Chapter 1, Problem 6P

Interpretation Introduction

(a)

Interpretation:

The pH of the 0.1 M HCl solution needs to be calculated.

Concept introduction:

The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.

It is mathematically represented as follows:

$\text{pH}=-\log \left[{\text{H}}^{+}\right]$

Here, $\left[{\text{H}}^{+}\right]$ is the concentration of hydrogen ion.

Interpretation Introduction

(b)

Interpretation:

The pH of 0.1 M NaOH needs to be calculated.

Concept introduction:

The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.

It is mathematically represented as follows:

$\text{pH}=-\log \left[{\text{H}}^{+}\right]$

Here, $\left[{\text{H}}^{+}\right]$ is the concentration of hydrogen ion.

Interpretation Introduction

(c)

Interpretation:

The pH of 0.05 M HCl solution needs to be calculated.

Concept introduction:

The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.

It is mathematically represented as follows:

$\text{pH}=-\log \left[{\text{H}}^{+}\right]$

Here, $\left[{\text{H}}^{+}\right]$ is the concentration of hydrogen ion.

Interpretation Introduction

(d)

Interpretation:

The pH of 0.05 M NaOH needs to be calculated.

Concept introduction:

The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.

It is mathematically represented as follows:

$\text{pH}=-\log \left[{\text{H}}^{+}\right]$

Here, $\left[{\text{H}}^{+}\right]$ is the concentration of hydrogen ion.