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Potassium fluoride Crystalline structure of potassium fluoride. __ K + __ F – Identification","datePublished":"2019-02-28","dateModified":"2019-02-28","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/44a4cee54c4c053e967fe3e7d054edd4?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/44a4cee54c4c053e967fe3e7d054edd4?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/c\/c0\/NaCl_polyhedra.png\/160px-NaCl_polyhedra.png","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/c\/c0\/NaCl_polyhedra.png\/160px-NaCl_polyhedra.png","height":"137","width":"160"},"url":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/potassium-fluoride-wikipedia\/","wordCount":3420,"articleBody":"     (adsbygoogle = window.adsbygoogle || []).push({});before-content-x4A wikipedia article, free l’encyclop\u00e9i. Potassium fluoride  Crystalline structure of potassium fluoride. __ K +  __ F – Identification UICPA name potassium fluoride  N O CAS 7789-23-3 (anhydrous) 13455-21-1 (dihydrate) N O Echa 100,029.228 N O THIS 232-151-5 N O RTECS TT0700000 Pubchem 522689  SMILES  Inches Inches:  3D view  Inchi=1\/fh.k\/h1H;\/Q;+1\/P-1 InChIKey\u00a0:  NOCBHXJPEDAR-UHFFFAOYSA-M Appearance Powder or crystals, white sometimes greenish, underdoors [ first ] Chemicals Formula FK\u00a0\u00a0 [Isomers] KF Molar mass [ 3 ] 58.096 7 \u00b1 0,000 1 g\/mol F\u00a032,7\u00a0%,  K\u00a067,3\u00a0%,  Dipolar moment 8,585 \u00b1 0.003 D [ 2 ] Physical properties T\u00b0 fusion 858 \u00b0C [ first ] T\u00b0 boiling 1 502 \u00b0C [ first ] Solubility 485  g \u00b7 l -first (water, 20 \u00b0C ) [ first ] Volumic mass 2.48  g \u00b7 cm -3 [ first ] Crystallography Structure type NaCl [ 4 ] Precautions SGH [ 5 ] Danger        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4H301 , H311 And H331 H301 : Toxic in case of ingestion H311 : Toxic by skin contact H331 : Toxic by inhalation        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4Simdut [ 6 ] D1B, D2a, D1B : Toxic material with severe immediate effects Transport of dangerous goods: class 6.1 Group III D2a : Very toxic material with other toxic effects Chronic toxicity: fluorosis Disclosure at 1.0% according to the ingredient disclosure list Transport [ first ] Code Kemler\u00a0: 60 : toxic material or with a minor degree of toxicity UN number: 1812 : Potassium fluoride Class: 6.1 Label : 6.1 : Toxic materials Ecotoxicology DL 50  245 mg\u00a0kg \u22121 (rat, oral) [ 7 ] IS units and CNTP , unless otherwise stated. modifier  The potassium fluoride is an inorganic compound of Formula KF. After hydrogen fluoride, it is the main source of fluoride ion used in industry and chemistry. It is an alkaline metal halogenure (in) Naturally present in the form of a rare mineral, carobbiitis. KF solutions can attack glass due to the formation of soluble fluorosilicates, even if fluorhydrical acid is more effective for this task.        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4  Potassium fluoride is in the form of a hygroscopic white powder, generally in its dihydrate form. Dihydrate melts to forty six \u00b0C in its crystallization water. We can dissolve 485 g potassium fluoride in a liter of water to 20 \u00b0C . Potassium fluoride has a standard \u0394H formation enthalpy f \u00b0 = -569 kj \/ times [ 8 ] Because natural potassium contains 0.0118% of the radiisotope 40 K, KF’s radioactivity is 20,979 Bq kg \u22121 , at 89.28% of beta radiation and to and 10.72% gamma radiation of 1,460 83  MeV . Potassium fluoride can be prepared by dissolving excess potassium carbonate in fluorhydric acid. During the evaporation of the solution, potassium bifluoride crystals are formed. By heating this bifluoride you get potassium fluoride: K 2 CO 3 + 4 HF aq \u2192 2 KHF 2 + CO 2 \u2191 + H 2 O KHF 2 \u2192 KF + HF\u2191 This salt obviously cannot be prepared in a glass or porcelain container because it would be attacked by flurohydrical acid. A plastic container (PTFE) resistant to heat or platinum should be used. Chemistry [ modifier | Modifier and code ] In organic chemistry, potassium fluoride can be used for the conversion of organochlorine compounds into organofluor\u00e9s compounds, via the finkelstein reaction [ 9 ] . For such reactions we generally use a polar solvent such as dimethylformamide (DMF), glycol ethylene or dimethylsulfoxide (DMSO) [ ten ] . Others [ modifier | Modifier and code ] Potassium fluoride is used in enamel production, as an additive for cement, as an oxidant in the aluminum weld powder. It is also used as a wooden conservation agent and for glass engraving. It can also be used as a source of fluoride ions in oral hygiene products (toothpaste, mouthwash, etc.) and for fluoridated foods (food salt, water). Like other sources of fluoride ions, KF is toxic, even if the lethal doses are of the gram level for humans. It is dangerous by inhalation and ingestion. It is highly corrosive, any contact with the skin that can cause severe burns. \u2191 a b c d e and f Potassium fluoride input in the chemical product database Achievement IFA (German organization responsible for occupational safety and health) ( German , English ), access on October 22, 2015 (Javascript required)  \u2191 (in) David R. Like, Handbook of chemistry and physics , Boca Raton, CRC, June 16, 2008 , 89 It is  ed. , 2736 p.  (ISBN\u00a0 978-1-4200-6679-1 And 1-4200-6679-X ) , p. 9-50  \u2191 Molar mass calculated after ‘ Atomic weights of the elements 2007 \u00bb , on www.chem.qmul.ac.uk .  \u2191 (in) My body. do Rablass, ah-hand hut, Structure and Chemistry of Crystalline Solids , Pittsburgh, PA, USA, Springer Science + Business Media, Inc., 2006 , 346 p.  (ISBN\u00a0 0-387-26147-8 ) , p. sixty four  \u2191 Index number 009-005-00-2 In Table 3.1 of Annex VI of CE Regulation N \u00b0 1272\/2008 (December 16, 2008)  \u2191 ‘ Potassium fluoride \u00bbIn the chemical product database Reptox of the CSST (Quebec organization responsible for occupational safety and health), consulted on April 25, 2009  \u2191 )U.S. Atomic Energy Commission, University of Rochester, Research and Development Reports. Vol. UR-154, Pg. 1951  \u2191 (of) A. F. Holleman, E. Wiberg, N. Wiberg, Inorganic chemistry textbook , Berlin, from Gruyter, 1995 (ISBN\u00a0 3-11-012641-9 ) , p. 1170  \u2191 Vogel, A. I.; Leicester, J.; Macey, W. A. T., n-Hexyl Fluoride , Org. Synth., coll. \u00a0\u00ab\u00a0vol. 4\u00a0\u00bb, p. 525  \u2191 Han, Q.; Li, H-Y. “Potassium Fluoride” in Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley & Sons,New York. DOI\u00a0 10.1002\/047084289X.rp214         (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4"},{"@context":"http:\/\/schema.org\/","@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"item":{"@id":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/#breadcrumbitem","name":"Enzyklop\u00e4die"}},{"@type":"ListItem","position":2,"item":{"@id":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/potassium-fluoride-wikipedia\/#breadcrumbitem","name":"Potassium fluoride – Wikipedia"}}]}]