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{{Use dmy dates|date=August 2022}}
{{chembox {{chembox
| Watchedfields = changed | Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 450965154 | verifiedrevid = 455304200
⚫ | ImageFile = Ferric amm sulfate.jpg
| Name =
| ImageFile1 = Ferric Ammonium Sulfate Dodecahydrate formula.png
⚫ | ImageFile = Ferric amm sulfate.jpg
⚫ | ImageSize1 = 250px
| IUPACName = Ammonium iron(III) sulfate | ImageFile1 = Ferric Ammonium Sulfate Dodecahydrate formula.png
| ImageFile2 = Ammonium-iron(III)-sulfate-3D-balls-ionic.png
⚫ | OtherNames = Ferric ammonium sulfate<br/>Iron alum
⚫ | ImageSize1 = 250px
⚫ | Section1 = {{Chembox Identifiers
| IUPACName = Ammonium iron(III) sulfate
⚫ | OtherNames = Ferric ammonium sulfate<br />Ferric alum
| SystematicName =
⚫ | Section1 = {{Chembox Identifiers
| index_label = anhydride
| index1_label = dodecahydrate
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 55405 | ChemSpiderID = 55405
Line 16: Line 23:
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = XGGLLRJQCZROSE-UHFFFAOYSA-K | StdInChIKey = XGGLLRJQCZROSE-UHFFFAOYSA-K
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 10138-04-2 | CASNo = 10138-04-2
| CASNo1_Ref = {{cascite|correct|CAS}}
| CASOther = <br/>7783-83-7 (dodecahydrate)
| PubChem = | CASNo1 = 7783-83-7
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = LUX2X1H1IC
| UNII1_Ref = {{fdacite|correct|FDA}}
| UNII1 = 65390568Z5
| EINECS = 233-382-4
| PubChem1 = 61485
| SMILES = .S(=O)(=O).S()(=O)=O. | SMILES = .S(=O)(=O).S()(=O)=O.
}} }}
| Section2 = {{Chembox Properties | Section2 = {{Chembox Properties
| Formula = FeNH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub> | Formula = FeNH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub>•12H<sub>2</sub>O
| MolarMass = 482.25 g/mol (dodecahydrate) | MolarMass = 482.25 g/mol (dodecahydrate)
| Appearance = Pale violet octahedral crystals | Appearance = Pale violet octahedral crystals
| Odor = weak ammonia-like
| Density = 1.71 g/cm<sup>3</sup> | Density = 1.71 g/cm<sup>3</sup>
| MeltingPt = 39-41 °C | MeltingPtC = 39 to 41
| MeltingPt_notes =
| BoilingPt = | BoilingPt =
| Solubility = 1240 g/L | Solubility = 1240 g/L
}} }}
| Section3 = {{Chembox Hazards | Section3 = {{Chembox Hazards
| MainHazards = Irritant ('''Xi''') | MainHazards = Irritant
| RPhrases = | GHSPictograms =
| SPhrases = | GHSSignalWord =
| HPhrases = {{HPhrases|}}
| PPhrases = {{PPhrases|}}
| GHS_ref =
| FlashPt = | FlashPt =
| ExternalMSDS = | ExternalSDS =
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| 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>
}} }}
| Section4 = {{Chembox Related | Section4 = {{Chembox Related
| OtherAnions = ]<br>] | OtherAnions = ]<br />]
| OtherCations = ]<br>] | OtherCations = ]<br />]
| OtherFunctn = | OtherFunction =
| Function = | OtherFunction_label =
| OtherCpds = ] | OtherCompounds= ]
}} }}
| Section5 =
| Section6 =
}} }}
'''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>. '''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>


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. 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.


==Preparation== ==Preparation==
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. 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.


'''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 :Oxidation: {{chem2 | 6 FeSO4 + 2 HNO3 + 3 H2SO4 -> 3 Fe2(SO4)3 + 2 NO + 4 H2O }}


:Synthesis: {{chem2 | Fe2(SO4)3 + (NH4)2SO4 -> 2 NH4Fe(SO4)2 }}
'''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>

'''Procedure<ref>Hecht, Horstmar: “Prãparative Anorganische Chemie”, ''Springer-verlag, Berlin'', 1951. p. 127</ref>''':

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.

⚫ ]


==Uses== ==Uses==
⚫ 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>


==Gallery==
⚫ 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>.
<gallery>
⚫ Ammoniumeisenalaun.jpg|Crystals of ferric ammonium sulfate
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
</gallery>


==References== ==References==
{{Reflist}} {{Reflist}}

{{Ammonium salts}}
{{iron compounds}}
{{sulfates}}


{{DEFAULTSORT:Ammonium Iron(Iii) Sulfate}} {{DEFAULTSORT:Ammonium Iron(Iii) Sulfate}}
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] ]
] ]
]

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Latest revision as of 18:18, 18 October 2024

Ammonium iron(III) sulfate
Names
IUPAC name Ammonium iron(III) sulfate
Other names Ferric ammonium sulfate
Ferric alum
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.335 Edit this at Wikidata
EC Number
  • anhydride: 233-382-4
PubChem CID
UNII
CompTox Dashboard (EPA)
InChI
  • InChI=1S/Fe.H3N.2H2O4S/c;;2*1-5(2,3)4/h;1H3;2*(H2,1,2,3,4)/q+3;;;/p-3Key: XGGLLRJQCZROSE-UHFFFAOYSA-K
  • anhydride: InChI=1/Fe.H3N.2H2O4S/c;;2*1-5(2,3)4/h;1H3;2*(H2,1,2,3,4)/q+3;;;/p-3Key: XGGLLRJQCZROSE-DFZHHIFOAY
SMILES
  • anhydride: .S(=O)(=O).S()(=O)=O.
Properties
Chemical formula FeNH4(SO4)2•12H2O
Molar mass 482.25 g/mol (dodecahydrate)
Appearance Pale violet octahedral crystals
Odor weak ammonia-like
Density 1.71 g/cm
Melting point 39 to 41 °C (102 to 106 °F; 312 to 314 K)
Solubility in water 1240 g/L
Hazards
Occupational safety and health (OHS/OSH):
Main hazards Irritant
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1 0 0
Related compounds
Other anions Ammonium iron(III) citrate
Ammonium chloride
Other cations Ammonium aluminium sulfate
potassium aluminium sulfate
Related compounds Ammonium iron(II) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). ☒N verify (what is  ?) Infobox references
Chemical compound

Ammonium iron(III) sulfate, NH4Fe(SO4)2·12 H2O, or NH4(SO4)2·6 H2O, also known as ferric ammonium sulfate (FAS) or iron alum, is a double salt in the class of alums, which consists of compounds with the general formula AB(SO4)2 · 12 H2O. It has the appearance of weakly violet, octahedrical crystals. There has been some discussion regarding the origin of the crystals' color, with some ascribing it to impurities in the compound, and others claiming it to be a property of the crystal itself.

FAS is paramagnetic, acidic and toxic towards microorganisms. It is a weak oxidizing agent, capable of being reduced to Mohr's salt, ferrous ammonium sulfate.

Preparation

FAS can be prepared by crystallization from a solution of ferric sulfate and ammonium sulfate. Iron(II) in ferrous sulfate is oxidized to ferric sulfate by addition of sulfuric and nitric acid. 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 degree of hydration of the material.

Oxidation: 6 FeSO4 + 2 HNO3 + 3 H2SO4 → 3 Fe2(SO4)3 + 2 NO + 4 H2O
Synthesis: Fe2(SO4)3 + (NH4)2SO4 → 2 NH4Fe(SO4)2

Uses

Areas of use for FAS include waste water treatment, tanning, production of dyestuffs, and as an etching agent in the production of electronic components. It has been used in a wide area of applications, including adiabatic refrigeration equipment, biochemical analysis, and organic synthesis.

Gallery

  • Crystals of ferric ammonium sulfate Crystals of ferric ammonium sulfate
  • Crystals of ammonium iron(III) sulfate after 16 days in the air Crystals of ammonium iron(III) sulfate after 16 days in the air

References

  1. "Material Safety Data Sheet. Iron (III) Ammonium Sulfate Dodecahydrate". fscimage.fishersci.com. Retrieved 8 June 2023.
  2. Considine, Douglas M: Chemical and process technology encyclopedia, McGraw-Hill, New York, 1974, p. 993
  3. 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: 173–95.
  4. Bonnell, Jane; Philip Perman, Edgar (1921). "CCXXIX.—The colour of iron alum". J. Chem. Soc., Trans. 119: 1994–1997. doi:10.1039/CT9211901994.
  5. Cooke, Meyer; Wolf (1956). "The Specific Heats of Three Paramagnetic salts at Very Low Temperatures". Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences. 237 (1210): 395–403. Bibcode:1956RSPSA.237..395C. doi:10.1098/rspa.1956.0185. S2CID 97076961.
  6. Wang, Fei; et al. (2008). "Microcalorimetric investigation of the toxic action of ammonium ferric(III)sulfate on the metabolic activity of pure microbes". Environmental Toxicology and Pharmacology. 25 (3): 351–357. Bibcode:2008EnvTP..25..351W. doi:10.1016/j.etap.2007.11.004. PMID 21783873.
  7. ^ Wiley Encyclopedia of inorganic chemistry: Volume 4, p. 1704:
  8. Chen et al.: United States Patent 5518131 – "Etching molydbenum with ferric sulfate and ferric ammonium sulfate"
  9. 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
  10. 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.
  11. Yu, Shanxin; et al. (2005). "Application of ammonium ferric sulfate dodecahydrate in organic synthesis". General Review. 17 (1): 27–30.
Ammonium salts
Inorganic salts
monatomic anions
oxyanions
other anions
Organic salts
Iron compounds
Fe(−II)
Fe(0)
Fe(I)
Organoiron(I) compounds
  • (C5H5FeCO)2(CO)2
    • Fe(0,II)
    Fe(II)
    Organoiron(II) compounds
    Fe(0,III)
    Fe(II,III)
    Fe(III)
    Organoiron(III) compounds
    Fe(IV)
    Fe(VI)
    Purported
    sort
    Compounds containing the sulfate group (SO2−4)
    H2SO4 He
    Li2SO4 BeSO4 B2S2O9
    -BO3
    +BO3     		esters
    ROSO−3
    (RO)2SO2
    +CO3
    +C2O4     		(NH4)2SO4
    [N2H5]HSO4
    (NH3OH)2SO4
    NOHSO4
    +NO3     		H2OSO4 +F Ne
    Na2SO4
    NaHSO4     		MgSO4 Al2(SO4)3
    Al2SO4(OAc)4     		Si +PO4 SO2−4
    HSO3HSO4
    (HSO4)2
    +SO3     		+Cl Ar
    K2SO4
    KHSO4     		CaSO4 Sc2(SO4)3 TiOSO4 VSO4
    V2(SO4)3
    VOSO4     		CrSO4
    Cr2(SO4)3     		MnSO4 FeSO4
    Fe2(SO4)3     		CoSO4
    Co2(SO4)3     		NiSO4
    Ni2(SO4)3     		CuSO4
    Cu2SO4
    SO4     		ZnSO4 Ga2(SO4)3 Ge(SO4)2 As +SeO3 +Br Kr
    RbHSO4
    Rb2SO4     		SrSO4 Y2(SO4)3 Zr(SO4)2 Nb2O2(SO4)3 MoO(SO4)2
    MoO2(SO4)     		Tc Ru(SO4)2 Rh2(SO4)3 PdSO4 Ag2SO4
    AgSO4     		CdSO4 In2(SO4)3 SnSO4
    Sn(SO4)2     		Sb2(SO4)3 TeOSO4 I2(SO4)3
    (IO)2SO4
    +IO3     		Xe
    Cs2SO4
    CsHSO4     		BaSO4 * Lu2(SO4)3 Hf(SO4)2 Ta WO(SO4)2 Re2O5(SO4)2 OsSO4
    Os2(SO4)3
    Os(SO4)2     		IrSO4
    Ir2(SO4)3     		Pt2(SO4)5 AuSO4
    Au2(SO4)3     		Hg2SO4
    HgSO4     		Tl2SO4
    Tl2(SO4)3     		PbSO4
    Pb(SO4)2     		Bi2(SO4)3 PoSO4
    Po(SO4)2     		At Rn
    Fr RaSO4 ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
     
    * La2(SO4)3 Ce2(SO4)3
    Ce(SO4)2     		Pr2(SO4)3 Nd2(SO4)3 Pm2(SO4)3 Sm2(SO4)3 EuSO4
    Eu2(SO4)3     		Gd2(SO4)3 Tb2(SO4)3 Dy2(SO4)3 Ho2(SO4)3 Er2(SO4)3 Tm2(SO4)3 Yb2(SO4)3
    ** Ac2(SO4)3 Th(SO4)2 Pa U2(SO4)3
    U(SO4)2
    UO2SO4     		Np(SO4)2 Pu(SO4)2 Am2(SO4)3 Cm2(SO4)3 Bk Cf2(SO4)3 Es Fm Md No
    Categories: