1 mole of NaCl dissociates into 2 particles (1 Na⁺ and 1 Cl⁻), so there are 2 particles in solution.

The freezing point of a solvent decreases when a solute is added, a phenomenon known as freezing point depression.

The boiling point elevation is calculated using the formula ΔT_b = i * K_b * m, where i is the van 't Hoff factor, K_b is the ebullioscopic constant, and m is the molality.

Colligative properties depend on the concentration of solute particles in a solution, not their identity.

The addition of a solute decreases the vapor pressure of the solvent, which requires a higher temperature to reach the boiling point.

The van 't Hoff factor (i) for NaCl is 2 because it dissociates into two ions: Na+ and Cl-.

Colligative properties depend primarily on the number of solute particles, not the nature of the solute.

Density is not a colligative property; it does not depend on the number of solute particles.

0.1 m CaCl2 produces three particles (Ca2+ and 2 Cl-), leading to the highest boiling point elevation among the options.