7789-23-3

Basic information

• Product Name: Potassium fluoride
• Synonyms: POTASSIUM FLUORIDE;POTASSIUM FLUORIDE IN D2O NMR REFERENCE STANDARD;POTASSIUM FLUORIDE ON CELITE(R);Fluorure de potassium;fluoruredepotassium;KF;Potassium fluoride (KF);Potassium fluorure
• CAS NO: 7789-23-3
• Molecular Formula: FK
• Molecular Weight: 58.1
• EINECS: 232-151-5
• Product Categories: Inorganics;Chemistry;Reagent Grade;Fluoride SourcesMetal and Ceramic Science;Crystal Grade Inorganics;Potassium Salts;PotassiumMetal and Ceramic Science;Protection and Derivatization;ACS GradeProtection and Derivatization;Deprotecting Reagents;Essential Chemicals;Fluoride Sources;Routine Reagents;Potassium SaltsEssential Chemicals;Metal and Ceramic Science;Reagent Plus;Salts;Analytical Reagents for General Use;O-P, Puriss p.a.;Puriss p.a.;metal halide;Essential Chemicals;Inorganic Salts;Materials Science;Metal and Ceramic Science;Potassium Salts;Reagent Plus;Research Essentials;Solutions and Reagents;Fluoride
• Mol File: 7789-23-3.mol

Chemical Properties

• Melting Point: 858 °C(lit.)
• Boiling Point: 1505 °C
• Flash Point: 1505°C
• Appearance: White/spray-dried
• Density: 2.48
• Vapor Density: 2 (vs air)
• Vapor Pressure: 922mmHg at 25°C
• Refractive Index: 1.363
• Storage Temp.: Store at RT.
• Solubility: H2O: 1 M at 20 °C, clear, colorless
• Water Solubility: 92.3 g/100 mL (18 ºC)
• Sensitive: Hygroscopic
• Stability: Stable. Protect from moisture. Incompatible with strong acids, strong bases.
• Merck: 14,7632
• BRN: 3902818
• CAS DataBase Reference: Potassium fluoride(CAS DataBase Reference)
• NIST Chemistry Reference: Potassium fluoride(7789-23-3)
• EPA Substance Registry System: Potassium fluoride(7789-23-3)

Safety Data

• Hazard Codes: T
• Statements: 25-23/24/25
• Safety Statements: 45-26-36/37
• RIDADR: UN 1812 6.1/PG 3
• WGK Germany: 3
• RTECS: TT0700000
• F: 3
• TSCA: Yes
• HazardClass: 6.1
• PackingGroup: III
• Hazardous Substances Data: 7789-23-3(Hazardous Substances Data)

Usage

Chemical Properties

Different sources of media describe the Chemical Properties of 7789-23-3 differently. You can refer to the following data:
1. Potassium fluoride, KF, is a colorless, deliquescent crystalline solid that has a melting point of 846 °C(1550 °F). Potassium fluoride has a salty taste and is poisonous. It is soluble in water,but insoluble in alcohol. Potassium fluoride is used in etching glass,preservatives, and insecticides.
2. White, crystalline, deliquescent powder; sharp saline taste.Soluble in water and hydrogen fluoride, insoluble in alcohol.
3. Potassium fluoride is a white crystalline solid.

Physical and Chemical Properties

Potassium fluoride is basis raw material of manufacturing fluoride, chemical formula is KF. Molecular weight is 58.10. It is colorless cubic crystal or white powder. It is poisonous! It is deliquescent. Taste is salty. Specific gravity is 2.48. Melting point is 858℃. Boiling point is 1505℃. It is soluble in water. It was dissolved in hydrofluoric acid and ammonia. It is insoluble in ethanol, acetone. Aqueous solution is alkaline and it can corrode glass and porcelain. It can cause irritation for human skin, mucous membrane and eye. When belows 40.2℃, it can crystallize in an aqueous solution to give dihydrate KF·2H2O, which is monoclinic, it is self-dissolved crystalline water at 41℃. It can be obtained by the thermal decomposition of potassium hydrogen fluoride or potassium carbonate (or potassium hydroxide) and hydrofluoric acid (40% or anhydrous). It can be used for glass engraving, food preservation, it can be also used as welding flux, fluoride, pesticides,etc. Figure 1 the structural formula of potassium fluoride.

Uses

Different sources of media describe the Uses of 7789-23-3 differently. You can refer to the following data:
1. Anhydrous Potassium fluoride is used in organic synthesis as a catalyst for various reactions, or to introduce fluorine into organic molecules. For example, fluoro compounds can be prepared by replacing labile chlorine atoms by fluorine atoms, as in the manufacture of sodium fluoroacetate, a rat poison. The nucleophilic strength of F? and the solubility of KF in aprotic organic solvents may be improved by using crown ethers. The “naked” fluoride ion obtained is an efficient fluorinating agent.
2. ▼▲ Industry Application Role/benefit Organic synthesis Preparation of various organic fluoride Fluorinating agent/replaces other halide ions like chlorine, bromine etc. Chemical manufacture Manufacture of polyurethanes and alkyl benzenes Catalyst/promote the reaction rate Manufacture of pesticides and insecticides Fluorinating agent; ingredient Manufacture of potassium bifluoride Raw material Metallurgy Soldering Soldering fluxes/help to remove oxide film Tin plating Plating composition/source of fluoride Glass Etching of glass Glass etching composition; source of fluoride Others Food and wood preservative Source of fluoride Absorption of hf and moisture Adsorbent/anhydrous potassium fluoride has hydroscopicity Complexometric titration of tantalum Masking agent Extraction of tantalum from ore Precipitator/reacts with fluorotantalic acid to precipitate potassium fluorotantalate
3. Potassium fluoride is used in metal finishing, batteries, coatings and photographic chemicals. It is utilized for the study of ion-specific swelling and de-swelling of ampholytic polymer gels as well as in the measurement of electronic polarizabilities of ions in polymers of alkali halides. It finds application in the electronic industry as a metal surface treatment product. It is used as a preservative, a food additive, a catalyzer and a water absorbing agent. In the Finkelstein reaction, it is actively involved in the conversion of chlorocarbons to fluorocarbons using polar solvents like dimethyl formamide and ethylene glycol.

Preparation

Potassium fluoride is prepared by reacting potassium carbonate (or KOH) with aqueous hydrofluoric acid. Care is necessary in handling the anhydrous salt, to prevent its hydration.

Reactivity Profile

Potassium fluoride reacts with acids to evolve corrosive and toxic hydrogen fluoride. Aqueous solutions corrode glass and consequently are prepared and stored in polyethylene containers. The pure solid may be stored in glass containers. Reacts violently with (Pt + BrF3). [NTP 1992].

Health Hazard

TOXIC; 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 Hazard

Non-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 Profile

Poison by ingestion and intraperitoneal routes. Moderately toxic by subcutaneous route. Experimental teratogenic effects. A corrosive irritant to the eyes, skin, and mucous membranes. Mutation data reported. A very reactive material. When heated to decomposition it emits toxic fumes of K2O and F-. Used in etchmg glass, as a presewative, as an insecticide, and in organic synthesis. See also FLUORIDES and HYDROFLUORIC ACID.

Potential Exposure

Potassium fluoride is used in etching glass; as a preservative and insecticide.

Shipping

UN1812 Potassium fluoride, solid, Hazard Class: 6.1; Labels: 6.1-Poisonous materials.

Incompatibilities

Incompatible with strong acids; reacts releasing hydrogen fluoride. Aqueous solutions corrode glass and consequently are prepared and stored in polyeth- ylene containers. The pure solid may be stored in glass containers. Reacts violently with (Pt 1 BrF 3 )

InChI:InChI=1/FH.K/h1H;/q;+1/p-1

Upstream product

• 7664-39-3 hydrogen fluoride 
• 7440-09-7 potassium 
• 1310-58-3 potassium hydroxide 
• 354-87-0 pentafluoroethanesulfonyl fluoride 
• 423-40-5 1-perfluoropropanesulfonyl fluoride 
• 335-05-7 Trifluoromethanesulfonyl fluoride 
• 584-08-7 potassium carbonate 
• 1493-05-6 difluoro-nitro-methane 
• 865-47-4 potassium tert-butylate 
• 7783-41-7 difluoroether 
• 1279123-63-5 potassium hydrogenfluoride 
• 13455-22-6 potassium fluorosulfonate 
• 7732-18-5 water 
• 7558-02-3 potassium bromide 

Downstream Products

• 1236360-42-1 9-thia-10-boraanthracene-(C₆H₂Me₂NMe₃)(F) 
• 1015761-62-2 K[1,2-ferrocenediyl(BMeF₂))(SnMe₂Ph)] 
• 1015761-73-5 [(C₅H₅)Fe(C₅H₄Sn(CH₃)2F)] 
• 1015761-70-2 [(C₅H₅)Fe(C₅H₄Sn(CH₃)2C₆H₅)] 
• 767355-17-9 bis[fluoro(di-n-octyl)stannyl]methane 
• 82762-26-3 K⁽¹⁺⁾*[F₄Sn(CH₂)4OH]^(1-) = K[F₄Sn(CH₂)4OH] 
• 6698-89-1 3,5-Cl₂C₆F₃SO₂F 
• 49640-78-0 pentacyanofluorobenzene 
• 18114-69-7 trifluorophenylborate anion 
• 141585-15-1 (C₆H₅)4P⁽¹⁺⁾*(((C₅(CH₃)5)TiF₃)4F₂)K^(1-) = {(C₆H₅)4P}{(((C₅(CH₃)5)TiF₃)4F₂)K} 
• 945905-31-7 2,4,6-trimethylphenyl-fluoroborane-(C₆H₄)2-methyl-phenyl-phosphonium 
• 192998-33-7 1,3-bis(diphenylfluorostannylmethyl)dimethylsilane 
• 16893-92-8 potassium hexafluoroantimonate 

Relevant articles and documents

Investigation of KYF4: Yb, Er // KYF4 nanocrystals - Mechanism of the KYF4 formation

This paper presents our investigation of the formation mechanism of cubic phase Yb3+ and Er 3+ doped nanoscale KYF4. We generated Yb, Er doped KYF4 nanoparticles, modified with undoped KYF4 following

Phase transitions in K3AlF6

Phase transitions in the elpasolite-type K3AlF6 complex fluoride were investigated using differential scanning calorimetry, electron diffraction and X-ray powder diffraction. Three phase transitions were identified with critical temperatures T1=132°C, T2=153°C and T3=306°C. The α-K3AlF6 phase is stable below T1 and crystallizes in a monoclinic unit cell with a=18.8588(2)A, b=34.0278(2)A, c=18.9231(1)A, β=90.453(1)° (a=2ac-cc, b=4bc, c=ac+2cc; ac, bc, cc - the basic lattice vectors of the face-centered cubic elpasolite structure) and space group I2/a or Ia. The intermediate β phase exists only in very narrow temperature interval between T1 and T2. The γ polymorph is stable in the T2a=36.1229(6)A, b=17.1114(3)A, c=12.0502(3)A (a=3ac-3cc, b=2bc, c=a c+cc) at 250 °C and space group Fddd. Above T 3 the cubic δ polymorph forms with ac=8.5786(4)A at 400 °C and space group Fm3m. The similarity between the K 3AlF6 and K3MoO3F3 compounds is discussed.

Two anhydrous salts of tetrafluoroterephthalic acid (H2tF-BDC): K2tF-BDC and Rb2tF-BDC

Two new anhydrous salts of tetrafluoroterephthalic acid (H 2tF-BDC), namely K2tF-BDC (1) and Rb2tF-BDC (2), were synthesized and structurally characterized. The crystal structure of 1 (I2/m, Z = 2) was solved and refined from X-ray single crystal data. K + (CN = 8) is coordinated by six oxygen atoms of five different tF-BDC2- linkers and two fluorine atoms of two of these linkers, which connect the KO6F2 polyhedra to a 3D network. The crystal structure of 2 (P1, Z = 1) was refined from X-ray powder diffraction data. It crystallizes in a structure type already known from Tl 2tF-BDC. Rb+ (CN = 8) is also coordinated by six oxygen and two fluorine atoms. But six tF-BDC2- linkers are involved in the coordination. Again, a 3D network is formed. Both compounds can be obtained as single-phase samples. They are not porous and stable in air. The thermal stability was investigated by DTA/TG measurements. The decomposition starts at approx. 200°C (1) and 230°C (2). Their good solubility in water makes them interesting starting materials for the synthesis of new MOFs with the perfluorinated linker tF-BDC2-. Copyright

Measurement of absolute rate data for the reaction of atomic potassium, K(4 2S1/2), with CF3Cl, CF2Cl2, CFCl3, CF3Br and SF6 as a function of temperature by time-resolved atomic resonance absorption spectroscopy at λ = 404 nm [k(5 2PJ) ← K(4 2S1/2)]

We present a kinetic study of the reactions of atomic potassium in its electronic ground state, K(42S1/2), with the molecules CF3Cl, CF2Cl2, CFCl3, CF3Br and SF6. Atomic potassium was generated by pulsed irradiation of potassium halide vapour at elevated temperatures and monitored in the 'single-shot mode' by time-resolved atomic resonance absorption using the Rydberg doublet at λ = 404 nm [K(5 2PJ) ← K(4 2S1/2)]. Absolute rate constants for reaction with these molecules were determined as a function of temperature yielding the following Arrhenius parameters (errors 1σ): A/10-10 cm3 molecules-1 s-1 E/kJ mol-1 CF3Cl 1.1±0.5 13.8±2.5 CF2Cl2 2.1±0.6 5.5±0.5 CFCl3 ca. 1 ca. 0 CF3Br 3.9±0.4 12.3±0.6 SF6 8.4±1.33 12.3±0.9 CF4 exhibited anomalous kinetic behaviour. These results represent the first kinetic measurements, relative or absolute, for these fundamental reactions of atomic potassium. This new set of absolute rate data are compared with analogous results reported hitherto for atomic sodium, Na(3 2S1/2), both alkali-metal atoms exhibiting rapid reactions characterised by small energy barriers and being highly exothermic in character.

Exploration on anion ordering, optical properties and electronic structure in K3WO3F3 elpasolite

Room-temperature modification of potassium oxyfluorotungstate, G2-K 3WO3F3, has been prepared by low-temperature chemical route and single crystal growth. Wide optical transparency range of 0.39.4 μm and forbidden band gap Eg=4.32 eV have been obtained for G2-K3WO3F3 crystal. Meanwhile, its electronic structure has been calculated with the first-principles calculations. The good agreement between the theorectical and experimental results have been achieved. Furthermore, G2-K3WO3F3 is predicted to possess the relatively large nonlinear optical coefficients. 2012 Elsevier Inc.

Wet chemical synthesis of LiBaF3 phosphor

LiBaF3 has great potential applications as X-ray storage phosphor, slow neutron imaging, scintillator, vacuum ultraviolet (VUV) optical lithography, etc. Conventionally, LiBaF3 is prepared by solid state reaction between the constituent fluorides. However, the preparation of phase pure material and especially single crystals is rather tricky due to incongruent melting. For the first time, a wet chemical preparation of rare earth activated LiBaF3 is described here. As precipitated powders containing Ce 3+ or Tb3+ exhibited characteristic luminescence. For observing Eu2+ emission, it was necessary to heat the powders in a reductive atmosphere. It is suggested that phosphors prepared by this method may prove useful in applications like OSL, X-ray imaging, etc. which do not require large single crystals.

The mild hydrothermal synthesis of complex fluorides of AZnF3 (A = Na, K)

The complex fluorides of AZnF3 (A = Na, K), which are isostructural with perovskite phases were obtained by the method of hydrothermal synthesis at 160-220 °C. Compared with traditional high-temperature solid-state method, the products were pure and contained lower amount of oxygen.

A novel 18F labelled imidazo-oxazolopyridine derivative as β-amyloid imaging agent: Synthesis and preliminary evaluation

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Molecular Beam Study of Steric Effects in the Reaction K + HF (v = 1, j = 2) -> KF + H

HF molecules were optically aligned by use of linearly polarized infrared radiation generated by a color center laser tuned to the R1(l) line of HF.The state-specific integral cross section of the reaction K + HF (v = 1, j = 2) -> KF + H was measured for the two different preparations of the approach geometry which result when the plane of polarization is positioned either parallel (?) or perpendicular (?) to the most probable relative velocity of the reagents.At a translational energy of Etr = 0.46 eV the resulting relative difference of the cross sections (? - ?)/?(? = 1/2(? + ?)) amounts to 17 +/- 5percent.This steric effect decreases with rising Etr and reaches zero near 1.2 eV.The data strongly suggest that the reaction occurs via a collinear transition state.

The crystal structure of α-K3AIF6: Elpasolites and double perovskites with broken corner-sharing connectivity of the octahedral framework

The crystal structure of α-K3AIF6 was solved and refined from a combination of powder X-ray and neutron diffraction data (a = 18.8385(3)A, c = 33.9644(6)A, S.G. /41 Z= 80, R P(X-ray) = 0.037, Rp(neutr