Question

A buffer solution is prepared such that the concentration of Hf and its salt NAF are respectively 0.1mol and 0.4 molecules. Calculate the PH of the solution given that the Ka of Hf is 6.7 X 10-⁴

Answer 1

The pH of the buffer solution is 3.17.

Step-by-step explanation:

First, we need to calculate the ratio of the concentration of the conjugate base (F-) to the concentration of the weak acid (HF) using the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

Given that the concentration of HF is 0.1 M and the concentration of NaF is 0.4 M, we can substitute these values into the equation:

pH = -log(6.7 x 10-4) + log(0.4/0.1) = 3.17

Therefore, the pH of the solution is 3.17.