Difference between revisions of "Sodium peroxide"
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It reacts with [[carbon dioxide]] to produce oxygen and [[sodium carbonate]]. | It reacts with [[carbon dioxide]] to produce oxygen and [[sodium carbonate]]. | ||
| − | Attempts to calcine the octahydrate result in its decomposition, the crystals turn into sodium hydroxide. There is no easily available way to turn the octahydrate into the anhydrous salt. | + | Attempts to calcine the octahydrate result in its decomposition, the crystals turn into sodium hydroxide. There is no easily available way to turn the octahydrate into the anhydrous salt, but there were reports that putting it in a desiccator with very concentrated (98%) sulfuric acid for a long time does the trick. |
== Availability == | == Availability == | ||
Revision as of 17:27, 14 October 2015
Sodium peroxide is a sodium salt of hydrogen peroxide. Its formula is Na2O2. It is somewhat unstable and a strong oxidizer.
Contents
Properties
Physical
Sodium peroxide exists in two forms: anhydrous and octahydrate Na2O2*8H2O.
Anhydrous sodium peroxide is a yellow powder. The octahydrate appears as colorless crystals with a low melting point (30 Celsius).
Chemical
Anhydrous sodium peroxide reacts with water. Part of it is hydrolyzed irreversibly into oxygen, sodium hydroxide and water. Part is converted into the hydrate, which undergoes reversible hydrolysis and can be crystallized out of the solution by adding ethanol. The octahydrate is soluble in water without decomposition.
It reacts with carbon dioxide to produce oxygen and sodium carbonate.
Attempts to calcine the octahydrate result in its decomposition, the crystals turn into sodium hydroxide. There is no easily available way to turn the octahydrate into the anhydrous salt, but there were reports that putting it in a desiccator with very concentrated (98%) sulfuric acid for a long time does the trick.
Availability
Sodium peroxide, usually anhydrous, is commonly sold by various chemical suppliers.
Preparation
Anhydrous sodium peroxide is usually prepared by burning sodium metal in air. The octahydrate can be easily prepared by a simple neutralization reaction with hydrogen peroxide (a weak acid) and sodium hydroxide. The crystals can be displaced out of solution with ethanol.
Handling
Safety
Avoid contact of anhydrous hydrogen peroxide with organic solvents. This may result in fire or explosions.
Storage
Anhydrous sodium peroxide should be kept in a tightly closed jar, to avoid contact with water vapor. The octahydrate should be kept in a cold place.
Disposal
Any form of sodium peroxide can be neutralized by adding any acid and manganese dioxide. This reduces the component to a sodium salt of that acid and oxygen.
