What will be the osmotic pressure in $atm$ of a $0.2 \ M$ $K_4[Fe(CN)_6]$ solution at $27 \ ^oC$?

Calculate the approximate $\Delta T_b$ (in $K$) for $0.001 \ m$ $KCl$ solution, if its van't-Hoff factor is $1.98$ [$K_b$ of water is $0.52 \ K \ kg \ mol^{-1}$].

Calculate the molality of an aqueous solution of an electrolyte that freezes at $-0.93 \text{ }^\circ\text{C}$. Given that $K_f$ for water is $1.86 \text{ K kg mol}^{-1}$ and the van't Hoff factor $(i)$ is $1.25$. (Freezing point of pure water $= 0 \text{ }^\circ\text{C}$) (in $\text{ m}$)

The freezing point of an equimolal aqueous solution will be highest for:

The osmotic pressure of equimolar solutions of urea,$BaCl_2$,and $AlCl_3$ will be in the order:

The boiling point of $0.01 \, M$ aqueous solutions of sucrose,$NaCl$ and $CaCl_2$ would be