the setup of the galvanic cell includes the following details:
- **Electrodes and Half-Cells**:
- The left half-cell contains a platinum (Pt) electrode immersed in a solution with 0.22 M Na\(_2\)Cr\(_2\)O\(_7\) and 0.25 M Cr(NO\(_3\))\(_3\).
- The right half-cell contains a silver (Ag) electrode immersed in a solution of 0.20 M AgNO\(_3\).
- **Porous Barrier**:
- A porous barrier separates the two solutions, allowing ionic movement while preventing the direct mixing of the different solutions.
- **Voltage Measurement**:
- A voltmeter (V) is connected between the two electrodes to measure the cell voltage.
**Question**
If the cell voltage is 0.257 V, what is the pH of the cell?
---
The diagram visually represents the galvanic cell, which is a type of electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. The setup includes key components necessary for understanding galvanic cells' operations, such as electrodes, electrolyte solutions, and voltage measurement. This configuration is typical in educational contexts to demonstrate fundamental principles of electrochemistry.
---
**Answer Calculation**
To answer the question regarding the pH of the cell, additional calculation steps involving the Nernst equation would be necessary.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5d4e0e1f-a295-43e5-adcc-ec19e6606cd6%2Fbb4fbb23-bfd8-4723-afd4-7799353758fd%2F9i0mkgl.jpeg&w=3840&q=75)
Transcribed Image Text:### Educational Resource: Galvanic Cell Chemistry
**Galvanic Cell Setup and Reaction**
The following acidic galvanic cell is set up with the overall cell reaction:
\[ 14 \text{ H}^+ (\text{aq}) + \text{Cr}_2\text{O}_7^{2-} (\text{aq}) + 6 \text{ Ag} (\text{s}) \rightarrow 6 \text{ Ag}^+ (\text{aq}) + 2 \text{ Cr}^{3+} (\text{aq}) + 7 \text{ H}_2\text{O} (\text{l}) \]
**Diagram Explanation**
The diagram showing the setup of the galvanic cell includes the following details:
- **Electrodes and Half-Cells**:
- The left half-cell contains a platinum (Pt) electrode immersed in a solution with 0.22 M Na\(_2\)Cr\(_2\)O\(_7\) and 0.25 M Cr(NO\(_3\))\(_3\).
- The right half-cell contains a silver (Ag) electrode immersed in a solution of 0.20 M AgNO\(_3\).
- **Porous Barrier**:
- A porous barrier separates the two solutions, allowing ionic movement while preventing the direct mixing of the different solutions.
- **Voltage Measurement**:
- A voltmeter (V) is connected between the two electrodes to measure the cell voltage.
**Question**
If the cell voltage is 0.257 V, what is the pH of the cell?
---
The diagram visually represents the galvanic cell, which is a type of electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. The setup includes key components necessary for understanding galvanic cells' operations, such as electrodes, electrolyte solutions, and voltage measurement. This configuration is typical in educational contexts to demonstrate fundamental principles of electrochemistry.
---
**Answer Calculation**
To answer the question regarding the pH of the cell, additional calculation steps involving the Nernst equation would be necessary.
Transcribed Image Text:**Standard Reduction Potentials**
The table of standard reduction potentials provides a comparison of the ability of various chemical species to gain electrons, thus reducing. This data is presented in volts (ℰ°) against the standard hydrogen electrode, which is set at 0.00 volts. Understanding these potentials is crucial for predicting the direction of redox reactions and for the calculation of electromotive force (EMF) in electrochemical cells.
| Couple | ℰ° (Volts) | Couple | ℰ° (Volts) |
|-------------------------|------------|-----------------------|------------|
| F2 ---- HF (H⁺) | +3.03 | SO4²⁻ ---- H2SO3 (H⁺) | +0.20 |
| F2 ---- F⁻ | +2.87 | Sn4⁺ ---- Sn2⁺ | +0.15 |
| S2O8²⁻ ---- SO4²⁻ | +2.05 | S ---- H2S (H⁺) | +0.141 |
| BiO3⁻ ---- Bi³⁺ | +2.0 | Hg2Br2 ---- Hg (Br⁻) | +0.140 |
| H2O2 ---- H2O (H⁺) | +1.78 | AgBr ---- Ag (Br⁻) | +0.0713 |
| PbO2 ---- PbSO4 (H⁺, SO4²⁻) | +1.685 | H⁺ ---- H2 | +0.0000 |
| Ce4⁺ ---- Ce³⁺ | +1.61 | Pb²⁺ ---- Pb | -0.126 |
| MnO4⁻ ---- Mn2⁺ (H⁺) | +1.491 | Sn2⁺ ---- Sn | -0.136 |
| ClO3⁻ ---- Cl¹⁻ | +1.47 | AgI ---- Ag (I⁻) | -0.152 |
| PbO2 ---- Pb2⁺ (H⁺) | +1.46 | Ni2⁺ ---- Ni | -0.250 |
| Au3⁺ ---- Au
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