Chapter 8, Problem 8.66P

Use the solubility rules listed in Section 8.3B to predict whether each of the following ionic compounds is soluble in water.

1. ${\text{Al(NO}}_{\text{3}}{)}_3$

${\text{NaHCO}}_{\text{3}}$

${\text{Cr(OH)}}_{\text{2}}$

$\text{LiOH}$

${\text{CuCO}}_3$

${{\text{(NH}}_{\text{4}}\text{)}}_{\text{2}}{\text{SO}}_{\text{4}}$

${\text{Fe(NO)}}_3$

${{\text{(NH}}_{\text{4}}\text{)}}_{\text{3}}{\text{PO}}_{\text{4}}$

Interpretation Introduction

(a)

Interpretation:

Whether $\text{Al}{\left({\text{NO}}_3\right)}_2$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like. This means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  $\text{Al}{\left({\text{NO}}_3\right)}_2$ is soluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

Since $\text{Al}{\left({\text{NO}}_3\right)}_2$ contains ${\text{Al}}^{3+}$ cation and ${\text{NO}}_3{}^{-}$ anion. Although ${\text{Al}}^{3+}$ salts are not soluble however the salts that contain ${\text{NO}}_3{}^{-}$ anion are water-soluble as per the solubility rules and therefore $\text{Al}{\left({\text{NO}}_3\right)}_2$ is water-soluble.

Interpretation Introduction

(b)

Interpretation:

Whether ${\text{NaHCO}}_{\text{3}}$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  ${\text{NaHCO}}_{\text{3}}$ issoluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

Since ${\text{NaHCO}}_{\text{3}}$ contains ${\text{Na}}^{+}$ cation and ${\text{HCO}}_{\text{3}}{}^{-}$ anion. All sodium salts are soluble as ${\text{Na}}^{+}$ belong to the category of group IA cations and therefore ${\text{NaHCO}}_{\text{3}}$ is water-soluble.

Interpretation Introduction

(c)

Interpretation:

Whether $\mathrm{Cr}{\left(OH\right)}_2$ is soluble in water or not should to be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  $\mathrm{Cr}{\left(OH\right)}_2$ isinsoluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

Since ${\mathrm{Cr}}^{2+}$ do not belong to the category of group IA cations and further the hydroxides anions are water insoluble so it is not soluble in water.

Interpretation Introduction

(d)

Interpretation:

Whether $\text{LiOH}$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  $\text{LiOH}$ is soluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

Since $\text{LiOH}$ contains ${\text{Li}}^{+}$ ion that belongs to group IA cations and as all lithium salts are soluble. In addition to this iodides are also soluble hence $\text{LiOH}$ is soluble in water.

Interpretation Introduction

(e)

Interpretation:

Whether ${\text{CuCO}}_3$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  ${\text{CuCO}}_3$ isinsoluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

The ionic compound ${\text{CuCO}}_3$ reacts with water as follows:

  ${\text{CuCO}}_3\left(s\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)\to {\text{Cu}}_3{\left({\text{CO}}_3\right)}_2{\left(\text{OH}\right)}_2\left(s\right)+{\text{CO}}_2\left(g\right)$

Since ${\text{CuCO}}_3$ contains ${\text{Cu}}^{2+}$ cation and ${\text{CO}}_3{}^{2-}$ anion. ${\text{Cu}}^{2+}$ salts are not soluble and in addition the salts that contain ${\text{CO}}_3{}^{2-}$ anion are water-insoluble as per the solubility rules and therefore ${\text{CuCO}}_3$ is water-insoluble.

Interpretation Introduction

(f)

Interpretation:

Whether ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{SO}}_4$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{SO}}_4$ is soluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

  ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{SO}}_4$ is soluble in waterbecause ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{SO}}_4$ contains ${\text{NH}}_{\text{4}}{}^{+}$ cation and ${\text{SO}}_4{}^{2-}$ anion. All salts of ${\text{NH}}_{\text{4}}{}^{+}$ are water-soluble.Further the sulphates anion present along with ${\text{NH}}_{\text{4}}{}^{+}$ and therefore ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{SO}}_4$ is water-soluble.

Interpretation Introduction

(g)

Interpretation:

Whether $\text{Fe}{\left(\text{OH}\right)}_3$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  $\text{Fe}{\left(\text{OH}\right)}_3$ is insoluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

Since $\text{Fe}{\left(\text{OH}\right)}_3$ contains ${\text{Fe}}^{3+}$ cation and ${\text{OH}}^{-}$ anion. ${\text{Fe}}^{3+}$ cation does not belong to group IA cations, and the salts that contain ${\text{OH}}^{-}$ anion are water-soluble and therefore $\text{Fe}{\left(\text{OH}\right)}_3$ is water-insoluble.

Interpretation Introduction

(h)

Interpretation:

Whether ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{PO}}_4$ is soluble in water or not should be identified.

Concept introduction:

The criteria to determine the solubility of a given solute in a particular solvent is governed by the principle of like dissolves like which means that the polar solvents such as water and alcohols tend to dissolve polar compounds while the non-polar solvents like hexane and urea dissolve covalent or non-polar compounds. Several forces are responsible for solubility of various compounds. For example, the sodium chloride solution is held by electrostatic forces of interaction. Polar molecules such as ethanol that are uncharged dissolved in water via hydrogen bonding interactions.

Water is a polar solvent as it contains highly electronegative oxygen atom and electropositive hydrogen atoms. Therefore the ionic solids and some polar molecules which are relatively small can dissolve in water.

Answer to Problem 8.66P

  ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{PO}}_4$ is soluble in water.

Explanation of Solution

The solubility of ionic solids is controlled by two basic principles as follows:

1. The compound that consists of group IA cations that include either of the ions ${\text{Li}}^{+}{\text{/Na}}^{+}{\text{/K}}^{+}{\text{/Rb}}^{+}{\text{/Cs}}^{+}$ or ${\text{NH}}_4{}^{+}$ ion is soluble in water.

2.The compound that consists of ${\text{NO}}_3{}^{-}$ , acetate, sulphate, or halides such as ${\text{Cl}}^{-}/{\text{Br}}^{-}/{\text{I}}^{-}$ are also soluble in water.

  ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{PO}}_4$ is soluble in water because ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{PO}}_4$ contains ${\text{NH}}_{\text{4}}{}^{+}$ cation and ${\text{PO}}_4{}^{3-}$ anion. All salts of ${\text{NH}}_{\text{4}}{}^{+}$ are water-soluble regardless of the anionic species present along with ${\text{NH}}_{\text{4}}{}^{+}$ and therefore ${\left({\text{NH}}_{\text{4}}\right)}_3{\text{PO}}_4$ is water-soluble.