Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Problem Statement:**
Determine the pH of a buffer formed by dissolving 20.0 g of NaCH₃COO into a 500.0 mL solution of 0.150 M of CH₃COOH. Assume the volume of the solution does not change. The value of Kₐ for CH₃COOH is 1.8 × 10⁻⁵.
**Instructions:**
1. Use the ICE (Initial, Change, Equilibrium) table and the definition of Kₐ to set up the expression.
2. Do not combine or simplify terms.
**Expression for Kₐ:**
\[ K_a = \frac{\text{[H⁺][A⁻]}}{\text{[HA]}} = 1.8 \times 10^{-5} \]
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Transcribed Image Text:**Problem Statement:**
Determine the pH of a buffer formed by dissolving 20.0 g of NaCH₃COO into a 500.0 mL solution of 0.150 M of CH₃COOH. Assume the volume of the solution does not change. The value of Kₐ for CH₃COOH is 1.8 × 10⁻⁵.
**Instructions:**
1. Use the ICE (Initial, Change, Equilibrium) table and the definition of Kₐ to set up the expression.
2. Do not combine or simplify terms.
**Expression for Kₐ:**
\[ K_a = \frac{\text{[H⁺][A⁻]}}{\text{[HA]}} = 1.8 \times 10^{-5} \]
**Navigation:**
- PREV (1)
- CURRENT (2)
- NEXT (3)
![**Instruction:**
**Determine the pH of a buffer formed by dissolving 20.0 g NaCH₃COO into a 500.0 mL solution of 0.150 M of CH₃COOH. Assume the volume of the solution does not change. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵.**
**Buffer Preparation Steps:**
1. **Calculate Molarity of NaCH₃COO:**
- Dissolve 20.0 g NaCH₃COO in a 500.0 mL solution.
- Determine moles and convert to molarity.
2. **Use ICE Table to calculate equilibrium concentrations:**
- **Initial Concentrations (M):**
- CH₃COOH(aq): [Initial]
- H₂O(l): [Pure Liquid, not included in equilibrium]
- H₃O⁺(aq): 0
- CH₃COO⁻(aq): [Initial]
- **Change in Concentrations (M):**
- Change due to reaction.
- **Equilibrium Concentrations (M):**
- Use changes to find equilibrium concentrations.
**ICE Table Setup:**
| Reactant/Product | CH₃COOH(aq) | H₂O(l) | ⇌ | H₃O⁺(aq) | CH₃COO⁻(aq) |
|------------------|-------------|------------|---|------------|--------------|
| Initial (M) | | | | | |
| Change (M) | | | | | |
| Equilibrium (M) | | | | | |
**Next Steps:**
1. Calculate pH using equilibrium concentrations.
2. Use the buffer equation and equilibrium data to confirm calculations.
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Transcribed Image Text:**Instruction:**
**Determine the pH of a buffer formed by dissolving 20.0 g NaCH₃COO into a 500.0 mL solution of 0.150 M of CH₃COOH. Assume the volume of the solution does not change. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵.**
**Buffer Preparation Steps:**
1. **Calculate Molarity of NaCH₃COO:**
- Dissolve 20.0 g NaCH₃COO in a 500.0 mL solution.
- Determine moles and convert to molarity.
2. **Use ICE Table to calculate equilibrium concentrations:**
- **Initial Concentrations (M):**
- CH₃COOH(aq): [Initial]
- H₂O(l): [Pure Liquid, not included in equilibrium]
- H₃O⁺(aq): 0
- CH₃COO⁻(aq): [Initial]
- **Change in Concentrations (M):**
- Change due to reaction.
- **Equilibrium Concentrations (M):**
- Use changes to find equilibrium concentrations.
**ICE Table Setup:**
| Reactant/Product | CH₃COOH(aq) | H₂O(l) | ⇌ | H₃O⁺(aq) | CH₃COO⁻(aq) |
|------------------|-------------|------------|---|------------|--------------|
| Initial (M) | | | | | |
| Change (M) | | | | | |
| Equilibrium (M) | | | | | |
**Next Steps:**
1. Calculate pH using equilibrium concentrations.
2. Use the buffer equation and equilibrium data to confirm calculations.
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