the relation between the values of osmotic pressure of 0.1M solution of KNO₃(P1) and CH₃COOH(P2) is

1) P1 P2

2) P2 P1

$$\begin{gathered} Osmotic pressure \left(P\right) =i CRT \\ where \\ i= van\text{'}t Hoff factor \\ i =1+(n-1)a \\ a= degree of dissociation \\ n= no. of species into which it dissociates \end{gathered}$$

Since KNO₃ is a strong electrolyte and CH₃COOH is a weak electrolyte
Therefore
i for KNO₃ is > ​i for CH₃COOH

Degree of dissociation i.e a = 1 For KNO3 whereas it is less than 1 (<1) for CH₃COOH.

No. of species dissociated (n) = 2 for both.

therefore

P1> P2