   Chapter 16, Problem 104GQ

Chapter
Section
Textbook Problem

The equilibrium constant for the reaction of hydrochloric acid and ammonia is 1.8 × 109 (page 726). Confirm this value.

Interpretation Introduction

Interpretation:

The equilibrium constant of the reaction is 1.8×109 has to be proved.

Concept introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Explanation

Hydrochloric acid reacts with water to form H3O+. It reacts with NH3 to form NH4+. The conjugate acid of NH3 and H2O.

Let’s write the equilibrium chemical reaction between NH3 and H3O+

H3O+(aq)+NH3(aq)NH4+(aq)+H2O(l)

Equilibrium expression:

K= [NH4+][NH3][H3O+]= 1.8×109                             (1)

H2O(l)H3O+(aq)+OH-(aq)Kw= [H3O+][OH-] = 1×10-14                     �

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