Chapter 18, Problem 9E

Interpretation Introduction

Interpretation:

The number of milligrams of magnesium palmitate that would precipitate from $965\text{ mL}$ solution of magnesium palmitate should be calculated.

Concept introduction:

Solubility product constant $\left(K_{\text{sp}}\right)$ is also an equilibrium constant, and is calculated as the product of the equilibrium concentration of the ions present in the salt raised to the power of their coefficients respectively in the balanced chemical equation.

For a general salt ${\text{A}}_{\text{x}}{\text{B}}_{\text{y}}$, the balanced chemical reaction for its equilibrium is given as,

${\text{A}}_x{\text{B}}_y\left(s\right)\rightleftharpoons x{\text{A}}^{y+}\left(aq\right)+y{\text{B}}^{-x}\left(aq\right)$

The expression of the solubility product is written as follows:

$K_{\text{sp}}={\left[{\text{A}}^{y+}\right]}^x{\left[{\text{B}}^{-x}\right]}^y$

The conversion factor to convert $\text{g}$ to $\text{mg}$ is,

$1\text{ mg}={\text{10}}^{-3}\text{ g}$

The conversion factor to convert $\text{mL}$ to $\text{L}$ is,

$1\text{ mL}={\text{10}}^{-3}\text{ L}$