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.
|Systematic IUPAC name
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||178.95 g/mol|
|Melting point||37 °C (99 °F; 310 K)|
|Boiling point||100 °C (212 °F; 373 K)|
|118 g/100 ml(10oC)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Preparation, reactions, usesEdit
- MnO + 2 HNO3 → Mn(NO3)2 + H2O
It can also be prepared from manganese dioxide and nitrogen dioxide:
- 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.
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