45g of ethylene glycol (`C_2H_6O_2`) is mixed with 600g of water. Calculate
The freezing point depression

45g of ethylene glycol (C_2H_6O_2) is mixed with 600 g of water. Calculate: the freezing point of the solution. (K_f for water=1.86K kg mol^-1) .

An antifreeze solution is prepared fro, 222.6g of ethylene glycol, C_2H_4(OH)_2 and 200g of water. Calculate the molality of the solution . If the density of the solution is 1.072g mL^-1 , then what shall be the molarity of the solution?

31 gm of ethylene glycol (C_2H_6O_2) is mixed with 500 gm of solvent. (K_f = 2 K kg "mol"^(-1)) . What is the freezing point of the solution in K ? (freezing point of solvent = 273K)

K_f for water is 1.86K kg mol^-1 . If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C_2H_6O_2) must you add to get the freezing point of the solution lowered to 0.8^@C ?

How many grams of ethylene glycol (molar mass = 62) should be added to 10 kg of water, so that the resulting solution freezes at -10^(@)C ( K_(f) for water = 1.86 K "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) .

19.5 g of CH_2FCOOH is dissolved in 500 g of water. The depression in the freezing point of water observed is 1.0° C. Calculate the van’t Hoff factor and dissociation constant of fluoroacetic acid.