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: An Educational Guide**
**1. Balance the following redox equation in basic solution:**
\[
\text{AgO} + \text{HClO} \rightarrow \text{Ag} + \text{HClO}_2
\]
In this task, you are required to balance the given redox reaction, ensuring that the number of atoms and the charge are balanced on both sides of the equation in a basic solution. Follow these general steps to balance the redox reaction:
1. **Separate the reactions into half-reactions:**
- Oxidation half-reaction
- Reduction half-reaction
2. **Balance all elements in the half-reactions except hydrogen and oxygen.**
3. **Balance oxygen atoms by adding \(\text{H}_2\text{O}\).**
4. **Balance hydrogen atoms by adding \(\text{H}^+\).**
5. **Balance the charge by adding electrons (\(e^-\)).**
6. **Combine the half-reactions and ensure that electrons are canceled out.**
7. **Convert to a basic solution by adding \(\text{OH}^-\) ions to both sides of the equation to neutralize any \(\text{H}^+\) ions and form water.**
8. **Simplify the equation if necessary by canceling out water molecules on both sides.**
By following these steps, more in-depth and specific calculations can be executed, leading to the balanced redox equation appropriate for a basic solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2704aedc-cd59-4651-b157-0d8c71ae74f0%2F2666b818-a8db-4ab7-abf5-6f9bf6324a89%2Fhims5zn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing Redox Reactions: An Educational Guide**
**1. Balance the following redox equation in basic solution:**
\[
\text{AgO} + \text{HClO} \rightarrow \text{Ag} + \text{HClO}_2
\]
In this task, you are required to balance the given redox reaction, ensuring that the number of atoms and the charge are balanced on both sides of the equation in a basic solution. Follow these general steps to balance the redox reaction:
1. **Separate the reactions into half-reactions:**
- Oxidation half-reaction
- Reduction half-reaction
2. **Balance all elements in the half-reactions except hydrogen and oxygen.**
3. **Balance oxygen atoms by adding \(\text{H}_2\text{O}\).**
4. **Balance hydrogen atoms by adding \(\text{H}^+\).**
5. **Balance the charge by adding electrons (\(e^-\)).**
6. **Combine the half-reactions and ensure that electrons are canceled out.**
7. **Convert to a basic solution by adding \(\text{OH}^-\) ions to both sides of the equation to neutralize any \(\text{H}^+\) ions and form water.**
8. **Simplify the equation if necessary by canceling out water molecules on both sides.**
By following these steps, more in-depth and specific calculations can be executed, leading to the balanced redox equation appropriate for a basic solution.
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