Manganese(II) nitrate
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| Names | |
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| Systematic IUPAC name
Manganese(II) nitrate | |
| Other names
Manganese dinitrate
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.741 |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 2724 |
CompTox Dashboard (EPA)
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| Properties | |
| Mn(NO3)2 | |
| Molar mass | 178.95 g/mol |
| Appearance | white powder |
| Density | 1.536 g/cm3 |
| Melting point | 37 °C (99 °F; 310 K) |
| Boiling point | 100 °C (212 °F; 373 K) |
| 118 g/100 ml(10oC) | |
| Related compounds | |
Other anions
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Manganese chloride |
Other cations
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Magnesium nitrate Calcium nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Manganese(II) nitrate are the inorganic compounds with formula Mn(NO3)2·(H2O)n. Each formula unit is composed of one Mn2+ cation and two NO3− anions and varying amounts of water. Most common is the tetrahydrate Mn(NO3)2·4H2O, but mono- and hexahydrates are also known as well as the anhydrous compound. Some of these compounds are useful precursors to the oxides of manganese.[1]
Preparation, reactions, uses
Manganese(II) nitrate is prepared by dissolving manganese(II) oxide in nitric acid:
- MnO + 2 HNO3 → Mn(NO3)2 + H2O
It can also be prepared from manganese dioxide and nitrogen dioxide:[1]
- MnO2 + 2 NO2 → Mn(NO3)2
On heating to 300 °C, aqueous solutions of manganese(II) nitrate thermally decompose to form MnO2 and NO2.
Manganese(II) nitrate is the precursor to manganese carbonate, which is used in fertilizers and as a colorant. The advantage of this method, use of ammonia and carbon dioxide, being that the side product ammonium nitrate is also useful as a fertilizer.[1]
References
- ^ 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
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