Iron(II) carbonate

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iron(II) carbonate
Names
Other names
ferrous carbonate
Identifiers
  • 563-71-3 checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.008.418 Edit this at Wikidata
E number E505 (acidity regulators, ...)
UNII
  • InChI=1S/CH2O3.Fe/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
    Key: RAQDACVRFCEPDA-UHFFFAOYSA-L
  • C(=O)([O-])[O-].[Fe+2]
Properties
FeCO3
Molar mass 115.854 g/mol
Appearance white powder or crystals
Density 3.9 g/cm3[1]
Melting point decomposes
0.0067 g/l;[2] Ksp = 1.28 × 10−11 [3]
3.13×10−11[4]
+11,300·10−6 cm3/mol
Structure
Hexagonal scalenohedral / Trigonal (32/m)
Space group: R 3c, a = 4.6916 Å, c = 15.3796 Å
6
Related compounds
Other anions
 iron(II) sulfate
Other cations
 copper(II) carbonate, zinc carbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

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) cations Fe2+
 and carbonate anions CO2−
3.[5]

Preparation[]

Ferrous carbonate can be prepared by reacting solution of the two ions, such as iron(II) chloride and sodium carbonate:[5]

FeCl
2 + Na
2CO
3 → FeCO
3 + 2NaCl

Ferrous carbonate can be prepared also from solutions of an iron(II) salt, such as iron(II) perchlorate, with sodium bicarbonate, releasing carbon dioxide:[6]

Fe(ClO
4)2 + 2NaHCO
3 → FeCO
3 + 2NaClO
4 + CO
2 + H
2O

Sel and others used this reaction (but with FeCl
2 instead of Fe(ClO
4)2) at 0.2 M to prepare amorphous FeCO
3.[7]

Care must be taken to exclude oxygen O
2 from the solutions, because the Fe2+
 ion is easily oxidized to Fe3+
, especially at pH above 6.0.[6]

Ferrous carbonate also forms directly on steel or iron surfaces exposed to solutions of carbon dioxide, forming an "iron carbonate" scale:[3]

Fe + CO
2 + H
2O → FeCO
3 + H
2

Properties[]

The dependency of the solubility in water with temperature was determined by Wei Sun and others to be

where T is the absolute temperature in kelvins, and I is the ionic strength of the liquid.[3]

Uses[]

Ferrous carbonate has been used as an iron dietary supplement to treat anemia.[8] It is noted to have very poor bioavailability in cats and dogs.[9]

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).[10]

References[]

  1. ^ D R. Lide, ed.(2000): "CRC Handbook of Chemistry and Physics". 81st Edition. Pages 4-65.
  2. ^ Patty, F., ed. (1963): "Industrial Hygiene and Toxicology"; volume II: 'Toxicology". 2nd ed. Interscience. Page 1053.
  3. ^ a b c Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.
  4. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 1138561630.
  5. ^ a b (1995): "Kirk-Othmer Encyclopedia of Chemical Technology". 4th ed. Volume 1.
  6. ^ a b Philip 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
  7. ^ 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
  8. ^ A .Osol and J. E. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775
  9. ^ "AAFCO methods for substantiating nutritional adequacy of dog and cat foods (proposed for 2014 publication)" (PDF). AAFCO. 2013.
  10. ^ 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
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