Final answer:
Supersaturation is the colligative property that is not associated with freezing-point depression, vapor-pressure lowering, or boiling-point elevation. It refers to the state of a solution containing more dissolved material than it normally could, which is different from the other properties determined by the number of solute particles present.
Step-by-step explanation:
The colligative property of a solution that is not among freezing-point depression, vapor-pressure lowering, or boiling-point elevation is supersaturation. Colligative properties depend only on the number of particles in a solution and not on their chemical identity. Freezing point depression is the process where the freezing point of a solvent is lowered by adding a solute, ultimately making the solution freeze at a lower temperature than the pure solvent. Vapor-pressure lowering occurs when a solute is added to a solvent, resulting in a lower vapor pressure than that of the pure solvent. The boiling point elevation is where the boiling point of a solution is higher than the boiling point of the pure solvent. Unlike these colligative properties, supersaturation refers to a state where a solution contains more dissolved material than it could under normal circumstances, which is a result of non-equilibrium conditions and not merely determined by the number of particles.