Answer:
Vapor pressure of solution = 17.02 Torr
T° of boiling point for the solution is 100.79°C
T° of freezing point for the solution is -2.9°C
Explanation:
Let's state the colligative properties with their formulas
- <u>Vapor pressure lowering</u>
ΔP = P° . Xm . i
- <u>Boiling point elevation</u>
ΔT = Kb . m . i
-<u> Freezing point depressión</u>
ΔT = Kf . m . i
ΔP = Vapor pressure pure solvent (P°) - Vapor pressure solution
ΔT = T° boling solution - T° boiling pure solvent
ΔT = T° freezing pure solvent - T° freezing solution
i represents the Van't Hoff factor (ions dissolved in the solution). If we assume that the solute is non-volatile and the solution is ideal i = 1
Kf and Kb are cryoscopic and ebulloscopic constant, they are specific to each solvent.
Vapor pressure works with mole fraction (Xm) and the only data we have is molality, so we consider 1.56 moles of solute and 1000 g of solvent mass.
Moles of solvent → solvent mass / molar mass of solvent
Moles of solvent → 1000 g / 18 g/mol = 55.5 moles
Mole fraction is moles of solute / Total moles (mol st + mol sv)
Mole fraction: 1.56 / (1.56 + 55.5) = 0.027
- Vapor pressure lowering
ΔP = P° . Xm . i
17.5 Torr - Vapor pressure of solution = 17.5 Torr . 0.027 . 1
Vapor pressure of solution = - (17.5 Torr . 0.027 . 1 - 17.5 Torr)
Vapor pressure of solution = 17.02 Torr
- Boiling point elevation
ΔT = Kb . m . i
T° boiling solution - 100° = 0.512 °C/ m . 1.56 m . 1
T°boiling solution = 0.512 °C/ m . 1.56 m . 1 + 100°C
T°boiling solution = 100.79°C
- Freezing point depression
ΔT = Kf . m . i
0°C - T° freezing solution = 1.86 °C/m . 1.56 m . 1
T° freezing solution = - (1.86 °C/m . 1.56 m)
T° freezing solution = -2.9°C
