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Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759

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BuyFindarrow_forward

Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759
Chapter 8, Problem 8.66P
Textbook Problem
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8-66 Calculate the pH of an aqueous solution containing the following:

(a) 0.80 M lactic acid and 0.40 M lactate ion

(b) 0.30 M and 1.50 M NH4+

Interpretation Introduction

(a)

Interpretation:

The pH of an aqueous solution containing 0.80 m lactic acid and 0.40 m lactate ion should be calculated.

Concept Introduction:

The pH of buffer can be calculated using the Henderson-Hasselbalch equation as follows:

pH=pKa+log[A][HA]

Here, pH is negative log of hydrogen ion, pKa is negative log of acid dissociation constant, [A] is concentration of conjugate base and [HA] is concentration of acid.

Explanation of Solution

Given Information:

The concentration of lactic acid lactate ion is 0.80 m and 0.40 m respectively.

Calculation:

For the given buffer, the Henderson-Hasselbalch equation is as follows:

pH=pKa+log[lactate ion][lactic acid]

The pKa value of lactic acid is 3

Interpretation Introduction

(b)

Interpretation:

The pH of an aqueous solution containing 0.30 m NH3 and 1.50 m NH4+ should be calculated.

Concept Introduction:

The pH of buffer can be calculated using the Henderson-Hasselbalch equation as follows:

pH=pKa+log[A][HA]

Here, pH is negative log of hydrogen ion, pKa is negative log of acid dissociation constant, [A] is concentration of conjugate base and [HA] is concentration of acid.

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Chapter 8 Solutions

Introduction to General, Organic and Biochemistry
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Ch. 8.11 - Problem 8-11 What is the pH of a boric acid buffer...Ch. 8.12 - Problem 8-12 What is the pH of a solution made by...Ch. 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 - 8-22 Write the formula for the conjugate acid of...Ch. 8 - 8-23 Write the formula for the conjugate acid of...Ch. 8 - 8-24 Show how the amphiprotic ion hydrogen...Ch. 8 - 8-25 Draw the acid and base reactions for the...Ch. 8 - 8-26 For each equilibrium, label the stronger...Ch. 8 - 8-27 For each equilibrium, label the stronger...Ch. 8 - 8-28 Will carbon dioxide be evolved as a gas when...Ch. 8 - 8-29 Which has the larger numerical value? (a) The...Ch. 8 - 8-30 In each pair, select the stronger acid. (a)...Ch. 8 - 8-31 Which solution will be more acidic; that is,...Ch. 8 - 8-32 Which solution will be more acidic; that is,...Ch. 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 - 8-40 Which is more acidic, a beer with or a wine...Ch. 8 - 8-41 What is the [OH-] and pOH of each solution?...Ch. 8 - 8-42 What is the purpose of an acid—base...Ch. 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 - 8-52 Why does a titration not tell us the acidity...Ch. 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 - 8-56 What is meant by buffer capacity?Ch. 8 - 8-57 How can you change the pH of a buffer? How...Ch. 8 - 8-58 What is the connection between buffer action...Ch. 8 - 8-59 Give two examples of a situation where you...Ch. 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 - 8-64 Show that when the concentration of the weak...Ch. 8 - 8-65 Show that the pH of a buffer is 1 unit higher...Ch. 8 - 8-66 Calculate the pH of an aqueous solution...Ch. 8 - 8-67 The pH of 0.10 M HCI is 1.0. When 0.10 mol of...Ch. 8 - 8-68 If you have 100 mL of a 0.1 M buffer made of...Ch. 8 - 8-69 Write an equation showing the reaction of...Ch. 8 - 8-70 What is the pH of a solution that is 0.1 M in...Ch. 8 - 8-71 Explain why you do not need to know the...Ch. 8 - 8-72 If you have a HEPES buffer at pH 4.75, will...Ch. 8 - 8-73 Which of the compounds listed in Table 8-6...Ch. 8 - 8-74 Which of the compounds listed in Table 8-6...Ch. 8 - 8-75 (Chemical Connections 8A) Which weak base is...Ch. 8 - 8-76 (Chemical Connections 8B) Name the most...Ch. 8 - 8-77 (Chemical Connections 8C) What causes (a)...Ch. 8 - 8-78 (Chemical Connections 8D) Explain how the...Ch. 8 - 8-79 (Chemical Connections 8D) Another form of the...Ch. 8 - 8-80 4-Methylphen01, CH3C6H4OH is only slightly...Ch. 8 - 8-81 Benzoic acid, C6H5COOH is only slightly...Ch. 8 - 8-82 Assume that you have a dilute solution of HCI...Ch. 8 - 8-83 Which of the two solutions from Problem 8-82...Ch. 8 - 8-84 What is the pH of a solution if you mix 300....Ch. 8 - 8-85 What is the molarity of a solution made by...Ch. 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 - 8-88 If pure water self-ionizes to give H3O+ and...Ch. 8 - 8-89 Can an aqueous solution have a pH of zero?...Ch. 8 - 8-90 If an acid, HA, dissolves in water such that...Ch. 8 - 8-91 A scale of Kbvalues for bases could be set up...Ch. 8 - 8-92 Do a 1.0 M CH3COOH solution and a 1.0 M HCI...Ch. 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 - 8-95 In the past, boric acid was used to rinse an...Ch. 8 - 8-96 Suppose you want to make a CH3COOH/CH3COO-...Ch. 8 - 8-97 For an acid—base reaction, one way to...Ch. 8 - 8-98 When a solution prepared by dissolving 4.00 g...Ch. 8 - 8-99 Write equations to show what happens when, to...Ch. 8 - 8-100 If we add 0.10 mol of NH3 to 0.50 mol of HCI...Ch. 8 - 8-101 Suppose you have an aqueous solution...Ch. 8 - 8-102 The pH of a 0.10 M solution of acetic acid...Ch. 8 - 8-103 Suppose you have a phosphate buffer...Ch. 8 - 8-104 Suppose you have a bicarbonate buffer...Ch. 8 - 8-105 A student pulls a bottle of TRIS offa shelf...Ch. 8 - 8-106 Unless under pressure, carbonic acid in...Ch. 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 - 8-109 What is the ratio of HPO42-/H2PO4- in a...Ch. 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 - 8-113 A 1.00 L sample of HE gas at 20.0°C and...Ch. 8 - 8-114 A laboratory student is given an alloy or...Ch. 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 - 8-117 Over the past 250 years, the average...

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