Chapter 4, Problem 4.31P

4-31 Predict whether a precipitate will form when aqueous solutions of the following compounds are mixed. If a precipitate will form, write its formula and write a net ionic equation for its formation. To make your predictions, use the solubiity generalizations in

Section 4-3.

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction gives precipitate or not should be determined. If yes, the formula of the product should be written along with the net ionic equation.

${\text{CaCl}}_{\text{2}}(\text{a}q){\text{+K}}_{\text{3}}{\text{PO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }$

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)\text{+CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow \text{+CB}(\text{a}q)$

Here, $\text{AD}\left(s\right)$ represents a precipitate.

Answer to Problem 4.31P

Phosphate of calcium are insoluble, hence they separate out as precipitate.

Precipitate - ${\text{Ca}}_{\text{3}}{\left({\text{PO}}_{\text{4}}\right)}_{\text{2}}\text{(s)}\downarrow$

Net Reaction.

$3{\text{CaCl}}_{\text{2}}(\text{a}q)+2{\text{K}}_{\text{3}}{\text{PO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{Ca}}_{\text{3}}{\left({\text{PO}}_{\text{4}}\right)}_{\text{2}}(s)\downarrow +6{\text{K}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

${\text{CaCl}}_{\text{2}}(\text{a}q)+{\text{K}}_{\text{3}}{\text{PO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place ,then the product of the reaction would be-

$3{\text{CaCl}}_2(\text{a}q)+2{\text{K}}_{\text{3}}{\text{PO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{Ca}}_{\text{3}}{\left({\text{PO}}_{\text{4}}\right)}_2(s)\downarrow +6{\text{K}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)$

The products are phosphate of calcium and chloride of potassium.

Phosphates of calcium are insoluble; hence, they separate out as precipitate, chlorides of potassium are soluble, they remain as aqueous solution.

The net reaction is as-

$3{\text{CaCl}}_{\text{2}}(\text{a}q)+2{\text{K}}_{\text{3}}{\text{PO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{Ca}}_{\text{3}}{\left({\text{PO}}_{\text{4}}\right)}_{\text{2}}(s)\downarrow +6{\text{K}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)$.

Interpretation Introduction

(b)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

No precipitate.

Net Reaction.

$2\text{KCl}(\text{a}q)+{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }2{\text{K}}^{+}(\text{a}q)+{\text{SO}}_{\text{4}}{}^{2-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

$\mathrm{KCl}(\text{a}q)+{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place ,then the product of the reaction would be-

$2\text{KCl}(\text{a}q)+{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }2K^{+}(\text{a}q)+{\text{SO}}_{\text{4}}{}^{2-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)$

The products are sulphate of potassium and chloride of Sodium.

Sulphates of potassium are soluble, they remain as aqueous solution.

Chlorides of sodium are soluble, they remain as aqueous solution.

The net reaction is as-

$2\text{KCl}(\text{a}q)+{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }2{\text{K}}^{+}(\text{a}q)+{\text{SO}}_{\text{4}}{}^{2-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)$.

Interpretation Introduction

(c)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

Phosphate of Calcium are insoluble, hence they separate out as precipitate.

Precipitate - ${\text{BaCO}}_{\text{3}}(s)\downarrow$

Net Reaction.

${\left({\text{NH}}_{\text{4}}\right)}_{\text{2}}{\text{CO}}_{\text{3}}(\text{a}q)+\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)\stackrel{}{\to }{\text{BaCO}}_{\text{3}}(s)\downarrow +2{\text{NH}}_{\text{4}}{}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

${\left({\text{NH}}_{\text{4}}\right)}_{\text{2}}{\text{CO}}_{\text{3}}(\text{a}q)+\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place ,then the product of the reaction would be-

${\left({\text{NH}}_{\text{4}}\right)}_{\text{2}}{\text{CO}}_{\text{3}}(\text{a}q)+\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_2(\text{a}q)\stackrel{}{\to }{\text{BaCO}}_{\text{3}}(s)\downarrow +2{\text{NH}}_4{}^{+}(\text{a}q)+2{\text{NO}}_3{}^{-}(\text{a}q)$

The products are Carbonate of Barium and Nitrate of Ammonium.

Carbonate of Barium are insoluble, hence they separate out as precipitate.

Nitrate of Ammonium are soluble, they remain as aqueous solution.

The net reaction is as-

${\left({\text{NH}}_{\text{4}}\right)}_{\text{2}}{\text{CO}}_{\text{3}}(\text{a}q)+\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)\stackrel{}{\to }{\text{BaCO}}_{\text{3}}(s)\downarrow +2{\text{NH}}_{\text{4}}{}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.

Interpretation Introduction

(d)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

No precipitate.

Net Reaction.

${\text{FeCl}}_{\text{2}}(\text{a}q)+2\text{KOH}(\text{a}q)\stackrel{}{\to }2{\text{K}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)+\text{F}{\text{e}}^{2+}(\text{a}q)+2\text{O}{\text{H}}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

${\text{FeCl}}_{\text{2}}(\text{a}q)+\text{KOH}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place, then the product of the reaction would be-

${\text{FeCl}}_{\text{2}}(\text{a}q)+2\text{KOH}(\text{a}q)\stackrel{}{\to }2{\text{K}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)+{\text{Fe}}^{2+}(\text{a}q)+2{\text{OH}}^{-}(\text{a}q)$

The products are Chloride of Potassium and Hydroxide of Iron.

Chloride of Potassium are soluble, they remain as aqueous solution.

Hydroxide of Iron are soluble, they remain as aqueous solution.

The net reaction is as-

${\text{FeCl}}_{\text{2}}(\text{a}q)+2\text{KOH}(\text{a}q)\stackrel{}{\to }2{\text{K}}^{+}(\text{a}q)+2{\text{Cl}}^{-}(\text{a}q)+\text{F}{\text{e}}^{2+}(\text{a}q)+2\text{O}{\text{H}}^{-}(\text{a}q)$.

Interpretation Introduction

(e)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

No precipitate.

Net Reaction.

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+2\text{NaOH}(\text{a}q)\stackrel{}{\to }{\text{Ba}}^{2+}(\text{a}q)+2{\text{OH}}^{-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_2(\text{a}q)+\text{NaOH}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place, then the product of the reaction would be-

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+2\text{NaOH}(\text{a}q)\stackrel{}{\to }{\text{Ba}}^{2+}(\text{a}q)+2{\text{OH}}^{-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{NO}}_3{}^{-}(\text{a}q)$

The products are Hydroxide of Barium and Nitrate of Sodium.

Hydroxide of Barium are soluble, they remain as aqueous solution.

Nitrate of Sodium are soluble, they remain as aqueous solution.

The net reaction is as-

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+2\text{NaOH}(\text{a}q)\stackrel{}{\to }{\text{Ba}}^{2+}(\text{a}q)+2{\text{OH}}^{-}(\text{a}q)+2{\text{Na}}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.

Interpretation Introduction

(f)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

Phosphate of Calcium are insoluble, hence they separate out as precipitate.

Precipitate - ${\text{Sb}}_{\text{2}}{\text{S}}_{\text{3}}(s)\downarrow$

Net Reaction.

${\text{3Na}}_{\text{2}}\text{S}(\text{a}q)+2{\text{SbCl}}_{\text{3}}(\text{a}q)\stackrel{}{\to }6{\text{Na}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)+{\text{Sb}}_{\text{2}}{\text{S}}_{\text{3}}(s)\downarrow$.

Explanation of Solution

The given reaction is as-

${\text{Na}}_{\text{2}}\text{S}(\text{a}q)+{\text{SbCl}}_{\text{3}}(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place, then the product of the reaction would be-

$3{\text{Na}}_{\text{2}}\text{S}(\text{a}q)+2{\text{SbCl}}_{\text{3}}(\text{a}q)\stackrel{}{\to }6{\text{Na}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)+{\text{Sb}}_{\text{2}}{\text{S}}_{\text{3}}(s)\downarrow$

The products are Chloride of Sodium and Sulphide of Antimony.

Chloride of Sodium are soluble, they remain as aqueous solution.

Sulphide of Antimony are insoluble, hence they separate out as precipitate.

The net reaction is as-

${\text{3Na}}_{\text{2}}\text{S}(\text{a}q)+2{\text{SbCl}}_{\text{3}}(\text{a}q)\stackrel{}{\to }6{\text{Na}}^{+}(\text{a}q)+6{\text{Cl}}^{-}(\text{a}q)+{\text{Sb}}_{\text{2}}{\text{S}}_{\text{3}}(s)\downarrow$.

Interpretation Introduction

(g)

Interpretation:

The precipitation or double-displacement reaction is to be determined.

Concept Introduction:

When two aqueous solutions are mixed together, this may or may not result in formation of an insoluble solid in the solution. This insoluble solid is called precipitate and this reaction is called precipitation reaction.

For example, a reaction in which A and C displace each other from their respective solutions. Since two displacement takes place, this reaction is also called double displacement reaction.

$\text{AB}(\text{a}q)+\text{CD}(\text{a}q)\stackrel{}{\to }\text{AD}(s)\downarrow +\text{CB}(\text{a}q)$

Here, AD(s) represents a precipitate.

Answer to Problem 4.31P

Sulphate of Lead are insoluble, hence they separate out as precipitate.

Precipitate - ${\text{PbSO}}_{\text{4}}(s)\downarrow$

Net Reaction.

$\text{Pb}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+{\text{K}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{PbSO}}_{\text{4}}(s)\downarrow +2{\text{K}}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.

Explanation of Solution

The given reaction is as-

$\text{Pb}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+{\text{K}}_{\text{2}}{\text{SO}}_4(\text{a}q)\stackrel{}{\to }$

If the double displacement-reaction takes place, then the product of the reaction would be-

$\text{Pb}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+{\text{K}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{PbSO}}_{\text{4}}(s)\downarrow +2{\text{K}}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$

The products are Sulphate of Lead and Nitrate of Potassium.

Chloride of Sodium are soluble, they remain as aqueous solution.

Sulphate of Lead are insoluble, hence they separate out as precipitate.

The net reaction is as-

$\text{Pb}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}(\text{a}q)+{\text{K}}_{\text{2}}{\text{SO}}_{\text{4}}(\text{a}q)\stackrel{}{\to }{\text{PbSO}}_{\text{4}}(s)\downarrow +2{\text{K}}^{+}(\text{a}q)+2{\text{NO}}_{\text{3}}{}^{-}(\text{a}q)$.