Chapter 3, Problem 20PS

(a)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}{\text{, Br}}^{\text{-}}{\text{, I}}^{\text{-}}\left(\text{halides}\right)$ are soluble.  But some of the halides are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ are insoluble.

Salts of F^- are soluble.  But some of the fluoride salt of ${\text{Mg}}^{\text{2+}}{\text{, Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}$ are insoluble.

Salts of $\text{sulfate }\left({\text{SO}}_{\text{4}}{}^{\text{2-}}\right)$ are soluble.  But sulfates of ${\text{Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}{\text{, Ag}}^{\text{+}}\text{,}$ are insoluble.

Insoluble compounds in water:

Most of the salts of $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

Product and balanced net ionic equation for the given aqueous solution is,

  

Explanation of Solution

The given compound is lead nitrate and potassium bromidewhich is soluble in water.  In this reaction Pb²⁺ and K⁺ cations exchange the anions (NO₃^- and Br^-) to give lead bromide and potassium nitrate.

  

Balance the equation,

Balance the bromine atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients.

There are two bromine atoms in the right side and one bromine atom in the left side. Therefore two molecule of sodium bromide is added to left side of reaction.  Therefore the balanced equation is given below.

  

Balance the sodium atom in the given equation, there are two sodium atoms in the left side and one sodium atom in the right side.  Therefore two molecule of sodium nitrate is added to right side of reaction.  Therefore the balanced equation is given below.

  

Therefore the balanced equation is given below.

  

Almost all the salts of ${\text{Cl}}^{\text{-}}{\text{, Br}}^{\text{-}}{\text{, I}}^{\text{-}}\left(\text{halides}\right)$ are soluble.  But some of the halides are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ are insoluble.  Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

  

In this reaction, all the soluble ionic dissociates and forms the ions in solution.

The ionic equation is given below,

To get the net ionic equation, remove the spectator ions.  Therefore the net ionic equation is given below,

  

(b)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}{\text{, Br}}^{\text{-}}{\text{, I}}^{\text{-}}\left(\text{halides}\right)$ are soluble.  But some of the halides are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ are insoluble.

Salts of F^- are soluble.  But some of the fluoride salt of ${\text{Mg}}^{\text{2+}}{\text{, Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}$ are insoluble.

Salts of $\text{sulfate }\left({\text{SO}}_{\text{4}}{}^{\text{2-}}\right)$ are soluble.  But sulfates of ${\text{Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}{\text{, Ag}}^{\text{+}}\text{,}$ are insoluble.

Insoluble compounds in water:

Most of the salts of $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

Product and balanced net ionic equation for the given aqueous solution is,

  

Explanation of Solution

The given compound is calcium nitrate and potassium fluoride which is soluble in water.  In this reaction Ca²⁺ and K⁺ cations exchange the anions (NO₃^- and F^-) to give calcium fluoride and potassium nitrate.

  

Balance the equation,

Balance the fluorine atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients.

There are two fluorine atoms in the right side and one fluorine atom in the left side.  Therefore two molecule of potassium fluoride is added to left side of reaction.  Therefore the balanced equation is given below.

  

Balance the potassium atom in the given equation, there are two potassium atoms in the left side and one potassium atom in the right side.  Therefore two molecule of potassium nitrate is added to right side of reaction.  Therefore the balanced equation is given below.

  

Therefore the balanced equation is given below.

  

Almost all the salts of ${\text{Cl}}^{\text{-}}{\text{, Br}}^{\text{-}}{\text{, I}}^{\text{-}}\left(\text{halides}\right)$ are soluble.  But some of the halides are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ are insoluble. Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

  

In this reaction, all the soluble ionic dissociates and forms the ions in solution.

The ionic equation is given below,

To get the net ionic equation, remove the spectator ions.  Therefore the net ionic equation is given below,

    

(c)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}{\text{, Br}}^{\text{-}}{\text{, I}}^{\text{-}}\left(\text{halides}\right)$ are soluble.  But some of the halides are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ are insoluble.

Salts of F^- are soluble.  But some of the fluoride salt of ${\text{Mg}}^{\text{2+}}{\text{, Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}$ are insoluble.

Salts of $\text{sulfate }\left({\text{SO}}_{\text{4}}{}^{\text{2-}}\right)$ are soluble.  But sulfates of ${\text{Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}{\text{, Ag}}^{\text{+}}\text{,}$ are insoluble.

Insoluble compounds in water:

Most of the salts of $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

Product and balanced net ionic equation for the given aqueous solution is,

  

Explanation of Solution

The given compound is calcium nitrate and sodium oxalatewhich is soluble in water.  In this reaction Ca²⁺ and Na⁺ cations exchange the anions (NO₃^- and C₂O₄^2-) to give calciumoxalate and sodium nitrate.

  

Balance the equation,

Balance the sodium atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients.

There are two sodium atoms in the left side and one sodium atom in the right side. Therefore two molecule of sodium nitrate is added to right side of reaction.  Therefore the balanced equation is given below.

  

Therefore the balanced equation is given below.

  

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.  Most of the salts of $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

  

In this reaction, all the soluble ionic dissociates and forms the ions in solution.

The ionic equation is given below,

To get the net ionic equation, remove the spectator ions.  Therefore the net ionic equation is given below,