hydrogen fluoride Property

Density 

1.14 g/cm3 (20 °C)

storage temp. 

Store at +2°C to +8°C.

PH

<7 (H2O, 20°C)

EPA Substance Registry System

Fluorine-18 (13981-56-1)

Safety

WGK Germany 

WGK 2 significantly water endangering

HS Code 

3824 99 96

Hazard and Precautionary Statements (GHS)

Signal word

Danger

hydrogen fluoride Chemical Properties,Usage,Production

Chemical Properties

Colorless, fuming gas or liquid. Very soluble in water. The liquid and gas consist of associated molecules. The vapor density corresponds to hydrogen fluoride only at high temperatures.Nonflammable.

Uses

Catalyst in alkylation, isomerization, condensation, dehydration, and polymerization reactions; fluorinating agent in organic and inorganic reactions; production of fluorine and aluminum fluoride; additive in liquid rocket propellants; refining of uranium

Definition

ChEBI: The radioactive isotope of fluorine with relative atomic mass 18.000938. The longest-lived fluorine radionuclide with half-life of 109.77 min.

Hazard

Toxic by ingestion and inhalation, strong irritant to eyes, skin, and mucous membranes.

Industrial uses

Hydrogen fluoride is the hydride of fluorine and the first member of the family of halogen acids. Anhydrous hydrogen fluoride is a mobile, colorless liquid that fumes strongly in air.
Anhydrous hydrogen fluoride is an extremely powerful acid, exceeded in this respect only by 100% sulfuric acid. Like water, hydrogen fluoride is a liquid of high dielectric constant that undergoes self-ionization and forms conducting solutions with many solutes. Because anhydrous hydrogen fluoride is a superacid, many organic solutes dissolve in it to form stable carbonium ions.
Hydrogen fluoride is a widely used industrial chemical. It was formerly used in the petroleum refining industry for the isomerization of aliphatic hydrocarbons to form more desirable automotive fuels, but this application has been superseded by other methods. The largest industrial use of hydrogen fluoride is in making fluorine- containing refrigerants (Freons, Genetrons).
Another important use of hydrogen fluoride is in the preparation of organic fluorocarbon compounds by the Simons electrochemical process. In this procedure, an organic compound is dissolved in hydrogen fluoride, and an electric current is passed through the solution, whereupon the hydrogen atoms in the organic solute are replaced by fluorine. Hydrogen fluoride is employed in the electrochemical preparation of fluorine and for the preparation of inorganic fluorides. Thus, hydrogen fluoride is used for the conversion of uranium dioxide to uranium tetrafluoride, an intermediate in the preparation of uranium metal and uranium hexafluoride. With the great increase in nuclear energy-produced electricity, this represents an important use of hydrogen fluoride.
Both hydrogen fluoride and hydrofluoric acid cause unusually severe burns; appropriate precautions must be taken to prevent any contact of the skin or eyes with either the liquid or the vapor.