fe2 o3 + h2 so4

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Iron(III) sulfate
Iron(III) sulfate
IUPAC name

Iron(III) sulfate

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Other names

Ferric sulfate


CAS Number

  • 10028-22-5 check

3D model (JSmol)

  • Interactive image
  • CHEBI:53438 check
  • 23211 check
ECHA InfoCard 100.030.054 Edit this at Wikidata

PubChem CID

  • 24826
RTECS number
  • NO8505000
  • 4YKQ1X5E5Y ☒

CompTox Dashboard (EPA)

  • DTXSID5029712 Edit this at Wikidata


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


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



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


Chemical formula

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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)
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


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).

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Infobox references

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 khuông 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]

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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.


Ferric sulfate solutions are usually generated from iron wastes. The actual identity of the iron species is often vague, but many applications vì thế 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[edit]

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 khuông of iron(III) sulfate. This anhydrous khuông 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[edit]

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


  1. ^ NIOSH Pocket Guide vĩ đại Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH).
  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). "Iron Compounds". 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". minerals.gps.caltech.edu. Retrieved 2023-03-01.
  8. ^ "Minerals Colored by Metal Ions". minerals.gps.caltech.edu. Retrieved 2023-03-01.

External links[edit]

  • Material Safety Data Sheet