Chapter 7, Problem 37E

(a)

Interpretation Introduction

Interpretation:

The [H⁺] and [OH^-] in pure water at 40 ⁰C should be calculated.

Concept Introduction :

The ionization constant of water is represented as follows:

  $K_w=\left[{\text{H}}_3{\text{O}}^{+}\right]\left[{\text{OH}}^{-}\right]$

The pH of solution is represented as follows:

  $\text{pH = }-\log \left[{\text{H}}_3{\text{O}}^{+}\right]$

(b)

Interpretation Introduction

Interpretation:

The pH of water at 40 ⁰C should be determined.

Concept Introduction :

The pH of solution is represented as follows:

  $\text{pH = }-\log \left[{\text{H}}_3{\text{O}}^{+}\right]$

(c)

Interpretation Introduction

Interpretation:

If the hydroxide ion concentration in a solution is 0.10 M, the pH at 40 ⁰C should be calculated.

Concept Introduction :

The ionization constant of water is represented as follows:

  $K_w=\left[{\text{H}}_3{\text{O}}^{+}\right]\left[{\text{OH}}^{-}\right]$

The pH of solution is represented as follows:

  $\text{pH = }-\log \left[{\text{H}}_3{\text{O}}^{+}\right]$