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 Specific Solute Specific SolventGas 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

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 0C? ___________________________________

23. Which substance is least soluble at 0C? ___________________________________

24. Which two substances have the same solubility at 73C? _______________________

25. What is the most KNO3 that can be dissolved at 70C? ________________________

26. What is the most NH4Cl that can be dissolved at 70C?________________________

27. At 70C 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 30C? ____________________________________

31. What is the solubility at KNO3 at 70C? ____________________________________

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

20C to 100C? _____________________________________________________________

36. What is the difference between the solubilities of KNO3 and NaCl at 24C? ______________

37. What is the difference between the solubilities of KNO3 and NaCl at 73C? ______________ 38. What type of solution will be formed if 120 grams of KI dissolved in 100 ml of water at 10C?

__________________________________

39. What type of solution will be formed if 120 grams of NaNO3 dissolve in 100 ml of water at 40C?

________________________________

40. How many grams of NaCl are needed to make a saturated solution at 100C? ________________

41. A saturated solution of KCl is made at 70C. 100 ml of solution is cooled to 50C and stirred.

How many grams of KCl solid will appear on the bottom of the beaker? ______________

42. At 100C, the least soluble compound is ______________________.

43. At OC, 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 Beaker #3 Beaker #4

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:

______________ _______________ _______________ _______________

Salt & Water

Iodine & Water

Salt & CCl4

Iodine & CCl4

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 / largedissolve(s) homogeneous /heterogeneous solute / solventfilter phase solid / liquid / gasfiltration scatters solution / suspension108. 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? _____________________