Question

Complete and balance the following equation and also state the type of reaction that is taking place:

$\mathrm{Mg}{\left(\mathrm{OH}\right)}_2+\mathrm{HCl}\to$

Answer 1

Part 1:

Balance equation:

• A balanced chemical equation has the same number of atoms on the reactant and product sides for each element involved in the reaction.

The balanced equation is:

$$\begin{gathered} \mathrm{Mg}{\left(\mathrm{OH}\right)}_2+2\mathrm{HCl}\to {\mathrm{MgCl}}_2+2{\mathrm{H}}_2\mathrm{O} \\ \mathrm{Magnesium}\mathrm{Hydrogen}\mathrm{Magnesium}\mathrm{Water} \\ \mathrm{hydroxide}\mathrm{chloride}\mathrm{chloride} \end{gathered}$$

Part 2: This is a neutralization reaction.

Neutralization reaction:

• Neutralization reaction involving the mixing of an acid and base to form water and salt.
• A neutralization reaction can be defined as a chemical reaction in which an acid and base quantitatively react together to form salt and water as products.
• In a neutralization reaction, there is a combination of ${\mathrm{H}}^{+}$ions and ${\mathrm{OH}}^{-}$ ions which form water.
• A neutralization reaction is generally an acid-base neutralization reaction.