Colligative properties depend primarily on:

Colligative properties are defined as properties of solutions that depend on the number of solute particles present in a given quantity of solvent, rather than on the identity or type of solute particles. These properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure.

For example, if you dissolve salt in water, the increase in boiling point or the decrease in freezing point is determined by how many particles of salt enter the solution, not the specific nature of the salt itself. Thus, adding more solute particles will have a proportional effect on these properties, which is a hallmark of colligative behavior.

In this context, factors such as the identity or size of the solute particles do not significantly affect colligative properties. Additionally, while temperature does impact the physical state and therefore can influence colligative properties, the essential factor determining colligative behavior is still the number of solute particles in the solution.