Chapter 16.8, Problem 13PE

(a)

Interpretation Introduction

To determine: The change in $\text{pH}$ when $0.286$ mole ${\text{H}}^{+}$ is added o $1.00\text{L}$ of buffer containing a $0.584\text{M}$ solution of pyridine $\left(\text{py}\right)$ containing $0.500\text{M}$ ${\text{pyH}}^{+}$.

Interpretation: The change in $\text{pH}$ when $0.286$ mole ${\text{H}}^{+}$ is added o $1.00\text{L}$ of buffer containing a $0.584\text{M}$ solution of pyridine $\left(\text{py}\right)$ containing $0.500\text{M}$ ${\text{pyH}}^{+}$ is to be stated.

Concept introduction: The $\text{pH}$ is defined as the measure of hydrogen ion concentration. It is the numerical scale which is used to determine whether the given solution is acidic or basic in nature.

The $\text{pH}$ of the solution is calculated by Henderson-Hasselbalch equation,

$\text{pH}=\text{p}{K}_{\text{a}}+\text{log}\left(\frac{\left[\text{Base}\right]}{\left[\text{Conjugate}\text{Acid}\right]}\right)$

Where,

• $\text{p}{K}_{\text{a}}$ is the acid dissociation constant.

(b)

Interpretation Introduction

To determine: The change in $\text{pH}$ when $0.286$ mole ${\text{H}}^{+}$ is added o $1.00\text{L}$ of buffer containing a $0.682\text{M}$ solution of aniline $\left(\text{an}\right)$ containing $0.964\text{M}$ ${\text{anH}}^{+}$.

Interpretation: The change in $\text{pH}$ when $0.286$ mole ${\text{H}}^{+}$ is added o $1.00\text{L}$ of buffer containing a $0.682\text{M}$ solution of aniline $\left(\text{an}\right)$ containing $0.964\text{M}$ ${\text{anH}}^{+}$ is to be stated.

Concept introduction: The $\text{pH}$ is defined as the measure of hydrogen ion concentration. It is the numerical scale which is used to determine whether the given solution is acidic or basic in nature.

The $\text{pH}$ of the solution is calculated by Henderson-Hasselbalch equation,

$\text{pH}=\text{p}{K}_{\text{a}}+\text{log}\left(\frac{\left[\text{Base}\right]}{\left[\text{Conjugate}\text{Acid}\right]}\right)$

Where,

• $\text{p}{K}_{\text{a}}$ is the acid dissociation constant.