Chapter 9, Problem 9.110P

Interpretation Introduction

(a)

Interpretation:

The need of $\text{HF}$ and ${\text{F}}^{\text{-}}$ to prepare the buffer solution should be determined.

Concept Introduction:

A buffer solution is a mixture of weak acid or base with its conjugate base that resists any change in pH of the solution even after the addition of a little amount of acid or base. Thus, there is no change in pH of buffer solution even after the addition of acid or base to the solution.

This is because weak acid reacts with excess ions to form its conjugate base and water whereas, the conjugate base reacts with excess ions to form a respective weak acid.

Interpretation Introduction

(b)

Interpretation:

The effect on concentration of $\text{HF}$ and ${\text{F}}^{\text{-}}$ buffer solution after addition of small amount of acid should be determined.

Concept Introduction:

A buffer solution is a mixture of weak acid or base with its conjugate base that resists any change in pH of the solution even after the addition of a little amount of acid or base. Thus, there is no change in pH of buffer solution even after the addition of acid or base to the solution.

This is because weak acid reacts with excess ions to form its conjugate base and water whereas the conjugate base reacts with excess ions to form a respective weak acid.

Interpretation Introduction

(c)

Interpretation:

The effect on concentration of $\text{HF}$ and ${\text{F}}^{\text{-}}$ buffer solution after addition of small amount of base should be determined.

Concept Introduction:

A buffer solution is a mixture of weak acid or base with its conjugate base that resists any change in pH of the solution even after the addition of a little amount of acid or base. Thus, there is no change in pH of buffer solution even after the addition of acid or base to the solution.

This is because weak acid reacts with excess ions to form its conjugate base and water whereas, the conjugate base reacts with excess ions to form a respective weak acid.