Statement I: The boiling point of 0.1 m - urea solution is less than that of 0.1 m - KCl solution.

Statement II: Elevation of boiling point is directly proportional to the number of species present in the solution.

If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.

The correct answer is (1) If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.

Statement I: The boiling point of a 0.1 m urea solution is less than that of a 0.1 m KCl solution.

This statement is correct. The boiling point elevation depends on the concentration of solute particles in a solution. A 0.1 m urea solution has a lower boiling point compared to a 0.1 m KCl solution. This is because urea dissociates into one solute particle, while KCl dissociates into two solute particles when dissolved in water. The presence of more solute particles in the KCl solution leads to a higher boiling point elevation.

Statement II: The elevation of boiling point is directly proportional to the number of species present in the solution.

This statement is also correct. The boiling point elevation is indeed directly proportional to the number of solute particles (species) present in the solution. According to Raoult's law, the change in boiling point (∆Tb) is given by the equation:

\(\Delta T_b = K_bmi\)

where Kb is the molal boiling point elevation constant (a property of the solvent), m is the molality of the solute, and i is the van't Hoff factor representing the number of particles the solute dissociates into in the solution. Therefore, as the number of solute particles increases, the boiling point elevation also increases.

Statement II provides the correct explanation for Statement I because the presence of more solute particles (species) in the KCl solution compared to the urea solution leads to a greater boiling point elevation. Therefore, the correct answer is: If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.