Potassium selenate

Potassium selenate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.029.286 Edit this at Wikidata
EC Number
  • 232-214-7
RTECS number
  • VS6600000
UNII
  • InChI=1S/2K.H2O4Se/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
    Key: YAZJAPBTUDGMKO-UHFFFAOYSA-L
  • [K+].[K+].[O-][Se]([O-])(=O)=O
Properties
K
2SeO
4
Molar mass 221.2 g/mol[1]
Appearance colorless crystals
hygroscopic
Odor odorless
Density 3.07 g/cm3[2]
1.07 g/ml (0 °C)
1.11 g/ml (20 °C)
1.22 g/ml (100 °C)
1.539
Structure
orthorhombic
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
1
0
Related compounds
Other anions
 Potassium sulfate
Other cations
 Sodium selenate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Potassium selenate, K
2SeO
4, is an odorless, white solid that forms as the potassium salt of selenic acid.

Preparation

Potassium selenate is produced by the reaction of selenium trioxide and potassium hydroxide.

SeO3 + 2 KOH → K2SeO4 + H2O

Alternatively, it can be made by treating selenous acid with potassium hydroxide, followed by oxidation of the resulting potassium selenite with bromine water.[3]

H2SeO3 + 2 KOH → K2SeO3 + 2 H2O
K2SeO3 + 2 KOH + Br2 → K2SeO4 + 2 KBr + H2O

Uses

Potassium selenate can be used to produce selenium trioxide.[4] It can also use to treat selenium deficiency in livestock.[5]

References

  1. ^ "Potassium Selenate K2SeO4 Molecular Weight". EndMemo. Retrieved 2019-09-03.
  2. ^ "Potassium Selenate". American Elements. Retrieved 2019-09-03.
  3. ^ Rosenfeld, Irene; Beath, Orville A. (2013). Selenium: Geobotany, Biochemistry, Toxicity, and Nutrition. Elsevier Science. p. 305. ISBN 978-1-4832-7590-1.
  4. ^ Sicius, Hermann (2015). Chalkogene : elemente der sechsten hauptgruppe (in German). Springer. p. 28. ISBN 978-3-658-10522-8. OCLC 919684689.
  5. ^ Wolfgang Löscher, Angelika Richter, Heidrun Potschka (2014). Pharmakotherapie bei Haus- und Nutztieren (in German). Stuttgart: Enke. ISBN 978-3-8304-1250-2. OCLC 891036290.{{cite book}}: CS1 maint: multiple names: authors list (link)