Chapter 3, Problem 81GQ

Balance equations for these reactions that occur in aqueous solution, and then classify each as a precipitation, add-base, or gas-forming reaction. Show states for the products (s, ℓ, g, aq), give their names, and write the net ionic equation.

(a) K₂CO₃ + HClO₄ → KClO₄ + CO₂ + H₂O

(b) FeCl₂ + (NH₄)₂S → FeS + NH₄Cl

(c) Fe(NO₃)₂ + Na₂CO₃(aq) → FeCO₃ + NaNO₃

(d) NaOH + FeC1₃ → NaCl + Fe(OH)₃

Interpretation Introduction

Interpretation:

The state of the reaction, balanced of the reaction, net ionic equation of the reaction and the type of the 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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{,}\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 81GQ

The state 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.

  ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)+}{\text{2HClO}}_{\text{4}}\text{(aq)}\to {\text{2KClO}}_{\text{4}}\text{(aq)}\text{+}{\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

Net ionic equation of the given reaction shown below

  ${\text{CO}}_{\text{3}}^{\text{2-}}{\text{(aq)+2H}}_{\text{3}}{\text{O}}^{\text{+}}\text{(aq)}\to {\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

Name of the reactant: Potassium carbonate, Perchloric acid

Name of the product: Potassium perchlorate and carbon dioxide and water.

Explanation of Solution

The state 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,

  ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)+}{\text{2HClO}}_{\text{4}}\text{(aq)}\to {\text{2KClO}}_{\text{4}}\text{(aq)}\text{+}{\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

The given compound is Potassium carbonate and Perchloric acid which is soluble in water.  In this reaction Potassium carbonate reaction with Perchloric acid to give Potassium perchlorate and carbon dioxide and water.

  ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)+}{\text{HClO}}_{\text{4}}\text{(aq)}\to {\text{KClO}}_{\text{4}}\text{(aq)}\text{+}{\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

Balance the equation,

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

${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)+}{\text{HClO}}_{\text{4}}\text{(aq)}\to 2{\text{KClO}}_{\text{4}}\text{(aq)}\text{+}{\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

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

${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)+}2{\text{HClO}}_{\text{4}}\text{(aq)}\to 2{\text{KClO}}_{\text{4}}\text{(aq)}\text{+}{\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

Net ionic equation of the given reaction shown below

  ${\text{CO}}_{\text{3}}^{\text{2-}}{\text{(aq)+2H}}_{\text{3}}{\text{O}}^{\text{+}}\text{(aq)}\to {\text{CO}}_{\text{2}}\text{(g)+}{\text{H}}_{\text{2}}\text{O(l)}$

Name of the reactant: Potassium carbonate, Perchloric acid

Name of the product: Potassium perchlorate and carbon dioxide and water.

Interpretation Introduction

Interpretation:

The state of the reaction, balanced of the reaction, net ionic equation of the reaction and the type of the 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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{,}\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 81GQ

The state 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.

  ${\text{FeCl}}_{\text{2}}\text{(aq)}{\text{+(NH}}_{\text{4}}{\text{)}}_{\text{2}}\text{S(aq)}\to \text{FeS(s)}\text{+}{\text{2NH}}_{\text{4}}\text{Cl(aq)}$

Net ionic equation of the given reaction shown below

  ${\text{Fe}}_{\text{2}}\text{+(aq)}\text{+}{\text{S}}^{\text{2-}}\text{(aq)}\to \text{FeS(s)}$

Name of the reactant Iron(II) chloride, Ammonium sulfide

Name of the product: Iron(II) sulfide and Ammonium chloride.

Explanation of Solution

The state 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

  ${\text{FeCl}}_{\text{2}}\text{(aq)}{\text{+(NH}}_{\text{4}}{\text{)}}_{\text{2}}\text{S(aq)}\to \text{FeS(s)}\text{+}{\text{NH}}_{\text{4}}\text{Cl(aq)}$

The given compound is Iron(II) chloride and Ammonium sulfide which is soluble in water.  In this reaction Iron(II) chloride reaction with Ammonium sulfide to give Iron(II) sulfide and Ammonium chloride.

  ${\text{FeCl}}_{\text{2}}\text{(aq)}{\text{+(NH}}_{\text{4}}{\text{)}}_{\text{2}}\text{S(aq)}\to \text{FeS(s)}\text{+}{\text{NH}}_{\text{4}}\text{Cl(aq)}$

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 ammonium chloride is added to right side of reaction.  Therefore the balanced equation is given below.

  ${\text{FeCl}}_{\text{2}}\text{(aq)}{\text{+(NH}}_{\text{4}}{\text{)}}_{\text{2}}\text{S(aq)}\to \text{FeS(s)}\text{+}{\text{2NH}}_{\text{4}}\text{Cl(aq)}$

Net ionic equation of the given reaction shown below

  ${\text{Fe}}_{\text{2}}\text{+(aq)}\text{+}{\text{S}}^{\text{2-}}\text{(aq)}\to \text{FeS(s)}$

Name of the reactant: Iron(II) chloride, Ammonium sulfide

Name of the product: Iron(II) sulfide and Ammonium chloride.

Interpretation Introduction

Interpretation:

The state of the reaction, balanced of the reaction, net ionic equation of the reaction and the type of the 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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{,}\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 81GQ

The state 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.

  ${\text{Fe(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\text{+}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}\text{+}{\text{2NaNO}}_{\text{3}}\text{(aq)}$

Net ionic equation of the given reaction shown below

  ${\text{Fe}}^{\text{2+}}\text{(aq)}\text{+}{\text{CO}}_{\text{3}}^{\text{2-}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}$

Name of the reactant Iron(II) Nitrate, Sodium carbonate

Name of the product: Iron(II) carbonate and sodium nitrate.

Explanation of Solution

The state 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

  ${\text{Fe(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\text{+}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}\text{+}{\text{NaNO}}_{\text{3}}\text{(aq)}$

The given compound is Iron(II) Nitrate and Sodium carbonate which is soluble in water. In this reaction Iron(II) Nitrate reaction with Sodium carbonate to give Iron(II) carbonate and sodium nitrate.

  ${\text{Fe(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\text{+}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}\text{+}{\text{NaNO}}_{\text{3}}\text{(aq)}$

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 atoms in the right side.  Therefore two molecule of sodium nitrate is added to right side of reaction.  Therefore the balanced equation is given below.

  ${\text{Fe(NO}}_{\text{3}}{\text{)}}_{\text{2}}\text{(aq)}\text{+}{\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}\text{+}{\text{2NaNO}}_{\text{3}}\text{(aq)}$

Net ionic equation of the given reaction shown below

  ${\text{Fe}}^{\text{2+}}\text{(aq)}\text{+}{\text{CO}}_{\text{3}}^{\text{2-}}\text{(aq)}\to {\text{FeCO}}_{\text{3}}\text{(s)}$

Name of the reactant Iron(II) Nitrate, Sodium carbonate

Name of the product: Iron(II) carbonate and sodium nitrate.

Interpretation Introduction

Interpretation:

The state of the reaction, balanced of the reaction, net ionic equation of the reaction and the type of the 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 ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{,}\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{,}\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{and}\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{,}\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{,}\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{,}\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{and}\left({\text{S}}^{\text{2-}}\right)$ 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 81GQ

The state 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.

  $\text{3NaOH(aq)}\text{+}{\text{FeCl}}_{\text{3}}\text{(aq)}\to {\text{3NaCl(aq)+Fe(OH)}}_{\text{3}}\text{(s)}$

Net ionic equation of the given reaction shown below

  ${\text{3OH}}^{\text{-}}\text{(aq)+}{\text{Fe}}^{\text{3+}}\text{(aq)}\to {\text{Fe(OH)}}_{\text{3}}\text{(s)}$

Name of the reactant: Sodium hydroxide, Iron(III) chloride.

Name of the product: Sodium chloride and Ferric hydroxide.

Explanation of Solution

The state 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.

  $\text{NaOH(aq)}\text{+}{\text{FeCl}}_{\text{3}}\text{(aq)}\to {\text{NaCl(aq)+Fe(OH)}}_{\text{3}}\text{(s)}$

The given compound is Sodium hydroxide, Iron(III) chloride which is soluble in water. In this reaction Sodium hydroxide reaction with Iron(III) chloride to give Sodium chloride and Ferric hydroxide.

  $\text{NaOH(aq)}\text{+}{\text{FeCl}}_{\text{3}}\text{(aq)}\to {\text{NaCl(aq)+Fe(OH)}}_{\text{3}}\text{(s)}$

Balance the equation,

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

  $\text{NaOH(aq)}\text{+}{\text{FeCl}}_{\text{3}}\text{(aq)}\to {\text{3NaCl(aq)+Fe(OH)}}_{\text{3}}\text{(s)}$

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 three sodium atoms in the right side and one sodium atom in the right side.  Therefore three molecule of sodium hydroxide is added to left side of reaction.  Therefore the balanced equation is given below.

  $\text{3NaOH(aq)}\text{+}{\text{FeCl}}_{\text{3}}\text{(aq)}\to {\text{3NaCl(aq)+Fe(OH)}}_{\text{3}}\text{(s)}$

Net ionic equation of the given reaction shown below

  ${\text{3OH}}^{\text{-}}\text{(aq)+}{\text{Fe}}^{\text{3+}}\text{(aq)}\to {\text{Fe(OH)}}_{\text{3}}\text{(s)}$

Name of the reactant: Sodium hydroxide, Iron(III) chloride.

Name of the product: Sodium chloride and Ferric hydroxide.