How do you determine the formula for the conjugate base of HSO_4^(-)?

Dec 7, 2016

For the conjugate base of $\text{bisulfate ion, } H S {O}_{4}^{-}$, we simply remove a proton to give $S {O}_{4}^{2 -}$.

Explanation:

To form the conjugate base or conjugate acid of any species, we simply remove OR add a proton, ${H}^{+}$.

As for all chemical reactions, even these conceptual ones, we CONSERVE mass and charge. What do I mean by this?

So the conjugate base of $\text{sulfuric acid}$, ${H}_{2} S {O}_{4}$, is $H S {O}_{4}^{-}$, and the conjugate base of $\text{bisulfate ion}$ is $S {O}_{4}^{2 -}$.

What's the conjugate base of $N {H}_{3}$? And its conjugate acid?