Write an ionic equation for the reaction of acetic acid with each of the following, and specify whether the equilibrium favors starting materials or products. What is the value of K for each?
(a) Sodium ethoxide
(b) Potassium tert-butoxide
(c) Sodium bromide
(d) Sodium acetylide
(e) Potassium nitrate
(f) Lithium amide
Sample Solution (a) This is an acid-base reaction; ethoxide ion is the base.
The position of equilibrium lies well to the right. Ethanol, with pKa = 16, is a much weaker acid than acetic acid (pKa = 4.7). The equilibrium constant K is 10(16−4.7) or 1011.3.
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