9. With the help of chemical equations prove that aluminums oxide is an amphoteric oxide.
Answers
Answer:
Aluminium oxide is amphoteric. It has reactions as both a base and an acid.
Reaction with water: Aluminum oxide is insoluble in water and does not react like sodium oxide and magnesium oxide. The oxide ions are held too strongly in the solid lattice to react with the water.
Reaction with acids: Aluminum oxide contains oxide ions, and thus reacts with acids in the same way sodium or magnesium oxides do. Aluminum oxide reacts with hot dilute hydrochloric acid to give aluminum chloride solution.
\[Al_2O_3 + 6HCl \rightarrow 2AlCl_3 + 3H_2O\]
This reaction and others display the amphoteric nature of aluminum oxide.
Reaction with bases: Aluminum oxide also displays acidic properties, as shown in its reactions with bases such as sodium hydroxide. Various aluminates (compounds in which the aluminum is a component in a negative ion) exist, which is possible because aluminum can form covalent bonds with oxygen. This is possible because the electronegativity difference between aluminum and oxygen is small, unlike the difference between sodium and oxygen, for example (electronegativity increases across a period)
Aluminum oxide reacts with hot, concentrated sodium hydroxide solution to produce a colorless solution of sodium tetrahydroxoaluminate:
\[Al_2O_3 + 2NaOH +3H_2O \rightarrow 2NaAl(OH)_4\]
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Answer:
HERE IS YOUR ANSWER :-
➡️Al2O3(s) + 6HCl(aq) -------> 2AlCl3(aq) + 3H20(l). In this reaction, aluminium oxide behaves as a basic oxide and reacts with an acid to produce salt and water.
➡️Aluminium oxide is an amphoteric substance, because it can react with both acids and bases, such as hydrofluoric acid and sodium hydroxide, acting as an acid with a base and a base with an acid, neutralising the other and producing a salt.
➡️Reaction with acids: Aluminum oxide contains oxide ions, and thus reacts with acids in the same way sodium or magnesium oxides do.