Chapter 17, Problem 108AP

Interpretation Introduction

(a)

Interpretation:

The balanced chemical equation, along with its expression for ${\text{K}}_{\text{sp}}$, which describes the dissolving of the given sparingly metal hydroxide in water are to be stated.

Concept Introduction:

The chemical equilibrium is the state in which the rates of both forward and backward reactions become equal. The concentration of both reactants and products do not change on reaching an equilibrium state.

The general chemical equation is shown below.

$\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$

The general equilibrium expression for a reaction is shown below.

$\text{K}=\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$.

Answer to Problem 108AP

A balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of $\text{Cu}{\left(\text{OH}\right)}_{\text{2}}\left(\text{s}\right)$ in water have been rightfully stated.

Explanation of Solution

The given metal hydroxide is $\text{Cu}{\left(\text{OH}\right)}_{\text{2}}\left(\text{s}\right)$.

The balanced chemical equation of $\text{Cu}{\left(\text{OH}\right)}_{\text{2}}\left(\text{s}\right)$ that describes its dissolution in water is shown below.

$\text{Cu}{\left(\text{OH}\right)}_{\text{2}}\left(\text{s}\right)\rightleftharpoons {\text{Cu}}^{2+}\left(\text{a}\text{q}\right)+2{\text{OH}}^{-}\left(\text{a}\text{q}\right)$

The substances that are present in a solid state are not written in the equilibrium expression.

The expression of ${\text{K}}_{\text{sp}}$ for the above chemical equation is shown below.

${\text{K}}_{\text{sp}}=\left[{\text{Cu}}^{2+}\right]{\left[{\text{OH}}^{-}\right]}^2$

Therefore, a balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given metal hydroxide in water have been rightfully stated.

Interpretation Introduction

(b)

Interpretation:

The balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given sparingly metal hydroxide in water are to be stated.

Concept Introduction:

The chemical equilibrium is the state in which the rates of both forward and backward reactions become equal. The concentration of both reactants and products do not change on reaching an equilibrium state.

The general chemical equation is shown below.

$\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$

The general equilibrium expression for a reaction is shown below.

$\text{K}=\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$.

Answer to Problem 108AP

A balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of $\text{Cr}{\left(\text{OH}\right)}_3\left(\text{s}\right)$ in water have been rightfully stated.

Explanation of Solution

The given metal hydroxide is $\text{Cr}{\left(\text{OH}\right)}_3\left(\text{s}\right)$.

The balanced chemical equation of $\text{Cr}{\left(\text{OH}\right)}_3\left(\text{s}\right)$ that describes its dissolution in water is shown below.

$\text{Cr}{\left(\text{OH}\right)}_3\left(\text{s}\right)\rightleftharpoons {\text{Cr}}^{3+}\left(\text{a}\text{q}\right)+3{\text{OH}}^{-}\left(\text{a}\text{q}\right)$

The substances that are present in a solid state are not written in the equilibrium expression.

The expression of ${\text{K}}_{\text{sp}}$ for the above chemical equation is shown below.

${\text{K}}_{\text{sp}}=\left[{\text{Cr}}^{3+}\right]{\left[{\text{OH}}^{-}\right]}^3$

Therefore, a balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given metal hydroxide in water have been rightfully stated.

Interpretation Introduction

(c)

Interpretation:

The balanced chemical equation, along with its expression for ${\text{K}}_{\text{sp}}$, which describes the dissolving of the given sparingly metal hydroxide in water are to be stated.

Concept Introduction:

The chemical equilibrium is the state in which the rates of both forward and backward reactions become equal. The concentration of both reactants and products do not change on reaching an equilibrium state.

The general chemical equation is shown below.

$\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$

The general equilibrium expression for a reaction is shown below.

$\text{K}=\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$.

Answer to Problem 108AP

A balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of ${\text{BaOH}}_2\left(\text{s}\right)$ in water have been rightfully stated.

Explanation of Solution

The given metal hydroxide is ${\text{BaOH}}_2\left(\text{s}\right)$.

The balanced chemical equation of ${\text{BaOH}}_2\left(\text{s}\right)$ that describes its dissolution in water is shown below.

${\text{BaOH}}_2\left(\text{s}\right)\rightleftharpoons {\text{Ba}}^{2+}\left(\text{a}\text{q}\right)+2{\text{OH}}^{-}\left(\text{a}\text{q}\right)$

The substances that are present in a solid state are not written in the equilibrium expression.

The expression of ${\text{K}}_{\text{sp}}$ for the above chemical equation is shown below.

${\text{K}}_{\text{sp}}=\left[{\text{Ba}}^{2+}\right]{\left[{\text{OH}}^{-}\right]}^2$

Therefore, a balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given metal hydroxide in water have been rightfully stated.

Interpretation Introduction

(d)

Interpretation:

The balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given sparingly metal hydroxide in water are to be stated.

Concept Introduction:

The chemical equilibrium is the state in which the rates of both forward and backward reactions become equal. The concentration of both reactants and products do not change on reaching an equilibrium state.

The general chemical equation is shown below.

$\text{aA}+\text{bB}\rightleftharpoons \text{cC}+\text{dD}$

The general equilibrium expression for a reaction is shown below.

$\text{K}=\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$.

Answer to Problem 108AP

A balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of $\text{Sn}{\left(\text{OH}\right)}_2\left(\text{s}\right)$ in water have been rightfully stated.

Explanation of Solution

The given metal hydroxide is $\text{Sn}{\left(\text{OH}\right)}_2\left(\text{s}\right)$.

The balanced chemical equation of $\text{Sn}{\left(\text{OH}\right)}_2\left(\text{s}\right)$ that describes its dissolution in water is shown below.

$\text{Sn}{\left(\text{OH}\right)}_2\left(\text{s}\right)\rightleftharpoons {\text{Sn}}^{2+}\left(\text{a}\text{q}\right)+2{\text{OH}}^{-}\left(\text{a}\text{q}\right)$

The substances that are present in a solid state are not written in the equilibrium expression.

The expression of ${\text{K}}_{\text{sp}}$ for the above chemical equation is shown below.

${\text{K}}_{\text{sp}}=\left[{\text{Sn}}^{2+}\right]{\left[{\text{OH}}^{-}\right]}^2$

Therefore, a balanced chemical equation along with its expression for ${\text{K}}_{\text{sp}}$ which describes the dissolving of the given metal hydroxide in water have been rightfully stated.