A 0.1m solution of `K_2SO_4` in water has freezing point of `-4.3^@C`. What is the value of van't Hoff factor if Kf for water is `1.86 K kgmol^(-1)`.

0.2m aqueous solution of KCI freezes at -0.680^@C . Calcuate van't Hoff factor and osmotic pressure of solution at 0^@C . (K_f=1.86 K kg mol^(-1) .

The freezing point of 0.05 molal solution of non- electrolyte in water is _____. (K_(f) = 1.86 ^(@)Ckg mol ^(-1))

What is the molality of solution of a certain solute in a solvent .If there is a freezing point depression of 0.184 ""^(@) C and if the freezing point constant is 18.4 K kg mol^(-1) ?

The boiling point of 0.1 molal K_4 [Fe(CN)_6 ] solution will be (given K_b for water = 0.52 k kg mol^(-1))

The observed depression in the freezing print of water for a particular solution is 0.087 K. Calculate the molality of the solution if molal depression constant for water is 1.86 K kg. mol^(-1) .

Assuming complete dissociation, calculate the molality of an aqueous solution of KBr whose freezing point is -2.95^@C . K, for water is 1.86 K kg mol^(-1) .