Sodium molybdate

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title: "Sodium molybdate" type: doc version: 1 created: 2026-02-28 author: "Wikipedia contributors" status: active scope: public tags: ["molybdates", "sodium-compounds", "dietary-minerals", "inorganic-compounds", "corrosion-inhibitors"] topic_path: "general/molybdates" source: "https://en.wikipedia.org/wiki/Sodium_molybdate" license: "CC BY-SA 4.0" wikipedia_page_id: 0 wikipedia_revision_id: 0

| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 447916589 | ImageFile = Molybdenan sodný.JPG | ImageName = Sodium molybdate | ImageFile1 = Na2MoO4.svg | ImageFile2 = | IUPACName = Sodium molybdate | OtherNames = Disodium molybdate |Section1={{Chembox Identifiers | CASNo_Ref = | CASNo = 7631-95-0 | CASNo2_Ref = | CASNo2 = 10102-40-6 | CASNo2_Comment = (dihydrate) | UNII_Ref = | UNII = 948QAQ08I1 | UNII2 = 8F2SXI1704 | UNII2_Ref = | UNII2_Comment = (dihydrate) | ChemSpiderID_Ref = | ChemSpiderID = 55350 | PubChem = 61424 | ChEBI_Ref = | ChEBI = 75215 | EINECS = 231-551-7 | RTECS = QA5075000 | InChI = 1S/Mo.2Na.4O/q;2*+1;;;2*-1 | SMILES = [O-] Mo(=O)[O-].[Na+].[Na+] |Section2={{Chembox Properties | Formula = Na2MoO4 | MolarMass = 205.92 g/mol (anhydrous) 241.95 g/mol (dihydrate) | Appearance = White powder | Density = 3.78 g/cm3, solid | Solubility = 84 g/100 ml (100 °C) | MeltingPtC = 687 | BoilingPt = | RefractIndex = 1.714 |Section7={{Chembox Hazards | ExternalSDS = External MSDS | GHS_ref = | GHSPictograms = | GHSSignalWord = Warning | HPhrases = | PPhrases = | MainHazards = | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = | FlashPt = Non-flammable | LC50 = 2080 mg/m3 (rat, 4 hr) | LD50 = 4000 mg/kg (rat, oral) |Section8={{Chembox Related | OtherAnions = Sodium chromate Sodium tungstate | OtherCations = Ammonium molybdate Sodium molybdate, Na2MoO4, is useful as a source of molybdenum. This white, crystalline salt is often encountered as the dihydrate, Na2MoO4·2H2O.

Structure

thumb|left|structure of solid sodiium molybdate dihydrate. In aqueous solution, sodium molybdate features dissociated sodium ions and tetrahedral molybdate (), which adopts a sulfate-like structure. The solid dihydrate material has a complex structure typical for alkali metal salts of oxyanions. The subunits are tetrahedral with Mo-O distances near 178 pm.

Preparation

Dissolution of MoO3 in sodium hydroxide at 50–70 °C followed by crystallizing the filtered product. If crystallized below 10 °C, the decahydrate forms. Above 10 °C, the dihydate crystallizes. The anhydrous salt is obtained by heating this product at 100 °C. :MoO3 + 2NaOH + H2O - Na2MoO4*2H2O

Uses

The agriculture industry uses 500 tons per year as a fertilizer. In particular, its use has been suggested for treatment of whiptail in broccoli and cauliflower in molybdenum-deficient soils. However, care must be taken because at a level of 0.3 ppm sodium molybdate can cause copper deficiencies in animals, particularly cattle.

It is used in industry for corrosion inhibition, as it is a non-oxidizing anodic inhibitor. In industrial water treatment applications where galvanic corrosion is a potential due to bimetallic construction, the application of sodium molybdate is preferred over sodium nitrite. Sodium molybdate has the advantage in that the dosing of lower ppm's of molybdate allow for lower conductivity of the circulating water. Sodium molybdate at levels of 50-100 ppm offer the same levels of corrosion inhibition as sodium nitrite at levels of 800+ ppm. By utilizing lower concentrations of sodium molybdate, conductivity is kept at a minimum and thus galvanic corrosion potentials are decreased.

Reactions

When treated with sodium borohydride, molybdate is reduced to molybdenum(IV) oxide: :Na2MoO4 + NaBH4 + 2H2O - NaBO2 + MoO2 + 2NaOH + 3H2

Sodium molybdate reacts with the acids of dithiophosphates: :Na2MoO4 + (RO)2PS2H - [MoO2(S2P(OR)2)2] with R = Me, Et

which further reacts to form [MoO3(S2P(OR)2)4].

Safety

Sodium molybdate supports the biosynthesis of molybdoenzymes, which are found in all higher forms of life. The LC50 for freshwater fish ranges from 60 to 7630 mg/L. The toxicity of soluble molybdate to marine organisms has also been reported.

References

References

  1. PubChem. "Sodium Molybdate".
  2. {{IDLH. moly-mo. Molybdenum (soluble compounds, as Mo)
  3. {{Greenwood&Earnshaw1st
  4. Braithwaite, E.R.; Haber, J. ''Molybdenum: An outline of its Chemistry and Uses.'' 1994. Elsevier Science B.V. Amsterdam, the Netherlands.
  5. (1975). "The Crystal Structure of Sodium Molybdate Dihydrate, Na2MoO4·2H2O". Bulletin of the Chemical Society of Japan.
  6. Spitsyn, Vikt. I.; Kuleshov, I. M. ''Zhurnal Obshchei Khimii'' 1951. 21. 1701-15.
  7. Plant, W.. (1950). "Use of Lime and Sodium Molybdate for the Control of 'Whiptail' in Broccoli". Nature.
  8. Davies, E. B.. (1945). "A Case of Molybdenum Deficiency in New Zealand". Nature.
  9. The addition of sodium molybdate significantly reduces the nitrite requirement of fluids inhibited with nitrite-amine, and improves the corrosion protection of carboxylate salt fluids.Vukasovich, Mark S. ''Lubrication Engineering'' 1980. 36(12). 708-12.
  10. M. Houser, Corrosion Control Services, Inc., Introduction Handbook
  11. (1997). "Synthesis of lower-valent molybdenum oxides in aqueous solutions by reducing Na2MoO4 with NaBH4". Journal of Materials Chemistry.
  12. (23 April 2014). "Linus Pauling Institute page on molybdenum".
  13. (2012). "The chronic toxicity of molybdate to marine organisms. I. Generating reliable effects data". Science of the Total Environment.

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molybdatessodium-compoundsdietary-mineralsinorganic-compoundscorrosion-inhibitors