{{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|Ã…]], c = 15.3796 Ã…
  }}
|Section4={{Chembox Thermochemistry
| DeltaHf = 
| HeatCapacity = 
| DeltaGf = 
| Entropy = 
 }}
|Section7={{Chembox Hazards
| ExternalSDS = 
| GHSPictograms = 
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| 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 

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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)