Chapter 9, Problem 9.47E

Interpretation Introduction

(a)

Interpretation:

The preparation of about $750\text{mL}$ of $\text{0}\text{.5}\text{M}{\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ from dilute sulfuric acid using Table 9.4 is to be stated.

Concept introduction:

The $\text{pH}$ 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 preparation of about $200\text{mL}$ of $\text{0}\text{.1}\text{M}\text{NaOH}$ from stock sodium hydroxide solution using Table 9.4 is to be stated.

Concept introduction:

The $\text{pH}$ 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 preparation of about $1.0\text{L}$ of $1\text{M}$ acetic acid from glacial acid using Table 9.4 is to be stated.

Concept introduction:

The $\text{pH}$ 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.