Based on acetic acid $\left(K_{\mathrm{a}}^{\circ }=1.8\times {10}^{-5}\right)$ solution,

The concentration of ${\mathrm{H}}^{+}$ in 0.05 M acetic acid solution is

$\left[{\mathrm{H}}^{+}\right]=c\alpha =\left(0.05\mathrm{M}\right)\left(0.019\right)=9.5\times {10}^{-4}\mathrm{M}$

The concentration of ${\mathrm{H}}^{+}$ in 0.05 M acetic acid solution is $9.5\times {10}^{-4}\mathrm{M}$

Since pH is the logarithm of the reciprocal of the hydrogen ion concentration in grime moles per liter, it is a more practical way to represent hydrogen ion concentration.