Chapter 16, Problem 16.129SP

(a)

Interpretation Introduction

Interpretation:

The equations showing proton transfer between the given acids and acetic acid has to be written.

Concept Introduction:

Strength of acid

The degree to which an acid produces hydrogen ion determines the strength of an acid.

In other words, it refers to the tendency or ability of an acid to lose a proton. The strength of all the acids will not be same.  The strength of an acid is measurable.

Based on the strength of the acid, acids can be classified as strong acids and weak acids.

Acids ionize in water.  Strong acids ionize completely whereas weak acids ionize to some limited extent.

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.

Weak acids:

In weak acids, the ionization of acid is not complete.  This implies that the concentration of the hydrogen ion or hydronium ion will not be equal to the initial concentration of the acid at equilibrium.

For strong acids the concentration of acid will be same as that of the concentration of hydrogen ions, because strong acids undergo complete ionization.

In case of weak acid, the concentration of hydrogen ion will be less than the concentration of given acid; since weak acid does not ionize completely.

(b)

Interpretation Introduction

Interpretation:

Lewis structure should be drawn for the given conjugated acid.

Concept Introduction:

Lewis Theory: This theory relates acid-base behaviour of molecules of their molecular structure.

Lewis acid: A species that is an electron pair acceptor

Lewis base: A species that is an electron pair donor.

  $\begin{array}{l}{H}^{+}+N{H}_3\underset{}{\to }N{H}_4^{+}\\ H^{+}--Acceptor\\ N{H}_3--Donor\end{array}$