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 Solutions**
**Reaction to Balance:**
\[ \text{I}_2(s) + \text{Cu}^{2+}(aq) \rightarrow \text{IO}_3^{-}(aq) + \text{Cu}^{+}(aq) \]
In this redox reaction, iodine (\(\text{I}_2\)) reacts with copper ions (\(\text{Cu}^{2+}\)) in an acidic solution to form iodate ions (\(\text{IO}_3^{-}\)) and copper (\(\text{Cu}^{+}\)).
**Steps for Balancing:**
1. **Identify Oxidation and Reduction**:
- **Oxidation**: Iodine (\(\text{I}_2\)) is oxidized to iodate (\(\text{IO}_3^{-}\)).
- **Reduction**: Copper ions (\(\text{Cu}^{2+}\)) are reduced to copper (\(\text{Cu}^{+}\)).
2. **Separate Into Half-Reactions**:
- **Oxidation Half-Reaction**: \(\text{I}_2 \rightarrow \text{IO}_3^{-}\)
- **Reduction Half-Reaction**: \(\text{Cu}^{2+} \rightarrow \text{Cu}^{+}\)
3. **Balance Atoms Other than O and H**:
- For iodine, it is already balanced.
- For copper, it is already balanced.
4. **Balance Oxygen Atoms**:
- Add water molecules (\(\text{H}_2\text{O}\)) to the side lacking oxygen in the oxidation half-reaction.
5. **Balance Hydrogen Atoms**:
- Add hydrogen ions (\(\text{H}^+\)) to balance hydrogen from water molecules added.
6. **Balance Charges**:
- Add electrons (\(e^-\)) to balance the charge in both half-reactions.
7. **Combine Half-Reactions**:
- Ensure electrons lost in oxidation equals electrons gained in reduction.
**Final Balanced Equation:** (The exact balanced equation would be provided after carrying out the steps.)
After completing these steps, the balanced reaction will accurately represent the conservation of mass and charge in an acidic solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2F17c233f6-43ff-45f5-b11c-f7145ab0d69f%2Fk6aidtg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing Redox Reactions in Acidic Solutions**
**Reaction to Balance:**
\[ \text{I}_2(s) + \text{Cu}^{2+}(aq) \rightarrow \text{IO}_3^{-}(aq) + \text{Cu}^{+}(aq) \]
In this redox reaction, iodine (\(\text{I}_2\)) reacts with copper ions (\(\text{Cu}^{2+}\)) in an acidic solution to form iodate ions (\(\text{IO}_3^{-}\)) and copper (\(\text{Cu}^{+}\)).
**Steps for Balancing:**
1. **Identify Oxidation and Reduction**:
- **Oxidation**: Iodine (\(\text{I}_2\)) is oxidized to iodate (\(\text{IO}_3^{-}\)).
- **Reduction**: Copper ions (\(\text{Cu}^{2+}\)) are reduced to copper (\(\text{Cu}^{+}\)).
2. **Separate Into Half-Reactions**:
- **Oxidation Half-Reaction**: \(\text{I}_2 \rightarrow \text{IO}_3^{-}\)
- **Reduction Half-Reaction**: \(\text{Cu}^{2+} \rightarrow \text{Cu}^{+}\)
3. **Balance Atoms Other than O and H**:
- For iodine, it is already balanced.
- For copper, it is already balanced.
4. **Balance Oxygen Atoms**:
- Add water molecules (\(\text{H}_2\text{O}\)) to the side lacking oxygen in the oxidation half-reaction.
5. **Balance Hydrogen Atoms**:
- Add hydrogen ions (\(\text{H}^+\)) to balance hydrogen from water molecules added.
6. **Balance Charges**:
- Add electrons (\(e^-\)) to balance the charge in both half-reactions.
7. **Combine Half-Reactions**:
- Ensure electrons lost in oxidation equals electrons gained in reduction.
**Final Balanced Equation:** (The exact balanced equation would be provided after carrying out the steps.)
After completing these steps, the balanced reaction will accurately represent the conservation of mass and charge in an acidic solution.
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