Practice: An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.
Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.
Concept #1: Boiling Point Elevation
Boiling Point of the solvent will increase with the addition of a solute.
Example #1: Calculate the boiling point of a 3.71 m aqueous CaBr2 solution.
Practice: An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.
Practice: Pure water boils at 100ºC. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl3, to 615 g water?
Practice: What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15ºC?
Practice: Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7ºC?
