Two solutions, A and B, are prepared by dissolving a non-volatile solute in different solvents. Solution A has a higher boiling point elevation than solution B, even though both solutions have the same molality. Which of the following statements is the MOST likely explanation for this observation?

If molality of the dilute solution is doubled, the value of molal depression constant $({K_f})$ will be

The depression in f.p. is directly proportional to :

Abnormal colligative properties are observed only when the dissolved non-volatile solute in a given dilute solution

The difference between the boiling point and freezing point of an aqueous solution containing sucrose (mol wt. $= {\rm{ }}342{\rm{ }}g\;{\rm{mo}}{{\rm{l}}^{ - 1}}$) in 100 g of water is $105.0^\circ C$. If ${K_f}\;{\rm{and}}\;{K_b}$ of water are 1.86 and $0.51{\rm{ }}K\;{\rm{mo}}{{\rm{l}}^{ - 1}}$ respectively, the weight of sucrose in the solution is about

The order of osmotic pressure of isomolar solution of $BaC{l_2},NaCl\;and\;sucrose$ is

The phenomenon in which cells are shrinked down if placed in hypertonic solution is called :

Which of the following shows maximum depression in freezing point?

Van’thoff factor of $Ca{(N{O_3})_2}$ is

Camphor is used as solvent to determine mol. wt. of non-volatile solute by Rast method because for camphor :

The reverse of fusion is freezing and it is :