Potassium fluoride

Potassium fluoride

Names
IUPAC name Potassium fluoride
Identifiers
CAS Number	7789-23-3 (anhydrous) Y 13455-21-5 (dihydrate) Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL1644027 N
ChemSpider	23006 Y
ECHA InfoCard	100.029.228
EC Number	232-151-5
PubChem CID	522689
RTECS number	TT0700000
UNII	9082WG1G3F Y 95R1D12HEH (dihydrate) Y
CompTox Dashboard (EPA)	DTXSID8031940
InChI InChI=1S/FH.K/h1H;/q;+1/p-1 Y Key: NROKBHXJSPEDAR-UHFFFAOYSA-M Y InChI=1S/FH.K/h1H;/q;+1/p-1 Key: NROKBHXJSPEDAR-REWHXWOFAI Key: NROKBHXJSPEDAR-UHFFFAOYSA-M
SMILES [F-].[K+]
Properties
Chemical formula	KF
Molar mass	58.0967 g/mol (anhydrous) 94.1273 g/mol (dihydrate)
Appearance	colourless
Density	2.48 g/cm3
Melting point	858 °C (1,576 °F; 1,131 K) (anhydrous) 41 °C (dihydrate) 19.3 °C (trihydrate)
Boiling point	1,502 °C (2,736 °F; 1,775 K)
Solubility in water	anhydrous: 92 g/100 mL (18 °C) 102 g/100 mL (25 °C) dihydrate: 349.3 g/100 mL (18 °C)
Solubility	soluble in HF insoluble in alcohol
Magnetic susceptibility (χ)	−23.6·10−6 cm3/mol
Structure
Crystal structure	cubic
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H301, H311, H331[1]
Precautionary statements	P261, P264, P270, P271, P280, P301+P310, P302+P352, P304+P340, P311, P312, P321, P322, P330, P361, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)	3 0 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	245 mg/kg (oral, rat)[2]
Related compounds
Other anions	Potassium chloride Potassium bromide Potassium iodide
Other cations	Lithium fluoride Sodium fluoride Rubidium fluoride Caesium fluoride Francium fluoride
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 fluoride is the chemical compound with the formula KF. After hydrogen fluoride, KF is the primary source of the fluoride ion for applications in manufacturing and in chemistry. It is an alkali halide salt and occurs naturally as the rare mineral carobbiite. Solutions of KF will etch glass due to the formation of soluble fluorosilicates, although HF is more effective.

Preparation

Potassium fluoride is prepared by reacting potassium carbonate with hydrofluoric acid. Evaporation of the solution forms crystals of potassium bifluoride. The bifluoride on heating yields potassium fluoride:

${\displaystyle {\ce {K2CO3 + 4HF -> 2KHF2 + CO2 ^ + H2O}}}$

${\displaystyle {\ce {KHF2 -> KF + HF ^}}}$

Platinum or heat resistant plastic containers are often used for these operations.

Potassium chloride converts to KF upon treatment with hydrogen fluoride. In this way, potassium fluoride is recyclable.^[3]

Crystalline properties

KF crystallizes in the cubic NaCl crystal structure. The lattice parameter at room temperature is 0.266 nm.^[4]

Applications in organic chemistry

In organic chemistry, KF can be used for the conversion of chlorocarbons into fluorocarbons, via the Finkelstein (alkyl halides)^[5] and Halex reactions (aryl chlorides).^[3] Such reactions usually employ polar solvents such as dimethyl formamide, ethylene glycol, and dimethyl sulfoxide.^[6] More efficient fluorination of aliphatic halides can be achieved with a combination of crown ether and bulky diols in acetonitrile solvent.^[7]

Potassium fluoride on alumina (KF/Al₂O₃) is a base used in organic synthesis. It was originally introduced in 1979 by Ando et al. for inducing alkylation reactions.^[8] It is ^{[9][verification needed]}

Safety considerations

Like other sources of the fluoride ion, F⁻, KF is poisonous, although lethal doses approach gram levels for humans. It is harmful by inhalation and ingestion. It is highly corrosive, and skin contact may cause severe burns.

References