Problem 19 - Chemistry: An Atoms-Focused Approach

Question

What is the conjugate acid of the bisulfate ion, \(\mathrm{HSO}_{4}^{-}\) and what is its conjugate base?

Step-by-Step Solution

Answer

Answer: The conjugate acid of the bisulfate ion (HSO4-) is sulfuric acid (H2SO4), and its conjugate base is the sulfate ion (SO4^2-).

Step 1: Identify the bisulfate ion

The bisulfate ion is given by the formula \(\mathrm{HSO}_{4}^{-}\).

Step 2: Find the conjugate acid

To find the conjugate acid, we add a proton (H+) to the bisulfate ion: \(\mathrm{HSO}_{4}^{-} + \mathrm{H}^{+} \rightarrow \mathrm{H}_{2}\mathrm{SO}_{4}\) The product, \(\mathrm{H}_{2}\mathrm{SO}_{4}\), is the conjugate acid of the bisulfate ion.

Step 3: Find the conjugate base

To find the conjugate base, we remove a proton (H+) from the bisulfate ion: \(\mathrm{HSO}_{4}^{-} \rightarrow \mathrm{SO}_{4}^{2-} + \mathrm{H}^{+}\) The product, \(\mathrm{SO}_{4}^{2-}\), is the conjugate base of the bisulfate ion.

Step 4: Write the conclusion

The conjugate acid of the bisulfate ion (\(\mathrm{HSO}_{4}^-\)) is sulfuric acid (\(\mathrm{H}_{2}\mathrm{SO}_{4}\)) and its conjugate base is the sulfate ion (\(\mathrm{SO}_{4}^{2-}\)).