Final answer:
The true statement about a solute dissolved in a solvent is that the solute raises the boiling point of the solvent. This is known as boiling point elevation. Additionally, the solute also lowers the freezing point of the solvent, a phenomenon called freezing point depression.
Step-by-step explanation:
When a solute is dissolved in a solvent, it alters the physical properties of the solvent. One of the key effects is boiling point elevation, where the boiling point of a solution is higher than that of the pure solvent. This occurs because the solute particles reduce the vapor pressure of the solvent, necessitating a higher temperature to reach boiling point. For example, adding salt to water will increase the boiling point of the solution.
Conversely, the process of freezing point depression is observed when a solute is added to a solvent. Here, the freezing point of the solution is lower than that of the pure solvent. The interactions between the solute and solvent particles inhibit the formation of a solid phase at the normal freezing temperature of the solvent, thus requiring a lower temperature to achieve freezing. Salting roads in winter to prevent ice formation is a practical application of this phenomenon.
Both boiling point elevation and freezing point depression are examples of colligative properties. These properties depend on the number of solute particles present in the solution rather than the specific type of solute molecules.