Chapter 4, Problem 9QAP

Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed.

(a) copper(II) sulfate and sodium chloride

(b) manganese(II) nitrate and ammonium hydroxide

(c) silver nitrate and hydrochloric acid

(d) nickel(II) sulfate and potassium hydroxide

(e) ammonium carbonate and sodium nitrate

Interpretation Introduction

(a)

Interpretation:

The net ionic equation should be written when copper(II) sulfate and sodium chloride are mixed.

Concept introduction:

Solubility of any compound is predicted by above solubility chart.

Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.

Boxes with grey small box will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.

Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.

A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.

Answer to Problem 9QAP

No precipitation occurs.

Explanation of Solution

Copper(II) sulfate: ${\text{CuSO}}_4$

Sodium chloride: $\text{NaCl}$

Reaction for the solution of copper(II) sulfate and sodium chloride is written as:

${\text{CuSO}}_4\text{+NaCl}\to {\text{CuCl}}_2{\text{+Na}}_{\text{2}}{\text{SO}}_{\text{4}}$

Reactants:

Ions in solution: ${\text{CuSO}}_4$ : ${\text{Cu}}^{\text{2+}}$ and ${\text{SO}}_4{}^{2-}$

Ions in solution: $\text{NaCl}$ : ${\text{Na}}^{+}$ and ${\text{Cl}}^{-}$

Products:

Ions in solution: ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ : ${\text{Na}}^{+}$ and ${\text{SO}}_4{}^{2-}$

Ions in solution: ${\text{CuCl}}_2$ : ${\text{Cu}}^{\text{2+}}$ and ${\text{Cl}}^{-}$

Now, ${\text{CuCl}}_2$ and ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ both are soluble in water or in aqueous solution. Thus, no precipitation occurs.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation should be written when manganese(II) nitrate and ammonium hydroxide are mixed.

Concept introduction:

Solubility of any compound is predicted by above solubility chart.

Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.

Boxes with grey small box will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.

Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.

A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.

Answer to Problem 9QAP

Precipitation occurs

The net ionic equation is:

${\text{Mn}}^{\text{+2}}\text{(aq)}+{\text{2OH}}^{-}(\text{aq})\to {\text{Mn(OH)}}_2(\text{s})$

Explanation of Solution

Manganese(II) nitrate: ${\text{Mn(NO}}_3{)}_2$

Ammonium hydroxide: ${\text{NH}}_4\text{OH}$

Reaction for the solution of manganese(II) nitrate and ammonium hydroxide is written as:

${\text{Mn(NO}}_3{)}_2+{\text{NH}}_4\text{OH}\to {\text{NH}}_4{\text{NO}}_{\text{3}}\text{+Mn(OH}{)}_2$

Reactants:

Ions in solution: ${\text{Mn(NO}}_3{)}_2$ : ${\text{Mn}}^{\text{+2}}$ and ${\text{NO}}_{\text{3}}{}^{-}$

Ions in solution: ${\text{NH}}_4\text{OH}$ : ${\text{NH}}_4^{+}$ and ${\text{OH}}^{-}$

Products:

Ions in solution: ${\text{NH}}_4{\text{NO}}_{\text{3}}$ : ${\text{NH}}_4^{+}$ and ${\text{NO}}_{\text{3}}{}^{-}$

Ions in solution: $\text{Mn(OH}{)}_2$ : ${\text{Mn}}^{\text{+2}}$ and ${\text{OH}}^{-}$

Now, $\text{Mn(OH}{)}_2$ is solid, not soluble in water whereas ${\text{NH}}_4{\text{NO}}_{\text{3}}$ is soluble in water.

So, the equation will be:

${\text{Mn}}^{\text{+2}}{\text{(aq)+ NO}}_{\text{3}}{}^{-}(\text{aq})+{\text{NH}}_4^{+}{\text{(aq)+OH}}^{-}(\text{aq})\to {\text{Mn(OH)}}_2(\text{s}){\text{+NH}}_4^{+}{\text{(aq)+NO}}_{\text{3}}{}^{-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{NO}}_{\text{3}}{}^{\text{-}}$, ${\text{NH}}_4^{+}$), the final or net ionic equation is:

${\text{Mn}}^{\text{+2}}\text{(aq)}+{\text{2OH}}^{-}(\text{aq})\to {\text{Mn(OH)}}_2(\text{s})$

Interpretation Introduction

(c)

Interpretation:

The net ionic equation should be written when silver nitrate and hydrochloric acid are mixed.

Concept introduction:

Solubility of any compound is predicted by above solubility chart.

Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.

Boxes with grey small box will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.

Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.

A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.

Answer to Problem 9QAP

Precipitation occurs

The net ionic equation is:

${\text{Ag}}^{\text{+}}\text{(aq)}+{\text{Cl}}^{-}(\text{aq})\to \text{AgCl}(\text{s})$

Explanation of Solution

Silver nitrate: ${\text{AgNO}}_{\text{3}}$

Hydrochloric acid: $\text{HCl}$

Reaction for the solution of silver nitrate and hydrochloric acid is written as:

${\text{AgNO}}_{\text{3}}+\text{HCl}\to {\text{HNO}}_{\text{3}}\text{+AgCl}$

Reactants:

Ions in solution: ${\text{AgNO}}_{\text{3}}$ : ${\text{Ag}}^{\text{+}}$ and ${\text{NO}}_3{}^{-}$

Ions in solution: $\text{HCl}$ : ${\text{H}}^{\text{+}}$ and ${\text{Cl}}^{-}$

Products:

Ions in solution: ${\text{HNO}}_{\text{3}}$ : ${\text{H}}^{\text{+}}$ and ${\text{NO}}_3{}^{-}$

Ions in solution: $\text{AgCl}$ : ${\text{Ag}}^{\text{+}}$ and ${\text{Cl}}^{-}$

Now, $\text{AgCl}$ is solid, not soluble in water whereas ${\text{HNO}}_{\text{3}}$ is soluble in water.

So, the equation will be:

${\text{Ag}}^{\text{+}}{\text{(aq)+ NO}}_{\text{3}}{}^{-}(\text{aq})+{\text{H}}^{+}{\text{(aq)+Cl}}^{-}(\text{aq})\to \text{AgCl}(\text{s}){\text{+H}}^{+}{\text{(aq)+NO}}_3{}^{-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{NO}}_{\text{3}}{}^{\text{-}}$, ${\text{H}}^{\text{+}}$), the final or net ionic equation is:

${\text{Ag}}^{\text{+}}\text{(aq)}+{\text{Cl}}^{-}(\text{aq})\to \text{AgCl}(\text{s})$

Interpretation Introduction

(d)

Interpretation:

The net ionic equation should be written when nickel(II) sulfate and potassium hydroxide are mixed.

Concept introduction:

Solubility of any compound is predicted by above solubility chart.

Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.

Boxes with grey small box will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.

Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.

A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.

Answer to Problem 9QAP

Precipitation occurs

The net ionic equation is:

${\text{Ni}}^{\text{2+}}\text{(aq)}+2{\text{OH}}^{-}(\text{aq})\to {\text{Ni(OH)}}_2(\text{s})$

Explanation of Solution

Nickel(II) sulfate: ${\text{NiSO}}_4$

Potassium hydroxide: $\text{KOH}$

Reaction for the solution of silver nitrate and hydrochloric acid is written as:

${\text{NiSO}}_4+\text{KOH}\to {\text{Ni(OH)}}_2{\text{+K}}_{\text{2}}{\text{SO}}_{\text{4}}$

Reactants:

Ions in solution: ${\text{NiSO}}_4$ : ${\text{Ni}}^{\text{2+}}$ and ${\text{SO}}_4{}^{2-}$

Ions in solution: $\text{KOH}$ : ${\text{K}}^{\text{+}}$ and ${\text{OH}}^{-}$

Products:

Ions in solution: ${\text{Ni(OH)}}_2$ : ${\text{Ni}}^{\text{2+}}$ and ${\text{OH}}^{-}$

Ions in solution: ${\text{K}}_{\text{2}}{\text{SO}}_{\text{4}}$ : ${\text{K}}^{\text{+}}$ and ${\text{SO}}_4{}^{2-}$

Now, ${\text{Ni(OH)}}_2$ is solid, not soluble in water whereas ${\text{K}}_{\text{2}}{\text{SO}}_{\text{4}}$ is soluble in water.

So, the equation will be:

${\text{Ni}}^{\text{2+}}{\text{(aq)+ SO}}_4{}^{2-}(\text{aq})+{\text{K}}^{+}{\text{(aq)+OH}}^{-}(\text{aq})\to {\text{Ni(OH)}}_2(\text{s}){\text{+K}}^{+}{\text{(aq)+SO}}_4^{2-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{SO}}_4{}^{\text{2-}}$, ${\text{K}}^{\text{+}}$), the final or net ionic equation is:

${\text{Ni}}^{\text{2+}}\text{(aq)}+2{\text{OH}}^{-}(\text{aq})\to {\text{Ni(OH)}}_2(\text{s})$

Interpretation Introduction

(e)

Interpretation:

The net ionic equation should be written when ammonium carbonate and sodium nitrate are mixed.

Concept introduction:

Solubility of any compound is predicted by above solubility chart.

Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.

Boxes with grey small box will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.

Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.

A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.

Answer to Problem 9QAP

No precipitation occurs.

Explanation of Solution

Ammonium carbonate: ${{\text{(NH}}_4\text{)}}_2{\text{CO}}_3$

Sodium nitrate: ${\text{NaNO}}_3$

Reaction for the solution of silver nitrate and hydrochloric acid is written as:

${{\text{(NH}}_4\text{)}}_2{\text{CO}}_3+{\text{NaNO}}_3\to {\text{Na}}_2{\text{CO}}_{\text{3}}{\text{+NH}}_4{\text{NO}}_3$

Reactants:

Ions in solution: ${{\text{(NH}}_4\text{)}}_2{\text{CO}}_3$ : ${\text{NH}}_4^{+}$ and ${\text{CO}}_3{}^{2-}$

Ions in solution: ${\text{NaNO}}_3$ : ${\text{Na}}^{\text{+}}$ and ${\text{NO}}_3^{-}$

Products:

Ions in solution: ${\text{Na}}_2{\text{CO}}_{\text{3}}$ : ${\text{Na}}^{\text{+}}$ and ${\text{CO}}_3{}^{2-}$

Ions in solution: ${\text{NH}}_4{\text{NO}}_3$ : ${\text{NH}}_4^{+}$ and ${\text{NO}}_3^{-}$

Now, ${\text{Na}}_2{\text{CO}}_{\text{3}}$ and ${\text{NH}}_4{\text{NO}}_3$ both are soluble in water or in aqueous solution. Thus, no precipitation occurs.