Download _______1. solution a. capable of being dissolved _______2. solute

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 ___________________________________________________________________
_________________________________________________________________________________
Solutions Practice
Circle One:
11. Which state’s streams will trout survive in better?
Georgia
Maine
12. Which will the fizz remain better in soda?
in the refrigerator
at the beach
13. Which will dissolve more sugar in your drink?
ice tea
hot tea
14. Does CO2 dissolve more in soda under
high pressure
low pressure
neither
15. 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
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 Curves
Name ______________________________
Date ________________ Period _________
Using the solubility graph, answer the following questions.
21. Which substance does not appear to increase greatly in solubility as the temperature is
increased? ____________
22. Which substance(s) appears to decrease in solubility as the temperature is increased?
__________________________________________________________________
23. Which substance appears to increase most in solubility as the temperature is increased?
______________
24. Which substance is most soluble at 0C? ___________________________________
25. Which substance is least soluble at 0C? ___________________________________
26. Which two substances have the same solubility at 73C? _______________________
27. What is the most KNO3 that can be dissolved at 70C? ________________________
28. What is the most NH4Cl that can be dissolved at 70C?________________________
29. At 70C which substance, KNO3 or NH4Cl, can form the more concentrated solution?
_______________
30. At what temperature would you need 100 g of water to dissolve 70 g of NH4Cl? __________
31. At what temperature would you need 100 g of water to dissolve 70 g of KNO3? __________
Solubility Worksheet
32. What is the solubility of KNO3 at 30C? ____________________________________
33. What is the solubility at KNO3 at 70C? ____________________________________
34. Which compound varies the least in solubility over the temperature range of the graph?
_________________
35. In general, what can you say about the solubility of most solids in relationship to temperature?
___________________________________________________________________________
36. Which compounds do not appear to follow this trend? _______________________________
37. What change occurs in the solubility of NH3 as the temperature of the solution increases from
20C to 100C? _____________________________________________________________
38. What is the difference between the solubilities of KNO3 and NaCl at 24C? ______________
39. What is the difference between the solubilities of KNO3 and NaCl at 73C? ______________
40. What type of solution will be formed if 120 grams of KI dissolved in 100 ml of water at 10C?
__________________________________
41. What type of solution will be formed if 120 grams of NaNO3 dissolve in 100 ml of water at
40C?
________________________________
42. How many grams of NaCl are needed to make a saturated solution at 100C?
________________
43. 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? ______________
44. At 100C, the least soluble compound is ______________________.
45. 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:
a. the forward reaction to increase, producing a shift to the right in the equilibrium
b. the reverse reaction to increase, producing a shift to the left in the equilibrium
85. 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.
86. Suppose more molecules of “C” are added to the system: the increased number of “C” molecules can
react with _______ molecules, forming more molecules of __________.
87. In other words, when more molecules of “C” are added to the system, the equilibrium shifts to the left,
forming more (reactants / products).
88. In the following system:
2H2O  2H2 + O2
If more H2O is introduced, will there be (more / less) H2 and O2 formed?
89. Therefore, to relieve the stress of extra H2O, the equilibrium shifts to the (right / left) forming more
(products / reactants).
90. Considering the same system used in #6, if more H2 is added to the system, which reaction is
increased? (forward / reverse)
91. Therefore, to relieve the stress of extra H2, the equilibrium shifts to the (right / left).
92. Factor #2 – Pressure
93. 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.
94. 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)?
97. 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.
99. 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 / C and 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?
102.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]
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?
[NH3]
HEAT
SHIFT
Chart #2
Fill in all blanks with increase (↑), decrease (↓), or no change (NC). Under the SHIFT column show
LEFT (←) or RIGHT (→).
107.
H2(g)
Stress
[H2]
+
F2(g)
↔
[F2]
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?
2HF(g)
[HF]
H = +541 KJ
HEAT
SHIFT
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)
Stress
Add
O2
[NH3]
+
5O2(g)
4 NO(g) + 6 H2O(g)
[O2]
[NO]
 H = -906 kJ
[H2O]
Shift
Remove
NO
Remove
O2
Add
H 2O
Decrease
volume
Decrease
temperature
109.
C2H6(g)
Stress
Increase volume
Increase pressure
Remove
C2H6
Add
H2
Remove
C2H4
[C2H6]
H2(g)
+
[H2]
C2H4(g)
[C2H4]
Shift
110.
PbSO 4(s)
Stress
+
H+(aq)
Pb+2(aq) + 2HSO4-(aq)
[H+]
[PbSO4]
[Pb+2]
[HSO4-]
Shift
Heat
Shift
Add
PbSO4
Add
H+
Remove
Pb+2
Add
HSO4Remove
PbSO4
Remove
H+
Increase
pressure
111.
N2(g)
Stress
Add N2
[N2]
+ 3H2(g)
2NH3(g) +
[H2]
[NH3]
Heat
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 SO 3.
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
decrease the 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.
128.
Kinetic Energy: energy of ________________. This includes both ___________ and
_________________ (speed and direction.)
129.
Activation Energy: difference in energy from the ____________ of the diagram to the energy of
the __________________.
130.
Activated Complex: a _____________-lived complex formed during bond ________________
and _________________. It is neither _________________ nor ___________________.
131.
The Collision Theory states that __________________ must collide in order to react.
132.
A collision is effective if it leads to the formation of ________________.
133.
In an effective _________________, the particles must be oriented in a favorable position that
allows bonds to break and atoms to rearrange.
134.
Conservation of energy means that energy is __________________ from one form to another.
135.
The energy required to break bonds among reactants comes from the _______________
________________ (motion) of the reacting particles.
136.
The difference between energy at the peak of the activation diagram and the energy of the
reactants is called the ____________________ ___________________.
137. When particles collide with energy equal to the activation energy, existing ___________ are
disrupted and new bonds form.
138.
During the transition state, the reactants form an __________________ _______________ which
is short-lived and is neither reactant nor __________________.
139. The _________________ __________________ may then reform the original
__________________
or form new bonds and separate into ________________________.
140. The activated complex is a very short-lived molecular complex in which the _________ are in the
process of being broken and reformed.
141. 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?
_____________
142. 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.
a. Which reaction requires a higher activation energy, photosynthesis or oxidation? ______________
b. Which reaction requires a net energy input, photosynthesis or oxidation? ____________________
c. Does activation energy have any effect of the net energy change of a reaction? _______ Explain.
_______________________________________________________________________________