:Vanadium(III) sulfate

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| Reference =

{{Citation

| last = Lide

| first = David R.

| year = 1998

| title = Handbook of Chemistry and Physics

| edition = 87

| location = Boca Raton, FL

| publisher = CRC Press

| isbn = 0-8493-0594-2

| pages = 4–93

}}

| ImageFile = (V(aq)6)2(SO4)3.svg

| ImageSize =

| IUPACName = Vanadium(III) sulfate

| OtherNames = Vanadium trisulfate
Divanadium trisulfate

|Section1={{Chembox Identifiers

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| CASNo = 13701-70-7

| CASNo_Ref = {{cascite|correct|CAS}}

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 1EQF3LAK57

| EINECS = 237-226-6

| PubChem = 166888

| ChemSpiderID =19990317

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|Section2={{Chembox Properties

| Formula = V₂(SO₄)₃

| MolarMass = 390.074 g/mol

| Appearance = Yellow powder

| Density =

| MeltingPtC = 400

| MeltingPt_notes = Decomposes

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| Solubility = Slightly soluble

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|Section7={{Chembox Hazards

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Vanadium(III) sulfate is the inorganic compound with the formula V₂(SO₄)₃. It is a pale yellow solid that is stable to air, in contrast to most vanadium(III) compounds. It slowly dissolves in water to give the green aquo complex [V(H₂O)₆]³⁺.

The compound is prepared by treating V₂O₅ in sulfuric acid with elemental sulfur:{{cite book | doi = 10.1002/9780470132388.ch28| chapter = Vanadium(III) Sulfate| title = Inorganic Syntheses| date = 1963| last1 = Claunch| first1 = Robert T.| last2 = Jones| first2 = Mark M.| last3 = Wolsey| first3 = Wayne C.| volume = 7| pages = 92–94| isbn = 978-0-470-13166-4}}

:{{chem2 | V2O5 + S + 3 H2SO4 -> V2(SO4)3 + SO2 + 3 H2O }}

This transformation is a rare example of a reduction by elemental sulfur.

When heated in vacuum at or slightly below 410 °C, it decomposes into vanadyl sulfate (VOSO₄) and SO₂. Vanadium(III) sulfate is stable in dry air but upon exposure to moist air for several weeks forms a green hydrate form.

Vanadium(III) sulfate is a reducing agent.