Hydrogen fluoride
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| Chemical formula | HF |
|---|---|
| OTP appearance | ultra-pale yellow gas |
| Molar Mass(g/mol) | 20.01 |
| Density(g/cc) | .00115 |
| Melting Point(°C) | -83.6 |
| Boiling Point(°C) | 19.5 |
| NFPA 704 |  0
4
1
|
Uses
Primary
- Key fluorine ion source
- Feedstock for industrial chemical hydrofluoric acid
- Feedstock for sodium aluminum hexafluoride, essential for aluminum production
Natural occurrence
- Hydrogen fluoride does not occur naturally.
Hazards
This is a highly dangerous substance.
- Pure gaseous hydrogen fluoride is toxic and corrosive. It is very dangerous.
- Aqueous hydrogen fluoride (hydrofluoric acid) is also toxic and corrosive, but less so.
Treatment
- Intravenous (IV) magnesium sulfate and intra/trans-dermal calcium gluconate are sometimes used after cutaneous exposure to hydrofluoric acid[1]
Production
Synthesis
Combine and heat sulfuric acid with fluorite or fluorapatite, producing hydrofluoric acid.
- CaF2 + H2SO4 → CaSO4 + 2 HF
- 2 Ca5(PO4)3F + 7 H2SO4 + 3 H2O → 7 CaSO4 + Ca3(PO4)2 + H3PO4 + 2 HF
Storage
Hydrogen fluoride must be stored in polyethylene (LDPE, HDPE, etc) or fluorinated versions thereof (PTFE/teflon). Container-in-container storage is preferred. Magnesium sulfate can be used to absorb spills.
Disposal
- First dissolve in water, producing more manageable hydrofluoric acid. Then dispose of that.
See Also
References
- ↑ Cox, RD; Osgood, KA (1994) "Evaluation of intravenous magnesium sulfate for the treatment of hydrofluoric acid burns".
J Clin Toxicol. 32(2); pp123-36.