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Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

Chemistry
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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### Buffer pH Calculation **Problem:** Calculate the pH of a buffer system containing 1.0 M CH₃COOH and 1.2 M CH₃COONa. The \( K_a \) for the acid is \( 1.8 \times 10^{-5} \). To find the pH of the buffer system, use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where: - \(\text{p}K_a = -\log K_a\) - \([\text{A}^-]\) is the concentration of the conjugate base (CH₃COONa) - \([\text{HA}]\) is the concentration of the weak acid (CH₃COOH) ### Step-by-Step Solution: 1. **Calculate \(\text{p}K_a\):** \[ \text{p}K_a = -\log (1.8 \times 10^{-5}) \] \[ \text{p}K_a \approx 4.74 \] 2. **Apply the Henderson-Hasselbalch Equation:** \[ \text{pH} = 4.74 + \log \left( \frac{1.2}{1.0} \right) \] \[ \text{pH} = 4.74 + \log (1.2) \] \[ \text{pH} = 4.74 + 0.079 \] \[ \text{pH} \approx 4.82 \] So, the pH of the buffer system is approximately 4.82.
Transcribed Image Text:### Buffer pH Calculation **Problem:** Calculate the pH of a buffer system containing 1.0 M CH₃COOH and 1.2 M CH₃COONa. The \( K_a \) for the acid is \( 1.8 \times 10^{-5} \). To find the pH of the buffer system, use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where: - \(\text{p}K_a = -\log K_a\) - \([\text{A}^-]\) is the concentration of the conjugate base (CH₃COONa) - \([\text{HA}]\) is the concentration of the weak acid (CH₃COOH) ### Step-by-Step Solution: 1. **Calculate \(\text{p}K_a\):** \[ \text{p}K_a = -\log (1.8 \times 10^{-5}) \] \[ \text{p}K_a \approx 4.74 \] 2. **Apply the Henderson-Hasselbalch Equation:** \[ \text{pH} = 4.74 + \log \left( \frac{1.2}{1.0} \right) \] \[ \text{pH} = 4.74 + \log (1.2) \] \[ \text{pH} = 4.74 + 0.079 \] \[ \text{pH} \approx 4.82 \] So, the pH of the buffer system is approximately 4.82.
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