Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Iron(III) oxide-hydroxide: Difference between pages
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{{Short description|Hydrous ferric oxide (HFO)}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid [{{fullurl:Iron(III)_oxide-hydroxide|oldid=476165643}} 476165643] of page [[Iron(III)_oxide-hydroxide]] with values updated to verified values.}} |
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{{Chembox |
{{Chembox |
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| verifiedrevid = 455286792 |
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| verifiedrevid = 477000862 |
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| ImageFile = Hydroxid železitý.PNG |
| ImageFile = Hydroxid železitý.PNG |
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| ImageFile_Ref = {{chemboximage|correct|??}} |
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| ImageSize = 244 |
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| ImageName = Samples of iron(III) oxide-hydroxide monohydrate in a vial, and a spoon |
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| IUPACName = Iron(III) oxide-hydroxide |
| IUPACName = Iron(III) oxide-hydroxide |
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| OtherNames = |
| OtherNames = Metaferric acid<br/>Ferric oxyhydroxide<br/>[[Goethite]] |
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|Section1={{Chembox Identifiers |
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| CASNo = 1310-14-1 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| CASNo1 = 20344-49-4 |
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| UNII = 87PZU03K0K |
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| CASNo1_Ref = {{cascite|correct|CAS}} |
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| CASNo1 = 20344-49-4 |
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| CASNo1_Ref = {{cascite|correct|CAS}} |
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| PubChem = 91502 |
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| ChemSpiderID = 82623 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| EINECS = 215-176-6 |
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| EINECS = 215-176-6 |
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| MeSHName = Goethite |
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| StdInChI = 1S/Fe.H2O.O/h;1H2;/q+1;;/p-1 |
| SMILES = O=[Fe]O |
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| StdInChI = 1S/Fe.H2O.O/h;1H2;/q+1;;/p-1 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = AEIXRCIKZIZYPM-UHFFFAOYSA-M |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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}} |
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|Section2={{Chembox Properties |
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| Formula = FeO(OH) |
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| Appearance = Vivid, dark orange, opaque crystals |
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| Fe = 1 |
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| Odor = odorless |
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| Density = 4.25 g/cm<sup>3</sup> |
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| Solubility = insoluble at pH 7 |
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| Appearance = Vivid, dark orange, opaque crystals |
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| SolubilityProduct = 2.79×10<sup>−39</sup> for Fe(OH)<sub>3</sub><ref>{{cite web |url=http://bilbo.chm.uri.edu/CHM112/tables/KspTable.htm |title=Solubility product constants at 25 oC |access-date=2015-02-23 |url-status=dead |archive-url=https://web.archive.org/web/20150226121932/http://bilbo.chm.uri.edu/CHM112/tables/KspTable.htm |archive-date=2015-02-26 }}</ref> |
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}} |
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|Section3={{Chembox Hazards |
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| NFPA-H = 1 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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}} |
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| Section6 = {{Chembox Pharmacology |
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| ATCCode_prefix = B03 |
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| ATCCode_suffix = AB04 |
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}} |
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}} |
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'''Iron(III) oxide-hydroxide''' or '''ferric oxyhydroxide'''<ref name=mack60>A. L. Mackay (1960): " |
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The compound is often encountered as one of its [[hydrate]]s, {{chem|FeO(OH)}}·''n''[[Water|{{chem|H|2|O}}]] [rust]. The monohydrate {{chem|FeO(OH)}}·{{chem|H|2|O}} is often referred to as '''iron(III) hydroxide''' {{chem|Fe|(|OH|)|3}},<ref name=":0">CAS {{CASREF|CAS=51274-00-1}}, C.I. 77492</ref> '''hydrated iron oxide''', '''yellow iron oxide''', or '''Pigment Yellow 42'''.<ref name=":0" /> |
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==Natural occurrences == |
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=== Minerals === |
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Anhydrous ferric hydroxide occurs in the nature as the exceedingly rare mineral [[bernalite]], Fe(OH)<sub>3</sub>·''n''H<sub>2</sub>O (''n'' = 0.0–0.25).<ref name=Mindat>{{Cite web|url=https://www.mindat.org/min-635.html|title = Bernalite}}</ref><ref name=IMA>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> Iron oxyhydroxides, {{chem|FeOOH}}, are much more common and occur naturally as structurally different [[mineral]]s (polymorphs) denoted by the Greek letters |
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* [[Goethite]], |
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* [[Akaganeite]] is the |
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* [[Lepidocrocite]], the |
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* [[Feroxyhyte]] ( |
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=== Non-mineral === |
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* [[Siderogel]] is a naturally occurring [[colloid]]al form of iron(III) oxide-hydroxide. |
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Goethite and lepidocrocite, both crystallizing in orthorhombic system, are the most common forms of iron(III) oxyhydroxide and the most important mineral carriers of iron in soils. |
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=== Mineraloids === |
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Iron(III) oxyhydroxide is the main component of other minerals and [[mineraloid]]s: |
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* [[Limonite]] is a commonly occurring mixture of mainly goethite, lepidocrocite, [[quartz]] and [[clay minerals]]. |
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* [[Ferrihydrite]] is an amorphous or [[nanocrystal]]line hydrated mineral, officially {{chem|FeOOH·1.8H|2|O}} but with widely variable hydration. |
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==Properties== |
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The color of iron(III) oxyhydroxide ranges from yellow through dark-brown to black, depending on the degree of hydration, particle size and shape, and crystal structure. |
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===Structure=== |
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The crystal structure of |
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===Chemistry=== |
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On heating, |
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==Uses== |
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[[Limonite]], a mixture of various hydrates and polymorphs of ferric oxyhydroxide, is one of the three major [[iron ore]]s, having been used since at least 2500 BC.<ref name=maceach>MacEachern, Scott (1996): [http://www.panafprehistory.org/images/papers/IRON_AGE_BEGINNINGS_NORTH_OF_THE_MANDARA_MOUNTAINS_CAMEROON_AND_NIGERIA_Scott_MacEachern.pdf "Iron Age beginnings north of the Mandara Mountains, Cameroon and Nigeria"]. ''In'' ''In'' Pwiti, Gilbert and Soper, Robert (editors) (1996) ''Aspects of African Archaeology: Proceedings of the Tenth Pan-African Congress'' University of Zimbabwe Press, Harare, Zimbabwe, {{ISBN|978-0-908307-55-5}}, pages 489-496. Archived [https://web.archive.org/web/20120311184136/http://www.panafprehistory.org/images/papers/IRON_AGE_BEGINNINGS_NORTH_OF_THE_MANDARA_MOUNTAINS_CAMEROON_AND_NIGERIA_Scott_MacEachern.pdf here] on 2012-03-11.</ref><ref>Diop-Maes, Louise Marie (1996): [http://www.ankhonline.com/revue/diop_lm_metallurgie_fer_afrique.htm "La question de l'Âge du fer en Afrique" ("The question of the Iron Age in Africa")]. ''Ankh'', volume4/5, pages 278-303. [https://web.archive.org/web/20080125103929/http://www.ankhonline.com/revue/diop_lm_metallurgie_fer_afrique.htm Archived] on 2008-01-25.</ref> |
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Yellow iron oxide, or Pigment Yellow 42, is [[Food and Drug Administration]] (FDA) approved for use in [[cosmetics]] and is used in some [[tattoo]] inks. |
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Iron oxide-hydroxide is also used in [[aquarium]] water treatment as a [[phosphate]] binder.<ref>{{URL| http://www.reefkeeping.com/issues/2004-11/rhf/index.php |Iron Oxide Hydroxide (GFO) Phosphate Binders}}</ref> |
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Iron oxide-hydroxide [[nanoparticle]]s have been studied as possible [[adsorbent]]s for lead removal from aquatic media.<ref>Safoora Rahimi, Rozita M. Moattari, Laleh Rajabi, Ali Ashraf Derakhshan, and Mohammad Keyhani (2015): "Iron oxide/hydroxide ( |
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=== Medication === |
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Iron polymaltose is used in treatment of [[iron-deficiency anemia]]. |
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==Production== |
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Iron(III) oxyhydroxide precipitates from solutions of iron(III) salts at [[pH]] between 6.5 and 8.<ref name=grund>Tim Grundl and Jim Delwiche (1993): "Kinetics of ferric oxyhydroxide precipitation". ''Journal of Contaminant Hydrology'', volume 14, issue 1, pages 71-87. {{doi|10.1016/0169-7722(93)90042-Q}}</ref> |
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Thus the oxyhydroxide can be obtained in the lab by reacting an iron(III) salt, such as [[ferric chloride]] or [[ferric nitrate]], with [[sodium hydroxide]]:<ref name=gayer>K. H. Gayer and Leo Woontner (1956): "The Solubility of Ferrous Hydroxide and Ferric Hydroxide in Acidic and Basic Media at 25°". ''Journal of Physical Chemistry'', volume 60, issue 11, pages 1569–1571. {{doi|10.1021/j150545a021}}</ref> |
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:{{chem|FeCl|3}} + 3 NaOH → {{chem|Fe|(|OH|)|3}} + 3 NaCl |
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:{{chem|Fe(NO|3|)|3}} + 3 NaOH → {{chem|Fe|(|OH|)|3}} + 3 {{chem|NaNO|3}} |
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In fact, when dissolved in water, pure {{chem|FeCl|3}} will [[hydrolysis|hydrolyze]] to some extent, yielding the oxyhydroxide and making the solution acidic:<ref name=grund/> |
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:{{chem|FeCl|3}} + 2 {{chem|H|2|O}} ↔ {{chem|FeOOH}} + 3 {{chem|HCl}} |
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Therefore, the compound can also be obtained by the decomposition of acidic solutions of iron(III) chloride held near the boiling point for days or weeks:<ref name=matij>Egon Matijević and Paul Scheiner (1978): "Ferric hydrous oxide sols: III. Preparation of uniform particles by hydrolysis of Fe(III)-chloride, -nitrate, and -perchlorate solutions". ''Journal of Colloid and Interface Science'', volume 63, issue 3, pages 509-524. {{doi|10.1016/S0021-9797(78)80011-3}}</ref> |
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: {{chem|FeCl|3}} + 2 {{chem|H|2|O}} → {{chem|Fe|OOH}}<sub>(s)</sub> + 3 {{chem|HCl}}<sub>(g)</sub> |
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(The same process applied to [[iron(III) nitrate]] {{chem|Fe|(|NO|3|)|3}} or perchlorate {{chem|Fe|(|ClO|4|)|3}} solutions yields instead particles of |
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Another similar route is the decomposition of iron(III) nitrate dissolved in [[stearic acid]] at about 120 °C.<ref name=danli1997>Dan Li, Xiaohui Wang, Gang Xiong, Lude Lu, Xujie Yang and Xin Wang (1997): "A novel technique to prepare ultrafine {{chem|Fe|2|O|3}} via hydrated iron(III) nitrate". ''Journal of Materials Science Letters'' volume 16, pages 493–495 {{doi|10.1023/A:1018528713566}}</ref> |
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The oxyhydroxide prepared from ferric chloride is usually the |
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Whittemore and Donald Langmuir (1974): "Ferric Oxyhydroxide Microparticles in Water". ''Environmental Health Perspective'', volume 9, pages 173-176. {{doi|10.1289/ehp.749173}}</ref> |
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The oxyhydroxide can also be produced by a solid-state transformation from [[iron(II) chloride]] tetrahydrate {{chem|FeCl|2}}·4{{chem|H|2|O}}.<ref name=mack62/> |
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The compound also readily forms when [[iron(II) hydroxide]] is exposed to air: |
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:4{{chem|Fe|(|OH|)|2}} + {{chem|O|2}} → 4 {{chem|FeOOH}} + 2 {{chem|H|2|O}} |
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The iron(II) hydroxide can also be oxidized by [[hydrogen peroxide]] in the presence of an acid: |
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:2{{chem|Fe|(|OH|)|2}} + {{chem|H|2|O|2}} → 2 {{chem|Fe|(|OH|)|3}} |
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==See also== |
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*[[Rust]] |
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*[[Iron oxide]] |
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*[[Yellow boy]], a yellow precipitate when acidic runoff such as mine waste, is then neutralised |
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==References== |
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{{reflist}} |
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{{Iron compounds}} |
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{{Antianemic preparations}} |
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[[Category:Iron(III) compounds]] |
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[[Category:Hydroxides]] |
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[[Category:Transition metal oxides]] |