Van’t Hoff’s factor for 0.01M aqueous solution acetic acid is 1.04, the pH of that solution is

Given data : It is given to identify  Van’t Hoff’s factor for 0.01M aqueous solution acetic acid is 1.04, the pH of that solution is

Explanation:|
Van't hoff factor = 1.04
$$\begin{gathered} We know, i=l+\alpha (n-1) \\ Here n = 2 \\ So, i = 1+\alpha \\ \alpha = 0.04 \\ \left[H^{+}\right] = C\alpha =0.01 (0.04) = 4 \times {10}^{-4} \\ \mathrm{pH}=-\log \left[{\mathrm{H}}^{+}\right]=-\log \left[4\times {10}^{-4}\right]=4-\log 4 \\ \mathrm{pH}=4-0.6=3.4 \end{gathered}$$

Hence, the correct option (A).3.4