Acids, alkalis and titrations

A student carries out a titration to determine the volume of hydrochloric acid needed to neutralise a solution of barium hydroxide.

She starts with $cm320.0\text{ cm}^3$ of barium hydroxide solution of concentration $mol/dm30.150\text{ mol/dm}^3$ .

She adds $mol/dm30.250\text{ mol/dm}^3$ hydrochloric acid until the barium hydroxide is completely neutralised.

The equation for this reaction is:

\text{Ba(OH)}_2 + 2\text{HCl} \rightarrow \text{BaCl}_2 + 2\text{H}_2\text{O}

Calculate the amount, in moles, of barium hydroxide used.

[2]

Calculate the amount, in moles, of hydrochloric acid needed to neutralise this amount of barium hydroxide.

[2]

Calculate the volume, in $cm3\text{cm}^3$ , of hydrochloric acid needed to neutralise this status of barium hydroxide.

[2]

Acids, alkalis and titrations Questions