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Solutions for Introduction and Review O HCH3CH2 CH3 N H H NCH3 CH3CH3CH2 C O H O CH3CH2 O N CH3CH3 H H N HCH3 H CH3CH2 C O O CH3CH2 C O O 17 In Solved Problem 4, the structure of methylamine is shown to be similar to ammonia. It is reasonable to infer that their acid-base properties are also similar. (a) This problem can be viewed in two ways. 1) Quantitatively, the pKa values determine the order of acidity. 2) Qualitatively, the stabilities of the conjugate bases determine the order of acidity (see Solved Problem 4 for structures): the conjugate base of acetic acid, acetate ion, is resonance- stabilized, so acetic acid is the most acidic; the conjugate base of ethanol has a negative charge on a very electronegative oxygen atom; the conjugate base of methylamine has a negative charge on a mildly electronegative nitrogen atom and is therefore the least stabilized, so methylamine is the least acidic. (The first two pK values are from text Table 5.)a acetic acid > ethanol > methylamine pKa 4.74 pKa 15.9 pKa ≈ 40 (from text Appendix 4) strongest acid weakest acid (b) Ethoxide ion is the conjugate base of ethanol, so it must be a stronger base than ethanol; Solved Problem 4 and text Table 5 indicate ethoxide is analogous to hydroxide in base strength. Methylamine has pKb 3.36. The basicity of methylamine is between the basicity of ethoxide ion and ethanol. ethoxide ion > methylamine > ethanol strongest base weakest base 18 Curved arrows show electron movement, as described in text Section 14. + conjugate base (a) (b) + + + conjugate base conjugate acid conjugate acid stronger acid stronger base weaker base weaker acidequilibrium favors PRODUCTS stronger acid stronger base weaker acid weaker base equilibrium favors PRODUCTS O HCH3 O S SO O O O O OS O O O OO O S O O O H H O HCH3 H H HH (c) conjugate base, weaker base conjugate acidstronger base weaker acid equilibrium favors PRODUCTS stronger acid + + more stable anion— negative charge on the more electronegative atom resonance stabilized resonance stabilized 14