Chapter 3.9, Problem 3.10CYU

(a)

Interpretation Introduction

Interpretation:

The product, balanced equation, net ionic equation and the type of the given reaction should be identified.

Concept introduction:

Precipitation reaction: The formation of the product is insoluble when the ions combine in the solution is called precipitation reaction.

Acid - base reaction: Formation of the salt from the cation from the base and anion from the acid and formation of water is also the product.

Gas forming reaction: The reaction of acid and metal carbonates which produce carbonic acid. The carbonic acid decomposes which gives water and carbon dioxide.

Oxidation - reduction reaction: The electrons are transferred to one to other is called oxidation reduction reaction.

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 bit 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 3.10CYU

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is gas forming reaction and the balanced equation is shown below

  

Net ionic equation of the given reaction shown below (a)

Explanation of Solution

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is gas forming reaction and the balanced equation is shown below

  

The given compound is copper carbonate and sulfuric acid which is soluble in water. In this reaction copper carbonate reaction with sulfuric acid to give copper sulfate and carbon dioxide and water.

  

Balance the equation,

The reaction is already balanced. Therefore the balanced equation is given below.

  

The net ionic equation is given below,

(b)

Interpretation Introduction

Interpretation:

The product, balanced equation, net ionic equation and the type of the given reaction should be identified.

Concept introduction:

Precipitation reaction: The formation of the product is insoluble when the ions combine in the solution is called precipitation reaction.

Acid - base reaction: Formation of the salt from the cation from the base and anion from the acid and formation of water is also the product.

Gas forming reaction: The reaction of acid and metal carbonates which produce carbonic acid. The carbonic acid decomposes which gives water and carbon dioxide.

Oxidation - reduction reaction: The electrons are transferred to one to other is called oxidation reduction reaction.

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 bit 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 3.10CYU

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is oxidation-reduction reaction and the balanced equation is shown below (b)

     

Net ionic equation of the given reaction shown below (b)

     

Explanation of Solution

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is oxidation-reduction reaction and the balanced equation is shown below

     

The given compound is gallium and oxygen. In this reaction gallium reaction with oxygen to give gallium oxide, sulfur dioxide. Here the oxidation state of gallium is zero in the reactant and $+2$ in the product, gallium loss the electron similarly the oxidation state of oxygen is zero in the reactant $-2$ in the product. Therefore it is oxidation-reduction reaction.

     

Balance the equation,

Balance the oxygen atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients. There are two oxygen atoms in the left side and one oxygen atoms in the right side. Therefore two molecule of gallium oxide is added to right side of reaction. Therefore the balanced equation is given below.

     

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

     

Net ionic equation of the given reaction shown below

     

(c)

Interpretation Introduction

Interpretation:

The product, balanced equation, net ionic equation and the type of the given reaction should be identified.

Concept introduction:

Precipitation reaction: The formation of the product is insoluble when the ions combine in the solution is called precipitation reaction.

Acid - base reaction: Formation of the salt from the cation from the base and anion from the acid and formation of water is also the product.

Gas forming reaction: The reaction of acid and metal carbonates which produce carbonic acid. The carbonic acid decomposes which gives water and carbon dioxide.

Oxidation - reduction reaction: The electrons are transferred to one to other is called oxidation reduction reaction.

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 bit 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 3.10CYU

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is acid-base reaction and the balanced equation is shown below (c)

    

Net ionic equation of the given reaction shown below (c)

    

Explanation of Solution

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is acid-base reaction and the balanced equation is shown below

    

The given compound is barium hydroxide and nitric acid. In this reaction barium hydroxide reaction with nitric acid to give barium nitrate and formation of water is also the product.

    

Balance the equation,

Balance the nitrogen atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients. There are two nitrogen atoms in the right side and one nitrogen atoms in the left side. Therefore two molecule of nitric acid is added to left side of reaction. Therefore the balanced equation is given below.

    

Balance the hydrogen atom in the given equation. There are two hydrogen atoms in the right side and four hydrogen atoms in the left side. Therefore two molecule of water is added to right side of reaction. Therefore the balanced equation is given below.

    

Net ionic equation of the given reaction shown below

    

(d)

Interpretation Introduction

Interpretation:

The product, balanced equation, net ionic equation and the type of the given reaction should be identified.

Concept introduction:

Precipitation reaction: The formation of the product is insoluble when the ions combine in the solution is called precipitation reaction.

Acid - base reaction: Formation of the salt from the cation from the base and anion from the acid and formation of water is also the product.

Gas forming reaction: The reaction of acid and metal carbonates which produce carbonic acid. The carbonic acid decomposes which gives water and carbon dioxide.

Oxidation - reduction reaction: The electrons are transferred to one to other is called oxidation reduction reaction.

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 bit 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 3.10CYU

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is precipitation reaction and the balanced equation is shown below.

    

Net ionic equation of the given reaction shown below (a)

Explanation of Solution

The product of the reaction, balancing of the reaction and the type of the reaction is shown below, the given reaction is precipitation reaction and the balanced equation is shown below

    

The given compound is copper chloride and ammonium sulfide. In this reaction copper chloride reaction with ammonium sulfide to give copper sulfide and ammonium chloride.

the given reaction is precipitation reaction.

    

Balance the equation,

Balance the nitrogen atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients. There are two nitrogen atoms in the left side and one nitrogen atoms in the right side. Therefore two molecule of ammoniu chloride is added to right side of reaction. Therefore the balanced equation is given below.