Chapter 17, Problem 17.83QP

Interpretation Introduction

Interpretation:

The $\text{pH}$ at which ${\text{Fe(OH)}}_{\text{3}}$ can precipitate out has to be determined.

Concept introduction:

• The solubility product constant ( ${\text{K}}_{\text{sp}}$) is defined as the equilibrium between compound and its ions in an aqueous solution.
• Solubility product is the multiplication of concentration of dissolved ion,  raised to the power of coefficients.
• Ionic compound ${\text{A}}_{\text{3}}\text{B}$ ${\text{K}}_{\text{sp}}\text{=}{\left[\text{A}\right]}^{\text{3}}\left[\text{B}\right]$

To calculate: The $\text{pH}$ of $\text{0}{\text{.010 M Fe}}^{\text{3+}}\text{ion}$ , $\text{0}{\text{.010 M Zn}}^{\text{2+}}\text{ion}$ and predict the $\text{pH}$ at which ${\text{Fe(OH)}}_{\text{3}}$ precipitate.