chap4questionbank.rtf

40. Which of the following salts is insoluble in water? A) Na2S B) K2CO3 C) Pb(NO3)2 D) CaCl2 E) All of these are soluble in water.

E) All of these are soluble in water.

9. The man who discovered the essential nature of acids through solution conductivity studies is A) Priestly B) Boyle C) Einstein D) Mendeleev E) Arrhenius

E) Arrhenius

45. Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed? A) Al3+, S2- B) Pb2+, Cl- C) Ba2+, PO43- D) Pb2+, OH- E) Mg2+, SO42-

E) Mg2+, SO42-

76. In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are: A) NaSO4 + H2O B) NaSO3 + 2H2O C) 2NaSO4 + H2O D) Na2S + 2H2O E) Na2SO4 + 2H2O

E) Na2SO4 + 2H2O

39. Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? A) Both KNO3 and NH4SO4 precipitate from solution. B) A gas is released. C) NH4SO4 will precipitate from solution. D) KNO3 will precipitate from solution. E) No reaction will occur.

E) No reaction will occur.

75. When solutions of carbonic acid and copper(II) hydroxide react, which of the following are spectator ions? A) hydrogen ion B) carbonate ion C) copper(II) ion D) hydroxide ion E) none of these

E) none of these

33. The following reactions: Pb2+ + 2I- → PbI2 2Ce4+ + 2I- → I2 + 2Ce3+ HOAc + NH3 → NH4+ + OAc- are examples of A) acid-base reactions B) unbalanced reactions C) precipitation, acid-base, and redox reactions, respectively D) redox, acid-base, and precipitation reactions, respectively E) precipitation, redox, and acid-base reactions, respectively

E) precipitation, redox, and acid-base reactions, respectively

58. When solutions of strontium chloride and sodium sulfate react, which of the following is a spectator ion? A) strontium ion B) chloride ion C) sodium ion D) sulfate ion E) two of these

E) two of these

72. When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in the complete ionic equation? A) hydrogen ion B) carbonate ion C) potassium ion D) hydroxide ion E) water

A) hydrogen ion

41. How many of the following salts are expected to be insoluble in water? sodium sulfide barium nitrate ammonium sulfate potassium phosphate A) none B) 1 C) 2 D) 3 E) 4

A) none

20. A 74.28-g sample of Ba(OH)2 is dissolved in enough water to make 2.450 liters of solution. How many mL of this solution must be diluted with water in order to make 1.000 L of 0.100 M Ba(OH)2? A) 565 mL B) 177 mL C) 17.7 mL D) 4.34 mL E) 231 mL

A) 565 mL

51. The net ionic equation contains which of the following terms? A) Ag+(aq) B) Ba2+(aq) C) NO3- (aq) D) H+ (aq) E) AgCl(aq)

A) Ag+(aq)

37. You have exposed electrodes of a light bulb in a solution of H2SO4 such that the light bulb is on. You add a dilute solution and the bulb grows dim. Which of the following could be in the solution? A) Ba(OH)2 B) NaNO3 C) K2SO4 D) Cu(NO3)2 E) none of these

A) Ba(OH)2

57. When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms will be present in the net ionic equation? A) CoCO3(s) B) H+(aq) C) 2CoCO3(s) D) 2Cl-(aq) E) two of these

A) CoCO3(s)

36. All of the following reactions 2Al(s) + 3Br2(l) → 2AlBr3(s) 2Ag2O(s) → 4Ag(s) + O2(g) CH4(l) + 2O2(g) → CO2(g) + 2H2O(g) can be classified as A) oxidation-reduction reactions B) combustion reactions C) precipitation reactions D) A and B E) A and C

A) oxidation-reduction reactions

In the reaction C(s) + O2(g) → CO2(g) carbon is __________. A) the reducing agent B) the electron acceptor C) reduced D) the oxidizing agent E) more than one of these

A) the reducing agent

46. A solution contains the ions Ag+, Pb2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and Na2S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order? A) Na2SO4, NaCl, Na2S B) Na2SO4, Na2S, NaCl C) Na2S, NaCl, Na2SO4 D) NaCl, Na2S, Na2SO4 E) NaCl, Na2SO4, Na2S

A) Na2SO4, NaCl, Na2S

In the reaction Zn + H2SO4 → ZnSO4 + H2, which, if any, element is oxidized? A) zinc B) hydrogen C) sulfur D) oxygen E) none of these

A) zinc

62. If all of the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample? A) 50.52% B) 13.53% C) 1.425% D) 7.391% E) none of the above

B) 13.53%

18. A 38.1-g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution. A) 27.0 M B) 2.14 M C) 53.7 M D) 0.339 M E) none of these

B) 2.14 M

78. An unknown diprotic acid requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580-g sample. Calculate the approximate molar mass of the acid. A) 406 g/mol B) 235 g/mol C) 118 g/mol D) 59 g/mol E) 203 g/mol

B) 235 g/mol

79. You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base? A) The HCl solution. B) The H2SO4 solution. C) You need to know the acid concentrations to answer this question. D) You need to know the volume and concentration of the NaOH solution to answer this question. E) C and D

A) The HCl solution.

2. The interaction between solute particles and water molecules, which tends to cause a salt to fall apart in water, is called A) hydration B) polarization C) dispersion D) coagulation E) conductivity

A) hydration

69. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.72 M solution of AgNO3(aq). Calculate the concentration of Ag+ after the two solutions are mixed together. A) 0.00 M B) 0.538 M C) 1.08 M D) 0.088 M E) 0.215 M

A) 0.00 M

19. What mass of solute is contained in 256 mL of a 0.838 M ammonium chloride solution? A) 11.5 g B) 175 g C) 16.3 g D) 215 g E) 3.27 g

A) 11.5 g

22. How many grams of NaOH are contained in 5.0 × 102 mL of a 0.74 M sodium hydroxide solution? A) 15 g B) 74 g C) 0.37 g D) 30 g E) 370 g

A) 15 g

21. What volume of 18 M sulfuric acid must be used to prepare 2.30 L of 0.145 M H2SO4? A) 19 mL B) 0.33 mL C) 1.1 × 103 mL D) 2.9 mL E) 6.0 mL

A) 19 mL

77. A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid. A) 247 g/mol B) 171 g/mol C) 165 g/mol D) 151 g/mol E) 82.7 g/mol

A) 247 g/mol

71. You mix 55 mL of 1.00 M silver nitrate with 25 mL of 0.84 M sodium chloride. What mass of silver chloride should you form? A) 3.0 g B) 6.0 g C) 3.3 g D) 6.6 E) none of these

A) 3.0 g

64. A 3.00-g sample of an alloy (containing only Pb and Sn) was dissolved in nitric acid (HNO3). Sulfuric acid was added to this solution, which precipitated 2.37 g of PbSO4. Assuming that all of the lead was precipitated, what is the percentage of Sn in the sample? (molar mass of PbSO4 = 303.3 g/mol) A) 46.0% Sn B) 0.781% Sn C) 79.0% Sn D) 54.0% Sn E) 1.62% Sn

A) 46.0% Sn

34. The following reactions 2K(s) + Br2(l) → 2KBr(s) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) HCl(aq) + KOH(aq) → H2O(l) + KCl(aq) are examples of A) precipitation reactions B) redox, precipitation, and acid-base, respectively C) precipitation (two) and acid-base reactions, respectively D) redox reactions E) none of these

B) redox, precipitation, and acid-base, respectively

87. The oxidation state of chlorine in ClO- is: A) 0 B) +1 C) -1 D) +3 E) -3

B) +1

68. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.01 M solution of AgNO3(aq). Calculate the concentration of CrO42- after the two solutions are mixed together. A) 0.00 M B) 0.309 M C) 0.938 M D) 0.251 M E) 2.50 M

B) 0.309 M

49. Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced molecular equation contains which one of the following terms? A) AgCl (s) B) 2AgCl (s) C) 2Ba(NO3)2 (aq) D) BaNO3 (aq) E) 3AgCl (aq)

B) 2AgCl (s)

16. Which of the following aqueous solutions contains the greatest number of ions? A) 400.0 mL of 0.10 M NaCl B) 300.0 mL of 0.10 M CaCl2 C) 200.0 mL of 0.10 M FeCl3 D) 200.0 mL of 0.10 M KBr E) 800.0 mL of 0.10 M sucrose

B) 300.0 mL of 0.10 M CaCl2

56. When solutions of phosphoric acid and iron(III) nitrate react, which of the following terms will be present in the balanced molecular equation? A) HNO3(aq) B) 3HNO3(aq) C) 2FePO4(s) D) 3FePO4(s) E) 2HNO3(aq)

B) 3HNO3(aq)

15. How many grams of NaCl are contained in 350. mL of a 0.287 M solution of sodium chloride? A) 16.8 g B) 5.87 g C) 11.74 g D) 100.5 g E) none of these

B) 5.87 g

65. A mixture contained no fluorine compound except methyl fluoroacetate, FCH2COOCH3 (molar mass = 92.07 g/mol). When chemically treated, all the fluorine was converted to CaF2 (molar mass = 78.08 g/mol). The mass of CaF2 obtained was 35.8 g. Find the mass of methyl fluoroacetate in the original mixture. A) 60.7 g B) 84.4 g C) 30.4 g D) 42.2 g E) 21.1 g

B) 84.4 g

6. All of the following are weak acids except A) HCNO B) HBr C) HF D) HNO2 E) HCN

B) HBr

8. Which of the following is paired incorrectly? A) H2SO4 - strong acid B) HNO3 - weak acid C) Ba(OH)2 - strong base D) HCl - strong acid E) NH3 - weak base

B) HNO3 - weak acid

In the reaction shown below, what species is oxidized? 2NaI + Br2 → 2NaBr + I2 A) Na+ B) I- C) Br2 D) Br- E) I2

B) I-

10. A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the following is true? I. II. A) In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong acid. B) In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid. C) In both cases, HX is acting like a strong acid. D) In both cases, HX is acting like a weak acid. E) HX is not soluble in water.

B) In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid.

44. Which of the following compounds is soluble in water? A) Ni(OH)2 B) K3PO4 C) BaSO4 D) CoCO3 E) PbCl2

B) K3PO4

85. In which of the following does nitrogen have an oxidation state of +4? A) HNO3 B) NO2 C) N2O D) NH4Cl E) NaNO2

B) NO2

In the following reaction, which species is oxidized? 8NaI + 5H2SO4 → 4I2 + H2S + 4Na2SO4 + 4H2O A) sodium B) iodine C) sulfur D) hydrogen E) oxygen

B) iodine

1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar B) polar C) either polar or nonpolar D) nonpolar E) none of these

B) polar

In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is A) oxidized B) reduced C) the electron donor D) the reducing agent E) two of these

B) reduced

90. In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is A) the reducing agent B) the oxidizing agent C) oxidized D) the electron donor E) two of these

B) the oxidizing agent

82. Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base: A 0.165-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for a complete reaction. What is the molarity of the KOH solution? A) 0.00170 M B) 8.76 M C) 0.0876 M D) 0.0330 M E) none of these

C) 0.0876 M

70. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.88 M solution of AgNO3(aq). Calculate the concentration of NO3- after the two solutions are mixed together. A) 0.00 M B) 0.588 M C) 1.18 M D) 2.35 M E) 4.50 M

C) 1.18 M

30. A 230.0-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.29 M. What volume of solvent has evaporated from the 0.275 M solution? A) 49.0 mL B) 63.3 mL C) 181.0 mL D) 230. mL E) 279.0 mL

C) 181.0 mL

25. You have two solutions of chemical A. To determine which has the highest concentration of A in molarity, what is the minimum number of the following you must know? I. the mass in grams of A in each solution II. the molar mass of A III. the volume of water added to each solution IV. the total volume of the solution A) 0 B) 1 C) 2 D) 3 E) You must know all of them.

C) 2

How many of the following are oxidation-reduction reactions? NaOH + HCl → NaCl + H2O Cu + 2AgNO3 → 2Ag + Cu(NO3)2 Mg(OH)2 → MgO + H2O N2 + 3H2 → 2NH3 A) 0 B) 1 C) 2 D) 3 E) 4

C) 2

67. You have 88.6 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.50 M solution of AgNO3(aq). Calculate the concentration of Na+ after the two solutions are mixed together. A) 0.00 M B) 1.04 M C) 2.07 M D) 5.00 M E) 0.443 M

C) 2.07 M

50. The balanced complete ionic equation contains which of the following terms? A) 2Ba2+(aq) B) Cl-(aq) C) 2Ag+(aq) D) NO3- (aq) E) AgCl(aq)

C) 2Ag+(aq)

27. You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have much more of the 4.00 M solution and you add the solutions together. Which of the following could be the concentration of the final solution? A) 2.70 M B) 3.00 M C) 3.50 M D) 6.00 M E) 8.10 M

C) 3.50 M

59. The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species? A) 3Al3+(aq) B) OH-(aq) C) 3OH-(aq) D) 2Al3+(aq) E) 2Al(OH)3(s)

C) 3OH-(aq)

80. What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H2SO4? A) 2.7 g B) 0.7 g C) 5.4 g D) 135 g E) none of these

C) 5.4 g

66. A 1.59-g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. Calculate the molar mass of M. A) 70.9 g/mol B) 28 g/mol C) 55.9 g/mol D) 63 g/mol E) 72.4 g/mol

C) 55.9 g/mol

23. An analytical procedure requires a solution of chloride ions. How many grams of NaCl must be dissolved to make 1.95 L of 0.0561 M Cl-? A) 3.28 g B) 0.595 g C) 6.39 g D) 1.64 g E) 12.8 g

C) 6.39 g

89. In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized? A) O2 B) O2- C) Ca D) Ca2+ E) none of these

C) Ca

43. Which of the following ions is most likely to form an insoluble sulfate? A) K+ B) Li+ C) Ca2+ D) S2- E) Cl-

C) Ca2+

47. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. What is the formula of the solid formed in the reaction? A) Ca(PO4)2 B) CaPO4 C) Ca3(PO4)2 D) Ca3(PO3)2 E) none of these

C) Ca3(PO4)2

42. When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. Its formula is: A) Cu(NH)3 B) Cu(NO3)2 C) Cu(OH)2 D) Cu(NH3)22+ E) CuO

C) Cu(OH)2

38. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct? A) Both NaCl and CuS precipitate from solution. B) No reaction will occur. C) CuS will precipitate from solution. D) NaCl will precipitate from solution. E) A gas is released.

C) CuS will precipitate from solution.

5. Which of the following is a strong acid? A) HF B) KOH C) HClO4 D) HClO E) HBrO

C) HClO4

Which of the following are oxidation-reduction reactions? I. PCl3 + Cl2 → PCl5 II. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag III. CO2 + 2LiOH → Li2CO3 + H2O IV. FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl A) III B) IV C) I and II D) I, II, and III E) I, II, III, and IV

C) I and II

74. When solutions of carbonic acid and aluminum hydroxide react, which of the following are NOT present in the net ionic equation? I. hydrogen ion II. carbonate ion III. aluminum ion IV. hydroxide ion A) I and II B) I, II, and III C) I and IV D) I and III E) II and III

C) I and IV

52. In writing the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species? A) KOH B) Mg(NO3)2 C) Mg(OH)2 D) KNO3 E) All of the above would be written as ionic species.

C) Mg(OH)2

7. Which of the following is not a strong base? A) Ca(OH)2 B) KOH C) NH3 D) LiOH E) Sr(OH)2

C) NH3

In the reaction P4(s) + 10Cl2(g) → 4PCl5(s), the reducing agent is A) chlorine B) PCl5 C) phosphorus D) Cl- E) none of these

C) phosphorus

35. The following reactions ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s) KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) are examples of A) oxidation-reduction reactions B) acid-base reactions C) precipitation reactions D) A and C E) none of these

C) precipitation reactions

86. The oxidation state of iodine in IO3- is: A) 0 B) +3 C) -3 D) +5 E) -5

D) +5

83. A student weighs out 0.512 g of KHP (molar mass = 204.22 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one acidic proton. A) 0.00251 M B) 0.092 M C) 0.0139 M D) 0.0682 M E) none of these

D) 0.0682 M

14. 1.00 mL of a 4.05 × 10-4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. How many grams of oleic acid are 5.00 mL of solution B? (Molar mass for oleic acid = 282 g/mol) A) 5.71 × 10-6 g B) 1.59 × 10-5 g C) 2.28 × 10-2 g D) 1.14 × 10-5 g E) 5.71 × 10-4 g

D) 1.14 × 10-5 g

31. For the reaction 4FeCl2(aq) + 3O2(g) → 2Fe2O3(s) + 4Cl2(g), what volume of a 0.760 M solution of FeCl2 is required to react completely with 6.36 × 1021 molecules of O2? A) 5.26 × 103 mL B) 10.7 mL C) 10.4 mL D) 18.5 mL E) 6.02 mL

D) 18.5 mL

81. With what volume of 5.00 M HF will 4.72 g of calcium hydroxide react completely, according to the following reaction? A) 12.7 mL B) 127 mL C) 637 mL D) 25.5 mL E) 39.2 mL

D) 25.5 mL

54. When sodium chloride and lead(II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation? A) PbCl(s) B) Pb2Cl(s) C) NaNO3(aq) D) 2NaNO3(aq) E) 2PbCl2(s)

D) 2NaNO3(aq)

12. A 16.4-g sample of HF is dissolved in water to give 2.0 × 102 mL of solution. The concentration of the solution is: A) 0.82 M B) 0.16 M C) 0.08 M D) 4.1 M E) 8.2 M

D) 4.1 M

63. A mixture of BaCl2 and NaCl is analyzed by precipitating all the barium as BaSO4. After addition of an excess of Na2SO4 to a 3.725-g sample of the mixture, the mass of precipitate collected is 2.734 g. What is the mass percentage of barium chloride in the mixture? A) 82.28% B) 73.40% C) 43.18% D) 65.47% E) 19.60%

D) 65.47%

3. Consider two organic molecules, ethanol and benzene. One dissolves in water and the other does not. Why? A) They have different molar masses. B) One is ionic, the other is not. C) One is an electrolyte, the other is not. D) Ethanol contains a polar O-H bond, and benzene does not. E) Two of these are correct.

D) Ethanol contains a polar O-H bond, and benzene does not.

73. When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the net ionic equation? I. hydrogen ion II. acetate ion III. sodium ion IV. hydroxide ion A) I and II B) I, II, and III C) I and IV D) I and III E) II and III

D) I and III

29. Which of the following do you need to know to be able to calculate the molarity of a salt solution? I. the mass of salt added II. the molar mass of the salt III. the volume of water added IV. the total volume of the solution A) I, III B) I, II, III C) II, III D) I, II, IV E) You need all of the information.

D) I, II, IV

28. You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes would make the solution having the highest molar concentration? A) NaOH B) KCl C) KOH D) LiOH E) all the same

D) LiOH

60. Consider the reaction between 15.0 mL of a 1.00 M aqueous solution of AgNO3 and 10.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed. What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution. A) Ag+, NO3-, K+, CrO42-, water B) Ag+, NO3-, K+, water C) K+, CrO42-, water D) NO3-, K+, CrO42-, water E) water

D) NO3-, K+, CrO42-, water

61. You mix 275.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.85 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false? A) The final concentration of Pb2+ ions is 0.0913 M. B) You form 128 g of lead(II) iodide. C) The final concentration of K+ is 0.965 M. D) The final concentration of NO3- is 0.965 M. E) All are true.

D) The final concentration of NO3- is 0.965 M.

88. Which of the following statements is not true? A) When a metal reacts with a nonmetal, an ionic compound is formed. B) A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction. C) Two nonmetals can undergo an oxidation-reduction reaction. D) When two nonmetals react, the compound formed is ionic. E) A metal-nonmetal reaction involves electron transfer.

D) When two nonmetals react, the compound formed is ionic.

26. Diabetics often need injections of insulin to help maintain the proper blood glucose levels in their bodies. How many moles of insulin are needed to make up 45 mL of 0.0062 M insulin solution? A) 0.00056 mol B) 0.14 mol C) 7.3 mol D) 0.28 mol E) 0.00028 mol

E) 0.00028 mol

55. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. Write and balance the equation for this reaction to answer the following question.What is the sum of the coefficients when the molecular equation is balanced in standard form? A) 4 B) 5 C) 7 D) 11 E) 12

E) 12

53. The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species? A) 2Br-(aq) B) PO43-(aq) C) 2Ca3(PO4)2(s) D) 6NaBr(aq) E) 3Ca2+(aq)

E) 3Ca2+(aq)

32. Phosphoric acid, H3PO4, is a triprotic acid. What is the total number of moles of H+ available for reaction in 2.50 L of 0.700 M H3PO4? A) 0.233 mole B) 2.10 mole C) 0.583 mole D) 3.00 moles E) 5.25 moles

E) 5.25 moles

17. What mass of calcium chloride, CaCl2, is needed to prepare 3.950 L of a 1.49 M solution? A) 294 g B) 5.89 g C) 41.9 g D) 111 g E) 653 g

E) 653 g

13. 1.00 mL of a 3.50 × 10-4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. What is the concentration of solution B? A) 3.50 × 10-6 M B) 9.72 × 10-6 M C) 7.00 × 10-5 M D) 7.78 × 10-5 M E) 7.00 × 10-6 M

E) 7.00 × 10-6 M

Which of the following statements is(are) true? Oxidation and reduction A) cannot occur independently of each other B) accompany all chemical changes C) describe the loss and gain of electron(s), respectively D) result in a change in the oxidation states of the species involved E) A, C, and D

E) A, C, and D

Which of the following reactions does not involve oxidation-reduction? A) CH4 + 3O2 → 2H2O + CO2 B) Zn + 2HCl → ZnCl2 + H2 C) 2Na + 2H2O → 2NaOH + H2 D) MnO2 + 4HCl → Cl2 + 2H2O + MnCl2 E) All are oxidation-reduction reactions.

E) All are oxidation-reduction reactions.

11. An acid is a substance that produces OH- ions in water. True or False?

False

24. The concentration of a salt water solution that sits in an open beaker decreases over time. True or False?

False

48. The filtrate is the solid formed when two solutions are mixed. True or False?

False

84. A chemical that changes color at the endpoint of a reaction is called a colorimeter. True or False?

False

4. Polar molecules have an unequal distribution of charge within the molecule. True or False?

True