Question

Calculate the pH of a solution that is 0.100 M HONH₂ and 0.100 M HONH₃Cl.

Short answer

The pH of the solution ispH=6.04.

Step-by-step solution

Given Information

The concentration of HONH₂ and HONH₃Clis 0.1 M.

Substituting in the equation

It can be calculated as,

$\begin{array}{l}pH=p{K}_b\left(HON{H}_2\right)+\log \frac{\left[HON{H}_{3}Cl\right]}{\left[HON{H}_2\right]}\\ K_b\left(HON{H}_2\right)=1.1\times {10}^{-8}\\ p{K}_b=-\log \left(K_b\right)+\log \frac{\left[HON{H}_{3}Cl\right]}{\left[HON{H}_2\right]}\\ pH=-\log (1.1\times {10}^{-8})+\log \frac{\left[0.1M\right]}{\left[0.1M\right]}\\ pOH=7.96\\ pH=14-pOH\\ pH=6.04\end{array}$