Chapter 14, Problem 14.136MP

Interpretation Introduction

Interpretation:

The balanced net ionic equations for the neutralization reactions and $pH$ of the solution should be identified.

Concept Introduction:

Neutralization reaction: It is type of chemical reaction in which, reaction of the acid with base results in formation of salt and water.

$K_a$: Acid dissociation constant ${\text{K}}_{\text{a}}$ represents how strong the acid is in a solution.

Equilibrium constant ${\text{K}}_{\text{eq}}$ represents extend of dissociation of acid in aqueous solution.

For a dissociation of acid $\left(HA\right)$ in aqueous solution,

$HA+H_{2}O\underset{}{\overset{}{\rightleftharpoons }}{H}_3{O}^{+}+A^{-}$

$k_{eq}=\frac{\left[H_3{O}^{+}\right]\left[A^{-}\right]}{\left[HA\right]\left[H_{2}O\right]}$

Where,

${\text{K}}_{\text{a}}\to \text{acid ionization constant}$

${\text{[H}}^{\text{+}}\text{]}\to \text{concentration of hydrogen ion}$

${\text{[A}}^{\text{-}}\text{]}\to \text{concentration of acid anion}$

$\text{[HA]}\to \text{concentration of the acid}$

$\text{pH}$: 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.

It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

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

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.

Moles: One mole is equivalent to the mass of the substance consists of same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

Molarity: The concentration for solutions is expressed in terms of molarity as follows,

$\text{Molarity = }\frac{\text{No}\text{. of moles of solute}}{\text{Volume of solution in L}}$

Bronsted-Lowry acid: If a species loses a proton then it is considered as Bronsted-Lowry acid.