Chapter 13, Problem 102E

Interpretation Introduction

Interpretation: The percent of pyridine $\left({\text{C}}_{\text{5}}{\text{H}}_{\text{5}}\text{N}\right)$ that leads to the formation of pyridium ion $\left({\text{C}}_{\text{5}}{\text{H}}_{\text{5}}{\text{NH}}^{\text{+}}\right)$ in a $0.10\text{M}$ aqueous solution of pyridine is to be calculated.

Concept introduction: The $\text{pH}$ of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The $\text{pH}$ of a solution is calculated by the formula, $\text{pH}=-\log \left[{\text{H}}^{+}\right]$

At equilibrium, the equilibrium constant expression is expressed by the formula,

$K_{\text{b}}=\frac{\text{Concentration}\text{of}\text{products}}{\text{Concentration}\text{of}\text{reactants}}$

The percent ionization of an acid is calculated by the formula,

$\text{Percent}\text{ionization}=\frac{\text{Equilibrium}\text{concentration}\text{of}\left[{\text{OH}}^{-}\right]}{\text{Initial}\text{concentration}\text{of}\text{the}\text{base}}\times 100$