Chapter 4, Problem 7QAP

Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction.

(a) potassium nitrate and magnesium sulfate

(b) silver nitrate and potassium carbonate

(c) ammonium carbonate and cobalt(lll) chloride

(d) sodium phosphate and barium hydroxide

(e) barium nitrate and potassium hydroxide

Interpretation Introduction

(a)

Interpretation:

Whether a precipitate will form when the given solutions are mixed should be determined along with the net ionic equation should be written, if precipitate will form.

Potassium nitrate and magnesium sulfate

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 7QAP

No precipitation occurs

Explanation of Solution

Potassium nitrate: ${\text{KNO}}_{\text{3}}$

Magnesium sulfate: ${\text{MgSO}}_4$

Reaction for the solution of magnesium nitrate and potassium hydroxide is written as:

${\text{KNO}}_{\text{3}}+{\text{MgSO}}_4\to \text{Mg(NO}\text{)}{}_{\text{2}}+{\text{K}}_2{\text{SO}}_4$

Reactants:

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

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

Products:

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

Ions in solution: ${\text{K}}_2{\text{SO}}_4$ : ${\text{K}}^{\text{+}}$ and ${\text{SO}}_{\text{4}}{}^{2-}$

Now, $\text{Mg(NO}\text{)}{}_{\text{2}}$ and ${\text{K}}_2{\text{SO}}_4$ both are soluble in water. No precipitation occurs.

Interpretation Introduction

(b)

Interpretation:

Whether a precipitate will form when the given solutions are mixed should be determined along with the net ionic equation should be written, if precipitate will form.

Silver nitrate and potassium carbonate

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 7QAP

Precipitation occurs

The net ionic equation is:

${\text{2Ag}}^{\text{+}}{\text{(aq)+CO}}_3{}^{2-}(\text{aq})\to {\text{Ag}}_2{\text{CO}}_{\text{3}}(\text{s})$

Explanation of Solution

Silver nitrate: ${\text{AgNO}}_3$

Potassium carbonate: ${\text{K}}_2{\text{CO}}_3$

Reaction for the solution of silver nitrate and potassium carbonate is written as:

${\text{AgNO}}_3+{\text{K}}_2{\text{CO}}_3\to {\text{Ag}}_2{\text{CO}}_{\text{3}}{\text{+KNO}}_{\text{3}}$

Reactants:

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

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

Products:

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

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

Now, ${\text{Ag}}_2{\text{CO}}_{\text{3}}$ is solid, not soluble in water whereas ${\text{KNO}}_{\text{3}}$ is soluble in water.

So, the equation will be:

${\text{2Ag}}^{\text{+}}{\text{(aq)+CO}}_3{}^{2-}(\text{aq})+2{\text{K}}^{\text{+}}{\text{(aq)+NO}}_{\text{3}}{}^{-}(\text{aq})\to {\text{Ag}}_2{\text{CO}}_{\text{3}}(\text{s})+2{\text{K}}^{\text{+}}{\text{(aq)+NO}}_{\text{3}}{}^{-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{NO}}_{\text{3}}{}^{\text{-}}$ ,2 ${\text{K}}^{\text{+}}$), the final or net ionic equation is:

${\text{2Ag}}^{\text{+}}{\text{(aq)+CO}}_3{}^{2-}(\text{aq})\to {\text{Ag}}_2{\text{CO}}_{\text{3}}(\text{s})$

Interpretation Introduction

(c)

Interpretation:

Whether a precipitate will form when the given solutions are mixed should be determined along with the net ionic equation should be written, if precipitate will form.

Ammonium carbonate and cobalt(III) chloride

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 7QAP

Precipitation occurs

The net ionic equation is:

${\text{2Co}}^{\text{3+}}{\text{(aq)+3CO}}_3{}^{2-}(\text{aq})\to {\text{Co}}_2{{\text{(CO}}_3)}_3(\text{s})$

Explanation of Solution

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

Cobalt(III) chloride: ${\text{CoCl}}_{\text{3}}$

Reaction for the solution of ammonium carbonate and cobalt(III) chloride is written as:

${{\text{(NH}}_4\text{)}}_2{\text{CO}}_3+{\text{CoCl}}_{\text{3}}\to {\text{NH}}_4{\text{Cl+Co}}_2{{\text{(CO}}_3)}_3$

Reactants:

Ions in solution: ${{\text{(NH}}_4\text{)}}_2{\text{CO}}_3$ : ${\text{NH}}_4{}^{\text{+}}$ and ${\text{CO}}_{\text{3}}{}^{2-}$

Ions in solution: ${\text{CoCl}}_{\text{3}}$ : ${\text{Co}}^{\text{3+}}$ and ${\text{Cl}}^{-}$

Products:

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

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

Now, ${\text{Co}}_2{{\text{(CO}}_3)}_3$ is solid, not soluble in water whereas ${\text{NH}}_4\text{Cl}$ is soluble in water.

So, the equation will be:

${\text{2NH}}_4{}^{\text{+}}{\text{(aq)+3CO}}_3{}^{2-}(\text{aq})+2{\text{Co}}^{\text{3+}}{\text{(aq)+3Cl}}^{-}(\text{aq})\to {\text{Co}}_2{{\text{(CO}}_3)}_3(\text{s})+{\text{2NH}}_4{}^{\text{+}}{\text{(aq)+3Cl}}^{-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{3Cl}}^{-},$ 2 ${\text{NH}}_4{}^{\text{+}}$), the final or net ionic equation is:

${\text{2Co}}^{\text{3+}}{\text{(aq)+3CO}}_3{}^{2-}(\text{aq})\to {\text{Co}}_2{{\text{(CO}}_3)}_3(\text{s})$

Interpretation Introduction

(d)

Interpretation:

Whether a precipitate will form when the given solutions are mixed should be determined along with the net ionic equation should be written, if precipitate will form.

Sodium phosphate and barium hydroxide

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 7QAP

Precipitation occurs

The net ionic equation is:

$3{\text{Ba}}^{\text{2+}}{\text{(aq)+2PO}}_4{}^{3-}(\text{aq})\to {\text{Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}(\text{s})$

Explanation of Solution

Sodium phosphate: ${\text{Na}}_{\text{3}}{\text{PO}}_{\text{4}}$

Barium hydroxide: ${\text{Ba(OH)}}_2$

Reaction for the solution of sodium phosphate and barium hydroxide is written as:

${\text{Na}}_{\text{3}}{\text{PO}}_{\text{4}}+{\text{Ba(OH)}}_2\to {\text{NaOH+Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}$

Reactants:

Ions in solution: ${\text{Na}}_{\text{3}}{\text{PO}}_{\text{4}}$ : ${\text{Na}}^{\text{+}}$ and ${\text{PO}}_4{}^{3-}$

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

Products:

Ions in solution: $\text{NaOH}$ : ${\text{Na}}^{\text{+}}$ and ${\text{OH}}^{-}$

Ions in solution: ${\text{Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}$ : ${\text{Ba}}^{\text{2+}}$ and ${\text{PO}}_4{}^{3-}$

Now, ${\text{Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}$ is solid, not soluble in water whereas $\text{NaOH}$ is soluble in water.

So, the equation will be:

${\text{3Na}}^{\text{+}}{\text{(aq)+2PO}}_4{}^{3-}(\text{aq})+3{\text{Ba}}^{\text{2+}}{\text{(aq)+2OH}}^{-}(\text{aq})\to {\text{Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}(\text{s})+3{\text{Na}}^{\text{+}}{\text{(aq)+2OH}}^{-}(\text{aq})$

Now, cancelling out the ions which appear on both sides of the equation ( ${\text{3Na}}^{-},$ 2 ${\text{OH}}^{-}$), the final or net ionic equation is:

$3{\text{Ba}}^{\text{2+}}{\text{(aq)+2PO}}_4{}^{3-}(\text{aq})\to {\text{Ba}}_{\text{3}}{{\text{(PO}}_{\text{4}}\text{)}}_{\text{2}}(\text{s})$

Interpretation Introduction

(e)

Interpretation:

Whether a precipitate will form when the given solutions are mixed should be determined along with the net ionic equation should be written, if precipitate will form.

Barium nitrate and potassium hydroxide

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 7QAP

No precipitation occurs

Explanation of Solution

Barium nitrate: ${\text{Ba(NO}}_3{)}_2$

Potassium hydroxide: $\text{KOH}$

Reaction for the solution of sodium phosphate and potassium hydroxide is written as:

${\text{Ba(NO}}_3{)}_2+\text{KOH}\to {\text{KNO}}_{\text{3}}{\text{+Ba(OH)}}_{\text{2}}$

Reactants:

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

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

Products:

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

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

Now, ${\text{Ba(OH)}}_{\text{2}}$ and ${\text{KNO}}_{\text{3}}$ both are soluble in water. No precipitation occurs.