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| Names | |
|---|---|
| IUPAC name
Sodium vanadate(V)
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| Other names
Sodium vanadium oxide
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ECHA InfoCard | 100.033.883 |
PubChem CID
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| RTECS number |
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| Na3VO4 | |
| Molar mass | 183.908 g/mol |
| Appearance | white powder |
| Density | 2.16 g/cm3, solid |
| Melting point | 858 °C (1,576 °F; 1,131 K) |
| 22.17 g/100 mL | |
| Solubility | insoluble in ethanol |
| Structure | |
| cubic | |
| Thermochemistry | |
Heat capacity (C)
|
164.8 J/mol K |
Std molar
entropy (S⦵298) |
190 J/mol K |
Std enthalpy of
formation (ΔfH⦵298) |
−1757 kJ/mol |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
Harmful. |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
330 mg/kg (oral, rat) |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium orthovanadate is the inorganic compound with the chemical formula Na3V O4. It forms a dihydrate Na3VO4·2H2O. Sodium orthovanadate is a salt of the VO3−4 oxyanion. It is a colorless, water-soluble solid.[2]
Synthesis and structure[edit]
Sodium orthovanadate is produced by dissolving vanadium(V) oxide in a solution of sodium hydroxide:
- V2O5 + 6 NaOH → 2 Na3VO4 + 3 H2O
The salt features tetrahedral VO3−4 anion centers linked to octahedral Na+ cation sites.[3]
Condensation equilibria[edit]
Like many oxometalates, orthovanadate is subject to a number of reactions, which have been analyzed by 51V NMR studies. At high pH, VO3−4 ions exist in equilibrium with HVO2−4.[4] At lower pH's, condensation ensues to give various polyoxovanadates. Ultimately, decavanadate is formed.[5]
Biochemistry[edit]
Vanadates exhibit a variety of biological activities, in part because they serve as structural mimics of phosphates.[6][7] It acts as a competitive inhibitor of ATPases, alkaline and acid phosphatases, and protein-phosphotyrosine phosphatases,[8] and its inhibitory effects can be reversed by dilution or the addition of ethylenediaminetetraacetic acid (EDTA).[9]
Orthovanadate is activated by boiling and adjusting pH to ~10; this depolymerizes decavanadate into the active inhibitor, monovanadate.[8]
References[edit]
- ^ "Archived copy". Archived from the original on 2016-03-04. Retrieved 2017-09-28.
{{cite web}}: CS1 maint: archived copy as title (link) - ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Kato, K.; Takayama-Muromachi, E. (1987). "Die Struktur des Trinatriumvanadattrihydrats" [The structure of trisodium vanadate trihydrate] (PDF). Acta Crystallogr. C43 (6): 1030–1032. Bibcode:1987AcCrC..43.1030K. doi:10.1107/S0108270187093120.
- ^ Rehder, D.; Polenova, T.; Bühl, M. (2007). Vanadium-51 NMR. Annual Reports on NMR Spectroscopy. Vol. 62. pp. 49–114. doi:10.1016/S0066-4103(07)62002-X. ISBN 9780123739193.
- ^ Klemperer, W. G.; Yaghi, O. (1983). "Tetrabutylammonium Trihydrogen Decavanadate(V)". Inorg. Synth. 27: 83. doi:10.1002/9780470132586.ch15.
- ^ Korbecki, Jan; Baranowska-Bosiacka, Irena; Gutowska, Izabela; Chlubek, Dariusz (2012). "Biochemical and medical importance of vanadium compounds" (PDF). Acta Biochim. Pol. 59 (2): 195–200. doi:10.18388/abp.2012_2138. PMID 22693688.
- ^ Crans, D. C.; Chatterjee, P. B. (2013). "Vanadium biochemistry". In Reedijk, Jan; Poeppelmeier, Kenneth (eds.). Comprehensive Inorganic Chemistry II: From Elements to Applications. Comprehensive Inorganic Chemistry II. Vol. 3. pp. 323–342. doi:10.1016/B978-0-08-097774-4.00324-7. ISBN 978-0-08-097774-4.
- ^ a b "Sodium orthovanadate" (PDF). Sigma-Aldrich. Retrieved September 7, 2018.
- ^ Biolabs, New England. "Sodium Orthovanadate (Vanadate) | NEB". www.neb.com. Retrieved 2018-09-07.