Sulfuric acid, iron(3+) salt (3:2)
|Molar mass||399.88 g/mol (anhydrous)
489.96 g/mol (pentahydrate)
562.00 g/mol (nonahydrate)
|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)
440 g/ 100g (20 ºC) 
|Solubility||sparingly soluble in alcohol
negligible in acetone, ethyl acetate
insoluble in sulfuric acid, ammonia
Refractive index (nD)
|EU Index||Not listed|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|500 mg/kg (oral, rat)|
|US health exposure limits (NIOSH):|
|TWA 1 mg/m3|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is: / ?)(|
Iron(III) sulfate (or ferric sulfate), is the chemical compound with the formula Fe2(SO4)3, the sulfate of trivalent iron. Usually yellow, it is a rhombic crystalline salt and soluble in water at room temperature. It is used in dyeing as a mordant, and as a coagulant for industrial wastes. It is also used in pigments, and in pickling baths for aluminum and steel. Medically it is used as an astringent and styptic.
Mikasaite, a mixed iron-aluminium sulfate of chemical formula (Fe3+, Al3+)2(SO4)3 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 met 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 compounds connected with Fe-bearing primary minerals (mainly pyrite and marcasite) oxidation in ore beds. In the solutions of the ore beds oxidation zones the iron(III) sulfate is also an important oxidative agent.
- 2FeSO4 + H2SO4 + H2O2 → Fe2(SO4)3 + 2H2O
Ferric sulfate and jarosite have been detected by the two martian rovers Spirit and Opportunity. These substances are indicative of strongly oxidizing conditions prevailing at the surface of Mars. In May 2009, the Spirit rover became stuck when it drove over a patch of soft ferric sulfate that had been hidden under a veneer of normal-looking soil. Because iron sulfate has very little cohesion, the rover's wheels could not gain sufficient traction to pull the body of the rover out of the iron sulfate patch. Multiple techniques were attempted to extricate the rover, but the wheels eventually sunk so deeply into the iron sulfate that the body of the rover came to rest on the martian surface, preventing the wheels from exerting any force on the material below them. As the JPL team failed to recover the mobility of Spirit, it signified the end of the journey for the rover.
- David R., Lide (2010). "Physical Constants of Inorganic Compounds", in CRC Handbook of Chemistry and Physics, 90th Edition (Internet Version 2010). CRC Press/Taylor and Francis, Boca Raton, FL. ISBN 1-4200-9084-4.
- "NIOSH Pocket Guide to Chemical Hazards #0346". National Institute for Occupational Safety and Health (NIOSH).
- Ferric sulfate. The Columbia Encyclopedia, Sixth Edition. Retrieved November, 2007.
- Ferric sulfate. Online medical dictionary. Retrieved November, 2007
- Iron compounds. Encyclopædia Britannica Article. Retrieved November, 2007
- Chang, Kenneth (2009-05-19). "Mars rover’s 5 working wheels are stuck in hidden soft spot". The New York Times. ISSN 0362-4331. Retrieved 2009-05-19.
|Salts and the ester of the sulfate ion|