Which of the following statements is true regarding boiling point elevation?

Boiling point elevation is a colligative property, which means it depends on the number of solute particles in a solution rather than the type of solute. The addition of a solute to a solvent decreases the vapor pressure of the solvent due to solute-solvent interactions. This not only requires a higher temperature to reach the boiling point but also results in an overall elevation of the boiling point of the solvent.

When a solute is added, it disrupts the ability of solvent molecules to escape into the vapor phase, which effectively increases the boiling point. This phenomenon can occur with both ionic and molecular compounds, as long as they are dissolved in a solvent.

The other options misrepresent the concept of boiling point elevation. For instance, the notion that only ionic compounds can cause boiling point elevation overlooks the fact that many molecular compounds, particularly those that dissociate into multiple particles or interact significantly with the solvent, can also contribute to this property. Additionally, the concept of boiling point elevation being inversely related to solute concentration is inaccurate; higher solute concentration generally leads to greater boiling point elevation.