The freezing point of one molal $NaCl$ solution,assuming $NaCl$ to be $100\%$ dissociated in water,is ............ $^oC$. (molal depression constant $= 1.86$)

The molal elevation constant of water is $0.51 \ K \, kg \, mol^{-1}$. The boiling point of $0.1 \ m$ aqueous $NaCl$ solution is nearly .......... $^oC$.

The freezing point depression constant for water is $1.86 \, ^oC \, kg \, mol^{-1}.$ If $5.00 \, g$ of $Na_2SO_4$ is dissolved in $45.0 \, g$ of $H_2O,$ the freezing point is lowered by $3.82 \, ^oC.$ Calculate the van't Hoff factor for $Na_2SO_4.$

Osmotic pressure of a $4.44\%$ solution of anhydrous $CaCl_2$ was found to be $16.42 \ atm$ at $27 \, ^\circ C$. What is the degree of dissociation of $CaCl_2$ in $\%$?

Consider the following solutions at $25\,^oC$:
$(I)$ $0.01\, M$ aqueous solution of glucose
$(II)$ $0.01\, M$ aqueous solution of $KNO_3$
$(III)$ $0.01\, M$ solution of acetic acid in benzene
Select the correct statement.

Which of the following has the lowest freezing point?