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

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Answer 1 · 2016-12-07T07:28:30

For the conjugate base of $"bisulfate ion, "HSO_4^-$ , we simply remove a proton to give $SO_4^(2-)$ .

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 $"sulfuric acid"$ , $H_2SO_4$ , is $HSO_4^-$ , and the conjugate base of $"bisulfate ion"$ is $SO_4^(2-)$ .

What's the conjugate base of $NH_3$ ? And its conjugate acid?

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