Question

Give the formula of the conjugate base of HSO₄-

Answer 1

Concepts and reason

This problem is based on the concept of conjugate acid and conjugate base. A chemical species generates a negatively charged or neutral species on losing one proton, which is called its conjugate base. It is usually anionic or negative in nature whereas gaining one proton it generates a species which is either positively charged or neutral in nature, this species is called conjugate acid.

Fundamentals

Conjugate base and conjugate acid can be determined for any chemical species with the help of protonation and deprotonation.

 

Bisulphate anion on deprotonation reaction gives a sulphate anion which is a conjugate base for bisulphate anion.

The formation of conjugate base of \(\mathrm{HSO}_{4}^{-}\) is given below:

\(\mathrm{HSO}_{4}^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_{4}^{-2}\)

Thus, the conjugate base will be \(\mathrm{SO}_{4}^{-2}\).

Formula of conjugate base for \(\mathrm{HSO}_{4}^{-}\) is \(\mathrm{SO}_{4}^{-2}\).

 

Bisulphate anion on protonation reaction gives sulfuric acid, which is a conjugate acid for bisulphate anion.

The formation of conjugate acid of \(\mathrm{HSO}_{4}^{-}\) is given below:

\(\mathrm{HSO}_{4}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\)

Thus, the conjugate acid will be \(\mathrm{H}_{2} \mathrm{SO}_{4}\).

Formula of conjugate base for \(\mathrm{HSO}_{4}^{-}\) is \(\mathrm{H}_{2} \mathrm{SO}_{4}\).