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Manganese(II) acetate are chemical compounds with the formula Mn(CH3CO2)2.(H2O)n where n = 0, 2, 4.. It is used as a catalyst and as fertilizer.[3]

Manganese(II) acetate[1]
Manganese acetate.png
IUPAC name
Manganese(II) acetate
Other names
Manganese diacetate
3D model (JSmol)
ECHA InfoCard 100.010.305
Mn(CH3CO2)2 (anhydrous)
Mn(CH3CO2)2·4H2O (tetrahydrate)
Molar mass 173.027 g/mol (anhydrous)
245.087 g/mol (tetrahydrate)
Appearance white crystals (anhydrous)
light pink monoclinic crystals (tetrahydrate)
Density 1.74 g/cm3 (anhydrous)
1.59 g/cm3 (tetrahydrate)
Melting point 210 °C (410 °F; 483 K) (anhydrous)
80 °C (tetrahydrate)
Solubility soluble in water (about 700g/L at 20°C for tetrahydrate), methanol, acetic acid (anhydrous)
soluble in water, ethanol (tetrahydrate)
+13,650·10−6 cm3/mol
NFPA 704
Flammability code 0: Will not burn. E.g. waterHealth code 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point > 130 °C (266 °F; 403 K) (tetrahydrate)
Lethal dose or concentration (LD, LC):
2940 mg/kg (rat, oral)[2]
Related compounds
Other anions
Manganese(II) fluoride
Manganese(II) chloride
Manganese(II) bromide
Other cations
Zinc acetate
Mercury(II) acetate
Silver acetate
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


Manganese(II) acetate can be formed by treating either manganese(II,III) oxide or manganese(II) carbonate with acetic acid:[4]

MnCO3 + 2 CH3CO2H → Mn(CH3CO2)2 + CO2 + H2O


The anhydrous material and dihydrate Mn(CH3CO2)2.2H2O are coordination polymers. The dihydrate has been characterized by X-ray crystallography. Each Mn(II) center is surrounded by six oxygen centers provided by aquo ligands and acetates.

Subunit of the structure of the dihydrate of manganese(II) acetate.[5]


  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. ^ "Manganese compounds (as Mn)". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  3. ^ Thomas Scott; Mary Eagleson (1994), Concise encyclopedia chemistry, Walter de Gruyter, p. 620, ISBN 3-11-011451-8, retrieved 2009-07-20
  4. ^ Arno H. Reidies (2002). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123.CS1 maint: uses authors parameter (link)
  5. ^ Chih-Yi Cheng, Sue-Lein Wang (1991). "Structure of manganese acetate dihydrate". Acta Crystallographica Section C. 47: 1734. doi:10.1107/S0108270191002202.CS1 maint: uses authors parameter (link)