Calculate the freezing point of an aqueous solution containing 10.50 g of `MgBr_2` in 200 g of water. `(Molar mass of MgBr_2=184, for water=1.86kg 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

Calculate the molality of a solution containing 3g glucose dissolved in 30g of water. (molar mass of glucose = 180 )

Calculate the molality of a solution containing 5.3 g of anhydrous Na2CO3 in 400 g water .

Calculate the molality and mole fraction of the solute in aqueous solution containing 3.0 g urea per 250 g of water (molecular mass of urea = 60g).

Calculate the amount of ice that will be separate out on cooling a solution containing 50 g of ethylene glycol in 200 g of water to -9.3^@C . (K_f for water=1.86 Km^-1)

Calculate the molarity of a solution containing 11.7 g of NaCl in 2.0 L solution. (M_(NaCl)=58.5 g mol^-1)

Calculate the freezing point of a one molar aqueous solutoin (density 1.04gL^-1) of KCl. ( K_f of water=1.86Kg mol^-1 , atomic masses of K=39, Cl=35.5)

Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.0 g of water. (K_b for water= 0.512 K kg mol^-1) and molar mass of NaCl= 58.44 g mol^-1

Ethylene glycol (molar mass = 62gmol^-1) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. Would it be advisable to keep this substance in car radiator during summer? (K_f for water=1.86Km^-1 and K_b for water=0.512Km^-1) .