An aqueous solution of urea (molar mass $= 60 \ g \ mol^{-1}$) boils at $100.18^o C$ at atmospheric pressure. If $K_f = 1.86 \ K \ kg \ mol^{-1}$ and $K_b = 0.512 \ K \ kg \ mol^{-1}$ for water,then the freezing point of the solution is equal to ..... $^o C$.

An aqueous solution of a non-volatile solute boils at $100.15\,^{\circ}C$. If the solution is diluted with an equal volume of water,the freezing point of the resulting solution will be ...... $^{\circ}C$. (Given: $K_b = 0.512\,K\,kg\,mol^{-1}$ and $K_f = 1.86\,K\,kg\,mol^{-1}$ for water)

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
$K_{b}(H_2 O) = 0.512^{\circ} C \ kg \ mol^{-1}$,
$K_{f}(H_2 O) = 1.86^{\circ} C \ kg \ mol^{-1}$

At $35^{\circ} C$,the vapour pressure of $CS_{2}$ is $512 \; mm \; Hg$ and that of acetone is $344 \; mm \; Hg$. $A$ solution of $CS_{2}$ in acetone has a total vapour pressure of $600 \; mm \; Hg$. The false statement amongst the following is

$A$ non-volatile, non-electrolyte solid solute when dissolved in $40 \text{ g}$ of a solvent, the vapour pressure of the solvent decreased from $760 \text{ mm Hg}$ to $750 \text{ mm Hg}$. If the same solution boils at $320 \text{ K}$, then the number of moles of the solvent present in the solution is . . . . . . . (Nearest integer) [Given: boiling point of the pure solvent = $319.5 \text{ K}$, $K_b$ of the solvent = $0.3 \text{ K kg mol}^{-1}$]

When a solute is added to a solvent,the freezing point of the solution decreases to $1.86 \ K$. What is the value of $\Delta T_b$? $[K_f = 1.86, K_b = 0.512]$