Hydrofluoric acid

Hydrofluoric acid
Names
	Other names fluoric acid; fluorhydric acid
Identifiers
CAS Number	7664-39-3 ;
3D model (JSmol)	Interactive image;
EC Number	231-634-8;
RTECS number	MW7875000;
CompTox Dashboard (EPA)	DTXSID1049641 ;
	SMILES F;
Properties
Chemical formula	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)
Solubility in water	Miscible.
Acidity (pKa)	3.15
Hazards
MSDS	duPont MSDS
EU classification	Very toxic (T+); Corrosive (C)
EU Index	009-003-00-1
	0 4 2 COR
R-phrases	R26/27/28, R35
S-phrases	(S1/2), S7/9, S26, S36/37, S45
Flash point	flammable
Related compounds
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)

Related pages

References

↑ 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.{{cite journal}}: CS1 maint: multiple names: authors list (link)

Other websites

International Chemical Safety Card 0283
National Pollutant Inventory - Fluoride and compounds fact sheet Archived 2006-01-16 at the Wayback Machine
NIOSH Pocket Guide to Chemical Hazards
Hydrofluoric Acid Burn, The New England Journal of Medicine Acid burn case study

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[1] Jolly W.L. (1984) Modern Inorganic Chemistry, McGraw-Hill, p.177

[2] 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.{{cite journal}}: CS1 maint: multiple names: authors list (link)

[2]

[1]