Question

What are the substances produced when $KO{H_{\left( {aq} \right)}}$ neutralizes $HC{l_{\left( {aq} \right)}}$?

Answer 1

Different types of reaction occur when reactants combine with each other to form a product. Neutralization reaction is also a type of chemical reaction which basically involves combination of acid with base to form a salt and water.

Complete answer:
In a neutralization reaction, acid and base react in a specific quantity to form a neutral compound which is commonly known as salt and water as a by-product.
When acid and base react in equivalent amounts there is complete neutralization that takes place with no excess hydronium ion and hydroxide ions in the solution.
Neutralization reaction is expressed as:
Acid $+$Base $\to$ Salt $+$ Water
Reaction between $KO{H_{\left( {aq} \right)}}$ and $HC{l_{\left( {aq} \right)}}$ is a type of neutralization reaction between strong base and strong acid. Here, $KO{H_{\left( {aq} \right)}}$ acts as a strong base while $HC{l_{\left( {aq} \right)}}$ acts as a strong acid.
When they both react with each other hydroxide ion from potassium hydroxide $KO{H_{\left( {aq} \right)}}$ combines with hydrogen ion of the hydrochloric acid $HC{l_{\left( {aq} \right)}}$ to form water. Similarly, potassium ions combine with chloride ions to form salt potassium chloride. The overall reaction is expressed as:
$KO{H_{\left( {aq} \right)}}$ $+$ $HC{l_{\left( {aq} \right)}}$ $\to$ $KCl + {H_2}O$
When equivalent amount of $KO{H_{\left( {aq} \right)}}$ is taken to completely neutralizes $HC{l_{\left( {aq} \right)}}$ there is no excess hydrogen ions remain left in the solution. The final solution become neutral with pH close to value of $7$ which means it is not acidic and basic in nature.
$\Rightarrow$ $KCl$ and ${H_2}O$ are produced when $KO{H_{\left( {aq} \right)}}$ neutralizes $HC{l_{\left( {aq} \right)}}$.

Note:
Neutralization comes under the category of the exothermic reaction because it is associated with release of heat. The final pH range of the solution will depend upon the strength of acid and base we used in the reaction.