Vanadium(III) sulfate: Difference between revisions
Appearance
Content deleted Content added
m oops doi |
image |
||
(22 intermediate revisions by 16 users not shown) | |||
Line 2: | Line 2: | ||
| Reference = <ref name="hand"> |
| Reference = <ref name="hand"> |
||
{{Citation |
{{Citation |
||
| last = Lide |
|||
| first = David R. |
|||
| year = 1998 |
|||
⚫ | |||
| last2 = |
|||
| edition = 87 |
|||
⚫ | |||
| author2-link = |
|||
⚫ | |||
| publication-date = |
|||
⚫ | |||
| date = |
|||
| pages = 4–93 |
|||
⚫ | |||
| edition = 87 |
|||
| volume = |
|||
| series = |
|||
⚫ | |||
| place = |
|||
⚫ | |||
| id = |
|||
⚫ | |||
| doi = |
|||
| oclc = |
|||
| pages = 4–93 |
|||
| url = |
|||
| accessdate = |
|||
}}</ref> |
}}</ref> |
||
| ImageFile = |
| ImageFile = (V(aq)6)2(SO4)3.svg |
||
| ImageSize = |
| ImageSize = |
||
| IUPACName = Vanadium(III) sulfate |
| IUPACName = Vanadium(III) sulfate |
||
| OtherNames = Vanadium trisulfate |
| OtherNames = Vanadium trisulfate<BR>Divanadium trisulfate |
||
| |
|Section1={{Chembox Identifiers |
||
| Abbreviations = |
| Abbreviations = |
||
| CASNo = 13701-70-7 |
| CASNo = 13701-70-7 |
||
| CASNo_Ref = {{cascite|correct|CAS}} |
|||
| UNII_Ref = {{fdacite|correct|FDA}} |
|||
| UNII = 1EQF3LAK57 |
|||
| EINECS = 237-226-6 |
| EINECS = 237-226-6 |
||
| PubChem = 166888 |
| PubChem = 166888 |
||
| ChemSpiderID=19990317 |
| ChemSpiderID =19990317 |
||
| SMILES = |
| SMILES = |
||
| InChI = |
| InChI = |
||
Line 41: | Line 30: | ||
| MeSHName = |
| MeSHName = |
||
| ChEBI = |
| ChEBI = |
||
| KEGG = |
| KEGG = |
||
}} |
|||
| ATCCode_prefix = |
|||
⚫ | |||
| ATCCode_suffix = |
|||
⚫ | |||
⚫ | |||
| Formula = V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
| Formula = V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
||
| MolarMass = 390.074 g/mol |
| MolarMass = 390.074 g/mol |
||
| Appearance = |
| Appearance = Yellow powder |
||
| Density = |
| Density = |
||
| |
| MeltingPtC = 400 |
||
| MeltingPt_notes = Decomposes |
|||
| Melting_notes = |
|||
| BoilingPt = |
| BoilingPt = |
||
| |
| BoilingPt_notes = |
||
| Solubility = |
| Solubility = Slightly soluble |
||
| SolubleOther = |
| SolubleOther = |
||
| Solvent = |
| Solvent = |
||
| pKa = |
| pKa = |
||
| pKb = }} |
| pKb = }} |
||
| |
|Section6={{Chembox Pharmacology |
||
| |
| ATCCode_prefix = |
||
| |
| ATCCode_suffix = |
||
⚫ | |||
| EUIndex = |
|||
}} |
|||
|Section7={{Chembox Hazards |
|||
| ExternalSDS = |
|||
| MainHazards = |
| MainHazards = |
||
| NFPA-H = |
| NFPA-H = |
||
| NFPA-F = |
| NFPA-F = |
||
| NFPA-R = |
| NFPA-R = |
||
| NFPA- |
| NFPA-S = |
||
| |
| HPhrases = |
||
| |
| PPhrases = |
||
| |
| GHS_ref = |
||
| FlashPt = |
| FlashPt = |
||
| |
| AutoignitionPt = |
||
| ExploLimits = |
| ExploLimits = |
||
| PEL = }} |
| PEL = |
||
}} |
|||
}} |
}} |
||
'''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>. |
'''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>. |
||
The compound is prepared by treating V<sub>2</sub>O<sub>5</sub> in [[sulfuric acid]] with elemental [[sulfur]]:<ref> |
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> |
||
:{{chem2 | V2O5 + S + 3 H2SO4 -> V2(SO4)3 + SO2 + 3 H2O }} |
|||
:V<sub>2</sub>O<sub>5</sub> + S + 3 H<sub>2</sub>SO<sub>4</sub> → V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> + SO<sub>2</sub> + 3 H<sub>2</sub>O |
|||
This transformation is a rare example of a reduction by elemental sulfur. |
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]] (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. |
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. |
||
Vanadium(III) sulfate is a [[reducing agent]]. |
Vanadium(III) sulfate is a [[reducing agent]]. |
||
Line 91: | Line 82: | ||
{{Vanadium compounds}} |
{{Vanadium compounds}} |
||
{{Sulfates}} |
|||
[[Category:Vanadium compounds]] |
[[Category:Vanadium(III) compounds]] |
||
[[Category:Sulfates]] |
[[Category:Sulfates]] |
||
{{inorganic-compound-stub}} |
{{inorganic-compound-stub}} |
||
[[nl:Vanadium(III)sulfaat]] |
Latest revision as of 16:07, 30 June 2024
![]() | |
Names | |
---|---|
IUPAC name
Vanadium(III) sulfate
| |
Other names
Vanadium trisulfate
Divanadium trisulfate | |
Identifiers | |
ChemSpider | |
ECHA InfoCard | 100.033.827 |
EC Number |
|
PubChem CID
|
|
UNII | |
CompTox Dashboard (EPA)
|
|
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).
|
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.