Freezing point of urea solution is `-0.6^(@)C`. How much urea (M.W.`=60g/(mol)`) is required to be dissolved in `3kg` of water?
(`K_(f)=1.5^(@)C.kg.mol^(-1)`)

The depression in the freezing point of a sugar solution was found to be 0.402^(@)C . Calculate the osmotic pressure of the sugar solution at 27^(@)C. (K_(f) = 1.86" K kg mol"^(-1)) .

Calculate the freezing point of a solution containing 60 g glucose (Molar mass = 180 g mol^(-1) ) in 250 g of water . ( K_(f) of water = 1.86 K kg mol^(-1) )

Some ethylene glycol HOCH_(2)CH_(2)OH is added to your car cooling system along with 5 kg of water .If the freezing point of water glycol solution is -15.0^(@)C what is the boiling point of the solution ? (k_(b)=0.52 kg mol^(-1) and k_(f)=1.86 kg mol^(-1) for water)

Calculate the boiling point of urea solution when 6 g of urea is dissolved in 200 g of water. ( K_(b) for water = 0·52 K kg mol^(-1) , boiling point of pure water = 373 K, mol.wt. of urea = 60)

The freezing point (.^(@)C) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (molecular weight 329) on 100 g of water (K_(f)=1.86 K kg mol^(-1))

When 36.0 g of a solute having the empirical formula CH_(2)O is dissovled in 1.20 kg of water, the solution freezes at -0.93^(@)C . What is the moleculer formula of the solute ? ( K_(f) = 1.86^(@)C kg mol^(-1) )

Calculate the freezing point depression and boiling point elevation of a solution of 10.0 g of urea (M_(B)=60) in 50.0 g of water at 1 atm . pressure. K_(b) and K_(f) for water 0.52^(@)C m^(-1) and 1.86^(@)C m^(-1) respectively.

The freezing point of a 1.00 m aqueous solution of HF is found to be -1.91^(@)C . The freezing point constant of water, K_(f) , is 1.86 K kg mol^(-1) . The percentage dissociation of HF at this concentration is:-

Calculate the freezing point of a solution containing 0.5 g KCl (Molar mass = 74.5 g/mol) dissolved in 100 g water, assuming KCl to be 92% ionized. K_(f) of water = 1.86 K kg/mol.

On adding 1g arsenic to 80 g benzene, the freezing point of benzene is lowered by 0.213^(@)C . The formula of arsenic molecule is : (Atomic mass of arsenic = 75) ( K_(f) = 5.12 K kg/mol)