Chapter 14, Problem 121CP

a.

Interpretation Introduction

Interpretation: The [H₃O]⁺ of 0.05 M KOH should be determined.

Concept Introduction :

The water dissociation expression, K_wis given as:

  $K_w={\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}{\text{][OH}}^{\text{-}}\text{]}$

Where square brackets indicate concentration.

The value of K_w is $1\times {10}^{-14}$ .

b.

Interpretation Introduction

Interpretation: The pH of the 0.05 M KOH should be determined.

Concept Introduction :

• pH stands for "potential of hydrogen", it is a measure of alkalinity or acidity of water-soluble substances. pH number ranges from 0 to 14.
• pH is a logarithmic scale which specify the acidity or basicity of the solution.

  $pH=-\log [H^{+}]$

pOH = -log [OH]^-

pH + pOH = 14

c.

Interpretation Introduction

Interpretation: The pOH of the 0.05 M KOH should be determined.

Concept Introduction :

• pH stands for "potential of hydrogen", it is a measure of alkalinity or acidity of water-soluble substances. pH number ranges from 0 to 14.
• pH is a logarithmic scale which specify the acidity or basicity of the solution.

  $pH=-\log [H^{+}]$

pOH = -log [OH]^-

pH + pOH = 14

d.

Interpretation Introduction

Interpretation:

The balanced chemical equation for the KOH with H₂SO₄ should be determined.

Concept Introduction:

The balanced reaction is that chemical reaction in which the number of atoms of each element in the product side and on reactant side are equal.

e.

Interpretation Introduction

Interpretation: The volume of KOH solution should be determined.

Concept Introduction :

A laboratory procedure said to be titration is used in which an acid sample is neutralized with a known amount of base and by using indicator in order to determine the end-point (generally determined by color change).

Using dilution law:

  ${\text{Molarity}}_{\text{acid}}\times {\text{Volume}}_{\text{acid}}\text{=}{\text{Molarity}}_{\text{base}}\times {\text{Volume}}_{\text{base}}$