{{Use dmy dates|date=February 2025}} {{chembox | ImageFile = Potassium hypochlorite.svg | ImageFileL1 = Potassium-3D.png | ImageFileR1 = Hypochlorite-3D-vdW.png | ImageName = Potassium hypochlorite | OtherNames = {{ubl|Hypochlorous acid, potassium salt (1:1)<ref name=pubchem>{{cite web | url=https://pubchem.ncbi.nlm.nih.gov/compound/Potassium-hypochlorite | title=Potassium hypochlorite }}</ref>|Potassium chloroxide}} | IUPACName = Potassium hypochlorite | SystematicName = | Section1 = {{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 56409 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = G27K3AQ7DW | InChI = InChI=1/ClO.K/c1-2;/q-1;+1 | InChIKey = SATVIFGJTRRDQU-UHFFFAOYAH | SMILES = [K+].[O-]Cl | CASNo = 7778-66-7 | CASNo_Ref = {{cascite|correct|CAS}} | PubChem = 23665762 | UNNumber = 1791 | EINECS = 231-909-2 }} | Section2 = {{Chembox Properties | Formula=KOCl | K=1|O=1|Cl=1 | Appearance = Colorless liquid (light yellow when impure) (aqueous solution)<ref name=pubchem /> | Odor = Pungent irritating chlorine-like (aqueous solution)<ref name=pubchem /> | Density = 1.160 g/cm<sup>3</sup> | Solubility = 25%{{clarify|reason=Define "%"! Because it can be mass/mass, volume/volume, mol/mol, mass/volume or anything else! And we can't read the source author's mind, sorry!|date=March 2024}} | MeltingPtC = -2 | BoilingPtC = 102 | BoilingPt_notes = (decomposes) }} | Section3 = | Section4 = | Section5 = | Section6 = {{Chembox Pharmacology | ATCCode_prefix = D08 }} | Section7 = {{Chembox Hazards | ExternalSDS = [http://www.kasteelchemicals.com/tinymce/filemanager/files/pot_hypo.pdf MSDS ] | GHSPictograms = {{GHS07}}{{GHS09}} | GHSSignalWord = Warning | HPhrases = {{H-phrases|336|411}} | PPhrases = {{P-phrases|261|271|273|304+340|312|391|403+233|405|501}} }} | Section8 = {{Chembox Related | OtherAnions = {{ubl|Potassium chloride|Potassium chlorite|Potassium chlorate|Potassium perchlorate}} | OtherCations = {{ubl|Lithium hypochlorite|Sodium hypochlorite|Calcium hypochlorite|Barium hypochlorite|Silver hypochlorite}} |OtherCompounds = {{ubl|Hypochlorite|Chlorine monoxide|Hypochlorous acid|Methyl hypochlorite}} }} }}
'''Potassium hypochlorite''' is a chemical compound with the chemical formula {{chem2|KOCl|auto=1}}, also written as KClO. It is the potassium salt of hypochlorous acid. It consists of potassium cations ({{chem2|K+}}) and hypochlorite anions ({{chem2|−OCl}}). It is used in variable concentrations, often diluted in water solution. Its aqueous solutions are colorless liquids (light yellow when impure) that have a strong chlorine smell.<ref name=pubchem /> It is used as a biocide and disinfectant.<ref name=pubchem />
==Preparation== Potassium hypochlorite is produced by the disproportionation reaction of chlorine with a solution of potassium hydroxide:<ref>{{cite book|last1=Uri Zoller, Paul Sosis|title=Handbook of Detergents, Part F: Production|publisher=CRC Press|page=452|url=https://books.google.com/books?id=dXn3aB1DKk4C&pg=PA452|access-date=4 May 2016|isbn=9781420014655|date=20 November 2008}}</ref> :{{chem2|Cl2 + 2 KOH → KCl + KOCl + H2O}}
This is the traditional method, first used by Claude Louis Berthollet in 1789.<ref name="ullhyp">{{citation |author1=Helmut Vogt |author2=Jan Balej |author3=John E. Bennett |author4=Peter Wintzer |author5=Saeed Akhbar Sheikh |author6=Patrizio Gallone |contribution=Chlorine Oxides and Chlorine Oxygen Acids |title=Ullmann's Encyclopedia of Industrial Chemistry |edition=7th |publisher=Wiley |year=2007 |page=2|title-link=Ullmann's Encyclopedia of Industrial Chemistry}}</ref>
Another production method is electrolysis of potassium chloride solution. With both methods, the reaction mixture must be kept cold to prevent formation of potassium chlorate.
==Uses== Potassium hypochlorite is used for sanitizing surfaces as well as disinfecting drinking water. Because its degradation leaves behind potassium chloride rather than sodium chloride, its use has been promoted in agriculture, where addition of potassium to soil is desired.<ref name=envirotech>{{cite web|title=Enviro Klor: 12.5% POTASSIUM HYPOCHLORITE BLEACH ALTERNATIVE|url=http://www.envirotech.com/pdf/EnviroKlor.pdf|access-date=14 September 2014|archive-url=https://web.archive.org/web/20140915073111/http://www.envirotech.com/pdf/EnviroKlor.pdf|archive-date=15 September 2014|url-status=dead}}</ref>
==History== Potassium hypochlorite was first produced in 1789 by Claude Louis Berthollet in his laboratory located in Javel in Paris, France, by passing chlorine gas through a solution of potash lye. The resulting liquid, known as "''Eau de Javel''" ("Javel water"), was a weak solution of potassium hypochlorite. Due to production difficulties, the product was then modified using sodium instead of potassium, giving rise to sodium hypochlorite, widely used today as a disinfectant.
==Safety and toxicology== Like sodium hypochlorite, potassium hypochlorite is an irritant. It can cause severe damage on contact with the skin, eyes, and mucous membranes.<ref>[https://federalregister.gov/a/2011-4534 , Environmental Protection Agency].2 March 2011.</ref> Inhalation of a mist of KOCl can cause bronchus and lung irritation, difficulty breathing, and in severe cases pulmonary edema. Ingestion of strong concentrations can be lethal.<ref name=msds>{{cite web|title=Material Safety Data Sheet: Potassium Hypochlorite|url=http://www.kasteelchemicals.com/tinymce/filemanager/files/pot_hypo.pdf|website=kasteelchemicals.com/|access-date=15 September 2014}}</ref> Symptoms of contact or inhalation can be delayed.<ref name=pubchem />
Potassium hypochlorite is not considered to cause a fire or explosive hazards by itself.<ref name=msds /> However, it can react explosively with numerous chemicals, including urea, ammonium salts, methanol, acetylene, and many organic compounds. Heating and acidification can produce toxic chlorine gas.<ref name=chemicalbook>{{cite web|title=Potassium Hypochlorite|url=https://www.chemicalbook.com/ChemicalProductProperty_EN_CB8332697.htm|website=Chemical Book|access-date=15 September 2014}}</ref> Containers may explode upon exposure to heat.<ref name=pubchem /> Potassium hypochlorite forms highly explosive {{chem2|NCl3}} upon contact with urea or ammonia.<ref name=pubchem />
==References== {{reflist}}
{{Antiseptics and disinfectants}} {{Potassium compounds}} {{Hypochlorites}}
{{DEFAULTSORT:Potassium Hypochlorite}} Category:Potassium compounds Category:Hypochlorites Category:Antiseptics Category:Disinfectants Category:Oxidizing agents