Explanation:

Volatility refers to the tendency of a substance to vaporize or evaporate. In the case of hydrogen fluoride (HF), its volatility is low due to its strong hydrogen bonding.

1. Strong Hydrogen Bonding:
HF molecules are polar, with the hydrogen atom having a partial positive charge and the fluorine atom having a partial negative charge. Due to this polarity, HF molecules can form hydrogen bonds with each other. Hydrogen bonding occurs when the partially positive hydrogen atom of one molecule is attracted to the partially negative atom (in this case, fluorine) of another molecule.

2. Energy Required to Break Hydrogen Bonds:
Hydrogen bonds are relatively strong intermolecular forces compared to other types of intermolecular forces such as London dispersion forces or dipole-dipole interactions. In order for a substance to vaporize, the intermolecular forces between its molecules must be overcome. In the case of HF, a significant amount of energy is required to break the strong hydrogen bonds between its molecules. This results in a higher boiling point and lower volatility compared to substances with weaker intermolecular forces.

3. Low Volatility:
The strong hydrogen bonding in HF leads to a lower volatility because it requires more energy to break the intermolecular bonds and convert the substance from a liquid to a gas. As a result, HF has a lower tendency to vaporize and a higher boiling point compared to substances with weaker intermolecular forces.

Conclusion:
In conclusion, the low volatility of HF is primarily due to its strong hydrogen bonding. The hydrogen bonds between HF molecules require a significant amount of energy to break, resulting in a lower tendency to vaporize and a higher boiling point.