Back حمض الهيدروفلوريك Arabic Ácidu fluorhídricu AST هیدروفلوئوریک اسید AZB Фторыставадародная кіслата Byelorussian Флуороводородна киселина Bulgarian Fluoridna kiselina BS Àcid fluorhídric Catalan Kyselina fluorovodíková Czech Плавик йӳçекĕ CV Flussyre Danish
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| Names | ||
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| Other names
fluoric acid; fluorhydric acid
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| Identifiers | ||
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3D model (JSmol)
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| EC Number |
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| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | ||
| HF | ||
| Molar mass | not applicable (see hydrogen fluoride) | |
| Appearance | Colorless solution | |
| Density | 1.15 g/mL (for 48% soln.) | |
| Melting point | not applicable (see hydrogen fluoride) | |
| Boiling point | not applicable (see hydrogen fluoride) | |
| Miscible. | ||
| Acidity (pKa) | 3.15 [1] | |
| Hazards | ||
| MSDS | duPont MSDS | |
| EU classification | Very toxic (T+) Corrosive (C) | |
| EU Index | 009-003-00-1 | |
| NFPA 704 |
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| R-phrases | R26/27/28, R35 | |
| S-phrases | (S1/2), S7/9, S26, S36/37, S45 | |
| Flash point | flammable | |
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| Other anions | {{{value}}} | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | ||
| Infobox references | ||
Hydrofluoric acid (HF) is a solution of hydrogen fluoride in water.[2] Its chemical formula is HF. It is a very dangerous acid, being very corrosive and extremely toxic. It can dissolve glass to make hexafluorosilicic acid. If it gets on the skin, it can kill you. It is made by reacting fluorite with sulfuric acid. It is used in the processing of petroleum. It is also used to make various other chemicals containing fluorine, such as teflon (the coating in a frying pan), freon (the cooling agent in an air conditioner), and fluorocarbons (used as propellants in aerosol cans). It is used to clean metals. It is very toxic because it bonds with calcium ions in the body and makes them so they cannot be used. As an acid, it can be deprotonated to produce fluorides, which are also the salts of hydrofluoric acid.
If someone gets hydrofluoric acid on them, medical attention is needed, as just small amounts are very toxic. (Flesh eater)
- ↑ Jolly W.L. (1984) Modern Inorganic Chemistry, McGraw-Hill, p.177
- ↑ Ayotte, P; Hébert, M; Marchand, P (Nov 2005). "Why is hydrofluoric acid a weak acid?". J. Chem. Phys. 123 (18): 184501. Bibcode:2005JChPh.123r4501A. doi:10.1063/1.2090259. PMID 16292908.
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