|Hydrogen Iodide||Hydrogen Selenide||Hydrogen Sulfide||Hydrogen Telluride||Hydrogen Tetracarbonylferrate(II)|
|Jmol-3D images||Image 1|
|Molar mass||20.01 g mol−1|
|Density||1.15 g/L, gas (25 °C)
0.99 g/mL, liquid (19.5 °C)
|Melting point||−83.6 °C; −118.5 °F; 189.6 K|
|Boiling point||19.5 °C; 67.1 °F; 292.6 K|
|Solubility in water||miscible|
|Refractive index (nD)||1.00001|
|Dipole moment||1.86 D|
|8.687 J/g K (gas)|
|Std enthalpy of
|−13.66 kJ/g (gas)
−14.99 kJ/g (liquid)
|Other anions||Hydrogen chloride
|Other cations||Sodium fluoride|
|Related compounds||Hydrofluoric acid|
(what is: / ?)|
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Hydrogen fluoride is a chemical compound with the formula HF. This colorless gas is the principal industrial source of fluorine, often in the aqueous form as hydrofluoric acid, and thus is the precursor to many important compounds including pharmaceuticals and polymers (e.g. Teflon). HF is widely used in the petrochemical industry and is a component of many superacids. Hydrogen fluoride boils just below room temperature whereas the other hydrogen halides condense at much lower temperatures. Unlike the other hydrogen halides, HF is lighter than air and diffuses relatively quickly through porous substances.
Hydrogen fluoride is a highly dangerous gas, forming corrosive and penetrating hydrofluoric acid upon contact with tissue. The gas can also cause blindness by rapid destruction of the corneas.
French chemist Edmond Frémy (1814–1894) is credited with discovering anhydrous hydrogen fluoride while trying to isolate fluorine, although Carl Wilhelm Scheele prepared hydrofluoric acid in large quantities in 1771, and this acid was known about in the glass industry before then.