Question

Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF.

Short answer

The pH of the solution ispH=3.37.

Step-by-step solution

Given Information 

The concentration of HF and KF are 0.6 and 1 M.

Substituting in the equation

It can be calculated as,

$\begin{array}{l}pH=p{K}_a\left(HF\right)+\log \frac{\left[KF\right]}{\left[HF\right]}\\ K_a\left(HF\right)=7.2\times {10}^{-4}\\ pH=-\log \left(K_a\right)+\log \frac{\left[KF\right]}{\left[HF\right]}\\ pH=-\log (7.2\times {10}^{-4})+\log \frac{\left[1M\right]}{\left[0.6M\right]}\\ pH=3.143+0.222\\ pH=3.37\end{array}$