Sodium manganate: Difference between revisions
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'''Sodium manganate''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[Sodium|Na]]<sub>2</sub>[[Manganese|Mn]][[Oxygen|O]]<sub>4</sub>. This |
'''Sodium manganate''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[Sodium|Na]]<sub>2</sub>[[Manganese|Mn]][[Oxygen|O]]<sub>4</sub>. This deep green solid is a rarely encountered analogue of the related salt [[Potassium manganate|K<sub>2</sub>MnO<sub>4</sub>]]. Sodium manganate is rarely encountered because it cannot be readily prepared from the oxidation of manganese dioxide and sodium hydroxide. Instead this oxidation stops at the level of Na<sub>3</sub>MnO<sub>4</sub>, and this Mn(V) salt is unstable in solution.<ref>Arno H. Reidies, “Manganese Compounds” in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. {{DOI|10.1002/14356007.a16_123}}</ref> Sodium manganate can be produced by [[Redox|reduction]] of sodium permanganate under basic conditions: |
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:4 NaOH + 4NaMnO<sub>4</sub> → 4 Na<sub>2</sub>MnO<sub>4</sub> + 2 H<sub>2</sub>O + O<sub>2</sub> |
:4 NaOH + 4NaMnO<sub>4</sub> → 4 Na<sub>2</sub>MnO<sub>4</sub> + 2 H<sub>2</sub>O + O<sub>2</sub> |
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Because Na<sub>3</sub>MnO<sub>4</sub> is difficult to prepare, [[sodium permanganate]] is more expensive than [[potassium permanganate]]. |
Because Na<sub>3</sub>MnO<sub>4</sub> is difficult to prepare, [[sodium permanganate]] is more expensive than [[potassium permanganate]]. |
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Revision as of 18:29, 10 July 2014
| Identifiers | |
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CompTox Dashboard (EPA)
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| Properties | |
| MnNa2O4 | |
| Molar mass | 164.914 g·mol−1 |
| Appearance | deep green solid |
| Related compounds | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium manganate is the inorganic compound with the formula Na2MnO4. This deep green solid is a rarely encountered analogue of the related salt K2MnO4. Sodium manganate is rarely encountered because it cannot be readily prepared from the oxidation of manganese dioxide and sodium hydroxide. Instead this oxidation stops at the level of Na3MnO4, and this Mn(V) salt is unstable in solution.[1] Sodium manganate can be produced by reduction of sodium permanganate under basic conditions:
- 4 NaOH + 4NaMnO4 → 4 Na2MnO4 + 2 H2O + O2
Because Na3MnO4 is difficult to prepare, sodium permanganate is more expensive than potassium permanganate.
References
- ^ Arno H. Reidies, “Manganese Compounds” in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
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