Calculate the freezing point of a solution that contains 5.42 g of glucose, a non-electrolyte, dissolved in 102 g of water.
Lets calculate molality first
Molar mass of C6H12O6,
MM = 6*MM(C) + 12*MM(H) + 6*MM(O)
= 6*12.01 + 12*1.008 + 6*16.0
= 180.156 g/mol
mass(C6H12O6)= 5.42 g
use:
number of mol of C6H12O6,
n = mass of C6H12O6/molar mass of C6H12O6
=(5.42 g)/(180.156 g/mol)
= 3.009*10^-2 mol
m(solvent)= 102 g
= 0.102 kg
use:
Molality,
m = number of mol / mass of solvent in Kg
=(3.009*10^-2 mol)/(0.102 Kg)
= 0.295 molal
lets now calculate ΔTf
ΔTf = Kf*m
= 1.86*0.295
= 0.5486 oC
This is decrease in freezing point
freezing point of pure liquid = 0.0 oC
So, new freezing point = 0 - 0.5486
= -0.5486 oC
Answer: -0.549 oC
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