Sodium molybdate

From Wikipedia, the free encyclopedia

Sodium molybdate
Sodium molybdate
IUPAC name Sodium molybdate(VI)
Other names Disodium molybdate.
Identifiers
CAS number [7631-95-0]
Properties
Molecular formula Na2MoO4
Molar mass Anhydrous 206 g/mol

Dihydrate 241.95 g/mol

Appearance White powder.
Density 3.78 g/cm3, solid
Melting point

687°C

Solubility in water 65.5 g/100 g Water
Hazards
MSDS External MSDS
EU classification Irritant (I)
R-phrases R36, R37, R38.
S-phrases None listed.
Flash point Non-flammable.
Related compounds
Other anions None listed.
Other cations None listed.
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Sodium molybdate, Na2MoO4, is useful as a source of molybdenum.[citation needed] It is often found as the dihydrate, Na2MoO4·2H2O.

The molybdate(VI) anion is tetrahedral. Two sodium cations coordinate with every one anion.[1]

Contents

[edit] History

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

MoO3 + 2NaOH → Na2MoO4·2H2O

[edit] 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.[1]

It is used for water treatment.[citation needed]

It is used in industry for corrosion inhibition, as it is a non-oxidizing anodic inhibitor.[1] 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’.[citation needed]

[edit] Reactions

When reacted with sodium borohydride, molybdenum is reduced to a lower valent oxide:[4]

Na2MoO4 + NaBH4 + 2H2O→ NaBO2 + MoO2+2NaOH+ 3 H2

Sodium molybdate reacts with the acids of dithiophosphates:[1]

Na2MoO4 + (RO)2PS2H (R = Me, Et) → [MoO2(S2P(OR)2)2]

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

[edit] 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.[citation needed]

[edit] References

  1. ^ a b c d e Braithwaite, E.R.; Haber, J. Molybdenum: An outline of its Chemistry and Uses. 1994. Elsevier Science B.V. Amsterdam, The Netherlands.
  2. ^ Spitsyn, Vikt. I.; Kuleshov, I. M. Zhurnal Obshchei Khimii 1951. 21. 1701-15.
  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.

[edit] See also

[edit] External links

Languages