Chapter 17.3, Problem 17.5WE

Interpretation Introduction

Interpretation:

The $\text{pH}$ at the equivalence point of titration $\text{HCl}\text{Vs}{\text{NH}}_{\text{3}}$ has to be calculated

Concept introduction:

• $\text{pH}$ is the logarithm of the reciprocal of the concentration  of ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ in a solution.
• $\text{pH}$ is used to determine the acidity of an aqueous solution.
• $\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$
• Acid dissociation constant ${\text{K}}_{\text{a}}$ is defined as measure of acid strength in a given solution
• ${\text{K}}_{\text{a}}\text{=}\frac{{\text{[A}}^{\text{-}}{\text{][H}}^{\text{+}}\text{]}}{\text{[HA]}}$
• when the number of moles of standard solution equals to concentration of analyte  in titration is called equivalence point.

To calculate: The $\text{pH}$ at the equivalence point of titration $\text{HCl}\text{Vs}{\text{NH}}_{\text{3}}$.