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Aluminium oxide reacts with hydrochloric acid to form aqueous aluminium chloride solution and hydrogen gas. This reaction is a type of redox reaction. Aluminium loses electrons to the protons of the acid to become an aluminium ion, and hydrogen gains electrons to become hydrogen gas.
The chemical properties of aluminium oxide are not well defined. It is an inorganic metal oxide and is known by the chemical symbol Al2O3. It has a wide range of uses as a raw material and industrial catalyst. It is also an important refractory material. The crystalline form is called corundum and is used to make abrasives and cutting tools. It is also used as a filter in water purification and to manufacture aluminium foil. The oxide is a very hard substance and is not soluble in water, but is soluble in dilute acids like hydrochloric acid.
When you place a piece of aluminium in an acid solution it doesn’t immediately react because it has a layer of aluminium oxide which protects it from reacting with water. When the layer is corroded however, it will start to react and produce hydrogen gas.
The aluminium oxide reacts with hydrochloric acid because it contains oxide ions. It behaves like a base and reacts with acids by losing its oxide ions to the acid and forming a solution of aluminium chloride. It is this reaction that demonstrates the amphoteric nature of aluminium oxide. It is a reaction that also occurs with other metal oxides such as sodium oxide and magnesium oxide.