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Write equations for the following acid–base reactions.

Chapter 1, Problem 18P

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QUESTION:

Write equations for the following acid–base reactions. Label the conjugate acids and bases, and show any resonance stabilization. Predict whether the equilibrium favors the reactants or products. If in doubt, you can consult Appendix 4 for acids not shown in Table 1-5.

(a)   \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{NH}^{-}\)

(b)  \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{NHCH}_{3}\)

(c)  \(\mathrm{CH}_{3} \mathrm{OH}+\mathrm{H}_{2} \mathrm{SO}_{4}\)

(d)  \(\mathrm{NaOH}+\mathrm{H}_{2} \mathrm{~S}\)

(e)  \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{CH}_{3} \mathrm{O}^{-}\)

(f)  \(\mathrm{CH}_{3} \mathrm{O}^{-}+\mathrm{CH}_{3} \mathrm{COOH}\)

(g)  \(\mathrm{CH}_{3} \mathrm{SO}_{3}^{-}+\mathrm{CH}_{3} \mathrm{COOH}\)

(h)  \(\mathrm{CF}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{COO}^{-}\)

(i)  \(\mathrm{CH}_{3} \mathrm{CHFCOOH}+\mathrm{FCH}_{2} \mathrm{CH}_{2} \mathrm{COO}^{-}\)

(j)  \(\mathrm{CF}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}+\mathrm{FCH}_{2} \mathrm{CH}_{2} \mathrm{OH}\)

Equation Transcription:

Text Transcription:

CH_3CH_2OH+CH_3NH-

CH_3CH_2COOH+CH_3NHCH_3

CH_3OH+H_2SO_4

NaOH+H_2S

CH_3NH_3++CH_3O-

CH_3O-+CH_3COOH

CH_3SO_3-+CH_3COOH

CF_3COOH+CH_3COO-

CH_3CHFCOOH+FCH_2CH_2COO-

CF_3CH_2O-+FCH_2CH_2OH

Questions & Answers

QUESTION:

Write equations for the following acid–base reactions. Label the conjugate acids and bases, and show any resonance stabilization. Predict whether the equilibrium favors the reactants or products. If in doubt, you can consult Appendix 4 for acids not shown in Table 1-5.

(a)   \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{NH}^{-}\)

(b)  \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{NHCH}_{3}\)

(c)  \(\mathrm{CH}_{3} \mathrm{OH}+\mathrm{H}_{2} \mathrm{SO}_{4}\)

(d)  \(\mathrm{NaOH}+\mathrm{H}_{2} \mathrm{~S}\)

(e)  \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{CH}_{3} \mathrm{O}^{-}\)

(f)  \(\mathrm{CH}_{3} \mathrm{O}^{-}+\mathrm{CH}_{3} \mathrm{COOH}\)

(g)  \(\mathrm{CH}_{3} \mathrm{SO}_{3}^{-}+\mathrm{CH}_{3} \mathrm{COOH}\)

(h)  \(\mathrm{CF}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{COO}^{-}\)

(i)  \(\mathrm{CH}_{3} \mathrm{CHFCOOH}+\mathrm{FCH}_{2} \mathrm{CH}_{2} \mathrm{COO}^{-}\)

(j)  \(\mathrm{CF}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}+\mathrm{FCH}_{2} \mathrm{CH}_{2} \mathrm{OH}\)

Equation Transcription:

Text Transcription:

CH_3CH_2OH+CH_3NH-

CH_3CH_2COOH+CH_3NHCH_3

CH_3OH+H_2SO_4

NaOH+H_2S

CH_3NH_3++CH_3O-

CH_3O-+CH_3COOH

CH_3SO_3-+CH_3COOH

CF_3COOH+CH_3COO-

CH_3CHFCOOH+FCH_2CH_2COO-

CF_3CH_2O-+FCH_2CH_2OH

ANSWER:

Solution 18P :

Step 1:

A resonance form is another way of drawing a Lewis dot structure for a compound when there is more than one possibility of placing valence or lone pairs of electrons, but the atoms in the resonance forms should have identical position. Equivalent Lewis structures of same compound are called resonance forms.

The arrows in the diagrams below shows the movement of the electrons.

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