Ammonium fluoride
| |||
Names | |||
---|---|---|---|
IUPAC name
Ammonium fluoride
| |||
Other names
Neutral ammonium fluoride
| |||
Identifiers | |||
3D model (
JSmol ) |
|||
ChEBI | |||
ChemSpider | |||
ECHA InfoCard
|
100.031.975 | ||
EC Number |
| ||
PubChem CID
|
|||
RTECS number
|
| ||
UNII | |||
UN number | 2505 | ||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
Properties | |||
NH4F | |||
Molar mass | 37.037 g/mol | ||
Appearance | White crystalline solid hygroscopic
| ||
Density | 1.009 g/cm3 | ||
Melting point | 100 °C (212 °F; 373 K) (decomposes) | ||
83.5 g/100 ml (25 °C) [1] | |||
Solubility | slightly soluble in alcohol, insoluble in liquid ammonia | ||
−23.0×10−6 cm3/mol | |||
Structure | |||
Wurtzite structure (hexagonal)
| |||
Hazards | |||
GHS labelling:[2] | |||
Danger | |||
H301, H311, H314, H330, H331 | |||
P260, P261, P264, P270, P271, P280, P284, P301+P310, P301+P330+P331, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P310, P311, P312, P320, P321, P322, P330, P361, P363, P403+P233, P405, P501 | |||
NFPA 704 (fire diamond) | |||
Flash point | Non-flammable | ||
Safety data sheet (SDS) | ICSC 1223 | ||
Related compounds | |||
Other anions
|
Ammonium chloride Ammonium bromide Ammonium iodide | ||
Other cations
|
Sodium fluoride Potassium fluoride | ||
Related compounds
|
Ammonium bifluoride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Ammonium fluoride is the inorganic compound with the formula NH4F. It crystallizes as small colourless prisms, having a sharp saline taste, and is highly soluble in water. Like all fluoride salts, it is moderately toxic in both acute and chronic overdose.[3]
Crystal structure
Ammonium fluoride adopts the
Reactions
On passing
- NH4F + HF → NH4HF2
It sublimes when heated—a property common among ammonium salts. In the sublimation, the salt decomposes to ammonia and hydrogen fluoride, and the two gases can recombine to give ammonium fluoride, i.e. the reaction is reversible:
- [NH4]F ⇌ NH3 + HF
Uses
This substance is commonly called "commercial ammonium fluoride". The word "neutral" is sometimes added to "ammonium fluoride" to represent the neutral salt [NH4]F as opposed to the "acid salt" (NH4HF2). The acid salt is usually used in preference to the neutral salt in the
It is also used for preserving wood, as a mothproofing agent, in printing and dyeing textiles, and as an antiseptic in breweries.[6]
References
- ^ "Ammonium Fluoride". pubchem.ncbi.nlm.nih.gov.
- ^ "Ammonium Fluoride". pubchem.ncbi.nlm.nih.gov.
- ^ "Fluoride Toxicity - an overview | ScienceDirect Topics". www.sciencedirect.com. Retrieved 2020-12-16.
- ^ A. F. Wells, Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984.
- S2CID 4146351.
- ISBN 3-527-30673-0.