Iron(III) sulfate

Names
IUPAC name

Iron(III) sulfate

Other names

Ferric sulfate

Identifiers

CAS Number

* 10028-22-5 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:53438 Y

ChemSpider |

* 23211 Y

PubChem CID

* 24826

RTECS number |

* NO8505000

UNII |

* 4YKQ1X5E5Y N

InChI

* InChI=1S/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6 Y

Key: RUTXIHLAWFEWGM-UHFFFAOYSA-H Y

* InChI=1/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6

Key: RUTXIHLAWFEWGM-CYFPFDDLAR

SMILES

* [Fe+3].[Fe+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O

Properties

Chemical formula

| Fe2(SO4)3
Molar mass | 399.88 g/mol (anhydrous)
489.96 g/mol (pentahydrate)
562.00 g/mol (nonahydrate)
Appearance  | grayish-white crystals
Density | 3.097 g/cm3 (anhydrous)
1.898 g/cm3 (pentahydrate)
Melting point |  480 °C (896 °F; 753 K) (anhydrous)(decomposes)
175 °C (347 °F) (nonahydrate)

Solubility in water

| 256g/L (monohydrate, 293K)
Solubility | sparingly soluble in alcohol
negligible in acetone, ethyl acetate
insoluble in sulfuric acid, ammonia

Refractive index (nD)

| 1.814 (anhydrous)
1.552 (nonahydrate)
Hazards
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 500 mg/kg (oral, rat)
NIOSH (US health exposure limits):

REL (Recommended)

| TWA 1 mg/m3[1]
Related compounds

Other anions

| Iron(III) chloride
Iron(III) nitrate

Related compounds

| Iron(II) sulfate

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Iron(III) sulfate (or ferric sulfate), is a family of inorganic compounds with the formula Fe2(SO4)3(H2O)n. A variety of hydrates are known, including the most commonly encountered form of "ferric sulfate". Solutions are used in dyeing as a mordant, and as a coagulant for industrial wastes. Solutions of ferric sulfate are also used in the processing of aluminum and steel.[2][3]

## Contents

* 1 Speciation
* 2 Production
* 3 Natural occurrences
* 4 See also
* 5 References
* 6 External links

## Speciation

The various crystalline forms of Fe2(SO4)3(H2O)n are well-defined, often by X-ray crystallography. The nature of the aqueous solutions is often less certain, but aquo-hydroxo complexes such as [Fe(H2O)6]3+ and [Fe(H2O)5(OH)]2+ are often assumed.[4] Regardless, all such solids and solutions feature ferric ions, each with five unpaired electrons. By virtue of this high spin d5 electronic configuration, these ions are paramagnetic and are weak chromophores.

## Production

Ferric sulfate solutions are usually generated from iron wastes. The actual identity of the iron species is often vague, but many applications do not demand high purity materials. It is produced on a large scale by treating sulfuric acid, a hot solution of ferrous sulfate, and an oxidizing agent. Typical oxidizing agents include chlorine, nitric acid, and hydrogen peroxide.[5]

2 FeSO4 \+ H2SO4 \+ H2O2 → Fe2(SO4)3 \+ 2 H2O

## Natural occurrences

Iron sulfates occur as a variety of rare (commercially unimportant) minerals. Mikasaite, a mixed iron-aluminium sulfate of chemical formula (Fe3+, Al3+)2(SO4)3[6] is the name of mineralogical form of iron(III) sulfate. This anhydrous form occurs very rarely and is connected with coal fires. The hydrates are more common, with coquimbite[7] (nonahydrate) as probably the most often met among them. Paracoquimbite is the other, rarely encountered natural nonahydrate. Kornelite (heptahydrate) and quenstedtite (decahydrate) are rarely found. Andradite garnet is a yellow-green example found in Italy.[8] Lausenite (hexa- or pentahydrate) is a doubtful species. All the mentioned natural hydrates are unstable connected with the weathering (aerobic oxidation) of Fe-bearing primary minerals (mainly pyrite and marcasite).

Coquimbite crystal structure

## See also

* Iron(II) sulfate or ferrous sulfate
* Ammonium iron(II) sulfate
* Ammonium iron(III) sulfate

## References

1. ↑ NIOSH Pocket Guide to Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0346.html.
2. ↑ Ferric sulfate. The Columbia Encyclopedia, Sixth Edition. Retrieved November, 2007.
3. ↑ Wildermuth, Egon; Stark, Hans; Friedrich, Gabriele; Ebenhöch, Franz Ludwig; Kühborth, Brigitte; Silver, Jack; Rituper, Rafael (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a14_591.
4. ↑ Grant, M.; Jordan, R. B. (1981). "Kinetics of Solvent Water Exchange on Iron(III)". Inorganic Chemistry 20: 55–60. doi:10.1021/ic50215a014.
5. ↑ Iron compounds. Encyclopædia Britannica Article. Retrieved November, 2007
6. ↑ Mikasaite
7. ↑ "Minerals Colored by Metal Ions". http://minerals.gps.caltech.edu/color_causes/Metal_Ion/index.html.
8. ↑ "Minerals Colored by Metal Ions". http://minerals.gps.caltech.edu/color_causes/Metal_Ion/index.html.

## External links

* Material Safety Data Sheet

* v
* t
* e

Iron compounds

Fe(-II)|

* Na2Fe(CO)4

Fe(0)|

* Fe(CO)5
* Fe2(CO)9
* Fe3(CO)12
* Fe(CO)3CH3COC2H2C6H6

Fe(I)|

* FeH

| Organoiron(I) compounds|

* (C5H5FeCO)2(CO)2

|

Fe(0,II)|

* Fe3C

Fe(II)|

* FeBr2
* FeCl2
* FeF2
* FeI2
* FeH2
* FeMoO4
* FeO
* Fe(OH)2
* FeS
* FeSO4
* FeSe
* FeSeO4
* FeSi2
* FeTiO3
* FeCO3
* FeC2O4
* Fe(C2H3O2)2
* Fe(C3H5O3)2
* FeC6H6O7
* FeC12H22O14
* Fe2CrO4
* Fe3(PO4)2
* H2Fe(CO)4
* Fe(HCO3)2
* Mg2FeH6

| Organoiron(II) compounds|

* Fe(C5H5)2
* Fe(C5H4P(C6H5)2)2
* C4H4Fe(CO)3
* C4H6Fe(CO)3

|

Fe(0,III)|

* Fe3P

Fe(II,III)|

* Fe3O4
* Fe3S4

Fe(III)|

* FeBr3
* FeCl3
* FeF3
* FeI3
* Fe(NO3)3
* Fe(acac)3
* FeOCl
* FeO(OH)
* FePO4
* Fe4(P2O7)3
* Fe2(CrO4)3
* Fe2(C2O4)3
* Fe2O3
* Fe2S3
* Fe2(SO4)3
* FeBO3
* FeB

| Organoiron(III) compounds|

* Fe(C5H5)2BF4
* C6H8O7⋅xFe3+⋅yNH3

|

Fe(VI)|

* K2FeO4
* BaFeO4

* v
* t
* e

Compounds containing the sulfate group

H2SO4 |  |  |  | He

|
|
|
|

Li2SO4 | BeSO4 | B  | esters
ROSO3−
(RO)2SO2 | (NH4)2SO4
[N2H5]HSO4
(NH3OH)2SO4
NOHSO4 | HOSO4 | F  | Ne
Na2SO4
NaHSO4 | MgSO4 | Al2(SO4)3
Al2SO4(OAc)4 | Si  | P  | SO42−
HSO3HSO4
(HSO4)2 | Cl  | Ar
K2SO4
KHSO4 | CaSO4 | Sc2(SO4)3 | TiOSO4 | VSO4
V2(SO4)3
VOSO4 | CrSO4
Cr2(SO4)3 | MnSO4 | FeSO4
Fe2(SO4)3 | CoSO4 | NiSO4 | CuSO4
Cu2SO4
[Cu(NH3)4(H2O)]SO4 | ZnSO4 | Ga2(SO4)3 | Ge  | As  | Se  | Br  | Kr
RbHSO4
Rb2SO4 | SrSO4 | Y2(SO4)3 | Zr(SO4)2 | Nb  | Mo  | Tc  | Ru  | Rh2(SO4)3 | PdSO4 | Ag2SO4 | CdSO4 | In2(SO4)3 | SnSO4
Sn(SO4)2 | Sb2(SO4)3 | Te  | I  | Xe
Cs2SO4
CsHSO4 | BaSO4 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt  | AuSO4
Au2(SO4)3 | Hg2SO4
HgSO4 | Tl2SO4
Tl2(SO4)3 | PbSO4 | Bi2(SO4)3 | Po  | At  | Rn
Fr  | Ra  |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce2(SO4)3
Ce(SO4)2 | Pr2(SO4)3 | Nd  | Pm  | Sm  | Eu  | Gd  | Tb  | Dy  | Ho  | Er  | Tm  | Yb2(SO4)3 | Lu
Ac  | Th  | Pa  | U(SO4)2
UO2SO4 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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