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Aluminum oxide is an amphoteric metal oxide with both basic and acidic properties. When a weak acid solution is added, aluminum oxide is selectively precipitated. It is also used as a coagulant in flocculation.
Aluminum oxide is not flammable and does not react with water. This allows it to be safely disposed of in normal trash. However, its acidity causes irritation of the eyes and upper respiratory tract. To avoid these effects, aluminium oxide should not be inhaled. Instead, it should be stored in a closed bottle.
The chemical reaction between aluminum and sodium hydroxide is fairly straightforward. In the presence of an alkali, the solution reacts to produce sodium tetrahydroxoaluminate. A more concentrated form of the compound is produced in the presence of a stronger base.
To prepare the reaction, the aluminum is dissolved in a diluted aqueous NaOH solution. The resulting solution is cooled to a solid mass. As the mixture is heated, carbon dioxide is bubbled through the solution.
At a temperature of 900-1100degC, the reaction takes place. As the reaction progresses, the aluminum samples become darker. Eventually, the final product is a white crystalline material known as sodium aluminate. Sodium aluminate is used in the production of fire bricks, paper and concrete.
The concentration of the reaction is affected by the concentration of the alkali and the temperature. Aluminum is more susceptible to the reaction when the concentration is low, while at higher concentrations, the reaction proceeds more slowly.
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