Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 3, Problem 73GQ

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

(a)

Expert Solution
Check Mark
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 Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides (Ag+, Hg22+, Pb2+) are insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and(S2-) 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, Ba(OH)2and Sr(OH)2 are soluble in water.

Answer to Problem 73GQ

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.

  K2CO3(aq)+2HClO4(aq)2KClO4(aq)+CO2(g)+H2O(l)

Net ionic equation of the given reaction shown below

  CO32-(aq)+2H3O+(aq)CO2(g)+H2O(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,

  K2CO3(aq)+2HClO4(aq)2KClO4(aq)+CO2(g)+H2O(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.

  K2CO3(aq)+HClO4(aq)KClO4(aq)+CO2(g)+H2O(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.

K2CO3(aq)+HClO4(aq)2KClO4(aq)+CO2(g)+H2O(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.

K2CO3(aq)+2HClO4(aq)2KClO4(aq)+CO2(g)+H2O(l)

Net ionic equation of the given reaction shown below

  CO32-(aq)+2H3O+(aq)CO2(g)+H2O(l)

Name of the reactant: Potassium carbonate, Perchloric acid

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

(b)

Expert Solution
Check Mark
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 Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides (Ag+, Hg22+, Pb2+) are insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and(S2-) 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, Ba(OH)2and Sr(OH)2 are soluble in water.

Answer to Problem 73GQ

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.

  FeCl2(aq)+(NH4)2S(aq)FeS(s)+2NH4Cl(aq)

Net ionic equation of the given reaction shown below

  Fe2+(aq)+S2-(aq)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

  FeCl2(aq)+(NH4)2S(aq)FeS(s)+NH4Cl(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.

  FeCl2(aq)+(NH4)2S(aq)FeS(s)+NH4Cl(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.

  FeCl2(aq)+(NH4)2S(aq)FeS(s)+2NH4Cl(aq)

Net ionic equation of the given reaction shown below

  Fe2+(aq)+S2-(aq)FeS(s)

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

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

(c)

Expert Solution
Check Mark
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 Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides (Ag+, Hg22+, Pb2+) are insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and(S2-) 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, Ba(OH)2and Sr(OH)2 are soluble in water.

Answer to Problem 73GQ

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.

  Fe(NO3)2(aq)+Na2CO3(aq)FeCO3(s)+2NaNO3(aq)

Net ionic equation of the given reaction shown below

  Fe2+(aq)+CO32-(aq)FeCO3(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

  Fe(NO3)2(aq)+Na2CO3(aq)FeCO3(s)+NaNO3(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.

  Fe(NO3)2(aq)+Na2CO3(aq)FeCO3(s)+NaNO3(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.

  Fe(NO3)2(aq)+Na2CO3(aq)FeCO3(s)+2NaNO3(aq)

Net ionic equation of the given reaction shown below

  Fe2+(aq)+CO32-(aq)FeCO3(s)

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

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

(d)

Expert Solution
Check Mark
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 Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides (Ag+, Hg22+, Pb2+) are insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and(S2-) 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, Ba(OH)2and Sr(OH)2 are soluble in water.

Answer to Problem 73GQ

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.

  3NaOH(aq)+FeCl3(aq)3NaCl(aq)+Fe(OH)3(s)

Net ionic equation of the given reaction shown below

  3OH-(aq)+Fe3+(aq)Fe(OH)3(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.

  NaOH(aq)+FeCl3(aq)NaCl(aq)+Fe(OH)3(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.

  NaOH(aq)+FeCl3(aq)NaCl(aq)+Fe(OH)3(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.

  NaOH(aq)+FeCl3(aq)3NaCl(aq)+Fe(OH)3(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.

  3NaOH(aq)+FeCl3(aq)3NaCl(aq)+Fe(OH)3(s)

Net ionic equation of the given reaction shown below

  3OH-(aq)+Fe3+(aq)Fe(OH)3(s)

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

Name of the product: Sodium chloride and Ferric hydroxide.

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Chapter 3 Solutions

Chemistry & Chemical Reactivity

Ch. 3.5 - In each of the following cases, aqueous solutions...Ch. 3.5 - Prob. 1RCCh. 3.5 - What is the net ionic equation for the reaction of...Ch. 3.6 - Prob. 1CYUCh. 3.6 - Prob. 2CYUCh. 3.6 - Prob. 1RCCh. 3.6 - 2. The hydrogen phosphate ion is amphiprotic....Ch. 3.6 - What is the net ionic equation for the reaction of...Ch. 3.6 - Prob. 4RCCh. 3.7 - Prob. 1CYUCh. 3.7 - Prob. 1RCCh. 3.8 - Assign an oxidation number to the underlined atom...Ch. 3.8 - Prob. 2CYUCh. 3.8 - 1. What is the oxidation number of Mn in...Ch. 3.8 - Prob. 2RCCh. 3.8 - 3. In which of the manganese compounds below does...Ch. 3.9 - Prob. 1CYUCh. 3.9 - 1. Sometimes a reaction can fall in more than one...Ch. 3.9 - Prob. 1QCh. 3.9 - Prob. 2QCh. 3.9 - Prob. 3QCh. 3.9 - Prob. 4QCh. 3.9 - Prob. 5QCh. 3 - Write balanced chemical equations for the...Ch. 3 - Write balanced chemical equations for the...Ch. 3 - Prob. 3PSCh. 3 - Prob. 4PSCh. 3 - Prob. 5PSCh. 3 - Balance the following equations, and name each...Ch. 3 - Equal amounts of two acidsHCl and HCO2H (formic...Ch. 3 - Prob. 8PSCh. 3 - What is an electrolyte? How can you differentiate...Ch. 3 - Name and give the formulas of two acids that are...Ch. 3 - Which compound or compounds in each of the...Ch. 3 - Which compound or compounds in each of the...Ch. 3 - The following compounds are water-soluble. What...Ch. 3 - The following compounds are water-soluble. What...Ch. 3 - Decide whether each of the following is...Ch. 3 - Decide whether each of the following is...Ch. 3 - Balance the equation for the following...Ch. 3 - Balance the equation for the following...Ch. 3 - Predict the products of each precipitation...Ch. 3 - Prob. 20PSCh. 3 - Write a balanced equation for the ionization of...Ch. 3 - Write a balanced equation for the ionization of...Ch. 3 - Prob. 23PSCh. 3 - Phosphoric add can supply one, two, or three H3O+...Ch. 3 - Prob. 25PSCh. 3 - Prob. 26PSCh. 3 - Prob. 27PSCh. 3 - Prob. 28PSCh. 3 - Prob. 29PSCh. 3 - Prob. 30PSCh. 3 - Write an equation that describes the equilibrium...Ch. 3 - Write an equation that describes the equilibrium...Ch. 3 - Prob. 33PSCh. 3 - Write two chemical equations, one in which H2PO4...Ch. 3 - Balance the following equations, and then write...Ch. 3 - Balance the following equations, and then write...Ch. 3 - Prob. 37PSCh. 3 - Balance each of the following equations, and then...Ch. 3 - Write balanced net ionic equations for the...Ch. 3 - Write balanced net ionic equations for the...Ch. 3 - Siderite is a mineral consisting largely of...Ch. 3 - The mineral rhodothrosite is manganese()...Ch. 3 - Prob. 43PSCh. 3 - Prob. 44PSCh. 3 - Determine the oxidation number of each element in...Ch. 3 - Determine the oxidation number of each element in...Ch. 3 - Prob. 47PSCh. 3 - Which two of the following reactions are...Ch. 3 - In the following reactions, decide which reactant...Ch. 3 - In the following reactions, decide which reactant...Ch. 3 - Balance the following equations, and then classify...Ch. 3 - Prob. 52PSCh. 3 - Classify each of the following reactions as a...Ch. 3 - Prob. 54PSCh. 3 - Balance each of the following equations, and...Ch. 3 - Complete and balance the equations below, and...Ch. 3 - Prob. 57PSCh. 3 - Prob. 58PSCh. 3 - Balance the following equations: (a) for the...Ch. 3 - Balance the following equations: (a) for the...Ch. 3 - Prob. 61GQCh. 3 - Give the formula for each of the following...Ch. 3 - Prob. 63GQCh. 3 - Name two anions that combine with Al3+ ion to...Ch. 3 - Write the net ionic equation and identify the...Ch. 3 - Identify and name the water-insoluble product in...Ch. 3 - Bromine is obtained from sea water by the...Ch. 3 - Identify each of the blowing substances as a...Ch. 3 - The mineral dolomite contains magnesium...Ch. 3 - Aqueous solutions of ammonium sulfide, (NH4)2S,...Ch. 3 - Prob. 71GQCh. 3 - Prob. 72GQCh. 3 - Balance equations for these reactions that occur...Ch. 3 - Prob. 74GQCh. 3 - You are given mixtures containing the following...Ch. 3 - Identify, from each list below, the compound or...Ch. 3 - Prob. 77GQCh. 3 - Prob. 78GQCh. 3 - Gas evolution was observed when a solution of Na2S...Ch. 3 - Prob. 81ILCh. 3 - Prob. 82ILCh. 3 - Prob. 83ILCh. 3 - A Suggest a laboratory method for preparing barium...Ch. 3 - The Toliens test for the presence of reducing...Ch. 3 - There are many ionic compounds that dissolve in...Ch. 3 - Most naturally occurring acids are weak acids....Ch. 3 - You want to prepare barium chloride, BaC12, using...Ch. 3 - Prob. 89SCQCh. 3 - A Describe how to prepare zinc chloride by (a) an...Ch. 3 - A common method for analyzing for the nickel...Ch. 3 - The presence of arsenic in a sample that may also...
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