5. Calculate the concentration of Ag⁺ in a solution prepared by mixing 150.0 mL 1.0×10^－3 M AgNO₃ with 200.0 mL 5.00 M Na₂S₂O₃.(K₁ = 7.4×10⁸, K₂ = 3.9×10⁴)
(A) 1.8 x 10^-18 mol/L
(B) 4.3 x 10^-4 mol/L
(C) 3.8 x 10^-9 mol/L
(D) 8.30 x 10^-4 mol/L
(E) 2.86 x 10^-3 mol/L

1. Which of the following names is correct? (A) iodine trichlorite, ICl3 (B) phosphorus pentoxide, P2O5 (C) chlorous acid, HClO2 (D) lithium hydrogen, LiH (E) calcium(II) oxide, CaO

2. Calculate the pH of a 0.010 M aluminium chloride solution. The Ka value for Al(H2O)63+ is 1.4 × 10-5. (A) pH=1.35 (B) pH=2.38 (C) pH=3.43 (D) pH=4.31 (E) pH=5.36

3. Hydrogen cyanide gas (HCN), a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka =6.2 ×10-10) when dissolved in water. If a 50.0 mL sample of 0.100M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution at the equivalence point of the titration. (A) pH=3.05 (B) pH=8.49 (C) pH=9.21 (D) pH=10.95 (E) pH=11.36

4. Which of the following molecules are nonlinear?NO2–, C2H2, N3–, HCN, CO2, H2O2 , N2O (central atom is N) (A) C2H2, HCN (B)NO2–, H2O2 (C)CO2, N3–(D) N3–, NO2–(E) N2O, H2O2

6. An aqueous solution of 10.00 g of catalase, an enzyme found in the liver, has a volume of 1.00 L at 27℃. The solution’s osmotic pressure at 27℃ is found to be 0.745 torr. Calculate the molar mass of catalase. (A) 3.86 x 108 g/mol (B) 4.15 x 104g/mol (C) 9.8 x 106 g/mol (D) 3.30 x 102g/mol (E) 2.51 x 105 g/mol

7. You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka value of HA ? (A) 2.1 x 10-6 (B) 3.8 x 10-6 (C) 4.7 x 10-2 (D) 7.4 x 10-8 (E) 6.3 x 10-4

8. Which of the following is the correct order for molecules from most to least polar? (A) CH4 > CF2Cl2 > CF2H2 > CCl4 > CCl2H2 (B) CH4 > CF2H2 > CF2Cl2 > CCl4 > CCl2H2 (C) CF2Cl2 > CF2H2 > CCl2H2 > CH4 = CCl4   (D) CF2H2 > CCl2H2 > CF2Cl2 > CH4 = CCl4 (E) CF2Cl2 > CF2H2 > CCl4 > CCl2H2 > CH4

9. Which of the following molecules exhibits chirality? I. 1-chloroethanol II. 2-chloroethanol III. 2-chloropropane IV. 2-chlorobutane V. 3-chloropentane (A) I, III (B) II, IV (C) II, III (D) I, IV (E) II, V

10. At a particular temperature, 12.0 moles of SO3 is placed into a 3.0 L rigid container, and the SO3 dissociates by the reaction 2SO3(g)⇌ 2SO2(g) + O2(g)At equilibrium, 3.0 moles of SO2 is present. Calculate K for this reaction. (A) 0.033 (B) 0.056 (C) 0.44 (D) 0.22 (E) 0.55

11. Assuming that the combustion of hydrogen gas provides three times as much energy per gram as gasoline, calculate the volume of liquid H2 (density = 0.0710 g/mL) required to furnish the energy contained in 80.0 L (about 20 gal) of gasoline (density = 0.740 g/mL). Calculate also the volume that this hydrogen would occupy as a gas at 1.00 atm and 25°C. At 1.00 atm and 25°C, the hydrogen gas needed to replace 20 gal of gasoline occupies a volume of                   L. (A) 277 (B) 19700 (C) 59200 (D) 239000 (E) 977000