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This article resulted from my subdividing Manganate so that we had a real data table on a real compound vs just an anion. So the writing might be a little redundant between the two reports - feel free to revise and parse as you see fit. -- Smokefoot 02:41, 20 May 2006 (UTC) reply

I removed the bold sentence below (my boldening):

In the 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 bold comment does not make sense given the equation above. Perhaps it was meant for the "opposite" reaction, the disproportionation of K₂MnO₄ into KMnO₄ + MnO₂? -- Jorge Stolfi ( talk) 19:50, 3 June 2019 (UTC) reply