Permanganic acid

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Permanganic acid
Permanganic acid
Names
IUPAC name
Permanganic acid
Other names
Manganic(VII) acid
Hydroxy(trioxo)manganese
Hydrogen permanganate
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.033.346 Edit this at Wikidata
EC Number
  • 236-695-4
  • InChI=1S/Mn.H2O.3O/h;1H2;;;/q+1;;;;/p-1
    Key: ZJBYBXHCMWGGRR-UHFFFAOYSA-M
  • O=[Mn](=O)(=O)O
Properties
HMnO4
Molar mass 119.94 g mol−1
Appearance Violet
Acidity (pKa) about -4.6 to -2.3 [1][2]
Conjugate base
 Permanganate
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Oxidant, Corrosive
Related compounds
Other cations
 Potassium permanganate
Sodium permanganate
Calcium permanganate
Related compounds
 Pertechnetic acid
Perrhenic acid
Perchloric acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Permanganic acid (or manganic(VII) acid) is the

conjugate acid of permanganate
salts. It is the subject of few publications and its characterization as well as its uses are very limited.

Preparation and structure

Permanganic acid is most often prepared by the reaction of dilute sulfuric acid with a solution of barium permanganate, the insoluble barium sulfate byproduct being removed by filtering:[3]

Ba(MnO4)2 + H2SO4 → 2 HMnO4 + BaSO4↓

The sulfuric acid used must be dilute; reactions of permanganates with concentrated sulfuric acid yield the

anhydride, manganese heptoxide
.

Permanganic acid has also been prepared through the reaction of

hydrofluorosilicic acid with potassium permanganate,[4] through electrolysis, and through hydrolysis of manganese heptoxide, though the last route often results in explosions.[5]

Crystalline permanganic acid has been prepared at low temperatures as the dihydrate, HMnO4·2H2O.[3]

Although its structure has not been verified spectroscopically or crystallographically, HMnO4 is assumed to be adopt a tetrahedral structure akin to that for perchloric acid.

Reactions

As a strong acid, HMnO4 is deprotonated to form the intensely purple coloured permanganates. Potassium permanganate, KMnO4, is a widely used, versatile and powerful oxidising agent.

Permanganic acid solutions are unstable, and gradually decompose into manganese dioxide, oxygen, and water, with initially formed manganese dioxide catalyzing further decomposition.[6] Decomposition is accelerated by heat, light, and acids. Concentrated solutions decompose more rapidly than dilute.[6]

References

  1. doi:10.1139/v63-164
    .
  2. doi:10.1039/JR9600000290
    .
  3. ^
    PMID 5823192
    .
  4. ^ Black, Homer Van Valkenburg (1900). The permanganates of barium, strontium, and calcium. Easton, PA. p. 6.{{cite book}}: CS1 maint: location missing publisher (link)
  5. ^ Olsen, J. C. (1900). Permanganic Acid by Electrolysys. Easton, PA: The Chemical Publishing Company.
  6. ^ a b Byers, Horace Greeley (1899). A Study of the Reduction of Permanganic acid by Manganese Dioxide. Chemical Publishing Company.
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