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Potassium fluoride

Ionic compound (KF)

Ionic compound (KF)

94.1273 g/mol (dihydrate) 41 °C (dihydrate) 19.3 °C (trihydrate) 92 g/100 mL (18 °C) 102 g/100 mL (25 °C) dihydrate: 349.3 g/100 mL (18 °C) insoluble in alcohol | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = Potassium bromide Potassium iodide Sodium fluoride Rubidium fluoride Caesium fluoride Francium fluoride

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: : : 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.

Crystalline properties

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

Applications in organic chemistry

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

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.

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

References

  1. "Potassium Fluoride".
  2. Chambers, Michael. "ChemIDplus - 7789-23-3 - NROKBHXJSPEDAR-UHFFFAOYSA-M - Potassium fluoride - Similar structures search, synonyms, formulas, resource links, and other chemical information.".
  3. "Potassium fluoride". [[University College London]].
  4. (1956). "n-Hexyl Fluoride".
  5. (2002). "Fluorine Compounds, Organic".
  6. 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
  7. (2020-12-04). "Nucleophilic Fluorination with KF Catalyzed by 18-Crown-6 and Bulky Diols: A Theoretical and Experimental Study". The Journal of Organic Chemistry.
  8. (2002). "KF/Al2O3 Mediated organic synthesis". Tetrahedron.
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