Chapter 15, Problem 122QRT

(a)

Interpretation Introduction

Interpretation:

The $\text{pH}$ of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ solution has to be calculated.

Concept Introduction:

The dissociation constant of water, $K_{\text{w}}$ is the product of concentration of hydronium ion and hydroxide ion present in the solution.  In case of pure water the concentration of hydronium ion is equal to the concentration of hydroxide ions.  The $\text{pH}$ of a solution is measure of hydronium ion present in the solution.  The $\text{pOH}$ of a solution is measure of hydroxide ions present in a solution.

(b)

Interpretation Introduction

Interpretation:

The $K_{\text{sp}}$ of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ has to be calculated.  The reason as to why there is a difference in the calculated and theoretical $K_{\text{sp}}$ values has to be stated.

Concept Introduction:

Solubility product relates the solubility of a salt with the concentration of ions present in the salt.  Solubility product holds a direct relation with the solubility of the salt.  The solubility product is the ability of the solid to dissolve in aqueous solution.  The more the solubility product the more the solid dissolves in solution.  It is denoted as $K_{\text{sp}}$.  It is known as solubility product constant.