Alícia Rosa
1. When solid CuCl2 and water are mixed a clear liquid results. What
is the CuCl2 called?
a. A precipitate
b. A solute
c. A solution
d. A solvent
2. In which of the following phases can a solution be made?
a. Solid and liquid phases only
b. Liquid and gas phases only
c. Gas and solid phases only
d. Solid, liquid and gas phases
3. Carbon tetrachloride, a liquid, settles to the bottom of a test tube
after being shaken with water. The 2 liquids are said to be
a. Miscible
b. Immiscible
c. Alloys
d. Soluble
4. Which of the following is not a solution?
a. C2H5OH(l)
b. Air
c. An alloy of copper, zinc and tin
d. Salt water
5. Which of the following sugar solutions is the most concentrated?
a. 2 g of sugar in 100 mL of water
b. 12 g of sugar in 30 mL of water
c. 15 g of sugar in 25 mL of water
d. 25 g of sugar in 60 mL of water
6. Solubility is
a. the amount of solvent that will dissolve a given amount of a solute
at any temperature
b. the amount of solute that will dissolve in a given amount of solvent
at any temperature
c. the process of dissolving a solute in a solvent
d. the amount of solute that will dissolve in a given amount of solvent
at a certain temperature
7. A solute that has been dissolved in a solvent
a. can be recovered by a process involving its physical properties
b. cannot be recovered by a process involving its physical properties
c. is chemically changed
d. can be recovered by a process involving its chemical properties
8. Solid potassium chloride is added to water until no more can be
dissolved at that temperature. Some solid remains at the bottom of
the beaker. How would you describe the solution?
a. It is a concentrated solution.
b. It is a saturated solution.
c. It is an unsaturated solution.
d. It is a heterogeneous solution.
9. Stirring a solute/solvent mixture
a. increases the solubility of the solute in the solvent
b. does not affect the rate of dissolution
c. makes the solute dissolve faster
d. increases the capacity of the solvent to dissolve the solute
10. If a solute dissolves in a solvent, what is likely to be true?
a. The solute-solute attractions are greater than the solvent-solvent
attractions.
b. The solute-solute attractions are less than the solvent-solvent
attractions.
c. The solute-solvent attraction is greater than the sum of the solutesolute and solvent-solvent attraction.
d. There is a strong attraction between solute and solvent molecules.
11. Water is an example of a molecule
a. with a permanent dipole
b. capable of hydrogen bonding to another water molecule
c. with a partial positive charge on its hydrogen atoms
d. All of the above are true.
12. Which combination of solid and liquid would likely form a
solution?
a. Ionic solid and non-polar liquid
c. Non-polar solid and polar liquid
b. Ionic solid and polar liquid
d. Polar solid and non-polar liquid
13. What happens when KBr (s) is dissolved in water?
a. Br– ions are attracted to the oxygen atoms of the water molecules.
b. Br– ions are repelled by the hydrogen atoms of the water
molecules.
c. K+ ions are attracted to the oxygen atoms of the water molecules.
d. K+ ions are repelled by the oxygen atoms of the water molecules.
14. What is the term for a substance that provides ions when
dissolved in water?
a. An electrolyte c. A non-electrolyte
b. A molecular solute
c. A non-electrolyte
d. A covalent compound
15. The ΔEN for the binary compound CuCl is 1.26. Which statement
is true about CuCl?
a. This ionic compound is probably soluble in water.
b. This ionic compound is probably not soluble in water.
c. This polar compound is probably soluble in water.
d. This polar compound is probably not soluble in water.
16. Increasing the temperature of the solvent
a. increases the solubility of solid, liquid and gaseous solutes
b. decreases the solubility of gaseous solute
c. increases the solubility of liquid solutes more than solid solutes
d. affects the solubility of solid solutes only
17. In which the following cases is pressure a factor in the solubility
of the solute in the solvent?
a. Sugar is dissolved in water.
b. Alcohol is dissolved in water.
c. Acetylene gas is mixed with oxygen in a blowtorch.
d. Carbon dioxide is dissolved in sparking wine.
18. Which of the following is not an acceptable way to express
concentration?
a. Mass of solute/volume of solution
b. Mass of solute/mass of solution
c. Mass of solute/100 g of water
d. Volume of solute/volume of solution
19. A student adds 6.00 g of a solid to 30.0 mL of water. What is the
concentration of this solution expressed as mass/mass percent?
(Assume that 1.00 mL of water has a mass of 1.00 g.)
a. 0.167%
b. 0.200%
c. 16.7%
d. 20.0%
22. What mass of solute is present in 250. mL of a 0.100 mol/L
solution of NaOH.
a. 0.625 g
b. 1.00 g
c. 6.25 g
d. 1000 g
23. A student dilutes 50.0 mL of a 0.10 mol/L solution of HCl to 0.010
mol/L by adding water. Which statement is true?
a. The volume of the solution remains the same.
b. The volume of the solvent remains the same.
c. The total amount of solute remains the same.
d. The total amount of solute decreases.
24. When preparing a dilute acid solution from a concentrated acid
solution,
a. adding the acid to the water aids the mixing process
b. adding the acid to the water prevents the splattering of hot acid
c. wear appropriate protective clothing and goggles and work in a
fume hood
d. all of the above are true
25. How would you prepare 500.0 mL of a 2.00 mol/L solution of HCl
from a solution of 12.0 mol/L?
a. To some water in a 500.0 mL volumetric flask, add 83.3 mL of
concentrated acid, then dilute to the mark.
b. To some water in a 500.0 mL volumetric flask, add 8.33 mL of
concentrated acid, then dilute to the mark.
c. To some water in a 500.0 mL volumetric flask, add 3.00 mL of
concentrated acid, then dilute to the mark.
d. Pour 83.3 mL of concentrated acid into a 500.0 mL volumetric
flask. Dilute with water to the mark.