Calculate the freezing point and boiling point of a solution containing 8.15 g of ethylene glycol (C2H6O2) in 96.3 mL of ethanol. Ethanol has a density of 0.789 g/cm3. You may want to reference (Pages 558 - 568) Section 13.6 while completing this problem.

The freezing point of solution is -117.54°C and the boiling point of solution is 80.48°C

Explanation:

To calculate the mass of ethanol, we use the equation:

Density of ethanol = 0.789 g/mL

Volume of ethanol = 96.3 mL

Putting values in above equation, we get:

Depression in freezing point is defined as the difference in the freezing point of pure solution and freezing point of solution.

The equation used to calculate depression in freezing point follows:

To calculate the depression in freezing point, we use the equation:

Or,

where,

Freezing point of pure solution = -114.1 °C

i = Vant hoff factor = 1 (For non-electrolytes)

= molal freezing point elevation constant = 1.99°C/m

= Given mass of solute (ethylene glycol) = 8.15 g

= Molar mass of solute (ethylene glycol) = 62 g/mol

= Mass of solvent (ethanol) = 75.98 g

Putting values in above equation, we get:

Hence, the freezing point of solution is -117.54°C

Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.

The equation used to calculate elevation in boiling point follows:

To calculate the elevation in boiling point, we use the equation:

Or,

where,

Boiling point of pure solution = 78.4°C

i = Vant hoff factor = 1 (For non-electrolytes)

= molal boiling point elevation constant = 1.20°C/m.g

= Given mass of solute (ethylene glycol) = 8.15 g

= Molar mass of solute (ethylene glycol) = 62  g/mol

= Mass of solvent (ethanol) = 75.98 g

Putting values in above equation, we get:

Hence, the boiling point of solution is 80.48°C

56 moles of   lieter in chemistry

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