* Colligative Properties: The change in boiling point is a colligative property, meaning it depends on the number of solute particles dissolved in the solvent, not their specific identity.
* Dissociation: When CaCl2 dissolves in water, it dissociates into three ions: one Ca²⁺ ion and two Cl⁻ ions. This means that one molecule of CaCl2 produces three particles in solution.
* Boiling Point Elevation: The presence of these dissolved ions disrupts the equilibrium between liquid water molecules and water vapor. It becomes harder for water molecules to escape into the vapor phase, requiring a higher temperature to reach the boiling point.
In summary: The increased concentration of particles (ions) in the water due to the dissolved CaCl2 raises the boiling point.
Important Note: The magnitude of the boiling point elevation is directly proportional to the molality of the solution (moles of solute per kilogram of solvent). So, a higher concentration of CaCl2 will lead to a greater increase in the boiling point.
