When acetic acid is dissolved in benzene,its molecular mass:

$0.004 \ M \ Na_2SO_4$ is isotonic with $0.01 \ M$ glucose. The degree of dissociation of $Na_2SO_4$ is ........... $\%$.

The observed osmotic pressure of a solution of benzoic acid in benzene is less than its expected value because:

$75.2 \ g$ of $C_6H_5OH$ (phenol) is dissolved in a solvent of $K_f = 14 \ K \ kg \ mol^{-1}$. If the depression in freezing point is $7 \ K$,then find the percentage of phenol that dimerises. (in $\%$)

$1.2 \ mL$ of acetic acid having density $1.06 \ g \ cm^{-3}$ is dissolved in $1 \ L$ of water. The depression in freezing point observed for this concentration of acid was $0.041^{\circ} C$. The van't Hoff factor of the acid is $(K_f \text{ of water } = 1.86 \ K \ kg \ mol^{-1})$

If $0.15 \ m$ aqueous solution of $KCl$ freezes at $-0.51^{\circ} C$,calculate the van't Hoff factor of $KCl$ (cryoscopic constant of water is $1.86 \ K \ kg \ mol^{-1}$).