Introduction to General, Organic and Biochemistry
12th Edition
ISBN: 9780357119303
Author: Bettelheim, Frederick A., Brown, William H., Campbell, Mary K., FARRELL, Shawn O., Torres, Omar
Publisher: Cengage Learning
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Chapter 8, Problem 30P
Interpretation Introduction
Interpretation:
Interpret the purpose for
Concept Introduction:
Titration is the technique required to determine the concentration of unknown solution in presence of solution which concentration is known. The concentration of unknown solution can be determined as follows:
M1 V1 =M2 V2.
M1 is the molarity of known solution.
V1 is the volume of known solution.
M2 is the molarity of unknown solution.
V2 is the volume of unknown solution.
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Chapter 8 Solutions
Introduction to General, Organic and Biochemistry
Ch. 8.3 - Problem 8-1 Draw the acid and base reactions for...Ch. 8.4 - Prob. 8.2QCCh. 8.5 - Prob. 8.3QCCh. 8.5 - Problem 8-4 Which is the stronger acid? (a)...Ch. 8.6 - Problem 8-5 Write the balanced net ionic equation...Ch. 8.7 - Problem 8-6 The [OH-] of an aqueous solution is M....Ch. 8.8 - Problem 8-7 (a) The [H3O+] of an acidic solution...Ch. 8.8 - Problem 8-8 The [OH-] of a solution is M. What are...Ch. 8.9 - Problem 8-9 Calculate the concentration of an...Ch. 8.10 - Problem 8-10 What is the pH of a buffer solution...
Ch. 8.11 - Problem 8-11 What is the pH of a boric acid buffer...Ch. 8.12 - Prob. 8.12QCCh. 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. 10PCh. 8 - Prob. 11PCh. 8 - Prob. 12PCh. 8 - 8-25 Draw the acid and base reactions for the...Ch. 8 - Prob. 14PCh. 8 - Prob. 15PCh. 8 - 8-28 Will carbon dioxide be evolved as a gas when...Ch. 8 - Prob. 17PCh. 8 - Prob. 18PCh. 8 - Prob. 19PCh. 8 - Prob. 20PCh. 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. 28PCh. 8 - 8-41 What is the [OH-] and pOH of each solution?...Ch. 8 - Prob. 30PCh. 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. 40PCh. 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. 44PCh. 8 - Prob. 45PCh. 8 - 8-58 What is the connection between buffer action...Ch. 8 - Prob. 47PCh. 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. 52PCh. 8 - Prob. 53PCh. 8 - Prob. 54PCh. 8 - Prob. 55PCh. 8 - 8-66 Calculate the pH of an aqueous solution...Ch. 8 - Prob. 57PCh. 8 - 8-68 If you have 100 mL of a 0.1 M buffer made of...Ch. 8 - Prob. 59PCh. 8 - Prob. 60PCh. 8 - 8-71 Explain why you do not need to know the...Ch. 8 - Prob. 62PCh. 8 - Prob. 63PCh. 8 - Prob. 64PCh. 8 - Prob. 65PCh. 8 - 8-76 (Chemical Connections 8B) Name the most...Ch. 8 - Prob. 67PCh. 8 - Prob. 68PCh. 8 - 8-79 (Chemical Connections 8D) Another form of the...Ch. 8 - Prob. 70PCh. 8 - Prob. 71PCh. 8 - 8-82 Assume that you have a dilute solution of HCI...Ch. 8 - Prob. 73PCh. 8 - Prob. 74PCh. 8 - Prob. 75PCh. 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. 78PCh. 8 - Prob. 79PCh. 8 - Prob. 80PCh. 8 - Prob. 81PCh. 8 - Prob. 82PCh. 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. 85PCh. 8 - 8-96 Suppose you want to make a CH3COOH/CH3COO-...Ch. 8 - Prob. 87PCh. 8 - 8-98 When a solution prepared by dissolving 4.00 g...Ch. 8 - Prob. 89PCh. 8 - Prob. 90PCh. 8 - 8-101 Suppose you have an aqueous solution...Ch. 8 - Prob. 92PCh. 8 - 8-103 Suppose you have a phosphate buffer...Ch. 8 - Prob. 94PCh. 8 - Prob. 95PCh. 8 - Prob. 96PCh. 8 - 8-107 Following are pH ranges for several human...Ch. 8 - Prob. 98PCh. 8 - Prob. 99PCh. 8 - 8-108 What is the ratio of HPO42-/H2PO4- in a...Ch. 8 - Prob. 101PCh. 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. 105PCh. 8 - Prob. 106PCh. 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. 109PCh. 8 - Prob. 110PCh. 8 - Prob. 111P
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- 8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.arrow_forward8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?arrow_forward8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water is titrated with 0.200 M NaOH, 30.0 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown diprotic acid?arrow_forward
- 8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.arrow_forward8-58 What is the connection between buffer action and Le Chatelier's principle?arrow_forward8-53 Write equations to show what happens when, to a buffer solution containing equimolar amounts of CH3COOH and CH3COO-, we add: (a) H3O (b) OH-arrow_forward
- What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.arrow_forwardWhen might a pH meter be better than an indicator to determine the end point of an acid-base titration?arrow_forward8-47 A sample of 27.0 mL of 0.310 M NaOH is titrated with 0.740 M H2SO4. How many milliliters of the H2SO4 solution are required to reach the end point?arrow_forward
- 8-14 Write an equation for the reaction that takes place when each acid is added to water. (a) HNO3 (b) HBr (c) HCO3- (d) NH4+arrow_forward8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4 and solid Na2HPO4. How many grams of the solid Na2HPO4 must be added to the stock solution to accomplish this task? (Assume that the volume remains 1 L.)arrow_forward8-62 What is the pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1 L of water?arrow_forward
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