AII(OH)3+HCI>AICI3+H2O

The reaction you've provided is a classic acid-base reaction involving aluminum hydroxide \((\text{A}l(OH)_3)\) and hydrochloric acid \((\text{HCl})\). In this reaction, aluminum hydroxide acts as a base, while hydrochloric acid acts as an acid.

The balanced chemical equation for the reaction can be written as:

\[ \text{Al(OH)}_3 + 3 \text{HCl} \rightarrow \text{AlCl}_3 + 3 \text{H}_2\text{O} \]

Explanation of the Reaction:

1. Reactants:

   • Aluminum Hydroxide \((\text{Al(OH)}_3)\): A compound that acts as a weak base in this reaction.
   • Hydrochloric Acid \((\text{HCl})\): A strong acid that donates protons (H⁺ ions) to the reaction.

2. Products:

   • Aluminum Chloride \((\text{AlCl}_3)\): A salt formed by the combination of aluminum ions and chloride ions.
   • Water \((\text{H}_2\text{O})\): A byproduct of the neutralization reaction.

Steps to Understand the Reaction:

• Acid-Base Reaction: The \(\text{HCl}\) donates protons to the \(\text{Al(OH)}_3\), resulting in the formation of water and aluminum ions.
• Ion Exchange: The aluminum ions from \(\text{Al(OH)}_3\) combine with the chloride ions from \(\text{HCl}\) to form \(\text{AlCl}_3\).

Conclusion:

This equation describes the neutralization of aluminum hydroxide by hydrochloric acid, resulting in aluminum chloride and water. Remember to balance the equation properly for stoichiometry when performing calculations related to the reactants and products.