# Find the volume of 0.1 M hydrochloric acid required to react with 22.0ml of 0.07 M barium hydroxide.

## Question:

Find the volume of 0.1 M hydrochloric acid required to react with 22.0ml of 0.07 M barium hydroxide.

## Reaction

A neutralization reaction happens when an acid reacts with a base, thereby producing salt and water. The number of equivalents of acid is equal to the number of equivalents of base for complete neutralization to happen.

{eq}Ba(OH)_2 + 2HCl \rightarrow BaCl2 + 2H_2O {/eq}

This reaction tells that 1 mole of barium hydroxide require 2 moles of hydrochloric acid to react completely.

Now, number of moles of barium hydroxide = Volume of barium hydroxide used* Molarity of barium hydroxide = 0.0022* 0.07

Number of moles of hydrochloric acid = Volume of hydrochloric acid used* Molarity of hydrochloric acid = V* 0.1

{eq}0.0022* 0.07 = 2*V* 0.1 \\ V = 0.00077\ L = 0.77\ mL {/eq}