{{chembox | Verifiedfields = | Watchedfields = | verifiedrevid = | ImageFile = | ImageSize = 100px | ImageFileL1 = | ImageSizeL1 = 100px | ImageFileR1 = | ImageSizeR1 = 120px | ImageFile2 = | ImageSize2 = 200px | Name = iron(II) carbonate | OtherNames = ferrous carbonate |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|??|chemspider}} | ChemSpiderID = | ChEMBL_Ref = {{ebicite|??|EBI}} | ChEMBL = | UNII_Ref = {{fdacite|??|FDA}} | UNII = | InChI = 1S/CH2O3.Fe/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 | InChIKey = RAQDACVRFCEPDA-UHFFFAOYSA-L | SMILES = C(=O)([O-])[O-].[Fe+2] | StdInChI_Ref = {{stdinchicite|??|chemspider}} | StdInChI = | StdInChIKey_Ref = {{stdinchicite|??|chemspider}} | StdInChIKey = | CASNo = 563-71-3 | CASNo_Ref = {{cascite|??|CAS}} | PubChem = 11248 | EINECS = | RTECS = | UNNumber = }} |Section2={{Chembox Properties | Formula = | MolarMass = 115.854 g/mol | Appearance = white powder or crystals | Density = 3.9 g/cm3 | MeltingPtC = | MeltingPt_notes = decomposes | BoilingPtC = | BoilingPt_notes = | Solubility = 0.0067 g/l; Ksp = 1.28 × 10-11 | SolubleOther = | Solubility1 = | Solvent1 = | Solubility2 = | Solvent2 = | Solubility3 = | Solvent3 = | RefractIndex = | SolubilityProduct = }} |Section3={{Chembox Structure | Coordination = 6 | CrystalStruct = Hexagonal scalenohedral / Trigonal ({{overline|3}}2/m)
[[Space group]]: R {{overline|3}}c, a = 4.6916 [[angstrom|Å]], c = 15.3796 Å }} |Section4={{Chembox Thermochemistry | DeltaHf = | HeatCapacity = | DeltaGf = | Entropy = }} |Section7={{Chembox Hazards | ExternalSDS = | GHSPictograms = | GHSSignalWord = | HPhrases = | PPhrases = | EUClass = | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = | RPhrases = | SPhrases = | FlashPt = }} |Section8={{Chembox Related | OtherAnions = | OtherCations = }} }} [[Trigonal]]
class | symmetry = | gravity = 3.96 InChI key (?) density solubility: '''iron(II) carbonate''', or '''ferrous carbonate''', is a chemical compound with formula {{chem|Fe|C|O|3}}, that occurs naturally as the mineral [[siderite]]. At ordinary ambient temperatures, it is a white [[ionic compound|ionic solid]] consisting or [[iron|iron(II)]] [[cations]] {{chem|Fe|2+}} and [[carbonate]] [[anions]] {{chem|C|O|3|2-}}. ==Preparation== Ferous carbonate can be prepared by reacting solution of the two ions, such as [[iron(II) chloride]] and [[sodium carbonate]]: : {{chem|Fe|Cl|2}} + {{chem|Na|2|C|O|3}} &arrow; {{chem|Fe|C|O|3}} + 2{{chem|Na|Cl}} Ferrous carbonate can be prepared also from solutions of an iron(II) salt, such as [[ferrous perchlorate]], with [[sodium bicarbonate]], with release of [[carbon dioxide]]: : {{chem|Fe}}({{chem|Cl|O|4}})2 + 2{{chem|Na|H|C|O|3}} &arrow; {{chem|Fe|C|O|3}} + 2{{chem|Na|Cl|O|4}} + {{chem|C|O|2}} + {{chem|H|2|O}} Sela and others used this reaction (but with {{chem|Fe|Cl|2}} instead of {{chem|Fe}}({{chem|Cl|O|4}})2)at 0.2 [[molarity|M]] to prepare amorphous {{chem|Fe|C|O|3}}. Care must be taken to exclude [[oxygen]] {{chem|O|2}} from the solutions, because the {{chem|Fe|2+}} ion is esily [[oxidation|oxidized]] to {{chem|Fe|3+}}, especially at [[acidity|pH]] above 6.0. Ferrous carbonate also forms directly on steel or iron surfaces exposed to solutios of carbon dioxide, forming an "iron carbonate" scale: : {{chem|Fe}} + {{chem|C|O|2}} + {{chem|H|2|O}} &arrow; {{chem|Fe|C|O|3}} + {{chem|H|2}} ==Properties== The dependency of the solubility in water with temperature was determined by Wei Sun and others to be : \log K_{\mathit{sp}} = -59.3498 - 0.041377 T - 2.1963/T + 24.5724 \log T + 2.518 \sqrt{I} - 0.657 I where ''T'' is the absolute temperature in [[kelvin]], and ''I'' is the [[ionic strength]] of the liquid. ==Uses== Ferrous carbonate was used to treat [[anemia]]. ==Toxicity== Ferrous carbonate is moderately toxic; the probable oral lethal dose is between 0.5 and 5 g/kg (between 35 and 350 g for a 70 kg person). (1995): "Kirk-Othmer Encyclopedia of Chemical Technology". 4th ed. Volume 1. Patty, F., ed. (1963): "Industrial Hygiene and Toxicology"; volume II: 'Toxicology". 2nd ed. Interscience. Page 1053. D R. Lide, ed.(2000): "CRC Handbook of Chemistry and Physics". 81st Edition. Pages 4-65. A .Osol and J. E. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775 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. http://www.jstor.org/stable/41266171 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 Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University. 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}} {{carbonates}} {{iron compounds}} ---------------------------------------------------------------------- Formerly, the most common forms of iron therapy employed in the U.S. included...ferrous carbonate... 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 ---------------------------------------------------------------------- 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. http://www.jstor.org/stable/41266171 Ferrous carbonate was prepared from ferrous perchlorate and sodium bicarbonate with excess perchloric acid. System was flushed wth N2 to remove all traces of O2 Fe(II) is rapidly oxidated by O2 at pH above 6.0 ---------------------------------------------------------------------- Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University. formed in the "iron carbonate scale" corrosion of steel exposed to solutions of CO2. (also of of gas/oil steel pipes exposed to CO2/H2S, but many other products are present there.) The iron carbonate solubility limit (in mol^2/l^2 ) at room temperature and the assumed ionic strength I =0 is reported ranging from 3.72 x 10^{-11}. to 9.33 x 10^{-12}. Adopted 1.28 x 10^{-11} Temeperature dependency: log K_{sp} = -59.3498 - 0.041377 T - 2.1963/T + 24.5724 log T + 2.518 sqrt(I) - 0.657 I (T in kelvin, I = ionic strength) Fe + CO2 + H2O --> FeCO3 + H2 ---------------------------------------------------------------------- Talanta Volume 38, Issue 2, February 1991, Pages 205-211 Cover image Solubility of iron(II) carbonate at temperatures between 30 and 80° Author links open the overlay panel. Numbers correspond to the affiliation list which can be exposed by using the show more link. Robert D. Braun Show more doi:10.1016/0039-9140(91)80131-I ---------------------------------------------------------------------- Solubility product of siderite (FeCO3) as a function of temperature (25–250 °C) Chemical Geology, Volume 265, Issues 1–2, 15 July 2009 P. Bénézeth, J.L. Dandurand, J.C. Harrichoury Used natural siderite. ---------------------------------------------------------------------- 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}} From FeCl2(H2O)4 + NaHCO3 (0.2 M of both)