Iron(II) carbonate, or ferrous carbonate, is a chemical compound with formula FeCO 3, that occurs naturally as the mineral
siderite. At ordinary ambient temperatures, it is a green-brown
ionic solid consisting of
iron(II)cationsFe2+ and
carbonateanionsCO2− 3.[5]
Iron carbonate decomposes at about 500–600 °C (773–873 K).[8]
Uses
Ferrous carbonate has been used as an iron
dietary supplement to treat
anemia.[9] It is noted to have very poor bioavailability in cats and dogs.[10]
Toxicity
Ferrous carbonate is slightly toxic; the probable oral lethal dose is between 0.5 and 5 g/kg (between 35 and 350 g for a 70 kg person).[11]
Iron(III) carbonate
Unlike iron(II) carbonate, iron(III) carbonate has not been isolated. Attempts to produce iron(III) carbonate by the reaction of aqueous ferric ions and carbonate ions result in the production of
iron(III) oxide with the release of
carbon dioxide or
bicarbonate.[12]
References
^D R. Lide, ed.(2000): "CRC Handbook of Chemistry and Physics". 81st Edition. Pages 4-65.
^
abcWei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.
^John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188.
ISBN1138561630.
^
ab(1995): "Kirk-Othmer Encyclopedia of Chemical Technology". 4th ed. Volume 1.
^
abPhilip C. Singer and Werner Stumm (1970): "The solubility of ferrous iron in carbonate-bearing waters". Journal of the American Water Works Association, volume 62, issue 3, pages 198-202.
https://www.jstor.org/stable/41266171
^Ozlem Sel, A.V. Radha, Knud Dideriksen, and Alexandra Navrotsky (2012): "Amorphous iron (II) carbonate: Crystallization energetics and comparison to other carbonate minerals related to CO2 sequestration". Geochimica et Cosmochimica Acta, volume 87, issue 15, pages 61–68.
doi:
10.1016/j.gca.2012.03.011
^Gosselin, R.E., H.C. Hodge, R.P. Smith, and M.N. Gleason. Clinical Toxicology of Commercial Products. 4th ed. Baltimore: Williams and Wilkins, 1976., p. II-97