Chem 1C Final Exam
1. Which one of the following is not a redox reaction? A. Al(OH)4(aq) + 4H(aq) → Al3+(aq) + 4H2O(l) B. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) C. Na6FeCl8(s) + 2Na(l) → 8NaCl(s) + Fe(s) D. 2H2O2(aq) → 2H2O(l) + O2(g) E. CO2(g) + H2(g) → CO(g) + H2O(g)
A
30. Isoamyl salicylate ( = 208.25 g/mol) has a pleasant aroma and is used in perfumes and soaps. Which of the following combinations gives a 0.75 m solution of isoamyl salicylate in ethyl alcohol (d = 0.7893 g/mL)? A. 117.2 g isoamyl salicylate in 950.0 mL of ethyl alcohol B. 117.2 g isoamyl salicylate in 750.0 mL of ethyl alcohol C. 117.2 g isoamyl salicylate in 750.0 mL of solution D. 117.2 g isoamyl salicylate in 592.0 g of ethyl alcohol E. None of these choices are correct.
A
27. What is the molality of a solution prepared by dissolving 86.9 g of diethyl ether, C4H10O, in 425 g of benzene, C6H6? A. 0.362 m B. 0.498 m C. 2.01 m D. 2.76 m E. None of these choices are correct.
D
23. What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H3PO4? A. 0.20 L B. 0.57 L C. 1.8 L D. 3.6 L E. 5.1 L
E
10. Which of the following atoms has the biggest radius? A. Ti B. Cr C. Fe D. Ni E. Zn
a
13. A phosphate buffer (H2PO4-/HPO42-) has a pH of 8.3. Which of the following changes will cause the pH to increase? A. dissolving a small amount of Na2HPO4 B. dissolving a small amount of NaH2PO4 C. adding a small amount of dilute hydrochloric acid D. adding a small amount of dilute phosphoric acid E. making the buffer more concentrated by removing some water
a
18. A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode? A. Al(s) → Al3+(aq) + 3e- B. Al3+(aq) + 3e → Al(s) C. Ni(s) → Ni2+(aq) + 2e- D. Ni2+(aq) + 2e- → Ni(s) E. None of these choices are correct.
a
2. Consider the reaction CuO(s) + H2(g) → Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively? A. CuO and H2 B. H2 and CuO C. CuO and Cu D. H2O and H2 E. None of these choices are correct.
a
22. The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s), indicates that A. copper metal is a product of the cell reaction. B. hydrogen gas (H2) is a product of the cell reaction. C. Cu is the anode. D. Pt is the cathode. E. Cu2+ is the reducing agent.
a
26. The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E°cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S2O82-(aq) + 2H+ + 2I-(aq) → 2HSO4-(aq) + I2(aq) A. -1.051 V B. -2.123 V C. 1.051 V D. 2.123 V E. None of these choices are correct
a
27. The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq) + Co(s) → Cu(s) + Co2+(aq) A. -0.28 V B. -0.96 V C. 0.28 V D. 0.96 V E. None of these choices are correct
a
3. The most common oxidation state for ions of the transition elements is A. +2. B. +3. C. +4. D. +5. E. +6.
a
32. The solubility of the oxidizing agent potassium permanganate is 7.1 g per 100.0 g of water at 25°C. What is the mole fraction of potassium permanganate in this solution? A. 0.0080 B. 0.0086 C. 0.066 D. 0.45 E. 0.48
a
33. A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? Ka = 1.7 × 10-4 A. 2.87 B. 3.72 C. 3.82 D. 3.95 E. 4.66
a
39. Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq) + 2H+(aq) + 2e- 2H2O(l) E° = 1.77 V Fe3+ (aq) + e- Fe2+(aq) E° = 0.77 V Overall reaction: 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq) A. E°cell = -1.00 V, nonspontaneous B. E°cell = -1.00 V, spontaneous C. E°cell = 1.00 V, nonspontaneous D. E°cell = 1.00 V, spontaneous E. E°cell = -0.23 V, nonspontaneous
a
39. What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 × 10-4. A. 1.3 g B. 0.69 g C. 6.9 g D. 23 g E. 1.5 g
a
4. Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq) → N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true? A. CuO(s) is the oxidizing agent and copper is reduced. B. CuO(s) is the oxidizing agent and copper is oxidized. C. CuO(s) is the reducing agent and copper is oxidized. D. CuO(s) is the reducing agent and copper is reduced. E. CuO(s) is the oxidizing agent and N2(g) is the reducing agent.
a
41. Procaine hydrochloride ( = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL. A. 2.272 M B. 4.056 M C. 4.216 M D. 4.666 M E. None of these choices are correct.
a
43. Write the formula for diamminedichloroethylenediaminecobalt(III) bromide. A. [CoCl2(en)(NH3)2]Br B. [CoCl2(en)(NH3)2]Br2 C. [CoCl2(en)2(NH3)2]Br D. [CoCl2(en)2(NH3)2]Br2 E. None of these choices are correct.
a
44. When a weak acid is titrated with a strong base, the pH at the equivalence point A. is greater than 7.0. B. is equal to 7.0. C. is less than 7.0. D. is equal to the pKa of the acid. E. is equal to 14.0 - pKb, where pKb is that of the base.
a
49. The value of E°cell for the reaction 2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) is 1.59 V. Calculate ΔG° for the reaction. A. -921 kJ B. -767 kJ C. -460 kJ D. -307 kJ E. None of these choices are correct
a
57. A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? Ka = 1.3 × 10-5 A. 5.75 B. 4.94 C. 4.83 D. 4.02 E. 3.95
a
58. In the presence of a strong octahedral ligand field, the number of unpaired electrons in Co(III) will be A. 0. B. 2. C. 4. D. 6. E. None of these choices are correct
a
75. What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes? A. 16.2 g B. 33.4 g C. 40.6 g D. 81.3 g E. 163 g
a
9. How many unpaired electrons are there in the Fe3+ ion? A. 5 B. 4 C. 3 D. 2 E. 1
a
12. An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease? A. dissolving a small amount of solid sodium acetate B. adding a small amount of dilute hydrochloric acid C. adding a small amount of dilute sodium hydroxide D. dissolving a small amount of solid sodium chloride E. diluting the buffer solution with water
b
18. Which of the following will be paramagnetic? A. V5+ B. Ni2+ C. Mn7+ D. Ti4+ E. Zn
b
19. A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell? A. Ni2+(aq) + Al(s) → Al3+(aq) + Ni(s) B. 3Ni2+(aq) + 2Al(s) → 2Al3+(aq) + 3Ni(s) C. Ni(s) + Al3+(aq) → Ni2+(aq) + Al(s) D. 3Ni(s) + 2Al3+(aq) → 3Ni2+(aq) + 2Al(s) E. None of these choices are correct
b
2. Which, if any, of the following aqueous mixtures would be a buffer system? A. CH3COOH, NaH2PO4 B. H2CO3, HCO3- C. H2PO4-, HCO3- D. HSO4-, HSO3- E. None of these choices are correct.
b
20. A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn2+(aq) || I-(aq) | I2(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction? A. 2I-(aq) + Zn2+(aq) → I2(s) + Zn(s) B. I2(s) + Zn(s) → 2I-(aq) + Zn2+(aq) C. 2I-(aq) + Zn(s) → I2(s) + Zn2+(aq) D. I2(s) + Zn2+(aq) → 2I-(aq) + Zn(s) E. None of these choices are correct.
b
22. What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 × 10-5 A. 4.49 B. 4.64 C. 4.85 D. 5.00 E. 5.52
b
23. A voltaic cell can be prepared from copper and tin.What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e- Cu(s) E° = 0.34 V Sn4+(aq) + 2e- Sn2+(aq) E° = 0.13 V A. 0.47 V B. 0.21 V C. -0.21 V D. -0.47 V E. 0.42 V
b
25. What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10-4 A. 1.1 × 10-4 M B. 2.6 × 10-4 M C. 4.3 × 10-4 M D. 6.7 × 10-5 M E. None of these choices are correct.
b
29. What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75? A. < 4.00 B. 4.63 C. 4.87 D. 5.02 E. > 5.50
b
3. Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution? A. 0.10 mol L-1 HCl and 0.05 mol L-1 NaOH B. 0.10 mol L-1 HCl and 0.15 mol L-1 NH3 C. 0.10 mol L-1 HCl and 0.05 mol L-1 NH3 D. 0.10 mol L-1 HCl and 0.20 mol L-1 CH3COOH E. 0.10 mol L-1 HCl and 0.20 mol L-1 NaCl
b
31. An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer? A. 4.77 B. 4.71 C. 4.68 D. 4.62 E. None of these choices are correct.
b
31. The chemist, Anna Lytic, must prepare 1.00 kg of 15.0% (w/w) acetic acid using a stock solution which is 36.0% (w/w) acetic acid (d = 1.045 g/mL). Which of the following combinations will give her the solution she wants? A. 417 mL of 36% acetic acid in 583 mL of distilled water B. 417 g of 36% acetic acid in 583 g of distilled water C. 360 mL of 36% acetic acid in 640 mL of distilled water D. 360 g of 36% acetic acid in 640 g of distilled water E. 150 g of 36% acetic acid in 850 g of distilled water
b
34. Examine the following half-reactions and select the strongest reducing agent among the species listed. HgO(s) + H2O(l) + 2e- Hg(l) + 2OH-(aq) E° = 0.0977 V Zn(OH)2(s) + 2e- Zn(s) + 2OH-(aq) E° = -1.25 V Ag2O(s) + H2O(l) + 2e- Ag(s) + 2OH-(aq) E° = 0.342 V B(OH)3(aq) + 7H+(aq) + 8e- BH4-(aq) + 3H2O(l) E° = -0.481 V A. Hg(l) B. Zn(s) C. Ag(s) D. BH4-(aq) E. Zn(OH)2(s)
b
34. If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, Ka = 6.8 × 10-4. A. 7.13 B. 2.54 C. 1.57 D. 3.17 E. 4.86
b
36. The nuclide Pb-210 undergoes three successive decays (beta, alpha, and beta, respectively) to form a stable nuclide. What are the three nuclides that form from Pb-210 in this decay series? A. Tl-210, Au-206, Pt-206 B. Bi-210, Tl-206, Pb-206 C. Pb-209, Hg-205, Hg-204 D. Bi-210, Pb-206, Bi-206 E. None of these choices are correct
b
38. Give the systematic name for [Cu(NH3)4]Cl2. A. dichlorotetraamminecuprate(II) B. tetraamminecopper(II) chloride C. copper(II) ammonium chloride D. tetraaminocopper(II) chloride E. None of these choices are correct
b
43. Children under the age of 6 with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead? A. 4.8 × 10-10 m B. 4.8 × 10-7 m C. 4.8 × 10-4 m D. 4.8 × 10-1 m E. None of these choices are correct.
b
43. When a strong acid is titrated with a strong base, the pH at the equivalence point A. is greater than 7.0. B. is equal to 7.0. C. is less than 7.0, but is not 3.5. D. is equal to the pKa of the acid. E. is equal to 3.5.
b
44. What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq) A. 1.2 × 105 B. 1.4 × 1010 C. 8.6 × 10-6 D. 7.1 × 10-11 E. 2.3 × 1023
b
47. Cesium-134 is a β emitter with a half-life of 2.0 years. How much of a 2.50-g sample of cesium-134 will remain after 10 years? A. 0.0024 g B. 0.078 g C. 0.25 g D. 0.50 g E. None of these choices are correct.
b
48. Consider the reaction in the lead-acid cell Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(aq) + 2H2O(l) for which E°cell = 2.04 V at 298 K. ΔG° for this reaction is A. -3.94 × 105 kJ. B. -3.94 × 102 kJ. C. -1.97 × 105 kJ. D. -7.87 × 102 kJ. E. None of these choices are correct.
b
55. In the spectrochemical series, which one of the following ligands has the strongest field? A. H2O B. CN- C. NH3 D. OH- E. Cl-
b
56. A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.77 × 10-4 A. 4.00 B. 3.88 C. 3.63 D. 3.51 E. 3.47
b
6. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO4(aq) + OH-(aq) → Al2O3(s) + S2-(aq) + H2O(l) A. 1. B. 3. C. 4. D. 8. E. None of these choices are correct
b
60. A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. mL NaOH added 5.00 10.00 1.00 2.00 pH 6.98 7.46 7.93 10.31 What is the Ka for HClO? A. 1.1 × 10-7 B. 3.5 × 10-8 C. 1.2 × 10-8 D. 4.9 × 10-11 E. None of these choices are correct.
b
64. A battery that cannot be recharged is a A. fuel cell. B. primary battery. C. secondary battery. D. simple battery. E. flow battery.
b
7. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO4(aq) → Re(s) + Zn2+(aq) (acidic solution) A. 2. B. 7. C. 8. D. 16. E. None of these choices are correct.
b
75. The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2? A. 4.9 × 10-2 B. 1.7 × 10-5 C. 8.5 × 10-6 D. 4.2 × 10-6 E. < 1.0 × 10-6
b
76. Lysine is an amino acid that is an essential part of nutrition but which is not synthesized by the human body. What is the molar mass of lysine if 750.0 mL of a solution containing 8.60 g of lysine has an osmotic pressure of 1.918 atm? Temperature = 25.0°C A. 110. g/mol B. 146 g/mol C. 220. g/mol D. 1340 g/mol E. 1780 g/mol
b
82. Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10-18 A. 4.0 × 10-5 M B. 1.8 × 10-5 M C. 4.0 × 10-6 M D. 1.5 × 10-5 M E. < 1.0 × 10-5 M
b
85. Which of the following substances has the greatest solubility in water? A. Ba(IO3)2, Ksp = 1.5 × 10-9 B. PbF2, Ksp = 3.6 × 10-8 C. SrSO4, Ksp = 3.2 × 10-7 D. CuCl, Ksp = 1.9 × 10-7 E. CdS, Ksp = 1.0 × 10-24
b
88. Use the following information to calculate the solubility product constant, Ksp, for CuCl. A saturated solution of CuCl in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid CuCl residue recovered in the beaker was found to weigh 0.041g. A. Ksp = 1.7 × 10y9 B. Ksp = 1.7 × 10y7 C. Ksp = 1.7 × 10-5 D. Ksp = 4.3 × 10-4 E. Ksp = 2.1 × 10-2
b
1. Select the type of interaction that best describes the attraction between Mg2+ ions and water molecules. A. dipole-dipole B. dipole-induced dipole C. ion-dipole D. ion-induced dipole E. ion-hydrogen bond
c
10. Consider the following redox equation Mn(OH)2(s) + MnO4(aq) → MnO42-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present? A. 4, reactant side B. 4, product side C. 6, reactant side D. 6, product side E. None of these choices are correct.
c
12. A solution of sucrose (sugar) in water is in equilibrium with solid sucrose. If more solid sucrose is now added, with stirring, A. the concentration of the solution will increase. B. the concentration of the solution will decrease. C. the concentration of the solution will remain the same. D. the volume of solution will increase. E. a supersaturated solution will be produced.
c
16. Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH? A. [CH3COOH] = 0.25 M, [CH3COO-] = 0.25 M B. [CH3COOH] = 0.75 M, [CH3COO-] = 0.75 M C. [CH3COOH] = 0.75 M, [CH3COO-] = 0.25 M D. [CH3COOH] = 0.25 M, [CH3COO-] = 0.75 M E. [CH3COOH] = 1.00 M, [CH3COO-] = 1.00 M
c
16. Which of the following ions is least likely to form colored compounds? A. Mn2+ B. Cr5+ C. Sc3+ D. Fe3+ E. Co2+
c
21. The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s), indicates that A. Co is the reducing agent. B. Co2+ ions are oxidized. C. Al is the reducing agent. D. Al3+ is the reducing agent. E. aluminum metal is the cathode
c
23. What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid) and 0.75 M NaHC6H6O6 (sodium ascorbate)? For ascorbic acid, Ka = 6.8 × 10-5 A. 3.76 B. 3.99 C. 4.34 D. 4.57 E. 5.66
c
24. What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? For NaH2PO4, Ka = 6.2 × 10-8 A. 6.51 B. 6.91 C. 7.51 D. 7.90 E. 8.13
c
25. What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4(aq) + 8H(aq) + 8e Cl-(aq) + 4H2O(l) E° = 1.389 V VO2(aq) + 2H(aq) + e- VO(aq) + H2O(l) E° = 0.991 V A. -0.398 V B. -2.380 V C. 0.398 V D. 2.380 V E. None of these choices are correct.
c
28. Which of the following is considered a bidentate ligand? A. cyanide, CN- B. thiocyanate, SCN- C. oxalate, C2O42- D. nitrite, NO2- E. hydroxide, OH-
c
3. Consider the following balanced redox reaction Mn2+(aq) + S2O82-(aq) + 2H2O(l) → MnO2(s) + 4H(aq) + 2SO42-(aq) Which of the following statements is true? A. Mn2+(aq) is the oxidizing agent and is reduced. B. Mn2+(aq) is the oxidizing agent and is oxidized. C. Mn2+(aq) is the reducing agent and is oxidized. D. Mn2+(aq) is the reducing agent and is reduced. E. Manganese does not change its oxidation number in this reaction.
c
32. Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr4(aq) + 3e- Au(s) + 4Br-(aq) E° = 0.854 V Mn2+(aq) + 2e- Mn(s) E° = -1.185 V K+(aq) + e- K(s) E° = -2.931 V F2O(aq) + 2H+(aq) + 4e- 2F-(aq) + H2O(l) E° = 2.153 V A. AuBr4-(aq) B. Mn2+(aq) C. K+(aq) D. F2O(aq) E. H+(aq)
c
35. Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)3(s) + 3e- Cr(s) + 3OH-(aq) E° = -1.48 V SnO2(s) + 2H2O(l) + 4e- Sn(s) + 4OH-(aq) E° = -0.945 V MnO2(s) + 4H+(aq) + 2e- Mn2+(aq) + 2H2O(l) E° = 1.224 V Hg2SO4(s) + 2e- 2Hg(l) + SO42-(aq) E° = 0.613 V A. Cr(s) B. Sn(s) C. Mn2+(aq) D. Hg(l) E. OH-(aq)
c
36. Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I2(s) + 2e- 2I-(aq) E° = 0.53 V Cr3+(aq) + 3e- Cr(s) E° = -0.74 V Overall reaction: 2Cr(s) + 3I2(s) → 2Cr3+(aq) + (aq) + 6I-(aq) A. E°cell = -1.27 V, spontaneous B. E°cell = -1.27 V, nonspontaneous C. E°cell = 1.27 V, spontaneous D. E°cell = 1.27 V, nonspontaneous E. E°cell = 1.54 V, spontaneous
c
39. A 0.89% (w/v) sodium chloride solution is referred to as physiological saline solution because it has the same concentration of salts as human blood. What is the molarity of a physiological saline solution? A. 0.0028 M B. 0.015 M C. 0.15 M D. 0.30 M E. 0.35 M
c
41. Give the systematic name for [CoCl3(H2O)]-. A. cobalt(II) chloride monohydrate B. aquatrichlorocobalt(II) C. aquatrichlorocobaltate(II) D. aquatrichlorocobaltite(I) E. None of these choices are correct
c
43. The isotope Mg has a half-life of 21 hours. If a sample initially contains exactly 10000 atoms of Mg approximately how many of these atoms will remain after one week? A. 1250 B. 78 C. 39 D. 0 E. None of these choices are correct.
c
44. The isotope Au has a half-life of 7.5 seconds. If a sample contains 144 atoms of approximately how many such atoms were there present 30 seconds earlier? A. 576 B. 1152 C. 2304 D. 4320 E. 4.30 × 108
c
44. Write the formula for sodium tetracyanonickelate(II). A. Na[Ni(CN)4] B. Na[Ni(CN)4]2 C. Na2[Ni(CN)4] D. Na4[Ni(CN)4] E. None of these choices are correct.
c
46. Iodine-131, t1/2 = 8.0 days, is used in diagnosis and treatment of thyroid gland diseases. If a laboratory sample of iodine-131 initially emits 9.95 × 1018 β particles per day, how long will it take for the activity to drop to 6.22 × 1017 β particles per day? A. 2.0 days B. 16 days C. 32 days D. 128 days E. None of these choices are correct.
c
48. From the following list of aqueous solutions and water, select the one with the highest boiling point. A. 1.0 m KNO3 B. 0.75 m NaCl C. 0.75 m CuCl2 D. 2.0 m C12H22O11 (sucrose) E. pure water
c
54. The crystal field splitting energy, Δ, A. is larger for tetrahedral complexes than for octahedral complexes. B. depends on the metal but not on the ligand. C. determines the color of a complex. D. is larger for ionic ligands like chloride than for molecular ligands like carbon monoxide, CO. E. determines the charge of a complex
c
56. Which of the following ions could exist in either the high-spin or low-spin state in an octahedral complex? A. Sc3+ B. Ni2+ C. Mn2+ D. Ti4+ E. Zn2+
c
58. A voltaic cell consists of a Hg/Hg22+ electrode (E° = 0.85 V) and a Sn/Sn2+ electrode (E° = -0.14 V). Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C. A. 0.0001 M B. 0.0007 M C. 0.005 M D. 0.03 M E. 0.05 M
c
59. Two aqueous solutions are prepared: 2.0 m Cu(NO3)2 and 2.0 m NaBr. Which of the following statements is true? A. The Cu(NO3)2 solution has a higher vapor pressure and lower freezing point than the NaBr solution. B. The Cu(NO3)2 solution has a higher vapor pressure and higher freezing point than the NaBr solution. C. The Cu(NO3)2 solution has a lower vapor pressure and lower freezing point than the NaBr solution. D. The Cu(NO3)2 solution has a lower vapor pressure and higher freezing point than the NaBr solution. E. None of these choices are correct.
c
6. Consider the expression below, showing the terms which contribute to the heat of solution, ΔHsoln: ΔHsoln = ΔHsolute + ΔHsolvent + ΔHmix Which of the following sets correctly shows the signs (positive or negative) of the three terms on the right hand side of the equation? A. ΔHsolute > 0; ΔHsolvent > 0; ΔHmix > 0 B. ΔHsolute < 0; ΔHsolvent < 0; ΔHmix < 0 C. ΔHsolute > 0; ΔHsolvent > 0; ΔHmix < 0 D. ΔHsolute < 0; ΔHsolvent < 0; ΔHmix > 0 E. ΔHsolute < 0; ΔHsolvent > 0; ΔHmix < 0
c
65. A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA? A. 37.0 g/mol B. 81.0 g/mol C. 128 g/mol D. 20.3 g/mol E. 211 g/mol
c
66. When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid. A. H2S B. H2C2O4 C. H2C4H4O6 D. H2Se E. H2Te
c
66. Which of the following materials is put into a nuclear reactor to slow the chain reaction? A. heavy water B. moderators C. control rods D. reflectors E. chlorine
c
67. It is believed that two carbon-12 nuclei can react in the core of a supergiant star to form sodium-23 and hydrogen-1. Calculate the energy released from this reaction for each mole of hydrogen formed. The masses of carbon-12, sodium-23, and hydrogen-1 are 12.0000 amu, 22.989767 amu, and 1.007825, respectively. A. 2.16 × 1014 kJ B. 2.16 × 1011 kJ C. 2.16 × 108 kJ D. 2.16 × 105 kJ E. None of these choices are correct
c
69. Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C A. 44.1 g/mol B. 65.8 g/mol C. 117 g/mol D. 131.6 g/mol E. 553 g/mol
c
7. The ground state electronic configuration of Cr2+ is A. [Ar]4s13d5. B. [Ar]4s23d4. C. [Ar]3d4. D. [Ar]4s13d3. E. [Ar]4s23d2.
c
79. The Tyndall effect A. is observed in concentrated solutions. B. is observed only in dilute solutions. C. is observed in colloidal dispersions. D. is caused by Brownian motion. E. is used to determine the osmotic pressure of solutions.
c
80. Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr2O72-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A? A. 6.2 minutes B. 12.4 minutes C. 18.6 minutes
c
81. Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 × 10-9 A. 1.4 × 10-3 M B. 3.4 × 10-4 M C. 8.7 × 10-4 M D. 5.1 × 10-5 M E. < 1.0 × 10-5 M
c
87. Use the following information to calculate the solubility product constant, Ksp, for PbCl2. A saturated solution of PbCl2 in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid PbCl2residue recovered in the beaker amounted to 0.0162 moles. A. Ksp = 6.9 × 10-8 B. Ksp = 4.3 × 10-6 C. Ksp = 1.7 × 10-5 D. Ksp = 2.6 × 10-4 E. Ksp = 3.2 × 10-2
c
9. Which of the following acids should be used to prepare a buffer with a pH of 4.5? A. HOC6H4OCOOH, Ka = 1.0 × 10-3 B. C6H4(COOH)2, Ka = 2.9 × 10-4 C. CH3COOH, Ka = 1.8 × 10-5 D. C5H5O5COOH, Ka = 4.0 × 10-6 E. HBrO, Ka = 2.3 × 10-9
c
1. Which of the following elements has the ground state electron configuration, [Xe]4f145d106s1? A. Hg B. Ag C. Hf D. Au E. Th
d
15. The Henry's Law constant (k) for carbon monoxide in water at 25°C is 9.71 × 10-4 mol/(L·atm). How many grams of CO will dissolve in 1.00 L of water if the partial pressure of CO is 2.75 atm? A. 3.53 × 10-4 g B. 2.67 × 10-3 g C. 9.89 × 10-3 g D. 7.48 × 10-2 g E. None of these choices are correct.
d
15. Which of the following ions is most likely to form colored compounds? A. Sc3+ B. Cu+ C. Zn2+ D. Cr3+ E. Ca2+
d
17. A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? A. Cu(s) → Cu2+(aq) + 2e- B. Cu2+(aq) + 2e- → Cu(s) C. Ag(s) → Ag+(aq) + e- D. Ag+(aq) + e- → Ag(s) E. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
d
18. A saturated solution of carbon dioxide in water contains 3.00 g of CO2 when the CO2 partial pressure is 8.0 atm. What mass of CO2 will escape if the partial pressure is lowered to 3.2 atm? A. 0.90 g B. 1.20 g C. 1.40 g D. 1.80 g E. 2.20 g
d
29. Which one of the following normally acts as a bidentate ligand in complexes with transition metal ions? A. CN- B. EDTA4- C. SCN- D. ethylene diamine E. ethylene, C2H4
d
30. Examine the following half-reactions and select the strongest oxidizing agent among the substances. [PtCl4]2-(aq) + 2e- Pt(s) + 4Cl-(aq) E° = 0.755 V RuO4(s) + 8H+(aq) + 8e- Ru(s) + 4H2O(l) E° = 1.038 V FeO42-(aq) + 8H+(aq) + 3e- Fe3+(aq) + 4H2O(l) E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e- XeO3(aq) + 3H2O(l) E° = 2.42 V A. [PtCl4]2-(aq) B. RuO4(s) C. HFeO4- (aq) D. H4XeO6(aq) E. Cl-(aq)
d
32. A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 × 10-5 A. 4.57 B. 4.52 C. 4.87 D. 4.92 E. 4.97
d
33. What is the coordination number of cobalt in the complex ion [Co(en)Cl4]-? (en = ethylenediamine) A. 1 B. 2 C. 4 D. 6 E. 8
d
33. What is the mole fraction of Ne in a mixture containing 10.1 g of Ne, 79.9 g of Ar, and 83.8 g of Kr? A. 0.40 B. 0.25 C. 0.20 D. 0.14 E. 0.058
d
35. A solution is prepared by dissolving 20.0 g of K2HPO4 and 25.0 g of KH2PO4 in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H3PO4), Ka2 = 6.2 × 10-8. A. 7.70 B. 7.42 C. 7.21 D. 7.00 E. 6.72
d
35. Which of the following series of radioactive decays would convert Pa-234 to Ra-226? A. beta, alpha, beta B. alpha, alpha C. beta, alpha, alpha, beta D. beta, alpha, alpha E. alpha, beta, gamma
d
37. Sodium hydroxide is a common ingredient in drain cleaners such as Drano. The mole fraction of sodium hydroxide in a saturated aqueous solution is 0.310. What is the molality of the solution? A. 0.310 m B. 0.690 m C. 1.24 m D. 12.4 m E. 25.0 m
d
38. Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O2(g) + 4H+(aq) + 4e- 2H2O(l) E° = 1.229 V Al3+(aq) + 3e- Al(s) E° = -1.662 V Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq) → 4Al3+(aq) + 6H2O(l) A. E°cell = -2.891 V, nonspontaneous B. E°cell = -2.891 V, spontaneous C. E°cell = 2.891 V, nonspontaneous D. E°cell = 2.891 V, spontaneous E. None of these choices are correct.
d
38. The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H2CO3) and the bicarbonate (hydrogen carbonate, HCO3-) ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, Ka1 = 4.2 × 10- 7. A. [bicarbonate]/[carbonic acid] = 0.11 B. [bicarbonate]/[carbonic acid] = 0.38 C. [bicarbonate]/[carbonic acid] = 2.65 D. [bicarbonate]/[carbonic acid] = 9.4 E. None of these choices are correct.
d
40. Give the systematic name for Cr(CO)3(NH3)3. A. chromiumtriaminotricarbonyl B. triamminechromium carbonate C. triamminetricarbonylchromate(0) D. triamminetricarbonylchromium(0)
d
45. What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.61 V 2Cr(s) + 3Pb2+(aq) 3Pb(s) + 2Cr3+(aq) A. 4.1 × 1020 B. 8.2 × 1030 C. 3.3 × 1051 D. 7.4 × 1061 E. > 9.9 × 109
d
46. The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of the non-volatile solute in the solution? A. 0.87 B. 0.69 C. 0.32 D. 0.13 E. 0.045
d
46. When a weak acid is titrated with a weak base, the pH at the equivalence point A. is greater than 7.0. B. is equal to 7.0. C. is less than 7.0. D. is determined by the sizes of Ka and Kb. E. is no longer affected by addition of base.
d
48. Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak base (0.10 mol L-1) with HCl of the same concentration? A. A B. B C. C D. D E. E
d
49. A pure sample of tritium, 3H, was prepared and sealed in a container for a number of years. Tritium undergoes β decay with a half-life of 12.32 years. How long has the container been sealed if analysis of the contents shows there are 5.25 mol of 3H and 6.35 mol of 3He present? A. 2.34 y B. 3.38 y C. 9.77 y D. 14.1 y E. 25.6 y
d
49. What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior? A. 0.60 M B. 0.40 M C. 0.30 M D. 0.15 M E. 0.10 M
d
5. When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be——. I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(l) A. 1 B. 2 C. 4 D. 10 E. None of these choices are correct.
d
5. Which, if any, of the following features is common to soaps, detergents, phospholipids, and channel-forming antibiotics? A. They all contain fatty acids. B. They all contain phosphate groups. C. They all contain polypeptide chains. D. Their function depends on the dual polarity of their molecules. E. None of these choices are correct.
d
50. Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.05 MNaOH? A. bromphenol blue, pH range: 3.0-4.5 B. bromcresol green, pH range: 3.8-5.4 C. alizarin, pH range: 5.7-7.2 D. phenol red, pH range: 6.9-8.2 E. phenolphthalein, pH range: 8.0-10.1
d
51. In living organisms, C-14 atoms disintegrate at a rate of 15.3 atoms per minute per gram of carbon. A charcoal sample from an archaeological site has a C-14 disintegration rate of 9.16 atoms per minute per gram of carbon. Estimate the age of this sample. The half-life of C-14 is 5730 years. A. 3170 years B. 3430 years C. 4020 years D. 4790 years E. 6750 years
d
54. Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) 6I-(aq) + 2MnO4(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 × 10-7. Calculate ΔG° for the reaction at 25°C. A. -15.1 kJ B. -34.7 kJ C. 15.1 kJ D. 34.7 kJ E. None of these choices are correct.
d
55. Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) 6I-(aq) + 2MnO4(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 × 10-7. Calculate E°cell for the reaction at 25°C. A. -0.36 V B. -0.18 V C. -0.12 V D. -0.060 V E. None of these choices are correct.
d
59. Which of the following octahedral complexes should have the largest crystal field splitting energy, Δ? A. [Cr(H2O)6]3+ B. [Cr(SCN)6]3- C. [Cr(NH3)6]3+ D. [Cr(CN)6]3- E. [Cr(en)3]3+ (en = ethylenediamine)
d
6. 108, 49 --> 108, 48 In the equation above, what particle or type of radiation needs to be included on the right-hand side in order to balance it? A. alpha B. beta C. gamma D. positron E. proton
d
6. Which of the following has the highest buffer capacity? A. 0.10 M H2PO4-/0.10 M HPO42- B. 0.50 M H2PO4-/0.10 M HPO42- C. 0.10 M H2PO4-/0.50 M HPO42- D. 0.50 M H2PO4-/0.50 M HPO42- E. They all have the same buffer capacity
d
63. Which one of the following statements relating to the glass electrode is correct? A. The glass electrode detects hydrogen gas. B. The glass of a glass electrode serves to conduct electrons. C. When pH is measured, only a single electrode, the glass electrode, need be used. D. The potential of the glass electrode varies linearly with the pH of the solution. E. None of these choices are correct
d
67. Carbon tetrachloride, once widely used in fire extinguishers and as a dry cleaning fluid, has been found to cause liver damage to those exposed to its vapors over long periods of time. What is the boiling point of a solution prepared by dissolving 375 g of sulfur (S8, = 256.5 g/mol) in 1250 g of CCl4? Kb = 5.05°C/m, boiling point of pure CCl4 = 76.7°C? A. 70.8°C B. 75.2°C C. 78.2°C D. 82.6°C E. >85°C
d
68. Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital ( = 184.2 g/mol) is one of the simplest of these drugs. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? Kb = 3.07°C/m; boiling point of pure acetic acid = 117.9°C A. 117.0°C B. 117.7°C C. 118.1°C D. 118.8°C E. >120°C
d
74. What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes? A. 0.419 g B. 6.29 g C. 12.6 g D. 25.2 g
d
76. The solubility of calcium chromate is 1.56 × 10-3 g/100 mL of solution. What is the Ksp for CaCrO4? A. 2.4 × 10-4 B. 1.5 × 10-5 C. 7.6 × 10-6 D. 1.0 × 10-8 E. < 1.0 × 10-8
d
8. The ground state electronic configuration of Zn2+ is A. [Ar]4s23d8. B. [Ar]4s23d10. C. [Ar]4s13d9. D. [Ar]3d10. E. [Ar]3d8.
d
16. Methane has a Henry's Law constant (k) of 9.88 × 10-2 mol/(L·atm) when dissolved in benzene at 25°C. How many grams of CH4 will dissolve in 3.00 L of benzene if the partial pressure of CH4 is 1.48 atm? A. 0.0667 g B. 0.146 g C. 2.34 g D. 4.83 g E. 7.02 g
e
17. Which of the following will be diamagnetic? A. Ni2+ B. Cr2+ C. Mn2+ D. Co3+ E. Ti4+
e
2. Under physiological conditions, amino acids in solution carry A. no electrical charges. B. a net positive charge, due to an -NH3+ group or groups. C. a net negative charge, due to a -COO- group or groups. D. both -NH2 and -COOH groups. E. both -NH3+ and -COO- groups
e
2. Which one of the following has the ground state electron configuration [Ar]3d104s1? A. In+ B. Cd2+ C. Ag+ D. Ag E. Cu
e
20. Potassium fluoride is used for frosting glass. Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution. A. 0.304 M B. 0.349 M C. 1.35 M D. 3.29 M E. 6.01 M
e
30. A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? A. 3.67 B. 3.78 C. 3.81 D. 3.85 E. 3.95
e
31. Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr2+(aq) + 2e- Cr(s) E° = -0.913 V Fe2+(aq) + 2e- Fe(s) E° = -0.447 V Sr2+(aq) + 2e- Sr(s) E° = -2.89 V Co2+(aq) + 2e- Co(s) E° = -0.28 V A. Cr2+(aq) B. Fe(s) C. Fe2+(aq) D. Sr2+(aq) E. Co2+(aq)
e
4. Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L-1 aqueous NH3, will produce a buffer solution? A. 0.10 mol L-1 HCl B. 0.20 mol L-1 HCl C. 0.10 mol L-1 CH3COOH D. 0.050 mol L-1 NaOH E. 0.20 mol L-1 NH4Cl
e
48. Palladium-107 undergoes β decay (t1/2 = 6.5 × 105 yr) to form silver-107. How long will it take for 0.150 mol of silver-107 to form from 1.25 mol of palladium-107? A. 2.0 × 107 y B. 1.4 × 107 y C. 1.2 × 106 y D. 8.3 × 105 y E. 1.2 × 105
e
5. A feature of transition metal chemistry is that these elements exhibit multiple oxidation states. Which one of the following elements exhibits the smallest number of different oxidation states? A. Ti B. Cr C. Mn D. Co E. Zn
e
57. A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V). Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C. A. 0.001 M B. 0.002 M C. 0.01 M D. 0.02 M E. 0.04 M
e
60. A voltaic cell consists of a Ag/Ag+ electrode (E° = 0.80 V) and a Fe2+/Fe3+ electrode (E° = 0.77 V) with the following initial molar concentrations: [Fe2+] = 0.30 M; [Fe3+] = 0.10 M; [Ag+] = 0.30 M. What is the equilibrium concentration of Fe3+? (Assume the anode and cathode solutions are of equal volume, and a temperature of 25°C.) A. 0.030 M B. 0.043 M C. 0.085 M D. 0.11 M E. 0.17
e
61. Which of the following ligands is most likely to form a high spin octahedral complex with cobalt(II)? A. CN- B. en (ethylenediamine) C. NO2- D. CO E. I-
e
65. Determine the freezing point of a solution that contains 0.31 mol of sucrose in 175 g of water. Kf = 1.86°C/m A. 3.3°C B. 1.1°C C. 0.0°C D. -1.1°C E. -3.3°C
e
9. If a solute dissolves in an endothermic process A. H bonds must exist between solvent and solute. B. strong ion-dipole forces must exist in the solution. C. the solute must be a gas. D. the entropy of the solution is immaterial. E. the entropy of the solution must be greater than that of its pure components.
e
