Question

Whether the conjugate base of $N{H_3}$ is $N{H^{3 + }}$ or not. Explain why?

Answer 1

A conjugate acid, within the Bronsted Lowry acid base theory, is a chemical compound formed when an acid donates a proton $({H^ + })$ to a base. It is a base with a hydrogen ion added to it, as in the reverse reaction it loses a hydrogen ion.

Complete answer:
A conjugate base is what is left over after an acid has donated a proton during a chemical reaction. Hence, a conjugate base is a species formed by the removal of a proton from an acid, as in the reverse reaction it is able to gain a hydrogen ion. Also, conjugate base is a species formed by the removal of a proton from an acid, as in the reverse reaction it is able to gain a hydrogen ion.
$Acid + base \rightleftharpoons \text{conjugate acid + conjugate base}$
$-$ Conjugate acid of $N{H_3}$ is $N{H_4}^ +$ . When $N{H_3}$ takes up a proton, it gets converted to its conjugate acid.
$-$ Conjugate base of $N{H_3}$ is $N{H_2}^ -$ . When $N{H_3}$ releases a proton it gets converted to its conjugate base.
However, we could move to a different solvent. Ammonia, which may be easily condensed in a laboratory undergoes a reaction
$2N{H_3} \rightleftharpoons N{H^{4 + }} + N{H^{2 - }}$
And thus here, ammonium ion, $N{H^{4 + }}$ , is the conjugate acid of ammonia, and amide ion, $N{H^{2 - }}$ , is its conjugate base.

Note:
The strength of a conjugate acid is directly proportional to its dissociation constant. If a conjugate acid is strong, its dissociation will have a higher equilibrium constant and the products of the reaction will be favored. The strength of a conjugate base can be seen as the tendency of the species to pull hydrogen protons towards itself.