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Chapter 15: Problem 19

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

Short Answer

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

Step by step solution

01

Identify the bisulfate ion

The bisulfate ion is given by the formula \(\mathrm{HSO}_{4}^{-}\).
02

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.
03

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.
04

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 (\(\mathrm{SO}_{4}^{2-}\)).

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Most popular questions from this chapter

The awful odor of dead fish is due mostly to trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N},\) one of three compounds related to ammonia in which methyl groups replace one, two, or all three of the \(\mathrm{H}\) atoms in ammonia. a. The \(K_{\mathrm{b}}\) of trimethylamine \(\left[\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\right]\) is \(6.5 \times\) \(10^{-5}\) at \(25^{\circ} \mathrm{C} .\) Calculate the \(\mathrm{pH}\) of \(3.00 \times 10^{-4} M\) trimethylamine. b. The \(K_{\mathrm{b}}\) of methylamine \(\left[\left(\mathrm{CH}_{3}\right) \mathrm{NH}_{2}\right]\) is \(4.4 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) Calculate the \(\mathrm{pH}\) of \(2.88 \times 10^{-3} \mathrm{M}\) methylamine. "c. The \(K_{\mathrm{b}}\) of dimethylamine \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\right]\) is \(5.9 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) What concentration of dimethylamine is needed for the solution to have the same \(\mathrm{pH}\) as the solution in part b?

What is the pH of \(0.75 M \mathrm{H}_{2} \mathrm{SO}_{4} ?\)

Why is it unnecessary to publish tables of \(K_{\mathrm{b}}\) values of the conjugate bases of weak acids whose \(K_{\mathrm{a}}\) values are known?

What is the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions in \(0.65 \mathrm{M} \mathrm{HNO}_{3} ?\)

Identify the conjugate acid of each of the following species: \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}, \mathrm{CH}_{3} \mathrm{COO}^{-}, \mathrm{HSO}_{4}^{-},\) and \(\mathrm{OH}^{-}\)
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