Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6M{\text{NaHCO}}_3$ that must be poured on the spill to react completely with $88\text{ mL}$ of $2.6M{\text{ H}}_2{\text{SO}}_4$ 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 bicarbonate $\left({\text{NaHCO}}_3\right)$ is a weak base. Sulfuric acid $\left({\text{H}}_2{\text{SO}}_4\right)$ dissociates completely into ions and the sodium bicarbonate $\left({\text{NaHCO}}_3\right)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

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

${\text{H}}_2{\text{SO}}_4\left(aq\right)+2{\text{NaHCO}}_3\left(aq\right)\to {\text{Na}}_2{\text{SO}}_4\left(aq\right)+2{\text{H}}_2\text{O}\left(l\right)+2{\text{CO}}_2\left(g\right)$