Question

The conjugate base of \[{(C{H_3})_2}NH_2^ + \] is:
A) $C{H_3}N{H_2}$
B) ${(C{H_3})_2}{N^ + }$
C) ${(C{H_3})_3}N$
D) ${(C{H_3})_2}NH$

Answer 1

HintFirstly we should be clear what exactly is the conjugate base for an acid. That we get as what we can describe as a left over after an acid has donated a proton during a chemical reaction. Now that means that if we take back a $({H^ + })$ from the acid then left over would be conjugate base.

Complete step by step answer:
Firstly we should be aware that the question is regarding the combining capacity of any atom of any element with another element.We can say that a conjugate base is what we can describe as a left over after an acid has donated a proton during a chemical reaction. Hence we get that a conjugate base is a derivative species that is formed by the removal of a proton from an acid. This can be considered as in the reverse reaction it is able to gain a hydrogen ion. Because some acids are capable of releasing multiple protons, we can say that the conjugate base of an acid could in turn itself be acidic.
Apart from that a more general definition is that a conjugate base is the base member, X-, of a pair of compounds that transform into each other by gaining or losing a proton.
Now after knowing that we know that to get the conjugate base we just have to take back a proton $({H^ + })$ .
So that would leave us with the conjugate base as ${(C{H_3})_2}NH$ .
Therefore, option (D) is correct.

Note:Johannes Nicolaus Brønsted and Martin Lowry introduced the Brønsted–Lowry theory, which proposed that any compound that can transfer a proton to any other compound is an acid, and the compound that accepts the proton is a base.