Here water is solvent and ethylene glycol is solute.
We know, Depression of freezing point,
ΔT
f = K
f . m
ΔTf=1.86×(1000250)(6262)
= 7.44
We know, freezing point of pure water (here solvent) is 0
oC. Which is represented by
Tf0.
We also know,
ΔTf=Tf0−Tf
where
Tf0 = Freezing point of pure solvent and
Tf = Freezing point of solution
∴ 7.44 = 0 -
Tf
⇒ Tf = -7.44
oC
So, not a single drop of water solution will become ice until temperature reaches -7.44
oC. When temperature decrease more than -7.44
oC then some part of the solution starts becoming ice staring from surface of the solution.
Now let W
l gm of solution still stays in liquid phase when temperature reaches -10
oC.
∴ 10=1.86×(1000Wl)(6262)
W
l = 186 gm
So, The amount of water (in g) separated as ice is
ΔW = (250
− 186) = 64 gm