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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Textbook Question
Chapter 8.11, Problem 8.11P
Problem 8-11
What is the pH of a boric acid buffer solution containing 0.25 moI/L of boric acid, H3BO3 and 0.50 mol/L of its conjugate base? See Table 8-3 for the pKaof boric acid.
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Problem 3A buffer made from which one of the acids below would be the best for a pH of 4.642?a) H2CO3 , Ka = 4.30e-7b) H2S, Ka = 9.10e-8c) CH3COOH , Ka = 1.75e-5d) H3PO4 , Ka = 7.52e-3
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Question 5
Which of the following mixtures would result in a buffered solution?
Mixing 100.0 mL of 0.100 MHC1 with 100.0 mL of 0.100 M NaOH.
Ⓒ Mixing 100.0 mL of 0.100 MNH3 (K=1.8 x 105) with 100.0 mL of 0.100 M NaOH.
Mixing 100.0 mL of 0.100 MHCI with 100.0 mL of 0.100 MNH3; (K=1.8×10)
Mixing 50.0 mL of 0.100 MHCI with 100.0 mL of 0.100 MNH3 (K₂=1.8 × 10-).
O At least two of the above mixtures would result in a buffered solution.
Chapter 17 problem 5PS
What is the ph of the solution of 30.0ml of 0.015 M KOH to 50.0ml of 0.015 M benzoic acid?
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. 8.2PCh. 8.5 - Prob. 8.3PCh. 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. 8.12PCh. 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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- EXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.arrow_forwardProblem 8-8 The [OH-] of a solution is M. What are the pOH and pH of this solution?arrow_forwardQUESTION 16 A solution is prepared by adding excess CaBr2 (Ksp = 3.2×10-11] to water, what is the [Ca2+] at equilibrium? (3 s.f, and express in decimals not scientific notation)arrow_forward
- Saved 3 attempts left Check my work Be sure to answer all parts A 10.0-mL solution of 0.870 M NH, is titrated with a 0.290 M HCl solution. Calculate the pH after the following additions of the HCI solution: (a) 0.00 mL (b) 10.0 mL (c) 30.0 mL (d) 40.0 mL ( Prev 7 of 12 Next > MacBook Proarrow_forwardPROBLEM 3 Calculate the pH of a 0.300 M NaF solution. The Ka value for HF is 7.20 x 10-4. Will the X solution be acidic, basic, or neutral? Explain.arrow_forwardReview I Constants I Periodic Table A 4.50 mL sample of an H3 PO4 solution of unknown concentration is titrated with a 1.050x10-2 M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. Part A What is the concentration of the unknown H3PO4 solution? want to reference (Pages 494 - 497) You may Section 14.6 while completing this problem. Express your answer with the appropriate units. HA **** Value Unitsarrow_forward
- 15 Question e See page 810 Calculate the change in pH when 0.254 mol H* is added to 1.00 L of each of the following buffers. 1st attempt Part 1 l See Periodic Table O See Hint If the final pH is lower than the initial, your answer should be a negative number. a 0.560 M solution of pyridine (py) containing 0.500 M pyH* change in pH = Part 2 If the final pH is lower than the initial, your answer should be a negative number. a 0.560 M solution of aniline (an) containing 0.920 M anH* change in pH =arrow_forwardPROBLEM 4: Calculate the pH of the following: a. 0.520 M in sodium formate and 0.100 M in formic acid b. 75 ml of 0.050 M in pyridine and 125 mL of 0.10 M in pyridinium chloridearrow_forwardPROBLEM 4: In the titration of 100 ml of weak acid, 27.63ml of 0.09381M of needed to reach the equivalence point. NaOH was Consequently, the pH at equivalence point was measured and the value was 10.99. Calculate the pH if the volume of the NAOH added is less than 8.16ml of the volume at equivalence point.arrow_forward
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