Q.Aluminium is described as an amphoteric metal. Write balanced equations for its reaction with

[!TLDR] Aluminium reacts with dilute HCl to give AlCl3 + H2, and with NaOH to give sodium aluminate + H2, showing its amphoteric character. [!ANSWER] $2\text{Al}+6\text{HCl}\rightarrow 2\text{AlCl}_3+3\text{H}_2$ and $2\text{Al}+2\text{NaOH}+2\text{H}_2\text{O}\righ …

Aluminium's amphoteric character means it reacts with both acids and bases, dissolving and liberating hydrogen gas in each case, though forming a different aluminium-containing product depending on which reagent is used. With dilute hydrochloric acid, aluminium is oxidised while $\text{H}^+$ is reduced to $\text{H}_2$, giving aluminium chloride in solution:\n$2\text{Al} + 6\text{HCl} \longrightarrow 2\text{AlCl}_3 + 3\text{H}_2$\nWith aqueous sodium hydroxide, aluminium again dissolves with the liberation of hydrogen gas, but here the aluminium ends up as the aluminate ion rather than a simple chloride salt:\n$2\text{Al} + 2\text{NaOH} + 2\text{H}_2\text{O} \longrightarrow 2\text{NaAlO}_2 + 3\text{H}_2$\n(the aluminate can equally be written as the hydrated complex $\text{Na}[\text{Al(OH)}_4]$, obtained by writing the reaction with one extra equivalent of water per aluminium: $2\text{Al}+2\text{NaOH}+6\text{H}_2\text{O}\rightarrow 2\text{Na}[\text{Al(OH)}_4]+3\text{H}_2$). In ordinary conditions, aluminium metal is protected by an extremely thin, tough, self-healing oxide lay …

Write and balance the two separate reactions of Al with dilute acid and with base, naming the distinct aluminium pr …

Leaving the equations unbalanced for hydrogen; naming the same product (e.g. AlCl3) for both reactions instead of recognising …