Article · Wikipedia archive · Last revised Jun 13, 2026

Sodium decavanadate

Sodium decavanadate describes any member of the family of inorganic compounds with the formula Na6[V10O28]·nH2O. These are sodium salts of the orange-colored decavanadate anion [V10O28]6−. Numerous other decavanadate salts have been isolated and studied since 1956 when it was first characterized.

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Jun 13, 2026
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Source
Wikipedia ↗
Sodium decavanadate
source ↗
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Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • (anhydrous): 235-375-1
  • InChI=1S/6Na.28O.10V/q6*+1;28*-2;10*+5
    Key: WSNCYQDYQWKFLZ-UHFFFAOYSA-N
  • (anhydrous): [O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[O-2].[Na+].[Na+].[Na+].[Na+].[Na+].[Na+].[V].[V].[V].[V].[V].[V].[V].[V].[V].[V]
Properties
Na6[V10O28]
Molar mass 1419.6 g/mol
Appearance orange solid
Related compounds
Other anions
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 decavanadate describes any member of the family of inorganic compounds with the formula Na6[V10O28]·nH2O. These are sodium salts of the orange-colored decavanadate anion [V10O28]6−.1 Numerous other decavanadate salts have been isolated and studied since 1956 when it was first characterized.2

Acid-base properties

Aqueous vanadate (V) compounds undergo various self-condensation reactions.3 Depending on pH, major vanadate anions in solution include VO2(H2O)2+4, VO3−4, V2O3−7, V3O3−9, V4O4−12, and V10O6−28. The anions often reversibly protonate.4 Decavanadate forms according to this equilibrium:23

H3V10O3−28 ⇌ H2V10O4−28 + H+
H2V10O4−28 ⇌ HV10O5−28 + H+
HV10O5−28(aq) ⇌ V10O6−28 + H+

The structure of the various protonation states of the decavanadate ion has been examined by 51V NMR spectroscopy.43 Each species gives three signals; with slightly varying chemical shifts around −425, −506, and −523 ppm relative to vanadium oxytrichloride; suggesting that rapid proton exchange occurs resulting in equally symmetric species.5 The three protonations of decavanadate have been shown to occur at the bridging oxygen centers, indicated as B and C in figure 1.5

Decavanadate is most stable in the pH 4–7 region.163 Solutions of vanadate turn bright orange at pH 6.5, indicating the presence of decavanadate. Other vanadates are colorless. Below pH 2.0, brown V2O5 precipitates as the hydrate.73

V10O6−28 + 6 H+ + 12 H2 ⇌ 5 V2O5

Structure

Figure 1: structure of decavanadate ion with equivalent V and O atoms indicated source ↗

The decavanadate ion consists of ten fused VO6 octahedra and has D2h symmetry.764 The structure of Na6[V10O28]·18H2O has been confirmed with X-ray crystallography.8

The decavanadate anions contains three sets of equivalent V atoms (see fig. 1).7 These include two central VO6 octahedra (Vc) and four each peripheral tetragonal-pyramidal VO5 groups (Va and Vb). There are seven unique groups of oxygen atoms (labeled A through G). Two of these (A) bridge to six V centers, four (B) bridge three V centers, fourteen of these (C, D and E) span edges between pairs of V centers, and eight (F and G) are peripheral.

The oxidation state of vanadium in decavanadate is +5.

Preparation

The preparation of decavanadate is achieved by acidifying an aqueous solution of orthovanadate (VO3−4:1

10 Na3[VO4] + 24 HOAc → Na6[V10O28] + 12 H2O + 24 NaOAc

The formation of decavanadate is optimized by maintaining a pH range of 4–7. Typical side products include metavanadate, VO−3, and hexavanadate, V6O2−16, ions.1

Potential uses

Decavanadate has been found to inhibit phosphoglycerate mutase, an enzyme which catalyzes step 8 of glycolysis. In addition, decavandate was found to have modest inhibition of Leishmania tarentolae viability, suggesting that decavandate may have a potential use as a topical inhibitor of protozoan parasites.9

Many decavanadate salts have been characterized. NH+4, Ca2+, Ba2+, Sr2+, and group I decavanadate salts are prepared by the acid–base reaction between V2O5 and the oxide, hydroxide, carbonate, or hydrogen carbonate of the desired positive ion.1

6 NH3 + 5 V2O5 + 3 H2O ⇌ (NH4)6[V10O28]

Other decavanadates:

(NH4)6[V10O28]·6H2O2
K6[V10O28]·9H2O2
K6[V10O28]·10H2O127
Ca3[V10O28]·16H2O27
K2Mg2[V10O28]·16H2O27
K2Zn2[V10O28]·16H2O127
Cs2Mg2[V10O28]·16H2O7
Cs4Na2[V10O28]·10H2O10
K4Na2[V10O28]·16H2O11
Sr3[V10O28]·22H2O10
Ba3[V10O28]·19H2O10
[(C6H5)4P]H3V10O28·4CH3CN5
Ag6[V10O28]·4H2O1213

Naturally occurring decavanadates include:

Ca3V10O28·17H2O (Pascoite)
Ca2Mg(V10O28)·16H2O (Magnesiopascoite)
Na4Mg(V10O28)·24H2O (Huemulite)
References

References

  1. Johnson, G.; Murmann, R. K. (1979). "Sodium and Ammonium Decayanadates(V)". Inorganic Syntheses. Vol. 19. pp. 140–145. doi:10.1002/9780470132500.ch32. ISBN 978-0-471-04542-7.
  2. Rossotti, F. J.; Rossotti, H. (1956). "Equilibrium Studies of Polyanions". Acta Chemica Scandinavica. 10: 957–984. doi:10.3891/acta.chem.scand.10-0957.
  3. Tracey, A.S.; Crans, D.C. (1998). Vanadium Compounds. Washington D.C.: American Chemical Society. ISBN 0-8412-3589-9.
  4. Rehder, D. (2008). Bioinorganic Vanadium Chemistry. Wiley & Sons. pp. 13–51. ISBN 978-0-470-06509-9.
  5. Day, V. W.; Klemperer, W. G.; Maltbie, D. J. (1987). "Where Are the Protons in H3V10O3−28?". Journal of the American Chemical Society. 109 (10): 2991–3002. doi:10.1021/ja00244a022. {{cite journal}}: templatestyles stripmarker in |title= at position 26 (help)
  6. Kustin, K.; Pessoa, J. C.; Crans, D. C. (2007). Vandadium: The Versatile Metal. Washington, D. C.: American Chemical Society. ISBN 978-0-8412-7446-4.
  7. Evans, H. T. Jr (1966). "The molecular structure of the isopoly complex ion, decavanadate". Inorg. Chem. 5: 967–977. doi:10.1021/ic50040a004.
  8. Durif, P.A.; Averbuch-Pouchot, M.T. (1980). "Structure d'un Décavanadate d'Hexasodium Hydraté". Acta Crystallogr. B. 36 (3): 680–682. Bibcode:1980AcCrB..36..680D. doi:10.1107/S0567740880004116.
  9. Turner, Timothy; Nguyen, Victoria; McLauchlan, Craig; Dymon, Zaneta; Dorsey, Benjamin; Hooker, Jaqueline; Jones, Marjorie (March 2012). "Inhibitory effects of decavanadate on several enzymes and Leishmania tarentolae In Vitro". Journal of Inorganic Biochemistry. 108: 96–104. doi:10.1016/j.jinorgbio.2011.09.009. PMID 22005446. Retrieved 23 January 2021.
  10. Dametto, A.C.; de Arauju, A.S.; de Souza Correa, R.; Guilherme, L.R.; Massabni, A.C. (2010). "Synthesis, infrared spectroscopy and crystal structure determination of a new decavanadate". J Chem Crystallogr. 40 (11): 897–901. Bibcode:2010JCCry..40..897G. doi:10.1007/s10870-010-9759-x. S2CID 97736357.
  11. Matias, P.M.; Pessoa, J.C.; Duarte, M.T.; Maderia, C. (2000). "Tetrapotassium disodium decavanadate(V) decahydrate". Acta Crystallogr. C. 57 (3): e75–e76. Bibcode:2000AcCrC..56E..75M. doi:10.1107/S0108270100001530. PMID 15263200.
  12. Escobar, M.E.; Baran, E.J. (1981). "Die Schwingungsspektren einiger kristalliner Dekavanadate". Monatshefte für Chemie. 112: 43–49. doi:10.1007/BF00906241. S2CID 101366009.
  13. Aureliano, Manuel; Crans, Debbie C. (2009). "Decavanadate (V10O6−28) and oxovanadates: Oxometalates with many biological activities". Journal of Inorganic Biochemistry. 103 (4): 536–546. doi:10.1016/j.jinorgbio.2008.11.010. ISSN 0162-0134. PMID 19110314. {{cite journal}}: templatestyles stripmarker in |title= at position 15 (help)