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]
Usesedit
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]
Toxicityedit
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) carbonateedit
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]
Referencesedit
^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
^"Kinetics of Thermal Decomposition of Iron Carbonate". Egyptian Journal of Chemistry. 53 (6): 871–884. 2010-12-31. doi:10.21608/ejchem.2010.1268. ISSN 2357-0245.
^ A .Osol and J. E. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775
^"AAFCO methods for substantiating nutritional adequacy of dog and cat foods (proposed for 2014 publication)" (PDF). AAFCO. 2013.
^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
^Ronald Rich (2007). "8 Iron through Hassium". Inorganic Reactions in Water (1st ed.). Springer Berlin, Heidelberg. p. 178. ISBN9783540739616.
December 15, 2023
iron, carbonate, ferrous, carbonate, chemical, compound, with, formula, feco3, that, occurs, naturally, mineral, siderite, ordinary, ambient, temperatures, green, brown, ionic, solid, consisting, iron, cations, carbonate, anions, iron, carbonate, namesother, n. Iron II carbonate or ferrous carbonate is a chemical compound with formula FeCO3 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 iron II carbonate NamesOther names ferrous carbonateIdentifiersCAS Number 563 71 3 Y3D model JSmol Interactive imageChemSpider 10774 NECHA InfoCard 100 008 418E number E505 acidity regulators PubChem CID 11248UNII MZ3Q72U52O YCompTox Dashboard EPA DTXSID8052225InChI InChI 1S CH2O3 Fe c2 1 3 4 h H2 2 3 4 q 2 p 2Key RAQDACVRFCEPDA UHFFFAOYSA LSMILES C O O O Fe 2 PropertiesChemical formula FeCO3Molar mass 115 854 g molAppearance white powder or crystalsDensity 3 9 g cm3 1 Melting point decomposesSolubility in water 0 0067 g L 2 Ksp 1 28 10 11 3 Solubility product Ksp 3 13 10 11 4 Magnetic susceptibility x 11 300 10 6 cm3 molStructureCrystal structure Hexagonal scalenohedral Trigonal 3 2 m Space group R 3 c a 4 6916 A c 15 3796 ACoordination geometry 6Related compoundsOther anions iron II sulfateOther cations copper II carbonate zinc carbonateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa Infobox references Contents 1 Preparation 2 Properties 3 Uses 4 Toxicity 5 Iron III carbonate 6 ReferencesPreparation editFerrous carbonate can be prepared by reacting solution of the two ions such as iron II chloride and sodium carbonate 5 FeCl2 Na2 CO3 FeCO3 2NaClFerrous 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 ClO4 2 2NaHCO3 FeCO3 2NaClO4 CO2 H2 OSel and others used this reaction but with FeCl2 instead of Fe ClO4 2 at 0 2 M to prepare amorphous FeCO3 7 Care must be taken to exclude oxygen O2 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 CO2 H2 O FeCO3 H2Properties editThe dependency of the solubility in water with temperature was determined by Wei Sun and others to be log K s p 59 3498 0 041377 T 2 1963 T 24 5724 log T 2 518 I 0 657 I displaystyle log K mathit sp 59 3498 0 041377T 2 1963 T 24 5724 log T 2 518 sqrt I 0 657I nbsp where T is the absolute temperature in kelvins and I is the ionic strength of the liquid 3 Iron carbonate decomposes at about 500 600 C 773 873 K 8 Uses editFerrous 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 editFerrous 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 editUnlike 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 edit D R Lide ed 2000 CRC Handbook of Chemistry and Physics 81st Edition Pages 4 65 Patty F ed 1963 Industrial Hygiene and Toxicology volume II Toxicology 2nd ed Interscience Page 1053 a b c Wei 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 ISBN 1138561630 a b 1995 Kirk Othmer Encyclopedia of Chemical Technology 4th ed Volume 1 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 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 Kinetics of Thermal Decomposition of Iron Carbonate Egyptian Journal of Chemistry 53 6 871 884 2010 12 31 doi 10 21608 ejchem 2010 1268 ISSN 2357 0245 A Osol and J E Hoover and others eds 1975 Remington s Pharmaceutical Sciences 15th ed Mack Publishing Page 775 AAFCO methods for substantiating nutritional adequacy of dog and cat foods proposed for 2014 publication PDF AAFCO 2013 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 Ronald Rich 2007 8 Iron through Hassium Inorganic Reactions in Water 1st ed Springer Berlin Heidelberg p 178 ISBN 9783540739616 Retrieved from https en wikipedia org w index php title Iron II carbonate amp oldid 1162368128, wikipedia, wiki, book, books, library,
