Silver permanganate
| Names | |
|---|---|
| IUPAC name
Silver(I) permanganate
| |
| Other names
Argentous permanganate
Silver(I) manganate(VII) | |
| Properties | |
| AgMnO4 | |
| Molar mass | 226.804 g/mol |
| Appearance | Purple or black solid |
| Odor | Odorless |
| Density | 4.50 g/cm3 (25 °C)[1] |
| Melting point | 160 °C (320 °F; 433 K) (decomposition) |
| Boiling point | Decomposes |
| 0.55 g/100 ml (0 °C) 1.69 g/100 ml (30 °C) | |
| Solubility | Reacts with acids, bases Insoluble in diethyl ether |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
42.717 J·mol-1·K-1[2] |
| Hazards | |
| Safety data sheet | ColonialMetals |
| Flash point | Non-flammable |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver permanganate is an inorganic compound with the chemical formula AgMnO4.
Contents
Properties
Chemical
It decomposes when heated and heating to high temperature may lead to explosion.
Silver permanganate forms a coordination complex with pyridine, bispyridinesilver permanganate, a useful and stable oxidizing reagent for organic reactions. More precisely, it's obtained by adding pyridine to an aq. solution of potassium permanganate, followed by addition of an aq. sol. of silver nitrate.[3]
Physical
Silver permanganate is a purple of black solid, poorly soluble in water. It decomposes at around 160 °C, but some sources give temperatures as low as 100-135 °C.[4]
Availability
Silver permanganate is somewhat difficult to find, as most chemical suppliers will not sell it.
Preparation
It can be produced through the reaction of silver nitrate and potassium permanganate:[5] Sodium permanganate, if available, can also be used.[6]
- AgNO3 + KMnO4 → AgMnO4 + KNO3
Due to its low solubility, silver permanganate will precipitate out of the solution.
Another possible route involves the addition of barium permanganate to silver perchlorate.
- 2 AgClO4 + Ba(MnO4)2 → 2 AgMnO4 + Ba(ClO4)2
Projects
- Make ammonium permanganate
- Preparation of other metal permanganates by double displacement with their chlorides
Handling
Safety
Silver permanganate is a strong oxidizer and it will stain badly.
Storage
Should not be stored for long.
Disposal
Can be reduced to silver metal and manganese dioxide using a reducing agent. The silver should be recycled, while manganese dioxide can either be recovered or dumped in the manganese waste.
References
- ↑ Chang, Fung Ming; Jansen, Martin; Zeitschrift fur Kristallographie; ; vol. 169; (1984); p. 295 - 298
- ↑ Zhuk, N. P.; Zhurnal Fizicheskoj Khimii; vol. 28; (1954); p. 1690 - 1697; C.A.; (1956); p. 31
- ↑ H. Firouzabadi, B. Vessal, M. Naderi, Tetrahedron Letters, Volume 23, Issue 17, 1982, Pages 1847-1850
- ↑ Goldstein, M. K.; Flanagan, T. B.; Journal of Chemical Education; vol. 41; (1964); p. 276 - 277
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann
- ↑ Sajó, István E.; Kovács, Gréta B.; Pasinszki, Tibor; Bombicz, Petra A.; May, Zoltán; Szilágyi, Imre M.; Jánosity, Anna; Banerji, Kalyan K.; Kant, Rajni; Kótai, László; Journal of Coordination Chemistry; vol. 71; nb. 16-18; (2018); p. 2884 - 2904
