SolutionsName:

______1. solutiona. capable of being dissolved

______2. soluteb. solution with water as the solvent

______3. solventc. substance that is dissolved in a solution

______4. solubled. substance that dissolves in water to form a solution that conducts

an electric current

______5. alloye. a solution containing two or more metals

______6. aqueous solutionf. homogeneous mixture of two or more substances in a single

physical state

______7. electrolyteg. 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 ______

______

Solutions PracticeCircle One:

11. Which state’s streams will trout survive in better?GeorgiaMaine

12. Which will the fizz remain better in soda?in the refrigeratorat the beach

13. Which will dissolve more sugar in your drink?ice teahot tea

14. Does CO2 dissolve more in soda under high pressurelow pressureneither

15. Does sugar dissolve more in soda under high pressurelow pressureneither

Beaker #1 Beaker #2 Beaker #3 Beaker #4

16. List the solute: ______

1

17. List the solvent: ______

18. Look at the beakers above, label solutes as either ionic or molecular:

______

19. Look at the beakers above, label solvents as either polar or nonpolar:

______

20. Label which solutions will be soluble or insoluble:

______

Interpreting Solubility CurvesName ______

Date ______Period ______

Using the solubility graph, answer the following questions.

  1. Which substance does not appear to increase greatly in solubility as the temperature is

increased? ______

  1. Which substance(s) appears to decrease in solubility as the temperature is increased?

______

  1. Which substance appears to increase most in solubility as the temperature is increased?

______

  1. Which substance is most soluble at 0C? ______
  1. Which substance is least soluble at 0C? ______
  1. Which two substances have the same solubility at 73C? ______
  1. What is the most KNO3 that can be dissolved at 70C? ______
  1. What is the most NH4Cl that can be dissolved at 70C?______
  1. At 70C which substance, KNO3 or NH4Cl, can form the more concentrated solution?

______

  1. At what temperature would you need 100 g of water to dissolve 70 g of NH4Cl? ______
  1. At what temperature would you need 100 g of water to dissolve 70 g of KNO3? ______

Solubility Worksheet

  1. What is the solubility of KNO3 at 30C? ______
  1. What is the solubility at KNO3 at 70C? ______
  1. Which compound varies the least in solubility over the temperature range of the graph?

______

  1. In general, what can you say about the solubility of most solids in relationship to temperature?

______

  1. Which compounds do not appear to follow this trend? ______
  1. What change occurs in the solubility of NH3 as the temperature of the solution increases from

20C to 100C? ______

  1. What is the difference between the solubilities of KNO3 and NaCl at 24C? ______
  1. What is the difference between the solubilities of KNO3 and NaCl at 73C? ______
  1. What type of solution will be formed if 120 grams of KI dissolved in 100 ml of water at 10C?

______

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

______

  1. How many grams of NaCl are needed to make a saturated solution at 100C? ______
  1. 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? ______

  1. At 100C, the least soluble compound is ______.
  1. At OC, the most soluble compound is ______.

46. Which salt is least soluble in water at 20◦C? ______

47. How many grams of potassium chloride, KCl, can be dissolved in 200 g of H2O at 80◦C? ______

48. At 40◦C, how much potassium nitrate, KNO3, can be dissolved in 300 g of H2O? ______

49. Which salt shows the least change in solubility from O◦C to 100◦C? ______

50. At 30◦C, if 90 g of sodium nitrate, NaNO3, is dissolved in 100 g of H2O is this solution saturated,

unsaturated or supersaturated? ______

51. 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? ______

52. What compound shows a decrease in solubility from 0◦C to 100◦C? ______why? ______

53. Which salt is most soluble at 10◦C? ______

54. Which salt is least soluble at 50◦C? ______

55. 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.

56. ______is the concentration of a solution expressed as the number of moles of solute

dissolved in each liter of solution.

57. A ______solution contains as much solute as can be possibly dissolved under

existing conditions of temperature and pressure.

58. The amount of solute in a given amount of solvent or solution is the ______of a

solution.

59. A solution that contains more solute particles than are needed to form a saturated solution is

______.

60. A solution that has less than the maximum amount of solute that can be dissolved is called a(n)

______solution.

61. 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?

62. 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?

63. 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?

64. How many grams of potassium chloride are needed to prepare 0.750 L of a 1.50 M solution of

potassium chloride in water?

65. 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?

66. To produce 3.00 L of a 1.90 M solution of sodium hydroxide, how many grams of sodium

hydroxide must be dissolved?

67. 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?

68. 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?

69. 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?

70. 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?

71. 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?

72. 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?

73. 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.

74. 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?

75. 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?

76. What is the molar concentration of 500.mL of a solution that contains 12.7 g of swimming

pool chlorinator, Ca(OCl)2?

77. 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?

78. 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?

79. 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?

80. 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.

81. 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?

82. 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.

Equilibrium Name ______

Le Chatelier’s Principle Period ______Date ______

83. In a chemical reaction, a dynamic equilibrium is established when the rate of the forward reaction is ______ to the rate of the reverse reaction, as represented by the general equation:

A + B  C + D

84. Now we will consider factors that disturb this equilibrium, causing either:

  1. the forward reaction to increase, producing a shift to the right in the equilibrium
  2. the reverse reaction to increase, producing a shift to the left in the equilibrium
  1. Factor #1 – Concentration

If more molecules of “A” are added to the system at equilibrium, then there will be more collisions between “A” molecules and the remaining “B” molecules, producing more the products, “C” and “D,” causing the equilibrium to shift to the right.

  1. Suppose more molecules of “C” are added to the system: the increased number of “C” molecules can react with ______ molecules, forming more molecules of ______.
  1. In other words, when more molecules of “C” are added to the system, the equilibrium shifts to the left, forming more (reactants / products).
  1. In the following system: 2H2O  2H2 + O2

If more H2O is introduced, will there be (more / less) H2 and O2 formed?

  1. Therefore, to relieve the stress of extra H2O, the equilibrium shifts to the (right / left) forming more (products / reactants).
  1. Considering the same system used in #6, if more H2 is added to the system, which reaction is increased? (forward / reverse)
  1. Therefore, to relieve the stress of extra H2, the equilibrium shifts to the (right / left).
  1. Factor #2 – Pressure
  1. Given: 2 A(g) + B(g)  C(g) + D(g)

If the above system is gaseous, in a closed container, at a constant temperature, then there are 3 volumes of reactants to every 2 volumes of products. If the pressure is increased on the system, (according to Boyle’s Law, increased pressure means ______volume), then the system will try to occupy a smaller volume which is accomplished by forming more products because 2 volumes occupy less space than 3 volumes. Therefore, the ______ reaction will increase forming more C and D.

  1. Conversely, if pressure is decreased, then the system will occupy a larger volume, which means the (forward / reverse) reaction will increase, forming more (products / reactants).

95. 2H2O(g)  2H2(g) + O2(g)

In the above gaseous system, at constant temperature, if the pressure is increased, which reaction will increase (forward / reverse)? (More / Less) products will form; (more / less) reactants will form.

96. CO(g) + NO2(g)  CO2(g) + NO(g)

Suppose the pressure on the above system is increased, which will increase (products/ reactants)?

  1. Factor #3 Temperature

A + B  C + D + heat

Note that the above reaction, reading from the left to right is exothermic, i.e., it ______ heat. Note that, reading from the right to left, the reverse reaction is endothermic, i.e., it ______ heat. If the temperature is increased on the above system, then the reaction which absorbs or uses heat will be increased, in this case, the reverse reaction ______.

98. 2HI  H2 + I2 + heat

If the temperature is increased, there be (more / less) HI formed as the result.

99. CH2OH + heat  CO + 2H2

If the temperature is increased, there be (more / less) CO and H2 as a result.

  1. Going back to the generalized equation in #15, if the temperature is decreased, then the reaction which produces heat is increased, in this case, the forward reaction, producing more (A and B / Cand D).

100. 2 SO2 + O2  2 SO3 + heat

If the temperature is decreased on the above system, which reaction increases, (forward / reverse)? There will be (more / less) SO3.

101. 2CO2 + heat  2 CO + O2

If the temperature is decreased on the above system, which reaction is increased? (forward / reverse) There will be (more / less) CO2. There will be (more / less) CO and O2?

  1. These examples have been illustrations of LeChatelier’s Principle which states that a system at equilibrium, when subjected to stress, will temporarily adjust itself to relieve the stress. This means that the shift to the right or left, or the increased forward or reverse reaction, will be temporary and a new equilibrium will be reestablished.

103. Apply these principles in the following equations:

2SO2(g) + O2(g)  2SO3(g) + heat

What conditions of temperature and pressure favor high equilibrium concentrations of SO3? (high / low) pressure; (high / low) temperature

104. 3 H2(g)+ N2(g)  2 NH3(g) + heat

The commercial production of ammonia uses the Haber Process which is expressed by the above equation. What condition of temperature and pressure will provide a maximum yield of NH3? (high / low) pressure: (high / low) temperature

105. 4HCl(g)+ O2(g)  2 H2O(g) + 2 Cl2(g) + heat

Increasing the temperature of the reaction will (increase / decrease) the forward reaction. Decreasing the pressure on the system will (increase / decrease) the forward reaction.

LeChatelier’s Principle

Fill in all blanks with increase (↑), decrease (↓), or no change (NC). Under the SHIFT column show

LEFT (←) or RIGHT (→).

106.

N2(g) + 3H2(g) ↔ 2NH3(g) + HEAT

Stress / [N2] / [H2] / [NH3] / HEAT / SHIFT
Add N2
Increase
Pressure
Cool Rxn.
Remove NH3
Remove H2
Add Heat
Add H2
Remove N2
Add NH3
Decrease
Pressure

How can you make the maximum amount of NH3?

Chart #2

Fill in all blanks with increase (↑), decrease (↓), or no change (NC). Under the SHIFT column show

LEFT (←) or RIGHT (→).

107.

H2(g) + F2(g) ↔ 2HF(g) H = +541 KJ

Stress / [H2] / [F2] / [HF] / HEAT / SHIFT
Add H2
Increase
Pressure
Cool Rxn.
Remove HF
Remove F2
Add Heat
Add F2
Remove H2
Add HF
Decrease
Pressure

How can you make the maximum amount of HF?

Directions: Indicate the effect of the stress on each substance in each reaction. Use the following symbols to show changes in concentration and shifts: () Increase, () Decrease, (NC) No change, () Shift to the left, () Shift to the right.

108. 4NH3(g) + 5O2(g) 4 NO(g) + 6 H2O(g)  H = -906 kJ

Stress / [NH3] / [O2] / [NO] / [H2O] / Shift
Add
O2
Remove
NO
Remove
O2
Add
H2O
Decrease volume
Decrease temperature

109. C2H6(g) H2(g) + C2H4(g)

Stress / [C2H6] / [H2] / [C2H4] / Shift
Increase volume
Increase pressure
Remove
C2H6
Add
H2
Remove
C2H4

110. PbSO4(s) + H+(aq) Pb+2(aq) + 2HSO4-(aq)

Stress / [PbSO4] / [H+] / [Pb+2] / [HSO4-] / Shift
Add
PbSO4
Add
H+
Remove
Pb+2
Add
HSO4-
Remove
PbSO4
Remove
H+
Increase pressure

111. N2(g) + 3H2(g) 2NH3(g) + Heat

Stress / [N2] / [H2] / [NH3] / Heat / Shift
Add N2
Increase Pressure
Cool the Mix
Remove NH3
Remove H2
Add Heat

112. Given the equilibrium reaction, list 4 factors which favor a high equilibrium concentration of SO3.

SO2(g) + ½ O2(g) SO3(g) + 23 kcal

Explain how each of the following can affect the rate of a reaction.

113. The nature of the reactants means ______

This can make the reaction slower if ______

This can make the reaction rate faster if ______

114. The temperature is equal to the ______

Typically reactions proceed faster if they are ______and proceed slower if they are ______,

because there will be more ______if particles are moving faster.

115. The concentration of reactants means ______

If the concentration of one of the reactants is increased the rate of the reaction will ______

If the concentration of one of the reactants is decreased the rate of the reaction will ______

116. Increasing the surface area of reactants means ______

If you increase the surface area of a reactant, the reaction will proceed ______. If you

decreasethe surface area of a reactant, the reaction will proceed ______.

117. Catalysts ______the rate of a reaction without being ______. This means

that catalysts are neither a ______nor a ______.

118. List three ways to increase the rate at which a reactions proceeds:

______

______

______

119. If a reaction takes place very slowly, the bonds that are broken and reformed may be ______

120. If you decrease the temperature of a reaction, the molecules will move ______. This

causes the rate of the reaction to ______.

121. Which will react faster with water, a lump of calcium or finely powdered calcium? ______

Explain: ______

122. A chemical reaction rate doubles when the concentration of one reactant is doubled. Explain this in

terms of the Collision Theory:______

______

123. Catalysts lower the energy of activation by ______

______

124. Inhibitors slow down a reaction by ______

______

125. Using the Kinetic-Molecular Theory, give two reasons why reactions occur more rapidly at high

temperatures: ______

126. On the energy diagram below draw a curve representing the same reaction with a catalyst.

How do the activation energies differ? ______

Does the addition of a catalyst change the final energy of the products? ______

Explain______

______

The Reaction Process

Define each term below:

127. Collision Theory: Theory that explains how molecules must ______with proper

______and with enough ______in order to react.

  1. Kinetic Energy: energy of ______. This includes both ______and ______(speed and direction.)
  2. Activation Energy: difference in energy from the ______of the diagram to the energy of the ______.
  3. Activated Complex: a ______-lived complex formed during bond ______and ______. It is neither ______nor ______.
  4. The Collision Theory states that ______must collide in order to react.
  5. A collision is effective if it leads to the formation of ______.
  6. In an effective ______, the particles must be oriented in a favorable position that allows bonds to break and atoms to rearrange.
  7. Conservation of energy means that energy is ______from one form to another.
  8. The energy required to break bonds among reactants comes from the ______(motion) of the reacting particles.
  9. The difference between energy at the peak of the activation diagram and the energy of the reactants is called the ______.
  10. When particles collide with energy equal to the activation energy, existing ______are disrupted and new bonds form.
  1. During the transition state, the reactants form an ______which is short-lived and is neither reactant nor ______.
  2. The ______may then reform the original ______

or form new bonds and separate into ______.

  1. The activated complex is a very short-lived molecular complex in which the ______are in the process of being broken and reformed.

  1. Label the energy diagram to the right by placing the terms reactants and products in the appropriate locations. Indicate the activation energy with a double headed arrow. Place an “X” where the activated complex is located.

How much activation energy is needed to start this reaction? ______

Is this reaction endo or exothermic? ______

  1. The diagram below shows the oxidation of glucose as the forward reaction. For this reaction, the activation energy hill is small. The reverse reaction, which is photosynthesis of glucose, has a higher activation energy hill.
  1. Which reaction requires a higher activation energy, photosynthesis or oxidation? ______
  1. Which reaction requires a net energy input, photosynthesis or oxidation? ______
  1. Does activation energy have any effect of the net energy change of a reaction? ______Explain.

______