Vanadyl sulfate

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Vanadyl sulfate
Vanadyl sulfate
Vanadyl sulfate.jpg
IUPAC name
Oxovanadium(2+) sulfate
Other names
Basic vanadium(IV) sulfate
Vanadium(IV) oxide sulfate
Vanadium(IV) oxysulfate
27774-13-6 N
Molar mass 163.00 g/mol
Appearance Blue crystalline solid
Melting point 105 °C (221 °F; 378 K) decomposes
Main hazards Irritant
Flash point Non-flammble
Related compounds
Other anions
Vanadyl chloride
Vanadyl nitrate
Other cations
Vanadium(III) sulfate
Related compounds
Vanadyl acetylacetonate
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

Vanadyl(IV) sulfate, VOSO4, is a well known inorganic compound of vanadium. This very hygroscopic blue solid is one of the most common sources of vanadium in the laboratory, reflecting its high stability. It features the vanadyl ion, VO2+, which has been called the "most stable diatomic ion."[1] Vanadyl sulfate is an intermediate in the extraction of vanadium from petroleum residues, a major commercial source of vanadium.[2] Vanadyl sulfate is a component of some food supplements and experimental drugs. Vanadyl sulfate exhibits insulin-like effects.[3]

Synthesis, structure, and reactions[edit]

Vanadyl sulfate is most commonly obtained by reduction of vanadium pentoxide with sulfur dioxide:

V2O5 + 7 H2O + SO2 + H2SO4 → 2 [V(O)(H2O)4]SO4

From aqueous solution, the salt crystallizes as the pentahydrate, the fifth water is not bound to the metal in the solid. Viewed as a coordination complex, the ion is octahedral, with oxo, four equatorial water ligands, and a monodentate sulfate.[1] The V=O bond distance is 160 pm in length, about 50 pm shorter than the V–OH2 bonds. In solution, the sulfate ion dissociates rapidly.

Being widely available, vanadyl sulfate is a common precursor to other vanadyl derivatives, such as vanadyl acetylacetonate:[4]

[V(O)(H2O)4]SO4 + 2C5H8O2 + Na2CO3 → [V(O)(C5H7O2)2] + Na2SO4 + 5 H2O + CO2

In acidic solution, oxidation of vanadyl sulfate gives yellow-coloured vanadyl(V) derivatives. Reduction, e.g. by zinc, gives vanadium(III) and vanadium(II) derivatives, which are characteristically green and violet, respectively.

Occurrence in nature[edit]

Like most water-soluble sulfates, vanadyl sulfate is only rarely found in nature. Anhydrous form is pauflerite, a mineral of fumarolic origin. Hydrated forms, also rare, include hexahydrate (stanleyite), pentahydrates (minasragrite, orthominasragrite, and anorthominasragrite) and trihydrate - bobjonesite.[citation needed]


  1. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 1157. ISBN 0-08-022057-6. 
  2. ^ Günter Bauer, Volker Güther, Hans Hess, Andreas Otto, Oskar Roidl, Heinz Roller, Siegfried Sattelberger in "Vanadium and Vanadium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.
  3. ^ Crans, D. C., Trujillo, A. M., Pharazyn, P. S., Cohen, M. D., "How environment affects drug activity: Localization, compartmentalization and reactions of a vanadium insulin-enhancing compound, dipicolinatooxovanadium(V)", Coord. Chem. Rev. 2011, 255, 2178. doi:10.1016/j.ccr.2011.01.032
  4. ^ Bryant, Burl E.; Fernelius, W. Conard (1957), "Vanadium(IV) Oxy(acetylacetonate)", Inorg. Synth. 5: 113–16, doi:10.1002/9780470132364.ch30