Manganese(II) acetate

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Manganese(II) acetate[1]
Manganese acetate.png
CAS number 638-38-0, (anhydrous)
[6156-78-1] (tetrahydrate)
PubChem 12525
ChemSpider 12008
Jmol-3D images Image 1
Molecular formula Mn(CH3COO)2 (anhydrous)
Mn(CH3COO)2·4H2O (tetrahydrate)
Molar mass 173.027 g/mol (anhydrous)
245.087 g/mol (tetrahydrate)
Appearance red crystals (anhydrous)
red monoclinic crystals (tetrahydrate)
Density 1.74 g/cm3 (anhydrous)
1.59 g/cm3 (tetrahydrate)
Melting point 210°C (anhydrous)
80°C (tetrahydrate)
Solubility soluble in water, methanol, acetic acid (anhydrous)
soluble in water, ethanol (tetrahydrate)
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point > 130°C (tetrahydrate)
Related compounds
Other anions Manganese(II) fluoride
Manganese(II) chloride
Manganese(II) bromide
Other cations Zinc acetate
Mercury(II) acetate
Silver acetate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Manganese(II) acetate is the chemical compound with the formula Mn(CH3COO)2. It is used as a desiccant, a catalyst, and as fertilizer.[2]


Manganese(II) acetate can be formed by reacting acetic acid with either manganese(II,III) oxide or manganese(II) carbonate:[2][3]

Mn3O4 + 2CH3COOH → Mn(CH3COO)2 + Mn2O3 + H2O

If manganese(II,III) oxide is used, manganese(III) oxide is produced as a byproduct.

If the anhydrous form needs to be produced, manganese(II) nitrate can be reacted with acetic anhydride.[2]


  1. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 3–354, 4–68, ISBN 0-8493-0594-2 
  2. ^ a b c Thomas Scott; Mary Eagleson (1994), Concise encyclopedia chemistry, Walter de Gruyter, p. 620, ISBN 3-11-011451-8, retrieved 2009-07-20 
  3. ^ Patnaik, Pradyot (2003), Handbook of Inorganic Chemical Compounds, McGraw-Hill Professional, pp. 81–82, ISBN 0-07-049439-8, retrieved 2009-07-20