Chapter 10, Problem 10.102CP

Interpretation Introduction

Interpretation:

Among the two given acids the more acid solution and the solution that has higher hydronium ion concentration and lower $\text{pH}$ should be identified.

Concept Introduction:

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

Strong Acids: Acids that dissociates into ions completely which results in easy donation of protons are considered as strong acids. Strong acid forms weaker conjugated base.

Weak Acids: Acids that do not easily dissociate into ions completely which has difficulty in proton donation are considered as weak acids. Weak acid forms stronger conjugated base

$\text{pH}$: The concentration of hydrogen ion is measured using $\text{pH}$ scale. The $\text{pH}$ of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

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

If the value of $\text{pH}$ is less than $7$, then the solution is acidic whereas if the value of $\text{pH}$ is greater than $7$, then the solution is basic.

Equivalent-(Eq) of Acid: Generally, 1 equivalent of ion is the number of ions which has charge of one mole. In case of acids positive charge is of interest therefore, one equivalent of acid consists of 1 mole of $H^{+}$ ions.

Equivalent-(Eq) of Base: In case of bases negative charge is of interest therefore, one equivalent of base consists of 1 mole of $O{H}^{-}$ ions.