What is the pH of a solution containing 0.4 M of a weak acid with a pKa of 6.0, and 0.2 M of its conjugate base?
Understand the Problem
The question is asking us to calculate the pH of a buffer solution. We can use the Henderson-Hasselbalch equation to solve this problem. The Henderson-Hasselbalch equation is: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.
Answer
The pH of the solution is 5.70.
The pH of the solution is 5.70. This is calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = 6.0 + log(0.2/0.4) = 6.0 + log(0.5) = 6.0 - 0.30 = 5.70.
Answer for screen readers
The pH of the solution is 5.70. This is calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = 6.0 + log(0.2/0.4) = 6.0 + log(0.5) = 6.0 - 0.30 = 5.70.
More Information
The Henderson-Hasselbalch equation is often used to estimate the pH of a buffer solution, which contains a weak acid and its conjugate base.
Tips
Make sure to use the correct concentrations for the acid and conjugate base in the Henderson-Hasselbalch equation. A common mistake is to mix up the concentrations or to forget to take the logarithm of the ratio.
Sources
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