Potassium bifluoride
Names | |
---|---|
IUPAC name Potassium bifluoride | |
Other names Potassium hydrogen difluoride | |
Identifiers | |
CAS Number |
|
3D model (JSmol) |
|
ChemSpider |
|
ECHA InfoCard | 100.029.233 |
EC Number |
|
PubChem CID |
|
RTECS number |
|
UNII |
|
UN number | 1811 |
CompTox Dashboard (EPA) |
|
InChI
| |
| |
Properties | |
Chemical formula | K[HF2] |
Molar mass | 78.103 g/mol |
Appearance | colourless solid |
Odor | slightly acidic |
Density | 2.37 g/cm3 |
Melting point | 238.7 °C (461.7 °F; 511.8 K) |
Boiling point | decomposes |
Solubility in water |
|
Solubility | soluble in ethanol |
Structure | |
monoclinic | |
Thermochemistry | |
Std molar entropy (S⦵298) | 45.56 J/(mol·K) [1] |
Std enthalpy of formation (ΔfH⦵298) | -417.26 kJ/(mol·K) |
Hazards | |
GHS labelling:[2] | |
Danger | |
H301, H310, H314 | |
P260, P262, P264, P270, P280, P301+P310, P301+P330+P331, P302+P350, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P322, P330, P361, P363, P405, P501 | |
Flash point | non flammable |
Related compounds | |
Other anions | Potassium fluoride |
Other cations | Sodium bifluoride, ammonium bifluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references |
Potassium bifluoride is the inorganic compound with the formula K[HF2]. This colourless salt consists of the potassium cation (K+) and the bifluoride anion ([HF2]−). The salt is used as an etchant for glass. Sodium bifluoride is related and is also of commercial use as an etchant as well as in cleaning products.[3]
Synthesis and reactions
The salt was prepared by Edmond Frémy by treating potassium carbonate or potassium hydroxide with hydrofluoric acid:
- 2 HF + KOH → K[HF2] + H2O
With one more equivalent of HF, K[H2F3] (CAS#12178-06-2, m.p. 71.7 C)[clarification needed] is produced:
- HF + K[HF2] → K[H2F3]
Thermal decomposition of K[HF2] gives hydrogen fluoride:
- K[HF2] → HF + KF
Applications
The industrial production of fluorine entails the electrolysis of molten K[HF2] and K[H2F3].[3] The electrolysis of K[HF2] was first used by Henri Moissan in 1886.
See also
References
- ^ Westrum, Edgar F. Jr.; Pitzer, Kenneth S. (June 1949). "Thermodynamics of the System KHF2-KF-HF, Including Heat Capacities and Entropies of KHF2, and KF. The Nature of the Hydrogen Bond in KHF2". J. Am. Chem. Soc. 71 (6): 1940–1949. doi:10.1021/ja01174a012.
- ^ "Potassium bifluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 27 December 2021.
- ^ a b Aigueperse, Jean; Mollard, Paul; Devilliers, Didier; Chemla, Marius; Faron, Robert; Romano, René; Cuer, Jean Pierre (2000). "Fluorine Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a11_307. ISBN 3527306730.
- v
- t
- e
- K3N
- KNH2
- KN3
- KNO2
- KNO3
- K3P
- KH2PO3
- K3PO4
- K2HPO4
- KH2PO4
- KPF6
- KAsO2
- K3AsO4
- K2HAsO4
- KH2AsO4
- B4K2O7
- K2CO3
- KHCO3
- K2SiO3
- K2SiF6
- K2Al2O4
- K2Al2B2O7
- K2PtCl4
- K2Pt(CN)4
- K2TiF6
- K2PtCl6
- K2ReCl6
- K2ZrF6
- K4Fe(CN)6
- K3Fe(CN)6
- K3Fe(C2O4)3
- K2FeO4
- K2MnO4
- KMnO4
- K3CrO4
- K2CrO4
- K3CrO8
- KCrO3Cl
- K2Cr2O7
- K2Cr3O10
- K2Cr4O13
- K4Mo2Cl8
- KHCO2
- KCH3CO2
- KCF3CO2
- K2C2O4
- KHC2O4
- KC12H23O2
- KC18H35O2
- C3H2K2O4
- C4H6KO4
- C5H7KO4