Chapter 16.7, Problem 16.16E

(a)

Interpretation Introduction

Interpretation:

The pH of the given points of the titration of ammonia with hydrochloric acid has to be calculated.

Before the addition on any $\text{HCl}$

Concept Introduction:

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{-}\text{]}$ concentration.

$\text{pOH}\text{=}{\text{-log[OH}}^{-}\text{]}$

Relationship between pH  and pOH:

$\text{pH + pOH = 14}$

(b)

Interpretation Introduction

Interpretation:

The pH of the given points of the titration of ammonia with hydrochloric acid has to be calculated.

Halfway to the equivalence point

Concept Introduction:

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{-}\text{]}$ concentration.

$\text{pOH}\text{=}{\text{-log[OH}}^{-}\text{]}$

Relationship between pH  and pOH:

$\text{pH + pOH = 14}$

(c)

Interpretation Introduction

Interpretation:

The pH of the given points of the titration of ammonia with hydrochloric acid has to be calculated.

At the equivalence point

Concept Introduction:

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{-}\text{]}$ concentration.

$\text{pOH}\text{=}{\text{-log[OH}}^{-}\text{]}$

Relationship between pH  and pOH:

$\text{pH + pOH = 14}$

(d)

Interpretation Introduction

Interpretation:

The pH of the given points of the titration of ammonia with hydrochloric acid has to be calculated.

After the addition of 175 mL of 0.100 M $\text{HCl}$

Concept Introduction:

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{-}\text{]}$ concentration.

$\text{pOH}\text{=}{\text{-log[OH}}^{-}\text{]}$

Relationship between pH  and pOH:

$\text{pH + pOH = 14}$