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Chapter 13: Problem 38

For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and the conjugate acid. a. \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\) b. \(\mathrm{H}_{2} \mathrm{O}+\mathrm{HONH}_{3}^{+} \rightleftharpoons \mathrm{HONH}_{2}+\mathrm{H}_{3} \mathrm{O}^{+}\) c. HOCl \(+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} \rightleftharpoons \mathrm{OCl}^{-}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)

Short Answer

Expert verified
a. Acid: \(\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}^{3+}\), Base: \(\mathrm{H}_{2}\mathrm{O}\), Conjugate base: \(\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\), Conjugate acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\) b. Acid: \(\mathrm{HONH}_{3}^{+}\), Base: \(\mathrm{H}_{2}\mathrm{O}\), Conjugate base: \(\mathrm{HONH}_{2}\), Conjugate acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\) c. Acid: HOCl, Base: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), Conjugate base: \(\mathrm{OCl}^{-}\), Conjugate acid: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)

Step by step solution

01

Identify the acid and the base

In this reaction, the acid donates a proton to the base, forming the products. We see that \(\mathrm{H}_{3}\mathrm{O}^{+}\) has an extra proton in comparison to \(\mathrm{H}_{2}\mathrm{O}\), so we can identify the substances as follows: - Acid: \(\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{6}^{3+}\) - Base: \(\mathrm{H}_{2}\mathrm{O}\)
02

Identify the conjugate base and the conjugate acid

The conjugate base is formed from the acid after it loses a proton, and the conjugate acid is formed from the base after it gains a proton. Therefore, we have: - Conjugate base: \(\mathrm{Al}\left(\mathrm{H}_{2}\mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\) - Conjugate acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\) b. $\mathrm{H}_{2} \mathrm{O}+\mathrm{HONH}_{3}^{+} \rightleftharpoons \mathrm{HONH}_{2}+\mathrm{H}_{3} \mathrm{O}^{+}$
03

Identify the acid and the base

Again, we look for the substances that donate and accept protons in this reaction. Here, \(\mathrm{HONH}_{3}^{+}\) donates the proton to \(\mathrm{H}_{2}\mathrm{O}\), leading to the formation of the products. Therefore, we can identify the substances as: - Acid: \(\mathrm{HONH}_{3}^{+}\) - Base: \(\mathrm{H}_{2}\mathrm{O}\)
04

Identify the conjugate base and the conjugate acid

As before, the conjugate base is formed from the acid after it loses a proton, and the conjugate acid is formed from the base after it gains a proton. In this case: - Conjugate base: \(\mathrm{HONH}_{2}\) - Conjugate acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\) c. HOCl $+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} \rightleftharpoons \mathrm{OCl}^{-}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}$
05

Identify the acid and the base

In this reaction, we can see that \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\) has an extra proton in comparison to \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), so it appears that HOCl donates a proton to \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\). This allows us to identify the substances as: - Acid: HOCl - Base: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\)
06

Identify the conjugate base and the conjugate acid

Following our definitions, the conjugate base is formed from the acid after it loses a proton, and the conjugate acid is formed from the base after it gains a proton. Thus, we have: - Conjugate base: \(\mathrm{OCl}^{-}\) - Conjugate acid: \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)

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Most popular questions from this chapter

Rank the following 0.10 \(M\) solutions in order of increasing pH. a. HI, HF, NaF, NaI b. \(\mathrm{NH}_{4} \mathrm{Br}, \mathrm{HBr}, \mathrm{KBr}, \mathrm{NH}_{3}\) c. \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{NO}_{3}, \mathrm{NaNO}_{3}, \mathrm{NaOH}, \mathrm{HOC}_{6} \mathrm{H}_{5}, \mathrm{KOC}_{6} \mathrm{H}_{5}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}, \mathrm{HNO}_{3}\)

Arrange the following 0.10 \(M\) solutions in order from most acidic to most basic. See Appendix 5 for \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values. $$\mathrm{CaBr}_{2}, \quad \mathrm{KNO}_{2}, \quad \mathrm{HClO}_{4}, \quad \mathrm{HNO}_{2}, \quad \mathrm{HONH}_{3} \mathrm{ClO}_{4}$$

What are the major species present in 0.250 \(M\) solutions of each of the following acids? Calculate the pH of each of these solutions. a. \(\mathrm{HNO}_{2}\) b. \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\)

Consider a \(0.67-M\) solution of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\left(K_{\mathrm{b}}=5.6 \times 10^{-4}\right)\) a. Which of the following are major species in the solution? i. \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\) ii. \(\mathrm{H}^{+}\) iii. OH \(^{-}\) iv. \(\mathrm{H}_{2} \mathrm{O}\) v. \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\) b. Calculate the \(p\) H of this solution.

Calculate the \(\mathrm{pH}\) of each of the following solutions containing a strong acid in water. a. \(2.0 \times 10^{-2} M \mathrm{HNO}_{3}\) b. \(4.0 \mathrm{M} \mathrm{HNO}_{3}\) c. \(6.2 \times 10^{-12} \mathrm{M} \mathrm{HNO}_{3}\)
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