Chapter 17, Problem 17.122SP

Interpretation Introduction

(a)

Interpretation:

The net reaction of dissolution of $\text{Zn}{\left(\text{OH}\right)}_2$ should be given. The equilibrium constant of $\text{Zn}{\left(\text{OH}\right)}_2$ to form ${\left[\text{Zn}{\left(\text{OH}\right)}_4\right]}^2{}^{-}$ 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 denoted by $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ is 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:

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

A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $\left(K_{\text{f}}\right)$.

The relation between $K_{\text{f}}$, $K_{\text{sp}}$ and $K$ is as follows:

$K=K_{\text{f}}\cdot K_{\text{sp}}$

Interpretation Introduction

(b)

Interpretation:

The net reaction of dissolution of $\text{Cu}{\left(\text{OH}\right)}_2$ should be given. The equilibrium constant of $\text{Cu}{\left(\text{OH}\right)}_2$ to form ${\left[\text{Cu}{\left({\text{NH}}_3\right)}_4\right]}^{2+}$ 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 denoted by $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ is 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:

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

A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $\left(K_{\text{f}}\right)$.

The relation between $K_{\text{f}}$, $K_{\text{sp}}$ and $K$ is as follows:

$K=K_{\text{f}}\cdot K_{\text{sp}}$

Interpretation Introduction

(c)

Interpretation:

The net reaction of dissolution of $\text{AgBr}$ should be given. The equilibrium constant of $\text{AgBr}$ to form ${\left[\text{Ag}{\left({\text{NH}}_3\right)}_2\right]}^{+}$ 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 denoted by $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ is 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:

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

A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant $\left(K_{\text{f}}\right)$.

The relation between $K_{\text{f}}$, $K_{\text{sp}}$ and $K$ is as follows:

$K=K_{\text{f}}\cdot K_{\text{sp}}$