Sodium molybdate

Sodium molybdate, Na₂MoO₄, is useful as a source of molybdenum.

It is often found as the dihydrate, Na₂MoO₄ . 2H₂O.

The structure of the Molybdate (IV) anion is tetrahedral. Two sodium cations coordinate with every one anion.^[2]

Additional recommended knowledge

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History

Sodium Molybdate was first synthesized by the method of hydration^[1]; however, a more convenient synthesis is done by dissolving MoO₃ in sodium hydroxide at 50-70 ºC and crystallizing the filtered product.^[2] The anhydrous salt is prepared by heating to 100 ºC.

MoO₃ + 2NaOH → Na₂MoO₄ ∙ 2H₂O

Uses

Sodium molybdate is used in biochemistry and medicinal chemistry to track various organic chemicals that are colorless after a chromatographical procedure, which it always stains blue. The blue color is also called molybdenum blue.

The agriculture industry uses 1 million pounds per year as a fertilizer. However, care must be taken because at a level of 0.3 ppm sodium molybdate can cause copper deficiencies in animals, particularly cattle.^[2]

It is used for water treatment.

It is used in industry for corrosion inhibition, as it is a non-oxidizing anodic inhibitor.^[2] 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.^[3]

According to an article from 1950 that was published in Nature, sodium molybdate is useful for curing a broccoli disease known as ‘whiptail’.

Reactions

When reacted with sodium borohydride, molybdenum is reduced to a lower valent oxide:

Na₂MoO₄ + NaBH₄ + 2H₂O→ NaBO₂ + MoO₂+2NaOH+ 3 H₂ ^[4]

Sodium molybdate reacts with the acids of dithiophosphates:

Na₂MoO₄ + (RO)₂PS₂H (R = Me, Et) → [MoO₂(S₂P(OR)₂)₂] which further reacts to form [MoO₃(S₂P(OR)₂)₄].^[2]

Precautions

Sodium Molybdate is incompatible with alkali metals, most common metals and oxidizing agents. It will explode on contact with molten magnesium. It will violently react with interhalogens (e.g., bromine pentafluoride; chlorine trifluoride). Its reaction with hot sodium, potassium or lithium is incandescent. (From the MSDS)

References

1. Spitsyn, Vikt. I.; Kuleshov, I. M. Zhurnal Obshchei Khimii 1951. 21. 1701-15.

2. Braithwaite, E.R.; Haber, J. Molybdenum: An outline of its Chemistry and Uses. 1994. Elsevier Science B.V. Amsterdam, The Netherlands.

3. Vukasovich, Mark S. Lubrication Engineering 1980. 36(12). 708-12.

4. Chi Fo Tsang and Arumugam Manthiram. Journal of Materials Chemistry 1997. 7(6). 1003–1006.

See also

• xanthine oxidase