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Sodium permanganate is the inorganic compound with the formula NaMnO4. It is closely related to the more commonly encountered potassium permanganate, but it is generally less desirable, because it is more expensive to produce. It is mainly available as the monohydrate. This salt absorbs water from the atmosphere and has a low melting point. Being about 15 times more soluble than KMnO4, sodium permanganate finds some applications where very high concentrations of MnO4 are sought.

Sodium permanganate
Sodium permanganate.png
Sodium permanganate solution.JPG
IUPAC name
Sodium manganate(VII)
Other names
Sodium permanganate, permanganate of sodium
3D model (JSmol)
ECHA InfoCard 100.030.215
RTECS number SD6650000
Molar mass 141.9254 g/mol
159.94 g/mol (monohydrate)
Appearance Red solid
Density 1.972 g/cm3 (monohydrate)
Melting point 36 °C (97 °F; 309 K) (170 °C for trihydrate)
90 g/100 mL
Main hazards Oxidizer
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Preparation and propertiesEdit

Sodium permanganate cannot be prepared analogously to the route to KMnO4 because the required intermediate manganate salt, Na2MnO4, does not form. Thus less direct routes are used including conversion from KMnO4.[1]

Sodium permanganate behaves similarly to potassium permanganate. It dissolves readily in water to give deep purple solutions, evaporation of which gives prismatic purple-black glistening crystals of the monohydrate NaMnO4·H2O. The potassium salt does not form a hydrate. Because of its hygroscopic nature, it is less useful in analytical chemistry than its potassium counterpart.

It can be prepared by the reaction of manganese dioxide with sodium hypochlorite:

2 MnO2 + 3 NaOCl + 2 NaOH → 2 NaMnO4 + 3 NaCl + H2O


Because of its high solubility, its aqueous solutions are used as etchants in printed circuitry.[1] It is gaining popularity in water treatment for taste, odor, and zebra mussel control.[2]


  1. ^ a b Arno H. Reidies "Manganese Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
  2. ^