Due to impurities, the boiling point (B.P) of a liquid increases. This phenomenon, known as boiling point elevation, is a colligative property observed in solutions. When a solute is added to a solvent, it lowers the vapor pressure of the solution compared to that of the pure solvent. As a result, a higher temperature is required for the vapor pressure of the solution to match the atmospheric pressure, leading to an increase in the boiling point. This effect is proportional to the concentration of the solute particles and is independent of their identity, making it a useful tool in various fields such as chemistry, biology, and industry. Boiling point elevation is utilized in processes like boiling water with salt to cook food faster or in antifreeze solutions for vehicles, where adding solutes to water raises its boiling point, preventing it from boiling off in the engine’s high-temperature environment. Therefore, due to impurities, the boiling point of a liquid increases.