Pre AP Chemistry Unit 12 HW Packet Name ______
WKS 12.1 – Introduction to Solutions (2 pages)
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. A homogeneous mixture that contains particles in a dispersed phase that do not settle out is a(n) ______.
8. Liquid solutes and solvents that are not soluble in each other are ______.
9. A(n) ______is a solution whose solute and solvent are both solid metals.
10. Dissolving is considered a ______change.
11. Ionic compounds will only dissolve in ______solvents.
12. The letter _____ is used to indicate the number of particles formed when a substance dissolves.
13. ______acids and bases completely dissociate in a water solution.
14. ______is the process of a compound splitting into ions when dissolved.
15. ______are substances that, when dissolved, conduct electricity.
16. Explain the meaning of the phrase “like dissolves like” in terms of polar and nonpolar substances.
17. Compare the properties of solutions, suspensions, and colloids.
18. Ethanol (CH3CH2OH) dissolves in water, but carbon tetrachloride does not. What can you conclude about ethanol and carbon tetrachloride?
19. Classify each of the following substances as a pure substance, heterogeneous mixture, or homogeneous mixture(solution):
Pre AP Chemistry Unit 12 HW Packet Name ______
a. Salad dressing
b. Chicken noodle soup
c. Milk
d. Sodium chloride
e. Sodium chloride dissolved in water
f. Air
g. Water
h. Chocolate chip cookie dough
i. Carbon
j. Gasoline (a mix of hydrocarbons)
Pre-AP Chemistry Unit 12 HW Packet Name ______
WKS 12.1 – Introduction to Solutions (continued)
Circle the best choice for each of the following multiple choice questions AND write a statement justifying and/or explaining your choice.
20. 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:
21. 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:
22. 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:
23. 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:
24. 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:
Answer the following questions.
25. Define unsaturated.
26. Define saturated.
27. Define supersaturated.
28. What are some ways to increase solubility amount of a solid?
29. What are some ways to increase solubility amount of a gas?
30. What are some ways to increase the rate of dissolution for a solid?
31. 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?
WKS 12.2 – Solubility of Covalents & Ionics (2 pages)
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 / Name / Structure(Lewis Dot) / Molecule polar or nonpolar? / Soluble in water or in oil?
1. CH4
2. CO2
3. C2H6
4. N2
5. H2O
6. HI
7. PH3
8. NBr3
WKS 12.2 – Solubility of Covalents & Ionics (continued)
For the following ionic compounds, give the name of the compound, and determine the state – (s) or (aq) – that it would have in a water solution.
Formula / Name / State / Formula / Name / StateCuCl2 / AgBr
Na3N / AlPO4
Mg(OH)2 / Na2CO3
SnCl4 / ZnSO3
Ca(C2H3O2)2 / Fe(NO3)2
BaSO4 / MgSO4
Fe2O3 / Ba(CN)2
NH4OH / FeI2
KClO4 / KBr
For the following ionic compounds, find the formula of the compound, and determine the state – (s) or (aq) – that it would have in a water solution.
Name / Formula / State / Name / Formula / StateCopper (II) chloride / Silver oxide
Barium phosphate / Zinc nitrate
Lithium sulfite / Sodium perchlorate
Lead (II) bromate / Cesium sulfide
Calcium chlorate / Iron (II) chlorate
Magnesium bromide / Potassium sulfate
Strontium hydroxide / Sodium iodate
Ammonium chloride / Aluminum cyanide
Potassium permanganate / Calcium carbonate
WKS 12.3 – Dissociation of Substances (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 / i1. Ba(OH)2
2. CaBr2
3. HNO3
4. CO2
5. BaI2
6. AgCl
7. H2SO4
8. NBr3
9. CCl4
10. KOH
11. NH4NO3
12. Al2(SO4)3
13. Na3PO4
14. HBr
15. HClO4
16. AgI
17. Cu2SO3
18. HF
19. ZnCO3
20. Br2
21. Li2CO3
WKS 12.4 – Electrolyte or Not??? (1 page)
Fill out the chart for each of the following substances.
Formula? / Ionic, Acid/Base, or Covalent? / Soluble in Water? / Electrolyte? / If electrolyte… strong or weak?Sodium chloride
Acetic acid
Strontium hydroxide
Hydrofluoric acid
Ammonium sulfate
Perchloric acid
Carbon dioxide
Aluminum sulfate
Silver bromide
Calcium nitrate
Sodium hydroxide
Hydrochloric acid
Lead (II) iodide
Butane
Magnesium chlorate
Sodium perchlorate
Ammonium iodide
Potassium hydroxide
Cesium nitrate
Aluminum sulfate
Bromine gas
WKS 12.5 – Solubility Curves (2 pages)
If a calculation is needed, show your work to earn credit!
1. What relationship exists between solubility and temperature for the ionic substances shown?
2. What relationship exists between solubility and temperature for the only gas, SO2, on the graph?
3. 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
4. How many grams of sodium nitrate will dissolve in 100. grams of water at 22.0°C?
5. 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?
6. How many grams of sodium nitrate will dissolve in 300. grams of water at 63.0°C? (≈384 g)
7. How many grams of ammonium chloride will dissolve in 1000. grams of water at 50.0°C? (≈500 g)
8. 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)
WKS 12.5 – Solubility Curves (continued)
9. 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)
10. 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)
11. 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)
12. 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)
13. 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)
14. 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)
WKS 12.6 – Molarity & Molality (1 page)
YOU MUST SHOW WORK TO EARN CREDIT FOR THE PROBLEMS!
1. 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)
2. What mass of zinc nitrate is needed to prepare 675 mL of 0.0012 M zinc nitrate aqueous solution? (0.15 g)
3. 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)
4. 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.
5. How many grams of water must be added to 455.0 grams of potassium sulfate in order to make a 1.500 m solution? (1743 g)
6. If 300. grams of magnesium acetate are added to 5000. grams of water, what is the molality of the solution? (0.423 m)
7. How many grams of lithium nitrate should be added to 800. grams of water in order to make a 2.00 m solution of lithium nitrate? (110. g)
8. Describe exactly how you would prepare a 2.50 m solution of potassium nitrate beginning with 1000 grams of water and potassium nitrate crystals.
WKS 12.7 – Dilution and Solution Stoichiometry (1 page)
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?
6. If I combined 15.0 grams of calcium hydroxide with 75.0 mL of 0.500 M HCl, how many grams of calcium chloride would be formed?
7. If 10.0 mL HNO3 completely neutralizes 25.0 mL of 0.351 M KOH, calculate the molarity of HNO3.
8. If 25.00 mL HCl acid with a concentration of 0.1234 M is neutralized by 23.45 mL of NaOH, what is the concentration of the base?
WKS 12.8 – Colligative Property Calculations (1 page)
YOU MUST SHOW WORK TO EARN CREDIT FOR THE PROBLEMS! You will need to use the Freezing & Boiling Point Constants reference chart in your notes to solve these problems.
1. What is the freezing point and boiling point of a solution where 67.3 grams of sodium chloride was dissolved in 755 grams of acetic acid? (BP = 127.3°C, FP = 4.7°C)
2. What is the freezing point and boiling point of a solution where 14.0 grams of glucose (C6H12O6) was dissolved in 250 grams of phenol? (BP = 182.9°C, FP = 40.7°C)
3. What is the molar mass of a substance which is known to ionize into 2 particles if 6.70 grams of it dissolved in 983 grams of water, and lowered the freezing point to -0.430°C? (59 g/mole)
4. What is the molecular mass of a non-ionizing (non-electrolyte) solute if 42.6 grams of it dissolved in 189 grams of water raises the boiling point of the solution to 100.68°C? (170. g/mole)
5. How many grams of potassium nitrate must be added to 500. grams of acetic acid in order to make a solution whose freezing point is 15.0°C? (10.4 g)
6. How many grams of aluminum sulfate must be added to 350. grams of water in order to make a solution whose boiling point is 101.8°C? (84.2 g)
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