Chapter 16, Problem 16.43QP

Interpretation Introduction

Interpretation:

A sample of acid rain collected from a pond was shown to have a $\text{pH}$ = 4.65. What concentration of  ${\text{HNO}}_{\text{3}}$ does this pH correspond to 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.

For example:

Consider ionization of $\text{HCl}$ (a strong acid)

0.10-M $\text{HCl}$ solution contains 0.10 M hydronium ions ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ in it, because all the $\text{HCl}$ molecules ionizes.

At equilibrium (after the completion of ionization), the concentration of $\text{[HCl]}$  will be zero since no $\text{HCl}$ molecules remains after ionization.

The concentration after ionization will be as follows,

$\text{[HCl]}$= 0M

${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ = 0.10 M

${\text{[Cl}}^{\text{-}}\text{]}$=0.1 M

$\text{pH}$ 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.

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

To Calculate: The concentration of ${\text{HNO}}_{\text{3}}$ corresponding to the $\text{pH}$ = 4.65