$1\%$ solution of $Ca(NO_3)_2$ has a freezing point:

The freezing point of a solution containing $10 \ mL$ of non-volatile and non-electrolyte liquid $A$ in $500 \ g$ of water is $-0.413^{\circ} C$. If $K_f$ of water is $1.86 \ K \ kg \ mol^{-1}$ and the molecular weight of $A = 60 \ g \ mol^{-1}$, what is the density of the solution in $g \ mL^{-1}$? (Assume $\Delta_{\text{mix}} V = 0$)

The freezing point of a $5\%$ (by mass) aqueous solution of sucrose is $271 \, K$ and the freezing point of pure water is $273.15 \, K$. The freezing point of a $5\%$ (by mass) aqueous solution of glucose is .......... $K$.

$K_f$ for water is $1.86 \, K \, kg \, mol^{-1}$. If your automobile radiator holds $1.0 \, kg$ of water,how many $gm$ of ethylene glycol $(C_2H_6O_2)$ must you add to lower the freezing point of the solution to $-2.8 \, ^oC$?

The freezing point of a solution prepared from $1.25 \ g$ of a non-electrolyte and $20 \ g$ of water is $271.9 \ K$. If the molar depression constant is $1.86 \ K \ kg \ mol^{-1}$,then the molar mass of the solute will be:

What will be the freezing point of a $1\%$ aqueous solution of $Ca(NO_3)_2$?