Question

What is the conjugate base of $$H_{2}S{O}_4$$?

Answer 1

Hint: Arrhenius is one of the concepts for acid and bases. Swedish chemist Arrhenius is the world's first chemist to talk about acid and bases. Depending on his concept and limitations later so many concepts are developed. Even Arrhenius is the birthplace of the concept of acids and bases. Followed by Arrhenius chemist the concept of acids and bases discuss Bronsted and Lowry in the world. In general, pH values of all acids are in between $$\text{0}\text{.9}$$-$$6.9$$and all the bases are in between$$7.1-14.0$$.

Complete answer:
As we know, according to the Arrhenius concept sulphuric acid $$H_{2}S{O}_4$$ is acidic because it can donate to protons. Bisulphate ion $$HS{O_4}^{-}$$ is a conjugate base of sulphuric acid because it is able to accept the protons.
The chemical reaction for the above discussion, given below,
 $$H_{2}S{O}_4\to H^{+}+HS{O_4}^{-}$$
According to the above discussion, we conclude $$HS{O_4}^{-}$$ is a conjugate base of $$H_{2}S{O}_4$$.

Note:
According to the Arrhenius concept one substance said to acid means, acid is nothing but a substance that dissociates to give hydrogen ion when decomposed in the water.
Examples of Arrhenius acids are hydrochloric acid ($$\text{HCl}$$), sulphuric acid ($${\text{H}}_{\text{2}}\text{S}{\text{O}}_{\text{4}}$$), nitric acid ($$\text{HN}{\text{O}}_{\text{3}}$$) etc,.
According to Arrhenius concept one substance said to base means, bases is nothing but a substance that dissociates to give hydroxyl ion when decomposed in water.
Examples of Arrhenius bases are sodium hydroxide ($$\text{NaOH}$$), calcium hydroxide ($$\text{Ca(OH}{\text{)}}_{\text{2}}$$) etc,.
But, Arrhenius theory has some limitations. One of the main limitations is not being able to explain the behaviour of acids and bases in non-aqueous solvents such as acetone etc,. It is not able to explain the acid which doesn't contain hydrogen and bases don’t contain hydroxyl ion in the formula. Ammonia is a well known base that is not accepted as base in Arrhenius base. These limitations are recovered by further coming theories like the Bronsted and Lowry concept of acids and bases.