`0.1` moles of `K_(4)[Fe(CN)_(6)]` is dissolved in 500 gm water . The freezing point of solution is :
[Given : Molal depression constant for water = 1.86 K-kg/mole]

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)]

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)]

0.534 g of solute is dissolved in 15g of water then freezing point temperature changes from 0^(@)C to -1.57^(@)C . Molal depression constant of water, k_(f)=1.85 K kg mol^(-1) . Find out : (i) Molal concentration (ii) Molecular mass of solute.

31 g of ethylene glycol (C_2H_6O_2) is dissolved in 600g of water. The freezing point depression of the solution is (K_f for water is 1.86 K Kg mol^-1)

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] in 100 g of water. (K_f=1.86 K kg mol^-1) is

5 g of a substance when dissolved in 50 g water lowers the freezing by 1.2^(@)C . Calculate molecular wt. of the substance if molal depression constant of water is 1.86 K kg mol^-1 .

The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water is (Molal depression constant of water=1.86Kkg/mol)

The observed depression in freezing point of water for a particular solution in 0.093^(@) k calculate the concentration of the solution in molality Given that molal depression constant for water is 1.86 K KG mol ^(-1 )