Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
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Chapter 8, Problem 8.107P

8-107 Following are pH ranges for several human biological materials. From the pH at the midpoint of each range, calculate the corresponding [H3O+]. Which materials are acidic, which are basic, and which are neutral? (a) Milk, pH 6.6-7.6

(b) Gastric contents, pH 1.0-3.0

(c) Spinal fluid, pH 7.3-7.5

(d) Saliva, pH 6.5-7.5

(e) Urine, pH 4.8-8.4

(f) Blood plasma, pH 7.35-7.45

(g) Feces, pH 4.6-8.4

(h) Bile, pH 6.8-7.0

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Basic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of milk is in the range 6.6-7.6. The midpoint of the pH range of milk is given by the below formula:

The midpoint of pH range = 6.6+7.62                                          = 7.1

Now, we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                7.1 = log[H3O+]antilog(7.1)=[H3O+]        [H3O+] = antilog(7.1)         [H3O+] = 7.9×108M

Thus, the concentration of hydronium ion [H3O+] = 7.9×108M. Hence, the given solution is basic, as the concentration of [H3 O+ ] is less than 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Acidic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Gastric contents is in the range 1.0-3.0. The midpoint of the pH range of Gastric contents is given by the below formula:

The midpoint of pH range = 1.0+3.02                                          = 2.0

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                2.0 = log[H3O+]antilog(2.0)=[H3O+]        [H3O+] = antilog(2.0)         [H3O+] = 1.0×102M

Thus, the concentration of hydronium ion [H3O+] = 1.0×102M. Hence, the given solution is acidic, as the concentration of [H3 O+ ] is more than 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(c)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Basic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Spinal Fluids is in the range 7.3-7.5. The midpoint of the pH range of Spinal Fluids is given by the below formula:

The midpoint of pH range = 7.3+7.52                                          = 7.4

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                7.4 = log[H3O+]antilog(7.4)=[H3O+]        [H3O+] = antilog(7.4)         [H3O+] = 4.0×108M

Thus, the concentration of hydronium ion [H3O+] = 4.0×108M. Hence, the given solution is basic, as the concentration of [H3 O+ ] is less than 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(d)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Neutral.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the saliva is in the range 6.5-7.5. The midpoint of the pH range of saliva is given by the below formula:

The midpoint of pH range = 6.5+7.52                                          = 7.0

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                7.0 = log[H3O+]antilog(7.0)=[H3O+]        [H3O+] = antilog(7.0)         [H3O+] = 1.0×107M

Thus, the concentration of hydronium ion [H3O+] = 1.0×107M. Hence, the given solution is neutral, as the concentration of [H3 O+ ] is equal to 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(e)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Acidic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Urine is in the range 4.8-8.4. The midpoint of the pH range of Urine is given by the below formula:

The midpoint of pH range = 4.8+8.42                                          = 6.6

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                7.0 = log[H3O+]antilog(6.6)=[H3O+]        [H3O+] = antilog(6.6)         [H3O+] = 2.5×107M

Thus, the concentration of hydronium ion [H3O+] =2.5×107M. Hence, the given solution is acidic, as the concentration of [H3 O+ ] is greater to 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(f)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

basic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Blood Plasma is in the range 7.35-7.45. The midpoint of the pH range of Blood Plasma is given by the below formula:

The midpoint of pH range = 7.35+7.452                                          = 7.4

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                7.4 = log[H3O+]antilog(7.4)=[H3O+]        [H3O+] = antilog(7.4)         [H3O+] = 4.0×108M

Thus, the concentration of hydronium ion [H3O+] = 4.0×108M. Hence, the given solution is basic, as the concentration of [H3 O+ ] is less than 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(g)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

acidic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Feces is in the range 4.6-8.4. The midpoint of the pH range of Feces is given by the below formula:

The midpoint of pH range = 4.6+8.42                                          = 6.5

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                6.5 = log[H3O+]antilog(6.5)=[H3O+]        [H3O+] = antilog(6.5)         [H3O+] = 3.2×107M

Thus, the concentration of hydronium ion [H3O+] = 3.2×107M. Hence, the given solution is acidic, as the concentration of [H3 O+ ] is greater than 1.0×107.

Expert Solution
Check Mark
Interpretation Introduction

(h)

Interpretation:

The concentration of hydronium ion for given pH value should be calculated and it should be identified as acidic, basic or neutral.

Concept Introduction:

A substance is said to be acidic if it gives hydrogen ions in the aqueous solution and it is basic if gives hydroxide ions. In pH scale, the substances with pH below 7 or more than 0 are said to be acidic in nature and substances with pH greater than or below 14 are basic in nature.

The pH of solution can be calculated by taking negative log of hydrogen or hydronium ion concentration.

pH=log[H3O+]

Here, [H3O+] is concentration of hydronium ion in the solution.

Answer to Problem 8.107P

Acidic.

Explanation of Solution

Given Information:

A solution is acidic if its pH is less than 7 and the [H3O+] is greater than 1.0×107

A solution is basic if its pH is greater than 7 and the [H3O+] is less than 1.0×107

A solution is acidic if its pH is equal to 7 and the [H3O+] = [OH] is equal to 1.0×107

The pH of the Bile is in the range 6.8-7.0. The midpoint of the pH range of Bile is given by the below formula:

The midpoint of pH range = 6.8+7.02                                          = 6.9

Now we need to determine the concentration of hydronium ion. The concentration of the hydronium ion can be calculated as shown below:

                pH  = log[H3O+]                6.9 = log[H3O+]antilog(6.9)=[H3O+]        [H3O+] = antilog(6.9)         [H3O+] = 1.25×107M

Thus, the concentration of hydronium ion [H3O+] = 1.25×107M. Hence, the given solution is acidic, as the concentration of [H3 O+ ] is greater than 1.0×107.

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Chapter 8 Solutions

Introduction to General, Organic and Biochemistry

Ch. 8.11 - Problem 8-11 What is the pH of a boric acid buffer...Ch. 8.12 - Prob. 8.12PCh. 8 - 8-13 Define (a) an Arrhenius acid and (b) an...Ch. 8 - 8-14 Write an equation for the reaction that takes...Ch. 8 - 8-15 Write an equation for the reaction that takes...Ch. 8 - 8-16 For each of the following, tell whether the...Ch. 8 - 8-17 For each of the following, tell whether the...Ch. 8 - 8-18 Which of these acids are monoprotic, which...Ch. 8 - 8-19 Define (a) a Brønsted—Lowry acid and (b) a...Ch. 8 - 8-20 Write the formula for the conjugate base of...Ch. 8 - 8-21 Write the formula for the conjugate base of...Ch. 8 - Prob. 8.22PCh. 8 - Prob. 8.23PCh. 8 - Prob. 8.24PCh. 8 - 8-25 Draw the acid and base reactions for the...Ch. 8 - Prob. 8.26PCh. 8 - Prob. 8.27PCh. 8 - 8-28 Will carbon dioxide be evolved as a gas when...Ch. 8 - Prob. 8.29PCh. 8 - Prob. 8.30PCh. 8 - Prob. 8.31PCh. 8 - Prob. 8.32PCh. 8 - 8-33 Write an equation for the reaction of HCI...Ch. 8 - 8-34 When a solution of sodium hydroxide is added...Ch. 8 - 8-35 Given the following values of [H3O+),...Ch. 8 - 8-36 Given the following values of [OH-],...Ch. 8 - 8-37 What is the pH of each solution given the...Ch. 8 - 8-38 What is the pH and pOH of each solution given...Ch. 8 - 8-39 What is the pH of each solution given the...Ch. 8 - Prob. 8.40PCh. 8 - 8-41 What is the [OH-] and pOH of each solution?...Ch. 8 - Prob. 8.42PCh. 8 - 8-43 What is the molarity of a solution made by...Ch. 8 - 8-44 What is the molarity of a solution made by...Ch. 8 - 8-45 Describe how you would prepare each of the...Ch. 8 - 8-46 If 25.0 mL of an aqueous solution of H2SO4...Ch. 8 - 8-47 A sample of 27.0 mL of 0.310 M NaOH is...Ch. 8 - 8-48 A 0.300 M solution of H2SO4 was used to...Ch. 8 - 8-49 A solution of NaOH base was titrated with...Ch. 8 - 8-50 The usual concentration of HCO3- ions in...Ch. 8 - 8-51 What is the end point of a titration?Ch. 8 - Prob. 8.52PCh. 8 - 8-53 Write equations to show what happens when, to...Ch. 8 - 8-54 Write equations to show what happens when, to...Ch. 8 - 8-55 We commonly refer to a buffer as consisting...Ch. 8 - Prob. 8.56PCh. 8 - Prob. 8.57PCh. 8 - 8-58 What is the connection between buffer action...Ch. 8 - Prob. 8.59PCh. 8 - 8-60 How is the buffer capacity affected by the...Ch. 8 - 8-61 Can 100 of 0.1 M phosphate buffer at pH 7.2...Ch. 8 - 8-62 What is the pH of a buffer solution made by...Ch. 8 - 8-63 The pH of a solution made by dissolving 1.0...Ch. 8 - Prob. 8.64PCh. 8 - Prob. 8.65PCh. 8 - 8-66 Calculate the pH of an aqueous solution...Ch. 8 - Prob. 8.67PCh. 8 - 8-68 If you have 100 mL of a 0.1 M buffer made of...Ch. 8 - Prob. 8.69PCh. 8 - Prob. 8.70PCh. 8 - 8-71 Explain why you do not need to know the...Ch. 8 - Prob. 8.72PCh. 8 - Prob. 8.73PCh. 8 - Prob. 8.74PCh. 8 - Prob. 8.75PCh. 8 - 8-76 (Chemical Connections 8B) Name the most...Ch. 8 - Prob. 8.77PCh. 8 - Prob. 8.78PCh. 8 - 8-79 (Chemical Connections 8D) Another form of the...Ch. 8 - Prob. 8.80PCh. 8 - Prob. 8.81PCh. 8 - 8-82 Assume that you have a dilute solution of HCI...Ch. 8 - Prob. 8.83PCh. 8 - Prob. 8.84PCh. 8 - Prob. 8.85PCh. 8 - 8-86 Following are three organic acids and the...Ch. 8 - 8-87 The pKavalue of barbituric acid is 5.0. If...Ch. 8 - Prob. 8.88PCh. 8 - Prob. 8.89PCh. 8 - Prob. 8.90PCh. 8 - Prob. 8.91PCh. 8 - Prob. 8.92PCh. 8 - 8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI...Ch. 8 - 8-94 Suppose you wish to make a buffer whose pH is...Ch. 8 - Prob. 8.95PCh. 8 - 8-96 Suppose you want to make a CH3COOH/CH3COO-...Ch. 8 - Prob. 8.97PCh. 8 - 8-98 When a solution prepared by dissolving 4.00 g...Ch. 8 - Prob. 8.99PCh. 8 - Prob. 8.100PCh. 8 - 8-101 Suppose you have an aqueous solution...Ch. 8 - Prob. 8.102PCh. 8 - 8-103 Suppose you have a phosphate buffer...Ch. 8 - Prob. 8.104PCh. 8 - Prob. 8.105PCh. 8 - Prob. 8.106PCh. 8 - 8-107 Following are pH ranges for several human...Ch. 8 - 8-108 What is the ratio of HPO42-/H2PO4- in a...Ch. 8 - Prob. 8.109PCh. 8 - 8-110 A concentrated hydrochloric acid solution...Ch. 8 - 8-111 The volume of an adult's stomach ranges from...Ch. 8 - 8-112 Consider an initial 0.040 M hypobromous acid...Ch. 8 - Prob. 8.113PCh. 8 - Prob. 8.114PCh. 8 - 8-115 When a solution prepared by dissolving 0.125...Ch. 8 - 8-116 A railroad tank car derails and spills 26...Ch. 8 - Prob. 8.117P
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