Chapter 16, Problem 25E

Interpretation Introduction

Interpretation:

A buffer solution of $350\text{ml}$ is $0.15\text{M}$ in $\text{HF}$ with $0.15\text{M}$ in $\text{NaF}$ another buffer of $350\text{ml}$ is $0.35\text{M}$ in $\text{HF}$ with $0.35\text{M}$ in $\text{NaF}$ . The mass of $\text{NaOH}$ that is added to both the buffer, to neutralize is to be calculated.

Concept introduction: A buffer solution consists of a specific amount of weak acid and its conjugate base or a specific amount of weak base and its conjugate acid.

Henderson-Hasselbalch equation provides an expression by which the pH of a buffer solution by initial concentrations of the components of the buffer solution can be calculated.

To determine: The mass of $\text{NaOH}$ to neutralize the buffer solution of $350\text{ml}$ is $0.15\text{M}$ in $\text{HF}$ with $0.15\text{M}$ in $\text{NaF}$ , before the $\text{pH}$ rises above $4.00$ and to neutralize the buffer solution of $350\text{ml}$ is $0.35\text{M}$ in $\text{HF}$ with $0.35\text{M}$ in $\text{NaF}$ , before the $\text{pH}$ rises above $4.00$ .