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{{Use dmy dates|date=August 2022}} |
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| ImageFile = Ferric amm sulfate.jpg |
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| ImageFile1 = Ferric Ammonium Sulfate Dodecahydrate formula.png |
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| ImageSize1 = 250px |
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| Name = |
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| IUPACName = Ammonium iron(III) sulfate |
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| ImageFile = Ferric amm sulfate.jpg |
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| ImageFile1 = Ferric Ammonium Sulfate Dodecahydrate formula.png |
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| OtherNames = Ferric ammonium sulfate<br/>Iron alum |
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| ImageFile2 = Ammonium-iron(III)-sulfate-3D-balls-ionic.png |
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| Section1 = {{Chembox Identifiers |
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| ImageSize1 = 250px |
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| IUPACName = Ammonium iron(III) sulfate |
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| OtherNames = Ferric ammonium sulfate<br />Ferric alum |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
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| index_label = anhydride |
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| index1_label = dodecahydrate |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 55405 |
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| ChemSpiderID = 55405 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = XGGLLRJQCZROSE-UHFFFAOYSA-K |
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| StdInChIKey = XGGLLRJQCZROSE-UHFFFAOYSA-K |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo = 10138-04-2 |
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| CASNo = 10138-04-2 |
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| CASNo1_Ref = {{cascite|correct|CAS}} |
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| CASOther = <br/>7783-83-7 (dodecahydrate) |
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| PubChem = |
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| CASNo1 = 7783-83-7 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = LUX2X1H1IC |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| UNII1 = 65390568Z5 |
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| EINECS = 233-382-4 |
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| PubChem1 = 61485 |
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| SMILES = .S(=O)(=O).S()(=O)=O. |
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| SMILES = .S(=O)(=O).S()(=O)=O. |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = NH<sub>4</sub>Fe(SO<sub>4</sub>)<sub>2</sub> |
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| Formula = FeNH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub>•12H<sub>2</sub>O |
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| MolarMass = 482.25 g/mol (dodecahydrate) |
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| MolarMass = 482.25 g/mol (dodecahydrate) |
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| Appearance = Pale violet octahedral crystals |
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| Appearance = Pale violet octahedral crystals |
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| Odor = weak ammonia-like |
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| Density = 1.71 g/cm<sup>3</sup> |
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| Density = 1.71 g/cm<sup>3</sup> |
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| MeltingPt = 39-41 °C |
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| MeltingPtC = 39 to 41 |
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| Solubility = 1240 g/L |
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| Solubility = 1240 g/L |
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| Section3 = {{Chembox Hazards |
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| MainHazards = Irritant ('''Xi''') |
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| MainHazards = Irritant |
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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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| NFPA_ref =<ref>{{cite web|title=Material Safety Data Sheet. Iron (III) Ammonium Sulfate Dodecahydrate | website=fscimage.fishersci.com | url=https://fscimage.fishersci.com/msds/09713.htm | access-date=8 June 2023}}</ref> |
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| Section4 = {{Chembox Related |
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| OtherAnions = ]<br>] |
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| OtherAnions = ]<br />] |
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| OtherCations = ]<br />] |
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'''Ammonium iron(III) sulfate''', NH<sub>4</sub>Fe(SO<sub>4</sub>)<sub>2</sub>·12 H<sub>2</sub>O, also known as '''ferric ammonium sulfate''' (FAS) or '''iron alum''', is a ] in the class of ]s, which consists of compounds with the general formula AB(SO<sub>4</sub>)<sub>2</sub> · 12 H<sub>2</sub>O<ref>Considine , Douglas M: “Chemical and process technology encyclopedia”, McGraw-Hill , New York , 1974, p. 993</ref>. It has the appearance of weakly violet, octahedrical ]s. There has been some discussion regarding the origin of the crystals' colour, with some ascribing it to impurities in the compound<ref>Christensen, Odin T: “On the Cause of the Amethyst Color of Ferric Alum and of Mixed Crystals of Ferric and Manganic Alum.” ''Chem. Lab. Roy. Vet. Agr. Hochschule, Kgl. Danske Vidsk. Selsk. Forh.'' (1906), p. 173-95</ref>, and others claiming it to be a property of the crystal itself<ref>Jane Bonnell and Edgar Philip Perman: "CCXXIX.—The colour of iron alum", ''J. Chem. Soc., Trans., 1921, 119, 1994 - 1997, DOI: 10.1039/CT9211901994''</ref>. |
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'''Ammonium iron(III) sulfate''', NH<sub>4</sub>Fe(SO<sub>4</sub>)<sub>2</sub>·12 H<sub>2</sub>O, or NH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub>·6 H<sub>2</sub>O, also known as '''ferric ammonium sulfate''' ('''FAS''') or '''iron alum''', is a ] in the class of ]s, which consists of compounds with the general formula AB(SO<sub>4</sub>)<sub>2</sub> · 12 H<sub>2</sub>O.<ref>Considine, Douglas M: ''Chemical and process technology encyclopedia'', McGraw-Hill, New York, 1974, p. 993</ref> It has the appearance of weakly violet, octahedrical ]s. There has been some discussion regarding the origin of the crystals' color, with some ascribing it to impurities in the compound,<ref>{{cite journal | last1 = Christensen | first1 = Odin T | title = On the Cause of the Amethyst Color of Ferric Alum and of Mixed Crystals of Ferric and Manganic Alum | journal = Chem. Lab. Roy. Vet. Agr. Hochschule, KGL. Danske Vidsk. Selsk. Forh. | volume = 1906 | pages = 173–95 }}</ref> and others claiming it to be a property of the crystal itself.<ref>{{cite journal | last1 = Bonnell | first1 = Jane | last2 = Philip Perman | first2 = Edgar | year = 1921 | title = CCXXIX.—The colour of iron alum | url = https://zenodo.org/record/1609699| journal = J. Chem. Soc., Trans. | volume = 119 | pages = 1994–1997 | doi = 10.1039/CT9211901994 }}</ref> |
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FAS is ]<ref>Cooke, Meyer, Wolf: “The Specific Heats of Three Paramagnetic salts at Very Low Temperatures” ''Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences'', Volume 237, Issue 1210, p. 395-403.</ref>, ] and ] towards ]s<ref>Fei Wang et al.: “Microcalorimetric investigation of the toxic action of ammonium ferric(III)sulfate on the metabolic activity of pure microbes:” doi:10.1016/j.etap.2007.11.004 ''Accesible via http://www.sciencedirect.com''</ref>. It is a weak oxidizing agent, capable of being reduced to ], ferrous ammonium sulfate. |
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FAS is ],<ref>{{cite journal | last1 = Cooke | first1 = Meyer | last2 = Wolf | year = 1956| title = The Specific Heats of Three Paramagnetic salts at Very Low Temperatures | journal = Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences | volume = 237 | issue = 1210| pages = 395–403 | doi=10.1098/rspa.1956.0185| bibcode = 1956RSPSA.237..395C | s2cid = 97076961 }}</ref> ] and ] towards ]s.<ref>{{cite journal | last1 = Wang | first1 = Fei | display-authors = etal | year = 2008| title = Microcalorimetric investigation of the toxic action of ammonium ferric(III)sulfate on the metabolic activity of pure microbes | journal = Environmental Toxicology and Pharmacology| volume = 25| issue = 3| pages = 351–357| doi = 10.1016/j.etap.2007.11.004 | pmid = 21783873 | bibcode = 2008EnvTP..25..351W }}</ref> It is a weak oxidizing agent, capable of being reduced to ], ferrous ammonium sulfate. |
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==Preparation== |
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==Preparation== |
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FAS can be prepared by crystallization from a solution of ] and ]. Iron(II) in ferrous sulfate is oxidized to Iron(III) in ferric sulfate by addition of ] and ]. Upon addition of ammonium sulfate to the solution and damping in of the solution, ferric ammonium sulfate crystals will precipitate. |
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FAS can be prepared by crystallization from a solution of ] and ]. Iron(II) in ferrous sulfate is oxidized to ferric sulfate by addition of ] and ]. Upon addition of ammonium sulfate to the solution and damping in of the solution, ferric ammonium sulfate crystals precipitate. Equations for these conversions ignore the ] of the material. |
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'''Oxidation''': 6 FeSO<sub>4</sub> + 2 HNO<sub>3</sub> + 3 H<sub>2</sub>SO<sub>4</sub> = 3 Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> + 2 NO + 4 H<sub>2</sub>O |
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:Oxidation: {{chem2 | 6 FeSO4 + 2 HNO3 + 3 H2SO4 -> 3 Fe2(SO4)3 + 2 NO + 4 H2O }} |
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:Synthesis: {{chem2 | Fe2(SO4)3 + (NH4)2SO4 -> 2 NH4Fe(SO4)2 }} |
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'''Synthesis''': Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> + (NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub> = 2 NH<sub>4</sub>Fe(SO<sub>4</sub>)<sub>2</sub> |
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'''Procedure<ref>Hecht, Horstmar: “Prãparative Anorganische Chemie”, ''Springer-verlag, Berlin'', 1951. p. 127</ref>''': |
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The nitric and sulfuric acid is reacted with the ferrous sulfate to make ferric sulfate, ], and water. The ferric sulfate is mixed with ] and crystallized to get ammonium iron(III) sulfate. The solution is normally tested to ensure that no more iron(II) is left. |
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==Uses== |
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==Uses== |
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Areas of use for FAS include ] treatment,<ref name="ReferenceA">''Wiley Encyclopedia of inorganic chemistry'': Volume 4, p. 1704:</ref> ],<ref name="ReferenceA" /> production of ]stuffs,<ref name="ReferenceA" /> and as an ] agent in the production of ].<ref>Chen et al.: ''United States Patent 5518131'' – "Etching molydbenum with ferric sulfate and ferric ammonium sulfate"</ref> It has been used in a wide area of applications, including adiabatic ] equipment,<ref>Grant W. Wilson, Peter T. Timbie: "Construction techniques for adiabatic demagnetization refrigerators using ferric ammonium alum". ''Cryogenics'', Volume 39, Number 4, (1999), pp. 319–322</ref> biochemical ],<ref>J. C. Whitehorn: "A system of blood analysis. Supplement II. Simplified method for the determination of chlorides in blood or plasma". ''Journal of Biological Chemistry'' (1921), 45 p. 449–60.</ref> and ].<ref>{{cite journal | last1 = Yu | first1 = Shanxin | display-authors = etal | year = 2005 | title = Application of ammonium ferric sulfate dodecahydrate in organic synthesis | journal = General Review | volume = 17 | issue = 1| pages = 27–30 }}</ref> |
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==Gallery== |
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Areas of use for FAS include ] treatment<ref name="ReferenceA">''Wiley Encyclopedia of inorganic chemistry'': Volume 4, p. 1704:</ref>, ]<ref name="ReferenceA" />, production of ]stuffs<ref name="ReferenceA" />, and as an ] agent in the production of ]<ref>Chen , et al.: ''United States Patent 5518131'' - ”Etching molydbenum with ferric sulfate and ferric ammonium sulfate”</ref>. It has been used in a wide area of applications, including adiabatic ] equipment<ref>Grant W. Wilson, Peter T. Timbie: Construction techniques for adiabatic demagnetization refrigerators using ferric ammonium alum. ''Cryogenics'', *Volume 39, Number 4, (1999) , p. 319-322</ref>, biochemical ]<ref>J.C. Whitehorn: A system of blood analysis. Supplement II. Simplified method for the determination of chlorides in blood or plasma. *''Journal of Biological Chemistry'' (1921), 45 p. 449-60.</ref> and ]<ref>Yu, Shanxin et al.: "Application of ammonium ferric sulfate dodecahydrate in organic synthesis", ''General Review 2005'': 17(1), p. 27-30.</ref>. |
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<gallery> |
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Ammoniumeisenalaun.jpg|Crystals of ferric ammonium sulfate |
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Ammonium iron(III) sulfate dodecahydrate in moist air, 2015-10-22 (1).jpg|Crystals of ammonium iron(III) sulfate after 16 days in the air |
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</gallery> |
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==References== |
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==References== |
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{{Reflist}} |
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{{Reflist}} |
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{{Ammonium salts}} |
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{{iron compounds}} |
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{{sulfates}} |
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{{DEFAULTSORT:Ammonium Iron(Iii) Sulfate}} |
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{{DEFAULTSORT:Ammonium Iron(Iii) Sulfate}} |
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