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| Potassium permanganate | |
|---|---|
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| IUPAC name | Potassium manganate(VII) |
| Other names | Potassium permanganate, Chameleon mineral, Condy's crystals |
| Identifiers | |
| CAS number | [7722-64-7] |
| PubChem | |
| KEGG | |
| SMILES |
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| Properties | |
| Molecular formula | KMnO4 |
| Molar mass | 158.04 g/mol |
| Appearance | purplish-bronze-gray needles; magenta–rose in solution |
| Density | 2.703 g/cm³, solid |
| Melting point |
270 °C decomp. |
| Solubility in water | 6.38 g/100 ml at 20 °C |
| Structure | |
| Crystal structure | Orthorhombic |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-813.4 kJ.mol-1 |
| Standard molar entropy S |
171.7 J.K-1.mol-1 |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Oxidant (O), Harmful (Xn), Dangerous for the environment (N) |
| NFPA 704 |
 0
2
0
OX
|
| R-phrases | R8, R22, R50/53 |
| S-phrases | (S2), S60, S61 |
| Related compounds | |
| Other cations | Sodium permanganate |
| Related compounds | Potassium manganate (K2MnO4); Manganese heptoxide; |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Potassium permanganate is the chemical compound KMnO4. In this salt, manganese is in the +7 oxidation state. The salt is also known as "permanganate of potash." The permanganate ion is a strong oxidizing agent. It dissolves in water to give deep purple solutions, evaporation of which gives prismatic purplish-black glistening crystals.[1] In 2000, worldwide production was estimated at 30 000 t/a.[2]
It forms orthorhombic crystals with constants: a = 9.105, b = 5.720, c = 7.425 Å. The Mn-O bond distances are 1.629 Å.
Contents |
Preparation
Potassium permanganate is manufactured on a large scale from manganese dioxide (pyrolusite, the mineral) is fused with potassium hydroxide and heated in air or with potassium nitrate (a source of oxygen). This process gives potassium manganate, which upon electrolytic oxidation in alkaline solution gives potassium permanganate.
- MnO2 + 2OH− + O2 → MnO42− + H2O
- MnO42− + Cl2 → MnO4− + 2Cl−
Permanganates can also be generated by treating a solution of Mn2+ ions with very strong oxidising agents like lead dioxide, PbO2, or sodium bismuthate, NaBiO3, and these reactions have been used to test for the presence of manganese due to the vivid violet colour of permanganate.
Uses
Almost all applications of potassium permanganate are derived from it being an oxidizing agent.[2] As a strong oxidant that does not generate toxic by products, KMnO4 has many niche uses.
Disinfectant and water treatment
As an oxidant, potassium permanganate can act as a disinfectant. For example, dilute solutions are used as a treatment for canker sores (ulcers), disinfectant for the hands and treatment for mild pompholyx, dermatitis, and fungal infections of the hands or feet.citation needed Potassium permanganate, obtainable at pool supply stores, is used in rural areas to remove iron and hydrogen sulfide (rotten egg smell) from well and waste water.
Biomedical uses
Related to the use of KMnO4 for water treatment, this salt is often employed as a specialized disinfectant for treating human and animal ailments. It has been used to induce abortions, although with risks.[3] In histology to bleach melanin which obscures tissue detail. Potassium permanganate can also be used to differentiate amyloid AA from other types of amyloid pathologically deposited in body tissues. Incubation of fixed tissue with potassium permanganate will prevent amyloid AA from staining with congo red whereas other types of amyloid are unaffected.[4][5]
Organic synthesis
Aside from its use in water treatment, the other major applicaton of KMnO4 is as a reagent for the synthesis of organic compounds.[6] Significant amounts are required for the synthesis of ascorbic acid, chloramphenicol, saccharine, isonicotinic acid, and pyrazinoic acid.[2]
Analytical chemistry
Potassium permanganate can also be used to quantitatively determine the total oxidisable 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. In a related way, it is used as a reagent to determine the Kappa number of wood pulp.
Aqueous, acidic solutions of KMnO4 are used to collect gaseous mercury in flue gas during stationary source emissions testing.[7]
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 permanganate solution; thus it is sometimes referred to as 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 impurities in a sample.
Under acidic conditions, the alkene double bond is cloven to give the appropriate carboxylic acid:[8]
- CH3(CH2)17CH=CH2 + [O] → CH3(CH2)17COOH
Potassium permanganate oxidizes aldehydes to carboxylic acids, such as the conversion of n-heptanal to heptanoic acid:[9]
- C6H13CHO + [O] → C6H13COOH
Even alkyl group (with a benzylic hydrogen) on an aromatic ring are oxidized, e.g. toluene to benzoic acid.
Glycols are highly reactive toward KMnO4. And this vigorous reaction is used in survival kits as a fire starter. For example, a mixture of potassium permanganate and glycerol or pulverized glucose ignites readily. Its sterilizing properties are another reason for inclusion of KMnO4 in a survival kit.[10] In a related application, it is used for artistic purposes as an agent to prepare paper for fast bleaching. Lemon juice is enough to quickly remove colour from the paper and applied with a paint brush this can create interesting aesthetics.
Acids and KMnO4
Concentrated sulfuric acid reacts with KMnO4 to give Mn2O7, which can be explosive.[11][12][13] Similarly 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) sulfate ([Mn(H2O)62+). In neutral solution, permanganate is only reduced by 3e− to give MnO2, wherein Mn is in a +4 oxidation state. This is the material that stains one's skin when handling KMnO4. KMnO4 spontaneously reduced in an alkaline solution to green K2MnO4, wherein manganese is in the +6 oxidation state. Potassium permanganate and sulfuric acid react to produce some ozone, which has a high oxidising power and rapidly oxidises the alcohol, causing it to combust. As a similar reaction produces explosive Mn2O7, this should only be attempted with great care. An approximate equation for the ozone formation is shown below.
- 6 KMnO4(aq) + 9 H2SO4(aq) → 6 MnSO4(aq) + 3 K2SO4(aq) + 9 H2O(l) + 5 O3(g)
History
In 1659 a German chemist, J.R. Glauber, fused a mixture of the mineral pyrolusite and potassium carbonate to obtain a material that, when dissolved in water, gave a green solution (potassium manganate) which slowly shifted to violet potassium permanganate and then finally red. This report represents the first description of the production of potassium permanganate.[14] Just under two hundred years later London chemist Henry Bollmann Condy had an interest in disinfectants, and marketed several products including ozonised water. He found that fusing pyrolusite with 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 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 in order to stop competitors from marketing products similar to Condy's Fluid or Condy's Crystals.
Early photographers used it as a component of flash powder. It is now replaced with other oxidizers, due to the instability of permanganate mixtures. Aqueous solutions of KMnO4 have been used together with T-Stoff (i.e. 80% hydrogen peroxide) as propellant for the rocket plane Messerschmitt Me 163. In this application, it was known as Z-Stoff. This combination of propellants is sometimes still used in torpedoes.
Safety
Solid KMnO4 is a strong oxidizer and in general it should be kept separated from oxidizable substances. Reaction with concentrated sulfuric acid produces the highly explosive manganese(VII) oxide (Mn2O7). As an oxidizer, potassium permanganate stains the hand and clothing as it is reduced to brown MnO2. It is also used as antidote for some poisons, on which it acts by oxidizing them.
References
- ^ F. Burriel, F. Lucena, S. Arribas and J. Hernández, (1985), Química Analítica Cualitativa, page 688, ISBN 84-9732-140-5.
- ^ a b c Arno H. Reidies "Manganese Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
- ^ Obeng, B. B. (1968). "The lay use of potassium permanganate as an abortifacient". Br J Clin Pract 22 (11): 465–9. PMID 5696512.
- ^ Wright, J. R.; Calkins E.; Humphrey R. L. (1977). "Potassium permanganate reaction in amyloidosis. A histologic method to assist in differentiating forms of this disease". Lab Invest. 36 (3): 274–81. PMID 839739.
- ^ van Rijswijk, M. H.; van Heusden, C. W. (1979). "The potassium permanganate method. A reliable method for differentiating amyloid AA from other forms of amyloid in routine laboratory practice". Am J Pathol. 97 (1): 43–58. PMID 495695.
- ^ A. Fatiadi (1987). "The Classical Permanganate Ion: Still a Novel Oxidant in Organic Chemistry" (review). Synthesis 1987 (2): 85–127. doi:.
- ^ Code of Federal Regulations(7-1-07) Edition,Title 40, Part 60, Appendix A-8, Method 29, Section 7.3.1
- ^ Donald G. Lee, Shannon E. Lamb, and Victor S. Chang (1990). "Carboxylic Acids from the Oxidation of Terminal Alkenes by Permanganate: Nonadecanoic Acid". Org. Synth.; Coll. Vol. 7: 397.
- ^ John R. Ruhoff. "n-Heptanoic acid". Org. Synth.; Coll. Vol. 2: 315.
- ^ Bob Gillis and Dino Labiste. "Chemical Fire".
- ^ F. A. Cotton, G. Wilkinson, C. A. Murillo, and M. Bochmann (April 1999). Advanced Inorganic Chemistry, 6th Edition. Wiley-VCH. ISBN 0-471-19957-5
- ^ Barthel, H. and Duvinage, B. (2000). "Clemens Winkler. His Experiments with Ozone in 1892". Praxis der Naturwissenschaften, Chemie 49: 18ff.
- ^ Dzhabiev, T. S.; Denisov, N. N.; Moiseev, D. N. and 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.
- ^ Weeks, M. E. and Leicester, H. M.; Discovery of the Elements, Journal of Chemical Education 1968
External links
- International Chemical Safety Card 0672
- National Pollutant Inventory: Manganese and compounds Fact Sheet
- The use of potassium permanganate in fish ponds
- Sugar, NaOH and KMnO4
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- This page was last modified on 11 July 2008, at 20:01.
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