Chapter 10 - Fundamental of General, Organic and Biological Chem PDF

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Fundamentals of General, Organic, and Biological Chemistry, 8e (McMurry) Chapter 10 Acids and Bases 1) Which statement concerning Arrhenius acid-base theory is not correct? A) An Arrhenius acid produces hydrogen ions in water solution. B) An Arrhenius base produces hydroxide ions in water solution. C) A neutralization reaction produces water plus a salt. D) Acid-base reactions must take place in aqueous solution. E) none of the above Answer: E Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 2) The H3O+ ion is called the ________ ion. A) hydroxide B) hydronium C) hydrogen D) protium E) water Answer: B Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 3) When acids and bases react the product other than water is a A) hydrogen ion. B) hydroxide ion. C) hydronium ion. D) metal. E) salt. Answer: E Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2

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4) A Brønsted-Lowry acid is a substance which A) produces hydrogen ions in aqueous solution. B) produces hydroxide ions in aqueous solution. C) donates protons to other substances. D) accepts protons from other substances. E) accepts hydronium ions from other substances. Answer: C Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 5) A Brønsted-Lowry base is a substance which A) produces hydrogen ions in aqueous solution. B) produces hydroxide ions in aqueous solution. C) donates protons to other substances. D) accepts protons from other substances. E) accepts hydronium ions from other substances. Answer: D Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 6) A necessary requirement for a Brønsted base is A) the presence of water as a reaction medium. B) the presence of hydroxide in its formula. C) a lone pair of electrons in its Lewis dot structure. D) the production of hydronium ion upon reaction with water. E) the presence of a metal ion in its formula. Answer: C Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 7) The base forms a new ________ bond in a Brønsted-Lowry acid-base reaction. A) covalent B) aquo C) hydrogen D) ionic E) metallic Answer: A Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 2 Copyright © 2017 Pearson Education, Inc.

8) Which of the following is a diprotic acid? A) acetic acid B) hydrochloric acid C) phosphoric acid D) sulfuric acid E) nitric acid Answer: D Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 9) What is the conjugate base of HSO4-? A) SO42B) H2SO4 C) H3O+ D) OHE) H2SO3 Answer: A Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 10) According to Brønsted-Lowry theory, acid-base reactions can be described as ________ reactions. A) electrolytic B) electron transfer C) gas phase D) nuclear transfer E) proton transfer Answer: E Diff: 2 Section: 10.1 LO: 10.1 Global LO: G2

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11) N+ C + HCO3In the reaction shown, the conjugate acid of A) N. B) C . C) . -. D) HCO3 E) . Answer: C Diff: 2 Section: 10.1 LO: 10.1 Global LO: G2 12) CH3NH2 + HCl

N is

CH3NH3+ + Cl-

A conjugate acid-base pair in the reaction shown is ________ and ________. A) CH3NH2; HCl B) CH3NH2; ClC) CH3NH3+; ClD) HCl; ClE) HCl; H3O+ Answer: D Diff: 2 Section: 10.1 LO: 10.1 Global LO: G2 13) Which of the following cannot act as a Brønsted base? A) HCO3B) CO32C) NH3 D) NH2E) NH4+ Answer: E Diff: 2 Section: 10.1 LO: 10.1 Global LO: G2

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14) In the following equation, which of the following is acting as the Bronsted acid? HClO4 + H2O → ClO4- + H3O+ A) HClO4 B) H2O C) ClO4D) H3O+ Answer: A Diff: 1 Section: 10.1 LO: 10.1 Global LO: G2 15) Which of the following is a triprotic acid? A) H3PO4 B) CH3COOH C) HNO3 D) NH3 E) Al(OH)3 Answer: A Diff: 3 Section: 10.1 LO: 10.1 Global LO: G2 16) What is the conjugate acid of HSO4-? A) SO42B) H2SO4 C) H3O+ D) OHE) H2SO3 Answer: B Diff: 3 Section: 10.1 LO: 10.1 Global LO: G2

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17) Consider the following reaction: NO2- + HCO3CO3-2 + HNO2 Identify the acid, base, conjugate acid and conjugate base. Answer: Acid: HCO3-; Conjugate Base: CO3-2; Base: NO2-; Conjugate Acid: HNO2 Diff: 2 Section: 10.1, 10.10 LO: 10.1, 10.11 Global LO: G2 18) Consider the reaction: H2SO3 + HCO3H2CO3 + HSO3A) Identify the acid, base, conjugate acid and conjugate base. B) Identify two substances from the reaction which could be used to prepare a buffer. Answer: A) Acid: H2SO3; Conjugate Base: HSO3-; Base: HCO3-; Conjugate Acid: H2CO3 B) Buffers: either conjugate acid base pair Diff: 2 Section: 10.1, 10.10 LO: 10.1, 10.11 Global LO: G2 19) Acetic acid is a weak acid in water because it is A) dilute. B) only slightly soluble. C) unable to hold onto its hydrogen ion. D) only slightly dissociated into ions. E) completely dissociated into hydronium ions and acetate ions. Answer: D Diff: 1 Section: 10.2 LO: 10.2 Global LO: G2 20) The classification of an acid or a base as weak or strong is determined by A) the solubility of the acid or base. B) the extent of dissociation of the dissolved acid or base. C) the concentrations of the acid or base. D) more than one choice is correct. Answer: B Diff: 1 Section: 10.2 LO: 10.2 Global LO: G2

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21) Hydrogen cyanide, HCN, is a weak acid. Which equation best represents its aqueous chemistry? A) HCN(aq) + H2O(l) CN-(aq) + H3O+(aq) B) HCN(aq) + H2O(l) H2CN+(aq) + OH-(aq) C) HCN(aq) H+(aq) + CN-(aq) D) HCN(aq) H-(aq) + CN+(aq) E) H2O(l) H+(aq) + OH-(aq) Answer: A Diff: 1 Section: 10.2 LO: 10.2 Global LO: G2 22) Which of the following is a strong acid? A) HNO3 B) H3PO4 C) NH4+ D) HCO3E) H2O Answer: A Diff: 2 Section: 10.2 LO: 10.2 Global LO: G2 23) Which of the following is a weak acid? A) HNO3 B) H3PO4 C) NH3 D) HCl E) OHAnswer: B Diff: 3 Section: 10.2 LO: 10.2 Global LO: G2

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24) Which reaction best illustrates the behavior of the weak base H2PO4- in aqueous solution? A) H2PO4-(aq) + H2O(l) HPO42-(aq) + H3O+(aq) B) H2PO4-(aq) + H2O(l) H3PO4(aq) + OH-(aq) C) H2PO4-(aq) 2H+(aq) + PO43-(aq) D) H2PO4-(aq) H+(aq) + HPO42-(aq) E) H2PO4-(aq) + H+(aq) Answer: B Diff: 3 Section: 10.2 LO: 10.2 Global LO: G2

H3PO4(aq)

25) Write a balanced equation for the transfer of a proton between dihydrogen phosphate ion and the hydroxide ion. Identify the conjugate acid-base pairs and determine which side of the reaction is favored. Answer: H2PO4-(aq) + OH-(aq) HPO42-(aq) + H2O(l) Conjugate acid-base pairs: H2PO4- and HPO42-; OH- and H2O The reaction process towards products since the hydroxide ion is a stronger base than the hydrogen phosphate. Diff: 3 Section: 10.2 LO: 10.2 Global LO: G2 26) Write a balanced equation for the transfer of a proton between the bicarbonate ion and the hydronium ion. Identify the conjugate acid-base pairs and determine which side of the reaction is favored. Answer: HCO3-(aq) + H3O+(aq) H2CO3(aq) + H2O(l) Conjugate acid-base pairs: HCO3- and H2CO3; H3O+ and H2O The reaction process towards products since the hydronium ion is a stronger acid than carbonic acid. Diff: 3 Section: 10.2 LO: 10.2 Global LO: G2

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27) Which one of the following is the weakest acid? A) HCN (Ka = 4.9 × 10-10) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HF (Ka = 6.8 × 10-4) Answer: A Diff: 2 Section: 10.3 LO: 10.3 Global LO: G4 28) Which one of the following weak acids is the strongest? A) HCN (Ka = 4.9 × 10-10) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HF (Ka = 6.8 × 10-4) Answer: C Diff: 3 Section: 10.3 LO: 10.3 Global LO: G4 29) Which compound has a very large value of Ka in aqueous solution? A) NaCl B) HNO3 C) H3PO4 D) KOH E) NH3 Answer: B Diff: 2 Section: 10.3 LO: 10.3 Global LO: G2

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30) Which compound has a value of Ka that is close to 10-5? A) NaCl B) HNO3 C) CH3CH2CO2H D) KOH E) NH3 Answer: C Diff: 2 Section: 10.3 LO: 10.3 Global LO: G2

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31) What is the correct Ka expression for the reaction below? H2PO4-(aq) + H2O(l)

HPO42-(aq) + H3O+(aq)

A)

B)

C)

D)

E)

Answer: D Diff: 2 Section: 10.3 LO: 10.3 Global LO: G4

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32) What is the correct Ka expression for the reaction below? CH3COOH(aq) + H2O(l)

CH3COO-(aq) + H3O+(aq)

A)

B)

C)

D)

E)

Answer: D Diff: 2 Section: 10.3 LO: 10.3 Global LO: G4 33) Propionic acid (CH3CH2COOH) has a Ka = 1.3 × 10-5 and phosphoric acid (H3PO4) has a Ka = 7.5 10 -3. Write the conjugate base for each. Which one is the stronger base? Answer: Propionate — CH3CH2COO1-; Dihydrogen phosphate — H2PO41Since phosphoric acid is the stronger acid its conjugate will be weaker: therefore propionate is the stronger base. Diff: 2 Section: 10.3 LO: 10.3 Global LO: G2

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34) Water and HSO4- can either accept protons or donate protons. Such substances are said to be A) amphoteric. B) conjugate. C) diprotic. D) monoprotic. E) triprotic. Answer: A Diff: 2 Section: 10.4 LO: 10.4 Global LO: G2 35) Explain the term "amphoteric." Use the hydrogen carbonate ion, HCO3- to illustrate amphoteric behavior. Answer: An amphoteric compound or ion is one that can behave either as an acid or a base in solution, depending on the chemical environment. In reaction (1), it acts as an acid by donating a hydrogen ion. In reaction (2), it acts as a base by accepting the hydrogen ion. (1) HCO3-(aq) + H2O(l) HCO+(aq) + CO32-(aq) (2) HCO3-(aq) + H2O(l) H2CO3(aq) + OH-(aq) Diff: 3 Section: 10.4 LO: 10.4 Global LO: G8 36) Which statement is correct for pure water? A) Pure water contains equal amounts of hydroxide, [OH-], and hydronium, [H3O+], ions. B) Pure water contains larger amounts of hydroxide, [OH-], ions than hydronium, [H3O+], ions. C) Pure water contains larger amounts of hydronium, [H3O+], ions than hydroxide, [OH-], ions. D) Pure water is an electrolyte. E) Pure water contains no ions. Answer: A Diff: 3 Section: 10.4 LO: 10.4 Global LO: G2

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37) What is the conjugate base of water? A) H2O(l) B) H3O+(aq) C) OH-(aq) D) H+(aq) E) O2-(aq) Answer: C Diff: 2 Section: 10.4 LO: 10.4 Global LO: G2 38) What is the conjugate acid of water? A) H2O(l) B) H3O+(aq) C) OH-(aq) D) H+(aq) E) O2-(aq) Answer: B Diff: 2 Section: 10.4 LO: 10.4 Global LO: G2 39) At 25°C, the value of Kw is A) 1.00. B) 1.00 × 10-7. C) 1.00 × 10-14. D) 1.00 × 107. E) 1.00 × 1014. Answer: C Diff: 2 Section: 10.4 LO: 10.5 Global LO: G2

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40) If the concentration of OH- in an aqueous solution is 1.4 × 10-7 M, the concentration of H3O+ is A) 7.1 × 10+6 M. B) 1.0 × 10-7 M. C) 1.4 × 10-7 M. D) 7.1 × 10-8 M. E) 1.3 × 10-8 M. Answer: D Diff: 2 Section: 10.4 LO: 10.5 Global LO: G4 41) If the concentration of H3O+ in an aqueous solution is 7.6 × 10-9 M, the concentration of OH- is A) 7.6 × 10-23 M. B) 1.3 × 10+8 M. C) 6.4 × 10-5 M. D) 1.3 × 10-6 M. E) 7.6 × 10-9 M. Answer: D Diff: 2 Section: 10.4 LO: 10.5 Global LO: G4 42) In an aqueous solution that is acidic, [H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-]. A) greater; less B) less; greater C) greater; greater D) less; less E) none of the above Answer: C Diff: 2 Section: 10.4 LO: 10.5 Global LO: G4

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43) If the concentration of OH- is 1 × 10-2 M, the concentration of H3O+ is ________ M. A) 1 × 100 B) 1 × 10-2 C) 1 × 10-7 D) 1 × 10-12 E) 1 × 10-14 Answer: D Diff: 3 Section: 10.4 LO: 10.5 Global LO: G4 44) If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH- is ________ M. A) 2.9 × 10-12 B) 1.0 × 10-12 C) 1.0 × 10-7 D) 3.5 × 10-11 E) 10.5 × 10-3 Answer: A Diff: 3 Section: 10.4 LO: 10.5 Global LO: G4 45) Which solution is basic? A) [H3O+] = 1.0 × 10-4 B) [H3O+] = 1.0 × 10-7 C) [H3O+] = 1.0 × 10-10 D) [OH-] = 1.0 × 10-7 E) [OH-] = 1.0 × 10-10 Answer: C Diff: 1 Section: 10.5 LO: 10.6 Global LO: G4

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46) In an aqueous solution that is basic, [H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-]. A) greater; less B) less; greater C) greater; greater D) less; less E) none of the above Answer: D Diff: 1 Section: 10.5 LO: 10.6 Global LO: G4 47) Which example is not acidic? A) orange juice B) soil for azaleas with pH of 4.8 C) a solution of NH4NO3 with pH < 7.00 D) lake water that turns blue litmus to red E) a solution in which [H3O+] = 1.00 × 10-7 Answer: E Diff: 1 Section: 10.5 LO: 10.6 Global LO: G7 48) An increase in solution pH corresponds to A) an increase in hydronium ion concentration. B) a decrease in hydronium ion concentration. C) no change in hydronium ion concentration. D) a decrease in hydroxide ion concentration. Answer: B Diff: 1 Section: 10.5 LO: 10.6 Global LO: G2

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49) Which example is not basic? A) shampoo B) vinegar C) window cleaner D) limewater E) Mg(OH)2, used in remedies for upset stomach Answer: B Diff: 1 Section: 10.5 LO: 10.6 Global LO: G5 50) Which of the following statements is correct? A) In an acidic solution, [H3O+] < 10-7; [OH-] < 10-7. B) In an acidic solution, [H3O+] > 10-7; [OH-] > 10-7. C) In an acidic solution, [H3O+] > 10-7; [OH-] < 10-7. D) In an acidic solution, [H3O+] < 10-7; [OH-] > 10-7. E) In an acidic solution, [H3O+] > 10-7; [OH-] = 10-7. Answer: C Diff: 2 Section: 10.5 LO: 10.6 Global LO: G4 51) Which of the following pH's corresponds to a strongly basic solution? A) 11.5 B) 2.7 C) 6.9 D) 7.4 E) 4.3 Answer: A Diff: 1 Section: 10.5 LO: 10.6 Global LO: G4

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52) Which of the following pH's corresponds to a neutral solution? A) 7.0 B) 1.8 C) 6.2 D) 8.5 E) 14.0 Answer: A Diff: 3 Section: 10.5 LO: 10.6 Global LO: G4 53) Which of the following pH's corresponds to a weakly acidic solution? A) 5.3 B) 1.4 C) 7.8 D) 9.2 E) 11.5 Answer: A Diff: 3 Section: 10.5 LO: 10.6 Global LO: G4 54) The pH of a cup of coffee is measured as 5.45. Express this measurement as [H+], using the correct number of significant figures. A) 3.548 × 10-6 M B) 3.55 × 10-6 M C) 3.6 × 10-6 M D) 4 × 10-6 M E) 2.82 × 105 M Answer: C Diff: 1 Section: 10.6 LO: 10.7 Global LO: G4

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55) What is the value of [H3O+] in a solution with pH = 10.82? A) 6.6 × 10-4 M B) 1.5 × 10-11 M C) 1.03 M D) 10.82 M E) 3.18 M Answer: B Diff: 2 Section: 10.6 LO: 10.7 Global LO: G4 56) The pH of a solution with [H3O+] = 5.9 × 10-3 M, to the correct number of significant figures, is A) 5.9 × 10-3. B) 2.2. C) 2.23. D) 1.01. E) 2.229. Answer: C Diff: 2 Section: 10.6 LO: 10.7 Global LO: G4 57) What is the pH of a solution in which [H3O+] = 3.8 × 10-8 M? A) 7.42 B) 6.58 C) 3.80 D) 1.0 × 10-8 E) 2.6 × 10-7 Answer: A Diff: 3 Section: 10.6 LO: 10.7 Global LO: G4

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58) What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M? A) 12.61 B) 1.39 C) 1.10 D) 12.90 E) 4.10 Answer: B Diff: 3 Section: 10.6 LO: 10.7 Global LO: G4 59) What is the hydrogen ion concentration in a solution with pH = 2.34? A) 4.6 × 10-3 M B) 2.3 × 10-3 M C) 2.2 × 10-12 M D) 1.2 × 101 M E) 4.3 × 10-12 M Answer: A Diff: 3 Section: 10.6 LO: 10.7 Global LO: G4 60) Calculate the hydrogen ion concentration in a solution with pH = 6.35. A) 7.65 M B) 6.35 M C) 4.5 × 10-7 M D) 0.80 M E) 2.2 × 10-8 M Answer: C Diff: 3 Section: 10.6 LO: 10.7 Global LO: G4

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61) The [OH-] and the pH of 0.035 M KOH at 25°C are, respectively, A) 0.035 M and +1.46. B) 0.035 M and -1.46. C) 2.9 × 10-13 M and -12.54. D) 0.035 and +12.54. E) 2.9 × 10-13 M and +12.54. Answer: D Diff: 3 Section: 10.6 LO: 10.7 Global LO: G4 62) All of the statements regarding equivalents of acids and bases are true except A) equivalents are the same as moles. B) equivalents of acid are based on the number of hydrogen ions produced per formula unit of acid. C) equivalents are used to determine normality of solutions. D) the equivalent weight of a base is the weight that produces one mole of hydroxide ions. E) one equivalent of any acid will neutralize one equivalent of any base. Answer: A Diff: 2 Section: 10.7 LO: 10.8 Global LO: G4 63) What is the normality of a solution containing 49 g of H2SO4 in enough water to make 400 mL of solution? A) 2.5 N B) 5.0 N C) 1.0 N D) 10 N E) 0.20 N Answer: A Diff: 2 Section: 10.7 LO: 10.8 Global LO: G4

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64) The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250. mL solution is ________ N. A) 2.70 B) 1.35 C) 0.675 D) 3.51 E) 1.75 Answer: A Diff: 2 Section: 10.7 LO: 10.8 Global LO: G4 65) The normality of a solution prepared by dissolving 50.0 g of Ca(OH)2 in water to make 250. mL solution is ________ N. A) 1.35 B) 2.70 C) 3.51 D) 5.40 E) 7.02 Answer: D Diff: 2 Section: 10.7 LO: 10.8 Global LO: G4 66) What is the normality of a solution containing 100. g HNO3 in 500. mL of solution? A) 1.26 N B) 1.59 N C) 3.17 N D) 0.500 N E) 0.630 N Answer: C Diff: 3 Section: 10.7 LO: 10.8 Global LO: G4

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67) What is the normality of a solution prepared by dissolving 75.0 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution? A) 0.173 N B) 0.0576 N C) 0.293 N D) 4.68 N E) 1.56 N Answer: D Diff: 3 Section: 10.7 LO: 10.8 Global LO: G4 68) What is the normality of a solution prepared by dissolving 37.5 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution? A) 2.34 N B) 0.780 N C) 0.147 N D) 0.0865 N E) 0.288 N Answer: A Diff: 3 Section: 10.7 LO: 10.8 Global LO: G4 69) Which substance produces carbon dioxide and water upon reaction with an acid? A) NaCH3CO2 B) NH4NO3 C) MgCO3 D) H2C2O4 E) C8H18 Answer: C Diff: 3 Section: 10.8 LO: 10.9 Global LO: G2 70) Write the balanced chemical equation for a reaction between sodium bicarbonate and hydrochloric acid. Answer: NaHCO3 + HCl → NaCl + H2CO3 H2CO3(aq) → H2O(l) + CO2(g) Diff: 1 Section: 10.8 LO: 10.9 Global LO: G2 24 Copyright © 2017 Pearson Education, Inc.

71) Write the balanced chemical reaction between methyl amine (CH3NH2) and hydrobromic acid (HBr). Answer: CH3NH2 + HBr → CH3NH3+ + Br– Diff: 1 Section: 10.8 LO: 10.9 Global LO: G2 72) Which of the following compounds is a salt? A) HBr B) KNO3 C) H2SO4 D) NaOH E) C6H12O6 Answer: B Diff: 1 Section: 10.9 LO: 10.10 Global LO: G2 73) Which of the following compounds is a salt? A) CH3CO2H B) NH3 C) NH4NO3 D) Al(OH)3 E) C6H6 Answer: C Diff: 1 Section: 10.9 LO: 10.10 Global LO: G2 74) Which compound produces an acidic solution when dissolved in water? A) NH4Cl B) NaF C) K2SO4 D) KCl E) Ca(NO3)2 Answer: A Diff: 2 Section: 10.9 LO: 10.10 Global LO: G2 25 Copyright © 2017 Pearson Education, Inc.

75) Which compound produces a basic solution when dissolved in water? A) NH4Cl B) NaF C) KClO4 D) KCl E) Ca(NO3)2 Answer: B Diff: 2 Section: 10.9 LO: 10.10 Global LO: G2 76) Of the following four substances, which would form a basic solution when dissolved in water: NH4Cl

Cu(NO3)2 K2CO3

NaF

A) NH4Cl, Cu(NO3)2 B) K2CO3, NH4Cl C) NaF, K2CO3 D) NaF only E) none of them Answer: C Diff: 2 Section: 10.9 LO: 10.10 Global LO: G2 77) To prepare a buffer using sodium phosphate, which of the following would also be needed? A) hydrochloric acid B) ammonium hydroxide C) ammonium phosphate D) phosphoric acid E) sodium hydroxide Answer: D Diff: 1 Section: 10.10 LO: 10.11 Global LO: G2

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78) A buffer solution A) is a salt solution. B) maintains pH at 7.00. C) is a strong base. D) neu...