An aqueous solution of urea has freezing point of `-0.52^(@)C`. If molarity and molality are same and `K'_(f)` for `H_(2)O = 1.86 K "molality"^(-1)` the osmotic pressure of solution would be:

An aqueous solution of urea has a freezing point of -0.52^(@)C . Assuming molarity same for the solution, the osmotic pressure of solution at 37^(@)C would be : (K_(f) of H_(2)O=1.86 K molarity .^(-1) )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

0.15 molal solution of NaCI has freezing point -0.52 ^(@)C Calculate van't Hoff factor . (K_(f) = 1.86 K kg mol^(-1) )

The freezing poing of an aqueous solution of a non-electrolyte is -0.14^(@)C . The molarity of this solution is [K_(f) (H_(2)O) = 1.86 kg mol^(-1)] :

0.1 mole of sugar is dissolved in 250 g of water. The freezing point of the solution is [K_(f) "for" H_(2)O = 1.86^(@)C "molal"^(-1)]