Selenic acid

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Selenic acid
Structural formula of selenic acid
Structural formula of selenic acid
Space-filling model of selenic acid
Space-filling model of selenic acid
Names
IUPAC name
Selenic(VI) acid
Other names
Selenic acid
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.029.072 Edit this at Wikidata
EC Number
  • 231-979-4
KEGG
RTECS number
  • VS6575000
UNII
UN number 1905
  • InChI=1S/H2O4Se/c1-5(2,3)4/h(H2,1,2,3,4) checkY
    Key: QYHFIVBSNOWOCQ-UHFFFAOYSA-N checkY
  • InChI=1/H2O4Se/c1-5(2,3)4/h(H2,1,2,3,4)
    Key: QYHFIVBSNOWOCQ-UHFFFAOYAI
  • O[Se+2]([O-])([O-])O
Properties
H2SeO4
Molar mass 144.9734 g/mol
Appearance Colorless deliquescent crystals
Density 2.95 g/cm3, solid
Melting point 58 °C (136 °F; 331 K)
Boiling point 260 °C (500 °F; 533 K) (decomposes)
130 g/(100 mL) (30 °C)
Acidity (pKa) pKa1 = −3
pKa2 = 1.9[1]
Conjugate base
 Biselenate
−51.2·10−6 cm3/mol
1.5174 (D-line, 20 °C)
Structure
tetrahedral at Se
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Corrosive, highly toxic
GHS labelling:[2]
GHS05: CorrosiveGHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Danger
H301, H315, H318, H331, H373, H410
P260, P261, P264, P270, P271, P273, P280, P301+P310, P302+P352, P304+P340, P305+P351+P338, P310, P311, P314, P321, P330, P332+P313, P362, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
2
OX
Related compounds
Other anions
selenious acid
hydrogen selenide
Other cations
 sodium selenate
potassium selenate
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Selenic acid is the

oxoacid of selenium, and its structure is more accurately described as O2Se(OH)2. It is a colorless compound. Although it has few uses, one of its salts, sodium selenate is used in the production of glass and animal feeds.[3]

Structure and bonding

The molecule is tetrahedral, as predicted by VSEPR theory. The Se–O bond length is 161 pm.[4] In the solid state, it crystallizes in an orthorhombic structure.[5]

Preparation

It is prepared by oxidising selenium compounds in lower oxidation states. One method involves the oxidation of selenium dioxide with hydrogen peroxide:

SeO2 + H2O2 → H2SeO4

Unlike the production sulfuric acid by hydration of sulfur trioxide, the hydration of selenium trioxide is an impractical method.[4] Instead, selenic acid may also be prepared by the oxidation of selenous acid (H2SeO3) with halogens, such as chlorine or bromine, or with potassium permanganate.[6] Using chlorine or bromine as the oxidising agents also produces hydrochloric or hydrobromic acid as a side-product, which needs to be removed from the solution since they can reduce the selenic acid to selenous acid.[7]

To obtain the anhydrous acid as a crystalline solid, the resulting solution is evaporated at temperatures below 140 °C (413 K; 284 °F) in a vacuum.[8]

Reactions

Like

hygroscopic and extremely soluble in water. Concentrated solutions are viscous. Crystalline mono- and di-hydrates are known.[6] The monohydrate melts at 26 °C, and the dihydrate melts at −51.7 °C.[4]

Selenic acid is a stronger

chloride ions, being reduced to selenous acid
in the process:

H2SeO4 + 2 H+ + 2 Cl− → H2SeO3 + H2O + Cl2

It decomposes above 200 °C, liberating oxygen gas and being reduced to selenous acid:[6]

2 H2SeO4 → 2 H2SeO3 + O2

Selenic acid reacts with barium salts to precipitate solid BaSeO4, analogous to the sulfate. In general, selenate salts resemble sulfate salts, but are more soluble. Many selenate salts have the same crystal structure as the corresponding sulfate salts.[4]

Treatment with fluorosulfuric acid gives selenoyl fluoride:[8]

H2SeO4 + 2 HSO3F → SeO2F2 + 2 H2SO4

Hot, concentrated selenic acid reacts with gold, forming a reddish-yellow solution of gold(III) selenate:[10]

2 Au + 6 H2SeO4 → Au2(SeO4)3 + 3 H2SeO3 + 3 H2O

Applications

Selenic acid is used as a specialized oxidizing agent.

References

  1. ISBN 9781439826232
    .
  2. ^ "Selenic acid". pubchem.ncbi.nlm.nih.gov. Retrieved 16 December 2021.
  3. doi:10.1002/14356007.a23_525
    .
  4. ^
    ISBN 978-1-4067-7302-6
    .
  5. ISBN 978-0-85404-366-8
    .
  6. ^
    ISBN 81-224-1384-6
    .
  7. doi:10.1021/ja01683a005
    .
  8. ^
    ISBN 0-471-07715-1
    . The report describes the synthesis of selenic acid.
  9. ISBN 978-0-08-037941-8
    .
  10. doi:10.1021/ja02018a005
    .
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