Bundle: Introduction to General, Organic and Biochemistry, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781305705159
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 8.87P
8-87 The pKavalue of barbituric acid is 5.0. If the H3O+ and barbiturate ion concentrations are each 0.0030 M, what is the concentration of the undissociated barbituric acid?
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c9
Overall: What is the concentration of the
HPO42- ion in the 0.50 M solution of
phosphoric acid?
The previous dissociation created H+ and H₂PO4-
in the concentrations shown in the RICE table.
R H₂PO HPO ² + H+
I
0.058
0
0.058
+ X
X
C
- X
E 0.058 - x
Ka₂ = 6.23 x 10-8
a2
+ X
0.058 + x
[HPO 2] = [?] x 10⁰²] M
Coefficient (green)
Exponent (yellow)
Enter
Arsenic acid, H3AsO4, is used industrially to manufacture insecticides. Arsenic acid is a polyprotic acid with Ka1 = 2.5 x 10-4, Ka2 = 5.6 x10-8, and Ka3 = 3.0 x 10-13. What is the concentration of the HAsO42- and AsO43- in a solution whose initial arsenic acid concentration was 0.35 M?
Chapter 8 Solutions
Bundle: Introduction to General, Organic and Biochemistry, 11th + OWLv2, 4 terms (24 months) Printed Access Card
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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- 8-51 What is the end point of a titration?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_forward8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?arrow_forward
- The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous exercise, is 1.36104. If 20.0 g of lactic acid is used to make a solution with a volume of 1.00 L, what is the concentration of hydronium ion in the solution?arrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forward8-34 When a solution of sodium hydroxide is added to a solution of ammonium carbonate and then heated, ammonia gas, NH3 is released. Write a net ionic equation for this reaction. Both NaOH and (NH4)2CO3 exist as dissociated ions in aqueous solution.arrow_forward
- 8-103 Suppose you have a phosphate buffer (H2PO4-/HPO42-) of pH 7.21. If you add more solid NaH2PO4 to this buffer, would you expect the pH of the buffer to increase, decrease, or remain unchanged? Explain.arrow_forwardTwo strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?arrow_forwardDefine or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw equilibrium constant d. pH e. pOH f. pKw Give the conditions for a neutral aqueous solution at 25C, in terms of [H+], pH, and the relationship between [H+] and [OH]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H+], and [OH]? As a solution becomes more basic, what happens to pH, pOH, [H+], and [OH]?arrow_forward
- Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 = 8.5 107 N2H5+(aq) + H2O() N2H62+(aq) + OH(aq) Kb2 = 8.9 1016 (a) What is the concentration of OH, N2H5+ and N2H62+ in a 0.010M aqueous solution of hydrazine? (b) What is the pH of the 0.010M solution hydrazine?arrow_forward8-33 Write an equation for the reaction of HCI with each compound. Which are acid—base reactions? Which are redox reactions? (a) Na2CO3 (b) Mg (c) NaOH (d) Fe2O3 (e) NH3 (f) CH3NH2 (g) NaHCO3 (h) AIarrow_forward8-50 The usual concentration of HCO3- ions in blood plasma is approximately 24 millimoles per liter (mmol/L). How would you make up 1.00 L of a solution containing this concentration of HCO3- ions?arrow_forward
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