NAME __________________________________________
PERIOD ____________
DATE _________________________________
CHAPTERS 14-15 TEST REVIEW
Show your work as well as units. Remember that you can use one 3x5 card (front and back) on the
test as notes. The only thing I will give you will be a Periodic Table.
Questions #1-10 are True or False. Write True or False on the blank next to each question.
1.
2.
3.
4.
5.
6.
7.
8.
9.
_____ Colloids undergo the Tyndall effect.
_____ 3 ions are formed from Fe3(PO4)2.
_____ A solution is another name for a heterogeneous mixture.
_____ Glucose is considered an electrolyte.
_____ The units for molarity are mol/L.
_____ Nonvolatile solutes depress the freezing point and elevate the boiling point.
_____ Electrolytes have a greater effect on freezing point depression than nonelectrolytes.
_____ 1 J equals 0.2390 cal
_____ Small values for specific heat mean that it takes a lot of heat and energy to raise the
temperature of the substance.
10. _____ When a chemical reaction or physical process loses energy it is considered an exothermic
process.
The following questions are multiple choice. Write A, B, C, or D on the blank next to each question.
11. _____ The freezing point of an aqueous solution that contains sucrose is -8.0°C. What is the
molality of the solution?
a. 4.3 m
c. 14.8 m
b. 4.5 m
d. 1.86 m
12. _____ Two liquids that can be mixed together but separate shortly after are:
a. Insoluble
c. Soluble
b. Miscible
d. Immiscible
13. _____ What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?
a. 0.0132 M
c. 0.0253 M
b. 1.363 M
d. 0.459 M
14. _____ What is the boiling point elevation of a solution made from 10.0 g of a nonelectrolyte
solute and 300.0 g of water? The molar mass of the solute is 50.0 g/mol.
a. 0.01°C
c. 0.34°C
b. 0.2°C
d. 0.32°C
15. _____ What is the molality of a solution that contain 31.0 g HCl in 5000.0 g water?
a. 15.5 m
c. 0.425 m
b. 0.062 m
d. 0.170 m
16. _____ Which of the following in an electrolyte?
a. CCl4
c. NH4OH
b. None of these
d. CH4
17. _____ Which of the following will dissolve most slowly?
a. Small salt crystals in unstirred
c. Large salt crystals in stirred
water
water
b. Small salt crystals in stirred
d. Large salt crystals in unstirred
water
water
18. _____ What is the approximate freezing point depression of a 0.010 m aqueous solution of
MgCl2?
a. 0.019°C
c. 0.037°C
b. 0.074°C
d. 0.056°C
19. _____ The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water.
How much NaCl is in the solution?
a. 89.3 g
c. 2.00 g
b. 117 g
d. 224 g
20. _____ What is the approximate freezing point depression of a 0.050 m aqueous solution of
Fe2(SO4)3?
a. 0.47°C
c. 0.11°C
b. 0.39°C
d. 0.22°C
21. _____ “Like dissolves like” is a very general rule used for predicting whether:
a. A reaction will reach equilibrium
b. One substance will form a solution with another
c. One substance will react with another
d. A mixture will contain two or three phases
22. _____ A solute crystal is dropped into a solution containing dissolved solute. It falls to the
bottom of the beaker and does not dissolve after vigorous stirring. What does this indicate
about the solution?
a. It is not at equilibrium
c. It is probably supersaturated
b. It is probably saturated
d. It is probably unsaturated
23. _____ Compared with a 0.01 m sugar solution, a 0.01 m MgCl2 solution has:
a. About four times the freezing point depression
b. The same freezing point depression
c. About three times the freezing point depression
d. About twice the freezing point depression
24. _____ Which of the following is NOT a factor that will increase solvation?
a. Agitation
b. Increasing the surface area of the solute
c. Increasing the temperature of the solvent
d. Decreasing the pressure
25. _____ Which of the following do we do to create a supersaturated solution?
a. Heat the solution and then slowly cool it
b. Only stir it
c. Mix in more solute
d. Wait, the supersaturated solution will create itself over time.
26. _____ Which of the following will increase the solubility of a gas?
a. Increase the temperature
c. Increase the pressure
b. Increase the volume
d. Decrease the pressure
27. _____ Which of the following words best describes the ability to do work?
a. Energy
c. Movement
b. Heat
d. Light
28. _____ Which of the following states that in any chemical reaction or physical process, energy
can be converted from one form to another, but it is neither created nor destroyed?
a. 2nd Law of Thermodynamics
c. Hess’s Law
b. Law of Conservation of Energy
d. Law of Conservation of Mass
29. _____ You are preforming a thermochemical experiment. Which part of the experiment are you
actually studying?
a. Universe
c. Surroundings
b. System
d. Lab
30. _____ Which of the following best describes the energy change in the formation of a product at
1 atm and 25°C?
a. ΔH°f
c. ΔH°comb
b. ΔHf
d. ΔHcomb
The following questions are short answer. Answer each question as completely as possible. Don’t
forget units!
31. A solution contains 85.0 g of NaNO3, and has a volume of 750 mL. What is the molarity of the
solution?
32. What is the molality of a solution formed by mixing 35 g of potassium hydroxide in 750 g of
water?
33. What volume, in milliliters, of a 2.00 M calcium chloride stock solution would you use to make
0.50 L of a 0.300 M of calcium chloride solution?
34. What is the new boiling point of a solution containing 17.1 g of sucrose in 100.0 g of water? The
molar mass of sucrose is 342 g/mol.
35. How much calcium hydroxide (Ca(OH)2), in grams, is needed to produce 1.5 L of a 0.25 M
solution?
36. Sodium chloride (NaCl) is often used to prevent icy roads and to freeze ice cream. What are the
boiling and freezing points of a 0.029m aqueous solution of NaCl?
37. A 155 g sample of an unknown substance was heated from 25.0°C to 40.0°C. In the process, the
substance absorbed 5696 J of energy. What is the specific heat of the substance?
38. A 4.50 g nugget of pure gold absorbed 276 J of heat. The initial temperature was 25.0°C. What
was the final temperature? The specific heat of gold is 0.129 J/g°C.
39. Stoichiometry Review. The decomposition of solid ammonium nitrate produces dinitrogen
monoxide gas and water vapor. If 25.0 g of solid ammonium nitrate decomposes, how many
grams of water vapor is produced?
40. Naming Review. Complete the following table.
Compound Name
Compound Formula
P 5S 8
HNO2
Trinitrogen monosulfide
Sodium phosphate
Iron (III) sulfate
Is it an acid, ionic, or molecular?