The relationship between the value of Osmotic pressure $\left(\pi \right)$ of the solution obtained by dissolving $6 \mathrm{g}.{\mathrm{L}}^{-1}$ of acetic acid $\left({\pi }_1\right)$ and$7.45 \mathrm{g}.{\mathrm{L}}^{-1}$ of KCl $\left({\pi }_2\right)$ is

Osmotic pressure, ${\displaystyle \pi =CRT}$
${\displaystyle n_{C{H}_{3}COOH}=\frac{6}{60}=0.1n_{KCI}=\frac{7.45}{74.5}=0.1}$
Here molar concentrations of both solutions are the same. Since ${\displaystyle KCI}$ ionizes more than ${\displaystyle C{H}_{3}COOH}$ , the number of particles in ${\displaystyle KCI}$ solution increases.

Therefore, option A is the right answer