Potassium fluoride

Potassium fluoride
Names
IUPAC name
Potassium fluoride
Identifiers
7789-23-3 (anhydrous) YesY
13455-21-5 (dihydrate) N
ChEMBL ChEMBL1644027 N
ChemSpider 23006 YesY
EC Number 232-151-5
Jmol interactive 3D Image
PubChem 522689
RTECS number TT0700000
UNII 9082WG1G3F YesY
Properties
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)
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
Structure
cubic
Hazards
Toxic (T)
R-phrases R23/24/25
S-phrases (S1/2), S26, S45
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
0
3
1
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
245 mg/kg (oral, rat)[1]
Related compounds
Other anions
 Potassium chloride
Potassium bromide
Potassium iodide
Other cations
 Lithium fluoride
Sodium fluoride
Rubidium fluoride
Caesium 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 YesYN ?)
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 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 dissolving potassium carbonate in excess hydrofluoric acid. Evaporation of the solution forms crystals of potassium bifluoride. The bifluoride on heating yields potassium fluoride:

K2CO3 + 4HF → 2KHF2 + CO2↑ + H2O
KHF2 → KF + HF↑

The salt must not be prepared in glass or porcelain vessels as HF and the aqueous solution of KF corrode glass and porcelain. Heat resistant plastic or platinum containers may be used.

Applications in organic chemistry

In organic chemistry, KF can be used for the conversion of chlorocarbons into fluorocarbons, via the Finkelstein reaction.[2] Such reactions usually employ polar solvents such as dimethyl formamide, ethylene glycol, and dimethyl sulfoxide.[3]

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

  1. ↑ http://chem.sis.nlm.nih.gov/chemidplus/rn/7789-23-3
  2. ↑ Vogel, A. I.; Leicester, J.; Macey, W. A. T. "n-Hexyl Fluoride". Org. Synth.; Coll. Vol. 4, p. 525
  3. ↑ Han, Q.; Li, H-Y. "Potassium Fluoride" in Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley & Sons,New York. doi:10.1002/047084289X.rp214
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