Chapter 4, Problem 4.72P

Interpretation Introduction

Interpretation:

The molarity of the acid solution if $26.25\text{ mL}$ of $0.1850M\text{ NaOH}$ solution reacts with $25.00\text{ mL}$ of ${\text{H}}_2{\text{SO}}_4$ 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.

Sulfuric acid $\left({\text{H}}_2{\text{SO}}_4\right)$ is a strong acid and sodium hydroxide $\left(\text{NaOH}\right)$ is a strong base. Sodium hydroxide $\left(\text{NaOH}\right)$ and sulfuric acid $\left({\text{H}}_2{\text{SO}}_4\right)$ both dissociate completely into ions. They both react to form sodium sulfate and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium hydroxide is:

${\text{H}}_2{\text{SO}}_4\left(aq\right)+2\text{NaOH}\left(aq\right)\to {\text{Na}}_2{\text{SO}}_4\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)$