Formula For Iron Ii Carbonate
| Names | |
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| Other names ferrous carbonate | |
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| ECHA InfoCard | 100.008.418 |
| E number | E505 (acidity regulators, ...) |
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| Backdrop | |
| Chemical formula | FeCOthree |
| Tooth mass | 115.854 g/mol |
| Advent | white powder or crystals |
| Density | three.9 g/cmthree [i] |
| Melting point | decomposes |
| Solubility in water | 0.0067 one thousand/L;[2] Grandsp = one.28 × 10−eleven [3] |
| Solubility production (Chiliad sp) | iii.13×10−11 [4] |
| Magnetic susceptibility (χ) | +11,300·10−6 cmthree/mol |
| Structure | |
| Crystal structure | Hexagonal scalenohedral / Trigonal (32/thou) Space group: R 3c, a = 4.6916 Å, c = 15.3796 Å |
| Coordination geometry | 6 |
| Related compounds | |
| Other anions | fe(2) sulfate |
| Other cations | copper(2) 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 | |
Fe(Two) carbonate, or ferrous carbonate, is a chemic 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 fe(II) cations Fe 2+
and carbonate anions CO ii−
3 .[v]
Preparation [edit]
Ferrous carbonate can be prepared by reacting solution of the two ions, such as iron(Ii) chloride and sodium carbonate:[5]
- FeCl
2 + Na
two CO
three → FeCO
iii + iiNaCl
Ferrous carbonate can be prepared also from solutions of an fe(Two) salt, such as iron(2) perchlorate, with sodium bicarbonate, releasing carbon dioxide:[6]
- Fe(ClO
iv )2 + iiNaHCO
3 → FeCO
3 + 2NaClO
4 + CO
2 + H
two O
Sel and others used this reaction (but with FeCl
2 instead of Iron(ClO
4 )ii) at 0.2 Thou to ready amorphous FeCO
3 .[7]
Care must be taken to exclude oxygen O
2 from the solutions, because the Atomic number 26 2+
ion is easily oxidized to Fe 3+
, especially at pH higher up 6.0.[6]
Ferrous carbonate also forms direct on steel or fe surfaces exposed to solutions of carbon dioxide, forming an "iron carbonate" calibration:[3]
- Atomic number 26 + CO
two + H
2 O → FeCO
3 + H
2
Properties [edit]
The dependency of the solubility in water with temperature was determined by Wei Sun and others to exist
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).[viii]
Uses [edit]
Ferrous carbonate has been used as an iron dietary supplement to treat anemia.[nine] It is noted to have very poor bioavailability in cats and dogs.[10]
Toxicity [edit]
Ferrous carbonate is slightly toxic; the probable oral lethal dose is between 0.5 and v 1000/kg (betwixt 35 and 350 g for a 70 kg person).[11]
References [edit]
- ^ D R. Lide, ed.(2000): "CRC Handbook of Chemical science 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 atomic number 26 sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemical science and Physics (99 ed.). CRC Press. pp. 5–188. ISBN1138561630.
- ^ a b (1995): "Kirk-Othmer Encyclopedia of Chemical Applied science". 4th ed. Volume i.
- ^ a b Philip C. Vocalizer and Werner Stumm (1970): "The solubility of ferrous iron in carbonate-bearing waters". Journal of the American H2o Works Association, book 62, issue 3, pages 198-202. https://world wide web.jstor.org/stable/41266171
- ^ Ozlem Sel, A.Five. 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, result xv, pages 61–68. doi:10.1016/j.gca.2012.03.011
- ^ "Kinetics of Thermal Decomposition of Iron Carbonate". Egyptian Journal of Chemical science. 53 (half-dozen): 871–884. 2010-12-31. doi:ten.21608/ejchem.2010.1268. ISSN 2357-0245.
- ^ A .Osol and J. Due east. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775
- ^ "AAFCO methods for substantiating nutritional adequacy of dog and true cat foods (proposed for 2014 publication)" (PDF). AAFCO. 2013.
- ^ Gosselin, R.Eastward., H.C. Hodge, R.P. Smith, and Yard.N. Gleason. Clinical Toxicology of Commercial Products. 4th ed. Baltimore: Williams and Wilkins, 1976., p. II-97
Formula For Iron Ii Carbonate,
Source: https://en.wikipedia.org/wiki/Iron%28II%29_carbonate
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