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A solution contains 0.285 M sodium acetate and 5.55x10-2 M acetic acid. The pH of this solution is

A solution contains 0.285 M sodium acetate and 5.55x10-2 M acetic acid. The pH of this solution is

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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**Calculating pH of a Buffer Solution** A solution contains **0.285 M sodium acetate** and **5.55×10^-2 M acetic acid**. The pH of this solution is **__________**. **Explanation:** To calculate the pH of this buffer solution, you can use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{p}K_\text{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where, - \( \text{p}K_\text{a} \) is the negative log of the acid dissociation constant of the weak acid. - \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate, in this case). - \([\text{HA}]\) is the concentration of the weak acid (acetic acid, in this case). For acetic acid: \[ \text{p}K_a \approx 4.76 \] \[ \text{pH} = 4.76 + \log \left( \frac{0.285}{5.55 \times 10^{-2}} \right) \] Fill in the blank box with the calculated pH value after you perform the computation.
Transcribed Image Text:**Calculating pH of a Buffer Solution** A solution contains **0.285 M sodium acetate** and **5.55×10^-2 M acetic acid**. The pH of this solution is **__________**. **Explanation:** To calculate the pH of this buffer solution, you can use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{p}K_\text{a} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] Where, - \( \text{p}K_\text{a} \) is the negative log of the acid dissociation constant of the weak acid. - \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate, in this case). - \([\text{HA}]\) is the concentration of the weak acid (acetic acid, in this case). For acetic acid: \[ \text{p}K_a \approx 4.76 \] \[ \text{pH} = 4.76 + \log \left( \frac{0.285}{5.55 \times 10^{-2}} \right) \] Fill in the blank box with the calculated pH value after you perform the computation.
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