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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Textbook Question
Chapter 8, Problem 3P
8-15 Write an equation for the reaction that takes place when each base is added to water.
(a) LiOH
(b) (CH3)2NH
(c) Sr(OH)2
(d) CH3CH2NH2
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Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2O
(i) What is the Arrhenius definition of an acid, give an example
Why is NH3 considered a base according to Bronsted-Lowry theory?
CH COOH
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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- Rank the Acidity of the following sets of compounds. Give an explanation for the answers.arrow_forwardHydroxide (-OH) can react as a Brønsted–Lowry base (and remove a proton), or a Lewis base (and attack a carbon atom). (a) What organic product is formed when -OH reacts with the carbocation (CH3)3C+ as a Brønsted–Lowry base? (b) What organic product is formed when -OH reacts with (CH3)3C+ as a Lewis base?arrow_forwardWrite equations for the following acid-base reactions.(a) HCOOH + -CN (b) CH3COO- + CH3OH(c) (CH3)2CHOH + NaNH2 (d) NaOCH3 + HCNarrow_forward
- In the following reactions, indicate the acid, base, conjugate acid, and conjugate base. (a)HF + NH3→NH4++ F – (b)NaHSO4+ HClO3⇌H2SO4+ NaClO3arrow_forwardWrite an equilibrium equation showing how benzoic acid (C6H5COOH) acts like a weak acid and identify both pairs of conjugate acid-base partners.arrow_forwardComplete the equation for the following acid-base reaction. COOH OCH₂ Naegarrow_forward
- (a) Ionic Solids do not dissolve in non-polar solvents. (TRUE OR FALSE) (b) H3AsO4 is a weak acid. (TRUE OR FALSE) (c) Once a chemical reaction has come to equilibrium, the reaction comes to a complete halt.(TRUE OR FALSE)arrow_forward8-14 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_forwardIdentify the ion (or ions) present in each of the salts in Problem 10-98 that will undergo hydrolysis in aqueous solution.arrow_forward
- 8-33 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_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_forwardCH3NH2 is a (a)Arrhenius acid. (b)Arrhenius base. (c)Bronsted-Lowry acid. (c)Bronsted-Lowry base. (e)Louis base.arrow_forward
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