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Chapter 4: Problem 11

Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. Label the original acid and its conjugate base; then label the original base and its conjugate acid. (a) \(\mathrm{NH}_{4}^{+}+\mathrm{OH}^{-} \rightleftharpoons\) (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} \rightleftharpoons\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}+\mathrm{NH}_{4}^{+} \rightleftharpoons\) (d) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \rightleftharpoons\)

Short Answer

Expert verified
Question: Identify the original acid and its conjugate base, and the original base and its conjugate acid in the following proton-transfer reaction: \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{CH}_{3} \mathrm{NH}_{2}+\mathrm{H}_{2}\mathrm{O}\). Answer: In this reaction, the original acid is \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) and its conjugate base is \(\mathrm{CH}_{3} \mathrm{NH}_{2}\). The original base is \(\mathrm{OH}^{-}\) and its conjugate acid is \(\mathrm{H}_{2}\mathrm{O}\).

Step by step solution

01

Identify the species

We have \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{OH}^{-}\) in the reaction.
02

Identify the acid and base

The \(\mathrm{NH}_{4}^{+}\) is the acid (donates a proton), while the \(\mathrm{OH}^{-}\) is the base (accepts a proton).
03

Show the proton transfer using curved arrows

The proton transfer can be shown as: \(\mathrm{NH}_{4}^{+}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{NH}_{3}+\mathrm{H}_{2}\mathrm{O}\)
04

Label the conjugate acid and base

In this reaction, the original acid is \(\mathrm{NH}_{4}^{+}\) and its conjugate base is \(\mathrm{NH}_{3}\). The original base is \(\mathrm{OH}^{-}\) and its conjugate acid is \(\mathrm{H}_{2}\mathrm{O}\). (b)
05

Identify the species

We have \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) and \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) in the reaction.
06

Identify the acid and base

The \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) is the base, while the \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) is the acid.
07

Show the proton transfer using curved arrows

The proton transfer can be shown as: \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{NH}_{2}\)
08

Label the conjugate acid and base

In this reaction, the original acid is \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) and its conjugate base is \(\mathrm{CH}_{3} \mathrm{NH}_{2}\). The original base is \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) and its conjugate acid is \(\mathrm{CH}_{3} \mathrm{COOH}\). (c)
09

Identify the species

We have \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\) and \(\mathrm{NH}_{4}^{+}\) in the reaction.
10

Identify the acid and base

The \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\) is the base, while the \(\mathrm{NH}_{4}^{+}\) is the acid.
11

Show the proton transfer using curved arrows

The proton transfer can be shown as: \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}+\mathrm{NH}_{4}^{+} \rightleftharpoons \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{NH}_{3}\)
12

Label the conjugate acid and base

In this reaction, the original acid is \(\mathrm{NH}_{4}^{+}\) and its conjugate base is \(\mathrm{NH}_{3}\). The original base is \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\) and its conjugate acid is \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\). (d)
13

Identify the species

We have \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) and \(\mathrm{OH}^{-}\) in the reaction.
14

Identify the acid and base

The \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) is the acid, while the \(\mathrm{OH}^{-}\) is the base.
15

Show the proton transfer using curved arrows

The proton transfer can be shown as: \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{CH}_{3} \mathrm{NH}_{2}+\mathrm{H}_{2}\mathrm{O}\)
16

Label the conjugate acid and base

In this reaction, the original acid is \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) and its conjugate base is \(\mathrm{CH}_{3} \mathrm{NH}_{2}\). The original base is \(\mathrm{OH}^{-}\) and its conjugate acid is \(\mathrm{H}_{2}\mathrm{O}\).

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Most popular questions from this chapter

Write an equation for the acid-base reaction between 2,4-pentanedione and sodium ethoxide, and calculate its equilibrium constant, \(K_{\text {eq. }}\). The \(\mathrm{p} K_{\mathrm{a}}\) of 2,4 -pentanedione is 9 ; that of ethanol is \(15.9\). 2,4-Pentanedione Sodium ethoxide

Following is a structural formula for guanidine, the compound by which migratory birds excrete excess metabolic nitrogen. The hydrochloride salt of this compound is a white crystalline powder, freely soluble in water and ethanol. (a) Write a Lewis structure for guanidine showing all valence electrons. (b) Does proton transfer to guanidine occur preferentially to one of its \(-\mathrm{NH}_{2}\) groups \((\) cation A) or to its = NH group (cation B)? Explain.

For each value of \(K_{\mathrm{a}}\), calculate the corresponding value of \(\mathrm{p} K_{\mathrm{a}}\). Which compound is the stronger acid? (a) Acetic acid, \(K_{\mathrm{a}}=1.74 \times 10^{-5}\) (b) Chloroacetic acid, \(K_{\mathrm{a}}=1.38 \times 10^{-3}\)

Benzoic acid, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\left(\mathrm{p} K_{\mathrm{a}} 4.19\right)\), is only slightly soluble in water, but its sodium salt, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-} \mathrm{Na}^{+}\), is quite soluble in water. In which solution(s) will benzoic acid dissolve? (a) Aqueous \(\mathrm{NaOH}\) (b) Aqueous \(\mathrm{NaHCO}_{3}\) (c) Aqueous \(\mathrm{Na}_{2} \mathrm{CO}_{3}\)

What is the strongest base that can exist in liquid ammonia as a solvent?
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