Chapter 17, Problem 17.113SP

(a)

Interpretation Introduction

Interpretation:

The $\text{pH}$ of buffer solution and acid solution has to be calculated and compared to each other.

Concept introduction:

• 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.
• Buffer solution is a combination of a weak acid and its conjugate base or vice-versa in an aqueous solution.
• Dilution is defined as reducing the concentration of solute by adding more solvent in a solution.

To calculate: The $\text{pH}$ of buffer solution (${\text{CH}}_{\text{3}}\text{COOH}+{\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}$) and its ten times diluted form

(b)

Interpretation Introduction

Interpretation:

The $\text{pH}$ of buffer solution and acid solution has to be calculated and compared to each other.

Concept introduction:

• 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.
• Buffer solution is a combination of a weak acid and its conjugate base or vice-versa in an aqueous solution.
• Dilution is defined as reducing the concentration of solute by adding more solvent in a solution.

To calculate: The $\text{pH}$ of acetic acid and its ten times diluted form