What mass of ethanol, C2H5OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at −10.0°C? Assume the density of water is 1.0 g/mL. Kf of water is 1.86°C/m.

Thus 2473 g of ethanol must be added to 10.0 L of water to give a solution that freezes at −10.0°C

Explanation:

Depression in freezing point is given by:

= Depression in freezing point

i= vant hoff factor  ( for non electrolytes , i= 1)

= freezing point constant for water=

m= molality

weight of solvent (water ) =

weight of solvent (water) =    ( 1L=1000ml)

Thus 2473 g of ethanol must be added to 10.0 L of water to give a solution that freezes at −10.0°C