Pre AP Chemistry Unit 12 HW Packet
KODER
Name ______________________________________
WKS 12.1 – Properties of Liquids & Vaporization (2 pages)
1. In your own words, define the following terms.
a. Cohesion:
b. Surface Tension:
c. Adhesion:
d. Capillary action:
2. Answer the following questions with either gas , liquid, or both.
a. Which is affected greatly by changes in pressure?
b. Which will not fill the entire volume of the container?
c. Which cannot have its molecules compressed together?
d. Which is considered to be “fluid”?
e. Which has large spaces between its molecules?
f.
Which is the end result of condensation?
g. Which is the end result of vaporization?
h. Which will take on the shape of the container it is in?
i.
Which has the fastest motion of its molecules?
j.
Which feels some imtermolecular forces?
k. Which has a higher density?
3. For WATER,
a. …which state of matter is the most dense?
b. …is this unexpected? Why?
c. What is at least one biological benefit of this characteristic?
4. What concept is the image to the right trying to illustrate? Give a brief
definition/explanation of the concept.
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Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.1 – Properties of Liquids & Vaporization (Continued)
5. Badwater Basin, located in Death Valley, California, is the point of the lowest elevation in North America at
282 feet (86 m) below sea level. If you tried to boil water in Badwater Basin, would you have to use more or
less heat than at sea level? Explain.
6. In your notes, it was stated that as temperature increases, the vapor pressure of a liquid will increase. Propose
a reason for this observation.
7. At a given temperature, would you expect a substance with a high vapor pressure to have a higher or a lower
boiling point temperature, in comparison to a substance with a low vapor pressure? Explain.
8. Liquid bromine (Br2) has a much lower boiling point than that of water (H2O). Propose a reason for this
observation.
9. Based on the previous question, would you expect liquid bromine or water to be considered more volatile?
Explain.
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Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.2 – Introduction to Solutions (2 Pages)
Fill in the blanks on the following table showing the classification of matter.
Fill in the following blanks to complete the statements.
1. A homogeneous mixture is also called a _____________________________.
2. The substance dissolved in a homogeneous mixture is the ___________________________.
3. A mixture that can be identified because it scatters light is a _______________________ mixture.
4. To conduct electricity, a solution must contain ___________________________.
5. Polar solvents will dissolve __________________ solutes.
6. Because water will dissolve most solutes, it is known as the ________________________________.
7. Liquid solutes and solvents that are not soluble in each other are _______________________.
8. A(n) ___________________ is a solution whose solute and solvent are both solid metals.
9. Dissolving is considered a __________________________ change.
10. Ionic compounds will only dissolve in _____________________ solvents.
11. The letter _____ is used to indicate the number of particles formed when a substance dissolves.
12. _________________ acids and bases completely dissociate in a water solution.
13. ___________________________ is the process of a compound splitting into ions when dissolved.
14. ___________________________ are substances that, when dissolved, conduct electricity.
Page 3 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.2 – Introduction to Solutions (Continued)
15. Explain the meaning of the phrase “like dissolves like” in terms of polar and nonpolar substances.
16. Compare the properties of solutions, suspensions, and colloids.
17. Ethanol (CH3CH2OH) dissolves in water, but carbon tetrachloride does not. What can you conclude about
ethanol and carbon tetrachloride?
18. Classify each of the following substances as a pure substance, heterogeneous mixture, or homogeneous
mixture(solution):
a. Salad dressing
f.
Air
b. Chicken noodle soup
g. Water
c. Milk
h. Chocolate chip cookie dough
d. Sodium chloride
i.
Carbon
e. Sodium chloride dissolved in water
j.
Gasoline (a mix of hydrocarbons)
Circle the best choice for each of the following multiple choice questions AND write a justification statement.
19. Substances whose water solutions conduct electric current:
a. are nonpolar
c. do not dissolve in water
b. ionize in water
d. decompose in water
Justification:
20. Which of the following does NOT increase the rate at which a solid dissolves in water?
a. raising the temperature
c. using large pieces of the solid
b. stirring
d. crushing the solid
Justification:
21. Raising the temperature of a solvent causes solute-solvent collisions to become:
a. less frequent and more energetic
c. less frequent and less energetic
b. more frequent and more energetic d. more frequent and less energetic
Justification:
22. Solubility of a solute depends on:
a. the nature of the solute and the temperature
b. the nature of the solute only
c. the temperature only
d. neither the nature of the solute nor the temperature
Justification:
23. A solution that contains a high concentration of solute but than can hold even more solute is:
a. unsaturated and dilute
c. unsaturated and concentrated
b. saturated and dilute
d. saturated and concentrated
Justification:
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Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.3 – Solubility (1 Page)
Name the following covalent (molecular) compounds, draw the structure, tell if the molecule is polar or non-polar, and state if
it will be soluble in water or oil.
Formula
Structure
(Lewis Dot)
Name
Molecule polar or
nonpolar?
Soluble in water
or in oil?
1. CH4
2. CO2
3. C2H6
4. NBr3
For the following ionic compounds, give the name or formula of the compound, and determine the state – (s) or (aq) – that it
would have in a water solution.
Formula
Name
State
Formula
CuCl2
AgBr
Na3N
AlPO4
Mg(OH)2
(NH4)2CO3
SnCl4
ZnSO3
Ca(C2H3O2)2
Fe(NO3)2
Name
Formula
State
Name
Copper (II) Chloride
Zinc Nitrate
Barium Phosphate
Strontium Hydroxide
Calcium Carbonate
Lead (II) Chloride
Aluminum cyanide
Lithium Chromate
Magnesium Bromate
Potassium Sulfide
Name
State
Formula
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State
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.4 – Dissociation and Electrolytes (1 page)
First: Determine whether the following ionics, covalents, or acids are soluble in water.
Second: Write equations for the dissociation of the following only if they are soluble.
Third: Determine the “i” if they are soluble.
Ionic,
Covalent, or
Acid?
Soluble in
water?
Dissociation Equation
i
1. Ba(OH)2
2. CaBr2
3. HNO3
4. CO2
5. BaI2
6. AgCl
7. H2SO3
8. NBr3
9. CCl4
10. KOH
Fill out the chart for each of the following substances to determine if it would form an electrolyte solution in water.
Formula?
Ionic, Acid/Base,
or Covalent?
Soluble in
Water?
Electrolyte?
If electrolyte…
strong or weak?
Acetic acid
Strontium hydroxide
Hydrofluoric acid
Ammonium sulfate
Perchloric acid
Carbon dioxide
Aluminum sulfate
Silver bromide
Calcium nitrate
Sodium hydroxide
Butane
Page 6 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.5 – Solubility & Dissolution (1 page)
Answer the following questions.
1. How does one form a supersaturated solution?
2. When a tiny crystal of solute was dropped into a solution containing the same solute, the tiny crystal completely
dissolved, and disappeared into the solution. How would you classify the saturation level of the initial solution?
3. When a tiny crystal of solute was dropped into a solution containing the same solute, the crystal appeared to grow
rapidly, and other crystals began to precipitate out of the solution. How would you classify the saturation level of the
initial solution?
4. What are some ways to increase solubility amount of a solid?
5. What are some ways to increase solubility amount of a gas?
6. What are some ways to increase the rate of dissolution for a solid?
7. Carbonated drinks are made by bubbling carbon dioxide through a colored sugary solution. Do you think Dr. Peppers
are more likely bottled at 10°C or at 50°C? Why?
8. What relationship exists between solubility and
temperature for the ionic substances shown?
9. What relationship exists between solubility and
temperature for the only gas, SO2, on the graph?
10. Are the following solutions saturated, unsaturated, or
supersaturated?
a. 20. grams of NH3 completely dissolved in 100.
grams of water at 80.°C
b. 80. grams of KNO3 completely dissolved in 100.
grams of water at 55°C
c. 110. grams of NaNO3 completely dissolved in 100.
grams of water at 45°C
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Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.6 – Solubility Curves and Molarity (2 pages)
If a calculation is needed, you must show your work to
earn credit!
1. How many grams of sodium nitrate will dissolve in
100. grams of water at 22.0°C?
2. Ninety grams of sodium nitrate is added to 100. grams
of water at 0.00°C. With constant stirring, to what
temperature must the solution be raised to produce a
saturated solution with no solid sodium nitrate
remaining?
3. How many grams of sodium nitrate will dissolve in
300. grams of water at 63.0°C? (≈384 g)
4. How many grams of ammonium chloride will dissolve
in 1000. grams of water at 50.0°C? (≈500 g)
5. 60.0 grams of potassium chlorate are added to 300.
grams of water at 10.0°C. To what temperature must
the solution be raised to produce a saturated solution
with no potassium chlorate solid remaining? (≈50°C)
6.
175 grams of ammonia are dissolved in 250. grams of water at 20.0°C. If the solution is heated to 80.0°C, how many
grams of ammonia will have bubbled out of solution? (≈143 g)
7. A saturated solution of potassium chlorate was made with 300. grams of water at 40.0°C. How much potassium
chlorate could be recovered by evaporating the solution to dryness? (≈48 g)
8. 500. grams of water are used to make a saturated solution of potassium chlorate at 10.0°C. How many MORE grams
of potassium chlorate could be dissolved if the temperature were raised to 100°C? (≈265 g more)
Page 8 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.6 – Solubility Curves and Molarity (Continued)
If a calculation is needed, you must show your work to earn credit! Use the solubility chart on the previous page.
9. A saturated solution of potassium nitrate in 200. grams of water at 50.°C is cooled to 20.°C. How much potassium
nitrate will precipitate out of solution? (≈94 g)
10. A saturated solution of ammonium chloride dissolved in 447 grams of water is cooled from 90°C to 30°C. How many
grams of ammonium chloride will be precipitated out of solution? (≈130 g)
11. 450 grams of sodium nitrate are added to 300 grams of water at 25°C. To what temperature Celsius must the
temperature be raised in order for all of the solute to dissolve? (≈85°C)
You must show your work to earn credit on the following Molarity problems.
12. What is the molarity of a solution in which 10.8 grams of calcium chloride is dissolved in enough water to make 125
mL of solution? (0.778 M)
13. What mass of zinc nitrate is needed to prepare 675 mL of 0.0012 M zinc nitrate aqueous solution? (0.15 g)
14. If 120. grams of copper (II) sulfate pentahydrate are added to enough water to make a solution whose molarity is 1.50
M, how many milliliters of solution do you have? (321 mL)
15. Describe exactly how you would go about preparing 1000 mL (1 liter) of a 0.33 M potassium hydroxide solution
beginning with solid KOH crystals.
Page 9 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.7 – Dilution and Solution Stoichiometry (2 pages)
YOU MUST SHOW WORK TO EARN CREDIT FOR THE PROBLEMS!
1. If 30.0 mL of 12.0 M hydrochloric acid solution is diluted to a volume of 500 mL, what is the molarity of the
dilute acid? (0.72 M)
2. Jack pours 130 mL of water into a beaker already containing 200.0 mL of 6.0 M copper (II) sulfate solution. What
is the molarity of the copper (II) sulfate solution now that it’s been diluted? (3.64 M)
3. If 250 mL of sulfuric acid at 18.0 M is diluted to a volume of 1000 mL, what is the molarity of the diluted acid
solution? (4.50 M)
4. If, when water is added to 27.5 mL of 16.0 M nitric acid stock solution, the new molarity was found to be 1.34 M,
how many mL of water were added to the original solution? (301 mL)
5. How many liters of 0.100 M HCl would be required to react completely with 5.00 grams of calcium hydroxide?
(1.35 L)
6. 40. mL of 0.85 M solution of barium bromide is reacted with excess cesium phosphite solution in a double
replacement reaction. How many grams of barium phosphite precipitate will be produced from the double
replacement reaction? (6.5 g)
2 Cs3PO3 + 3 BaBr2  6 CsBr
+ Ba3(PO3)2
Page 10 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.7 – Dilution and Solution Stoichiometry (Continued)
7. What mass of solid aluminum hydroxide is produced when 50.0 mL of 0.200 M aluminum nitrate solution is
added to 200. mL of 0.100 M potassium hydroxide solution? (NOTE: they give you amounts of TWO reactants…
this is a limiting reactant problem!)
(0.520 g)
8. If I combined 15.0 grams of Calcium Hydroxide with 75.0 mL of 0.500 M Sulfuric Acid, how many moles of
water would be formed? (0.0750 mol)
9. If 10.0 mL of Nitric Acid completely neutralizes 25.0 mL of 0.351 M of Strontium Hydroxide solution, calculate
the molarity of the acid. (1.76 M)
10. If 25.00 mL Hydrochloric Acid with a concentration of 0.124 M is neutralized by 23.5 mL of Potassium
Hydroxide solution, what is the concentration of the base? (0.134 M)
Page 11 of 12
Pre AP Chemistry Unit 12 HW Packet
Name ______________________________________
WKS 12.8 – A Little Bit of Everything… (1 Page)
Circle the best choice for each of the following multiple choice questions AND write a justification statement.
1. Which of the following solutions is the most dilute?
a. 100 mL of a 5.2 M solution of NaCl (aq)
b. 200 mL of a 4.8 M solution of NaCl (aq)
c. 150 mL of a 3.5 M solution of NaCl (aq)
d. 125 mL of a 2.3 M solution of NaCl (aq)
Justification:
2. Which of the following solutes would create the most change in the boling point and freezing point of a solvent?
a. CaCO3
c. NaBr
b. C6H12O6
d. CaCl2
Justification:
3. When NaCl is added to water, what is the effect on the boiling point?
a. The boiling point rises to above 100˚C.
c. The boiling point rises above 0˚C.
b. The boiling point falls below 100˚C.
d. The boiling point falls below 0˚C.
Justificaiton:
4. Which two factors must be considered when predicting whether two substances will dissolve in each other?
a. Number of bonds and size of molecules
c. Type of bonds and molecular polarity
b. Type of bonds and size of molecules
d. Number of bonds and molecular polarity
Justification:
5. Ammonia (NH3) and water have similar structures, but the forces between the molecules of ammonia are weaker.
How would the properties of ammonia differ from those of water?
a. Ammonia would have a greater molar mass.
c. Ammonia would have a higher surface tension.
b. Ammonia would be more cohesive.
d. Ammonia would have a lower boiling point.
Justification:
6. A student is asked to determine whether a given solution is unsaturated, saturated, or supersaturated. The student
drops a tiny crystal of the solute into the solution and observes carefully for any change in the size of the crystal.
Which of the following statements is true?
a. No observable change means the solution is supersaturated.
b. A decrease in crystal size means the solution is unsaturated.
c. A decrease in crystal size means the solution is saturated.
d. An increase in crystal size means the solution is unsaturated.
Justification:
7. An excess amount of aluminum reacts with concentrated sodium hydroxide to make a complex ion as shown
below. How many mL of a 0.250 M solution of sodium hydroxide would be required to form 230.0 mL of
hydrogen gas at 289˚C and 116 kPa? (15.2 mL)
6 H2O (l) + 2 Al (s) + 2 NaOH (aq)  2 Al(OH)4–1 (aq) + 3 H2 (g) + 2 Na+1 (aq)
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