Introduction: Boiling point is the temperature at which a liquid turns into a gas. It depends on the strength of the intermolecular forces between the particles in the liquid. In this context, we will compare the boiling points of 0.1 M NaCl and 0.1 M glucose.

Intermolecular forces: Intermolecular forces are the attractive forces between the molecules of a substance. They determine the physical properties of the substance, including its boiling point. There are three types of intermolecular forces: London dispersion forces, dipole-dipole forces, and hydrogen bonding.

NaCl: NaCl is an ionic compound. Its particles are ions, which are held together by strong electrostatic forces of attraction. These forces are much stronger than the intermolecular forces between the particles in a molecular compound like glucose. As a result, NaCl has a much higher boiling point than glucose.

Glucose: Glucose is a molecular compound. Its particles are molecules, which are held together by much weaker intermolecular forces than the electrostatic forces between ions in an ionic compound like NaCl. Glucose molecules have dipole-dipole forces and hydrogen bonding, but they are not as strong as the forces between ions in NaCl. Therefore, glucose has a lower boiling point than NaCl.

Conclusion: In conclusion, the boiling point of a substance depends on the strength of the intermolecular forces between its particles. NaCl has a higher boiling point than glucose because it is an ionic compound with strong electrostatic forces between its particles, whereas glucose is a molecular compound with weaker intermolecular forces.