# Chapter 16, Problem 16.124QP

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### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

#### Solutions

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### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933
Interpretation Introduction

Interpretation:

In a 0.080 M NH3 solution, what percent of the NH3 is present as NH4+ has to be calculated.

Concept Information:

Strong base and weak base:

Strong base dissociates into its constituent ions fully.  It produces more of hydroxide ions while dissolved in water.  Weak bases partially dissociates into its constituent ions.

According to Bronsted-Lowry, strong base is a good proton acceptor whereas weak base is a poor proton acceptor

Since, the ionization of a weak base is incomplete, it is treated in the same way as the ionization of a weak acid.

The ionization of a weak base B is given by the below equation.

B(aq)+H2O(l)HB+(aq)+OH-(aq)

The equilibrium expression for the ionization of weak base B will be,

Kb=[HB+][OH-][B]

Where,

Kb is base ionization constant,

[OH] is concentration of hydroxide ion

[HB+]   is concentration of conjugate acid

[B] is concentration of the base

Percent ionization:

A quantitative measure of the degree of ionization is percent ionization.

For a weak, base HB percent ionization can be calculated as follows,

percentionization=[OH-][HB]×100%

To Calculate: The percent of the NH3 is present as NH4+ in the given solution

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