If the $K_f$ value of $H_2O$ is $1.86$,what is the value of $\Delta T_f$ for a $0.1 \ m$ solution of a non-volatile solute?

The molal depression constant for water is $1.86\,^{\circ}C/m$. If $342\,g$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $1000\,g$ of water,the freezing point of the solution will be ............. $^{\circ}C$.

Calculate the molar mass of a nonvolatile solute when $1.5 \ g$ of it is dissolved in $90 \ g$ of solvent,decreasing its freezing point by $0.25 \ K$. Given: $K_{f} = 1.2 \ K \ kg \ mol^{-1}$.

$1.00 \ g$ of a non-electrolyte solute dissolved in $50 \ g$ of benzene lowered the freezing point of benzene by $0.40 \ K$. The ${K_f}$ for benzene is $5.12 \ K \ kg \ mol^{-1}$. The molecular mass of the solute will be ............ $g \ mol^{-1}$.

Which of the following will produce the maximum depression in freezing point of its aqueous solution?

In countries nearer to the polar region,the roads are sprinkled with $CaCl_{2}$. This is