Acetic acid Bronsted-Lowry theory

We saw in Section J that a salt is produced by the neutralization of an acid by a base. However, if we measure the pH of a solution of a salt, we do not in general find the neutral value (pH = 7). For instance, if we neutralize 0.3 M CHjCOOH(aq) with 0.3 M NaOH(aq), the resulting solution of sodium acetate has pH = 9.0. How can this be The Bronsted-Lowry theory provides the explanation. According to this theory, an ion may be an acid or a base. The acetate ion, for instance, is a base, and the ammonium ion is an acid. The pH of a solution of a salt depends on the relative acidity and basicity of its ions. 

The Bronsted-Lowry theory provides the answer. According to this theory, an ion may be an acid or a base. The acetate ion, for instance, is a base, and the ammonium ion is an acid. Therefore, it is hardly surprising that a solution of a salt is acidic or basic. 

The Bronsted-Lowry theory includes water as a reactant and considers its acidity or basicity in the reaction. In the partial ionization of acetic acid, water is a base because it accepts the hydrogen ion to form hydro-nium ion. 

The Bronsted-Lowry theory expands on this notion beyond solvents of just water, to cover others such as liquid ammonia, glacial acetic acid, anhydrous sulfuric acid, and all solvents containing hydrogen. Bases can accept protons but don t necessarily contain OH. ... 

To estimate the pH of the solution, we proceed in exactly the Scune way as for the addition of a conventioncd acid or base, for in the Bronsted-Lowry theory there is no distinction between conventional acids such is acetic add cUid the conjugate acids of bases (such asNHJ). 

The Bronsted-Lowry theory can be applied to acid-base reactions in nonaqueous solvents, where the relative strengths of acids and bases can differ from what they are in aqueous solutions. Indicate whether each of the following would be an acid, a base, or amphiprotic in pure liquid acetic acid, CH3COOH, as a solvent, (a) CHsCOO" (b) H2O (c) CH3COOH (d) HCIO4. [Hint Refer to Table 16.2.]... 

In the Bronsted—Lowry acid—base theory, there is competition for an H+. Consider the acid—base reaction between acetic acid, a weak acid, and ammonia, a weak base ... 

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