Ammonium hydrogen fluoride
Ammonium acid fluoride
|3D model (Jmol)||Interactive image
|Molar mass||57.04 g·mol−1|
|Density||1.50 g cm−3|
|Melting point||126 °C (259 °F; 399 K)(decomposes)|
|Boiling point||240 °C (464 °F; 513 K)|
|63g/100ml 20 °C|
|Solubility in alcohol||slightly soluble|
Refractive index (nD)
|Cubic, related to the CsCl structure|
|[NH4]+ cation: tetrahedral
[HF2]− anion: linear
|P280, P301+310, P305+351+338, P310|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Ammonium hydrogen fluoride is the inorganic compound with the formula NH4HF2 or NH4F·HF. It is produced from ammonia and hydrogen fluoride. This colourless salt is a glass-etchant and an intermediate in a once-contemplated route to hydrofluoric acid.
Ammonium bifluoride, as its name indicates, contains an ammonium cation (NH4+) and a bifluoride, or hydrogen(difluoride), anion (HF2−). The centrosymmetric triatomic bifluoride anion features the strongest known hydrogen bond, with a F−H length of 114 pm. and a bond energy greater than 155 kJ mol−1.
In solid [NH4][HF2], each ammonium cation is surrounded by four fluoride centers in a tetrahedron, with hydrogen-fluorine hydrogen bonds present between the hydrogen atoms of the ammonium ion and the fluorine atoms. Solutions contain tetrahedral [NH4]+ cations and linear [HF2]− anions.
Production and applications
Ammonium bifluoride is a component of some etchants. It attacks silica component of glass:
Potassium bifluoride is a related more commonly used etchant.
Ammonium bifluoride has been considered as an intermediate in the production of hydrofluoric acid from hexafluorosilicic acid. Thus, hexafluorosilicic acid is hydrolyzed to give ammonium fluoride, which thermally decomposes to give the bifluoride:
- H2SiF6 + 6 NH3 + 2 H2O → SiO2 + 6 NH4F
- 2 NH4F → NH3 + [NH4]HF2
The resulting ammonium bifluoride is converted to the sodium bifluoride, which thermally decomposes to release HF.
- Sigma-Aldrich Co., Ammonium bifluoride. Retrieved on 2013-07-20.
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
- Emsley, J. (1980) Very strong hydrogen bonds, Chemical Society Reviews, 9, 91–124. doi:10.1039/CS9800900091
- Jean Aigueperse, Paul Mollard, Didier Devilliers, Marius Chemla, Robert Faron, Renée Romano, Jean Pierre Cuer (2005), "Fluorine Compounds, Inorganic" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a11 307