Chapter 16, Problem 16.59QP

Interpretation Introduction

Interpretation:

The $\text{pH}$ value of saturated zinc hydroxide ${\text{Zn(OH)}}_{\text{2}}$ solution has to be calculated.

Concept introduction:

$\text{pH}$: The concentration of hydrogen ion is measured using $\text{pH}$ scale. The $\text{pH}$ of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

$\text{pOH}$: It is the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{\text{-}}\text{]}$ concentration.

$\text{pOH}\text{=}{\text{-log[OH}}^{\text{-}}\text{]}$

Relationship between $\text{pH}$ and $\text{pOH}$ is that $\text{pH}\text{+}\text{pOH}\text{=}\text{14}$.

Acid dissociation constant ${\text{K}}_{\text{a}}$ represents how strong the acid is in a solution. ${\text{pK}}_{\text{a}}$ is defined as negative logarithm of acid dissociation constant(${\text{K}}_{\text{a}}$).

$p{K}_a=-\log K_a$

The strength of acid decreases as the value of $p{K}_a$ increases

$p{K}_a$ represents the chance of losing proton from a compound.

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 its coefficients.

For ionic compound ${\text{A}}_{\text{3}}\text{B}$, ${\text{K}}_{\text{sp}}$ is denoted as ${\left[\text{A}\right]}^{\text{3}}\left[\text{B}\right]$.