Q.
Matching
Match each item with the correct statement below.
a. product
d. balanced equation
b. reactant
e. skeleton equation
c. chemical equation
____
1. a chemical equation that does not indicate relative amounts of reactants and products
____
2. a new substance formed in a chemical reaction
____
3. a starting substance in a chemical reaction
____
4. a concise representation of a chemical reaction
____
5. an equation in which each side has the same number of atoms of each element
Match each item with the correct statement below.
a. activity series of metals
c. combustion reaction
b. single-replacement reaction
d. decomposition reaction
____
6. a reaction in which a single compound is broken down into simpler substances
____
7. a reaction in which oxygen reacts with another substance, often producing heat or light
____
8. a reaction in which the atoms of one element replace the atoms of a second element in a compound
____
9. a list of metals in order of decreasing reactivity
Match each item with the correct statement below.
a. Henry's law
d. supersaturated solution
b. immiscible
e. concentration
c. saturated solution
____ 10. describes liquids that are insoluble in one another
____ 11. solution containing maximum amount of solute
____ 12. solution containing more solute than can theoretically dissolve at a given temperature
____ 13. At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas
above the liquid.
____ 14. measure of the amount of solute dissolved in a specified quantity of solvent
Match each item with the correct statement below.
a. boiling point elevation
d. molarity
b. molality
e. freezing point depression
c. mole fraction
____ 15. number of moles of solute dissolved in 1 L of solution
____ 16. a colligative property related to the fact that ice will form at higher temperatures in the Great Lakes than in
the ocean
____ 17. a colligative property related to a decrease in the vapor pressure of a solution
____ 18. number of moles of solute dissolved in 1 kg of solvent
____ 19. ratio of moles of solute in solution to total number of moles of both solvent and solute
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 20. Chemical reactions
a. occur only in living organisms.
b. create and destroy atoms.
c. only occur outside living organisms.
d. produce new substances.
____ 21. A net ionic equation
a. shows the spectator ions.
b. shows only those particles involved in the reaction.
c. is not necessarily balanced with respect to mass or charge.
d. shows dissolved ionic compounds as dissociated free ions.
____ 22. What does the symbol above the arrow in a chemical equation mean?
a. Heat is supplied to the reaction.
b. A catalyst is needed in the reaction.
c. Electricity is need in the reaction.
d. A precipitate will form during the reaction.
____ 23. Chemical equations
a. describe chemical reactions.
b. show how to write chemical formulas.
c. give directions for naming chemical compounds.
d. describe only biological changes.
____ 24. A skeleton equation shows just the reactants and products whereas a balanced equation shows the
a. approximate amounts of the reactants only.
b. approximate amounts of the products only.
c. products on the left, the reactants on the right.
d. relative amounts of reactants and products.
____ 25. Which of the following combinations of symbol and explanation of symbol is correct when used in a
chemical equation?
a. (g), grams
b. (l), liters
c. (aq), dissolved in water
d. s, solid product
____ 26. In the chemical equation H O (aq)  H O(l)
a. catalyst
b. solid
O (g), the
is a ____.
c. product
d. reactant
____ 27. This symbol (
) indicates that ____.
a. heat must be applied
b. an incomplete combustion reaction has occurred
c. a gas is formed by the reaction
d. the reaction is reversible
____ 28. A catalyst is
a. the product of a combustion reaction.
b. not used up in a reaction.
c. one of the reactants in single-replacement reactions.
d. a solid product of a reaction.
____ 29. Which of the following is the correct skeleton equation for the reaction that takes place when solid
phosphorus combines with oxygen gas to form diphosphorus pentoxide?
a. P(s) O (g)  PO (g)
b. P(s) O(g)  P O (g)
c. P(s) O2(g)  P O (s)
d. P O (s)  P (s) O (g)
____ 30. Rewrite the following word equation as a balanced chemical equation. What is the coefficient and symbol for
fluorine?
nitrogen trifluoride
nitrogen fluorine
a. 6F
b. F
c. 6F
d. 3F
____ 31. What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH
Al(OH)
NaCl
a. 1, 3, 1, 3
b. 3, 1, 3, 1
c. 1, 1, 1, 3
d. 1, 3, 3, 1
____ 32. What are the coefficients that will balance the skeleton equation below?
N +H
NH
a. 1, 1, 2
b. 1, 3, 3
c. 3, 1, 2
d. 1, 3, 2
____ 33. When the equation Fe
a. 1
b. 2
c. 3
d. 4
Cl
FeCl is balanced, what is the coefficient for Cl ?
____ 34. When the following equation is balanced, what is the coefficient for HCl?
Mg(s)
a. 6
b. 3
c. 1
d. 2
HCl(aq)
MgCl (aq)
H (g)
____ 35. Which of the following statements is true about what happens in all chemical reactions?
a. The ways in which atoms are joined together is not changed.
b. New atoms are formed as products.
c. The final substances are called reactants.
d. Bonds between atoms are broken and new bonds are formed.
____ 36. Chemical equations must be balanced to satisfy
a. the law of definite proportions.
b. the law of multiple proportions.
c. the law of conservation of mass.
d. Avogadro’s principle.
____ 37. When the equation KClO (s)
a. 1.
b. 2.
c. 3.
d. 4.
KCl(s) + O (g) is balanced, the coefficient of KClO3 is
____ 38. In every balanced chemical equation, each side of the equation has the same number of ____.
a. atoms of each element
b. molecules
c. moles
d. coefficients
____ 39. What are the missing coefficients for the skeleton equation below?
Cr(s) Fe(NO ) (aq)
Fe(s) Cr(NO ) (aq)
a. 4, 6, 6, 2
b. 2, 3, 2, 3
c. 2, 3, 3, 2
d. 1, 3, 3, 1
____ 40. What are the missing coefficients for the skeleton equation below?
Al (SO ) (aq) KOH(aq)  Al(OH) (aq) K SO (aq)
a. 1, 3, 2, 3
b. 2, 12, 4, 6
c. 4, 6, 2, 3
d. 1, 6, 2, 3
____ 41. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed.
The balanced equation for this reaction is ____.
a. KH BaCl
KCl BaH
b. KOH BaCl
KCl BaOH
c. 2KOH BaCl
2KCl Ba(OH)
d. KOH BaCl
KCl
BaOH
____ 42. The product of a combination reaction is Ba(OH) . If one of the reactants is H O, what is the other reactant?
a. Ba O
b. BaO
c. BaH
d. BaO
____ 43. In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that
shows the
a. periodic table.
b. activity series of metals.
c. common polyatomic ions.
d. ionic charges of representative elements.
____ 44. In order for the reaction 2Al 6HCl
2AlCl
a. Al must be above Cl on the activity series.
b. Al must be above H on the activity series.
c. Heat must be supplied for the reaction.
d. A precipitate must be formed.
3H to occur, which of the following must be true?
____ 45. In a combustion reaction, one of the reactants is
a. hydrogen.
b. nitrogen.
c. oxygen.
d. a metal.
____ 46. The products of a combustion reaction include
a. water, carbon dioxide, and carbon monoxide.
b. hydrogen, water, and carbon dioxide.
c. hydrogen and carbon monoxide.
d. hydrogen and water.
____ 47. The type of reaction that takes place when one element reacts with a compound to form a new compound and
a different element is a ____.
a. combination reaction
b. decomposition reaction
c. single-replacement reaction
d. double-replacement reaction
____ 48. In a double-replacement reaction, the
a. products are always molecular.
b. reactants are two ionic compounds.
c. reactants are two elements.
d. products are a new element and a new compound.
____ 49. Which of the following statements is correct?
a. All combustion reactions are also combination reactions.
b. All chemical reactions can be classified as one of five general types.
c. Incomplete combustion of a hydrocarbon may produce carbon monoxide and water.
d. A single reactant is the identifying characteristic of a single replacement reaction.
____ 50. Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a. PbO
Pb 2O
b. PbO
Pb O
c. Pb O
2Pb O
d. PbO
Pb O
____ 51. What are the correct formulas and coefficients for the products of the following double-replacement reaction?
RbOH H PO

a. Rb(PO ) H O
b. RbPO
2H O
c. Rb PO
3H O
d. H Rb PO OH
____ 52. When the equation for the complete combustion of one mole of C H OH is balanced, the coefficient for
oxygen is ____.
a. 13
2
b. 11
2
c. 7
2
d. 9
2
____ 53. Which of the following statements is true about the decomposition of a simple binary compound?
a. The products are unpredictable.
b. The reactants are the constituent elements.
c. The reactant is a single substance.
d. The product could be an ionic or a molecular compound.
____ 54. Which of the following statements is true about single-replacement reactions?
a. They are restricted to metals.
b. They involve a single product.
c. Two reactants produce two products.
d. Any metal replaces any other metal.
____ 55. In the activity series of metals, which metal(s) will displace hydrogen from an acid?
a. only metals above hydrogen
b. only metals below hydrogen
c. any metal
d. only metals from Li to Na
____ 56. Use the activity series of metals to complete a balanced chemical equation for the following single
replacement reaction.
Ag(s) KNO (aq) 
a. AgNO
K
b. AgK NO
c. AgKNO
d. No reaction takes place because silver is less reactive than potassium.
____ 57. In a double-replacement reaction, one of the products
a.
b.
c.
d.
may precipitate from solution.
will never be a gas.
may be a solid nonmetal.
may be a solid metal.
____ 58. In a double-replacement reaction,
a. the reactants are usually a metal and a nonmetal.
b. one of the reactants is often water.
c. the reactants are generally two ionic compounds in aqueous solution.
d. energy in the form of heat or light is often produced.
____ 59. One of the products when aqueous Na CO reacts with aqueous Sn(NO ) is
a. NaNO .
b. NaSn.
c. Sn(CO ) .
d. CNO .
____ 60. The complete combustion of which of the following substances produces carbon dioxide and water?
a. C H
b. K CO
c. CaHCO
d. NO
____ 61. Which of the following is the correctly balanced equation for the incomplete combustion of heptene, C H ?
a. C H
14O
7CO 7H O
b. C H
7O
7CO 7H O
c. 2C H
21O
14CO
14H O
d. C H
O
C O
7H
____ 62. The reaction 2Fe 3Cl
2FeCl is an example of which type of reaction?
a. combustion reaction
b. single-replacement reaction
c. combination reaction
d. decomposition reaction
____ 63. The equation Mg(s) 2HCl(aq)
a. combination reaction
b. single-replacement reaction
c. decomposition reaction
d. double-replacement reaction
MgCl (aq)
H g is an example of which type of reaction?
____ 64. The equation H PO
3KOH
K PO
a. double-replacement reaction
b. combination reaction
c. decomposition reaction
d. single-replacement reaction
3H O is an example of which type of reaction?
____ 65. The equation 2C H OH 9O
a. combustion reaction
b. single-replacement reaction
8H O is an example of which type of reaction?
6CO
c. double-replacement reaction
d. decomposition reaction
____ 66. A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium
hydroxide. One of the products of this reaction is
a. Co(OH) .
b. Co(OH) .
c. LiCo .
d. LiCl .
____ 67. If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is
____.
a. RuBr
b. Rb Br
c. RbBr
d. RbBr
____ 68. What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
a. Br
NaI
NaBr
I
b. Br
2NaI
2NaBr I
c. Br NaI
NaBrI
d. Br NaI
NaBr I
____ 69. What is the driving force in the following reaction?
Ni(NO ) (aq) K S(aq)
a. A gas is formed.
b. A precipitate is formed.
c. Ionic compounds are reactants.
d. Ionic compounds are products.
____ 70. Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
____ 71. The solubility of potassium chloride is
at 20 C. What is the maximum amount of KCl that can
dissolve in 200 g of water at 20 C?
a. 17 g
b. 34 g
c. 68 g
d. 6800 g
____ 72. What is the solubility of silver nitrate if 11.1 g can dissolve in 5.0 g of water at 20 C?
a.
at 20 C
b.
at 20 C
c.
d.
at 20 C
at 20 C
____ 73. How does shaking or stirring a mixture of solute and solvent affect a solution?
a. It increases the rate of dissolving.
b. It decreases the rate of dissolving.
c. It increases the solubility of the solute.
d. It decreases the solubility of the solute.
____ 74. Which of the following factors affect solubility?
a. temperature and the nature of the solvent
b. temperature and degree of mixing
c. particle size and degree of mixing
d. particle size and temperature
____ 75. If adding of a crystal of the solute to an aqueous solution causes many particles to come out of the solution,
the original solution was ____.
a. unsaturated
b. saturated
c. an emulsion
d. supersaturated
____ 76. Which of the following substances is less soluble in hot water than in cold water?
a. CO
b. NaCl
c. NaNO
d. KBr
____ 77. Which of the following generally occurs as temperature increases?
a. Solubility of a solid solute decreases.
b. Solubility of a solid solute increases.
c. Solubility of a solid solute remains the same.
d. Molarity of a solid solute doubles.
____ 78. Which phrase correctly describes the effect of pressure on the solubility of a gas in a liquid?
a. proportional to the square root of the pressure of the gas above the liquid
b. directly proportional to the pressure of the gas above the liquid
c. inversely proportional to the pressure of the gas above the liquid
d. unrelated to the pressure of the gas above the liquid
____ 79. If the solubility of a particular solute is
represent a supersaturated solution of that solute?
a.
at 25 C
b.
at 15 C
at 20 C, which of the following concentrations would
c.
d.
at 20 C
at 20 C
____ 80. What happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid decreases?
a. The solubility decreases.
b. The solubility increases.
c. The solubility remains the same.
d. The solubility cannot be determined.
____ 81. To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure
would have to be increased to ____.
a. 0.37 atm
b. 0.7 atm
c. 1.37 atm
d. 2.7 atm
____ 82. If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is
the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?
a. 0.75 atm
b. 1.3 atm
c. 4.0 atm
d. 12 atm
____ 83. What is the concentration of a solution?
a. a measure of the number of moles of solute dissolved
b. a measure of the amount of solute in a specified quantity of solvent
c. a measure of the volume of solvent used to make the solution
d. a measure of the amount of solute that can be dissolved
____ 84. What is the concentration of a solution that contains 6 moles of solute in 2 liters of solution?
a. 6M
b. 12M
c. 7M
d. 3M
____ 85. In which of the following is the solution concentration expressed in terms of molarity?
a.
b.
c.
d.
____ 86. Which of the following operations yields the number of moles of solute?
a. molarity moles of solution
b. molarity liters of solution
c. molarity mass of solution
d. moles of solution
volume of solution
____ 87. What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
a. 81M
b. 0.081M
c. 12M
d. 4.0M
____ 88. What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
a. 2.0M
b. 10M
c. 0.40M
d. 4.0M
____ 89. What is the number of moles of solute in 250 mL of a 0.4M solution?
a. 0.1 mol
b. 0.16 mol
c. 0.62 mol
d. 1.6 mol
____ 90. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute
= 26 g/mol)
a. 1.5M
b. 2.2M
c. 2.1M
d. 0.0022M
____ 91. What mass of sucrose, C H O , is needed to make 500.0 mL of a 0.200M solution?
a. 34.2 g
b. 100 g
c. 17.1 g
d. 68.4 g
____ 92. What mass of Na SO is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)
a. 178 g
b. 284 g
c. 356 g
d. 710 g
____ 93. Which of the following is unchanged when a solution is diluted by the addition of solvent?
a. volume of solvent
b. mass of solvent
c. number of moles of solute
d. molarity of solution
____ 94. How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
a. 25 mL
b. 50 mL
c. 100 mL
d. 150 mL
____ 95. The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____.
a. 0.128 mL
b. 7.8 mL
c. 281 mL
d. 362 mL
____ 96. If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute
solution?
a. 0.024M
b. 0.24M
c. 0.30M
d. 0.83M
____ 97. To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI
solution. What is the molarity of the new solution?
a. 180M
b. 2.8M
c. 0.35M
d. 0.18M
____ 98. If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in
solution?
a. 0.5 mL
b. 1.25 mL
c. 5.0 mL
d. 12.5 mL
____ 99. What measures are used to calculate the percent by volume of a solution?
a. mass of solute and volume of solvent
b. mass of solute and volume of solution
c. volume of solute and volume of solvent
d. volume of solute and volume of solution
____ 100. If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute
in solution?
a. 8.0 g
b. 50 g
c. 80 g
d. 800 g
____ 101. The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.
a. 372 mL
b. 40.0 mL
c. 248 mL
d. 580 mL
____ 102. How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution?
a. 252 mL
b. 228 mL
c. 145 mL
d. 142 mL
____ 103. In which of the following is concentration expressed in percent by volume?
a.
100%
b.
c.
d.
100%
100%
100%
____ 104. Which of the following is a colligative property of a solution?
a. boiling point elevation
b. melting point elevation
c. vapor pressure increase
d. freezing point increase
____ 105. Colligative properties depend upon the ____
a. nature of the solute.
b. nature of the solvent.
c. number of solute particles in a solution.
d. freezing point of a solute.
____ 106. A solute depresses the freezing point because the solute ____
a. is colder than the solvent.
b. disrupts crystal formation of the solvent.
c. tends to sink to the bottom of the solution.
d. has bigger molecules than the solvent.
____ 107. The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is ____.
a. 39m
b. 1.7m
c. 0.17m
d. 598m
____ 108. Which of the following is an expression of molality?
a.
b.
c.
d.
____ 109. What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
a. 0.375
b. 0.6
c. 1.67
d. 15
____ 110. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute
= 24 g)
a. 0.67m
b. 4m
c. 1.67m
d. 0.17m
____ 111. What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar
mass of solute = 30 g)
a. 0.24 kg
b. 2.4 kg
c. 0.11 kg
d. 1.1 kg
____ 112. To which of the following variables is change in boiling point directly proportional?
a. molarity of solution
b. molality of solution
c. percent by volume of solution
d. percent (mass/mass) of solution
____ 113. What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (K = 1.86 C/m)
a. –1.86 C
b. –3.72 C
c. –5.58 C
d. –7.44 C
____ 114. The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86 C/m;
molar mass of water = 18 g)
a. 1.66 C
b. –1.66 C
c. 3.33 C
d. –3.33 C
____ 115. What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (K = 0.512 C/m;
molar mass of water = 18 g)
a. 97 C
b. 99.7 C
c. 101.4 C
d. 103 C
____ 116. What is the molality of a solution of water and KCl if the freezing point of the solution is –3 C? (K = 1.86
C/m; molar mass of water = 18 g)
a. 0.6m
b. 1.2m
c. 0.8m
d. 6m
____ 117. What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (K = 0.512 C/m)
a. 100.06 C
b. 100.13 C
c. 100.26 C
d. 100.5 C
____ 118. What is the approximate molar mass of a molecular solute if 300 g of the solute in 1000 g of water causes the
solution to have a boiling point of 101 C? (K = 0.512 C/m; K = 1.86 C/m; molar mass of water = 18 g)
a. 15 amu
b. 30 amu
c. 150 amu
d. 300 amu
Short Answer
119. Balance the following everyday equation described in the following sentence. "A tricycle is made of a handle,
a body, three wheels, and two axles.”
H
B
W
A
HBW A
120. Write the net ionic equation for the following reaction and indicate the state of the products.
Ca(NO ) (aq)
(NH )2SO4(aq)
121. Balance the following equation.
NaClO
NaCl
O
122. Balance the following equation.
Mg
H PO
Mg (PO )
H
123. Balance the following equation.
(NH ) CO
NaOH
Na CO
NH
H O
124. Balance the following equation.
C H
O
CO
H O
125. Balance the following equation.
Ba
H O
Ba(OH)
H
126. Balance the following equation.
Au O
Au
O
127. Balance the following equation. Indicate the states of the products.
Na PO (aq)
ZnSO (aq)
Na SO
Zn (PO )
128. Complete and balance the following equation.
Al
Cl
129. Complete and balance the following equation.
CH
O
CO
130. Complete and balance the following equation.
Fe (SO )
Ba(OH)
131. Balance the following equation. Indicate whether combustion is complete or incomplete.
C H
O
CO
H O
132. Balance the following equation. Indicate whether combustion is complete or incomplete.
2C H OH
O
CO
H O
133. Write a balanced net ionic equation for the following reaction.
H PO (aq)
NaOH(aq)
Na PO (aq)
H O(l)
134. Complete and balance the following equation and indicate the precipitate, if any:
K PO (aq)
BaCl (aq)
135. What mass of KCl (solubility =
at 20 C) can dissolve in 3.30
10 g of water?
136. If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is
202 kPa?
137. How many liters of a 0.30M solution are needed to give 2.7 moles of solute?
138. What is the molarity of a solution containing 9.0 moles of solute in 2500 mL of solution?
139. What is the molarity of a solution containing 1.2 grams of solute in 450 mL of solution? (molar mass of solute
= 24 g)
140. What is the number of moles of solute in 650 mL of a 0.40M solution?
141. How many liters of a 1.5M solution are required to yield 5.0 grams of solute? (molar mass of solute = 30.0 g)
142. If 1.0 mL of 6.0M HCl is added to 499 mL of water to give exactly a 500-mL solution, what is the molarity of
the dilute solution?
143. If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute's percent by
volume?
144. What is the molality of a solution containing 5.0 moles of solute in 3.2 kg of solvent?
145. What is the molality of a solution containing 15 grams of solute in 0.50 kilograms of solvent? (molar mass of
solute = 24 g)
146. Calculate the molality of a solution prepared by dissolving 175 g of KNO in 750 g of water.
147. What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent?
148. How many kilograms of solvent are in a sample of 0.30 molal solution if the sample contains 13 moles of
solute?
149. What is the mole fraction of KCl in a 0.20 molal solution of KCl? (molar mass of KCl = 75 g; molar mass of
water = 18 g)
150. What is the freezing point of a solution that has 5.0 moles of NaI in 1250 g of water? (K = 1.86 C/m; molar
mass of water = 18.0 g)
Essay
151. In general, how are word equations written to describe chemical reactions?
152. Describe how to write the skeleton equation for the following reaction:
iron + oxygen
iron(III) oxide
153. Consider the description: copper(II) oxide reacts with sulfuric acid to produce copper(II) sulfate and water.
List the steps required to write its balanced chemical equation. State how to determine which of the five
general types of reaction this represents.
154. What determines whether one metal will replace another metal from a compound in a single-replacement
reaction?
155. Predict the precipitate that forms when aqueous solutions of silver nitrate and potassium chloride react to
form products in a double-replacement reaction. Include a discussion of how to write the complete chemical
equation describing this reaction.
156. Explain what a saturated solution is. Give a specific example.
157. Discuss the phenomenon of supersaturation. Indicate how crystallization can be initiated in a supersaturated
solution.
158. Discuss the different factors that can affect the solubility of a substance. Include specific examples in your
discussion.
159. Explain on a particle basis how the addition of a solute affects the boiling point, the freezing point, and the
vapor pressure of the solvent.
160. Compare and contrast molarity and molality.
Q.
Answer Section
MATCHING
1. ANS: E
PTS: 1
DIF: L1
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
2. ANS: A
PTS: 1
DIF: L1
REF: p. 346 | p. 347
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
3. ANS: B
PTS: 1
DIF: L1
REF: p. 346 | p. 347
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
4. ANS: C
PTS: 1
DIF: L1
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
5. ANS: D
PTS: 1
DIF: L1
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: knowledge
6. ANS: D
PTS: 1
DIF: L1
OBJ: 11.2.1 Describe the five general types of reactions.
7. ANS: C
PTS: 1
DIF: L1
OBJ: 11.2.1 Describe the five general types of reactions.
8. ANS: B
PTS: 1
DIF: L1
OBJ: 11.2.1 Describe the five general types of reactions.
9. ANS: A
PTS: 1
DIF: L1
OBJ: 11.2.1 Describe the five general types of reactions.
REF: p. 358
BLM: knowledge
REF: p. 363
BLM: knowledge
REF: p. 360
BLM: knowledge
REF: p. 361
BLM: knowledge
10. ANS: B
PTS: 1
DIF: L1
REF: p. 521
OBJ: 16.1.2 Describe the equilibrium in a saturated solution.
BLM: knowledge
11. ANS: C
PTS: 1
DIF: L1
REF: p. 521
OBJ: 16.1.2 Describe the equilibrium in a saturated solution.
BLM: knowledge
12. ANS: D
PTS: 1
DIF: L1
REF: p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: knowledge
13. ANS: A
PTS: 1
DIF: L1
REF: p. 523
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: knowledge
14. ANS: E
PTS: 1
DIF: L1
REF: p. 525
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: knowledge
15. ANS: D
PTS: 1
DIF: L1
REF: p. 525
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: knowledge
16. ANS: E
PTS: 1
DIF: L1
REF: p. 534 | p. 536
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: knowledge
17. ANS: A
PTS: 1
DIF: L1
REF: p. 534 | p. 537
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: knowledge
18. ANS: B
PTS: 1
DIF: L1
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: knowledge
19. ANS: C
PTS: 1
DIF: L1
REF: p. 540
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: knowledge
MULTIPLE CHOICE
20. ANS: D
PTS: 1
DIF: L2
REF: p. 346
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
21. ANS: B
PTS: 1
DIF: L1
REF: p. 370
OBJ: 11.3.1 Describe the information found in a net ionic equation.
BLM: knowledge
22. ANS: A
PTS: 1
DIF: L2
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
23. ANS: A
PTS: 1
DIF: L2
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
24. ANS: D
PTS: 1
DIF: L2
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: comprehension
25. ANS: C
PTS: 1
DIF: L2
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
26. ANS: C
PTS: 1
DIF: L2
REF: p. 347
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
27. ANS: D
PTS: 1
DIF: L1
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
28. ANS: B
PTS: 1
DIF: L1
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: knowledge
29. ANS: C
PTS: 1
DIF: L2
REF: p. 349
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: application
30. ANS: D
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
31. ANS: A
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
32. ANS: D
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
33. ANS: C
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
34. ANS: D
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
35. ANS: D
PTS: 1
DIF: L2
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: comprehension
36. ANS: C
PTS: 1
DIF: L2
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: comprehension
37. ANS: B
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
38. ANS: A
PTS: 1
DIF: L2
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: comprehension
39. ANS: C
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
40. ANS: D
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
41. ANS: C
PTS: 1
DIF: L2
REF: p. 351 | p. 352 | p. 353
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
42. ANS: B
PTS: 1
DIF: L2
REF: p. 356 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
43. ANS: B
PTS: 1
DIF: L2
REF: p. 361
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
44. ANS: B
PTS: 1
DIF: L2
REF: p. 361
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
45. ANS: C
PTS: 1
DIF: L1
REF: p. 363 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: knowledge
46. ANS: A
PTS: 1
DIF: L2
REF: p. 363 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
47. ANS: C
PTS: 1
DIF: L2
REF: p. 360 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
48. ANS: B
PTS: 1
DIF: L2
REF: p. 362 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
49. ANS: C
PTS: 1
DIF: L2
REF: p. 363 | p. 364
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
50. ANS: B
PTS: 1
DIF: L2
REF: p. 358 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
51. ANS: C
PTS: 1
DIF: L2
REF: p. 362 | p. 363
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
52. ANS: D
PTS: 1
DIF: L2
REF: p. 363 | p. 364 | p. 365
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
53. ANS: C
PTS: 1
DIF: L2
REF: p. 358
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
54. ANS: C
PTS: 1
DIF: L2
REF: p. 360 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
55. ANS: A
PTS: 1
DIF: L2
REF: p. 361
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
56. ANS: D
PTS: 1
DIF: L2
REF: p. 361 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: application
57. ANS: A
PTS: 1
DIF: L2
REF: p. 362
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
58. ANS: C
PTS: 1
DIF: L2
REF: p. 362
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
59. ANS: A
PTS: 1
DIF: L2
REF: p. 362 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
60. ANS: A
PTS: 1
DIF: L2
REF: p. 363
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: application
61. ANS: B
PTS: 1
DIF: L2
REF: p. 363 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
62. ANS: C
PTS: 1
DIF: L2
REF: p. 356 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
63. ANS: B
PTS: 1
DIF: L2
REF: p. 360 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
64. ANS: A
PTS: 1
DIF: L2
REF: p. 362 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: comprehension
65. ANS: A
PTS: 1
DIF: L2
REF: p. 363 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: application
66. ANS: A
PTS: 1
DIF: L2
REF: p. 362 | p. 367
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
67. ANS: D
PTS: 1
DIF: L2
REF: p. 356 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
68. ANS: B
PTS: 1
DIF: L2
REF: p. 360 | p. 366
OBJ: 11.2.1 Describe the five general types of reactions.
BLM: analysis
69. ANS: B
PTS: 1
DIF: L3
REF: p. 367 | p. 372
OBJ: 11.2.1 Describe the five general types of reactions. | 11.3.2 Predict the formation of a precipitate in a
double-replacement reaction.
BLM: analysis
70. ANS: A
PTS: 1
DIF: L1
REF: p. 519
OBJ: 16.1.1 Identify the factors that affect how fast a substance dissolves.
BLM: knowledge
71. ANS: C
PTS: 1
DIF: L2
REF: p. 521
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
72. ANS: D
PTS: 1
DIF: L2
REF: p. 521
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
73. ANS: A
PTS: 1
DIF: L1
REF: p. 519
OBJ: 16.1.1 Identify the factors that affect how fast a substance dissolves.
BLM: knowledge
74. ANS: A
PTS: 1
DIF: L1
REF: p. 521 | p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: knowledge
75. ANS: D
PTS: 1
DIF: L2
REF: p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: comprehension
76. ANS: A
PTS: 1
DIF: L2
REF: p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: application
77. ANS: B
PTS: 1
DIF: L2
REF: p. 521
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: comprehension
78. ANS: B
PTS: 1
DIF: L2
REF: p. 523
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: comprehension
79. ANS: D
PTS: 1
DIF: L2
REF: p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
80. ANS: A
PTS: 1
DIF: L1
REF: p. 523 | p. 524
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: knowledge
81. ANS: D
PTS: 1
DIF: L2
REF: p. 523 | p. 524
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
82. ANS: A
PTS: 1
DIF: L2
REF: p. 523 | p. 524
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
83. ANS: B
PTS: 1
DIF: L1
REF: p. 525
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: knowledge
84. ANS: D
PTS: 1
DIF: L1
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
85. ANS: D
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: application
86. ANS: B
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: comprehension
87. ANS: C
PTS: 1
DIF: L2
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
88. ANS: B
PTS: 1
DIF: L2
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
89. ANS: A
PTS: 1
DIF: L2
REF: p. 527
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
90. ANS: B
PTS: 1
DIF: L3
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
91. ANS: A
PTS: 1
DIF: L3
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
92. ANS: D
PTS: 1
DIF: L3
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
BLM: analysis
93. ANS: C
PTS: 1
DIF: L1
REF: p. 528
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: knowledge
94. ANS: B
PTS: 1
DIF: L2
REF: p. 528 | p. 529
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: analysis
95. ANS: D
PTS: 1
DIF: L2
REF: p. 528 | p. 529
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: analysis
96. ANS: A
PTS: 1
DIF: L2
REF: p. 528 | p. 529
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: analysis
97. ANS: D
PTS: 1
DIF: L2
REF: p. 528 | p. 529
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: analysis
98. ANS: C
PTS: 1
DIF: L2
REF: p. 529
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: analysis
99. ANS: D
PTS: 1
DIF: L1
REF: p. 529
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: knowledge
100. ANS: A
PTS: 1
DIF: L2
REF: p. 531
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: analysis
101. ANS: C
PTS: 1
DIF: L2
REF: p. 530
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: analysis
102. ANS: D
PTS: 1
DIF: L2
REF: p. 530
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: analysis
103. ANS: B
PTS: 1
DIF: L2
REF: p. 530
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: comprehension
104. ANS: A
PTS: 1
DIF: L1
REF: p. 534
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: knowledge
105. ANS: C
PTS: 1
DIF: L1
REF: p. 534
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: knowledge
106. ANS: B
PTS: 1
DIF: L2
REF: p. 534
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: comprehension
107. ANS: B
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
108. ANS: A
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: application
109. ANS: A
PTS: 1
DIF: L2
REF: p. 540
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
110. ANS: A
PTS: 1
DIF: L2
REF: p. 539
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
111. ANS: A
PTS: 1
DIF: L2
REF: p. 539
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
112. ANS: B
PTS: 1
DIF: L1
REF: p. 540
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: knowledge
113. ANS: B
PTS: 1
DIF: L2
REF: p. 542 | p. 543
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
114. ANS: D
PTS: 1
DIF: L2
REF: p. 542 | p. 543
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
115. ANS: C
PTS: 1
DIF: L2
REF: p. 542 | p. 544
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
116. ANS: C
PTS: 1
DIF: L3
REF: p. 542 | p. 544
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
117. ANS: C
PTS: 1
DIF: L2
REF: p. 543 | p. 544
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
118. ANS: C
PTS: 1
DIF: L3
REF: p. 542 | p. 544
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
SHORT ANSWER
119. ANS:
H + B + 3W + 2A  HBW A
PTS: 1
DIF: L2
REF: p. 350
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
120. ANS:
Ca2+(aq) SO42-(aq)
CaSO4(s)
PTS: 1
DIF: L3
REF: p. 371 | p. 372
OBJ: 11.3.1 Describe the information found in a net ionic equation. | 11.3.2 Predict the formation of a
precipitate in a double-replacement reaction.
BLM: analysis
121. ANS:
2NaClO
2NaCl 3O
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
122. ANS:
3Mg 2H PO
Mg (PO )
3H
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: application
123. ANS:
(NH ) CO
2NaOH
Na CO
2NH
2H O
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
124. ANS:
C H
3O
3CO
3H O
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
125. ANS:
Ba 2H O
Ba(OH)
H
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
126. ANS:
2Au O
4Au 3O
PTS: 1
DIF: L2
REF: p. 352
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation.
BLM: analysis
127. ANS:
2Na PO
3ZnSO
3Na SO (aq) Zn (PO ) (s)
PTS: 1
DIF: L3
REF: p. 352 | p. 372
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.3.2 Predict the formation
of a precipitate in a double-replacement reaction.
BLM: analysis
128. ANS:
2Al 3Cl
2AlCl
PTS: 1
DIF: L3
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
129. ANS:
CH
2O
CO
2H O
PTS: 1
DIF: L2
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
130. ANS:
Fe (SO )
3Ba(OH)
2Fe(OH)
3BaSO
PTS: 1
DIF: L3
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
131. ANS:
2C H
7O
6CO 8H O (incomplete)
PTS: 1
DIF: L3
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
132. ANS:
C H OH 3O
2CO
3H O (complete)
PTS: 1
DIF: L3
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
133. ANS:
H (aq)
OH (aq)
H O(l)
PTS: 1
DIF: L3
REF: p. 370 | p. 371
OBJ: 11.3.1 Describe the information found in a net ionic equation.
BLM: analysis
134. ANS:
2K PO (aq) 3BaCl (aq)
Ba (PO ) s 6KCl(aq)
PTS: 1
DIF: L3
REF: p. 367 | p. 372
OBJ: 11.2.1 Describe the five general types of reactions. | 11.3.2 Predict the formation of a precipitate in a
double-replacement reaction.
BLM: analysis
135. ANS:
PTS: 1
DIF: L2
REF: p. 521
OBJ: 16.1.2 Describe the equilibrium in a saturated solution.
136. ANS:
S =
=
BLM: analysis
= 3.8 g/L
PTS: 1
DIF: L2
REF: p. 523
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: analysis
137. ANS:
2.7 mol
= 9.0 L
PTS: 1
DIF: L2
REF: p. 527
OBJ: 16.2.1 Calculate the molarity of a solution.
138. ANS:
BLM: analysis
PTS: 1
DIF: L2
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
139. ANS:
BLM: analysis
PTS: 1
DIF: L2
REF: p. 526
OBJ: 16.2.1 Calculate the molarity of a solution.
140. ANS:
BLM: analysis
PTS: 1
DIF: L2
REF: p. 527
OBJ: 16.2.1 Calculate the molarity of a solution.
141. ANS:
BLM: analysis
PTS: 1
DIF: L2
REF: p. 527
OBJ: 16.2.1 Calculate the molarity of a solution.
142. ANS:
BLM: analysis
PTS: 1
DIF: L2
REF: p. 528 | p. 529
OBJ: 16.2.2 Describe the effect of dilution on the total moles of solute in solution.
BLM: analysis
143. ANS:
% = 2.0%
PTS: 1
DIF: L2
REF: p. 529
OBJ: 16.2.3 Express solution concentration as a percent by volume or percent by mass.
BLM: analysis
144. ANS:
PTS: 1
DIF: L1
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
145. ANS:
PTS: 1
DIF: L2
REF: p. 538
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
146. ANS:
molar mass KNO :
K: 1 39.1 g = 39.1 g
N: 1 14.0 g = 14.0 g
O: 3 16.0 g = 48.0 g
molar mass = 101.1 g
PTS: 1
DIF: L2
REF: p. 538 | p. 539
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
147. ANS:
Number of moles = mass of solvent molality
PTS: 1
DIF: L2
REF: p. 538 | p. 539
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
148. ANS:
PTS: 1
DIF: L2
REF: p. 539
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
149. ANS:
PTS: 1
DIF: L2
REF: p. 540 | p. 541
OBJ: 16.4.1 Identify the two ways of expressing the ratio of solute to solvent in a solution.
BLM: analysis
150. ANS:
= 15
PTS: 1
DIF: L2
REF: p. 543
OBJ: 16.4.2 Describe how the freezing-point depression and boiling-point elevation are related to molality.
BLM: analysis
ESSAY
151. ANS:
Reactants and products are written as words. An arrow is drawn between the reactants and the products with
its arrowhead pointing toward the right. Reactants are listed to the left of the arrow, and products are listed to
the right of the arrow. If more than one reactant or product is involved in the reaction, they are separated by
plus signs. The words describe substances that are part of the reaction. The arrow symbolizes that substances
react to produce products, or that reactants yield products.
PTS: 1
DIF: L2
REF: p. 348
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: comprehension
152. ANS:
A skeleton equation includes substances involved in a chemical reaction, but does not necessarily show the
relative quantities of each substance in the reaction. Chemical symbols and formulas are used to indicate the
substances that are part of the reaction. The state of each substance in the skeleton equation may be indicated
in parentheses, with s representing solid, g representing gas, l representing liquid, and aq representing an
aqueous solution. The skeleton equation for the reaction of iron with oxygen to produce iron(III) oxide is not
balanced. It is written as:
Fe(s) + O (g)
Fe O (s)
PTS: 1
DIF: L3
REF: p. 348 | p. 349
OBJ: 11.1.1 Describe how to write a skeleton equation.
BLM: analysis
153. ANS:
A first approach is to indicate the reactants and products in a word equation:
copper(II) oxide + sulfuric acid
copper(II) sulfate + water
Next, convert the word equation to a skeleton equation using chemical formulas:
CuO(s) + H SO (aq)
CuSO (aq) + H O(l)
Because the Cu is exchanged in this reaction involving an aqueous solution, and the molecular compound
H O is formed, the reaction type is double-replacement. In this case, the skeleton equation already is
balanced. Inspection of substances on the left and right of the equation shows that the same relative amounts
(number of atoms) of each element are present in the reactants and the products.
PTS: 1
DIF: L3
REF: p. 352 | p. 367
OBJ: 11.1.2 Describe the steps for writing and balancing a chemical equation. | 11.2.1 Describe the five
general types of reactions.
BLM: analysis
154. ANS:
Whether one metal will replace another is determined by the relative reactivity of the two metals. The activity
series of metals lists metals in order of decreasing reactivity. A reactive metal will replace any metal found
below it in the activity series.
PTS: 1
DIF: L2
REF: p. 361
OBJ: 11.2.1 Describe the five general types of reactions.
155. ANS:
BLM: comprehension
Because the reaction is a double-replacement type, cations are exchanged among compounds during the
reaction. The first step is to write the equation in skeleton form:
AgNO + KCl
AgCl + KNO
Inspection of this equation shows that the insoluble precipitate silver chloride forms in an aqueous solution of
potassium nitrate. The relative amounts of elements are the same on either side of the equation, so the
complete equation is:
AgNO (aq) + KCl(aq)
AgCl(s) + KNO (aq) (balanced)
PTS: 1
DIF: L3
REF: p. 371 | p. 372
OBJ: 11.2.1 Describe the five general types of reactions. | 11.3.2 Predict the formation of a precipitate in a
double-replacement reaction.
BLM: synthesis
156. ANS:
A saturated solution contains the maximum amount of solute for a given amount of solvent at a constant
temperature. For example, no more than 36.2 g of sodium chloride will dissolve in 100 g of water. In a
saturated solution, a dynamic equilibrium exists between the solid and its dissolved ions. In this equilibrium,
as many ions are going out of the solution as are going in per unit time.
PTS: 1
DIF: L2
REF: p. 520
OBJ: 16.1.2 Describe the equilibrium in a saturated solution.
BLM: application
157. ANS:
A solution that contains more solute than it can theoretically hold at a given temperature is a supersaturated
solution. Crystallization can be initiated by adding a seed crystal to the solution or by exposing the solution to
a rough surface. The latter can be done by scratching the inside of the container holding the solution.
PTS: 1
DIF: L2
REF: p. 522
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: application
158. ANS:
The factors are temperature, pressure, and the nature of the solute and solvent. Specific examples include the
following. Potassium nitrate is more soluble in water at high temperature than at low temperature. Gases are
less soluble at high temperatures than at low temperatures. The solubility of a particular gas increases as the
partial pressure of that gas above the solution increases. Sodium nitrate is much more soluble in water than is
barium sulfate, regardless of temperature, because the attractive forces between the ions in BaSO are
stronger than the attractive force of the solvent molecules.
PTS: 1
DIF: L2
REF: p. 521 | p. 523
OBJ: 16.1.3 Describe the factors that affect the solubility of a substance.
BLM: application
159. ANS:
Boiling point elevation, freezing point lowering, and vapor pressure lowering are colligative properties. They
depend on the number of particles in solution and not on the chemical nature of the solute. Boiling point
elevation: Additional attractive forces exist between solute and solvent; they must be overcome for the
solution to boil. Kinetic energy must be added to overcome these forces. Freezing point lowering: More
kinetic energy must be withdrawn from a solution because the solute particles are surrounded by shells of
solvent molecules. These shells interfere with the formation of the orderly pattern that the particles assume as
the solvent changes from liquid to solid. Vapor pressure lowering: The formation of solvent shells around the
solute particles reduces the number of solvent particles that have sufficient kinetic energy to vaporize.
PTS: 1
DIF: L3
REF: p. 534 | p. 535 | p. 536
OBJ: 16.3.1 Explain how colligative properties can be explained on a particle basis.
BLM: synthesis
160. ANS:
Molarity is a quantitative measure of the concentration of a solution. It is defined as the number of moles of
solute present in 1 L of solution. Molality is also a quantitative measure of the concentration of a solution. It
is defined as the number of moles of solute present in 1 kg of solvent. Molarity is a ratio of moles of solute to
1 L of solution. Molality is a ratio of moles of solute to 1kg of solvent.
Molarity:
; Molality:
PTS: 1
DIF: L2
REF: p. 525 | p. 538
OBJ: 16.2.1 Calculate the molarity of a solution. | 16.4.1 Identify the two ways of expressing the ratio of
solute to solvent in a solution.
BLM: analysis