Write reactions to justify amphoteric nature of aluminium.

"Aluminum's amphoteric nature is evident when it reacts with both acids and bases. When it encounters an acidic environment, such as hydrochloric acid, it forms aluminum chloride and hydrogen gas. On the other hand, in a basic solution like sodium hydroxide, aluminum reacts to form sodium aluminate and hydrogen gas. This ability to react with both acidic and basic substances showcases its amphoteric behavior."

"One clear demonstration of aluminum's amphoteric nature is its reaction with both strong acids and strong bases. When aluminum reacts with an acid like sulfuric acid, it produces aluminum sulfate and hydrogen gas. Conversely, when it interacts with a strong base like potassium hydroxide, it yields potassium aluminate and hydrogen gas. This dual reactivity illustrates its characteristic amphoteric behavior."

"Aluminum exhibits its amphoteric properties through its reactions with both acidic and basic solutions. For instance, when it reacts with an acid such as nitric acid, it forms aluminum nitrate and releases hydrogen gas. Similarly, when it comes into contact with a base like calcium hydroxide, it produces calcium aluminate and liberates hydrogen gas. These reactions clearly demonstrate aluminum's ability to behave as both an acid and a base."

"The amphoteric nature of aluminum becomes apparent in its reactions with acids and bases. When treated with an acid like hydrochloric acid, aluminum undergoes a reaction to form aluminum chloride and hydrogen gas. In contrast, when exposed to a base such as sodium hydroxide, aluminum reacts to produce sodium aluminate and hydrogen gas. These reactions underscore aluminum's dual propensity to interact with both acidic and basic environments, thus exhibiting its amphoteric character."