{{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/cm<sup>3</sup><ref name="lide"/> | MeltingPtC = | MeltingPt_notes = decomposes | BoilingPtC = | BoilingPt_notes = | Solubility = 0.0067 g/l<ref name="patty"/>; K<sub>sp</sub> = 1.28 × 10<sup>-11</sup> <ref name="weisun"/> | SolubleOther = | Solubility1 = | Solvent1 = | Solubility2 = | Solvent2 = | Solubility3 = | Solvent3 = | RefractIndex = | SolubilityProduct = }} |Section3={{Chembox Structure | Coordination = 6 | CrystalStruct = Hexagonal scalenohedral / Trigonal ({{overline|3}}2/m) <br/>[[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]] <br/> 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-}}. <ref name="kirk"/> ==Preparation== Ferous carbonate can be prepared by reacting solution of the two ions, such as [[iron(II) chloride]] and [[sodium carbonate]]:<ref name="kirk"/> : {{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]]:<ref name="singer"/> : {{chem|Fe}}({{chem|Cl|O|4}})<sub>2</sub> + 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}})<sub>2</sub>)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.<ref name="singer"/> Ferrous carbonate also forms directly on steel or iron surfaces exposed to solutios of carbon dioxide, forming an "iron carbonate" scale:<ref name="weisun"/> : {{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 :<math> \log K_{\mathit{sp}} = -59.3498 - 0.041377 T - 2.1963/T + 24.5724 \log T + 2.518 \sqrt{I} - 0.657 I </math> where ''T'' is the absolute temperature in [[kelvin]], and ''I'' is the [[ionic strength]] of the liquid.<ref name="weisun"/> ==Uses== Ferrous carbonate was used to treat [[anemia]]. <ref name="osol"/> ==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).<ref name="goss"/> <references> <ref name="kirk">(1995): "Kirk-Othmer Encyclopedia of Chemical Technology". 4th ed. Volume 1.</ref> <ref name="patty">Patty, F., ed. (1963): "Industrial Hygiene and Toxicology"; volume II: 'Toxicology". 2nd ed. Interscience. Page 1053.</ref> <ref name="lide">D R. Lide, ed.(2000): "CRC Handbook of Chemistry and Physics". 81st Edition. Pages 4-65.</ref> <ref name="osol"> A .Osol and J. E. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775</ref> <ref name="singer">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</ref> <ref name="goss">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</ref> <ref name="weisun">Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.</ref> <ref name="sel">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}}</ref> </references> {{carbonates}} {{iron compounds}} ---------------------------------------------------------------------- Formerly, the most common forms of iron therapy employed in the U.S. included...ferrous carbonate... <ref name="goss">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</ref> <ref name=""/> <ref name=""></ref> <ref name=""/> <ref name=""></ref> <ref name=""/> <ref name=""></ref> ---------------------------------------------------------------------- <ref name="singer">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</ref> Ferrous carbonate was prepared from ferrous perchlorate and sodium bicarbonate with excess perchloric acid.<ref name="singer"/> System was flushed wth N2 to remove all traces of O2 Fe(II) is rapidly oxidated by O2 at pH above 6.0 ---------------------------------------------------------------------- <ref name="weisun">Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.</ref> 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. ---------------------------------------------------------------------- <ref name="sel"/> <ref name="sel">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}}</ref> From FeCl2(H2O)4 + NaHCO3 (0.2 M of both)