A 0.5 percent solution of potassium chloride was found to freeze at ` - 0.24^(@)C`. The percentage dissocation of potassium chloride is______. (Nearest interger)
(Mola depression constant for water is 1.80 kg `mol^(-1)` and molar mass of KCl is `74.6g mol^(-1)`)

2 molal solution of a weak acid HA has a freezing point of 3.885^@C . The degree of dissociation of this acid is _______ xx10^(-3) .(Round off to the Nearest Integer). [Given : Molal depressing constant of water =1.85 K kg mol^(-1) Freezing point of pure water = 0^@C ]

A 0.5% aqueous solution of KCl was found to freeze at -0.24^(@)C . Calculate the Van,t Hoff factor and degree of dissociation of the solute at this concentration. ( K_(f) for water = 1.86 K kg mol ^(-1) )

A solution of urea in water freezes at -0.400^@C . What will be the boiling point of the same solution if the depression and elevation constants for water are 1.86 deg kg mol^(-1) and 0.512 deg kg mol^(-1) respectively?

The freezing point of an aqueous solutions is 272 .93 K . Calculate the molality of the solution if molal depression constant for water is 1.86 Kg mol^(-1)

By dissolving 13.6 g of a substance in 20 g of water, the freezing point decreased by 3.7^(@)C . Calculate the molecular mass of the substance. (Molal depression constant for water = 1.863K kg mol^(-1))

What is osmotic pressure of the aq. Solution of the given solute at 27^(@)C if depression in freezing point is 0.93^(@)C ? Molal depression constant of water is 1.86K mol^(-1) kg ? Assume molality as molarity.