Chapter 3, Problem 56PS

Complete and balance the equations below, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for reactants and products (s, ℓ, g, aq).

(a) NiCO₃ + H₂SO₄ →.

(b) Co(OH)₂ + HBr →

(c) AgCH₃CO₂ + NaCI →

(d) NiO + CO →.

Interpretation Introduction

Interpretation:

• The given reaction has to be classified as precipitation or acid-base or gas forming reaction and the reaction has to be balanced.
• State of the product and reactant should be shown.

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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 56PS

The given reaction is gas forming reaction and the balanced equation is shown below.

  

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 nickel carbonate and sulfuric acid.  In this reaction nickel carbonate reaction with sulfuric acid to give nickel sulfate and carbon dioxide and water.

  

Balance the equation,

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

  

Interpretation Introduction

Interpretation:

• The given reaction has to be classified as precipitation or acid-base or gas forming reaction and the reaction has to be balanced.
• State of the product and reactant should be shown.

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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 56PS

The given reaction is acid - base reaction and the state of the reaction is shown below.

  

Explanation of Solution

The given reaction is acid - base reaction and the state of the reaction is shown below

  

The given compound is Cobalt(II) hydroxide and hydrogen bromide.  In this reaction Cobalt(II) hydroxide reaction with hydrogen bromide to give cobalt(II) bromide and formation of water is also the product.

    

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 atoms in the left side.  Therefore two molecule of hydrogen bromide is added to left side of reaction.  Therefore the balanced equation is given below.

    

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

    

Interpretation Introduction

Interpretation:

• The given reaction has to be classified as precipitation or acid-base or gas forming reaction and the reaction has to be balanced.
• State of the product and reactant should be shown.

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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 56PS

The given reaction is precipitation reaction and the state of the reaction is shown below

  

Explanation of Solution

The given reaction is precipitation reaction and the state of the reaction is shown below

    

The given compound is silver acetate and sodium chloride.  In this reaction silver acetate reaction with sodium chloride to give sodium acetate and silver chloride.  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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ insoluble.  Therefore, the given reaction is precipitation reaction.

Balance the equation,

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

Interpretation Introduction

Interpretation:

• The given reaction has to be classified as precipitation or acid-base or gas forming reaction and the reaction has to be balanced.
• State of the product and reactant should be shown.

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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 56PS

The given reaction is oxidation and reduction reaction and the state of the reaction is shown below.

    

Explanation of Solution

The given reaction is oxidation and reduction reaction and the state of the reaction is shown below

    

The given compound is nickel oxide and carbon monoxide.  In this reaction nickel oxide reaction with carbon monoxide to give nickel and carbon dioxide gas.  Here the oxidation state of nickel is $+2$ in the reactant and zero in the product, nickel gets the electron similarly the oxidation state of carbon is $+2$ in the reactant $+4$ in the product.  Therefore it is oxidation-reduction reaction, and gas as carbon dioxide is evolved from the reaction.

     

Balance the equation,

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