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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![**Balancing Redox Reactions in Basic Solution**
**Problem Statement:**
Balance the following redox reaction in a basic solution:
\[ \text{SO}_3^{2-} \, (\text{aq}) + \text{Cr}_2\text{O}_7^{2-} \, (\text{aq}) \rightarrow \text{Cr}^{3+} \, (\text{aq}) + \text{SO}_4^{2-} \, (\text{aq}) \]
**Explanation:**
This equation represents a redox (reduction-oxidation) reaction. Redox reactions involve the transfer of electrons between species, resulting in changes in oxidation states. To balance a redox reaction in a basic solution, follow these general steps:
1. **Identify the Oxidation and Reduction half-reactions:**
- Determine the oxidation states of the elements involved in the reaction.
- Identify species that are oxidized and reduced.
2. **Balance Each Half-Reaction:**
- Balance elements other than O and H first.
- Balance O by adding H\(_2\)O.
- Balance H by adding H\(^+\) (note: we'll adjust for basic conditions later).
- Balance charge by adding electrons (e\(^-\)).
3. **Combine the Half-Reactions:**
- Ensure the total number of electrons in both half-reactions is equal.
- Add the half-reactions together.
4. **Adjust for Basic Conditions:**
- Add OH\(^-\) to both sides of the equation to neutralize any H\(^+\) present.
- Combine H\(^+\) and OH\(^-\) to form H\(_2\)O.
5. **Finalize the Balanced Equation:**
- Confirm that mass and charge are balanced.
This step-by-step process ensures the equation adheres to the conservation of mass and charge, reflecting the stoichiometry of the redox reaction occurring in a basic solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3b4aa68-1696-4204-931e-d52a90d9be65%2F5d3a7a14-917a-4140-ab8b-29a49156c916%2F3eoikg_processed.png&w=3840&q=75)
Transcribed Image Text:**Balancing Redox Reactions in Basic Solution**
**Problem Statement:**
Balance the following redox reaction in a basic solution:
\[ \text{SO}_3^{2-} \, (\text{aq}) + \text{Cr}_2\text{O}_7^{2-} \, (\text{aq}) \rightarrow \text{Cr}^{3+} \, (\text{aq}) + \text{SO}_4^{2-} \, (\text{aq}) \]
**Explanation:**
This equation represents a redox (reduction-oxidation) reaction. Redox reactions involve the transfer of electrons between species, resulting in changes in oxidation states. To balance a redox reaction in a basic solution, follow these general steps:
1. **Identify the Oxidation and Reduction half-reactions:**
- Determine the oxidation states of the elements involved in the reaction.
- Identify species that are oxidized and reduced.
2. **Balance Each Half-Reaction:**
- Balance elements other than O and H first.
- Balance O by adding H\(_2\)O.
- Balance H by adding H\(^+\) (note: we'll adjust for basic conditions later).
- Balance charge by adding electrons (e\(^-\)).
3. **Combine the Half-Reactions:**
- Ensure the total number of electrons in both half-reactions is equal.
- Add the half-reactions together.
4. **Adjust for Basic Conditions:**
- Add OH\(^-\) to both sides of the equation to neutralize any H\(^+\) present.
- Combine H\(^+\) and OH\(^-\) to form H\(_2\)O.
5. **Finalize the Balanced Equation:**
- Confirm that mass and charge are balanced.
This step-by-step process ensures the equation adheres to the conservation of mass and charge, reflecting the stoichiometry of the redox reaction occurring in a basic solution.
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