Vanadium(III) sulfate: Difference between revisions
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! {{chembox header}}| '''{{PAGENAME}}''' |
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{{Citation |
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| last = Lide |
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| align="center" colspan="2" bgcolor="#ffffff" | [[Image:{{PAGENAME}}.jpg|200px|{{PAGENAME}}]] <!-- replace if not identical with the pagename --> |
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| first = David R. |
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| year = 1998 |
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| [[Vanadium Trisulfate]] |
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| title = Handbook of Chemistry and Physics |
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| edition = 87 |
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| location = Boca Raton, FL |
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| publisher = CRC Press |
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| [[Molecular formula]] |
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| isbn = 0-8493-0594-2 |
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| V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
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| pages = 4–93 |
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}}</ref> |
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| [[Molar mass]] |
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| ImageFile = (V(aq)6)2(SO4)3.svg |
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| 390.07 g/mol |
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| IUPACName = Vanadium(III) sulfate |
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| [[Solubility]] ([[Water_(molecule)|water]]) |
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| OtherNames = Vanadium trisulfate<BR>Divanadium trisulfate |
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| Slowly soluble |
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| CASNo = 13701-70-7 |
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| Lemon-yellow power |
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| align="center" cellspacing="3" style="border: 1px solid #C0C090; background-color: #F8EABA; margin-bottom: 3px;" colspan="2" |<small>[[wikipedia:Chemical infobox|Disclaimer and references]]</small> |
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| UNII = 1EQF3LAK57 |
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| EINECS = 237-226-6 |
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| PubChem = 166888 |
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| ChemSpiderID =19990317 |
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| Formula = V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
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| MolarMass = 390.074 g/mol |
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| Appearance = Yellow powder |
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| Density = |
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| MeltingPtC = 400 |
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| MeltingPt_notes = Decomposes |
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| Solubility = Slightly soluble |
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'''Vanadium(III) sulfate''' is the [[inorganic compound]] with the formula V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>. 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 [[Metal aquo complex|aquo complex]] [V(H<sub>2</sub>O)<sub>6</sub>]<sup>3+</sup>. |
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'''Vanadium trisulfate'' is prepared by the reduction of V<sub>2</sub>O<sub>5</sub> in [[sulfuric acid]] with elemental sulfur. When heated in vacuum at or slightly below 410º, it decomposes into VOSO<sub>4</sub> and SO<sub>2</sub>. Vanadium trisulfate is stable in dry air but upon exposure to moist air for several weeks forms a green hydrate form. Vanadium trisulfate is a powerful [[reducing agent.]] |
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The compound is prepared by treating V<sub>2</sub>O<sub>5</sub> in [[sulfuric acid]] with elemental [[sulfur]]:<ref>{{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}}</ref> |
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==External links== |
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:{{chem2 | V2O5 + S + 3 H2SO4 -> V2(SO4)3 + SO2 + 3 H2O }} |
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This transformation is a rare example of a reduction by elemental sulfur. |
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When heated in vacuum at or slightly below 410 °C, it decomposes into [[vanadyl sulfate]] (VOSO<sub>4</sub>) and SO<sub>2</sub>. Vanadium(III) sulfate is stable in dry air but upon exposure to moist air for several weeks forms a green hydrate form. |
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Vanadium(III) sulfate is a [[reducing agent]]. |
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==References== |
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{{reflist}} |
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{{Vanadium compounds}} |
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{{Sulfates}} |
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[[Category:Vanadium(III) compounds]] |
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[[Category:Sulfates]] |
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[[Category:Vanadium compounds]] |
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[[Category:Oxides]] |
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{{inorganic-compound-stub}} |
{{inorganic-compound-stub}} |
Latest revision as of 16:07, 30 June 2024
![]() | |
Names | |
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IUPAC name
Vanadium(III) sulfate
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Other names
Vanadium trisulfate
Divanadium trisulfate | |
Identifiers | |
ChemSpider | |
ECHA InfoCard | 100.033.827 |
EC Number |
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PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
V2(SO4)3 | |
Molar mass | 390.074 g/mol |
Appearance | Yellow powder |
Melting point | 400 °C (752 °F; 673 K) Decomposes |
Slightly soluble | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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:[2]
- 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.
References
[edit]- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–93, ISBN 0-8493-0594-2
- ^ Claunch, Robert T.; Jones, Mark M.; Wolsey, Wayne C. (1963). "Vanadium(III) Sulfate". Inorganic Syntheses. Vol. 7. pp. 92–94. doi:10.1002/9780470132388.ch28. ISBN 978-0-470-13166-4.