Question

Calculate the pH of the solution using the Henderson-Hasselbalch equation.

• A. \( \text{pH} = \text{p}K_a + \log \left( \frac{\text{[acid]}}{\text{[salt]}} \right) \)
• B. \( \text{pH} = \text{p}K_a - \log \left( \frac{\text{[salt]}}{\text{[acid]}} \right) \)
• C. \( \text{pH} = \text{p}K_a + \log \left( \frac{\text{[salt]}}{\text{[acid]}} \right) \)
• D. None of the above

Hint:

The Henderson-Hasselbalch equation is ideal for calculating the pH of a buffer solution. Make sure to use the concentrations of the salt and acid correctly.

Answer 1

The Correct Option is C

The pH of a buffer solution is calculated using the Henderson-Hasselbalch equation: \[ \text{pH} = \text{p}K_a + \log \left( \frac{\text{[salt]}}{\text{[acid]}} \right) \] Here:
- \( \text{p}K_a \) is the negative logarithm of the acid dissociation constant (\( K_a \)).
- \( \text{[salt]} \) is the concentration of the conjugate base (salt).
- \( \text{[acid]} \) is the concentration of the weak acid.
Conclusion: Use the given concentrations and \( \text{p}K_a \) to calculate the pH.