Chapter 4, Problem 4.69P

Interpretation Introduction

Interpretation:

The milliliters of $0.383M\text{ HCl}$ needed to react with $16.2\text{ g}$ of ${\text{CaCO}}_3$ 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.

Hydrochloric acid $\left(\text{HCl}\right)$ is a strong acid and calcium carbonate $\left({\text{CaCO}}_3\right)$ is a weak base. Hydrochloric acid $\left(\text{HCl}\right)$ dissociates completely into ions and calcium carbonate $\left({\text{CaCO}}_3\right)$ dissociates to some extent into ions. They both react to form calcium chloride, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of hydrochloric acid and calcium carbonate is:

$\text{2HCl}\left(aq\right)+{\text{CaCO}}_3\left(s\right)\to {\text{CaCl}}_2\left(aq\right)+{\text{H}}_2\text{O}\left(l\right)+{\text{CO}}_2\left(g\right)$