Hydrogen fluoride

Hydrogen fluoride is a hydrofluoric acid, are strongly corrosive.

Structure of HF

Liquid HF also consists of chains of HF molecules, but the chains are shorter, consisting on average of only five or six molecules.^[2] The higher boiling point of HF relative to analogous species, such as HCl, is attributed to hydrogen bonding between HF molecules, as indicated by the existence of chains even in the liquid state.

Acidity

Dilute hydrogen fluoride solution is a weak acid due to the extensive intermolecular H-bonds present. The molecules tend to remain in chains rather than ionize to form H⁺ and F⁻ ions.

But in a more concentrated hydrogen fluoride solution, F⁻ ions forms a soluble [HF₂]⁻(aq) complex with HF molecules. HF molecules remaining ionize to compensate the loss of F⁻ ions. More H⁺ ions are thus formed, making concentrated HF an effectively strong acid.

Anhydrous hydrogen fluoride is an extremely strong acid (sulfuric acid (H₀ ~ -12).

Uses

HF is used for fluorinating isotopes.

Hydrogen fluoride can be found in consumer products for removing sulfuric acid:

CaF₂ + H₂SO₄ → CaSO₄ + 2 HF

The vapors from this reaction are a mixture of hydrogen fluoride, sulfuric acid, and a few minor byproducts, from which hydrogen fluoride can be isolated by distillation.

Health effects

Main article: Hydrofluoric acid

Upon contact with moisture, including tissue, hydrogen fluoride immediately converts to hydrofluoric acid, which is highly corrosive and toxic.

References

1. ^ Johnson, M. W.; Sándor, E.; Arzi, E. "The Crystal Structure of Deuterium Fluoride" Acta Crystallographica 1975, B31, pages 1998-2003.doi:10.1107/S0567740875006711
2. ^ Sylvia E. McLain, S. E.; Benmore, C. J.; Siewenie, J. E.; Urquidi, J.; Turner, J. F. C. "On the Structure of Liquid Hydrogen Fluoride" Angewandte Chemie, International Edition, 2004, volume 43, pages 1952-55 doi:10.1002/anie.200353289