Chapter 4.4, Problem 4.16BFP

Interpretation Introduction

Interpretation:

The molarity of a $\text{KOH}$ solution if $18.15\text{ mL}$ of it is required for the titration of a $20.00\text{mL}$ sample of a $0.2452M{\text{ HNO}}_3$ 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.

Potassium hydroxide $\left(\text{KOH}\right)$ is a strong base and nitric acid $\left({\text{HNO}}_3\right)$ is a strong acid. Potassium hydroxide $\left(\text{KOH}\right)$ and nitric acid $\left({\text{HNO}}_3\right)$ both dissociate completely into ions. They both react to form potassium nitrate and a water molecule.

The molecular equation for the acid-base reaction of potassium hydroxide and nitric acid is:

$\text{KOH}\left(aq\right)+{\text{HNO}}_3\left(s\right)\to {\text{KNO}}_3\left(aq\right)+{\text{H}}_2\text{O}\left(l\right)$