Chapter 16.5, Problem 16.5.1SR

Interpretation Introduction

Interpretation:

The $\text{pH}$ of the given 0.075-M solution of per chloric acid ${\text{HClO}}_{\text{4}}$ at ${\text{25}}^{\circ }\text{C}$ has to be calculated

Concept Information:

Strong acids:

In strong acids, the ionization of acid is complete.  This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

On rearranging, the concentration of hydrogen ion ${\text{[H}}^{+}\text{]}$ can be calculated using $\text{pH}$ as follows,

${\text{[H}}^{+}\text{]}\text{=}{\text{10}}^{\text{-pH}}$

To calculate: The $\text{pH}$ of the given 0.075-M solution of perchloric acid ${\text{HClO}}_{\text{4}}$