Iron(III) sulfate

  (Redirected from Ferric sulfate)

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

Iron(III) sulfate
Iron(III) sulfate
Names
IUPAC name
Iron(III) sulfate
Other names
Ferric sulfate
Sulfuric acid, iron(3+) salt (3:2)
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.054 Edit this at Wikidata
RTECS number
  • NO8505000
UNII
  • InChI=1S/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6 checkY
    Key: RUTXIHLAWFEWGM-UHFFFAOYSA-H checkY
  • 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
  • [Fe+3].[Fe+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
Properties
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)
175 °C (347 °F) (nonahydrate)
256g/dm3 (monohydrate, 293K)
Solubility sparingly soluble in alcohol
negligible in acetone, ethyl acetate
insoluble in sulfuric acid, ammonia
1.814 (anhydrous)
1.552 (nonahydrate)
Hazards
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
1
0
Lethal dose or concentration (LD, LC):
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 checkY☒N ?)
Infobox references

ProductionEdit

Generally, ferric sulfate is used as a solution generated from iron wastes. The actual speciation is vague but its applications do not demand high purity materials. As such iron(III) sulfate is generated and handled as an aqueous solution. 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.[4]

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

Natural occurrencesEdit

Iron sulfates occur as a variety of rare and commercially unimportant minerals.Mikasaite, a mixed iron-aluminium sulfate of chemical formula (Fe3+, Al3+)2(SO4)3[5] 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 (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. 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 alsoEdit

ReferencesEdit

  1. ^ NIOSH Pocket Guide to 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. ^ Iron compounds. Encyclopædia Britannica Article. Retrieved November, 2007
  5. ^ Mikasaite

External linksEdit