Chapter 17, Problem 17.89QP

Interpretation Introduction

Interpretation:

The concentration of hydroxide ion needs to reduce the concentration of magnesium in ${\text{Mg(NO}}_{\text{3}}{\text{)}}_{\text{2}}$ to $\text{1}\text{.0 ×}{\text{10}}^{\text{-10}}\text{M}$ has to be calculated.

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 required concentration of hydroxide ion