An aqueous solution of urea has a freezing point of `-0.515^@C`. Predict the osmotic pressure (in atm) of the same solution at `37^@C`. `k_f = 1.86 k kg (mol)^(-1)`

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit atm K^-1 mol^-1 .

What would be the osmotic pressure of a 0.02 molar aqueous solution of urea at 27^@C .

6gm of urea and 9gm of glucose are dissolved in 1 Litre aqueous solution. Calculate the osmotic pressure of the solution at 300K.

A 0.2 molal aqueous solution of weak acid HX is 20% ionized. The freezing point of solution is ( K_f =1.86 )

For a dilute solution containing 2.5 g of a non- volatile non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm pressure is 2^@C Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take k_b = 0.76 K kg mol^(-1)) .

A .001 molal solution of a complex [MA_8] in water has the freezing point of -0.0054^@C . Assuming 100% ionization of the complex salt and K,for H_2O 1.86Km^-1 , write the correct representation for the complex

KBr undergoes 80% dissociation in its 0.5(M) aqueous solution. Calculate osmotic pressure of the solution at 27^(@)C temperature.

The osmotic pressures of 0.1M glucose and 0.1M NaCl solutions are __________ .

KBr is 80% dissociated in aqueous solution. The freezing point of a 0.5 molal solution is K_f =1.86 K kg mol^-1