Chemistry:Calcium permanganate
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| IUPAC name
Calcium dipermanganate[1]
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| Properties | |
| Ca(MnO4)2 | |
| Molar mass | 277.9493 g/mol |
| Appearance | purple crystals deliquesent |
| Density | 2.49 g/cm3 |
| Melting point | 140 °C (284 °F; 413 K) (decomposes, tetrahydrate) |
| tetrahydrate: 331 g/100 mL (14 °C) 338 g/100 mL (25 °C) | |
| Solubility | soluble in ammonium hydroxide decomposes in alcohol |
| Related compounds | |
Other cations
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Sodium permanganate Ammonium permanganate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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Calcium permanganate is an oxidizing agent and chemical compound with the chemical formula Ca(MnO4)2. This salt consists of the metal calcium and two permanganate ions.
Preparation
The salt is prepared from the reaction of potassium permanganate with calcium chloride[2] or from the reaction of aluminium permanganate with calcium oxide. It can also be prepared by reacting manganese dioxide with a solution of calcium hypochlorite and a little bit of calcium hydroxide to increase the pH level.[citation needed]
Uses
Calcium permanganate is used in the textile industry, for sterilization of water, and as a deodorizer.[2] It is believed to help whiten teeth.[3] It was formerly used as a component of rocket fuel by the Luftwaffe.[4]
Safety
It is noncombustible, but being a strong oxidizing agent, it will accelerate the burning of combustible material. If the combustible material is finely divided, the resulting mixture may be explosive. Contact with liquid combustible materials may result in spontaneous ignition. Contact with sulfuric acid may cause fires or explosions. Mixtures with acetic acid or acetic anhydride can explode if not kept cold. Explosions can occur when mixtures of calcium permanganate and sulfuric acid come into contact with benzene, carbon disulfide, diethyl ether, ethyl alcohol, petroleum, or other organic matter.[5]
See also
References
- ↑ "CALCIUM PERMANGANATE, CAS Number: 10118-76-0". http://www.chemindustry.com/chemicals/1005888.html.
- ↑ 2.0 2.1 Perry, Dale L. (2011). Handbook of Inorganic Compounds (2nd ed.). Boca Raton: Taylor & Francis. pp. 94–95. ISBN 978-1-4398-1461-1.
- ↑ "Permanganate containing whitening compositions and methods of their use" EP patent 1786352A1, issued 2005-08-23
- ↑ Van Pelt, Michel (2012). Rocketing into the future : the history and technology of rocket planes. New York: Springer. p. 60. ISBN 978-1-4614-3200-5.
- ↑ "Calcium permanganate Safety Data Sheet". https://www.echemi.com/sds/calcium-permanganate-pd180727113398.html.
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