The depression in freezing point of a $0.01 \, m \, NaCl$ aqueous solution is $0.37^o C$. The depression in freezing point of a $0.02 \, m$ aqueous urea solution is ..... $^o C$.

The freezing point depression of $0.001 \ M$ of $A_x B_y[Fe(CN)_6]$ is $5.58 \times 10^{-3} \ K$. If the oxidation state of $Fe$ is $+2$ and $K_f = 1.86 \ K \ kg \ mol^{-1}$, then the total number of possibilities for different types of $A$ and $B$ cations are

Calculate the osmotic pressure in $atm$ of an aqueous solution of urea at $37\,^oC$,which has a freezing point of $0.52\,^oC$. Assume molality and molarity are numerically equal. $(K_f = 1.86\,^oC\, m^{-1})$

Match List-$I$ with List-$II$.

List-$I$	List-$II$
$A$. van't Hoff factor,$i$	$I$. Cryoscopic constant
$B$. $k_{f}$	$II$. Isotonic solutions
$C$. Solutions with same osmotic pressure	$III$. $\frac{\text{Normal molar mass}}{\text{Abnormal molar mass}}$
$D$. Azeotropes	$IV$. Solutions with same composition of vapour above it

Choose the correct answer from the options given below:

An aqueous solution of a non-volatile solute boils at $100.17^{\circ} C$. The temperature at which this solution will freeze (in $^{\circ} C$) is
$K_{b}(H_2 O) = 0.512^{\circ} C \ kg \ mol^{-1}$,
$K_{f}(H_2 O) = 1.86^{\circ} C \ kg \ mol^{-1}$

When $0.1 \, m$ $CH_3COOH$ is present in a solvent,it shows an elevation in boiling point of $0.75 \, ^oC$. The acid dissociation constant $(K_a)$ will be: (Given: $K_b = 5 \, K \, kg \, mol^{-1}$)