Solutions
Name:
_______1. solution
a. capable of being dissolved
_______2. solute
b. solution with water as the solvent
_______3. solvent
c. substance that is dissolved in a solution
_______4. soluble
d. substance that dissolves in water to form a solution that conducts
an electric current
_______5. alloy
e. a solution containing two or more metals
_______6. aqueous solution
f. homogeneous mixture of two or more substances in a single
physical state
_______7. electrolyte
g. substance that does the dissolving in a solution
In the space provided, describe and give an example of each of the following types of solutions.
8. alloy
_______________________________________________________________________
9. liquid solution _____________________________________________________________________
10. gaseous solution ___________________________________________________________________
Answer each of the following questions in the space provided.
11. Describe the properties of a solution. ___________________________________________________
_________________________________________________________________________________
12. Explain how to distinguish between the solvent and the solute in a solution. ____________________
_________________________________________________________________________________
13. Why might a construction company build a high-rise building with steel alloy beams instead of pure
iron beams? _______________________________________________________________________
__________________________________________________________________________________
14. Water and ethanol are miscible in all proportions, whereas oil and water are immiscible. Explain this
statement. ________________________________________________________________________
_________________________________________________________________________________
15. Why is water called the universal solvent? ______________________________________________
_________________________________________________________________________________
16. How could you determine experimentally whether a given substance is an electrolyte?
_________________________________________________________________________________
17. Give two examples of solutions in nature and explain why each is important. ___________________
_________________________________________________________________________________
18.
Type of Solution
Gas in Gas
Gas in Liquid
Gas in Solid
Liquid in Gas
Liquid in Liquid
Liquid in Solid
Solid in Gas
Solid in Liquid
Solid in Solid
Specific Solute
Specific Solvent
Interpreting Solubility Curves
Name ______________________________
Date ________________ Period _________
Using the solubility graph, answer the following questions.
19. Which substance does not appear to increase greatly in solubility as the temperature is
increased? ____________
20. Which substance(s) appears to decrease in solubility as the temperature is increased?
__________________________________________________________________
21. Which substance appears to increase most in solubility as the temperature is increased?
______________
22. Which substance is most soluble at 0C? ___________________________________
23. Which substance is least soluble at 0C? ___________________________________
24. Which two substances have the same solubility at 73C? _______________________
25. What is the most KNO3 that can be dissolved at 70C? ________________________
26. What is the most NH4Cl that can be dissolved at 70C?________________________
27. At 70C which substance, KNO3 or NH4Cl, can form the more concentrated solution?
_______________
28. At what temperature would you need 100 g of water to dissolve 70 g of NH4Cl? __________
29. At what temperature would you need 100 g of water to dissolve 70 g of KNO3? __________
Solubility Worksheet
30. What is the solubility of KNO3 at 30C? ____________________________________
31. What is the solubility at KNO3 at 70C? ____________________________________
32. Which compound varies the least in solubility over the temperature range of the graph?
_________________
33. In general, what can you say about the solubility of most solids in relationship to temperature?
___________________________________________________________________________
34. Which compounds do not appear to follow this trend? _______________________________
35. What change occurs in the solubility of NH3 as the temperature of the solution increases from
20C to 100C? _____________________________________________________________
36. What is the difference between the solubilities of KNO3 and NaCl at 24C? ______________
37. What is the difference between the solubilities of KNO3 and NaCl at 73C? ______________
38. What type of solution will be formed if 120 grams of KI dissolved in 100 ml of water at 10C?
__________________________________
39. What type of solution will be formed if 120 grams of NaNO3 dissolve in 100 ml of water at 40C?
________________________________
40. How many grams of NaCl are needed to make a saturated solution at 100C? ________________
41. A saturated solution of KCl is made at 70C. 100 ml of solution is cooled to 50C and stirred.
How many grams of KCl solid will appear on the bottom of the beaker? ______________
42. At 100C, the least soluble compound is ______________________.
43. At OC, the most soluble compound is ______________________.
The Nature of Solutions
_______44. solution
a. capable of being dissolved
_______45. solute
b. solution with water as the solvent
_______46. solvent
c. substance that is dissolved in a solution
_______47. soluble
d. substance that dissolves in water to form a solution that conducts
an electric current
_______48. alloy
e. a solution containing two or more metals
_______49. aqueous solution
f. homogeneous mixture of two or more substances in a single
physical state
_______50. electrolyte
g. substance that does the dissolving in a solution
In the space provided, describe and give an example of each of the following types of solutions.
51. alloy
_______________________________________________________________________
52. liquid solution _____________________________________________________________________
53. gaseous solution ___________________________________________________________________
Answer each of the following questions in the space provided.
54. Describe the properties of a solution. ___________________________________________________
_________________________________________________________________________________
55. Explain how to distinguish between the solvent and the solute in a solution. ____________________
_________________________________________________________________________________
56. Why might a construction company build a high-rise building with steel alloy beams instead of pure
iron beams? _______________________________________________________________________
__________________________________________________________________________________
57. Water and ethanol are miscible in all proportions, whereas oil and water are immiscible. Explain this
statement. ________________________________________________________________________
_________________________________________________________________________________
58. Why is water called the universal solvent? ______________________________________________
_________________________________________________________________________________
59. How could you determine experimentally whether a given substance is an electrolyte?
________________________________________________________________________________
60. Give two examples of solutions in nature and explain why each is important. ___________________
_________________________________________________________________________________
Solutions Practice
Circle One:
61. Which state’s streams will trout survive in better?
Georgia
Maine
62. Which will the fizz remain better in soda?
in the refrigerator
at the beach
63. Which will dissolve more sugar in your drink?
ice tea
hot tea
64. Does CO2 dissolve more in soda under
high pressure
low pressure
neither
65. Does sugar dissolve more in soda under
high pressure
low pressure
neither
Beaker #1
Beaker #2
Iodine
&
Water
Salt
&
Water
Beaker #3
Beaker #4
Salt
&
CCl4
Iodine
&
CCl4
66. List the solute: ____________
_______________
_______________
_______________
67. List the solvent: ___________
_______________
_______________
_______________
68. Look at the beakers above, label solutes as either ionic or molecular:
______________
_______________
_______________
_______________
69. Look at the beakers above, label solvents as either polar or nonpolar:
______________
_______________
_______________
_______________
70. Label which solutions will be soluble or insoluble:
______________
_______________
_______________
_______________
71. Which salt is least soluble in water at 20◦C? ________________
72. How many grams of potassium chloride, KCl, can be dissolved in 200 g of H2O at 80◦C? __________
73. At 40◦C, how much potassium nitrate, KNO3, can be dissolved in 300 g of H2O? ___________
74. Which salt shows the least change in solubility from O◦C to 100◦C? __________
75. At 30◦C, if 90 g of sodium nitrate, NaNO3, is dissolved in 100 g of H2O is this solution saturated,
unsaturated or supersaturated? ________________________
76. A saturated solution of potassium chlorate is formed in 100 g of H2O. If the saturated solution is
cooled from 80◦C to 50◦C, how many grams of precipitate are formed? _____________
77. What compound shows a decrease in solubility from 0◦C to 100◦C? ________ why? ______________
78. Which salt is most soluble at 10◦C? ____________
79. Which salt is least soluble at 50◦C? ____________
80. Which salt is least soluble at 90◦C? ____________
Molarity Problems
Concentration of Solutions: Complete each of the following sentences by filling in the appropriate word or
phrase. Then solve each of the following problems as directed. Show all your work.
81. ___________________is the concentration of a solution expressed as the number of moles of solute
dissolved in each liter of solution.
82. A ______________________ solution contains as much solute as can be possibly dissolved under
existing conditions of temperature and pressure.
83. The amount of solute in a given amount of solvent or solution is the ____________________ of a
solution.
84. A solution that contains more solute particles than are needed to form a saturated solution is
_________________________.
85. A solution that has less than the maximum amount of solute that can be dissolved is called a(n)
___________________________ solution.
86. What is the molarity of the solution formed by mixing 0.20 mol of sodium hydroxide with enough
water to make 150. ml of solution?
87. How many grams of potassium bromide should be added to water to prepare 0.50 L of solution with a
molarity of 0.125 M?
88. What is the molarity of the solution produced when 145 g of sodium chloride is dissolved in sufficient
water to prepare 2.75 L of solution?
89. How many grams of potassium chloride are needed to prepare 0.750 L of a 1.50 M solution of
potassium chloride in water?
90. What is the molarity of the solution produced when 85.6 g of hydrochloric acid is dissolved in
sufficient water to prepare 0.385 L of solution?
91. To produce 3.00 L of a 1.90 M solution of sodium hydroxide, how many grams of sodium
hydroxide must be dissolved?
92. If 8.77 g of potassium iodide are dissolved in sufficient water to make 4.75 L of solution,
what is the molarity of the solution?
93. In order to prepare 2.00 L of a 3.00 M solution of iron (III) chloride, how many grams of
iron (III) chloride must be used?
94. What is the molarity of the solution produced when 14.1 g of ammonia (NH3) is dissolved in
sufficient water to prepare 0.100 L of solution?
95. Copper (II) sulfate, an important copper salt, is used in copper electroplating cells and to kill
algae in swimming pools and water reservoirs. What is the molar concentration of an
electroplating solution in which 1.50 mol of copper (II) sulfate are dissolved in water to make
2.00 L of solution?
96. Sodium bicarbonate is used medicinally to counteract excess stomach acidity. How many
moles of solid sodium bicarbonate would be needed to make 100. mL of 0.660 mol/L
solution suitable for use as an antacid?
97. What is the molar concentration of a solution in which 0.240 mol of washing soda,
Na2CO3 10H2O, is dissolved in water to make 480. mL of a solution for softening wash
water?
98. A useful tile and household cleaner is (tri)sodium phosphate – (TSP). Find the number of
moles of Na3PO4 in 2.00 L of a 0.100 mol/L Na3PO4(aq) cleaning solution prepared for use at
home.
99. A given sample of household ammonia contains 156 g of NH3(g) dissolved in water to form
2.00 L of solution. What is the molar concentration of the household ammonia solution?
100. A rust stain remover may be prepared by dissolving potassium persulfate (K2SO5) in water.
How many moles of potassium persulfate are there in 500. mL of a 0.242 mol/L solution
suitable for removing dust stains?
101. What is the molar concentration of 500. mL of a solution that contains 12.7 g of swimming
pool chlorinator, Ca(OCl)2?
102. A car battery terminal protective coating can be prepared by dissolving 240.0 g of sodium
silicate, (Na2SiO3), in water to make 250. mL of solution. What is the molar concentration of
the solution?
103. Since a saturated solution of calcium chloride does not freeze until –55 ºC, calcium chloride
can be used to melt ice on roads and walks. What is the molar concentration of a saturated
solution in which 3.944 kg of calcium chloride is dissolved in water to make 5.00 L of
solution?
104. Sodium phosphate may be used to remove scale deposits from a car radiator. What volume
of a 0.075 mol/L solution would contain the necessary 1.10 mol of sodium phosphate to
remove the radiator scales?
105. Sodium thiosulfate pentahydrate, known as hypo, is used as a fixer in photography because it
readily dissolves silver compounds. Describe how to prepare 100. mL of a 0.120 mol/L hypo
solution.
106. A solution of sodium phosphate makes a very efficient cleaner for old brushes hardened with
paint. What volume of 0.700 mol/L brush cleaning solution can be prepared from the 126 g
sodium phosphate?
107. Ammonium carbonate is a suitable substitute replacement for the aqueous solution of
ammonia as a household cleaning agent because it yields ammonia readily. Describe how to
prepare 500. mL of a 0.450 mol/L solution of ammonium carbonate.
Solutions & Solubility Curves
Part A: Choose words from the word list to fill in the blanks in the following paragraphs relating to solutions and the
dissolving process. The list groups words with contrasting or related meanings.
WORD LIST:
atoms / ions / molecules
grams
small / large
dissolve(s)
homogeneous /heterogeneous
solute / solvent
filter
phase
solid / liquid / gas
filtration
scatters
solution / suspension
108. A solution is a _________________________________ mixture of two or more substances.
The composition of this mixture can vary within certain limits. In the case of a solution of table salt and water, careful
experiments show that a maximum of 35.7g of sodium chloride can be dissolved in 100g of water at 0oC. Thus, the
concentrations of aqueous solutions of sodium chloride can vary in any amount up to 35.7 _______________ of sodium
chloride per 100 ________________ of water.
A solution is composed of a solvent and at least one ______________________. One substance
is uniformly dispersed, or spread, throughout the other. In an ordinary solution, the substance present in the greatest
amount is called the ____________________________. The other substance, called the ______________________, is
uniformly dispersed throughout the solvent. The ___________________
is described as the dissolving medium; that is, the action of the _____________________________ has caused the
particles of the solute to become uniformly dispersed throughout the mixture. In many cases, one of the components
changes ______________________ as the solution is formed. The substance that changes phase is called the
________________________ while the substance that does not change phase is the _________________________. The
________________________ is considered to have dissolved the ______________________.
Water is a common solvent for many substances representing all three phases. Many
common solids such as table salt and sugar, dissolve in water to form solutions in the _______________
phase. Liquids such as ethyl alcohol and glycerine _______________________ in water. Ammonia is one
______________ that is very soluble in water. Other gases such as oxygen and carbon dioxide
_________________________ in water to a much lesser extent.
The particles of solute within a solution are very ____________________ in size. Most of these particles are
molecules, _____________________, or ______________________. Since the particle size is so small, solutions
cannot be separated into solute and solvent by _________________________.
Solute particles are too small to be trapped by the fibers of the _______________________.
A sample of a true ___________________________ is clear and transparent. It may have a color. The
______________________ size of the solute particles permits a beam of light to pass through a solution unchanged.
Some mixtures that appear to be solutions, but are actually __________________________, because they contain
particles too ____________________ to be true solutes. These particles, which are larger than molecules,
____________________ or ___________________, partially block and scatter a beam of light (the Tyndall Effect.)
Part B: Define the following words in reference to solutions:
 solubility:___________________________________________________________________
 saturated:___________________________________________________________________
 unsaturated:_________________________________________________________________
 supersaturated:_______________________________________________________________
Part C: Describe what would happen if a single crystal of solute were dropped into each of the three
types of solutions. The results of the addition of a single crystal to a solution is the test for the
type of solution.
 saturated:________________________________________________________________
 unsaturated:______________________________________________________________
 supersaturated:___________________________________________________________
Part D: Use your solubility curve to answer the following questions:
109. What is the solubility of NaNO3 at 20oC? ________________________________________
110. What is the solubility of NaNO3 at 40oC? ________________________________________
111. What type of solution will be formed if 120.g of KI dissolve in 100.g of water at 40oC?
_________________________
112. What type of solution will be formed if 80.g of NH4Cl dissolve in 100.g of water at
70.oC?__________________________
113. How many grams of KCl are needed to make a saturated solution at 100oC? ______________
114. A saturated solution of KNO3 is made at 70oC. 100. grams of solution is cooled to 50oC and
stirred. How many grams of solid KNO3 will appear on the bottom of the beaker? _________
115. At 100.oC, the least soluble solid compound is ___________________.
116. At 0oC, the most soluble solid compound is _____________________.
117. NH3, HCl and SO2 are gases. As temperature increases, what happens to their solubilities?
___________________________
118. Over the temperature range shown, the least soluble gas is ____________________
119. The gas which shows the greatest change over the temperature range is _________________
120. To make a saturated solution of NH4Cl at 60.oC, you would add ___________grams to 100.g
of H2O.
121. To make an unsaturated solution of KClO3 at 40.oC, you can add no more than __________g
of KClO3 to 100.g of H2O.
122. 100.g of a saturated solution of NH3(g) in H2O was heated from 20.oC to 50.oC. How many
grams of NH3 gas could be collected? _____________________