Microscopic explanation of colligative properties from the entropy related viewpoint

In the chapter 28.6 of book “Concepts in thermal physics “(2nd edition) written by Stephen J. Blundell, there is a sentence says “Adding a small quantity of solute to a solvent increases the entropy of the solvent because the solute atoms are randomly located in the solvent. This means that there is a weaker tendency to form a gas (which would increase the solvent’s entropy) because the entropy of the solvent has been increased anyway. This results in an elevation of the boiling point. Similarly, this additional entropy opposes the tendency to freeze and the freezing point is depressed.”

However, it looks to me that if there is a tendency to form a gas, then raising smaller temperature than the pure substance situation is able to trigger the phase change, which means the boiling point is lowered. Which part is wrong in my thinking?