Mass of ethylene glycol (antifreeze) to be added to $18.6 \ kg$ of water to protect the freezing point at $-24^{\circ} C$ is . . . . . . $kg$ (Molar mass in $g \ mol^{-1}$ for ethylene glycol $= 62$,$K_{f}$ of water $= 1.86 \ K \ kg \ mol^{-1}$)

$1.00 \, g$ of a non-electrolyte solute dissolved in $50 \, g$ of benzene lowered the freezing point of benzene by $0.40 \, K$. The freezing point depression constant of benzene is $5.12 \, K \, kg \, mol^{-1}$. Find the molar mass of the solute.

What is the molality of a solution that has a freezing point depression of $3 \ K$ and a freezing point depression constant of $5 \ K \ kg \ mol^{-1}$ (in $m$)?

$2 \ g$ of a non-electrolyte solute (molar mass is $500 \ g \ mol^{-1}$) was dissolved in $57.3 \ g$ of xylene. If the freezing point depression constant $K_f$ of xylene is $4.3 \ K \ kg \ mol^{-1}$,then the depression in freezing point of xylene is.......... (in $K$)

If the freezing point of a $5\%$ (by mass) aqueous solution of cane sugar is $271 \ K$ and the freezing point of pure water is $273.15 \ K$,then the freezing point of a $5\%$ (by mass) aqueous solution of glucose will be .......... $K$.

The freezing point of a $0.01 \ M$ aqueous glucose solution at $1 \ \text{atmosphere}$ is $-0.18 \ ^oC$. To it,an addition of an equal volume of $0.002 \ M$ glucose solution will produce a solution with a freezing point of nearly ........... $^oC$.