#### Which of the following statements is true about the elevation in boiling point of a solution?Option: 1 It is directly proportional to the number of solute particles in the solution.  Option: 2 It is inversely proportional to the molality of the solution.Option: 3 It is independent of the molar mass of the solute.  Option: 4 It is greater for a volatile solute compared to a non-volatile solute.

The elevation in boiling point of a solution is given by the formula:

$\Delta T_b = i \times K_b \times m$

where $\Delta T_b$ is the elevation in boiling point, i is the van't Hoff factor, $K_b$ is the molal boiling point elevation constant of the solvent, and m is the molality of the solution.

From the formula, we can see that the elevation in boiling point is directly proportional to the van't Hoff factor, which is a measure of the number of solute particles in the solution. This is because the presence of more solute particles leads to a greater reduction in the vapour pressure of the solvent, which in turn leads to a higher boiling point of the solution. Therefore, option a) is the correct answer.

Option b) is incorrect because the elevation in boiling point is directly proportional to the molality of the solution, not inversely proportional to it.

Option c) is incorrect because the elevation in boiling point depends on the molal boiling point elevation constant of the solvent, which in turn depends on the molar mass of the solvent.

Option d) is incorrect because the elevation in boiling point is greater for a non-volatile solute compared to a volatile solute, since a non-volatile solute has a greater effect on reducing the vapour pressure of the solvent.