Potassium hydrogen fluoride

Potassium hydrogen fluoride Basic information
Description References
Product Name:Potassium hydrogen fluoride
Synonyms:potassiummonohydrogendifluoride;POTASSIUM HYDROGEN FLUORIDE;POTASSIUM HYDROGEN DIFLUORIDE;POTASSIUM BIFLUORIDE;Potassium hydrogen fluoride, 99+% (metals basis);potassium bifluoride potassium hydrogen difluoride;Potassium Bifluoride, crystal;POTASSIUM HYDROGENFLUORIDE, 99.99+%
CAS:7789-29-9
MF:F2HK
MW:78.1
EINECS:232-156-2
Product Categories:Fluorination Reagents;Chemical Synthesis;C-X Bond Formation (Halogen);Fluorination;metal halide;Synthetic Reagents;Inorganic Chemicals;Inorganics;Synthetic Reagents
Mol File:7789-29-9.mol
Potassium hydrogen fluoride Structure
Potassium hydrogen fluoride Chemical Properties
Melting point 239 °C(lit.)
density 2.37 g/mL at 25 °C(lit.)
form Crystals or Crystalline Powder
Specific Gravity2.37
color White to light gray
Water Solubility 39 g/100 mL (20 ºC)
Sensitive Hygroscopic
Merck 14,7610
Exposure limitsACGIH: TWA 2.5 mg/m3
NIOSH: IDLH 250 mg/m3
CAS DataBase Reference7789-29-9(CAS DataBase Reference)
NIST Chemistry ReferencePotassium hydrogen fluoride(7789-29-9)
EPA Substance Registry SystemPotassium bifluoride (7789-29-9)
Safety Information
Hazard Codes T,C
Risk Statements 25-34
Safety Statements 26-36/37/39-45-37-22
RIDADR UN 3421 8/PG 2
WGK Germany 1
RTECS TS6650000
3
Hazard Note Corrosive
TSCA Yes
HazardClass 8
PackingGroup II
HS Code 28261990
MSDS Information
ProviderLanguage
SigmaAldrich English
ACROS English
ALFA English
Potassium hydrogen fluoride Usage And Synthesis
DescriptionPotassium hydrogen fluoride is used as an etchant to etch glass surface and it is used in the cleaning products. It is used as a fluorinating agent for fluorinated organic compounds, which could be applied as finishing agent for fabrics, components of extinguishing agents, electroplating bathes, lubricating oils, oxygen carriers in blood substitutes. For example, potassium hydrogen fluoride is used as fluorinating agent for ring opening of epoxides and cyclopropanes and in the synthesis of trifluoroborates from various organoborons. It may also serve as a fluoride ion source for the nucleophilic ring-opening reaction of epoxide.
References[1] Gary A. Molander, David J. Cooper and Stephen W. Wright, Potassium Hydrogen Fluoride, e-EROS Encyclopedia of Reagents for Organic Synthesis, 2001
[2] Bernd Basner, Houben-Weyl Methods of Organic Chemistry Vol. E 10b/1, 4th Edition, 1999
[3] Francis I. Onuska and Francis W. Karasek, Open Tubular Column Gas Chromatography in Environmental Sciences, 1984
[4] Michael Howe, Wheel cleaning composition containing acid fluoride salts, Patent “US 5556833 A”, 1996
[5] Grzegorz Lewandowski, Egbert Meissner and Eugeniusz Milchert, Special applications of fluorinated organic compounds, Journal of Hazardous Materials, 2006, vol. 136, 385-391



Chemical PropertiesWHITE TO LIGHT GREY CRYSTALS OR CRYSTALLINE POWDER
UsesIn the preparation of pure potassium fluoride; as an electrolyte in the manufacture of fluorine; frosting glass; treating coal to prevent slag formation; flux for silver solders; catalyst in the alkylation of benzene with olefins.
UsesPotassium hydrogen fluoride is widely used as an etchant in glass and cleaning products. It finds an important application in the synthesis of special optical glass viz. crown and crown flint glass and as a catalyst for polymerization. It is involved in the manufacturing of wood preservatives, soldering agents and brazing. It is also used in the manufacturing of organic and inorganic fluorine compounds.
General DescriptionColorless crystals, corrosive to tissues, etches glass.
Air & Water ReactionsWater soluble giving strongly acidic solutions.
Reactivity ProfileAcidic salts, such as Potassium hydrogen fluoride, are generally soluble in water. The resulting solutions contain moderate concentrations of hydrogen ions and have pH's of less than 7.0. They react as acids to neutralize bases. These neutralizations generate heat, but less or far less than is generated by neutralization of inorganic acids, inorganic oxoacids, and carboxylic acid. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible.
HazardCorrosive to tissue.
Health HazardTOXIC; inhalation, ingestion or skin contact with material may cause severe injury or death. Contact with molten substance may cause severe burns to skin and eyes. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.
Fire HazardNon-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated.
Safety ProfileA poison. Very corrosive and reactive. A corrosive irritant to the eyes, skin, and mucous membranes. When heated to decomposition it emits toxic fumes of F and K2O. See also FLUORIDES and HYDROFLUORIC ACID.
Purification MethodsIt crystallises from water. It is very soluble in hot H2O and 41% at 21o. [Kwasnik in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 237 1963.]
Ammonium hydrogen difluoride Potassium fluoride dihydrate POTASSIUM HYDROGENSULFIDE, Losartan potassium Potassium iodide Potassium sorbate Difluorochloromethane Potassium hydride Potassium persulfate Potassium borohydride Sodium hydrogen difluoride Hydrogen Hydrogen fluoride Potassium Acetate Potassium hydrogen fluoride Potassium Pyridine hydrofluoride Potassium sulfate

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