Chapter 17.3, Problem 4PPB

(a)

Interpretation Introduction

Interpretation:

The volume of base added in titration of  $\text{NaOH}\text{Vs}\text{HF}$ on various $\text{pH}$ has to be calculated.

Concept introduction:

• $\text{pH}$ is the logarithm of the reciprocal of the concentration  of ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ in a solution.
• The point at which amount of standard solution and analyte becomes equal and neutralisation happens in titration is called equivalence point.
• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation.
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base.
• Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

To calculate: The volume of base added in titration of $\text{NaOH}\text{Vs}\text{HF}$ when $\text{pH}\text{=}2.85$

(b)

Interpretation Introduction

Interpretation:

The volume of base added in titration of  $\text{NaOH}\text{Vs}\text{HF}$ on various $\text{pH}$ has to be calculated.

Concept introduction:

• $\text{pH}$ is the logarithm of the reciprocal of the concentration  of ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ in a solution.
• The point at which amount of standard solution and analyte becomes equal and neutralisation happens in titration is called equivalence point.
• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation.
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base.
• Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

To calculate: The volume of base added in titration of $\text{NaOH}\text{Vs}\text{HF}$ when $\text{pH}\text{= 3}\text{.15}$

 (c)

Interpretation Introduction

Interpretation:

The volume of base added in titration of  $\text{NaOH}\text{Vs}\text{HF}$ on various $\text{pH}$ has to be calculated.

Concept introduction:

• $\text{pH}$ is the logarithm of the reciprocal of the concentration  of ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ in a solution.
• The point at which amount of standard solution and analyte becomes equal and neutralisation happens in titration is called equivalence point.
• $\text{pH}\text{=}{\text{pK}}_{\text{a}}\text{+}\text{log}\frac{\text{[conjugate base]}}{\text{[acid]}}$ is Henderson-Hasselbalch equation.
• Buffer solution is defined as a solution that oppose changes in $\text{pH}$ while adding little amount of either an acid or a base.
• Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

To calculate: The volume of base added in titration of $\text{NaOH}\text{Vs}\text{HF}$ when $\text{pH}\text{= 11}\text{.89}$