1. Which of the following compounds is a strong electrolyte?

a.   H₂O

b.   CH₃OH

c.   CH₃CH₂OH

d.   NaF

2. Which of the following compounds is a weak electrolyte?

a.   HNO₃

b.   NaNO₃

c.   HNO₂

d.   NaNO₂

3. Based on the solubility rules, which one of the following compounds should be insoluble in water?

a.   NaCl

b.   MgBr₂

c.   FeCl₂

d.   AgBr

4. Based on the solubility rules, which one of the following compounds should be insoluble in water?

a.   CaCO₃

b.   (NH₄)₂CO₃

c.   Na₂CO₃

d.   K₂CO₃

5. Based on the solubility rules, which of the following will occur when a solution containing about 0.1g of Pb(NO₃)₂(aq) is mixed with a solution containing 0.1g of KI(aq) /100 mL?

a.   KNO₃ will precipitate; Pb²⁺ and I^- are spectator ions.

b.   No precipitate will form.

c.   Pb(NO₃)₂ will precipitate; K⁺ and I^- are spectator ions.

d.   PbI₂ will precipitate; K⁺ and NO₃^- are spectator ions.

6. Which of the following is the correct net ionic equation for the reaction that occurs when solutions of Pb(NO₃)₂ and NH₄Cl are mixed?

a.   Pb(NO₃)₂(aq) + 2NH₄Cl(aq) ® NH₄NO₃(aq) + PbCl₂(s)

b.   Pb²⁺(aq) + 2Cl^-(aq) ® PbCl₂(s)

c.   Pb²⁺(aq) + 2NO₃^- (aq) + 2NH(aq) + 2Cl^-(aq) ® 2NH(aq) + 2NO₃^- (aq) + PbCl₂(s)

d.   NH₄⁺(aq)+ NO₃^- (aq) ® 2NH₄NO₃(s)

7. The common constituent in all acid solutions is:

a.   H₂.

b.   H⁺.

c.   OH^-.

d.   H₂SO₄.

8. Identify the major ions present in an aqueous LiOH solution.

a.   Li²⁺, O^- , H^-

b.   Li⁺, OH^-

c.   LiO^-, H⁺

d.   Li⁺, O^2-, H⁺

9. What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide?

a.   CaO

b.   CaCl₂

c.   CaH₂

d.   CaCl

10. The oxidation number of N in NaNO₃ is:

a.   +6.

b.   +5.

c.   +3.

d.   -3.

11. Select the compound in which sulfur has its highest possible oxidation number.

a.   H₂S

b.   SO₂

c.   SCl₂

d.   Na₂SO₄

12. In the following redox reaction, which element is oxidized and which is reduced?  4NH₃ + 3Ca(ClO)₂ ® 2N₂ + 6H₂O + 3CaCl₂

a.   H is oxidized and N is reduced.

b.   N is oxidized and Cl is reduced.

c.   N is oxidized and O is reduced.

d.   Cl is oxidized and O is reduced.

13. Identify the reducing agent in the following chemical reaction: Cd + NiO₂ + 2H₂O ® Cd(OH)₂ + Ni(OH)_2.

a.   Cd

b.   NiO₂

c.   H₂O

d.   Cd(OH)₂

14. What element is oxidized in the following chemical reaction?  NiO₂ + Cd + 2H₂O ® Ni(OH)₂ + Cd(OH)_2.

a.   Ni

b.   Cd

c.   O

d.   H

15. Which of the following represents a metal displacement reaction?

a.   2NaN₃(s) ® 2Na(s) + 3N₂(g)

b.   Fe₂O₃(s) + 2Al(s) ® 2Fe(s) + Al₂O₃(s)

c.   3NO₂(g) + H₂O(l) ® 2HNO₃(aq) + NO(g)

d.   2P(s) + 3Cl₂(g) ® 2PCl₃(g)

16. Which of the following represents an acid-base neutralization reaction?

a.   2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

b.   SO₂(g) + H₂O(l) ® H₂SO₃(g)

c.   LiOH(aq) + HNO₃(aq) ® LiNO₃(aq) + H₂O(l)

d.   2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

17. What mass of K₂CO₃ is needed to prepare 200 mL of a solution having a potassium ion concentration of 0.150 M?

a.   4.15g

b.   10.4g

c.   13.8g

d.   2.07g

18. A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250.00 mL.  What is the concentration of nitric acid in the final solution?

a.   1.27 M

b.   8.12 x 10^-3 M

c.   0.406 M

d.   3.25 x 10^-2 M

19. 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H₂SO₄ solution.  What is the concentration of the original sulfuric acid solution?

a.   0.0229 M

b.   0.218 M

c.   0.0523 M

d.   0.209 M

20. If 73.5 mL of 0.200 M KI(aq) was required to precipitate all of the lead (II) ion from an aqueous solution of lead (II) nitrate, how many moles of Pb²⁺ were originally in the solution?

a.   7.35 x 10^-3 moles of  Pb²⁺

b.   73.5 x 10^-3 moles of  Pb²⁺

c.   73.5 x 10^-2 moles of  Pb²⁺

d.   7.35 x 10^-2 moles of  Pb²⁺

21. The pressure of a gas sample was measured to be 654 mmHg.  What is the pressure in kPa? (1 atm = 1.01325 x 10⁵ Pa)

a.   87.2 kPa

b.   118 kPa

c.   6.63 x 10⁴ kPa

d.   8.72 x 10⁴ kPa

22. Which of these properties is/are characteristic(s) of gases?

a.   High compressibility

b.   Relatively large distances between molecules

c.   Formation of homogeneous mixtures regardless of the nature of gases

d.   All of the choices apply

23. A sample of a gas occupies 1.40 x 10³ mL at 25°C and 760 mmHg.  What volume will it occupy at the same temperature and 380 mmHg?

a.   2,800 mL

b.   2,100 mL

c.   1,400 mL

d.   1,050 mL

24. The gas pressure in an aerosol can is 1.8 atm at 25°C.  If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475°C?

a.   0.095 atm

b.   0.717 atm

c.   3.26 atm

d.   4.52 atm

25. The temperature of an ideal gas in a 5.00 L container originally at 1 atm pressure and 25°C is lowered to 220 K.  Calculate the new pressure of the gas.

a.   1.0 atm

b.   1.35 atm

c.   8.8 atm

d.   0.738 atm

26. At what temperature will a fixed mass of gas with a volume of 125 L at 15°C and 750 mmHg occupy a volume of 101 L at a pressure of 645 mm Hg?

a.   -73°C

b.   10.4°C

c.   2°C

d.   34°C

27. Calculate the number of moles of gas contained in a 10.0 L tank at 22°C and 105 atm.  (R = 0.08206 L×atm/K×mol)

a.   1.71 x 10^-3 mol

b.   0.0231 mol

c.   1.03 mol

d.   43.4 mol

28. Calculate the volume occupied by 35.2g of methane gas (CH₄) at 25°C and 1.0 atm.  (R = 0.08206 L×atm/K×mol)

a.   0.0186 L

b.   4.5 L

c.   11.2 L

d.   53.7 L

29. Calculate the density, in g/L, of CO₂ gas at 27°C and 0.50 atm pressure.

a.   0.89 g/L

b.   1.12 g/L

c.   9.93 g/L

d.   46.0 g/L

30. Determine the molar mass of chloroform gas if a sample weighing 0.389g is collected in a flask with a volume of 102 cm³ at 97°C.  The pressure of the chloroform is 728 mmHg.

a.   187 g/mol

b.   121 g/mol

c.   112 g/mol

d.   31.6 g/mol

31. A mixture of three gases has a total pressure of 1,380 mmHg at 298 K.  The mixture is analyzed and is found to contain 1.27 mol CO₂, 3.04 mol CO and 1.50 mol Ar.  What is the partial pressure of Ar?

a.   0.258 atm

b.   301 mmHg

c.   356 mmHg

d.   5,345 mmHg

32. What volume of CO₂ gas at 645 torr and 800 K could be produced by the reaction of 45g of CaCO₃ according to the equation?  CaCO₃(s) ? CaO(s) + CO₂(g)

a.   0.449 L

b.   22.4 L

c.   25.0 L

d.   34.8 L

33. Which statement is false?

a.   The average kinetic energies of molecules from samples of different "ideal" gases is the same at the same temperature.

b.   The molecules of an ideal gas are relatively far apart.

c.   All molecules of an ideal gas have the same kinetic energy at constant temperature.

d.   Molecules of a gas undergo many collisions with each other and the container walls.

34. Which of these gas molecules have the highest average kinetic energy at 25°C?

a.   H₂

b.   O₂

c.   N₂

d.   All the gases have the same average kinetic energy

35. Deviations from the ideal gas law are greater at:

a.   low temperatures and low pressures.

b.   low temperatures and high pressures.

c.   high temperatures and high pressures.

d.   high temperatures and low pressures.