Chapter 17, Problem 17.22QP

(1)

Interpretation Introduction

Interpretation:

From the given figures predict highest and lowest $\text{pH}$, and number of dissimilar species present on addition of hydrogen ion and hydroxide ion have to be explained.

Concept introduction:

• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation
• If concentration of conjugate base is larger than weak acid then $\text{pH}>{\text{pK}}_{\text{a}}$
• If concentration of weak acid is larger than conjugate base then $\text{pH}<{\text{pK}}_{\text{a}}$
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $\text{pH}$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

To find: the solution with highest and lowest $\text{pH}$

(2)

Interpretation Introduction

Interpretation:

From the given figures predict highest and lowest $\text{pH}$, and number of dissimilar species present on addition of hydrogen ion and hydroxide ion have to be explained.

Concept introduction:

• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation
• If concentration of conjugate base is larger than weak acid then $\text{pH}>{\text{pK}}_{\text{a}}$
• If concentration of weak acid is larger than conjugate base then $\text{pH}<{\text{pK}}_{\text{a}}$
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $\text{pH}$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

To predict: what happens on addition of hydrogen ions

(3)

Interpretation Introduction

Interpretation:

From the given figures predict highest and lowest $\text{pH}$, and number of dissimilar species present on addition of hydrogen ion and hydroxide ion have to be explained.

Concept introduction:

• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation
• If concentration of conjugate base is larger than weak acid then $\text{pH}>{\text{pK}}_{\text{a}}$
• If concentration of weak acid is larger than conjugate base then $\text{pH}<{\text{pK}}_{\text{a}}$
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base. In general, addition of acid or base does not affect the $\text{pH}$ in buffer solution but if it is more than amount of conjugate base or conjugate acid, then buffer loses its buffering capacity.

To predict: what happens on addition of hydroxide ions