Iron(II) acetate

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Iron(II) acetate
Skeletal formula of iron(II) acetate
IUPAC name
Iron(II) acetate
Other names
Ferrous acetate
3D model (Jmol)
ECHA InfoCard 100.019.492
RTECS number AI3850000
Molar mass 173.93 g·mol−1
Appearance White crystals (anhydrous)
Light green crystals (tetrahydrate)
Odor Odorless
Density 1.734 g/cm3 (−73 °C)[1]
Melting point 190–200 °C (374–392 °F; 463–473 K)
Orthorhombic, oP75 (200 K)[1]
Pbcn, No. 60 (200 K)[1]
2/m 2/m 2/m (200 K)[1]
a = 18.1715(4) Å, b = 22.1453(5) Å, c = 8.2781(2) Å (200 K)[1]
α = 90°, β = 90°, γ = 90°
GHS pictograms The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)[3]
GHS signal word Warning
H315, H319, H335[3]
P261, P305+351+338[3]
Irritant Xi
R-phrases R36/37/38
S-phrases S26, S36
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform 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
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

Iron(II) acetate is an coordination complex with formula Fe(C2H3O2)2. It is a white solid, although impure samples can be slightly colored. A light green tetrahydrate is also known, which is highly soluble in water.

Preparation and structure[edit]

Iron powder reacts with hot acetic acid to give the product:[1]

Fe + 2 CH3CO2H → Fe(CH3CO2)2 + H2

It adopts a polymeric structure with octahedral Fe(II) centers bridged by acetate ligands. It is not a salt.[1]

The hydrate can be made by the reaction of ferrous oxide or ferrous hydroxide with acetic acid.[5]

Reaction of scrap iron with acetic acid affords a brown mixture of various iron(II) and iron(III) acetates that are used in dyeing.[6]


Ferrous acetate is used as a mordant by the dye industry. Ebonizing wood is one such process.[7]


  1. ^ a b c d e f g Weber, Birgit; Betz, Richard; Bauer, Wolfgang; Schlamp, Stephan (2011). "Crystal Structure of Iron(II) Acetate". Zeitschrift für anorganische und allgemeine Chemie. 637: 102–107. doi:10.1002/zaac.201000274. Retrieved 2014-08-02. 
  2. ^ a b Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0. 
  3. ^ a b c d Sigma-Aldrich Co., Iron(II) acetate. Retrieved on 2014-05-03.
  4. ^ "MSDS of Ferrous acetate". Fair Lawn, New Jersey: Fisher Scientific, Inc. Retrieved 2014-08-02.  External link in |website= (help)
  5. ^ Synthesis of Iron(II) acetate hydrate (ferrous acetate)
  6. ^ Wildermuth, Egon; Stark, Hans; Friedrich, Gabriele; Ebenhöch, Franz Ludwig; Kühborth, Brigitte; Silver, Jack; Rituper, Rafael (2005), "Iron Compounds", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a14_591 
  7. ^ Ebonizing Wood with Ferric Acetate