Chapter 4, Problem 4.74P

Interpretation Introduction

Interpretation:

The molarity of the sodium hydroxide solution that was standardized by the titration of the solution with $25.00\text{ mL}$ of $0.1528M$ standard hydrochloric acid and the initial and final reading of burette is $2.24\text{ mL}$ and $39.21\text{ mL}$ respectively 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 dissociates completely in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Hydrochloric acid $\left(\text{HCl}\right)$ is a strong acid and sodium hydroxide $\left(\text{NaOH}\right)$ is a strong base. Sodium hydroxide $\left(\text{NaOH}\right)$ and hydrochloric acid $\left(\text{HCl}\right)$ both dissociates completely into their ions. They both react to form sodium chloride and water molecule.

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

  $\text{HCl}\left(aq\right)+\text{NaOH}\left(aq\right)\to \text{NaCl}\left(aq\right)+{\text{H}}_2\text{O}\left(l\right)$