Here's why:
* Colligative properties: These properties of a solution depend solely on the number of solute particles present, not their specific identity.
* Boiling point elevation: When a solute (like NaCl or CaCl₂) is dissolved in a solvent (like water), it disrupts the solvent's vapor pressure. To reach the boiling point (where vapor pressure equals atmospheric pressure), the solution needs to be heated to a higher temperature than pure water.
Important Note:
* Dissociation: NaCl and CaCl₂ dissociate into ions in water. NaCl forms two ions (Na⁺ and Cl⁻), while CaCl₂ forms three ions (Ca²⁺ and 2Cl⁻). The more ions produced, the greater the effect on boiling point elevation.
* Molality: The extent of boiling point elevation is directly proportional to the molality of the solution (moles of solute per kilogram of solvent). A more concentrated solution will have a higher boiling point.
In summary:
Adding NaCl or CaCl₂ to water will raise its boiling point. The effect is greater with CaCl₂ due to its higher number of ions upon dissociation. The magnitude of the effect depends on the concentration of the solution.
