Chemistry
Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Chapter 16, Problem 152AP

Calculate the concentrations of all species in a 0 .100  M  H 3 PO 4 solution.

Expert Solution & Answer
Check Mark
Interpretation Introduction

Interpretation:

The concentrations of all the species present in the solution, which contains phosphoric acid, is to be determined.

Concept introduction:

The first ionization of the polyprotic acid takes place as

H3A(aq)+H2O(l)H3O+(aq)+H2A(aq)

Ka1 is the measure of the dissociation of the first proton of an acid and is known as the first acid-ionization constant, which is specific to a particular temperature.

Ka1=[H3O+][H2A][H3A] …… (1)

The second ionization of the polyprotic acid takes place as

H2A(aq)+H2O(l)H3O+(aq)+HA(aq)

Ka2 is the measure of the dissociation of the second proton of an acid and is known as the second acid-ionization constant, which is specific to a particular temperature.

Ka2=[H3O+][HA][H2A] …… (2)

The third ionization of the polyprotic acid takes place as

HA(aq)+H2O(l)H3O+(aq)+A(aq)

Ka3 is the measure of the dissociation of the third proton of an acid and is known as the third acid-ionization constant, which is specific to a particular temperature.

Ka3=[H3O+][A][HA] …… (3)

Percent ionization is the percentage of acid that gets dissociated upon addition to water. It depends on the hydronium ion concentration.

% dissociation=[H3O+]eq[H2A]o×100% …… (4)

Here, [H3O+]eq is the hydronium ion concentration at equilibrium and [H2A]o is the original acid concentration.

Answer to Problem 152AP

Solution:

[H3PO4]=0.076 M, [H2PO4]=0.0239 M, [HPO42]=6.2×108 M, [PO43]=1.1×1018M,[H3O+]=0.0239 M

Explanation of Solution

Given information:

The concentration of phosphoric acid (H3PO4) at 25°Cis 0.100 M.

Refer to Table 16.8 for Ka1, Ka2, and Ka3 values of phosphoric acid. The values are as given below:

Ka1=7.5×103Ka2=6.2×108Ka3=4.8×1013

When phosphoric acid is dissolved in water, the dissociation takes place in three steps, as it is a triprotic acid. First, one proton is partially dissociated, since phosphoric acid is a weak acid. Thus, the pH of the solution is determined by the contribution made by all the three proton dissociation steps.

The reaction of the first proton dissociation of phosphoric acid is depicted as

HPO4(aq)+H2O(l)H3O+(aq)+H2PO4(aq)

Prepare an equilibrium table and represent each of the species in terms of x as

H3PO4(aq)H2O(l)H3O+(aq)H2PO4(aq)Initial concentration(M)0.10000Change in concentration(M)x+x+xEquilibrium concentration(M)0.100xxx

Now, substitute these concentrations in equation (1) as

Ka1=(x)(x)(0.100x)

Since the value of Ka1 is small, the amount of acid dissociated is less. Therefore, (0.100x) can be approximated as 0.100. Now, substitute the value of Ka1 in above equation as

7.5×103=(x)(x)0.100x2=(7.5×103)0.100x=7.5×104x=2.74×102

Thus, [H3O+]1(eq)=2.74×102M and [H3PO4](O)=0.100 M

Calculate the percent dissociation from equation (4) as

% dissociation=2.74×1020.100×100%=27.4 %

Since the percent dissociation is more than 5%, the approximation is not valid. Thus, again solve for the value of x as

7.5×103=(x)(x)(0.100x)x2+(7.5×103)x=(7.5×104)x=0.031, 0.0239

Since concentration cannot be negative, x=0.0239.

Thus,

[H2PO4](O)=0.0239 M[H3O+]1=0.0239 M

Also,

[H3PO4]=(0.1000.0239) M=0.076 M

Now, the reaction of the second proton dissociation of phosphoric acid is depicted as

H2PO4(aq)+H2O(l)H3O+(aq)+HPO42(aq)

Prepare an equilibrium table and represent each of the species in terms of y as

H2PO4(aq)H2O(l)H3O+(aq)HPO42(aq)Initial concentration(M)0.02390.02390Change in concentration(M)y+y+yEquilibrium concentration(M)0.0239y0.0239+yy

Now, substitute these concentrations in equation (2) as

Ka2=(0.0239+y)(y)(0.0239y)

Since the value of Ka2 is very small, the amount of acid dissociated is less. Therefore, (0.0239y) and (0.0239+y) can be approximated as 0.0239. Now, substitute the value of Ka2 in above equation as

6.2×108=(0.0239)(y)0.0239y=6.2×108

Thus, [H3O+]2(eq)=6.2×108M and [H2PO4](O)=0.0239 M.

Also,

[H2PO4]=(0.02396.2×108) M0.0239 M

[H3O+]=0.0239 M

Calculate the percent dissociation from equation (4) as

% dissociation=6.2×1080.0239×100%=0.00026 %

Since the percent dissociation is significantly less than 5%, the approximation is valid.

Now, the reaction of the third proton dissociation of phosphoric acid is depicted as

HPO42(aq)+H2O(l)H3O+(aq)+PO43(aq)

Prepare an equilibrium table and represent each of the species in terms of z as

HPO42(aq)H2O(l)H3O+(aq)PO43(aq)Initial concentration(M)6.2×1080.02390Change in concentration(M)z+z+zEquilibrium concentration(M)(6.2×108)z(0.0239)+zz

Now, substitute these concentrations in equation (3) as

Ka3=((6.2×108)+z)(z)((6.2×108)z)

Since the value of Ka3 is very small, the amount of acid dissociated is less. Therefore, ((6.2×108)z) can be approximated as 6.2×108 and ((0.239)+z) can be approximated as 0.0239. Now, substitute the value of Ka3 in above equation as

4.8×1013=(0.0239)(z)6.2×108z=(4.8×1013)(6.2×108)0.0239z=1.1×1018M

Thus, [H3O+]3(eq)=1.1×1018M and [HPO42](O)=6.2×108 M

Calculate the percent dissociation from equation (4) as

% dissociation=1.1×1018M6.2×108×100%=0.0000 %

Since the percent dissociation is significantly less than 5%, the approximation is valid.

Also,

[HPO42]=(6.2×1084.8×1013) M6.2×108 M

And,

[PO43]=1.1×1018M

Also,

[H3O+]=[H3O+]1+[H3O+]2+[H3O+]3=(0.0239)+(6.2×108)+(1.1×1018M)0.0239 M

Therefore, the concentration of all the species in the phosphoric acid solution are as follows:

[H3PO4]=0.076 M, [H2PO4]=0.0239 M, [HPO42]=6.2×108 M, [PO43]=1.1×1018M[H3O+]=0.0239 M

Conclusion

Therefore, the concentration of all the species in the phosphoric acid solution are as follows:

[H3PO4]=0.076 M, [H2PO4]=0.0239 M, [HPO42]=6.2×108 M, [PO43]=1.1×1018M[H3O+]=0.0239 M

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 16 Solutions

Chemistry

Ch. 16.3 - Prob. 1PPACh. 16.3 - Practice Problem BUILD The value of at normal...Ch. 16.3 - Prob. 1PPCCh. 16.3 - Determine the pH of a solution at 25°C in which [...Ch. 16.3 - 16.3.2 Determine in a solution at...Ch. 16.3 - Determine the pOH of a solution at 25°C in which [...Ch. 16.3 - Determine [ OH − ] in a solution at 25°C if pH =...Ch. 16.4 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.4 - Practice Problem BUILD Determine the pH of a...Ch. 16.4 - Practice Problem CONCEPTUALIZE Strong acid is...Ch. 16.4 - Calculate the pH of a 0.075–-M solution of...Ch. 16.4 - 16.4.2 What is the concentration of in a solution...Ch. 16.4 - 16.4.3 What is the of a solution at that is...Ch. 16.4 - What is the concentration of KOH in a solution at...Ch. 16.4 - What is the pH of a solution at 25°C that is...Ch. 16.4 - What is the concentration of Ca ( OH ) 2 in a...Ch. 16.4 - Which diagram best represents a solution of...Ch. 16.5 - Practice Problem ATTEMPT Calculate the hydronium...Ch. 16.5 - Practice Problem BUILD Calculate the hydroxide ion...Ch. 16.5 - Practice Problem CONCEPTUALIZE What is the value...Ch. 16.5 - The K a of a weak acid is 5.5 × 10 − 4 . What is...Ch. 16.5 - A 0.042-M solution of a weak acid has pH 4.01 at...Ch. 16.5 - The diagrams show solutions of three different...Ch. 16.6 - Practice ProblemATTEMPT Determine the pOH of a...Ch. 16.6 - Practice Problem BUILD Determine the pH of a...Ch. 16.6 - Prob. 1PPCCh. 16.6 - What is the pH of a 0.63-M solution of weak base...Ch. 16.6 - A 0.12-M solution of a weak base has a pH of 10.76...Ch. 16.6 - The diagrams show solutions of three different...Ch. 16.7 - Practice Problem ATTEMPT Calculate the hydroxide...Ch. 16.7 - Practice ProblemBUILD Calculate the hydronium ion...Ch. 16.7 - Practice ProblemCONCEPTUALIZE What is the value of...Ch. 16.7 - 16.7.1 Calculate the of the cyanide ion . (See...Ch. 16.7 - Which of the anions listed is the strongest base?...Ch. 16.7 - The diagrams show solutions of three different...Ch. 16.8 - Practice Problem ATTEMPT Calculate the pH of an...Ch. 16.8 - Practice ProblemBUILD Calculate the pOH of an...Ch. 16.8 - Practice Problem CONCEPTUALIZE Estimate the pH of...Ch. 16.8 - Calculate the equilibrium concentration of CO 3 2...Ch. 16.8 - What is the pH of a 0.40-M solution of phosphoric...Ch. 16.8 - List the molecular and ionic species in order of...Ch. 16.8 - Which is true for any polyprotic acid? a) K a2 > K...Ch. 16.9 - Practice Problem ATTEMPT Calculate the...Ch. 16.9 - Practice Problem BUILD Calculate the concentration...Ch. 16.9 - Practice Problem CONCEPTUALIZE Which of the plots...Ch. 16.10 - Practice Problem ATTEMPT Calculate the pOH of the...Ch. 16.10 - Practice Problem BUILD Calculate the pH of the...Ch. 16.10 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.10 - Calculate the pH of a 0.075-M solution of...Ch. 16.10 - Calculate the pH of a 0.082-M solution of...Ch. 16.10 - Prob. 3CPCh. 16.10 - Prob. 4CPCh. 16.10 - The diagrams represent solutions of three salts...Ch. 16.11 - Practice Problem ATTEMPT An aqueous solution of a...Ch. 16.11 - Practice Problem BUILD An aqueous solution of a...Ch. 16.11 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.12 - Practice Problem ATTEMPT Calculate the pH at of a...Ch. 16.12 - Practice ProblemBUILD Calculate the pH at 25°C of...Ch. 16.12 - Practice Problem CONCEPTUALIZE The diagrams show...Ch. 16.12 - 16.12.1 Which of the following cannot act as a...Ch. 16.12 - Which of the following is a Lewis acid but not a...Ch. 16.13 - Practice Problem ATTEMPT Determine the pH and...Ch. 16.13 - Prob. 1PPBCh. 16.13 - Practice Problem CONCEPTUALIZE Which of the...Ch. 16.14 - Practice Problem ATTEMPT Calculate the of a weak...Ch. 16.14 - Practice Problem BUILD Calculate the of a weak...Ch. 16.14 - Practice Problem CONCEPTUALIZE Calculate K a...Ch. 16.15 - Practice Problem ATTEMPT Calculate the pH at of a...Ch. 16.15 - Practice ProblemBUILD Calculate the pH at 25°C of...Ch. 16.15 - Practice Problem CONCEPTUALIZE The diagrams...Ch. 16.16 - Practice ProblemATTEMPT Determine the K b of a...Ch. 16.16 - Practice Problem BUILD Determine the of a weak...Ch. 16.16 - Practice Problem CONCEPTUALIZE Determine the...Ch. 16.17 - Practice Problem ATTEMPT Determine (a) K b of the...Ch. 16.17 - Practice ProblemBUILD Determine (a) K b of the...Ch. 16.17 - Practice problemCONCEPTUALIZE Fee each week acid...Ch. 16.18 - Practice Problem ATTEMPT Calculate the...Ch. 16.18 - Practice Problem BUILD Calculate the...Ch. 16.18 - Practice ProblemCONCEPTURALIZE Which of the...Ch. 16.19 - Practice ProblemATTEMPT Indicate which is the...Ch. 16.19 - Practice Problem BUILD Based on the information in...Ch. 16.19 - Prob. 1PPCCh. 16.20 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.20 - Practice ProblemBUILD Determine the concentration...Ch. 16.20 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.21 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.21 - Practice ProblemBUILD Determine the concentration...Ch. 16.21 - Practice Problem CONCEPTUALIZE Which of the...Ch. 16.22 - Practice Problem ATTEMPT Predict whether a 0.10-M...Ch. 16.22 - Prob. 1PPBCh. 16.22 - Prob. 1PPCCh. 16.23 - Practice ProblemATTEMPT Identify the Lewis acid...Ch. 16.23 - Practice Problem BUILD Write formulas for the...Ch. 16.23 - Practice Problem CONCEPTUALIZE Which of the...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - 16.2 Determine pH at the equivalence point in the...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - 16.4 Determine pH at the equivalence point in the...Ch. 16 - Define Brønsted acids and bases. Give an example...Ch. 16 - For a species to act as a Brønsted base, an atom...Ch. 16 - 16.3 Classify each of the following species as a...Ch. 16 - Identify the acid-base conjugate pairs in each of...Ch. 16 - 16.5 Write the formulas of the conjugate bases of...Ch. 16 - Write the formula for the conjugate acid of each...Ch. 16 - Which of the following could represent a Brønsted...Ch. 16 - 16.8 Oxalic acid has the following structure: An...Ch. 16 - Rite the equilibrium expression for the...Ch. 16 - 16.10 In Section 15.3 we learned that when we...Ch. 16 - 16.11 The equilibrium constant for the...Ch. 16 - 16.12 Define the term amphoteric. Ch. 16 - 16.13 Compare the magnitudes of in aqueous...Ch. 16 - Calculate the OH - concentration in an aqueous...Ch. 16 - 16.15 Calculate the concentration in an aqueous...Ch. 16 - The value of K w at 50°C is 5.48 × 10 − 14 ....Ch. 16 - The value of K w at 100°C is 5.1 × 3 10 − 13 ....Ch. 16 - Prob. 18QPCh. 16 - Prob. 19QPCh. 16 - Prob. 20QPCh. 16 - Prob. 21QPCh. 16 - Prob. 22QPCh. 16 - Calculate the concentration of OH- ions in a 1 .4...Ch. 16 - Prob. 24QPCh. 16 - 16.25 Calculate the pH of each of the following...Ch. 16 - Calculate the pH of each of the following...Ch. 16 - Prob. 27QPCh. 16 - Prob. 28QPCh. 16 - 16.29 The pOH of a solution is 9.40 at . Calculate...Ch. 16 - Prob. 30QPCh. 16 - Prob. 31QPCh. 16 - 16.32 A solution is made by dissolving 18.4 g of ...Ch. 16 - Prob. 33QPCh. 16 - Prob. 34QPCh. 16 - Prob. 35QPCh. 16 - Prob. 36QPCh. 16 - Prob. 37QPCh. 16 - Prob. 38QPCh. 16 - Prob. 39QPCh. 16 - 16.40 Calculate the concentration of in a...Ch. 16 - Calculate the concentration of HNO 3 in a solution...Ch. 16 - Prob. 42QPCh. 16 - Prob. 43QPCh. 16 - Prob. 44QPCh. 16 - Prob. 45QPCh. 16 - Explain what is meant by the strength of an acid.Ch. 16 - Prob. 47QPCh. 16 - Prob. 48QPCh. 16 - Why do we normally not quote K a values for strong...Ch. 16 - Which of the following solutions has the highest...Ch. 16 - Without referring to the text, write the formulas...Ch. 16 - In biological and medical applications, it is...Ch. 16 - 16.53 The for benzoic acid is Calculate the pH...Ch. 16 - The K a for hydrofluoric acid is 7.1 × 10 − 4 ....Ch. 16 - Calculate the pH of an aqueous solution at 25°C...Ch. 16 - Calculate the pH of an aqueous solution at 25°C...Ch. 16 - 16.57 Determine the percent ionization of the...Ch. 16 - Prob. 58QPCh. 16 - Prob. 59QPCh. 16 - Prob. 60QPCh. 16 - Calculate the K a of a weak acid if a 0.19 − M...Ch. 16 - Prob. 62QPCh. 16 - What is the original molarity of a solution of...Ch. 16 - What is the original molarity of a solution of a...Ch. 16 - 16.65 Which of the following statements are true...Ch. 16 - Prob. 66QPCh. 16 - Prob. 67QPCh. 16 - Compare the pH values for 0.10 − M solutions of...Ch. 16 - Which of the following has a higher pH: (a) 1 .0 M...Ch. 16 - Prob. 70QPCh. 16 - The pH of a 0.30-M solution of a weak base is...Ch. 16 - What is the original molarity of an aqueous...Ch. 16 - Prob. 73QPCh. 16 - Prob. 74QPCh. 16 - Prob. 75QPCh. 16 - Prob. 76QPCh. 16 - Prob. 77QPCh. 16 - Prob. 78QPCh. 16 - 16.79 Calculate for each of the following ions: ...Ch. 16 - Prob. 80QPCh. 16 - Prob. 81QPCh. 16 - Prob. 82QPCh. 16 - Prob. 83QPCh. 16 - Prob. 84QPCh. 16 - Compare the pH of a 0 .040 M HCl solution with...Ch. 16 - What are the concentrations of HSO 4, – SO 2– 4 ,...Ch. 16 - 16.87 Calculate the concentrations of Ch. 16 - Calculate the pH at 25°C of a 0.25 − M aqueous...Ch. 16 - 16.89 Calculate the pH at of a aqueous solution...Ch. 16 - The first and second ionization constants of a...Ch. 16 - Prob. 91QPCh. 16 - Prob. 92QPCh. 16 - Prob. 93QPCh. 16 - Prob. 94QPCh. 16 - Prob. 95QPCh. 16 - Prob. 96QPCh. 16 - Prob. 97QPCh. 16 - Define salt hydrolysis. Categorize salts according...Ch. 16 - 16.99 Explain why small, highly charged metal ions...Ch. 16 - Al 3+ is not a Brønsted acid, but Al( H 2 O ) 6 3+...Ch. 16 - Specify which of the following salts will undergo...Ch. 16 - Prob. 102QPCh. 16 - Calculate the pH of a 0 .42 M NH 4 Cl solution . (...Ch. 16 - Prob. 104QPCh. 16 - Prob. 105QPCh. 16 - Prob. 106QPCh. 16 - 16.107 Predict whether the following solutions are...Ch. 16 - A certain salt, MX (containing the M + and X -...Ch. 16 - Prob. 109QPCh. 16 - Predict whether a solution containing the salt K 2...Ch. 16 - Prob. 111QPCh. 16 - Prob. 112QPCh. 16 - Prob. 113QPCh. 16 - Prob. 114QPCh. 16 - Prob. 115QPCh. 16 - Prob. 116QPCh. 16 - Prob. 117QPCh. 16 - Prob. 118QPCh. 16 - Prob. 119QPCh. 16 - Prob. 120QPCh. 16 - Prob. 121QPCh. 16 - Prob. 122QPCh. 16 - Prob. 123QPCh. 16 - Prob. 124QPCh. 16 - Identity the Lewis acid and the Lewis base in the...Ch. 16 - Predict the direction that predominates in this...Ch. 16 - Prob. 127APCh. 16 - Prob. 128APCh. 16 - Calculate the pH and percent ionization of a 0 .88...Ch. 16 - 16.130 Calculate the pH of a 0.20 M ammonium...Ch. 16 - Prob. 131APCh. 16 - Prob. 132APCh. 16 - 16.133 Like water, liquid ammonia undergoes...Ch. 16 - Prob. 134APCh. 16 - A solution contains a weak monoprotic acid HA and...Ch. 16 - Prob. 136APCh. 16 - Prob. 137APCh. 16 - Prob. 138APCh. 16 - Prob. 139APCh. 16 - A 10.0-g sample of white phosphorus was burned in...Ch. 16 - Prob. 141APCh. 16 - Prob. 142APCh. 16 - Prob. 143APCh. 16 - Prob. 144APCh. 16 - 16.145 Give an example of (a) a weak acid that...Ch. 16 - Prob. 146APCh. 16 - Prob. 147APCh. 16 - Prob. 148APCh. 16 - When chlorine reacts with water, the resulting...Ch. 16 - Prob. 150APCh. 16 - Calculate the pH of a 2 .00 M NH 4 CN solution.Ch. 16 - Calculate the concentrations of all species in a 0...Ch. 16 - Prob. 153APCh. 16 - 16.154 Calculate the concentrations of all the...Ch. 16 - Prob. 155APCh. 16 - Calculate the pH of a solution that is 1.00 M HCN...Ch. 16 - How many grams of NaCN would you need to dissolve...Ch. 16 - A solution of formic acid ( HCOOH ) has a pH of...Ch. 16 - Calculate the pH of a 1-L solution containing...Ch. 16 - 16.160 A 1.87-g sample of Mg reacts with 80.0 mL...Ch. 16 - Prob. 161APCh. 16 - Prob. 162APCh. 16 - A 0.400 M formic acid ( HCOOH ) solution freezes...Ch. 16 - Prob. 164APCh. 16 - Prob. 165APCh. 16 - Prob. 166APCh. 16 - 16.167 Both the amide ion and the nitride ion ...Ch. 16 - Determine whether each of the following statements...Ch. 16 - Prob. 169APCh. 16 - Prob. 170APCh. 16 - Prob. 171APCh. 16 - 16.172 A typical reaction between an antacid and...Ch. 16 - Prob. 173APCh. 16 - 16.174 Hemoglobin is a blood protein that is...Ch. 16 - Tooth enamel is largely hydroxyapatite [ Ca 3 ( PO...Ch. 16 - Prob. 176APCh. 16 - Prob. 177APCh. 16 - About half of the hydrochloric acid produced...Ch. 16 - Prob. 179APCh. 16 - Prob. 180APCh. 16 - Prob. 181APCh. 16 - (a) Use VSEPR to predict the geometry of the...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...
Knowledge Booster
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
  • Chemistry: Principles and Practice
    Chemistry
    ISBN:9780534420123
    Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
    Publisher:Cengage Learning
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
  • Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Introductory Chemistry For Today
    Chemistry
    ISBN:9781285644561
    Author:Seager
    Publisher:Cengage
    Chemistry by OpenStax (2015-05-04)
    Chemistry
    ISBN:9781938168390
    Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
    Publisher:OpenStax
  • Chemistry: Principles and Practice
    Chemistry
    ISBN:9780534420123
    Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
    Publisher:Cengage Learning
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
    Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Introductory Chemistry For Today
    Chemistry
    ISBN:9781285644561
    Author:Seager
    Publisher:Cengage
    Chemistry by OpenStax (2015-05-04)
    Chemistry
    ISBN:9781938168390
    Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
    Publisher:OpenStax
    General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY