Chapter 11, Problem 5PP

Interpretation Introduction

Interpretation:

The equations for the acid–base reactions, when ethanol is added to the given compounds by labelling the stronger acid and the stronger base, the weaker acid and the weaker base is to be written.

Concept introduction:

Acids are species that donate their protons to form a conjugate base and increases the hydronium ion concentration in an aqueous solution.

Bases are species that accept protons to form a conjugate acid and increases the hydroxide ion concentration in an aqueous solution.

The stronger the acid is, the more stable is its conjugate base. Weak acids have relatively unstable conjugate base and can recombine with a proton to form acids.

A strong acid has a weak conjugate base and a weak acid has a strong conjugate base.

A strong base has a weak conjugate acid and a weak base has a strong conjugate acid.

The loss of proton $\left({\text{H}}^{+}\right)$ from an acid forms its conjugate base and a base accepts a proton $\left({\text{H}}^{+}\right)$ to forms its conjugate acid.

$\begin{array}{c}\text{Acid}\rightleftharpoons \text{Conjugate base}+{\text{H}}^{+}\\ \text{Base}+{\text{H}}^{+}\rightleftharpoons \text{Conjugate acid}\end{array}$

The combined reaction is:

$\text{Acid}+\text{Base}\rightleftharpoons \text{Conjugate base}+\text{Conjugate acid}$