10. For which of the following compounds does 1.0 g represent 5.55×10-2 mol?
(A) NO2
(B) H2O
(C) C2H6
(D) NH3

11. A 12.0-g sample of HF is dissolved in water to give 3.1×102 mL of solution. The concentration of the solution is (A) 3.9 M (B) 3.7 M (C) 0.19 M (D) 1.9 M

12. Lead(II) nitrate reacts with sodium chloride in aqueous solution to form a precipitate. What is the net ionic equation for this reaction? (A) Pb2+(aq) + 2NO3–(aq)  Pb(NO3)2(s) (B) Na+(aq) + Cl–(aq)  NaCl(s) (C) Pb2+(aq) + 2Cl–(aq)  PbCl2(s) (D) Na+(aq) + NO3–(aq)  NaNO3(s)

13. Air is 79% N2 and 21% O2 by volume. Calculate the density of air at 1.0 atm, 25°C. (A) 0.590 g/L (B) 1.18 g/L (C) 2.46 g/L (D) 14.1 g/L

14. Which of the following is a conjugate acid-base pair? (A) HCl/OCl3– (B) H3PO4/PO43– (C) NH4+/NH3 (D) H3O+/OH–

15. The strong acid HA is added to water. Which of the following is the strongest base in the system? (A) HA (B) A– (C) H2O (D) H3O+

16. Identify the strongest base. (A) CH3O– (B) CH3OH (C) CN– (D) NO3–

17. What concentration of HF (Ka = 7.2×10–4) has the same pH as that of 0.068 M HCl? (A) 0.068 M (B) 0.16 M (C) 6.4 M (D) 0.011 M

18. A calorimeter contains 123 g of water at 27.0°C. A block of metal with a mass of 28 g is heated to 95.8°C and then placed in the water in the calorimeter. After sufficient time, the temperature of the water is measured and found to be 28.8°C. Calculate the heat capacity per gram of metal. Assume no heat is lost to the calorimeter or the surroundings. (A) 2.0 J/g°C (B) 0.12 J/g°C (C) 6.8×102 J/g°C (D) 0.49 J/g°C

19. 75.0 mL of a pure liquid at 245 K is mixed with 100.0 mL of the same pure liquid at 365. K. What is the final temperature of the mixture? (A) 295 K (B) 305 K (C) 314 K (D) 325 K

20. For which process is ΔS negative? (A) evaporation of 1 mol of CCl4(l) (B) mixing 5 mL of ethanol with 25 mL of water (C) compressing 1 mol of Ne at constant temperature from 1.5 atm to 0.5 atm (D) raising the temperature of 100 g of Cu from 275 K to 295 K

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