1. According to Bronsted-Lowry theory, water
(a) can act as an acid by accepting protons
(b) can be neither an acid nor a base
(c) acts as a base when it accepts a proton
(d) can accept but not donate protons
2. How many moles is 0.224 L of hydrogen gas at STP?
(a) 0.01 mol
(b) 0.02 mol
(c) 1 mol
(d) 0.2 mol
3. What volume of hydrogen peroxide is present in 1.20 L of a 35%(v/v) hydrogen peroxide solution
(a) 340 mL
(b) 29 mL
(c) 420 mL
(d) 36.2 mL
4. Which of the following changes would cause a decrease in the pressure of a gaseous system?
(a) The container is made larger
(b) Additional amounts of the same gas are added to the container
(c) The temperature is increased
(d) A different gas is added to the container
5. A gas mixture contains oxygen, helium and nitrogen. The total pressure is 500 mm Hg. If the partial pressures of O2 and He are 180 mm Hg and 280 mm Hg, respectively, what is the partial pressure of nitrogen?
(a) 100 mm Hg
(b) 20 mm Hg
(c) 30 mm Hg
(d) 40 mm Hg
6. A solution that contains 0.90 g NaCl in 100mL of solution is called physiologic saline because it is isotonic with red blood cells. What is the molarity of this solution?
7. At 25oC, your car has a tire pressure of 1.90 atm. After a ride on a hot day, the tires heat up to 80oC. What is the new tire pressure, assuming that the tire volume does not change?
(a) 2.3 atm
(b) 1.6 atm
(c) 6.1 atm
(d) 0.59 atm
8. What is the pH of a solution if [H+] = 4 x 10-10 M
9. How would an increase in the attractive forces between particles in a liquid affect the vapor pressure of the liquid?
(a) it would cause an increase
(b) it would cause a decrease
(c) there would be no change
(d) it is impossible to predict
10. Water is a liquid at room temperature because of
(a) its relatively high molar mass
(b) intermolecular polar bonds
(c) strong dispersion forces
(d) hydrogen bonds
11. What is the [OH-] in a solution with a pH of 2.1?
(a) 1.3 x 10-2M
(b) 2.1 x 10-12 M
(c) 1.3 x 10-12 M
(d) 2.1 x 10-2 M
12. When water molecules solvate a cation in aqueous solution:
(a) the oxygen end of the water molecule faces the cation
(b) the water molecules are randomly oriented about the cation
(c) ionic bonds form between the water molecules and the cation
(d) the vapor pressure increases
13. When comparing a salt water solution to pure water, the salt water solution has the
(a) lower freezing point
(b) higher boiling point
(c) higher vapor pressure
(d) all of these
14. If the hydrogen ion concentration of a solution increases by a factor of 10, the hydroxide ion concentration
(a) must increase by a factor of 10
(b) remains the same
(c) must decrease by a factor of 10
(d) must decrease by a factor of 100
15. You have a stock solution of 0.400M sodium hydroxide. How many milliliters of this solution must you dilute to make a total of 250mL of 0.0200M sodium hydroxide?
(a) 8.0 mL
(b) 12.5 mL
(c) 31.3 mL
(d) 100 mL
16. In an acidic aqueous solution:
(a) [H+] is less than [OH-]
(b) [H+] is less than 1 x 10-14 mol / L
(c) [H+] is greater than 1 x10-7 mol / L
(d) [OH-] is greater than 1 x 10-7 mol / L
17. A 50.0 mL sample of a sodium hydroxide solution was required to neutralize 18.0 mL of 0.20N hydrochloric acid. What is the concentration of the base?
18. Sulfur dioxide and oxygen combine to form sulfur trioxide.
2SO2(g) + O2(g) -->2SO3(g)
How many liters of oxygen at STP are required to produce 8.96 L SO3?
(a) 4.48 L
(b) 8.96 L
(c) 8.00 L
(d) 2.24 L
19. One mole of carbon dioxide gas at STP and one mole of chlorine gas at STP
(a) each occupy the same volume
(b) each contain the same number of gas molecules
(c) each have particles with the same average kinetic energy
(d) all of these
20. What would happen to the volume of a gas if its pressure doubled and its absolute temperature doubled?
(a) the volume would increase by a factor of four
(b) the volume would remain constant
(c) the volume would double
(d) the volume would decrease by a factor of four
21. The condensation of steam to water is
(a) also called sublimation
(b) an exothermic process
(c) an endothermic process
(d) both (a) and (c) are correct
22. As the pressure of a gas above a liquid increase, the solubility of the gas:
(b) varies, depending on the gas
(c) remains the same
23. Consider the H2CO3/NaHCO3 buffer. Show by means of equations how the pH of a solution can be kept almost constant when small amounts of acid or base are added.