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 Acidic Solution**
**Exercise:**
Complete and balance the following redox reaction in acidic solution.
\[ \text{Bi}_2\text{O}_3 (\text{aq}) + 2\text{S}_2\text{O}_3^{2-} (\text{aq}) + 6\text{H}^+ (\text{aq}) \rightarrow 2\text{Bi}^{3+} (\text{aq}) + \text{S}_4\text{O}_6^{2-} (\text{aq}) + 3\text{H}_2\text{O} (\text{l}) \]
In this exercise, our goal is to balance the given redox reaction. Redox reactions involve the transfer of electrons between chemical species, and balancing them requires ensuring that both mass and charge are conserved.
**Steps to Balance:**
1. **Identify the Oxidation and Reduction Half-Reactions:**
- Determine which species are oxidized and which are reduced.
2. **Balance Each Half-Reaction Separately:**
- Balance the atoms other than O and H.
- Balance the oxygen atoms by adding H₂O.
- Balance hydrogen atoms by adding H⁺.
- Balance the charges by adding electrons.
3. **Combine and Simplify the Balanced Half-Reactions:**
- Ensure that the electrons cancel out.
- Verify that all atoms and charges are balanced.
By applying these steps, chemists can ensure that redox reactions are properly balanced, reflecting the conservation of mass and charge.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F80e404cd-f8d6-49ee-9818-41f84b3d560a%2Fbf7236f4-1764-4570-9e1b-e806388b7078%2Fd2s7xsj.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing Redox Reactions in Acidic Solution**
**Exercise:**
Complete and balance the following redox reaction in acidic solution.
\[ \text{Bi}_2\text{O}_3 (\text{aq}) + 2\text{S}_2\text{O}_3^{2-} (\text{aq}) + 6\text{H}^+ (\text{aq}) \rightarrow 2\text{Bi}^{3+} (\text{aq}) + \text{S}_4\text{O}_6^{2-} (\text{aq}) + 3\text{H}_2\text{O} (\text{l}) \]
In this exercise, our goal is to balance the given redox reaction. Redox reactions involve the transfer of electrons between chemical species, and balancing them requires ensuring that both mass and charge are conserved.
**Steps to Balance:**
1. **Identify the Oxidation and Reduction Half-Reactions:**
- Determine which species are oxidized and which are reduced.
2. **Balance Each Half-Reaction Separately:**
- Balance the atoms other than O and H.
- Balance the oxygen atoms by adding H₂O.
- Balance hydrogen atoms by adding H⁺.
- Balance the charges by adding electrons.
3. **Combine and Simplify the Balanced Half-Reactions:**
- Ensure that the electrons cancel out.
- Verify that all atoms and charges are balanced.
By applying these steps, chemists can ensure that redox reactions are properly balanced, reflecting the conservation of mass and charge.
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