Potassium permanganate

Potassium permanganate
Names
IUPAC name
Potassium manganate(VII)
Other names
Potassium permanganate
Chameleon mineral
Condy's crystals
Permanganate of potash
Hypermangan
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.874
EC Number 231-760-3
KEGG
RTECS number SD6475000
UN number 1490
Properties
KMnO4
Molar mass 158.034 g/mol
Appearance purplish-bronze-gray needles
magenta–rose in solution
Odor odorless
Density 2.703 g/cm3
Melting point 240 °C (464 °F; 513 K) (decomposes)
6.4 g/100mL (20 °C)
25 g/100mL (65 °C)
Solubility decomposes in alcohol and organic solvents
+20.0·10−6 cm3/mol
1.59
Structure
Orthorhombic
Thermochemistry
119.2 J/mol K
171.7 J K−1 mol−1
−813.4 kJ/mol
-713.8 kJ/mol
Pharmacology
D08AX06 (WHO) V03AB18 (WHO)
Hazards
GHS pictograms
NFPA 704
Lethal dose or concentration (LD, LC):
1090 mg/kg (oral, rat)[1]
Related compounds
Other anions
 Potassium manganite
Potassium manganate
Other cations
 Sodium permanganate
Ammonium permanganate
Related compounds
 Manganese heptoxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Potassium permanganate is an inorganic chemical compound and medication. As a medication it is used for cleaning wounds and dermatitis.[2]

It has the chemical formula KMnO4 and is a salt consisting of K+ and MnO−
4 ions. It is a strong oxidizing agent. It dissolves in water to give intensely pink or purple solutions, the evaporation of which leaves prismatic purplish-black glistening crystals.[3] In 2000, worldwide production was estimated at 30,000 tonnes.[4] In this compound, manganese is in the +7 oxidation state.

The wholesale cost in the developing world is about US$0.01 per gram of powder.[5] In the United Kingdom a 400 milligram tablet costs the NHS roughly £0.51.[2]

Uses

Almost all applications of potassium permanganate exploit its oxidizing properties.[4] As a strong oxidant that does not generate toxic byproducts, KMnO4 has many niche uses.

Medical uses

Potassium permanganate is used for a number of skin conditions.[6] This includes fungal infections of the foot, impetigo, pemphigus, superficial wounds, dermatitis, and tropical ulcers.[2][6] It is on the WHO Model List of Essential Medicines, the most important medications needed in a basic health system.[7]

Water treatment

Potassium permanganate is used extensively in the water treatment industry. It is used as a regeneration chemical to remove iron and hydrogen sulfide (rotten egg smell) from well water via a "Manganese Greensand" Filter. "Pot-Perm" is also obtainable at pool supply stores and is used additionally to treat waste water. Historically it was used to disinfect drinking water[8][9] and can turn the water pink.[10] It currently finds application in the control of nuisance organisms such as zebra mussels in fresh water collection and treatment systems.[11]

Synthesis of organic compounds

A solution of KMnO4 in water, in a volumetric flask

Aside from its use in water treatment, the other major application of KMnO4 is as a reagent for the synthesis of organic compounds.[12] Significant amounts are required for the synthesis of ascorbic acid, chloramphenicol, saccharin, isonicotinic acid, and pyrazinoic acid.[4]

Called Baeyer's reagent after the German organic chemist Adolf von Baeyer, KMnO4 is used in Qualitative organic analysis to test for the presence of unsaturation. The reagent is an alkaline solution of potassium permanganate. Reaction with double or triple bonds (-C=C- or -C≡C-) causes the color to fade from purplish-pink to brown. Aldehydes and formic acid (and formic acid esters) also give a positive test.[13] The test is antiquated.

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 KMnO4 is sometimes used as an oxidizing titrant for redox titrations (permanganometry). In a related way, it is used as a reagent to determine the Kappa number of wood pulp. For the standardization of KMnO4 solutions, reduction by oxalic acid is often used.[14]

Aqueous, acidic solutions of KMnO4 are used to collect gaseous mercury in flue gas during stationary source emissions testing.[15]

In histology, potassium permanganate was used as a bleaching agent.[16][17]

Fruit preservation

Ethylene absorbents extend storage time of bananas 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.[18][19][20]

Survival kits

Potassium permanganate is typically included in survival kits: as a fire starter (mixed with antifreeze from a car radiator or glycerol),[21][22][23] water sterilizer, and for creating distress signals on snow.[24]

Fire service

Potassium permanganate is used in the "plastic sphere dispensers" used to set backfires, burnouts, and controlled burns. Polymer spheres resembling 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.[25][26] Both handheld[26] and helicopter-[25] or boat-mounted[26] 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 MnO2 creates "hundred-year-old" or "ancient" looks on Hessian cloth (burlap), ropes, timber, and glass.[27]

History

In 1659, Johann Rudolf Glauber fused a mixture of the mineral pyrolusite (manganese dioxide, MnO2) 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.[28] This report represents the first description of the production of potassium permanganate.[29] 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.[30]

Early photographers used it as a component of flash powder. It is now replaced with other oxidizers, due to the instability of permanganate mixtures.

Preparation

Potassium permanganate is produced industrially from manganese dioxide, which also occurs as the mineral pyrolusite. The MnO2 is fused with potassium hydroxide and heated in air or with another source of oxygen, like potassium nitrate or potassium chlorate.[4] This process gives potassium manganate:

2 MnO2 + 4 KOH + O2 → 2 K2MnO4 + 2 H2O

(With sodium hydroxide, the end product is not sodium manganate but an Mn(V) compound, which is one reason the potassium permanganate is more commonly used than sodium permanganate. Furthermore, the potassium salt crystallizes better.[4])

The potassium manganate is then converted into permanganate by electrolytic oxidation in alkaline media:

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 acid conditions.[31] The chlorine oxidation reaction is

2 K2MnO4 + Cl2 → 2 KMnO4 + 2 KCl

And the acid-induced disproportionation reaction may be written as

3 K2MnO4 + 4 HCl → 2 KMnO4 + MnO2 + 2 H2O + 4 KCl

A weak acid such as carbonic acid is sufficient for this reaction:

3 K2MnO4 + 2 CO2 → 2 KMnO4 + 2 K2CO3 + MnO2

Permanganate salts may also be generated by treating a solution of Mn2+ ions with strong oxidants such as lead dioxide (PbO2), sodium bismuthate (NaBiO3), or peroxydisulphate. Tests for the presence of manganese exploit the vivid violet color of permanganate produced by these reagents.

Structure

KMnO4 forms orthorhombic crystals with constants: a = 910.5 pm, b = 572.0 pm, c = 742.5 pm. The overall motif is similar to that for barium sulfate, with which it forms solid solutions.[32] In the solid (as in solution), each MnO4− centres are tetrahedral. The Mn–O distances are 1.62 Å.[33]

Reactions

Organic chemistry

Dilute solutions of KMnO4 convert alkenes into diols (glycols). This behaviour is also used as a qualitative 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 (MnO2). In this context, it is sometimes called Baeyer's reagent. However, bromine serves better in measuring unsaturation (double or triple bonds) quantitatively, since KMnO4, 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:[34]

CH3(CH2)17CH=CH2 + 2 KMnO4 + 3 H2SO4 → CH3(CH2)17COOH + CO2 + 4 H2O + K2SO4 + 2 MnSO4

Potassium permanganate oxidizes aldehydes to carboxylic acids, such as the conversion of n-heptanal to heptanoic acid:[35]

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.[36]

5 C6H5CH3 + 6 KMnO4 + 9 H2SO4 → 5 C6H5COOH + 14 H2O + 3 K2SO4 + 6 MnSO4

Glycols and polyols are highly reactive toward KMnO4. 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.[21] Its sterilizing properties are another reason for inclusion of KMnO4 in a survival kit.

By itself, potassium permanganate does not dissolve in many organic solvents. If an organic solution of permanganate is desired, "purple benzene" may be prepared, either by treating a two phase mixture of aqueous potassium permanganate and benzene with a quaternary ammonium salt,[37] or by sequestering the potassium cation with a crown ether.[38]

Reaction with acids

Concentrated sulfuric acid reacts with KMnO4 to give Mn2O7, which can be explosive.[39] The reaction of permanganate with concentrated hydrochloric acid gives chlorine. The Mn-containing products from redox reactions depend on the pH. Acidic solutions of permanganate are reduced to the faintly pink manganese(II) ion (Mn2+) and water. In neutral solution, permanganate is only reduced by three electrons to give manganese dioxide (MnO2), wherein manganese is in a +4 oxidation state. This is the material that stains one's skin when handling KMnO4. KMnO4 spontaneously reduces in an alkaline solution to green K2MnO4, wherein manganese is in the +6 oxidation state.

A curious reaction occurs upon addition of concentrated sulfuric acid to potassium permanganate. 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 Mn2O7, this should only be attempted with great care.[40][41]

Thermal decomposition

Solid potassium permanganate decomposes when heated:

2KMnO4 → K2MnO4 + MnO2(s) + O2

Here, the oxidation state of manganese changes as the potassium permanganate (oxidation state +7) decomposes to potassium manganate (oxidation state +6) and manganese dioxide (oxidation state +4). Oxygen gas is also liberated.

Safety and handling

Potassium permanganate poses risks as an oxidizer.[42]

Contact with skin will result in a long lasting pinkish/purple stain.[43]

References

  1. ↑ Chambers, Michael. "ChemIDplus - 7722-64-7 - VZJVWSHVAAUDKD-UHFFFAOYSA-N - Potassium permanganate [USP:JAN] - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Archived from the original on 13 August 2014. Retrieved 9 May 2018.
  2. 1 2 3 British Medical Association; Royal Pharmaceutical Society (2015). British national formulary (69 ed.). p. 840. ISBN 9780857111562.
  3. ↑ Burriel, F.; Lucena, F.; Arribas, S. and Hernández, J. (1985), Química Analítica Cualitativa, p. 688, ISBN 84-9732-140-5.
  4. 1 2 3 4 5 Reidies, Arno H. (2002) "Manganese Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
  5. ↑ "Potassium Permanganate". International Drug Price Indicator Guide. Archived from the original on 22 January 2018. Retrieved 8 December 2016.
  6. 1 2 WHO Model Formulary 2008 (PDF). World Health Organization. 2009. pp. 295, 300. ISBN 9789241547659. Archived (PDF) from the original on 13 December 2016. Retrieved 8 January 2017.
  7. ↑ "19th WHO Model List of Essential Medicines (April 2015)" (PDF). WHO. April 2015. Archived (PDF) from the original on May 13, 2015. Retrieved May 10, 2015.
  8. ↑ Assembly of Life Sciences (U.S.). Safe Drinking Water Committee (1977). Drinking water and health, Volume 2. National Academies Press. p. 98. ISBN 978-0-309-02931-5. Retrieved 2016-09-13.
  9. ↑ Downey, Robyn and Barrington, Mike (28 February 2005) "Red faces over pink water", The Northern Advocate.
  10. ↑ "Onoway apologizes for 'alarming' pink tap water". CBC News. 7 March 2017. Archived from the original on 7 March 2017. Retrieved 8 March 2017.
  11. ↑ EPA Guidance Manual Alternative Disinfectants and Oxidants Archived 2016-10-01 at the Wayback Machine.. epa.gov
  12. ↑ Fatiadi, A. (1987). "The Classical Permanganate Ion: Still a Novel Oxidant in Organic Chemistry". Synthesis. 1987 (2): 85–127. doi:10.1055/s-1987-27859.
  13. ↑ "Chemistry and Biochemistry". www.chemistry.ccsu.edu. Archived from the original on 24 January 2013. Retrieved 9 May 2018.
  14. ↑ Kovacs KA, Grof P, Burai L, Riedel M (2004). "Revising the Mechanism of the Permanganate/Oxalate Reaction". J. Phys. Chem. A. 108 (50): 11026. Bibcode:2004JPCA..10811026K. doi:10.1021/jp047061u.
  15. ↑ Code of Federal Regulations(7-1-07) Edition, Title 40, Part 60, Appendix A-8, Method 29, Section 7.3.1
  16. ↑ Picken, MM. (Apr 2010). "Amyloidosis-where are we now and where are we heading?". Arch Pathol Lab Med. 134 (4): 545–51. doi:10.1043/1543-2165-134.4.545. PMID 20367306.
  17. ↑ Murphy CL, Eulitz M, Hrncic R, Sletten K, Westermark P, Williams T, Macy SD, Wooliver C, Wall J, Weiss DT, Solomon A (2001). "Chemical typing of amyloid protein contained in formalin-fixed paraffin-embedded biopsy specimens". Am. J. Clin. Pathol. 116 (1): 135–42. doi:10.1309/TWBM-8L4E-VK22-FRH5. PMID 11447744.
  18. ↑ Scott, KJ, McGlasson WB and Roberts EA (1970). "Potassium Permanganate as an Ethylene Absorbent in Polyethylene Bags to Delay the Ripening of Bananas During Storage". Australian Journal of Experimental Agriculture and Animal Husbandry. 10 (43): 237. doi:10.1071/EA9700237.
  19. ↑ Scott KJ, Blake, JR, Stracha, G, Tugwell, BL and McGlasson WB (1971). "Transport of Bananas at Ambient Temperatures using Polyethylene Bags". Tropical Agriculture (Trinidad). 48: 163–165.
  20. ↑ Scott, KJ & Gandanegara, S (1974). "Effect of Temperature on the Storage Life of bananas Held in Polyethylene Bags with an Ethylene Absorbent". Tropical Agriculture (Trinidad). 51: 23–26.
  21. 1 2 Gillis, Bob & Labiste, Dino. "Fire by Chemical Reaction". Archived from the original on 2015-09-24.
  22. ↑ "pssurvival.com" (PDF). pssurvival.com. Archived (PDF) from the original on 4 August 2016. Retrieved 9 May 2018.
  23. ↑ "Making Fire with Potassium Permanganate and Glycerin". thesurvivalcache. 3 November 2012. Archived from the original on 13 May 2016. Retrieved 13 September 2016.
  24. ↑ "Distress Signals". Evening Post. CXXI (107): 5. 7 May 1936. Archived from the original on 5 November 2011.
  25. 1 2 "Missoula Technology and Development Center: Aerial Ignition, Plastic Sphere Dispenser Description". www.fs.fed.us. Archived from the original on 26 April 2016. Retrieved 9 May 2018.
  26. 1 2 3 ""Wetland Warrior"". Dirty Jobs. Season 6. Episode 2.
  27. ↑ Brody, Ester (February 2000). "Victor DeLor contractor profile". PaintPRO. 2 (1). Archived from the original on 2008-07-23. Retrieved 2009-11-12. 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.
  28. ↑ Glauber, Johann Rudolph, Prosperitas Germaniae (The prosperity of Germany), part 3 (Amsterdam, (Netherlands): Johann Jansson, 1659), pp. 93–94. From pp. 93–94: " … 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." ( … 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.) Available at: Bavarian State Library Archived 2016-12-20 at the Wayback Machine. English translation: Glauber, John Rudolph with Christopher Packe, trans., The Works of the Highly Experienced and Famous Chymist, John Rudolph Glauber: … (London, England: Thomas Millbourn, 1689), p. 353. Archived 2012-01-07 at the Wayback Machine. The reaction that produced the color changes that Glauber observed in his solution of potassium permanganate and potassium manganate (K2MnO4) is now known as the "chemical chameleon".
  29. ↑ Weeks, Mary Elvira with Henry M. Leicester, ed., Discovery of the Elements, 6th ed. (Easton, Pennsylvania: Journal of Chemical Education, 1956), pp. 172–173.
  30. ↑ "Important Trade Mark Case". Otago Witness. 2 (2420): 53. 2 August 1900. Archived from the original on 4 March 2016.
  31. ↑ Walton, H. F. (1948) Inorganic Preparations. New York.
  32. ↑ "Handbook of Preparative Inorganic Chemistry" Brauer, E., Ed.; Academic: New York, 1963.
  33. ↑ Palenik, Gus J. (1967). "Crystal structure of potassium permanganate". Inorg. Chem. 6 (3): 503–507. doi:10.1021/ic50049a015.
  34. ↑ Donald G. Lee, Shannon E. Lamb, and Victor S. Chang (1990). "Carboxylic Acids from the Oxidation of Terminal Alkenes by Permanganate: Nonadecanoic Acid". Organic Syntheses. ; Collective Volume, 7, p. 397
  35. ↑ Ruhoff, John R. "n-Heptanoic acid". Organic Syntheses. ; Collective Volume, 2, p. 315
  36. ↑ Gardner KA, Mayer JM (1995). "Understanding C-H Bond Oxidations: H· and H- Transfer in the Oxidation of Toluene by Permanganate". Science. 269 (5232): 1849–51. Bibcode:1995Sci...269.1849G. doi:10.1126/science.7569922. PMID 7569922.
  37. ↑ Arthur W. Herriott (1977). "Purple benzene: Solubilization of anions in organic solvents". J. Chem. Educ. 54 (4): 229. Bibcode:1977JChEd..54Q.229H. doi:10.1021/ed054p229.1.
  38. ↑ Doheny, Anthony J., Jr. & Ganem, Bruce (1980). "Purple benzene revisited". J. Chem. Educ. 57 (4): 308. Bibcode:1980JChEd..57..308D. doi:10.1021/ed057p308.1.
  39. ↑ Cotton, F. A.; Wilkinson, G.; Murillo, C. A. and Bochmann, M. (1999). Advanced Inorganic Chemistry, 6th Edition. Wiley-VCH. ISBN 0-471-19957-5
  40. ↑ Barthel, H. & Duvinage, B. (2000). "Clemens Winkler. His Experiments with Ozone in 1892". Praxis der Naturwissenschaften, Chemie. 49: 18ff.
  41. ↑ Dzhabiev, T. S.; Denisov, N. N.; Moiseev, D. N. & Shilov, A. E. (2005). "Formation of Ozone During the Reduction of Potassium Permanganate in Sulfuric Acid Solutions". Russian Journal of Physical Chemistry. 79: 1755–1760.
  42. ↑ Bretherick, L.; Urben, P. G.; Pitt, Martin John (2007), Bretherick's Handbook of Reactive Chemical Hazards, 1 (7 ed.), Elsevier Academic Press, pp. 1811&ndash, 7, ISBN 0-12-373945-4
  43. ↑ Griffin, Sharin. "How to Remove Potassium Permanganate". livestrong.com. Archived from the original on 13 April 2018. Retrieved 9 May 2018.
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