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 option 1. If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.

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

Boiling point elevation is a colligative property, meaning it depends on the number of particles in solution, not their identity. Urea \((NH_2CONH_2)\) is a non-electrolyte, so it does not dissociate into ions in solution. In a 0.1 m urea solution, the concentration of particles is 0.1 mol/kg.

\(KCl\) (potassium chloride) is an electrolyte and dissociates into \(K^+\) and \(Cl^-\) ions in solution. Therefore, a 0.1 m \(KCl\) solution produces 0.2 moles of particles per kilogram of solvent (1 mole of \(KCl\) produces 2 particles: \(K^+\) and \(Cl^-\)).

Given the same molality, the \(KCl\) solution has more particles in solution compared to the urea solution. Hence, the boiling point elevation will be higher for the \(KCl\) solution than for the urea solution.

Therefore, the boiling point of the 0.1 m \(KCl\) solution is higher than that of the 0.1 m urea solution. Statement I is correct because the boiling point of 0.1 m urea solution is indeed 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.

This statement is correct in the context of colligative properties. The elevation of the boiling point is directly proportional to the number of particles (species) present in the solution. This is expressed by the formula:

\(\Delta T_b = i \cdot K_b \cdot m\)

where:

\(\Delta T_b\) is the boiling point elevation,

\(i\) is the van't Hoff factor (number of particles the solute dissociates into),

\(K_b\) is the ebullioscopic constant of the solvent,

\(m\) is the molality of the solution.

For urea (which does not dissociate), \(i = 1\). For KCl (which dissociates into two ions), \(i = 2\). Thus, a 0.1 m KCl solution will cause a greater boiling point elevation than a 0.1 m urea solution due to the higher number of particles.

Conclusion:

Statement I is correct because the boiling point of a 0.1 m urea solution is lower compared to that of a 0.1 m KCl solution. Statement II is correct because the elevation of boiling point is indeed directly proportional to the number of species in the solution.

Thus, the correct answer is: If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.