16. In a 0.10-M aqueous solution of pyridine (Kь = 1.7 × 10^-9), the percentage of pyridine (C₅H₅N) that forms pyridinium ion, C₅H₅NH⁺, is _____%.
(A) 0.013
(B) 6.4
(C) 4.2
(D) 1.3
(E) 5.5

12. A certain metal fluoride crystalizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal ions occupy the body centers of half the cubes. The formula of the metal fluoride is thus_____. (A) MF (B) MF3 (C) MF5 (D) MF4 (E) MF2

13. The solubility of CaCl2 in cold water is 74.5 g per 100.0 g water. Assuming i = 2.6 for CaCl2, the freezing point for a saturated solution of CaCl2 will be _____°C. (A)0 (B) -0.32 (C) -13 (D) -32 (E) -37.4

14.For the reaction A →products, successive half-lives are observed to be 10.0, 20.0 and 40.0 min for an experiment in which [A]0 = 0.10 M. Based on the information, the concentration of A after 30 min of the reaction is ＿ M (A) 0.008 (B) 0.30 (C) 0.025 (D) 0.011 (E) 0.0021

15. Suppose the reaction system 2HI(g)⇌H2(g) + I2(g) has already reached equilibrium. Which of the following statements correctly predict the effect of each change on the equilibrium position? (A) Additional H2(g) added to the system will shift to the right to obtain the equilibrium. (B) As an exothermic reaction, the system will shift to the right to attain the equilibrium when increasing the system temperature. (C) When iodine gas is removed, the system will shift to the left to achieve the equilibrium. (D) Addition of argon gas into the reaction system will shift to the right to achieve the equilibrium. (E) When volume of the reaction container is doubled, the change will have no effects on its equilibrium.

17. Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. After adding 10.0 mL of the KOH solution, the pH of the resulting solution is _____. (A) 1.15 (B) 7.00 (C) 2.72 (D) 0.85 (E) 4.26

18. Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions are mixed? (A) 0.1 M KOH and 0.1 M CH3NH3Cl (B) 0.1 M KOH and 0.2 M CH3NH3Cl (C) 0.1 M KOH and 0.2 M CH3NH2 (D) 0.2 M KOH and 0.1 M CH3NH2 (E) 0.2 M KOH and 0.1 M CH3NH3CI

19. Which of the following substances does not show increased solubility as the pH of the solution becomes more acidic? (A) Hg2Cl2, Ksp = 1.1 × 10-18 (Hg22+ is the cation in solution.) (B) Ag3PO4, Ksp = 1.8 × 10-18 (C) CaCO3, Ksp = 8.7 × 10-9 (D) CdCO3, Ksp = 5.2 × 10-12 (E) Sr3(PO4)2, Ksp = 1.0 × 10-31

20. For the reaction at 800 K: N2(g) + 3F2(g)→2NF3(g), an equilibrium mixture contains the partial pressures of P(nitrogen) = 0.021 atm, P(fluorine) = 0.063 atm, and P(nitrogen trifluoride) = 0.48 atm. The △G° for the reaction at 527°C is thus _____kJ/mol. (A) 17 (B)-50 (C) 50 (D)-17 (E)-71

21. Which one of the following statements is correct? (A) The value of S° for N2O at 0 K is greater than that for He at 10 K. (B) At 1 atm and 25°C, the value of S° for He(g) is greater than that for N2O(g). (C) The sign of S° for the reaction of 2H2S(g) + SO2(g) → 3Srhombic(s) + 2H2O(g) is negative. (D) The sign of S° for the reaction of 2SO3(g) → 2SO2(g) + O2(g) is negative. (E) The sign of S° for the reaction of Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g) is only positive.

22. When electrolyzing a sodium chloride solution at 50°C and 2.50 atm, the volume of _____ L H2(g) is acquired in addition of the production of 257 L Cl2(g) with both volumes measured in the same time. (A) 257(B) 128.5(C) 85.7(D) 514(E) 771