Introduction:
Boiling point is the temperature at which a liquid changes its state from liquid to gas, and it depends on the strength of the intermolecular forces present in the liquid. In this context, we will compare the boiling points of 0.1M NaCl and 0.1M glucose solutions.

NaCl:
NaCl is an ionic compound that dissociates in water to form Na+ and Cl- ions. These ions attract each other through electrostatic forces of attraction called ionic bonds. These ionic bonds are very strong, and they require a lot of energy to break them. Therefore, NaCl has a high boiling point of 1413°C.

Glucose:
Glucose is a covalent compound that does not dissociate in water. Instead, it forms hydrogen bonds with water molecules through its -OH groups. These hydrogen bonds are weaker than ionic bonds, and they require less energy to break them. Therefore, glucose has a lower boiling point of 100°C.

Conclusion:
In conclusion, 0.1M NaCl has a higher boiling point than 0.1M glucose due to the stronger ionic bonds present in NaCl. The presence of these strong bonds requires more energy to break them, resulting in a higher boiling point.