   Chapter 16.10, Problem 2.2ACP

Chapter
Section
Textbook Problem

Other solvents also undergo autoionization. (a) Write a chemical equation for the autoionization of glacial acetic acid. (b) The equilibrium constant for the autoionization of glacial acetic acid is 32 × 10−15 at 25°C. Determine the concentration of [CH3CO2H2]+ in acetic acid at 25°C.

(a)

Interpretation Introduction

Interpretation: The chemical equation for the autoionization of glacial acetic acid should be writtern.

Concept introduction:

Pure acetic acid is known as glacial acetic acid. It is similar to water that it can both act as an acid and a base. It is a weak acid or base that it can not completely dissociate in a solution.

An equilibrium constant (K) is the ratio of the concentration of products and reactants raised to appropriate stoichiometric coefficient at equilibrium. The self-ionization reaction of an acid HA is written as,

HA(aq)H+(aq)+A(aq)

The relative strength of an acid and base in solution can be also expressed quantitatively with an equilibrium constant as follows:

Ka=[H+][A][HA]

The autoionization constant (K) of an acid is written as,

Ka=[H+][A][HA]Ka([HA])=[H+][A]K=[H+][A]                                                                                                (1)

Explanation

Pure acetic acid is known as glacial acetic acid. It is similar to water that it can both act as an acid and a base. It is a weak acid or base that it can not completely dissociate in a solution.

The chemical equation for the autoionization of glacial acetic acid is written as,

2CH3

(b)

Interpretation Introduction

Interpretation:

The concentration of CH3COOH2+ in acetic acid at 25°C has to be calculated.

Concept Introduction:

Pure acetic acid is known as glacial acetic acid. It is similar to water that it can both act as an acid and a base. It is a weak acid or base that it can not completely dissociate in a solution.

An equilibrium constant (K) is the ratio of the concentration of products and reactants raised to appropriate stoichiometric coefficient at equilibrium.

The self-ionization reaction of an acid HA is written as,

HA(aq)H+(aq)+A(aq)

The relative strength of an acid and base in solution can be also expressed quantitatively with an equilibrium constant as follows:

Ka=[H+][A][HA]

The autoionization constant (K) of an acid is written as,

Ka=[H+][A][HA]Ka([HA])=[H+][A]K=[H+][A]                                                                                               (1)

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