Barium permanganate
| Identifiers | |
|---|---|
7787-36-2  | |
| 3D model (Jmol) | Interactive image |
| ECHA InfoCard | 100.029.191 |
| EC Number | 232-110-1 |
| PubChem | 24587 |
| |
| |
| Properties | |
| Ba(MnO4)2[1] | |
| Molar mass | 375.198 g/mol |
| Appearance | dark violet to brown crystals |
| Odor | odorless |
| Density | 3.77 g/cm3 |
| Melting point | 200 °C (392 °F; 473 K) (decomposes) |
| 62.5 g/100 mL (29 °C) | |
| Solubility | decomposes in alcohol |
| Structure | |
| rhombic | |
| Hazards | |
| NFPA 704 | |
| Related compounds | |
| Other cations |
Magnesium permanganate Strontium permanganate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium permanganate is a chemical compound, with the formula Ba(MnO4)2. [2]
Preparation
Barium permanganate may be produced by disproportionation of barium manganate in a mildly acidic solution,[3] or by oxidation of barium manganate with strong oxidants. Preparations relying on aqueous reactions of barium manganate are extremely slow process due to the low solubility of the manganate.[3]
Reactions
Permanganic acid can be prepared by the reaction of dilute sulfuric acid with a solution barium permanganate, the insoluble barium sulfate byproduct being removed by filtering:[3]
- Ba(MnO4)2 + H2SO4 → 2 HMnO4 + BaSO4
The sulfuric acid used must be dilute; reactions of permanganates with concentrated sulfuric acid yield the anhydride, manganese heptoxide.
References
- ↑ Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. p. 4-50. ISBN 978-1-4200-9084-0.
- ↑ PubChem
- 1 2 3 Olsen, J. C. (1900). Permanganic Acid by Electrolysys. Easton, PA: The Chemical Publishing Company.
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