Chapter 4.4, Problem 4.16AFP

Interpretation Introduction

Interpretation:

The volume of $0.1292M\text{ Ba}{\left(\text{OH}\right)}_2$ that would neutralize $50.00\text{ mL}$ of a $0.1000M\text{ HCl}$ solution is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Barium hydroxide $\left(\text{Ba}{\left(\text{OH}\right)}_2\right)$ is a strong acid and hydrochloric acid $\left(\text{HCl}\right)$ is a strong base. Barium hydroxide $\left(\text{Ba}{\left(\text{OH}\right)}_2\right)$ and hydrochloric acid $\left(\text{HCl}\right)$ both dissociate completely into ions. They both react to form barium chloride and a water molecule.

The molecular equation for the acid-base reaction of barium hydroxide and hydrochloric acid is:

$\text{Ba}{\left(\text{OH}\right)}_2\left(aq\right)+2\text{HCl}\left(s\right)\to {\text{BaCl}}_2\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)$