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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]

Manganese(II) nitrate
Manganese(II) nitrate.svg
Manganese(II) nitrate tetrahydrate
Systematic IUPAC name
Manganese(II) nitrate
Other names
Manganese dinitrate
3D model (JSmol)
ECHA InfoCard 100.030.741
EC Number 233-828-8
UN number 2724
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
Manganese chloride
Other cations
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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Infobox references

Preparation, reactions, usesEdit

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]


  1. ^ 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
Salts and covalent derivatives of the nitrate ion