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]
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)]5+ 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 (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).
iron, sulfate, ferric, sulfate, family, inorganic, compounds, with, formula, variety, hydrates, known, including, most, commonly, encountered, form, ferric, sulfate, solutions, used, dyeing, mordant, coagulant, industrial, wastes, solutions, ferric, sulfate, a. 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 Iron III sulfate NamesIUPAC name Iron III sulfateOther names Ferric sulfateIdentifiersCAS Number 10028 22 5 Y3D model JSmol Interactive imageChEBI CHEBI 53438 YChemSpider 23211 YECHA InfoCard 100 030 054PubChem CID 24826RTECS number NO8505000UNII 4YKQ1X5E5Y NCompTox Dashboard EPA DTXSID5029712InChI InChI 1S 2Fe 3H2O4S c 3 1 5 2 3 4 h 3 H2 1 2 3 4 q2 3 p 6 YKey RUTXIHLAWFEWGM UHFFFAOYSA H YInChI 1 2Fe 3H2O4S c 3 1 5 2 3 4 h 3 H2 1 2 3 4 q2 3 p 6Key RUTXIHLAWFEWGM CYFPFDDLARSMILES Fe 3 Fe 3 O S O O O O S O O O O S O O OPropertiesChemical formula Fe2 SO4 3Molar mass 399 88 g mol anhydrous 489 96 g mol pentahydrate 562 00 g mol nonahydrate Appearance grayish white crystalsDensity 3 097 g cm3 anhydrous 1 898 g cm3 pentahydrate Melting point 480 C 896 F 753 K anhydrous 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 ammoniaRefractive index nD 1 814 anhydrous 1 552 nonahydrate HazardsNFPA 704 fire diamond 100Lethal 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 compoundsOther anions Iron III chlorideIron III nitrateRelated compounds Iron II sulfateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references Contents 1 Speciation 2 Production 3 Natural occurrences 4 See also 5 References 6 External linksSpeciation EditThe 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 5 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 EditFerric 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 H2ONatural occurrences EditIron 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 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 structureSee also EditIron II sulfate or ferrous sulfate Ammonium iron II sulfate Ammonium iron III sulfateReferences Edit 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 Wildermuth Egon Stark Hans Friedrich Gabriele Ebenhoch Franz Ludwig Kuhborth Brigitte Silver Jack Rituper Rafael 2000 Iron Compounds Ullmann s Encyclopedia of Industrial Chemistry Weinheim Wiley VCH doi 10 1002 14356007 a14 591 Grant M Jordan R B 1981 Kinetics of Solvent Water Exchange on Iron III Inorganic Chemistry 20 55 60 doi 10 1021 ic50215a014 Iron compounds Encyclopaedia Britannica Article Retrieved November 2007 MikasaiteExternal links EditMaterial Safety Data Sheet Retrieved from https en wikipedia org w index php title Iron III sulfate amp oldid 1115498588, wikipedia, wiki, book, books, library,
