This Document Contains Chapters 13 to 14 Chapter 13 Solutions True/False Questions 1. The tragedy at Lake Nyos in Cameroon, West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water. Answer: False 2. The tragedy at Lake Nyos in Cameroon, West Africa, was due to the sudden release of excessive amounts of carbon monoxide dissolved in the lake water. Answer: False 3. A solution is a homogeneous mixture of two or more substances. Answer: True 4. Air is an example of a gaseous solution. Answer: True 5. Steel is an example of a solid solution. Answer: True 6. The minor component in a solution is called the solvent. Answer: False 7. The major component in a solution is called the solute. Answer: False 8. The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes. Answer: True 9. Ionic solutes typically dissolve in nonpolar solvents. Answer: False 10. When a chunk of gold is melted and poured into the shape of an ingot, an aqueous solution of gold has been created. Answer: False 11. Solubility is formally defined as the amount of a compound that can be dissolved in water. Answer: False 12. A saturated solution holds the maximum amount of solute under the solution conditions. Answer: True 13. A supersaturated solution is unstable and crystallization usually occurs. Answer: True 14. Salt water is an example of a strong electrolyte solution. Answer: True 15. A sugar solution is an example of a weak electrolyte solution. Answer: False 16. The solubility of solids in water generally increases with increasing temperature. Answer: True 17. Tap water contains dissolved nitrogen and oxygen. Answer: True 18. The solubility of gases in water decreases with increasing temperature. Answer: True 19. Warm beer goes flat quicker than cold beer. Answer: True 20. The solubility of gases in water increases with increasing pressure above the water. Answer: True 21. Sugar solutions conduct electricity because the dissolved particles are molecules. Answer: False 22. Vitamin C is a water-soluble vitamin, so it is likely that this vitamin is polar. Answer: True 23. A solution that is 35 percent by mass NaCl contains 35 grams of NaCl dissolved in 100 grams of water. Answer: False 24. A solution that is 13.58 percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water. Answer: True 25. Molarity is defined as the moles of solute per liter of solution. Answer: True 26. The molarity of a solution prepared by dissolving 15.0 grams of NaCl in 1000 mL water is 0.15 M. Answer: False 27. One liter of 6.0 M HNO3 contains the same number of H+ ions as does one liter of 6.0 M H2SO4. Answer: False 28. If 50 grams of salt dissolves into 250 grams of water, the resulting solution must have a mass of 300 grams. Answer: True 29. A stock solution is a more concentrated form than what is typically used in a lab. It often requires further dilution. Answer: True 30. Upon completing a dilution from a stock solution, you will always have more volume of solution than you started with and it will have a lower concentration than the stock solution. Answer: True 31. Molality is calculated by dividing grams of solute by kilograms of solution. Answer: False 32. Colligative properties are independent of the amount of solute in solution. Answer: False 33. Adding a nonvolatile solute to a liquid will cause boiling point depression and freezing point elevation. Answer: False 34. A sample of salt water will freeze at a higher temperature than a sample of pure water. Answer: False 35. A 0.10 molality solution of the sugar glucose (molecular weight = 180.10 g/mol) and a 0.10 molality solution of sucrose (molecular weight = 342.34 g/mol) would both boil at the same temperature. Answer: True 36. A semipermeable membrane allows only half the amount of a substance to pass through it. Answer: False 37. Osmosis is the process in which a solvent moves from an area of low solute concentration to an area of high solute concentration. Answer: True 38. Osmotic pressure is the pressure required to completely reverse the direction of solvent movement in osmosis. Answer: False Multiple Choice Questions 39. The tragedy at Lake Nyos in Cameroon, West Africa, was caused by: A) the release of excessive amounts of nitrogen gas that had been dissolved in the water at the bottom of the lake. B) the release of excessive amounts of oxygen gas that had been dissolved in the water at the bottom of the lake. C) the release of excessive amounts of carbon dioxide that had been dissolved in the water at the bottom of the lake. D) the release of excess water stored in the volcanic lake which flooded the village below. E) none of the above Answer: C 40. Which of the following substances is NOT a solution? A) air B) brass C) vodka D) copper E) All of the above are solutions. Answer: D 41. Which of the following substances is NOT a solution? A) humid air B) beer C) oxygen D) steel E) All of the above are solutions. Answer: C 42. Which of the following substances is NOT a solution? A) homogenized milk B) bronze C) sea water D) soda E) All of the above are solutions. Answer: E 43. Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink composed of water. What is the solute in this type of martini? A) water B) alcohol C) ice D) olive E) none of the above Answer: B 44. The oxygen in the air we breath is classified as: A) the solute in a homogeneous gas mixture. B) the solvent in a homogeneous gas mixture. C) the solute in a heterogeneous gas-liquid mixture. D) the solvent in a simple mixture. E) none of the above Answer: A 45. Hexane, a nonpolar solvent, will dissolve which of the following substances? A) sodium chloride B) oil C) ammonium acetate D) vinegar (acetic acid) E) none of the above Answer: B 46. Which of these compounds would you expect to be least soluble in water? A) CH3OH B) NaCl C) N2 D) NH3 E) not enough information Answer: C 47. In order for a solute to dissolve in solution: A) the solute-solvent forces must be greater than the solute-solute forces. B) the solute-solute forces must be greater than the solute-solvent forces. C) the solute-solvent forces must equal the solute-solute forces. D) the polarity of the solute and solvent must be opposite. E) none of the above Answer: A 48. If the solubility of sodium acetate (Molar mass = 82 g/mol) is 76 grams per 100 grams of water, which of the following solutions would be considered supersaturated? A) 8.5 moles of sodium acetate dissolved in 1 L of water B) 5.5 moles of sodium acetate dissolved in 500 mL of water C) 1.8 moles of sodium acetate dissolved in 300 mL of water D) 1.2 moles of sodium acetate dissolved in 200 mL of water E) none of the above Answer: B 49. If the solubility of sodium chloride is 36 grams per 100 grams of water, which of the following solutions would be considered unsaturated? A) 5.8 moles of NaCl dissolved in 1 L of water B) 3.25 moles of NaCL dissolved in 500 ml of water C) 1.85 moles of NaCl dissolved in 300 ml of water D) none of the above Answer: A 50. The solubility of Pb(NO3)2 is 55 grams per 100 g H2O at 20°C. Which term would properly describe a solution where 44 grams of Pb(NO3)2 is added to 100 grams of water at this temperature? A) insoluble B) unsaturated C) saturated D) supersaturated E) none of the above Answer: B 51. If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the solution would be considered ________. A) unsaturated. B) saturated. C) supersaturated. D) thermally saturated. E) none of the above Answer: B 52. Which of the following compounds is a strong electrolyte? A) HCl B) NaCl C) NH4Cl D) NaC2H3O2 E) all of the above Answer: E 53. Which of the following compounds is a strong electrolyte? A) C6H12O6 B) C7H14O5 C) C4H8O2 D) NaC2H3O2 E) all of the above Answer: D 54. The solubility of solids in water: A) is independent of the temperature. B) increases with increasing temperature. C) decreases with increasing temperature. D) Solids are not soluble in water. E) none of the above Answer: B 55. The solubility of solids in water: A) is independent of pressure above solution. B) increases with increasing pressure above solution. C) decreases with increasing pressure above solution. D) Solids are not soluble in water. E) none of the above Answer: A 56. When an ionic compound dissolves in water: A) the solvent-solute attractive forces overcome the solute-solute attractions. B) the positive end of water dipoles attract the negative ions. C) the negative end of water dipoles attract the positive ions. D) each of the above (A, B, and C) occurs. E) none of the above (A, B, or C) occurs. Answer: D 57. Which among the following is NOT true about the solubility of a solid in water? A) The solubility is not affected by pressure. B) The solubility generally increases as temperature increases. C) Solid crystallizes when a saturated solution is prepared at a higher temperature and then cooled. D) A saturated solution prepared at a lower temperature becomes unsaturated when heated to a higher temperature. E) none of the above Answer: E 58. Solubility of gases in water: A) is independent of pressure above solution. B) increases with increasing pressure above solution. C) decreases with increasing pressure above solution. D) Gases are not soluble in water. E) none of the above Answer: B 59. The solubility of gases in water: A) is independent of temperature. B) increases with increasing temperature. C) decreases with increasing temperature. D) gases are not soluble in water. E) none of the above Answer: C 60. The solubility of a gas in a liquid can always be increased by: A) increasing the temperature of the solvent. B) decreasing the polarity of the solvent. C) decreasing the pressure of the gas above the solvent. D) increasing the pressure of the gas above the solvent. E) none of the above Answer: D 61. A solution is saturated in both nitrogen gas (N2) and sodium iodide (NaI) at 50°C. When the solution is cooled to 25°C, which of the following is most likely to occur? A) Some nitrogen gas bubbles out of solution. B) Some sodium iodide will precipitate out of solution. C) Both A) and B) will happen. D) Nothing will happen. E) not enough information Answer: B 62. When preparing sodium hydroxide solution, it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide. Removing the carbon dioxide can be accomplished by: A) vigorously stirring the solution. B) using water fresh out of the purification system. C) boiling the water. D) Nothing can be done to remove dissolved gases. E) none of the above Answer: C 63. We dissolve 2.45 g of sugar in 200.0 g water. What is the mass percent of sugar in the solution? A) 1.21% B) 1.23% C) 2.42% D) 123% E) none of the above Answer: A 64. A solution contains 100.0 g water, 10.0 g NaCl, and 15.0 g methanol. What is the weight percent of methanol in the solution? A) 8.00% B) 10.0% C) 12.0% D) 15.0% E) none of the above Answer: C 65. What is the mass percent of a solution prepared by dissolving 18.9 grams of solid into 39.5 grams of water? A) 47.8% B) 58.4% C) 32.4% D) The identity of the compound must be known. E) none of the above Answer: C 66. What is the mass percent of an ammonium carbonate solution prepared by dissolving 33.2 grams of solid into 39.5 grams of water? A) 84.1% B) 72.7% C) 45.7% D) 54.3% E) none of the above Answer: C 67. What is the mass percent of a sodium fluoride solution prepared by dissolving 0.64 moles of sodium fluoride into 63.5 grams of water? A) 26.9% B) 42.3% C) 70.3% D) 29.7% E) none of the above Answer: D 68. How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF? A) 55.9 B) 31.1 C) 13.1 D) 239 E) none of the above Answer: D 69. How many moles of NaF are in 34.2 grams of a 45.5% by mass NaF solution? A) 0.814 B) 75.2 C) 15.6 D) 0.371 E) none of the above Answer: D 70. What is the molarity of a solution prepared by dissolving 10.7 g NaI in 0.250 L? A) 42.8 B) 0.0714 C) 2.86x 10-4 D) 0.286 E) none of the above Answer: D 71. You need to prepare 2.00 L of 0.100 M Na2CO3 solution. The best procedure is to weigh out A) 10.6 g Na2CO3 and add 2.00 L of water to it. B) 21.2 g Na2CO3 and add 2.00 L of water to it. C) 10.6 g Na2CO3 and add water until the final solution has a volume of 2.00 L. D) 21.2 g Na2CO3 and add water until the final solution has a volume of 2.00 L. Answer: D 72. Given that you wished to use exactly 0.325 mole of NaCl to prepare a 2.50 M NaCl solution, how many milliliters of solution must you prepare? A) 130. mL B) 0.130 mL C) 7.69 mL D) 0.813 mL E) none of the above Answer: A 73. How many moles of KOH are contained in 750. mL of 5.00 M KOH solution? A) 6.67 mol B) 3.75 × 103 mol C) 56.1 mol D) 3.75 mol E) none of the above Answer: D 74. What is the molarity of a solution prepared by dissolving 54.3 g of Ca(NO3)2 into 355 mL of water? A) 0.331 M B) 0.932 M C) 0.117 M D) 1.99 M E) none of the above Answer: B 75. A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters. The molarity of the final solution is __________. A) 0.500 M B) 0.750 M C) 1.00 M D) 2.25 M E) none of the above Answer: B 76. How many grams of KCl are needed to make 50.0 mL of 2.45 M KCl? A) 9.13 B) 1.52 C) 91.3 D) 0.123 E) none of the above Answer: A 77. How many grams of LiF would be present in 575 mL of 0.750 M LiF solution? A) 11.2 B) 0.0338 C) 1.12 × 104 D) 19.9 E) 33.8 Answer: A 78. How many liters of a 2.18 M solution can be made from 200.0 g K2S? A) 0.832 B) 1.81 C) 0.252 D) 1.20 E) none of the above Answer: A 79. A 0.15 M solution of BaCl2 contains: A) 0.15 M Ba2+ ions and 0.15 M Cl- ions. B) 0.15 M Ba2+ ions and 0.30 M Cl- ions. C) 0.30 M Ba2+ ions and 0.15 M Cl- ions. D) 0.30 M Ba2+ ions and 0.30 M Cl- ions. E) none of the above Answer: B 80. What are the ion concentrations in a 0.12 M solution of AlCl3? A) 0.36 M Al3+ ions and 0.12 M Cl- ions B) 0.12 M Al3+ ions and 0.040 M Cl- ions C) 0.12 M Al3+ ions and 0.36 M Cl- ions D) 0.040 M Al3+ ions and 0.040 M Cl- ions E) none of the above Answer: C 81. Which solution below contains the highest total quantity of dissolved sodium ions? A) 100. mL of 4.0 M NaCl B) 75.0 mL of 3.0 M Na2SO4 C) 50.0 mL of 8.0 M NaOH D) 50.0 mL of 2.0 M Na3PO4 E) none of the above Answer: B 82. After you have completed the task of diluting a solution, which statement below must be TRUE? A) The new solution has more volume but has a lower concentration than before. B) The new solution has more volume but has a higher concentration than before. C) The new solution has less volume but has a lower concentration than before. D) The new solution has less volume but has a higher concentration than before. E) none of the above Answer: A 83. Oftentimes solubility of a compound limits the concentration of the solution that can be prepared. Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution. A) AgNO3 (solubility = 122 g/100 g H2O) B) KCl (solubility = 34.0 g/100 g H2O) C) NaNO3 (solubility = 89.0 g/100 g H2O) D) NH4Cl (solubility = 41.1 g/100 g H2O) E) none of the above Answer: C 84. What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 1.20 L? A) 0.504 M B) 3.50 M C) 0.420 M D) 0.350 M E) none of the above Answer: D 85. What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl? A) 21.9 mL B) 0.560 mL C) 257 mL D) 560. mL E) none of the above Answer: A 86. What volume of 9.00 M nitric acid is needed to make 6.50 L of 1.25 M solution? A) 903 mL B) 1.73 L C) 1.10 L D) 748 mL E) none of the above Answer: A 87. What molarity should the stock solution be if you want to dilute 25.0 mL to 2.00 L and have the final concentration be 0.103 M? A) 0.206 M B) 8.24 M C) 4.12 M D) 0.243 M E) none of the above Answer: B 88. If you add 4.00 mL of pure water to 6.00 mL of 0.750 M NaCl solution, what is the concentration of sodium chloride in the diluted solution? A) 0.250 M B) 0.450 M C) 0.500 M D) 1.13 M E) none of the above Answer: B 89. How many grams of barium sulfate are produced if 25.34 mL of 0.113 M BaCl2 completely react given the reaction: BaCl2 (aq) + Na2SO4(aq) → BaSO4 (s) + 2NaCl (aq) A) 5.90 B) 26.3 C) 1039 D) 0.668 E) none of the above Answer: D 90. What is the concentration of sodium chloride in the final solution if 25.34 mL of 0.113 M BaCl2 completely reacts and the total volume of the reaction is 110.4 mL, given the reaction: BaCl2 (aq) + Na2SO4(aq) → BaSO4 (s) + 2NaCl (aq) A) 0.226 B) 0.0259 C) 0.0519 D) 0.667 E) none of the above Answer: C 91. How many mL of 0.218 M sodium sulfate react with exactly 25.34 mL of 0.113 M BaCl2 given the reaction: BaCl2 (aq) + Na2SO4(aq) → BaSO4 (s) + 2NaCl (aq) A) 13.1 B) 5.52 C) 24.6 D) 2.86 E) none of the above Answer: A 92. How many milliliters of 0.755 M H2SO4 solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H2SO4 (aq) → 2 H2O (l) + K2SO4 (aq) A) 51.9 mL B) 182 mL C) 91.1 mL D) 17200 mL E) none of the above Answer: C 93. Which of the following statements about colligative properties is FALSE? A) The boiling point of a solution is increased by the addition of salt. B) The freezing point of a solution is lowered by the addition of salt. C) The change in temperature is proportional to the molality. D) The identity of the solute is not a factor. E) All of the above statements are true. Answer: E 94. In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl2 solution, A) the NaCl solution has the higher boiling point and the lower freezing point. B) the CaCl2 solution has the higher boiling point and the lower freezing point. C) the NaCl solution has the higher boiling point and the CaCl2 solution has the lower freezing point. D) the CaCl2 solution has the higher boiling point and the NaCl solution has the lower freezing point. E) both solutions have the same boiling point and the same freezing point. Answer: B 95. What is the molality of a solution made by dissolving 14.7 g of C6H12O6 into 150.0 mL of water? Assume the density of water is 1.00 g/mL. A) 0.544 B) 0.0816 C) 10.2 D) 0.980 E) none of the above Answer: A 96. What is the change in the boiling point of a solution made by dissolving 14.7 g of C6H12O6 into 150.0 mL of water? The density of water is 1.00 g/mL and Kb = 0.512°C/m. A) 0.502°C B) 5.22°C C) 0.0418°C D) 0.279°C E) none of the above Answer: D 97. What is the change in the freezing point of a solution made by dissolving 14.7 g of C6H12O6 into 150.0 mL of water? The density of water is 1.00 g/mL and Kf = 1.86°C/m. A) 0.152°C B) 1.01°C C) 18.97°C D) 1.82°C E) none of the above Answer: B 98. Why is NOT a good idea to drink seawater when people are lost at sea? A) The high concentration of salt forces water out of the cells lining your stomach and intestine. B) The osmotic pressure builds up in the cells of your intestine until they potentially rupture. C) The semipermeable membrane protecting your stomach is ruptured during osmosis. D) The seawater has fish urine in it and who wants to drink that? E) none of the above Answer: A 99. What will happen if a healthy red blood cell is placed into a container of pure water? A) The cell will totally dissolve in the water. B) The cell will remain unchanged. C) The cell will become swollen. D) The cell will shrink. E) none of the above Answer: D 100. Solution A has a concentration of 0.10 M sugar and Solution B has a concentration of 0.20 M sugar. If the two solutions are separated by a semipermeable membrane, which of the following occurs during osmosis? A) Solvent molecules move from B into A. B) Sugar molecules move from B into A. C) The molarity of A increases. D) The molarity of B increases. E) none of the above Answer: C 101. An osmosis cell is constructed of a "U" shaped tube with a semipermeable membrane separating the two arms of the tube. Suppose a concentrated solution is placed in the left arm of the U-tube, and a dilute concentration of the same substance is poured into the other arm to the same height. After a period of time has elapsed, you would expect to find that A) the level of liquid in the left arm is now higher. B) the level of the liquid in the right arm is now higher. C) the levels in both arms stay at the same height. D) no molecules of any type cross the membrane. E) none of the above Answer: A 102. Osmotic pressure is: A) the pressure required to stop the flow of solvent from a region of high solute concentration to a region of low solute concentration. B) the pressure required to stop the rupture of the semipermeable membrane. C) the pressure required to reverse the flow of solvent through a semipermeable membrane during osmosis. D) the pressure required to stop the flow of solvent from a region of low solute concentration through a semipermeable membrane into a region of high solute concentration. E) none of the above Answer: D Algorithmic Questions 103. Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water. A) 27.3 B) 72.3 C) 47.0 D) 37.6 E) none of the above Answer: A 104. Calculate the molarity of a KCl solution prepared by dissolving 0.525 moles of KCl in 250. mL of water. A) 0.476 B) 0.00210 C) 2.10 D) 2.02 E) none of the above Answer: C 105. Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500. mL. A) 0.331 B) 0.663 C) 0.166 D) 6.04 E) none of the above Answer: B 106. How many moles of KCl are present in 95.3 mL of2.10 M KCl? A) 0.0500 B) 5.00 C) 20.0 D) 0.200 E) none of the above Answer: D 107. How many grams of KCl are present in 75.0 mL of 2.10 M KCl? A) 5.59 B) 117 C) 2.66 D) 11.7 E) none of the above Answer: D 108. What volume (L) of 2.00 M KCl solution contains 25.0 g of KCl? A) 0.335 B) 0.168 C) 0.672 D) 1.49 E) none of the above Answer: B 109. What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L? A) 1.67 B) 0.600 C) 0.0167 D) 3.0 E) none of the above Answer: B 110. How many mL of 0.112 M Pb(N O3)2 are needed to completely react with 25.0 mL of 0.105 M KI? Given: Pb(NO3)2 (aq) + 2KI(aq) → PbI2 (s) + 2KNO3(aq) A) 11.7 B) 23.4 C) 0.147 D) 5.85 E) none of the above Answer: A 111. Calculate the molality of a solution prepared by dissolving 19.9 g of KCl in 750.0 mL of water. A) 0.200 B) 0.356 C) 4.99 D) 0.267 E) none of the above Answer: B 112. Given that the freezing point depression constant for water is 1.86°C kg/mol, calculate the change in freezing point for a 0.907 M sugar solution. A) 0.488°C B) 2.05°C C) 0.592°C D) 1.69°C E) none of the above Answer: D Chapter 14 Acids and Bases True/False Questions 1. Acids have a bitter taste. Answer: False 2. Acids produce H⁺ ions in solution. Answer: True 3. Acids turn litmus paper blue. Answer: False 4. The main component of stomach acid is sulfuric acid. Answer: False 5. The main component of vinegar is acetic acid. Answer: True 6. Bases have a bitter taste. Answer: True 7. Bases feel slippery. Answer: True 8. Bases feel slippery because they react with oils on your skin to form soap-like substances. Answer: True 9. Sodium hydroxide is often used in the manufacturing of soap. Answer: True 10. The sour taste of bases warns humans against eating poisonous alkaloids found in some plants. Answer: False 11. An Arrhenius base is a proton acceptor. Answer: False 12. A Bronsted-Lowry acid is a proton donor. Answer: True 13. H⁺ is called the hydronium ion. Answer: False 14. A conjugate acid-base pair are two substances related to each other by the transfer of a proton. Answer: True 15. The conjugate base to HSO4- is SO42-. Answer: True 16. H2SO3 and H2SO4 are considered an acid-base conjugate pair. Answer: False 17. The products of a neutralization reaction are carbon dioxide and water. Answer: False 18. The salt that forms due to neutralization of phosphoric acid by calcium hydroxide has the formula Ca3P2. Answer: False 19. When a metal reacts with an acid it produces salt and water. Answer: False 20. Aluminum is one of the few metals that dissolves in a strong base. Answer: True 21. In a titration, the indicator is used to signal when the endpoint has been reached. Answer: True 22. A 100 mL sample of 4.0 M H2SO4 could be neutralized by 100 mL of 4.0 M NH3. Answer: False 23. A strong acid is one that completely dissociates into ions in solution. Answer: True 24. The equation HCl (aq) + H2O (l) ↔ H3O+ (aq) + Cl- (aq) properly depicts the behavior of hydrochloric acid in water. Answer: False 25. A strong acid must also be a strong electrolyte. Answer: True 26. A strong acid is one that is very concentrated. Answer: False 27. A weak acid is a dilute acid that is not very powerful. Answer: False 28. In general, the stronger the acid, the weaker is its conjugate base. Answer: True 29. Water always acts as an acid in reactions. Answer: False 30. A neutral solution does not contain any H⁺ or OH⁻. Answer: False 31. The ion product constant for water (Kw) is best stated as Kw = [H2O] [H+]. Answer: False 32. A solution of pH 2 contains ten times more H3O+ than a solution of pH 3. Answer: True 33. The pH of 0.001 M HCl is 3.0. Answer: True 34. The pH of a 0.0001 M NaOH solution is 4. Answer: False 35. A solution that has a pH of 8.5 is considered a weak base. Answer: True 36. A pH of 7 is equivalent to a pOH of 7. Answer: True 37. A solution that has a pH of 10 would also have a pOH of 4. Answer: True 38. A buffer resists a change in pH by being able to react with an acid or a base. Answer: True 39. The burning of fossil fuels produces nitrogen oxides and sulfur oxides which can react to form acid rain (nitric and sulfuric acids). Answer: True 40. Rain is naturally somewhat acidic because of atmospheric carbon dioxide. Answer: True Multiple Choice Questions 41. Which of the following is NOT a property of acids? A) Acids have a slippery feel. B) Acids have a sour taste. C) Acids turn litmus paper red. D) Acids dissolve many metals. E) All of the above are properties of acids. Answer: A 42. Which of the following statements about acids are TRUE? 1. An acid is used in car batteries. 2. The active ingredient of vinegar is an acid. 3. Acids are used for cleaning metals. A) 1 and 2 only B) 2 and 3 only C) 1 and 3 only D) All of 1, 2, and 3 E) Neither 1, 2, or 3 Answer: D 43. Carboxylic acids can be found in A) grapes. B) apples. C) lemons. D) all of the above E) none of these Answer: D 44. Which among the following acids is commonly used for etching and frosting glass? A) Hydrochloric acid B) Nitric acid C) Hydrofluoric acid D) Hydrobromic acid E) All of the above are used. Answer: C 45. Which of the following acids is commonly used for manufacturing fertilizer? A) HCl B) HNO3 C) HF D) HBr E) all of the above Answer: B 46. Which of the following is NOT a property of bases? A) Bases have a slippery feel. B) Bases have a bitter taste. C) Bases turn litmus paper blue. D) Bases dissolve many metals. E) All of the above are properties of bases. Answer: D 47. Which of the following statements about a base are TRUE? 1. Bases are used in the manufacturing of soap. 2. Bases have a sour taste. 3. Fertilizer manufacture and cotton processing use bases. A) 1 and 2 only B) 1 and 3 only C) 2 and 3 only D) All of 1, 2, and 3 E) Neither 1, 2, or 3 Answer: B 48. Which of the following common bases is commonly used for manufacturing fertilizer? A) NH3 B) NaHCO3 C) KOH D) NaOH E) all of the above Answer: A 49. Which of the following is the active ingredient of baking soda? A) NH3 B) NaHCO3 C) KOH D) NaOH E) none of the above Answer: B 50. The Arrhenius definition of an acid is: A) a proton donor. B) a proton acceptor. C) produces H⁺ in solution. D) produces OH⁻ in solution. E) none of the above Answer: C 51. The Bronsted-Lowry definition of a base is: A) a proton donor. B) a proton acceptor. C) produces H⁺ in solution. D) produces OH⁻ in solution. E) none of the above Answer: B 52. The Bronsted-Lowry definition of an acid is: A) a proton donor. B) a proton acceptor. C) produces H⁺ in solution. D) produces OH⁻ in solution. E) none of the above Answer: A 53. Which of the following is NOT true? A) The Bronsted-Lowry Model applies to a wider range of acid-base phenomena than does the Arrhenius Model. B) The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry Model. C) The Bronsted-Lowry Model can apply to bases that do not contain hydroxide ions. D) The Arrhenius Model of acids and bases applies toward substances that are nonaqueous. E) none of the above Answer: D 54. In examining the formula for acetic acid, HC2H3O2, the ionizable hydrogen atom(s) is/are A) the H on the left. B) one of the H's on the right-side. C) all of the H's on the right-side. D) all four H's. E) none of the above. Answer: A 55. Which of the following is NOT an acid-base conjugate pair? A) H2CO3 and HCO3- B) H2O and OH- C) H2S and OH- D) NH4+ and NH3 E) none of the above Answer: C 56. In the following reaction: HCO3- (aq) + H2O (aq) → H2CO3 (aq) + OH- (aq) A) HCO3- is an acid and H2CO3 is its conjugate base. B) H2O is an acid and OH- is its conjugate base. C) HCO3- is an acid and OH- is its conjugate base. D) H2O is an acid and H2CO3 is its conjugate base. E) H2O is an acid and HCO3- is its conjugate base. Answer: B 57. In the following reaction: NH4+ (aq) + H2O (aq) → NH3 (aq) + H3O+ (aq) A) NH4+ is an acid and H2O is its conjugate base. B) H2O is a base and NH3 is its conjugate acid. C) NH4+ is an acid and H3O+ is its conjugate base. D) H2O is a base and H3O+ is its conjugate acid. E) NH4+ is a base and H2O is its conjugate acid. Answer: D 58. What is the conjugate acid of OH⁻? A) O2- B) H2O C) NaOH D) OH⁻ E) none of the above Answer: B 59. What is the conjugate base of H2O? A) O2- B) H2O+ C) NaOH D) OH⁻ E) none of the above Answer: D 60. A substance that acts as an acid or a base is called A) isoprotic. B) a salt. C) amphoteric. D) hydrophillic. E) none of the above Answer: C 61. What are the products of a neutralization reaction? A) salt and carbon dioxide B) carbon dioxide and water C) water and salt D) oil and water E) none of the above Answer: C 62. When an acid reacts with a metal, what is one of the usual products? A) water B) salt C) carbon dioxide D) hydrogen gas E) none of the above Answer: D 63. A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate. What was the formula of the acid that was neutralized? A) H2S B) H2SO4 C) HCl D) Na2SO4 E) none of the above Answer: B 64. A 25.0 ml sample of 0.105 M HCl was titrated with 31.5 ml of NaOH. What is the concentration of the NaOH? A) 0.0833 M B) 0.132 M C) 0.105 M D) 0.075 M E) none of the above Answer: A 65. A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH. What is the concentration of the KOH? A) 0.157 M B) 0.303 M C) 0.272 M D) 0.186 M E) none of the above Answer: D 66. Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH. What was the concentration of the H2SO4 solution? GIVEN: H2SO4 (aq) + 2NaOH (aq) → 2H2O (l) + Na2SO4 (aq) A) 5.63 M B) 0.622 M C) 0.00529 M D) 0.311 M E) none of the above Answer: D 67. Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water? A) OSHA regulations B) Water can be broken down by electricity. C) Water always has some ions dissolved in it. D) Water dissociates fully into its ions. E) none of the above Answer: C 68. Which of the following acids is diprotic? A) HClO4 B) HNO3 C) HI D) H2SO4 E) none of the above Answer: D 69. Which of the following acids is a diprotic, weak acid? A) sulfuric acid B) phosphoric acid C) hydrobromic acid D) carbonic acid E) none of the above Answer: D 70. Which of the following acids is a monoprotic, strong acid? A) sulfuric acid B) phosphoric acid C) hydrobromic acid D) carbonic acid E) none of the above Answer: C 71. A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is: A) a strong acid. B) a strong base. C) a weak acid. D) a weak base. E) none of the above Answer: C 72. What is the concentration of H⁺ in 2.0 M acetic acid, HC2H3O2? A) 1.0 M B) 2.0 M C) > 2.0 M D) < 2.0 M E) none of the above Answer: D 73. What is the concentration of H⁺ in 0.50 M hydroiodic acid? A) 0.50 M B) 1.0 M C) < 0.50 M D) 1.50 M E) none of the above Answer: A 74. Which of the following is a weak base? A) calcium hydroxide B) sodium fluoride C) potassium hydroxide D) ammonia E) none of the above Answer: D 75. Ammonia (NH3) ionizes in water to form a basic solution. What is the concentration of OH- ions in a 0.75 M NH3 solution? A) 0.75 M B) 0.75 M D) No OH- ions exist in a solution of NH3. E) none of the above Answer: B 76. Consider a 1.6 × 10-3 M solution of HNO3. Which of the following statements is NOT true? A) This solution would turn litmus to red. B) This solution could neutralize a base. C) This solution has a pH of 11.20. D) This solution could dissolve metal. E) none of the above Answer: C 77. Substances that can act both as an acid and as a base are called: A) neutral. B) buffers. C) indicators. D) amphoteric. E) none of these Answer: D 78. What is the concentration of the hydronium ions in a neutral solution? A) 0.0 M B) 1.0 × 10-7 M C) 1.0 × 10-14 M D) > 1.0 × 10-7 M E) 1.0 × 10-7 M E) 1.0 × 10-7 M E) < 1.0 × 10-7 M Answer: D 81. What is the value of the ion product constant for water (Kw)? A) 0.0 B) 1.0 × 10-7 C) 1.0 × 10-14 D) 1.0 × 1014 E) 1.0 × 107 Answer: C 82. What is the concentration of the hydroxide ion given that the concentration of the hydronium ion is 1.5 × 10-5 M? A) 6.7 × 10-10 M B) 1.5 × 109 M C) 1.0 × 10-14 M D) 1.0 × 10-19 M E) none of the above Answer: A 83. What is the concentration of hydronium ions in a solution given that the concentration of hydroxide ions is 2.31 × 10-4 M? A) 4.33 × 10-11 M B) 2.31 × 1010 M C) 2.31 × 10-18 M D) 1.01 × 10-5 M E) none of the above Answer: A 84. Which solution below has the highest concentration of hydroxide ions? A) pH = 3.21 B) pH = 12.49 C) pH = 7.00 D) pH = 10.12 E) pH = 7.93 Answer: B 85. The pH of a solution is 5.00. Which of the following is TRUE about the solution? A) Its [H3O+] is 1.0 × 10-9 M B) Its [H3O+] is 1.0 × 10-5 M C) Its [H3O+] is 1.0 × 105 M D) It is more acidic than a solution whose pH is 4.00. E) none of the above Answer: B 86. In order for a solution to be acidic, A) [H3O+] [OH-] C) [H3O+] = [OH-] D) pH = pOH E) none of the above Answer: B 87. In order for a solution to be basic, A) [H3O+] > [OH-] B) [H3O+] [OH-] B) [H3O+] [OH-] B) [H3O+] < [OH-] C) [H3O+] = [OH-] D) [H3O+] = [OH]/Kw E) none of the above Answer: A 90. Which solution below is considered to have basic character? A) pOH = 7 B) pH = 2 C) pOH = 4 D) pOH = 13 E) none of the above Answer: C 91. What is the pH of a solution that has a H⁺ concentration equal to 1.76 × 10-5 M? A) 4.77 B) 5.20 C) 0.22 D) 10.20 E) none of the above Answer: A 92. If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydronium ion concentration? A) It decreased. B) It became zero. C) It became less than zero. D) It increased. E) none of the above Answer: D 93. What is the pOH of a solution that has a OH- concentration equal to1.36 × 10-10 M? A) 9.89 B) 4.29 C) -4.3 D) 4.12 E) none of the above Answer: A 94. What is the [H⁺] in a solution that has a pH of 3.35? A) 1 × 103.35 M B) 2.2 × 103 M C) 4.5 × 10-4 M D) 3.35 × 10-14 M E) none of the above Answer: C 95. What is the [OH-] in a solution that has a pOH of 9.65? A) 4.5 × 10-9 M B) 4.5 × 105 M C) 9.8 × 10-1 M D) 2.2 × 10-10 M E) none of the above Answer: D 96. Which of the following is TRUE of alkaloid compounds? A) Alkaloids are organic bases. B) Alkaloids occur naturally in many plants. C) Some narcotic drugs are alkaloids. D) Some alkaloids are addictive. E) All of the above are true. Answer: E 97. A buffer solution is all of the following EXCEPT: A) a solution that resists a change in pH when a base is added. B) a solution that resists a change in pH when an acid is added. C) a solution that contains both a weak acid and its conjugate base. D) a solution that regulates pH by the addition of a strong acid or base. E) All of the above are true. Answer: D 98. Which of the following statements are TRUE of buffer solutions? 1. A buffer solution can be made by mixing equal concentrations of acetic acid and sodium acetate. 2. A buffer solution can be made by mixing equal concentrations of hydrochloric acid and sodium chloride. 3. A buffer solution resists changes in pH when small quantities of acid or base are added. A) 1 and 2 only B) 2 and 3 only C) 1 and 3 only D) All of 1, 2, and 3 E) None of 1, 2, and 3 Answer: C 99. Which combination below will be a buffer solution? A) HCl and Cl⁻ B) HNO3 and NaNO3 C) HC2H3O2 and NaC2H3O2 D) NaBr and NaOH E) All of the above are true. Answer: C 100. Which of the following contributes to acid rain? A) The use of volatile acids in industry. B) The reaction of metal oxides with water. C) The reaction of nonmetal oxides with water. D) The reaction of alkali metals with water. E) all of the above Answer: C 101. Acid rain legislation targeted the release of which compound by industry? A) CO2 B) SO2 C) dioxin D) benzene E) none of the above Answer: B Algorithmic Questions 102. The titration of 25.00 mL a 0.125 M HClO4 solution required 21.37 mL of KOH to reach the endpoint. What is the concentration of the KOH? A) 0.292 M B) 0.0668 M C) 0.146 M D) 0.134 M E) none of the above Answer: C 103. What is the concentration of H+ in a 0.121 M HCl solution? A) 1.0 × 10-14 M B) < 0.121 M C) 0.121 M D) not enough information E) none of the above Answer: C 104. What is the concentration of H+ in solution given the [OH⁻] = 2.54 × 10-4? A) 3.94 × 10-11 M B) 2.54 × 10-11 M C) 1.0 × 1014 M D) not enough information E) none of the above Answer: A 105. What is the pH of a solution that has a [H+] = 0.0045 M? A) 1.35 B) 2.35 C) 3.35 D) 7.0045 E) none of the above Answer: B 106. What is the concentration of H+ in a solution with pH = 2.00? A) 5.0 M B) 1.1 M C) 0.010 M D) 0.30 M E) none of the above Answer: C Test Bank for Introductory Chemistry Nivaldo J. Tro 9780321741028, 9780321687937, 9781256112938, 9781256161066, 9780134302386, 9780321910073
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