An ethylene glycol solution contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Determine the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)

Colligative properties are physical properties of solutions that depend on the number of solute particles in a given amount of solvent, rather than the identity of the solute. These properties include boiling point elevation and freezing point depression, which are crucial for determining how the presence of a solute like ethylene glycol affects the freezing and boiling points of water.

Freezing point depression is a colligative property that describes the lowering of the freezing point of a solvent when a solute is added. The extent of this depression can be calculated using the formula ΔTf = i * Kf * m, where ΔTf is the change in freezing point, Kf is the freezing point depression constant of the solvent, and m is the molality of the solution.

Boiling point elevation is another colligative property that indicates the increase in the boiling point of a solvent when a solute is dissolved in it. This can be calculated using the formula ΔTb = i * Kb * m, where ΔTb is the change in boiling point, Kb is the boiling point elevation constant of the solvent, and m is the molality of the solution. Understanding this concept is essential for determining how the boiling point of water changes in the presence of ethylene glycol.