Chromium(III) sulfate

Chromium(III) sulfate

Names
IUPAC name Chromium(III) sulfate
Other names Basic chromium sulfate, chromic sulfate
Identifiers
CAS Number	10101-53-8 Y 15244-38-9 (decahydrate) Y 10031-37-5 (pentadecahydrate) Y 13520-66-6 (octadecahydrate) N
3D model (JSmol)	Interactive image
ChEBI	CHEBI:53471
ChemSpider	23304 Y
ECHA InfoCard	100.030.217
EC Number	233-253-2
PubChem CID	24930
UNII	Y0C99N5TMZ Y 8Q759N78CX (decahydrate) Y E4T8TU3LE8 (pentadecahydrate) Y
UN number	2240 3077
CompTox Dashboard (EPA)	DTXSID20890642
InChI InChI=1S/2Cr.3H2O4S.12H2O/c;;3*1-5(2,3)4;;;;;;;;;;;;/h;;3*(H2,1,2,3,4);12*1H2/q2*+3;;;;;;;;;;;;;;;/p-6 N Key: ANNXSSGQVXBUEI-UHFFFAOYSA-H N InChI=1/2Cr.3H2O4S.12H2O/c;;3*1-5(2,3)4;;;;;;;;;;;;/h;;3*(H2,1,2,3,4);12*1H2/q2*+3;;;;;;;;;;;;;;;/p-6 Key: ANNXSSGQVXBUEI-CYFPFDDLAL
SMILES [Cr+3].[Cr+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O.O.O.O.O.O.O.O.O.O.O.O.O
Properties
Chemical formula	Cr2(SO4)3 • 12H2O
Molar mass	392.16 g/mol 608.363 g/mol (dodecahydrate) 716.45 g/mol (octadecahydrate)
Appearance	reddish-brown crystals (anhydrous), purple crystals (hydrated)
Density	3.10 g/cm3 (anhydrous) 1.86 g/cm3 (pentadecahydrate) 1.709 g/cm3 (octadecahydrate)
Melting point	90 °C
Boiling point	>700 °C (decomposes to chromic acid)
Solubility in water	insoluble (anhydrous) soluble (hydrated)
Solubility	soluble in alcohol practically insoluble in acid
Magnetic susceptibility (χ)	+11,800·10−6 cm3/mol
Hazards
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H314, H317, H332, H334, H335, H340, H350, H373, H412
Precautionary statements	P201, P202, P260, P261, P264, P271, P272, P273, P280, P281, P285, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P304+P341, P305+P351+P338, P308+P313, P310, P312, P314, P321, P333+P313, P342+P311, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)	1 0 0
Flash point	Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3[1]
REL (Recommended)	TWA 0.5 mg/m3[1]
IDLH (Immediate danger)	250 mg/m3[1]
Safety data sheet (SDS)	MSDS
Related compounds
Other cations	Aluminium sulfate
Related double salts	Chrome alum
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

Chromium(III) sulfate usually refers to the inorganic compounds with the formula Cr₂(SO₄)₃^.x(H₂O), where x can range from 0 to 18. Additionally, ill-defined but commercially important "basic chromium sulfates" are known. These salts are usually either violet or green solids that are soluble in water. It is commonly used in tanning leather.

Chromium(III) sulfates

Three chromium(III) sulfates are well characterized:

• Anhydrous chromium(III) sulfate, Cr₂(SO₄)₃, (CAS #10101-53-8) is a violet solid that dissolves in water upon addition of a reducing agent, which generates chromium(II) sulfates.
• Hydrated chromium(III) sulfate, Cr₂(SO₄)₃·18H₂O, (CAS #13520-66-6) is a violet solid that readily dissolves in water to give the metal aquo complex, [Cr(H₂O)₆]³⁺. The formula of this compound can be written more descriptively as [Cr(H₂O)₆]₂(SO₄)₃·6H₂O. Six of the eighteen water molecules in this formula unit are water of crystallization.
• Hydrated chromium(III) sulfate, Cr₂(SO₄)₃·15(H₂O), (CAS #10031-37-5) is a green solid that also readily dissolves in water. It is obtained by heating the 18-hydrate material above 70 °C. Further heating yields the anhydrous sulfate.

A variety of other chromium(III) sulfates are known, but also contain hydroxide or oxide ligands. Most important commercially is basic chromium sulfate, which is thought to be [Cr₂(H₂O)₆(OH)₄]SO₄ (CAS#39380-78-4).^[2] It results from the partial neutralization of the hexahydrates. Other chromium(III) hydroxides have been reported.^[3]

Production

The most useful source of chromium(III) sulfate are the Cr(III) wastes from the chromate oxidation of various organic compounds. Anthroquinone and quinone are produced on large scale by treatment of anthracene and phenol with chromic acid. A chromium(III) oxide coproduct is generated which is readily extracted into sulfuric acid. Evaporation of these acidic solutions affords the hydrate salt described above. The hydrated salts of chromium sulfate can also be produced, albeit impure, by extraction of various other chromium compounds, but these routes are not economically viable.. Extraction of chromite ore with sulfuric acid in the presence of some chromate gives solutions of chromium(III) sulfate contaminated with other metal ions. Similarly, dissolution of chrome alloys gives chromium sulfate together with ferrous sulfate.^{[citation needed]}

Basic chromium(III) sulfate

Basic chromium sulfate is produced from chromate salts by reduction with sulfur dioxide, although other methods exist.^[4][5] The reduction could formally be written:

Na₂Cr₂O₇ + 3 SO₂ + H₂O → Cr₂(SO₄)₃ + 2 NaOH

Since 33% of the anion charges are due to hydroxy ions the basicity is 33% (but in tanning jargon it is known as 33% reduced). Products with higher basicities, e.g. 42% or 50% may be obtained by the addition of sodium carbonate, these are often used in combination with sodium formate. The sodium sulfate is often left in the technical product since it is inert with respect to the tanning process. It is important to fully reduce the hexavalent chromium to trivalent since the hexavalent is more likely to cause health problems for tanners and leather consumers.^{[citation needed]}

Natural occurrence

Pure chromium(III) sulfate, both in anhydrous and hydrous form, is unknown as of 2020 among mineral species. There are three complex minerals that are in part Cr(III) sulfates: bentorite, reddingtonite, and putnisite.^[6][7][8][9]

References

This page was last edited on 3 April 2024, at 13:39