View source for Potassium permanganate

{{cs1 config|name-list-style=vanc|display-authors=6}}
{{Chembox
| Verifiedfields = changed
| verifiedrevid = 464362108
| Name = Potassium permanganate
| ImageFile1 = KMnO4.svg
| ImageSize1 = 144px
| ImageClass1 = skin-invert
| ImageFile2 = Potassium-permanganate-2004-unit-cell-3D-balls.png
| ImageClass2 = bg-transparent
| ImageFile3 = Potassium-permanganate-sample.jpg
| ImageSize3 = 220px
| IUPACName = Potassium manganate(VII)
| SystematicName = Potassium permanganate
| OtherNames = {{Unbulleted list|Chameleon mineral|Condy's crystals|Permanganate of potash|Hypermangan|Purple potion powder|Permanganic acid, potassium salt<ref name="k821"/>|Purple salt<ref name="k821"/>}}
| Section1 = {{Chembox Identifiers
|CASNo = 7722-64-7
|CASNo_Ref = {{cascite|correct|CAS}}
|PubChem = 516875
|ChemSpiderID = 22810
|SMILES = [K+].[O-][Mn](=O)(=O)=O
|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
|StdInChI=1S/K.Mn.4O/q+1;;;;;-1
|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
|StdInChIKey = VZJVWSHVAAUDKD-UHFFFAOYSA-N
|RTECS = SD6475000
|KEGG_Ref = {{keggcite|correct|kegg}}
|KEGG = D02053
|UNNumber = 1490
|EINECS = 231-760-3
|DrugBank = DB13831
|UNII = 00OT1QX5U4
|ChEMBL = 3833305
|ChEBI = 231501
}}
| Section2 = {{Chembox Properties
|K=1|Mn=1|O=4
|Appearance = Purplish-bronze-gray needles<br /> purple in solution<ref name="Burriel_1985">{{cite book | vauthors = Burriel F, Lucena F, Arribas S, Hernández J | date = 1985 | title = Química Analítica Cualitativa | trans-title = Qualitative Analytical Chemistry | language = Spanish | page = 688 | publisher = Ediciones Paraninfo, S.A. | isbn = 84-9732-140-5}}</ref>
|Odor = odorless
|Density = 2.7 g/cm<sup>3</sup><ref name=crc>{{cite book | veditors = Haynes WM | year = 2011 | title = CRC Handbook of Chemistry and Physics | edition = 92nd | publisher = [[CRC Press]] | isbn = 978-1439855119| title-link = CRC Handbook of Chemistry and Physics}}</ref>{{rp|4.83}}
|MeltingPtC = 240
|MeltingPt_notes = (decomposes)
|Solubility = 76 g/L (25 °C)<ref name=crc/><br /> 250 g/L (65 °C)
|SolubleOther = soluble in organic solvents; decomposes in [[Alcohol (chemistry)|alcohol]]
|RefractIndex = 1.59
|MagSus = +20.0·10<sup>−6</sup> cm<sup>3</sup>/mol<ref name=crc/>{{rp|4.134}}
}}
| Section3 = {{Chembox Structure
|Structure_ref =<ref>{{cite journal | vauthors = Hocart R, Mathieu-Sicaud A | title = A stabilization factor in the polymorphism of ammonium nitrate | date = 1945 | journal = Comptes Rendus Hebdomadaires des Séances de l'Académie des Sciences | trans-journal = Weekly Reports of the Sessions of the Academy of Sciences | language = French | volume = 221 | pages = 261–263}}</ref>
|CrystalStruct = [[Orthorhombic]], [[Pearson symbol|oP24]]
|SpaceGroup = Pnma, No. 62
|LattConst_a = 0.909 nm
|LattConst_b = 0.572 nm
|LattConst_c = 0.741 nm
|UnitCellFormulas = 4
}}
| Section4 = {{Chembox Thermochemistry
|DeltaHf = −813.4 kJ/mol
|Entropy = 171.7 J&thinsp;K<sup>−1</sup>&thinsp;mol<sup>−1</sup>
|HeatCapacity = 119.2 J/mol K
|DeltaGf = −713.8 kJ/mol
}}
| Section5 = {{Chembox Pharmacology
|ATCCode_prefix = D08
|ATCCode_suffix = AX06
|ATC_Supplemental = {{ATC|V03|AB18}}
}}
| Section7 = {{Chembox Hazards
|GHSPictograms = {{GHS03}} {{GHS07}} {{GHS09}}
|NFPA-H = 2
|NFPA-F = 0
|NFPA-R = 2
|NFPA-S = OX
|LD50 = 1090 mg/kg (oral, rat)<ref>{{cite web|url=https://pubchem.ncbi.nlm.nih.gov/#tab/sidsrcname=ChemIDplus&query=7722-64-7&input_type=text|id = ChemIDplus – CAS: 7722-64-7 InChi: VZJVWSHVAAUDKD-UHFFFAOYSA-N | title = Potassium permanganate [USP:JAN] – Similar structures search, synonyms, formulas, resource links, and other chemical information. | vauthors = Chambers M | work = ChemIDplus: A Toxnet database | publisher = U.S. National Library of Medicine |access-date=9 May 2018|url-status=live|archive-url=http://archive.wikiwix.com/cache/20140813083010/https://chem.nlm.nih.gov/chemidplus/rn/7722-64-7|archive-date=13 August 2014}}</ref>
}}
| Section8 = {{Chembox Related
|OtherAnions = [[Potassium pertechnetate]]<br />[[Potassium perrhenate]]
|OtherCations = [[Sodium permanganate]]<br />[[Ammonium permanganate]]<br />[[Calcium permanganate]]<br />[[Silver permanganate]]
|OtherCompounds = [[Manganese heptoxide]]
|OtherFunction = [[Potassium hypomanganate]]<br />[[Potassium manganate]]
|OtherFunction_label = manganates
}}
}}
'''Potassium permanganate''' is an [[inorganic compound]] with the [[chemical formula]] KMnO<sub>4</sub>. It is a purplish-black crystalline salt, which dissolves in water as [[potassium ion|K<sup>+</sup>]] and [[permanganate|{{chem|MnO|4|-}}]] ions to give an intensely pink to purple solution.

Potassium permanganate is widely used in the [[chemical industry]] and [[laboratory|laboratories]] as a strong [[oxidizing agent]], and also traditionally [[potassium permanganate (medical use)|as a medication]] for [[dermatitis]], for cleaning [[wound]]s, and general [[disinfection]]. It is on the [[WHO Model List of Essential Medicines|World Health Organization's List of Essential Medicines]].<ref name="WHO21st">{{cite book |title=World Health Organization model list of essential medicines: 21st list 2019 |vauthors=((World Health Organization)) |publisher=World Health Organization |year=2019 |location=Geneva |hdl=10665/325771 |id=WHO/MVP/EMP/IAU/2019.06. License: CC BY-NC-SA 3.0 IGO |author-link=World Health Organization |hdl-access=free}}</ref> It has a great variety of niche uses such as [[biocide]] for [[water treatment]] purposes{{cn|date=September 2025}} and for [[Tanning (leather)|tanning]] and [[dyeing]] cloth.<ref name="k821"/> In 2000, worldwide production was estimated at 30,000 tons.{{cn|date=August 2025}}

It is also referred to as chameleon mineral, Condy's crystals, permanganate of potash, hypermangan, purple potion powder, permanganic acid (potassium salt),<ref name="k821"/> and purple salt.<ref name="k821"/>

==Properties==
Potassium permanganate is the potassium salt of the tetrahedral [[transition metal oxo complex]] [[permanganate]], in which four {{chem2|O(2-)}} ligands are bound to a [[Manganese|manganese(VII)]] center.{{citation needed|date=June 2023}} Potassium permanganate is odorless and slightly sweet and astringent in taste.<ref name="k821">{{cite book | last=Ash | first=Michael | title=Handbook of Preservatives | publisher=Synapse Info Resources | publication-place=Endicott, New York | date=2004 | isbn=978-1-890595-66-1 | page=502-503 | url=https://books.google.com/books?id=XZ2QB7bu5LwC | id={{Google Books|id=XZ2QB7bu5LwC|title=Handbook of Preservatives}}}}</ref> It is soluble in water, [[sulfuric acid]], [[acetic anhydride]], and [[benzonitrile]], but dissolves best in [[methanol]] and [[acetone]].<ref name="k821"/>

===Structure===
{{chem2|KMnO4}} forms [[orthorhombic]] crystals with constants: ''a'' = 910.5&nbsp;[[picometre|pm]], ''b'' = 572.0&nbsp;pm, ''c'' = 742.5&nbsp;pm. The overall motif is similar to that for [[barium sulfate]], with which it forms [[solid solution]]s.<ref>{{cite book | title = Handbook of Preparative Inorganic Chemistry | veditors = Brauer E | publisher = Academic Press | location = New York | date = 1963}}</ref> In the solid (as in solution), each {{chem2|MnO4−}} centre is tetrahedral. The Mn–O distances are 1.62&nbsp;Å.<ref>{{cite journal | vauthors = Palenik GJ | year = 1967 | title = Crystal structure of potassium permanganate | journal = Inorg. Chem. | volume = 6 | issue = 3| pages = 503–507 | doi = 10.1021/ic50049a015}}</ref>

===Color===
The purplish-black color of solid potassium permanganate, and the intensely pink to purple color of its solutions, is caused by its permanganate anion, which gets its color from a strong [[Charge-transfer band|charge-transfer absorption band]] caused by excitation of electrons from oxo ligand orbitals to empty orbitals of the manganese(VII) center.<ref>{{cite book | vauthors = Miessler GL, Fischer PJ, Tarr DA |edition=5th |date=2014 |title=Inorganic Chemistry |publisher=Pearson |page=430 |isbn=978-0321811059}}</ref> The crystal form can range from purple to black or gray, and has a blue metallic sheen.<ref name="k821"/>

==Medical uses==
{{Infobox drug
| container_only = yes
|DailyMedID = Potassium_permanganate
}}
{{Main|Potassium permanganate (medical use)}}

===Mechanism of action===
Potassium permanganate functions as a strong<ref name="k821"/> [[oxidizing agent]]. Through this mechanism it results in [[disinfection]], [[astringency]], and reduced odors.<ref name="Derm2017">{{cite web |title=Potassium permanganate |url=https://www.dermnetnz.org/topics/potassium-permanganate/ | publisher=DermNet New Zealand | accessdate=11 October 2017 |website=www.dermnetnz.org |language=en}}</ref><ref name="WHO Prescribing">{{cite book |date=1997 |title=WHO Model Prescribing Information | location=Drugs Used in Skin Diseases > Antiseptic agents > Potassium permanganate | url=http://apps.who.int/medicinedocs/en/d/Jh2918e/25.2.html |url-status=dead | archive-url=https://web.archive.org/web/20090706195746/http://apps.who.int/medicinedocs/en/d/Jh2918e/25.2.html | archive-date=July 6, 2009 |accessdate=12 October 2017 | publisher=WHO Medicines Publications and Documentation | publication-place=Geneva, Switzerland | isbn=92-4-140106-0 | id=NLM Classification 250 |lang=en,fr|pages=92-93 (PDF pages 98-99)}}</ref><ref name="k821"/>

===Clinical use===
Potassium permanganate is no longer the preferred treatment for dermatological conditions<ref name="Derm2017"/> and no form of it is labeled for human use by the [[US Food and Drug Administration]].<ref name="Yanong"/> It should never be taken internally, because it is highly toxic and corrosive to [[mucous membrane]]s and skin.<ref name="Maronn"/><ref name="FDA20172"/><ref name="Derm2017"/><ref name="Olson"/><ref name="k821"/>

{{Blockquote|text=Potassium Permanganate, U.S.P., has a limited topical efficacy against bacteria and fungi. Concentrations of 1:5000 or more are necessary for an effective bactericidal action, but they are irritating to tissues. Consequently, solutions of 1: 10,000 are usually used. However, up to an hour may be required to kill many bacteria, and some strains survive exposure to this concentration. For this reason, permanganate has been made obsolete by much superior antiseptic and antifungal drugs.|title=Permanganates |source=[[Goodman and Gilman's The Pharmacological Basis of Therapeutics]], [https://archive.org/details/goodmangilmansphe6good/page/974/mode/2up?q=permanganate Sixth Edition] (1980), p. 974}}

Traditionally potassium permanganate was prescribed for a number of [[skin condition]]s, including [[tinea pedis|fungal infections of the foot]], [[impetigo]], [[pemphigus]], superficial wounds, [[dermatitis]], and topical ulcers.<ref name="BNF69">{{cite book|title=British national formulary |date=2015|author1=British Medical Association|author2-link=Royal Pharmaceutical Society|author2=Royal Pharmaceutical Society|isbn=9780857111562|page=840|publisher=Pharmaceutical Press |edition=69|author1-link=British Medical Association}}</ref><ref name="WHO2008">{{cite book | title = WHO Model Formulary 2008 | year = 2009 | isbn = 9789241547659 | vauthors = ((World Health Organization)) | veditors = Stuart MC, Kouimtzi M, Hill SR | hdl = 10665/44053 | id=[https://archive.org/details/whomodelformular00unse/page/n1/mode/1up Internet Archive whomodelformular00unse] | author-link = World Health Organization | publisher = World Health Organization | hdl-access=free | pages=295, 300}} [https://www.who.int/publications/i/item/9789241547659 Also accessible via WHO Publications.]</ref><ref name="k821"/> [[Radioactive contamination]] of the skin could be cleaned with potassium permanganate<ref name="k821"/> and vigorous scrubbing. For topical ulcers it was used together with [[procaine benzylpenicillin]].<ref name="WHO2008" /> Typically it was used in skin conditions that produce a lot of liquid.<ref name="BNF69" /> It could be applied as a soaked dressing or a bath.<ref name="WHO2008"/> Petroleum jelly may be used on the nails before soaking to prevent their discoloration.<ref name="Ox2011">{{cite book | vauthors = Burge S, Wallis D | chapter = Medical Management | chapter-url = https://books.google.com/books?id=CDxsjyTSnawC&pg=PA592 |title=Oxford Handbook of Medical Dermatology |date=2011 |publisher=OUP Oxford |isbn=9780199558322 |page=592 |language=en}}</ref> For treating eczema, it was recommended using for only a few days at a time due to irritating the skin.<ref name="Nurse20033">{{cite web |date=5 August 2003 |title=Should potassium permanganate be used in wound care? |url=https://www.nursingtimes.net/clinical-archive/wound-care/should-potassium-permanganate-be-used-in-wound-care/205220.article |accessdate=12 October 2017 |website=Nursing Times |language=en}}</ref>

The [[US Food and Drug Administration]] does not recommend its use in the crystal or tablet form. It should only be used in a diluted liquid form.{{cn|date=August 2025}}

=== Historical use ===
Potassium permanganate was first made in the 1600s and came into common medical use at least as early as the 1800s.<ref name="Stout_2013">{{cite book | vauthors = Stout M |chapter-url=https://books.google.com/books?id=BIfEfqS8iKcC&pg=RA1-PT234 |title=The Complete Idiot's Guide to Aquaponic Gardening |date=2013 |publisher=Penguin |isbn=9781615643332 |page= 234 | chapter = Chapter 16 |language=en |url-status=live |archive-url= https://web.archive.org/web/20170116172606/https://books.google.ca/books?id=BIfEfqS8iKcC&pg=RA1-PT234 |archivedate=2017-01-16}}</ref> During [[World War I|World War&nbsp;I]] Canadian soldiers were given potassium permanganate (to be applied mixed with an ointment) in an effort to prevent [[sexually transmitted infections]].<ref>{{cite book | vauthors = González-Crussi F | chapter = Pestilence and Mankind | chapter-url = https://books.google.com/books?id=bKpBZi8uG8IC&pg=PA111 |title=A Short History of Medicine |date=2008 |publisher=Random House Publishing Group |isbn=9781588368218 |page=111 |language=en}}</ref> Some have attempted to bring about an [[abortion]] by putting it in the vagina, though this is not effective.<ref>{{cite book | vauthors = Solinger R | chapter = No Extras, Curbing Fertility During the Great Depression | chapter-url = https://books.google.com/books?id=Xe6gBwAAQBAJ&pg=PA120 |title=Pregnancy and Power: A Short History of Reproductive Politics in America |date=2005 |publisher=NYU Press |isbn=9780814741191 |page=120 |language=en}}</ref><ref>{{cite book |url=https://books.google.com/books?id=SbVRAQAAMAAJ |title=Code of Federal Regulations: Record 2: 2007- |date=2008 |publisher=U.S. General Services Administration, National Archives and Records Service, Office of the Federal Register |page=178 |language=en}}</ref><ref name="FDA20172">{{cite web |title=CFR – Code of Federal Regulations Title 21 |url=https://www.accessdata.fda.gov/scripts/cdrh/cfdocs/cfcfr/CFRSearch.cfm?fr=250.108 |archive-url=https://web.archive.org/web/20021129030705/http://www.accessdata.fda.gov/scripts/cdrh/cfdocs/cfCFR/CFRSearch.cfm?FR=250.108 |url-status=dead |archive-date=November 29, 2002 |accessdate=11 October 2017 | date=April 1, 2002 |website=CDRH Super Search | publisher= U.S. Food and Drug Administration, Center for Devices and Radiological Health | quote=(a) There have been a number of reports in the medical literature of serious injuries to women resulting from the misuse of potassium permanganate in an effort to induce abortion. Reports from physicians who have treated such cases show that the injuries are commonly caused by introducing tablets or crystals of potassium permanganate into the vagina. Experience with these cases shows that such use of potassium permanganate is not effective in producing abortion, but that instead the drug produces serious and painful injury to the walls of the vagina, causing ulcers, massive hemorrhage, and infection. Such dangerous and useless employment of potassium permanganate is apparently encouraged among the misinformed by the mistaken idea that the vaginal bleeding caused by the corrosive action of the drug indicates a termination of pregnancy, which it does not.}}</ref> Other historical uses have included an effort to wash out the stomach in those with [[strychnine]] or [[picrotoxin]] poisoning.<ref>{{cite web |title=Potassium permanganate definition {{!}} Drugs.com |url=https://www.drugs.com/dict/potassium-permanganate.html |accessdate=11 October 2017 |website=Drugs.com}}</ref>

=== Side effects ===
Side effects from [[Topical medication|topical]] use include irritation of the skin and discoloration of clothing.<ref name="WHO2008"/> A harsh burn on a child from an undissolved tablet has been reported.<ref name="Nurse20033"/> Higher concentration solutions can result in [[chemical burn]]s.<ref name="Olson">{{cite book | vauthors = Olson KR |url=https://books.google.com/books?id=ju7diy73Z2wC |title=Poisoning and Drug Overdose | edition = Sixth |date=2011 |publisher=McGraw Hill Professional |isbn=9780071716765 |page=121 |language=en}}</ref> Therefore, in 2015 the [[British National Formulary]] recommended 100&nbsp;mg be dissolved in a liter of water before use to form a 1:10,000 (0.01%) solution.<ref name="Nurse20033"/><ref name="BNF692">{{cite book |author1=[[British Medical Association]] |title=British national formulary |author2=[[Royal Pharmaceutical Society]] |date=2015 |isbn=9780857111562 |edition=69 |page=840|publisher=Pharmaceutical Press }}</ref><ref name="WHO2008"/> Wrapping the dressings soaked with potassium permanganate is not recommended.{{citation needed|date=October 2023}}

=== Toxicology ===

Potassium permanganate is [[toxic]] if taken by mouth.<ref name="Maronn">{{cite book | vauthors = Maronn ML, Bree AF, Siegfried EC, Zvulunov A, Waisbourd-Zinman O, Ben-Amitai D | chapter = Principles of treatment in pediatric dermatology | veditors = Schachner LA, Hansen RC | chapter-url=https://books.google.com/books?id=tAlGLYplkacC&pg=PA131 |title=Pediatric Dermatology E-Book |date=2011 |publisher=Elsevier Health Sciences |isbn=978-0723436652 |page=131 |language=en}}</ref><ref name="k821"/> Concentrated solutions when drunk have resulted in [[Acute Respiratory Distress Syndrome|acute respiratory distress syndrome]] or swelling of the airway.<ref name="Schonwald_2004">{{cite book | vauthors = Schonwald S | chapter = Potassium Chloride and Potassium Permanganate | veditors = Dart RC | chapter-url=https://books.google.com/books?id=BfdighlyGiwC&pg=PA904 |title=Medical Toxicology |date=2004 |publisher=Lippincott Williams & Wilkins |isbn=9780781728454 |pages=904–905 |language=en}}</ref> Effects may include [[nausea]], [[vomiting]], and [[shortness of breath]].<ref name="Patnaik_2007">{{cite book | vauthors = Patnaik P | chapter= Oxidizers | chapter-url=https://books.google.com/books?id=-CRRJBVv5d0C&pg=PA710 |title=A Comprehensive Guide to the Hazardous Properties of Chemical Substances |date=2007 |publisher=John Wiley & Sons |isbn=9780471714583 |page=710 |language=en}}</ref> If a sufficiently large amount (about 10 grams) is eaten death may occur.<ref name="Patnaik_2007" /> Concentrated solutions of potassium permanganate and repeated exposure cause skin corrosion and [[dermatitis]].<ref name="k821"/>

Recommended measures for those who have ingested potassium permanganate include [[gastroscopy]].<ref name="Schonwald_2004" /> [[Activated charcoal (medication)|Activated charcoal]] or medications to cause vomiting are not recommended. While medications like [[ranitidine]] and [[acetylcysteine]] may be used in toxicity, evidence for this use is poor.<ref name="Schonwald_2004" />

=== Pharmaceuticals ===
In the United States the FDA requires tablets of the medication to be sold by [[Medical prescription|prescription]].<ref name="FDA20172"/> Potassium permanganate, however, does not have FDA approved uses<ref name="Yanong">{{cite web | vauthors = Yanong RP, Francis-Floyd R, Petty BD | title=Therapeutic Considerations in Aquaculture | website=Merck Veterinary Manual | date=October 28, 2021 | url=https://www.merckvetmanual.com/exotic-and-laboratory-animals/aquaculture/therapeutic-considerations-in-aquaculture | access-date=August 27, 2025 | quote=A few compounds, including copper sulfate and potassium permanganate, are not FDA approved but are legally available for limited use in food fish under the category "regulatory action deferred" pending further study.}}</ref> and therefore non medical grade potassium permanganate is sometimes used for medical purposes.{{citation needed|date=May 2025}}

It is available under a number of [[brand names]] including Permasol, Koi Med Tricho-Ex, and Kalii permanganas RFF.<ref>{{cite web |title=Potassium Permanganate - Drugs.com |url=https://www.drugs.com/international/potassium-permanganate.html |accessdate=11 October 2017 |website=Drugs.com}}</ref> It is occasionally called "Condy's crystals".<ref name="Derm20172">{{cite web |title=Potassium permanganate | work = DermNet New Zealand |url=https://www.dermnetnz.org/topics/potassium-permanganate/ |accessdate=11 October 2017 |language=en}}</ref>

=== Veterinary medicine ===
Potassium permanganate may be used to prevent the spread of [[glanders]] among horses.<ref>{{cite book | vauthors = Scott DW, Miller WH | chapter = Bacterial Skin Diseases | chapter-url = https://books.google.com/books?id=f0-v1vOq3x4C&pg=PA168 |title=Equine Dermatology – E-Book | date = 2010 | publisher = Elsevier Health Sciences |isbn=978-1437709216 |page=168 |language=en}}</ref>

==Industrial and other uses==
Almost all applications of potassium permanganate exploit its [[Redox|oxidizing]] properties.<ref name="Ullmann" /> As a strong oxidant that does not generate toxic byproducts, KMnO<sub>4</sub> has many niche uses.{{citation needed|date=June 2023}}

===Water treatment===
[[File:Potassium permanganate colors the water below the station neutralizing rotenone treatment in Soda Butte Creek (36781332291).jpg|thumb|Potassium permanganate colors the water purple and neutralizes [[rotenone]] treatment in [[Soda Butte Creek]].]]Potassium permanganate is used extensively in the water treatment industry.{{sfn|Office of Water|1999|p=5-3}} It is used to remove [[iron]]{{sfn|Office of Water|1999|p=5-2–5-3}} and [[hydrogen sulfide]] (rotten egg smell) from [[water well|well]] water via a "manganese greensand" filter.{{cn|date=August 2025}} "Pot-Perm" is also obtainable at [[swimming pool|pool]] supply stores and is used additionally to treat wastewater.{{cn|date=August 2025}} Historically it was used to disinfect drinking water,<ref>{{cite book|isbn = 978-0-309-02931-5|page = 98|url = https://books.google.com/books?id=uVlQ_TUP-f0C&pg=PA98I|title=Drinking water and health, Volume 2|author=Assembly of Life Sciences (U.S.). Safe Drinking Water Committee|publisher = National Academies Press|year = 1977|access-date = 2016-09-13}}</ref><ref name="Northern Advocate">{{cite web | vauthors = Downey R, Barrington M | date = 28 February 2005 |url=http://www.northernadvocate.co.nz/local/news/red-faces-over-pink-water/3625948/ |archive-url=https://web.archive.org/web/20110719003200/http://www.northernadvocate.co.nz/local/news/red-faces-over-pink-water/3625948/ |archive-date=2011-07-19 | title = Red faces over pink water | work = The Northern Advocate}}</ref> though the EPA considers it a poor disinfectant.{{sfn|Office of Water|1999|p=5-1}} It can turn water a [[Fuchsia (color)|fuchsia]] or pink color.<ref>{{cite news|title=Onoway apologizes for 'alarming' pink tap water|url=http://www.cbc.ca/news/canada/edmonton/onoway-water-chemical-pink-1.4013808|access-date=8 March 2017|work=[[CBC News]]|date=7 March 2017|url-status=live|archive-url=https://web.archive.org/web/20170307225245/http://www.cbc.ca/news/canada/edmonton/onoway-water-chemical-pink-1.4013808|archive-date=7 March 2017}}</ref><ref name="Northern Advocate"/>{{sfn|Office of Water|1999|p=5-1, 5-11}} Modern hiking and survivalist guides advise against using potassium permanganate in the field because it is difficult to dose correctly.<ref name="Vogel">{{cite book|title=Trinkwasserversorgung in Extremsituationen|author= Johannes Vogel |date= 2014 |publisher= Paul Pietsch Verlage GmbH|isbn=978-3613507845|language=German}}</ref> 

====Fisheries and aquatic management====

Potassium permanganate is not FDA approved for use with food fish in the United States, however it is categorized under "regulatory action deferred" and is legal to use because the FDA considers it "low regulatory priority" and at low risk for adverse human health effects.<ref name="Yanong"/><ref>{{cite web | title=FDA Answers Your Questions about Fish Drugs | website=U.S. Food and Drug Administration | date=October 19, 2017 | url=https://www.fda.gov/animal-veterinary/animal-health-literacy/fda-answers-your-questions-about-fish-drugs#regulatorypriority | access-date=August 27, 2025}}</ref><ref>{{harvnb|Durborow|Mitchell|Crosby|1998|p=4}}: "At the time of this writing, FDA has also given copper sulfate (CuSO 4) and potassium permanganate (KMnO4) deferred status, which means that these treatments may be used without legal prosecution, but they may lose deferred status if evidence is found of any danger to the human consumer."</ref>

Potassium permanganate is a treatment for ''[[Ichthyophthirius multifiliis]]'' (commonly known as "ich") and [[protozoa]] (such as ''[[Trichodina]]''), which infect and usually kill freshwater aquarium fish.<ref>{{cite book | date=October 2003 | vauthors = Durborow RM |title=SRAC Publications: Diseases |chapter=Protozoan Parasites |url=https://srac.tamu.edu/categories/view/26 |chapter-url=https://srac.tamu.edu/fact-sheets/serve/171 |location= |publisher=Southern Regional Aquaculture Center, Department of Rangeland, Wildlife and Fisheries Science, [[Texas A&M University]] & USDA [[National Institute of Food and Agriculture]] (NIFA) |page= |isbn= |access-date= | id=SRAC Publication No. 4701}}</ref> A minimum dose of 2 [[Parts-per-million|ppm]] is required. Water with more organic load and a higher number of organisms including [[algae]] requires more permanganate. High concentrations and use more than once per week kill fish. Food fish require a 7-day period after treatment before they can be consumed.<ref>{{harvnb|Durborow|Mitchell|Crosby|1998|p=5}}</ref><ref name="Yanong"/>

An alternative application is in the control of nuisance organisms such as [[zebra mussel]]s{{sfn|Office of Water|1999|p=5-3}} in freshwater collection and treatment systems.{{cn|date=August 2025}}

[[Rotenone]] can be deactivated in water with the use of potassium permanganate to lower toxicity to acceptable levels. A 1:1 ratio of permanganate to rotenone is insufficient to deactivate rotenone in most situations.<ref>{{harvnb|Cailteux, et al.|p=5-8}}</ref>

===Synthesis of organic compounds===<!-- [[Baeyer's reagent]] redirects to this section -->
[[File:Difuzija KMN05.JPG|thumb|upright|KMnO<sub>4</sub> in water]]
A major application of KMnO<sub>4</sub> is as a reagent for the synthesis of organic compounds.<ref>{{cite journal| vauthors = Fatiadi A |title = The Classical Permanganate Ion: Still a Novel Oxidant in Organic Chemistry|year = 1987|journal = [[Synthesis (journal)|Synthesis]]|volume = 1987|issue = 2|pages = 85–127|doi = 10.1055/s-1987-27859| s2cid=94121246}}</ref> Significant amounts are required for the synthesis of [[ascorbic acid]], [[chloramphenicol]], [[saccharin]], [[isonicotinic acid]], and [[pyrazinoic acid]].<ref name="Ullmann" />

KMnO<sub>4</sub> is used in [[qualitative organic analysis]] to test for the presence of [[Saturated and unsaturated compounds|unsaturation]]. It is sometimes referred to as '''Baeyer's reagent''' after the German organic chemist [[Adolf von Baeyer]]. The reagent is an alkaline solution of potassium permanganate. Reaction with double or triple bonds ({{chem2|R2C\dCR2}} or {{chem2|R\sC\tC\sR}}) causes the color to fade from purplish-pink to brown. [[Aldehyde]]s and [[formic acid]] (and [[formate]]s) also give a positive test.<ref>{{cite web | vauthors = Glagovich N | date = 2013 | work = Department of Chemistry and Biochemistry | publisher = Central Connecticut State University |url= http://www.chemistry.ccsu.edu/glagovich/teaching/316/qualanal/tests/baeyertest.html|title=Baeyer Test |access-date=9 May 2018 |url-status=dead |archive-url= https://web.archive.org/web/20130124005821/http://www.chemistry.ccsu.edu/glagovich/teaching/316/qualanal/tests/baeyertest.html |archive-date=24 January 2013}}</ref> The test is antiquated.
[[Image:Baeyer's Probe Alkenes V.2.svg|class=skin-invert-image|center|550px|Baeyer's reagent reaction]]

KMnO<sub>4</sub> solution is a common [[thin layer chromatography]] (TLC) stain for the detection of oxidizable functional groups, such as alcohols, aldehydes, alkenes, and ketones. Such compounds result in a white to orange spot on TLC plates.<ref>{{cite web | title = Thin Layer Chromatography stains | url = http://www.reachdevices.com/TLC_stains.html | work =  REACH Devices, LLC }}</ref><ref>{{cite book | vauthors = Jork H, Funk W, Fischer W, Wimmer H | date = 1990 | title = Thin-Layer Chromatography: Reagents and Detection Methods | volume = 1A | publisher = VCH | location = Weinheim | isbn = 3-527-278834}}</ref><ref>{{cite book | vauthors = Jork H, Funk W, Fischer W, Wimmer H | date = 1990 | title = Thin-Layer Chromatography: Reagents and Detection Methods | volume = 1B | publisher = VCH | location = Weinheim | isbn = 3-527-278834}}</ref>

===Analytical use===
Potassium permanganate can be used to quantitatively determine the total oxidizable organic material in an aqueous sample. The value determined is known as the ''permanganate value.'' In [[analytical chemistry]], a standardized [[aqueous]] solution of KMnO<sub>4</sub> is sometimes used as an oxidizing [[titration|titrant]] for [[redox titration]]s ([[permanganometry]]). As potassium permanganate is titrated, the solution becomes a light shade of purple, which darkens as excess of the titrant is added to the solution. In a related way, it is used as a [[reagent]] to determine the [[Kappa number]] of wood pulp. For the standardization of KMnO<sub>4</sub> solutions, reduction by [[oxalic acid]] is often used.<ref>{{cite journal|title = Revising the Mechanism of the Permanganate/Oxalate Reaction|vauthors=Kovacs KA, Grof P, Burai L, Riedel M |journal = J. Phys. Chem. A|doi = 10.1021/jp047061u|year = 2004|volume = 108|page = 11026|issue = 50|bibcode = 2004JPCA..10811026K |url=https://infoscience.epfl.ch/handle/20.500.14299/2553 |doi-access = free}}</ref> In agricultural chemistry, it is used for estimation of active [[carbon]]<!-- not quite the meaning of the [[active carbon]] article --> in soil.<ref>{{cite web |url= https://vro.agriculture.vic.gov.au/dpi/vro/vrosite.nsf/pages/soilhealth_potassium-permanganate |title= Quick Reference Guide: Potassium Permanganate Test for Active Carbon |website= Agriculture Victoria—Victorian Resources Online |date= August 2025 |publisher= [[Victoria, Australia]]}}</ref>

Aqueous, acidic solutions of KMnO<sub>4</sub> are used to collect gaseous [[mercury (element)|mercury]] in flue gas during stationary source emissions testing.<ref>[[Code of Federal Regulations]](7-1-07) Edition, [[Title 40 of the United States Code|Title 40]], Part 60, Appendix A-8, Method 29, Section 7.3.1</ref>

In [[histology]], potassium permanganate was used as a bleaching agent.<ref name="Picken_2010">{{cite journal | vauthors = Picken MM | title = Amyloidosis-where are we now and where are we heading? | journal = Archives of Pathology & Laboratory Medicine | volume = 134 | issue = 4 | pages = 545–551 | date = April 2010 | pmid = 20367306 | doi = 10.5858/134.4.545}}</ref><ref name="Murphy_2001">{{cite journal | vauthors = Murphy CL, Eulitz M, Hrncic R, Sletten K, Westermark P, Williams T, Macy SD, Wooliver C, Wall J, Weiss DT, Solomon A | title = Chemical typing of amyloid protein contained in formalin-fixed paraffin-embedded biopsy specimens | journal = American Journal of Clinical Pathology | volume = 116 | issue = 1 | pages = 135–142 | date = July 2001 | pmid = 11447744 | doi = 10.1309/TWBM-8L4E-VK22-FRH5 | doi-access = free}}</ref>

===Fruit preservation===
[[Ethylene]] absorbents extend storage time of [[banana]]s even at high temperatures. This effect can be exploited by packing bananas in [[polyethylene]] together with potassium permanganate. By removing ethylene by oxidation, the permanganate delays the ripening, increasing the fruit's shelf life up to 4 weeks without the need for refrigeration.<ref>{{cite journal| vauthors = Scott KJ, McGlasson WB, Roberts EA |title=Potassium Permanganate as an Ethylene Absorbent in Polyethylene Bags to Delay the Ripening of Bananas During Storage|journal= Australian Journal of Experimental Agriculture and Animal Husbandry |doi=10.1071/EA9700237|volume=10|issue=43|page= 237|year=1970}}</ref><ref>{{cite journal| vauthors = Scott KJ, Blake, JR, Stracha, G, Tugwell, BL and McGlasson WB |year=1971|title= Transport of Bananas at Ambient Temperatures using Polyethylene Bags|journal= Tropical Agriculture (Trinidad)|volume= 48|pages= 163–165}}</ref><ref>{{cite journal| vauthors = Scott KJ, Gandanegara S |year=1974|title= Effect of Temperature on the Storage Life of bananas Held in Polyethylene Bags with an Ethylene Absorbent|journal= Tropical Agriculture (Trinidad)|volume= 51|pages=23–26}}</ref>

The chemical reaction, in which [[ethylene]] (C<sub>2</sub>H<sub>4</sub>) is oxidised by potassium permanganate (KMnO<sub>4</sub>) to [[carbon dioxide]] (CO<sub>2</sub>), [[manganese oxide]] (MnO<sub>2</sub>) and [[potassium hydroxide]] (KOH), in the presence of water, is presented as follows:<ref>{{cite journal | title=Current scenario of adsorbent materials used in ethylene scavenging systems to extend fruit and vegetable postharvest life |vauthors=Álvarez-Hernández MH, Artés-Hernández F, Ávalos-Belmontes F, Castillo- Campohermoso MA, Contreras-Esquivel JC, Ventura-Sobrevilla JM, Martínez-Hernández GB | journal=Food Bioproc Technol | date=2018 | volume=11 |issue=3 | pages=511–525 | doi=10.1007/s11947-018-2076-7}}</ref>

3 C<sub>2</sub>H<sub>4</sub> + 12 KMnO<sub>4</sub> + 2 H<sub>2</sub>O → 6 CO<sub>2</sub> + 2 H<sub>2</sub>O + 12 MnO<sub>2</sub> + 12 KOH

===Survival kits===
Potassium permanganate is sometimes included in survival kits: as a [[hypergolic]] fire starter (when mixed with [[glycerol]] antifreeze from a car radiator);<ref name="Bob Gillis and Dino Labiste">{{cite web |url=http://www.primitiveways.com/chemical_fire.html |title=Fire by Chemical Reaction | vauthors = Gillis B, Labiste D |url-status=live |archive-url= https://web.archive.org/web/20150924081745/http://www.primitiveways.com/chemical_fire.html |archive-date=2015-09-24 | work = PrimitiveWays}}</ref><ref>{{cite web|url=http://pssurvival.com/PS/Chemistry/Uses_of_Potassium_Permanganate_2010.pdf#page=1|title=Potassium Permanganate |website=Pole Shift Survival Information |access-date=9 May 2018|url-status=dead|archive-url=https://web.archive.org/web/20160804172658/http://www.pssurvival.com/PS/Chemistry/Uses_of_Potassium_Permanganate_2010.pdf#page=1|archive-date=4 August 2016}}</ref><ref>{{cite web |url=http://thesurvivalcache.weebly.com/thesurvivalcaches-blog/making-fire-with-potassium-permanganate-and-glycerin |title=Making Fire with Potassium Permanganate and Glycerin |work=thesurvivalcache |date=3 November 2012 |access-date=13 September 2016 |url-status=live |archive-url=https://web.archive.org/web/20160513141530/http://thesurvivalcache.weebly.com/thesurvivalcaches-blog/making-fire-with-potassium-permanganate-and-glycerin |archive-date=13 May 2016}}</ref> as a water sterilizer; and for creating distress signals on snow.<ref>{{cite journal |url=http://paperspast.natlib.govt.nz/cgi-bin/paperspast?a=d&d=EP19360507.2.20 |title=Distress Signals |journal=Evening Post |volume=CXXI |issue=107 |date=7 May 1936 |page=5 |url-status=live |archive-url=https://web.archive.org/web/20111105110817/http://paperspast.natlib.govt.nz/cgi-bin/paperspast?a=d&d=EP19360507.2.20 |archive-date=5 November 2011}}</ref> Modern hiking and survivalist guides advise against using potassium permanganate in the field because it is difficult to dose correctly.<ref name="Vogel"/>

===Fire service===
[[File:Delayed aerial ignition devices containing potassium permanganate 02.jpg|thumb|Delayed aerial ignition devices containing potassium permanganate.]]Potassium permanganate is added to "plastic sphere dispensers" to create backfires, burnouts, and [[controlled burn]]s. Polymer spheres resembling [[Table tennis#Ball|ping-pong balls]] containing small amounts of permanganate are injected with [[ethylene glycol]] and projected towards the area where ignition is desired, where they spontaneously ignite seconds later.<ref name=usfs>{{cite web|url=http://www.fs.fed.us/eng/aerial_ign/plsphere/describe.htm| work = Missoula Technology and Development Center | publisher = USDA Forest Service | title = Aerial Ignition, Plastic Sphere Dispenser Description |access-date=9 May 2018|url-status=dead |archive-url= https://web.archive.org/web/20160426215606/http://www.fs.fed.us/eng/aerial_ign/plsphere/describe.htm |archive-date=26 April 2016}}</ref><ref name=dj>{{Cite episode |title= Wetland Warrior |series=[[Dirty Jobs]]|season=6 |number=2}}</ref> Both handheld{{r|dj}} helicopter-{{r|usfs}} unmanned aircraft systems (UAS) or boat-mounted{{r|dj}} plastic sphere dispensers are used.

===Other uses===
Potassium permanganate is one of the principal chemicals used in the film and television industries to "age" props and set dressings. Its ready conversion to brown [[Manganese dioxide|MnO<sub>2</sub>]] creates "hundred-year-old" or "ancient" looks on [[hessian cloth]] (burlap), ropes, timber and glass.<ref>{{cite journal|url = http://www.paintpro.net/Articles/PP201/PP201-Contractor_Profile.cfm|title = Victor DeLor contractor profile|access-date = 2009-11-12| vauthors = Brody E |journal = PaintPRO |volume = 2|issue = 1|date = February 2000|quote = One of the techniques DeLor is known for among designers and clients is the special effects he creates with various chemical solutions. When applied to wood surfaces, these chemicals give a weathered appearance to new wood. ... To achieve the aesthetic on interior surfaces, DeLor often uses a mixture of water and potassium permanganate, a dry powder chemical.|url-status = live|archive-url = https://web.archive.org/web/20080723213651/http://www.paintpro.net/Articles/PP201/PP201-Contractor_Profile.cfm|archive-date = 2008-07-23}}</ref>{{primary source inline|date=August 2025}}

Potassium permanganate is used as an [[oxidizing agent]] in the synthesis of [[cocaine]] and [[methcathinone]].<ref>{{cite journal | vauthors = Binder R, Machata G, Stead H | title = [Analysis of potassium permanganate as addictive drug "precursor"] | journal = Archiv für Kriminologie | volume = 211 | issue = 5–6 | pages = 160–165 | date = May 2003 | pmid = 12872685}}</ref> It can purify [[cocaine paste]] with oxidization to increase its stability. This led to the [[Drug Enforcement Administration]] launching Operation Purple in 2000, with the goal of monitoring the world supply of potassium permanganate; however, potassium permanganate derivatives and substitutes were soon used thereafter to avoid the operation.<ref>{{cite news |url=https://www.vice.com/en/article/the-cash-is-in-the-cut/ |publisher=[[Vice Media]] |title=The Terrifying Substances People Put in Cocaine | vauthors = Gosmer K, Vammen M |date=March 10, 2014}}</ref>

==History==
[[File:A solution of Potassium Permanganate being poured into a well in an Indian village to disinfect its water.jpg|thumb|Treating a well with potassium permanganate in India (1949).]]In 1659, [[Johann Rudolf Glauber]] fused a mixture of the mineral [[pyrolusite]] (manganese dioxide, MnO<sub>2</sub>) and [[potassium carbonate]] to obtain a material that, when dissolved in water, gave a green solution ([[potassium manganate]]) which slowly shifted to violet and then finally red.<ref>{{cite book | vauthors = Glauber JR | title = ''Prosperitas Germaniae'' | trans-title = The prosperity of Germany, part 3 | location = Amsterdam, Netherlands | publisher = Johann Jansson | date = 1659 | pages = 93–94 | quote = ''… donec tandem Magnesiam istam nitro fixo permixtam, in crucibulo forti coctione a nitro reseratam vidi, unde elegans color purpureus provenit, massam hanc effusam in pulvere redegi, aqua calida extraxi, per filtrum liquorem transmisi. Tandem vero elegantissimum purpureum, igneumque liquorem accepi, qui fere singulis horis in frigore tantummodo consistens colorem permutavit, sic ut jam viridis, jam caerulei, jam sanguinei coloris sponte sua factus sit, mox iterum alios elegantissimos colores receperit.'' | trans-quote = … until finally I saw [that] by mixing that ''magnesia'' [i.e., ''magnesia nigra'', [[pyrolusite]], the ore containing [[manganese dioxide]] ] with fixed [[niter]] [i.e., inert niter, potassium carbonate], by cooking [it] in a strong crucible, [the colored compound was] released by the niter, whence a fine purple color arises; this mass [was] poured out, reduced to powder, extracted with hot water, [and] the solution passed through a filter. Then I got a truly most elegant, purple, and fiery solution, which nearly every hour ([while] standing just in the cold) changed color, so that it was spontaneously made now green, now blue, now red in color; soon again it received other most elegant colors.}}</ref><ref>{{cite web |vauthors=Glauber JR |title=Prosperitatis Germaniae pars .... 3: In qua Salpetrae ex variis ubiq, obviis subiectis facillime atque copiose extrahendi modus traditur. Eiusve utilitates summae declarantur |trans-title=Part of the Prosperity of Germany .... 3: In which the method of extracting saltpeter from various everywhere, in the most convenient and abundant manner, is given. His interests are clearly stated |url=https://www.digitale-sammlungen.de/en/view/bsb10915847?page=100 |archive-url=https://web.archive.org/web/20161220151825/http://reader.digitale-sammlungen.de/en/fs1/object/display/bsb10915847_00100.html |archive-date=2016-12-20 |language=Latin |via=Bavarian State Library }}</ref><ref>Translated in: {{cite book |url=https://archive.org/stream/worksofhighlyexp00glau#page/352/mode/2up |title=The Works of the Highly Experienced and Famous Chymist, John Rudolph Glauber |vauthors=Glauber JR |date=1689 |publisher=Thomas Millbourn |location=London, England |page=353 |translator-last1=Packe C |archive-url=https://web.archive.org/web/20120107040133/http://www.archive.org/stream/worksofhighlyexp00glau |archive-date=2012-01-07}}</ref> The reaction that produced the color changes that Glauber observed in his solution of potassium permanganate and potassium manganate (K<sub>2</sub>MnO<sub>4</sub>) is now known as the "[[chemical chameleon]]".<ref>{{Cite web | vauthors = Chen J |date=2024-01-19 |title=How to use Chameleon Pigment for Chameleon Paint? |url=https://www.kingchroma.com/uses/how-to-use-chameleon-pigment-for-chameleon-paint |access-date=2024-06-07 |language=en-US}}</ref>

The case of the chameleon mineral alludes to a broader reflection on how epistemological framework dictates what early modern scientists perceived as meaningful discoveries.<ref>{{Cite journal | vauthors = Weeks ME, Leicester H, Dains FB | title = Discovery of the elements | journal = Journal of Chemical Education | volume = 6 | pages = 12 | date = 1956 | url = https://onlinebooks.library.upenn.edu/webbin/book/lookupid?key=olbp82411 }}</ref>  Little literature exists on Glauber’s accidental discovery of potassium permanganate and the importance of both its dismissal and its conversion into a modern medical and hygienic staple.  

The earliest description of the production of potassium permanganate is here.<ref>{{cite book | vauthors = Weeks ME | veditors = Leicester HM | title = Discovery of the Elements | edition = 6th | location = Easton, Pennsylvania | publisher = Journal of Chemical Education | date = 1956 | url = https://archive.org/stream/discoveryoftheel002045mbp#page/n185/mode/2up | pages = 172–173}}</ref> Just under 200 years later, London chemist [[Henry Bollmann Condy]] had an interest in disinfectants; he found that fusing pyrolusite with [[sodium hydroxide]] (NaOH) and dissolving it in water produced a solution with disinfectant properties. He patented this solution, and marketed it as 'Condy's Fluid'. Although effective, the solution was not very stable. This was overcome by using [[potassium hydroxide]] (KOH) rather than NaOH. This was more stable, and had the advantage of easy conversion to the equally effective potassium permanganate crystals. This crystalline material was known as 'Condy's crystals' or 'Condy's powder'. Potassium permanganate was comparatively easy to manufacture, so Condy was subsequently forced to spend considerable time in litigation to stop competitors from marketing similar products.<ref>{{cite journal |date=2 August 1900 |title=Important Trade Mark Case |url=http://www.paperspast.natlib.govt.nz/cgi-bin/paperspast?a=d&d=OW19000802.2.357 |url-status=live |journal=Otago Witness |volume=2 |issue=2420 |page=53 |archive-url=https://web.archive.org/web/20160304003229/http://paperspast.natlib.govt.nz/cgi-bin/paperspast?a=d&d=OW19000802.2.357 |archive-date=4 March 2016}}</ref> According to [[Varlam Shalamov]], potassium permanganate solution was used as a catch-all treatment for dysentery, frostbite and ulcers in the Gulag camps of Kolyma.

Early photographers used it as a component of [[flash powder]]. It is now replaced with other oxidizers, due to the instability of permanganate mixtures.{{citation needed|date=June 2023}}

== Preparation ==
Potassium permanganate is produced industrially from [[manganese dioxide]], which also occurs as the mineral [[pyrolusite]]. In 2000, worldwide production was estimated at 30,000 tonnes.<ref name="Ullmann">{{Ullmann|vauthors = Reidies AH |year=2002|title=Manganese Compounds|doi=10.1002/14356007.a16_123}}</ref> The MnO<sub>2</sub> is fused with [[potassium hydroxide]] and heated in [[air]] or with another source of oxygen, like [[potassium nitrate]] or [[potassium chlorate]].<ref name="Ullmann"/> This process gives [[potassium manganate]]:
:{{chem2 | 2 MnO2 + 4 KOH + O2 -> 2 K2MnO4 + 2 H2O }}

With sodium hydroxide, the end product is not [[sodium manganate]] but a Mn(V) compound, which is one reason why the potassium permanganate is more commonly used than [[sodium permanganate]]. Furthermore, the potassium salt crystallizes better.<ref name="Ullmann"/>

The potassium manganate is then converted into permanganate by [[electrolysis|electrolytic oxidation]] in alkaline media:
:{{chem2 | 2 K2MnO4 + 2 H2O -> 2 KMnO4 + 2 KOH + H2 }}

===Other methods===
Although of no commercial importance, potassium manganate can be oxidized by [[chlorine]] or by [[disproportionation]] under acidic conditions.<ref>{{cite book | vauthors = Walton HF | date = 1948 | title = Inorganic Preparations | location = New York | publisher = Prentice-Hall | pages = 150–151}}</ref> The chlorine oxidation reaction is
:{{chem2 | 2 K2MnO4 + Cl2 -> 2 KMnO4 + 2 KCl }}

and the acid-induced disproportionation reaction may be written as
:{{chem2 | 3 K2MnO4 + 4 HCl -> 2 KMnO4 + MnO2 + 2 H2O + 4 KCl }}

A weak acid such as [[carbonic acid]] is sufficient for this reaction:
:{{chem2 | 3 K2MnO4 + 2 CO2 -> 2 KMnO4 + 2 K2CO3 + MnO2 }}

Permanganate salts may also be generated by treating a solution of Mn<sup>2+</sup> ions with strong oxidants such as [[lead dioxide]] (PbO<sub>2</sub>), [[sodium bismuthate]] (NaBiO<sub>3</sub>), or [[peroxydisulfate]]. [[Qualitative inorganic analysis|Tests]] for the presence of manganese exploit the vivid violet color of permanganate produced by these reagents.

==Reactions==
===Organic chemistry===
Dilute solutions of KMnO<sub>4</sub> convert [[alkene]]s into [[diol]]s. This behaviour is also used as a [[qualitative chemical analysis|qualitative]] [[chemical test|test]] for the presence of double or triple bonds in a molecule, since the reaction decolorizes the initially purple [[permanganate]] solution and generates a brown precipitate (MnO<sub>2</sub>). In this context, it is sometimes called ''Baeyer's reagent''. However, [[bromine]] serves better in measuring unsaturation (double or triple bonds) quantitatively, since KMnO<sub>4</sub>, being a very strong [[oxidizing agent]], can react with a variety of groups.

Under acidic conditions, the alkene double bond is cleaved to give the appropriate [[carboxylic acid]]:<ref>{{OrgSynth|title = Carboxylic Acids from the Oxidation of Terminal Alkenes by Permanganate: Nonadecanoic Acid| vauthors = Lee DG, Lamb SE, Chang VS |collvol = 7 |collvolpages = 397 |year = 1990 |prep = cv7p0397}}</ref>
:{{chem2 | CH3(CH2)17CH\dCH2 + 2 KMnO4 + 3 H2SO4 -> CH3(CH2)17COOH + CO2 + 4 H2O + K2SO4 + 2 MnSO4 }}

Potassium permanganate oxidizes aldehydes to carboxylic acids, illustrated by the conversion of ''n''-[[heptanal]] to heptanoic acid:<ref>{{OrgSynth| vauthors = Ruhoff JR |title = ''n''-Heptanoic acid |collvol = 2 |collvolpages = 315 |prep = cv2p0315}}</ref>
:{{chem2 | 5 C6H13CHO + 2 KMnO4 + 3 H2SO4 -> 5 C6H13COOH + 3 H2O + K2SO4 + 2 MnSO4 }}

Even an alkyl group (with a benzylic hydrogen) on an [[aromatic ring]] is oxidized, e.g. [[toluene]] to [[benzoic acid]].<ref>{{cite journal | vauthors = Gardner KA, Mayer JM | title = Understanding C-H bond oxidations: H. and H- transfer in the oxidation of toluene by permanganate | journal = Science | volume = 269 | issue = 5232 | pages = 1849–1851 | date = September 1995 | pmid = 7569922 | doi = 10.1126/science.7569922 | bibcode = 1995Sci...269.1849G}}</ref>
:{{chem2 | 5 C6H5CH3 + 6 KMnO4 + 9 H2SO4 -> 5 C6H5COOH + 14 H2O + 3 K2SO4 + 6 MnSO4 }}

Glycols and [[polyol]]s are highly reactive toward KMnO<sub>4</sub>. For example, addition of potassium permanganate to an aqueous solution of [[sugar]] and [[sodium hydroxide]] produces the [[chemical chameleon]] reaction, which involves dramatic color changes associated with the various oxidation states of [[manganese]]. A related vigorous reaction is exploited as a fire starter in survival kits. For example, a mixture of potassium permanganate and [[glycerol]] or pulverized [[glucose]] ignites readily.<ref name="Bob Gillis and Dino Labiste"/> Its sterilizing properties are another reason for inclusion of KMnO<sub>4</sub> in a survival kit.{{citation needed|date=June 2023}}

===Ion exchange===
Treating a mixture of aqueous potassium permanganate with a [[quaternary ammonium salt]] results in ion exchange, precipitating the quat salt of permanganate. Solutions of these salts are sometimes soluble in organic solvents:<ref>{{cite journal | title = Purple benzene: Solubilization of anions in organic solvents | vauthors = Herriott AW | journal = J. Chem. Educ. | year = 1977 | volume = 54 | issue = 4 | page = 229 | doi = 10.1021/ed054p229.1| bibcode = 1977JChEd..54Q.229H}}</ref>
:{{chem2 | KMnO4 + R4NCl -> R4NMnO4 + KCl }}

Similarly, addition of a [[crown ether]] also gives a lipophilic salt.<ref>{{Cite journal | vauthors = Doheny Jr AJ, Ganem B | title = Purple benzene revisited | journal = J. Chem. Educ. | year = 1980 | volume = 57 | page = 308 | doi = 10.1021/ed057p308.1 | issue = 4|bibcode=1980JChEd..57..308D}}</ref>

===Reaction with acids and bases===
Permanganate reacts with concentrated [[hydrochloric acid]] to give [[chlorine]] and manganese(II):
:{{chem2 | 2 KMnO4 + 16 HCl -> 2 MnCl2 + 5 Cl2 + 2 KCl + 8 H2O }}

In [[pH|neutral]] solution, permanganate slowly reduces to [[manganese dioxide]] (MnO<sub>2</sub>). This is the material that stains one's skin when handling KMnO<sub>4</sub>.

KMnO<sub>4</sub> reduces in [[alkaline]] solution to give green [[potassium manganate|K<sub>2</sub>MnO<sub>4</sub>]]:<ref>{{cite book | doi = 10.1002/9780470132425.ch11 | vauthors = Nyholm RS, Woolliams PR | title = Inorganic Syntheses |author-link=Ronald Sydney Nyholm | chapter = Manganates (VI) | year = 1968 | volume = 11 | pages = 56–61 | isbn = 978-0-470-13242-5}}</ref>
:{{chem2 | 4 KMnO4 + 4 KOH -> 4 K2MnO4 + O2 + 2 H2O }}
This reaction illustrates the relatively rare role of hydroxide as a reducing agent.

Addition of concentrated sulfuric acid to potassium permanganate gives [[manganese(VII) oxide|Mn<sub>2</sub>O<sub>7</sub>]].<ref>{{cite book | vauthors = Cotton FA, Wilkinson G, Murillo CA, Bochmann M | date = 1999 | title = Advanced Inorganic Chemistry | edition = 6th | publisher = Wiley-VCH | isbn = 0-471-19957-5}}</ref> Although no reaction may be apparent, the vapor over the mixture will ignite paper impregnated with alcohol. Potassium permanganate and sulfuric acid react to produce some [[ozone]], which has a high oxidizing power and rapidly oxidizes the alcohol, causing it to combust. As the reaction also produces explosive Mn<sub>2</sub>O<sub>7</sub>, this should only be attempted with great caution.<ref>{{cite journal| vauthors = Barthel H, Duvinage B |title = Clemens Winkler. His Experiments with Ozone in 1892|journal = Praxis der Naturwissenschaften, Chemie |year = 2000|volume = 49|pages = 18ff}}</ref><ref>{{cite journal | vauthors = Dzhabiev TS, Denisov NN, Moiseev DN, Shilov AE |title = Formation of Ozone During the Reduction of Potassium Permanganate in Sulfuric Acid Solutions|journal = Russian Journal of Physical Chemistry|year = 2005|volume = 79|pages = 1755–1760}}</ref>

===Thermal decomposition===
Solid potassium [[permanganate]] decomposes when heated:<ref name="k821"/>
:{{chem2 | 2 KMnO4 -> K2MnO4 + MnO2 + O2 }}
It is a redox reaction.{{cn|date=September 2025}}

==Safety and handling==
Potassium permanganate poses risks as a strong<ref name="k821"/> [[oxidizer]].<ref name="Bretherick_2007">{{cite book | vauthors = Bretherick L, Urben PG, Pitt MJ | year = 2007 | title = Bretherick's Handbook of Reactive Chemical Hazards | edition = 7th | volume = 1| publisher = Elsevier Academic Press| isbn = 978-0-12-373945-2 | pages = 1811–7| title-link = Bretherick's Handbook of Reactive Chemical Hazards}}</ref> Contact with skin can cause skin irritation, skin and mucous membrane corrosion,<ref name="k821"/> and in some cases severe allergic reaction.{{cn|date=September 2025}} It is poisonous to humans and animals, and ingestion may lead to respiratory failure.<ref name="Schonwald_2004"/> It is incompatible with organic and readily oxidized materials and poses a violent reaction and explosion hazard. It is flammable during some chemical reactions and emits toxic fumes when burning.<ref name="k821"/>

It can also result in discoloration and clothing stains.<ref>{{cite web |url= https://www.livestrong.com/article/74289-remove-potassium-permanganate/ |title=How to Remove Potassium Permanganate| vauthors = Griffin S |website=livestrong.com|access-date=9 May 2018|url-status=deviated|archive-url= https://web.archive.org/web/20180413125030/https://www.livestrong.com/article/74289-remove-potassium-permanganate/|archive-date=13 April 2018}}</ref>

== References ==
{{Reflist}}

=== Bibliography ===
* {{cite book | author=Office of Water | url = https://nepis.epa.gov/Exe/ZyPDF.cgi/2000229L.PDF?Dockey=2000229L.PDF#page=179 | title = Alternative Disinfectants and Oxidants Guidance Manual | date = April 1999 | chapter=5. Potassium Permanganate | archive-url = https://web.archive.org/web/20250222013343/https://nepis.epa.gov/Exe/ZyPDF.cgi/2000229L.PDF?Dockey=2000229L.pdf | archive-date=February 22, 2025 | publisher = [[U.S. Environmental Protection Agency]] | id=EPA 815-R-99-014}} [https://nepis.epa.gov/Exe/ZyNET.exe/2000229L.TXT?ZyActionD=ZyDocument&Client=EPA&Index=1995+Thru+1999&Docs=&Query=&Time=&EndTime=&SearchMethod=1&TocRestrict=n&Toc=&TocEntry=&QField=&QFieldYear=&QFieldMonth=&QFieldDay=&IntQFieldOp=0&ExtQFieldOp=0&XmlQuery=&File=D%3A%5Czyfiles%5CIndex%20Data%5C95thru99%5CTxt%5C00000015%5C2000229L.txt&User=ANONYMOUS&Password=anonymous&SortMethod=h%7C-&MaximumDocuments=1&FuzzyDegree=0&ImageQuality=r75g8/r75g8/x150y150g16/i425&Display=hpfr&DefSeekPage=x&SearchBack=ZyActionL&Back=ZyActionS&BackDesc=Results%20page&MaximumPages=1&ZyEntry=1&SeekPage=x&ZyPURL# Access this document via National Service Center for Environmental Publications (NSCEP), pubnumber 815R99014]
* {{cite book | vauthors = Durborow RM, Mitchell AJ, Crosby MD | year = 1998 |title=SRAC Publications: Diseases |chapter=Ich (White Spot Disease) |url=https://srac.tamu.edu/categories/view/26 |chapter-url=https://srac.tamu.edu/fact-sheets/serve/123 |location= |publisher=Southern Regional Aquaculture Center, Department of Rangeland, Wildlife and Fisheries Science, [[Texas A&M University]] & USDA [[National Institute of Food and Agriculture]] (NIFA) |page= |isbn= |access-date= | id=SRAC Publication No. 476}}
*{{cite book |veditors=Cailteux RL, etal |title=Rotenone in Fisheries: Are the Rewards Worth the Risks? |date=2001 |url=https://fisheries.org/docs/books/55042P/com.pdf |archive-url=https://web.archive.org/web/20250828000708/https://fisheries.org/docs/books/55042P/com.pdf |archive-date=August 28, 2025 |url-status=live |publisher=American Fisheries Society |
isbn=1-888569-33-6 |lccn=2001093337 |location=Bethesda, Maryland}}

== Further reading ==
{{refbegin}}
* {{cite thesis | vauthors = Hopkins AJ | title = The Reaction Between Manganese Dioxide and Potassium Permanganate. | degree = Doctor of Philosophy | publisher = Johns Hopkins University | date = 1893 | url = https://www.gutenberg.org/ebooks/74154 }}
* {{cite web | url = http://www.npi.gov.au/resource/manganese-compounds | work = National Pollutant Inventory | title = Manganese and compounds Fact Sheet | publisher = Department of Climate Change, Energy, the Environment and Water | location = Australia}}
* {{cite web | vauthors = Lazur AM |url=http://edis.ifas.ufl.edu/fa032 |archive-url=https://web.archive.org/web/20110606090007/http://edis.ifas.ufl.edu/fa032 |archive-date=2011-06-06 | title = The use of potassium permanganate in fish ponds | date = 2009 | work = IFAS Extension | location = Gainesville, FL | publisher = University of Florida}}
{{refend}}

== External links ==
* {{ICSC|0672|06}}

{{Permanganates}}
{{Manganese compounds}}
{{Potassium compounds}}
{{Antiseptics and disinfectants}}
{{Antidotes}}
{{Organic reactions}}
{{portal bar|Medicine}}

[[Category:Potassium compounds]]
[[Category:Permanganates]]
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