Explanation:
The given data is as follows.
Concentration of acid, [HF] = 2 M
Concentration of salt, [NaF] = 0.472 M
Concentration of base, [NaOH] = 1.00 M
[tex]K_{a}[/tex] = [tex]7.2 \times 10^{-4}[/tex]
So, NaOH being a base will react with the acid that is, HF. And, according to Henderson-Hasselbalch equation we have he following.
pH = [tex]pK_{a} + log\frac{[salt]}{[acid]}[/tex]
Also, we known that [tex]pK_{a} = -log K_{a}[/tex]
so, [tex]pK_{a} = -log 7.2 \times 10^{-4}[/tex]
[tex]pK_{a}[/tex] = 3.1426
Hence, pH = [tex]3.1426 + log\frac{0.472 M}{2 M}[/tex]
pH = 2.5155
Thus, we can conclude that pH of the solution is 2.5155.
