Write an ionic equation for the reaction of acetic acid with...

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:
(a) Sodium ethoxide
(b) Potassium tert-butoxide
(c) Sodium bromide
(d) Sodium acetylide
(e) Potassium nitrate
(f) Lithium amide

Key Concepts

Bronsted-Lowry Acid-Base Reactions

This concept involves the transfer of a proton from an acid to a base. In any reaction involving acetic acid and a base, acetic acid acts as a proton donor, while the base accepts a proton to form its conjugate acid. This proton transfer is central to understanding the mechanism of the reaction.

Ionic Equations

Ionic equations are used to represent chemical reactions by focusing only on the species that undergo change, omitting spectator ions. In acid-base reactions, these equations neatly capture the net change occurring during the deprotonation process.

Reaction Equilibrium and Le Châtelier's Principle

This concept explains how the position of equilibrium in acid-base reactions is determined by the relative strengths of the acids and bases involved. When acetic acid reacts with a base, whether the equilibrium favors the reactants or products depends on how strongly the base deprotonates the acid and the relative stability of the resulting conjugate pairs.

Relative Strength of Bases

The strength of a base is crucial in determining both the extent of deprotonation and the position of the equilibrium. Strong bases efficiently remove a proton from acetic acid, pushing the equilibrium towards the formation of products, whereas weak bases may not effectively deprotonate the acid, leaving the equilibrium largely in favor of the starting materials.

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