Introduction:

Boiling point is the temperature at which the vapor pressure of a liquid becomes equal to the pressure exerted on the liquid by its surroundings. It depends on various factors such as intermolecular forces, molecular weight, and concentration of the solute. In this case, we need to compare the boiling point of 0.1 M NaCl and 0.1 M glucose.

Intermolecular forces:

Intermolecular forces are the attractive forces between molecules. The strength of these forces determines the boiling point of a substance. Ionic compounds such as NaCl have strong electrostatic forces between ions, while glucose has weaker intermolecular forces due to its covalent nature. Therefore, NaCl has a higher boiling point than glucose.

Molecular weight:

The molecular weight of a substance is directly proportional to its boiling point. NaCl has a higher molecular weight than glucose, which contributes to its higher boiling point.

Concentration of the solute:

When a solute is dissolved in a solvent, the boiling point of the solvent increases. This is due to the fact that the presence of solute particles interferes with the vaporization process of the solvent. In this case, both NaCl and glucose are dissolved in water. However, NaCl dissociates into two ions (Na+ and Cl-) in water, while glucose does not dissociate. Therefore, the concentration of particles in solution is higher for NaCl than for glucose, resulting in a higher boiling point for NaCl.

Conclusion:

In conclusion, NaCl has a higher boiling point than glucose due to its stronger intermolecular forces, higher molecular weight, and higher concentration of particles in solution.