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Potassium manganate
Image:Potassium manganate.jpg
General
Systematic name	Potassium manganate
Molecular formula	K2MnO4
Molar mass	197.13 g/mol
Appearance	dark green crystals
CAS number	[10294-64-1]
Properties
Density and phase	2.78 g/cm3, solid
Solubility in water	highly soluble
Melting point	190 °C
Acidity (pKa)	7.1
Structure
Coordination geometry	tetrahedral anion
Crystal structure	isomorphous with K2SO4
Hazards
MSDS	External MSDS
Main hazards	oxidizer
NFPA 704
R/S statement	R: 8-36/37/38 S: 17-26-36/37/39
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid
Spectral data	UV λmax (ε) = 610 nm (1500 M-1cm-1) IR νMn-O = 830 cm1-
Related compounds
Related compounds	KMnO4 MnO2 K2CrO4 K2FeO4
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references

Potassium manganate is the chemical compound with the formula K₂MnO₄. This green salt is an intermediate in the industrial synthesis of potassium permanganate, a common chemical.

Contents 1 Structure 2 Synthesis 3 Reactions 4 Literature cited 5 Other references 6 External links

K₂MnO₄ is a salt, consisting of K⁺ cations and MnO₄^2- anions. X-ray crystallography shows that the anion is tetrahedral, with Mn-O distances of 1.66 Å, ca. 0.03 Å longer than the Mn-O distances in KMnO₄.^[1]

The industrial route entails treatment of MnO₂ with air:

MnO₂ + 2 KOH + ½ O₂ → K₂MnO₄ + H₂O

The transformation gives a green-colored melt. In fact, one can test an unknown substance for the presence of Mn by heating the sample in strong KOH in air. The production of a green coloration indicates the presence of Mn. This green color is intense, with an extinction coefficient of 1500 M^-1cm^-1 at 610 nm.

In laboratory, K₂MnO₄ can be synthesized by heating a solution of KMnO₄ in concentrated KOH solution followed by cooling to give green crystals:^[1]

4 KMnO₄ + 4 KOH → 4 K₂MnO₄ + O₂ + 2 H₂O

This reaction illustrates the relatively rare role of hydroxide as a reducing agent. Solutions of K₂MnO₄ are generated by allowing a solution of KMnO₄ in 5-10 M KOH to stir for a day at room temperature followed by removal of MnO₂, which is insoluble. The concentration of K₂MnO₄ in such solutions can be checked by measuring their absorbance at 610 nm.

The one-electron reduction of permanganate to manganate can also be effected using iodide as the reducing agent:

KMnO₄ + KI → K₂MnO₄ + ½ I₂

The conversion is signaled by the color change from purple, characteristic of permanganate, to the green color of manganate. This reaction also illustates the fact that permanganate can serve as an electron acceptor in addition to its usual role as an oxygen-transfer reagent. Barium manganate, BaMnO₄, is generated by the reduction of KMnO₄ with iodide in the presence of barium chloride. Just like BaSO₄, BaMnO₄ exhibits low solubility in virtually all solvents.

At lower pH's, the manganate ion will disproportionate to permanganate ion and manganese dioxide:

3 K₂MnO₄ + 2 H₂O → 2 KMnO₄ + MnO₂ + 4 KOH

The colorful nature of this reaction has led the manganate/permanganate pair to be referred to as a "chemical chameleon." This disproportionation reaction, which becomes rapid when [OH^-] < 1M, follows bimolecular kinetics.^[2] see also Manganate

1. ^ Nyholm R.S. Woolliams P.R. (1986). ""Manganates(VI)"". Inorganic Syntheses XI: 56–61. 

• Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.

See category for a list.

• National Pollutant Inventory - Manganese and compounds Fact Sheet

• Links to external chemical sources