Chapter 17, Problem 17.112SP

Interpretation Introduction

(a)

Interpretation:

The molar solubility of ${\text{SrF}}_2$ in $0.010M$

$\text{Sr}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denotedby $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ an ionic compound. Its dissociation occurs as:

${\text{A}}_x{\text{B}}_y\rightleftharpoons x{\text{A}}^{y+}+y{\text{A}}^{x-}$

The expression for its $K_{\text{sp}}$ is as follows:

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

Interpretation Introduction

(b)

Interpretation:

The molar solubility of ${\text{SrF}}_2$ in $0.010M$

$\text{NaF}$ is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denotedby $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ an ionic compound. Its dissociation occurs as:

${\text{A}}_x{\text{B}}_y\rightleftharpoons x{\text{A}}^{y+}+y{\text{A}}^{x-}$

The expression for its $K_{\text{sp}}$ is as follows:

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