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Chapter 13: Problem 144

Which of the following represent conjugate acid-base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair. a. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}^{-}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) d. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)

Short Answer

Expert verified
a. \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{OH}^-\) are a conjugate acid-base pair. b. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{SO}_{4}^{2-}\) are not a conjugate pair; the correct conjugate base for \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is \(\mathrm{HSO}_{4}^-\). c. \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}^-\) are a conjugate acid-base pair. d. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^-\) are a conjugate acid-base pair.

Step by step solution

01

Identify the acid and base

In this pair, \(\mathrm{H}_{2} \mathrm{O}\) (water) can act as an acid, and \(\mathrm{OH}^{-}\) (hydroxide) can act as a base.
02

Check for conjugate acid-base pair

Water can lose one proton (H+) to form \(\mathrm{OH}^{-}\): \[\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{OH}^{-} + \mathrm{H}^{+}\] This means that \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{OH}^{-}\) are a conjugate acid-base pair. #b.# \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\)
03

Identify the acid and base

In this pair, \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (sulfuric acid) is the acid, and \(\mathrm{SO}_{4}^{2-}\) (sulfate) is the base.
04

Check for conjugate acid-base pair

We see that \(\mathrm{H}_{2} \mathrm{SO}_{4}\) can lose two protons (2 H+), but we need a species that only differs by one proton (H+), so sulfuric acid is not conjugate with sulfate. We must find the correct conjugate base for \(\mathrm{H}_{2}\mathrm{SO}_{4}\).
05

Find the correct conjugate base

\(\mathrm{H}_{2}\mathrm{SO}_{4}\) loses one proton to form \(\mathrm{HSO}_{4}^{-}\), so the correct conjugate base for \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is \(\mathrm{HSO}_{4}^{-}\). #c.# \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)
06

Identify the acid and base

In this pair, \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (phosphoric acid) is the acid, and \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (dihydrogen phosphate) is the base.
07

Check for conjugate acid-base pair

Phosphoric acid can lose one proton (H+) to form dihydrogen phosphate: \[\mathrm{H}_{3}\mathrm{PO}_{4} \rightleftharpoons \mathrm{H}_{2}\mathrm{PO}_{4}^{-} + \mathrm{H}^{+}\] This means that \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) are a conjugate acid-base pair. #d.# $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}$
08

Identify the acid and base

In this pair, \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}\) (acetic acid) is the acid, and \(\mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}\) (acetate) is the base.
09

Check for conjugate acid-base pair

Acetic acid can lose one proton (H+) to form acetate: \[\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2} \rightleftharpoons \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-} + \mathrm{H}^{+}\] This means that \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}\) and \(\mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}\) are a conjugate acid-base pair.

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