Question

The conjugate base of ${H_2}S{O_4}$ in the following reaction is:
${H_2}S{O_4} + {H_2}O \to {H_3}{O^ + } + HSO_4^ - $
A) ${H_2}O$
B) $HSO_4^ - $
C) ${H_3}{O^ + }$
D) $SO_4^{ - 2}$

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 the 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.
Now after knowing that we know that to get the conjugate base we just have to take back a proton $({H^ + })$ .
The reaction given to us is the ${H_2}S{O_4} + {H_2}O \to {H_3}{O^ + } + HSO_4^ - $
So the conversion of ${H_2}S{O_4}$ is done into $HSO_4^ - $ when the $({H^ + })$ is taken from it in the chemical reaction.
So that would leave us with the conjugate base as $HSO_4^ - $ .
Therefore, option (B) 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.