Sodium selenate
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| Names | |
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| IUPAC name
Sodium selenate
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| DrugBank | |
| ECHA InfoCard | 100.033.169 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII |
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| UN number | 2630 |
CompTox Dashboard (EPA)
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| Properties | |
| Na2O4Se | |
| Molar mass | 188.947 g·mol−1 |
| Appearance | White or grey powder |
| Density | 3.098 g/cm3 |
| soluble | |
| Pharmacology | |
| A12CE01 (WHO) | |
| Hazards | |
| GHS labelling: | |
  
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| Danger | |
| H301, H331, H373, H410 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Sodium sulfate |
Other cations
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Potassium selenate |
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 selenate is the inorganic compound with the formula Na
2SeO
4, not to be confused with sodium selenite. It exists as the anhydrous salt, the heptahydrate, and the decahydrate.[1] These are white, water-soluble solids. The decahydrate is a common ingredient in multivitamins and livestock feed as a source of selenium. The anhydrous salt is used in the production of some glass. Although the selenates are much more toxic, many physical properties of sodium selenate and sodium sulfate are similar.[2]
Production
Sodium selenate is produced by oxidation of selenium, first with nitric acid, producing selenous acid. The selenous acid is neutralized to form sodium selenite. The sodium selenite is oxidized in a basic medium hydrogen peroxide to form a selenate, which is then spray-dried.[3]
- Se + 2HNO3 → H2SeO3 + NO + NO2
- H2SeO3 + Na2CO3 → Na2SeO3 + H2O + CO2
- Na2SeO3 + H2O2 → Na2SeO4 + H2O.
It was prepared shortly after the discovery of selenium by Jöns Jacob Berzelius in 1817.
Industrial uses
Glass manufacturing
One of the earliest applications of sodium selenate was in the glass industry. Selenium produces a red hue in glass. The molten glass is treated with sodium selenate and then arsenic trioxide to reduce the compound and provide elemental selenium. Sodium selenate is also used as a decolorizing agent in glass production. The red hue it gives glass is complementary to the green hue given by ferrous oxides in the manufacturing process. When used together, the two compound produce a colourless glass.[4]
Pesticide
Sodium selenate is a common ingredient in some insecticides used against mites, aphids, and mealybugs. For most insects, a dose of 10 mg/kg is enough to be fatal.[5][6] It is also used in some fungicides.
Bio-fortification of crops
Sodium selenate is effectively used for bio-fortification of crops hence fortifying food/feed to mitigate selenium deficiency in humans and livestock. It can be applied as foliar spray or via rooting medium e.g. added in fertilizers.
Dietary supplement
Chosen for its selenium content and high solubility, sodium selenate is a common ingredient in over-the-counter vitamin supplements. Selenium is a trace essential element. Sodium selenate and selenite are also common in premix animal feed. Neither compound has demonstrated a difference in the amount of selenium absorbed. The US FDA regulates that animal feed contain no more than 5 ppm selenium content.[7] Controversy arose in 2009 when a group of 21 polo horses died from selenium poisoning from an incorrectly mixed dietary supplement.[8]
Toxicology
The US FDA and European Union currently classify sodium selenate as toxic, primarily if ingested or inhaled. Testing on rats showed a dose of 1.6 mg/kg to be lethal. A low lethal dose as this places the chemical as being 2 to 3 times more toxic than sodium cyanide. As such, it is extremely toxic and must be handled with care. For a 70 kilograms (150 lb) person, this dosage corresponds to 112 mg, or, in terms of 200 µg pills, 560 pills. Chronic exposure to sodium selenate can cause severe lung, kidney, and liver damage.[9]
Overexposure to selenium in the diet leads to a condition known as selenosis. Selenosis occurs at blood levels greater than 100 µg/dL. Symptoms include gastrointestinal upsets, hair loss, white blotchy nails, garlic breath odour, fatigue, irritability, and mild nerve damage.[10]
References
- ^ Kamburov, S.; Schmidt, H.; Voigt, W.; Balarew, C. (2014). "Similarities and peculiarities between the crystal structures of the hydrates of sodium sulfate and selenate". Acta Crystallographica Section B: Structural Science, Crystal Engineering and Materials. 70 (4): 714–22. doi:10.1107/S2052520614007653. PMID 25080250.
- ^ Langner, Bernd E. (2005). "Selenium and Selenium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Wiley. doi:10.1002/14356007.a23_525. ISBN 3527306730.
- ^ US patent 4605544, Björnberg, Arne; Martensson, Ulf S. & Paulsson, Karin M., "Method for producing selenium salts", issued 1986-08-12
- ^ Whitaker, Milton C. (1912-07-01). "Selenium Glass". Journal of Industrial and Engineering Chemistry. 7 (4): 539–540. doi:10.1021/ie50043a031.
- ^ Krieger, K. (2001). Handbook of Pesticide Toxicology. Vol. 1. San Diego, California: Academic Press.
- ^ Hanson, Brady; Lindblom, Stormy Dawn; Loeffler, Miriam L.; Pilon-Smits, Elizabeth A. H. (2004-04-05). "Selenium protects plants from phloem-feeding aphids due to both deterrence and toxicity". New Phytologist. 162 (3): 655–662. doi:10.1111/j.1469-8137.2004.01067.x. PMID 33873760.
- ^ Podoll, K. L.; Bernard, J. B.; Ullrey, D. E.; DeBar, S. R.; Ku, P. K.; Magee, W. T. (1992-06-01). "Dietary selenate versus selenite for cattle, sheep, and horses". Journal of Animal Science. 70 (6): 1965–1970. doi:10.2527/1992.7061965x. PMID 1321804.
- ^ "Officials blame mineral for horse deaths". Fort Worth Star-Telegram. Vol. 104, no. 4. 2009-04-29. p. A7.
- ^ Ganther, H. E.; Baumann, C.A. (1962-08-01). "Selenium Metabolism: II. Modifying Effects of Sulfate". The Journal of Nutrition. 77 (4): 408–414. doi:10.1093/jn/77.4.408. PMID 13896696.
- ^ "Selenium: Fact Sheet for Health Professionals". National Institutes of Health. 2021-03-26. Archived from the original on 2022-06-21. Retrieved 2022-06-21.
