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Chapter 14: Problem 150

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. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) d. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)

Short Answer

Expert verified
Pairs A, C, and D represent conjugate acid-base pairs. Pair B is not a conjugate acid-base pair, and the correct conjugate base for \(\mathrm{H}_2\mathrm{SO}_4\) is \(\mathrm{HSO}_4^-\).

Step by step solution

01

Pair A: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}^-\)

First, we need to evaluate if these species are related. In this case, the species could be an acid and its conjugate base. We find the conjugate base of \(\mathrm{H}_{2} \mathrm{O}\) by removing a proton: \[\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{OH}^- + H^+\] Since the conjugate species is the same as the given \(\mathrm{OH}^-\), pair A represents a conjugate acid-base pair.
02

Pair B: \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\)

Now, we evaluate if these species are related. The species could be an acid and its conjugate base. We find the conjugate base of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) by removing a proton: \[\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{HSO}_{4}^- + H^+\] The conjugate base found is \(\mathrm{HSO}_{4}^-\), which is different from the given \(\mathrm{SO}_{4}^{2-}\). Thus, pair B does not represent a conjugate acid-base pair, and the correct conjugate base for \(\mathrm{H}_2\mathrm{SO}_4\) is \(\mathrm{HSO}_4^-\).
03

Pair C: \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

We need to check if these species are related. The species could be an acid and its conjugate base. We find the conjugate base of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) by removing a proton: \[\mathrm{H}_{3} \mathrm{PO}_{4} \rightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^- + H^+\] Since the conjugate species is the same as the given \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\), pair C represents a conjugate acid-base pair.
04

Pair D: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)

Let's see if these species are related. They could be an acid and its conjugate base. We find the conjugate base of \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) by removing a proton: \[\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \rightarrow \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^- + H^+\] Since the conjugate species is the same as the given \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\), pair D represents a conjugate acid-base pair. In summary, pairs A, C, and D are conjugate acid-base pairs, while pair B is not. The correct conjugate base for pair B is \(\mathrm{HSO}_{4}^-\).

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Most popular questions from this chapter

Students are often surprised to learn that organic acids, such as acetic acid, contain \(-\) OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as \(\mathrm{H}_{2} \mathrm{SO}_{4}\), has the structural formula \(\mathrm{SO}_{2}(\mathrm{OH})_{2}\), where \(\mathrm{S}\) is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while \(\mathrm{NaOH}\) and \(\mathrm{KOH}\) are bases? a. \(\mathrm{SO}(\mathrm{OH})_{2}\) b. \(\mathrm{ClO}_{2}(\mathrm{OH})\) c. \(\mathrm{HPO}(\mathrm{OH})_{2}\)

For the reaction of hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right)\) in water. $$ \mathrm{H}_{2} \mathrm{NNH}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{NNH}_{3}^{+}(a q)+\mathrm{OH}^{-}(a q) $$ \(K_{\mathrm{b}}\) is \(3.0 \times 10^{-6}\). Calculate the concentrations of all species and the \(\mathrm{pH}\) of a \(2.0 \mathrm{M}\) solution of hydrazine in water.

Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced equations for the reactions causing the solution to be acidic or basic. The relevant \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values are found in Tables \(14.2\) and \(14.3 .\) a. \(\mathrm{KCl}\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}\) e. \(\mathrm{NH}_{4} \mathrm{~F}\) b. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(\mathrm{KF}\) f. \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{CN}\)

Consider \(1000 . \mathrm{mL}\) of a \(1.00 \times 10^{-4} M\) solution of a certain acid HA that has a \(K_{\mathrm{a}}\) value equal to \(1.00 \times 10^{-4} .\) How much water was added or removed (by evaporation) so that a solution remains in which \(25.0 \%\) of HA is dissociated at equilibrium? Assume that HA is nonvolatile.

A \(0.20 \mathrm{M}\) sodium chlorobenzoate \(\left(\mathrm{NaC}_{7} \mathrm{H}_{4} \mathrm{ClO}_{2}\right)\) solution has a \(\mathrm{pH}\) of \(8.65 .\) Calculate the \(\mathrm{pH}\) of a \(0.20 \mathrm{M}\) chlorobenzoic acid \(\left(\mathrm{HC}_{7} \mathrm{H}_{4} \mathrm{ClO}_{2}\right)\) solution.
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