General, Organic, and Biological Chemistry
General, Organic, and Biological Chemistry
7th Edition
ISBN: 9781285853918
Author: H. Stephen Stoker
Publisher: Cengage Learning
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Chapter 10, Problem 10.86EP

(a)

Interpretation Introduction

Interpretation:

For a given solution, [OH-] pH, [H3O+] and whether the solution is acidic or basic has to be determined.

Concept Introduction:

pH:

pH is a scale used to specify how acidic or basic a solution is.  It ranges from 0-14. pH 7.0 is considered as neutral solution, pH more than 7.00 is taken as basic solution whereas pH less than 7.0 is considered as acidic solution (at 25oC). It is the measurement of activity of free H+ and OH- in solution.

  pH=log[H3O+]

  pOH=log[OH]

From ionization constant of water Kw=[H+][OH-]

Ionization constant of water at 25οC Kw=1×1014.

Less the pH, more is the acidity of the solution.

(a)

Expert Solution
Check Mark

Explanation of Solution

Given that,

  [OH-]=7.2×105

Then,

  Kw=[H+][OH-][H3O+][OH-]=1×10-14[H3O+]=1×10-147.2×10-5[H3O+]=1.4×10-10

  pH=log[H3O+]pH=log(1.4×10-10)pH=9.86

In this solution [OH-] is greater than [H3O+] and pH is more than 7.00. Hence this solution is a basic solution.

Hence this is a basic solution having pH=9.86 and [H3O+]=1.4×10-10M.

(b)

Interpretation Introduction

Interpretation:

For a given solution, [H3O+] the value of [OH-], pH and whether the solution is acid or basic that has to be determined.

Concept Introduction:

Concept Introduction:

pH:

pH is a scale used to specify how acidic or basic a solution is. It ranges from 0-14.  pH 7.0 is considered as neutral solution, pH more than 7.00 is taken as basic solution whereas pH less than 7.0 is considered as acidic solution (at 25oC). It is the measurement of activity of free H+ and OH- in solution.

  pH=log[H3O+]

  pOH=log[OH]

From ionization constant of water Kw=[H+][OH-]

Ionization constant of water at 25οC Kw=1×1014.

Less the pH more is the acidity of the solution.

(b)

Expert Solution
Check Mark

Explanation of Solution

Given that,

  [H3O+]=6.3×10-3M

Then,

  pH=log[H3O+]pH=log(6.3×10-3)pH=2.20

  Kw=[H+][OH-][H+][OH-]=1×1014[OH-]=1×10146.3×10-3[OH-]=1.6×10-12

In this solution [H3O+] is greater than [OH-] and pH is less than 7.00 and hence the solution is acidic.

Hence this is an acidic solution having [OH-]=1.6×10-12M and pH=2.20.

(c)

Interpretation Introduction

Interpretation:

For a given pH, the value of the [H3O+] and [OH-] of the solution has to be calculated along with the prediction that whether the solution is acidic or basic.

Concept Introduction:

pH:

pH is a scale used to specify how acidic or basic a solution is.  It ranges from 0-14. pH 7.0 is considered as neutral solution, pH more than 7.00 is taken as basic solution whereas pH less than 7.0 is considered as acidic solution (at 25oC). It is the measurement of activity of free H+ and OH- in solution.

  pH=log[H3O+]

  pOH=log[OH]

From ionization constant of water Kw=[H+][OH-]

Ionization constant of water at 25οC Kw=1×1014.

Less the pH more is the acidity of the solution.

(c)

Expert Solution
Check Mark

Explanation of Solution

Given that,

  pH=2.00

  pH=log[H3O+]log[H3O+]=2.00[H3O+]=102.00[H3O+]=1.00×102M

  Kw=[H+][OH-][H+][OH-]=1×1014[OH-]=1×10141.00×10-2[OH-]=1.00×10-12

As in this solution [H3O+] is greater than [OH-] and pH is less than 7.00 and hence the solution is acidic.

Hence this acidic solution have [OH-]=1.00×10-12M and [H3O+]=1.00×102M.

(d)

Interpretation Introduction

Interpretation:

For a given pH, the value of [OH-], [H3O+] and whether the solution is acid or basic that has to be determined.

Concept Introduction:

pH:

pH is a scale used to specify how acidic or basic a solution is.  It ranges from 0-14. pH 7.0 is considered as neutral solution, pH more than 7.00 is taken as basic solution whereas pH less than 7.0 is considered as acidic solution (at 25oC). It is the measurement of activity of free H+ and OH- in solution.

  pH=log[H3O+]

  pOH=log[OH]

From ionization constant of water Kw=[H+][OH-]

Ionization constant of water at 25οC Kw=1×1014.

Less the pH more is the acidity of the solution.

(d)

Expert Solution
Check Mark

Explanation of Solution

Given that,

  pH=12.00

Then,

  pH=log[H3O+]log[H3O+]=12.00[H3O+]=1012.00[H3O+]=1.00×1012

  Kw=[H+][OH-][H+][OH-]=1×1014[OH-]=1×10141.00×10-12[OH-]=1.00×10-2

In this solution [OH-] is greater than [H3O+] and pH more than 7.00. Hence this solution is a basic solution.

Hence this basic solution have [H3O+]=1.00×1012M and [OH-]=1.00×10-2M.

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Chapter 10 Solutions

General, Organic, and Biological Chemistry

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Write the...Ch. 10 - The ion HPO42 is an amphiprotic ion. Write the...Ch. 10 - Classify each of the following acids as...Ch. 10 - Classify each of the following acids as...Ch. 10 - Prob. 10.21EPCh. 10 - For each of the acids in Problem 10-19 indicate...Ch. 10 - Write chemical equations showing the individual...Ch. 10 - Write chemical equations showing the individual...Ch. 10 - Prob. 10.25EPCh. 10 - The formula for tartaric acid is preferably...Ch. 10 - Pyruvic acid, which is produced in metabolic...Ch. 10 - Oxaloacetic acid, which is produced in metabolic...Ch. 10 - Classify each of the acids in Problem 10-19 as a...Ch. 10 - Classify each of the acids in Problem 10-20 as a...Ch. 10 - For each of the following pairs of acids, indicate...Ch. 10 - For each of the following pairs of acids, indicate...Ch. 10 - For each of the following pairings of acid and...Ch. 10 - For each of the following pairings of acid and...Ch. 10 - The HCl in a 0.10 M HCl solution is 100%...Ch. 10 - The HNO3 in a 0.50 M HNO3 solution is 100%...Ch. 10 - The following four diagrams represent aqueous...Ch. 10 - Using the diagrams shown in Problem 10-37, which...Ch. 10 - Which of the terms weak, strong, monoprotic,...Ch. 10 - Which of the terms weak, strong, monoprotic,...Ch. 10 - Write the acid ionization constant expression for...Ch. 10 - Write the acid ionization constant expression for...Ch. 10 - Prob. 10.43EPCh. 10 - Write the base ionization constant expression for...Ch. 10 - Prob. 10.45EPCh. 10 - Using the acid ionization constant information...Ch. 10 - A 0.00300 M solution of an acid is 12% ionized....Ch. 10 - A 0.0500 M solution of a base is 7.5% ionized....Ch. 10 - Is the monoprotic acid Y or the monoprotic acid Z...Ch. 10 - Is the monoprotic acid Y or the monoprotic acid Z...Ch. 10 - Classify each of the following substances as an...Ch. 10 - Classify each of the following substances as an...Ch. 10 - Prob. 10.53EPCh. 10 - Indicate whether or not both members of each of...Ch. 10 - Prob. 10.55EPCh. 10 - Write a balanced equation for the dissociation...Ch. 10 - Indicate whether each of the following reactions...Ch. 10 - Indicate whether each of the following reactions...Ch. 10 - Without writing an equation, specify the molecular...Ch. 10 - Without writing an equation, specify the molecular...Ch. 10 - Write a balanced chemical equation to represent...Ch. 10 - Write a balanced chemical equation to represent...Ch. 10 - Prob. 10.63EPCh. 10 - Write a balanced molecular equation for the...Ch. 10 - Prob. 10.65EPCh. 10 - What is the molar hydronium ion concentration in...Ch. 10 - Indicate whether each of the solutions in Problem...Ch. 10 - Prob. 10.68EPCh. 10 - Prob. 10.69EPCh. 10 - Prob. 10.70EPCh. 10 - Prob. 10.71EPCh. 10 - Indicate whether each of the solutions in Problem...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - Calculate the pH of solutions with the following...Ch. 10 - What is the [H3O+] value in solutions with each of...Ch. 10 - What is the [H3O+] value in solutions with each of...Ch. 10 - Prob. 10.81EPCh. 10 - What is the molar hydronium ion concentration in...Ch. 10 - Prob. 10.83EPCh. 10 - Indicate whether each of the following samples is...Ch. 10 - Selected information about five solutions, each at...Ch. 10 - Prob. 10.86EPCh. 10 - Consider the following four solutions: (1) apple...Ch. 10 - Consider the following four biological solutions:...Ch. 10 - For each of the following pairs of solutions,...Ch. 10 - Prob. 10.90EPCh. 10 - Calculate the pKa value for each of the following...Ch. 10 - Calculate the pKa value for each of the following...Ch. 10 - Acid A has a pKa value of 4.23, and acid B has a...Ch. 10 - Acid A has a pKa value of 5.71, and acid B has a...Ch. 10 - If a weak acid has a pKa value of 8.73, what is...Ch. 10 - If a weak acid has a pKa value of 7.21, what is...Ch. 10 - Classify each of the following salts as a strong...Ch. 10 - Classify each of the following salts as a strong...Ch. 10 - Prob. 10.99EPCh. 10 - Identify the ion (or ions) present in each of the...Ch. 10 - Prob. 10.101EPCh. 10 - Prob. 10.102EPCh. 10 - Both ions in the salt ammonium cyanide (NH4CN)...Ch. 10 - Both ions in the salt ammonium acetate (NH4C2H3O2)...Ch. 10 - Arrange the following 0.10 M aqueous solutions in...Ch. 10 - Arrange the following 0.10 M aqueous solutions in...Ch. 10 - Predict whether each of the following pairs of...Ch. 10 - Predict whether each of the following pairs of...Ch. 10 - Identify the two active species in each of the...Ch. 10 - Identify the two active species in each of the...Ch. 10 - Prob. 10.111EPCh. 10 - Write an equation for each of the following...Ch. 10 - Prob. 10.113EPCh. 10 - Prob. 10.114EPCh. 10 - Prob. 10.115EPCh. 10 - A buffer solution has a pH value of 9.8. 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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY