In an experiment, 16.8 g of k2so4 was dissolved in 1.00 kg of water to make a solution. the freezing point of the solution was m
easured to be −0.405°c . calculate the van't hoff factor (i) for this solution. the freezing point of pure water is 0°c (exactly) at 1 atm pressure and the molal freezing-point depression constant for water is 1.86°c/m.
Answer is: V<span>an't Hoff factor (i) for this solution is 2,26. </span>Change in freezing point
from pure solvent to solution: ΔT =i · Kf · m. <span>Kf - molal freezing-point depression constant for water is 1,86°C/m. </span>m - molality, moles of solute per kilogram of solvent. n(K₂SO₄) = 16,8 g ÷ 174,25 g/mol n(K₂SO₄) = 0,096 mol. m(K₂SO₄) = 0,096 mol/kg. ΔT = 0,405°C. i = 0,405 ÷ (1,86 · 0,096) i = 2,26.
