Chapter 9, Problem 9.42E

Interpretation Introduction

(a)

Interpretation:

The given $\text{pH}$ values are to be converted into both $\left[{\text{H}}^{+}\right]$ and $\left[{\text{OH}}^{-}\right]$.

Concept introduction:

$\text{pH}$ of a solution is represented as the negative logarithm of the concentration of protons.

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

This scale is defined from $1$ to $14$. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with $\text{pH}<\text{7}$ are acidic in nature, with $\text{pH}=\text{7}$ are neutral in nature and with $\text{pH}>\text{7}$ are basic in nature.

Interpretation Introduction

(b)

Interpretation:

The given $\text{pH}$ values are to be converted into both $\left[{\text{H}}^{+}\right]$ and $\left[{\text{OH}}^{-}\right]$.

Concept introduction:

$\text{pH}$ of a solution is represented as the negative logarithm of the concentration of protons.

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

This scale is defined from $1$ to $14$. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with $\text{pH}<\text{7}$ are acidic in nature, with $\text{pH}=\text{7}$ are neutral in nature and with $\text{pH}>\text{7}$ are basic in nature.

Interpretation Introduction

(c)

Interpretation:

The given $\text{pH}$ values are to be converted into both $\left[{\text{H}}^{+}\right]$ and $\left[{\text{OH}}^{-}\right]$.

Concept introduction:

$\text{pH}$ of a solution is represented as the negative logarithm of the concentration of protons.

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

This scale is defined from $1$ to $14$. It helps to determine whether the given solution is acidic, basic or neutral. The solutions with $\text{pH}<\text{7}$ are acidic in nature, with $\text{pH}=\text{7}$ are neutral in nature and with $\text{pH}>\text{7}$ are basic in nature.