Chapter 18, Problem 86E

Interpretation Introduction

(a)

Interpretation:

The equilibrium equation for the solubility product of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ is to be stated.

Concept introduction:

Solubility product constant ${\text{K}}_{\text{sp}}$ is the equilibrium constant for compounds with low solubility. The ${\text{K}}_{\text{sp}}$ expression depends only upon the products since the species on the left hand side of the equilibrium expression is solid.

Interpretation Introduction

(b)

Interpretation:

The substances which reduces and increases the solubility of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ are to be stated.

Concept introduction:

The solubility of the compounds can be altered by adding an acid or a base which changes the concentration of one of the product species. According to Le Chatelier’s Principle, the equilibrium will shift in the direction to counteract the change in the equilibrium expression.

Interpretation Introduction

(c)

Interpretation:

The class of substances that increases and reduces the $\left[{\text{OH}}^{-}\right]$ are to be stated.

Concept introduction:

The solubility of the compounds can be altered by adding an acid or a base which changes the concentration of one of the product species. According to Le Chatelier’s Principle, the equilibrium will shift in the direction that will use the increased concentration of the added species.