60g of urea is dissolved in 1100g solution. To keep `DeltaT//K_(f)" as "1" mol"//kg`, water separated in the form of ice is

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

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)

Find the K_(f) if 6 g of urea is dissolved in 0.1 dm^(3) of water and it corresponds to 0.15 ""^(@) C in Delta T_f ( Molecular weight of urea = 60 g mol ^(-1) )

3g urea is dissolved in 100ml water. Find the freezing point of solution ( K_f = 1.86k kg mol_(-1) )

Find the K_(f) if 6 g of urea is dissolved in 0.1 dm^(3) of water and it corresponds to 0.15 ""^(@) C in Delta T ( Molacular weight of urea = 60 g mol ^(-1) )

A solution containing 62g ethylene glycol in 276g water is cooled to -10^(@)C . If K_(f) for water is 1.86 kg mol^(-1) , the amount of water (in moles) separated as ice is ________.