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MULTIPLE CHOICE
Section 1.3 Elements and the Periodic Table
1. Which of the following elements has chemical properties similar to oxygen?
a) fluorine
b) hydrogen
c) nitrogen
d) sulfur
Section 1.4 Some Characteristics of the Elements
2. Which one of the following is a poor conductor of heat and electricity?
a) copper
b) fluorine
c) iron
d) lead
Section 1.6 Measuring Mass
3. Which of the following is the largest mass?
a) 1000 g
b) 1 x 10
kg
c) 1.0 x 10
cg
d) 1.00 x 10
Mg
Section 1.8 Derived Units: Measuring Volume
4. Which of the following is the smallest
a) 44 cm
b) 1.0 dL
c) 5.5 x 10 mL
d) 1 x 10 nL
volume?
Section 1.10 Accuracy, Precision, and Significant Figures in Measurement
5. How many significant figures are there in the answer to the following problem?
(8.881 x 2.100)
0.590 = ?
a) one
b) two
c) three
d) four
6. How many significant figures are there in the answer for the following problem?
(131.7 - 119) x 1.05
0.500
a)
b)
c)
d)
one
two
three
four
= ?
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Section 1.13 Properties of Matter: Density
7. Which of the following underlined items is not an extensive property?
a) The color of a cobalt compound.
b) The diameter of a soap bubble.
c) The mass of a diamond.
d) The volume of a glucose solution.
Sections 2.1 and 2.2 Atomic Theory
8. Methane and oxygen react to form carbon dioxide and water. What mass of water is
formed if 3.2 g of methane reacts with 12.8 g of oxygen to produce 8.8 g of carbon
dioxide?
a) 7.2 g
b) 8.8 g
c) 14.8 g
d) 16.0 g
9. Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of
sodium reacts with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide,
how much water was involved in the reaction?
a) 4.68 g
b) 5.98 g
c) 10.14 g
d) 10.56 g
Sections 2.3 - 2.6 Elements and Atoms
10. In
a)
b)
c)
d)
general, a stable atom has
more protons than neutrons or electrons
more neutrons than protons or electrons
more electrons than protons or neutrons
fewer neutrons than protons or electrons
Sections 2.7 and 2.8 Compounds and Mixtures, Molecules and Ions
11. A banana split is an example of
a) a compound.
b) an element.
c) a heterogeneous mixture.
d) a homogeneous mixture.
12. How many electrons are in the ion Zn
a) 28
b) 30
c) 32
d) 65
?
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13. The formula for a molecule of bromine is
a) Br
b) Br
c) Br
d) Br
Section 2.9 Acids and Bases
14. How many H
a) 1
b) 2
c) 3
d) 90
ions can the acid H CO
donate per molecule?
Section 2.10 Naming Compounds
15. What is the charge on the Cr in Cr O ?
a) 2b) 1+
c) 2+
d) 3+
16. What is the formula for strontium hydroxide?
a) SrH
b) SrOH
c) SrOH
d) Sr(OH)
17. The formula for dinitrogen trioxide is
a) N(OH)
b) (NO )
c) N O
d) N O
18. The sulfite ion is
a) S
b) S
c) SO
d) SO
19. The ions ClO , ClO , ClO , and ClO are named respectively
a) hypochlorate, chlorate, chlorite, perchlorite
b) hypochlorite, chlorite, chlorate, perchlorate
c) perchlorate, chlorate, chlorite, hypochlorite
d) perchlorite, chlorite, chlorate, hypochlorate
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Section 3.1 Balancing Chemical Equations
20. What is the sum of the coefficients when the following equation is balanced using
the lowest, whole numbered coefficients?
_____ B O (s) + _____ HF(l)
_____ BF (g) + _____ H O(l)
a) 8
b) 11
c) 15
d) none of these
Section 3.3 Avogadro's Number and the Mole
21. How many grams are there in 0.500 mol of dichlorodifluoromethane, CF Cl ?
a) 4.14 x 10
g
b) 60.5 g
c) 121 g
d) 242 g
22. What mass of sulfur hexafluoride, SF , has the same number of fluorine atoms as 25.0
g of oxygen difluoride, OF ?
a) 0.901 g
b) 8.33 g
c) 22.5 g
d) 203 g
23. Which of the following has the smallest
a) 3.50 x 10
molecules of I
b) 85.0 g of Cl
c) 2.50 mol of F
d) 0.050 kg of Br
mass?
Section 3.4 Stoichiometry: Chemical Arithmetic
24. How many moles of BF are needed to produce 25.0 g of HF(l) in the following
reaction?
BF (g) + 3 H O(l)
3 HF(l) + H BO (s)
a) 0.267 mol
b) 0.417 mol
c) 1.25 mol
d) 3.75 mol
25. When the following equation is balanced, how many grams of MgO are needed to produce
15.0 g of Fe O ?
_____ MgO(s) + _____ Fe(s)
____ Fe O (s) + _____ Mg(s)
a) 1.26 g
b) 3.78 g
c) 11.4 g
d) 178 g
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Section 3.5 Yields of Chemical Reactions
26. In the reaction between glucose and oxygen, 10.0 g of glucose reacts and 7.50 L of
carbon dioxide is formed. What is the percent yield if the density of CO is 1.26
g/L?
C H O (s) + 6 O (g)
6 CO (g) + 6 H O(l)
a) 26.1%
b) 40.6%
c) 43.1%
d) 64.7%
Section 3.9 Solution Stoichiometry
27. How many millilters of 0.200 M FeCl are needed to react with an excess of Na S if
the percent yield is 65.0% and 2.75 g of Fe S is produced?
3 Na S(aq) + 2 FeCl (aq)
Fe S (s) + 6 NaCl(aq)
a) 50.9 mL
b) 86.0 mL
c) 102 mL
d) 203 mL
Section 3.10 Titration
28. How many milliliters of 0.550 M hydroiodic acid are needed to react with 25.00 mL of
0.217 M CsOH?
HI(aq) + CsOH(aq) CsI(aq) + H O(l)
a) 0.209 mL
b) 4.77 mL
c) 9.86 mL
d) 101 mL
Section 3.11 Percent Composition and Empirical Formulas
29. Which of the following statements is false concerning the formula of a compound?
a) The empirical formula is the simplest whole numbered ratio of atoms in a
compound.
b) The molecular formula is the true ratio of atoms in a compound.
c) The molecular formula and empirical formula can be identical.
d) The number of atoms in a molecular formula is always greater than the number of
atoms in an empirical formula.
30. What is the empirical formula for perfluoropropane if the compound contains 81%
fluorine and 19% carbon by mass?
a) CF
b) C F
c) C F
d) C F
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Section 4.1 Some Ways that Chemical Reactions Occur
31. The reaction of Na PO (aq) + 3 AgNO (aq)
classified as a(n)
a) acid-base neutralization reaction
b) oxidation-reduction reaction
c) precipitation reaction
d) single replacement reaction
Ag PO (s) + 3 NaNO (aq) is best
Section 4.4 Precipitation Reactions and Solubility Rules
32. Write a balanced net ionic equation for the reaction of AgNO (aq) with Cu(s).
a) AgNO (aq) + Cu(s)
Ag(s) + CuNO (aq)
b) Ag (aq) + Cu(s)
Ag(s) + Cu (aq)
c) 2 AgNO (aq) + Cu(s)
2 Ag(s) + CuNO (aq)
d) 2Ag (aq) + Cu(s)
2 Ag(s) + Cu (aq)
Section 4.7 Identifying Redox Reactions
33. What is the oxidizing agent in the reaction
5 Fe (aq) + MnO (aq) + 8 H (aq)
Mn (aq) + 5 Fe
a) Fe
b) H
c) Mn
d) MnO
(aq) + 4 H O(l)?
Section 4.8 The Activity Series of the Elements
34. Using the following portion of the activity series for oxidation half reactions
Na(s)
Na+(aq) + e
Cr(s)
Cr (aq) + 3e
determine which reaction will occur.
a) Na(s) with Cr(s)
b) Na(s) with Cr (aq)
c) Na (aq) with Cr (aq)
d) Na (s) with Cr(s)
Section 4.11 Redox Titrations
35. According to the balanced chemical equation
5 H C O (aq) + 2 MnO (aq) + 6 H (aq)
10 CO (g) + 2 Mn (aq) + 8 H O(l)
one mole of oxalic acid, H C O , is equivalent to ____ moles of permanganate, MnO
a)
b)
c)
d)
1
2
2/5
5/2
.
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Sections 5.2-5.4 Electromagnetic Radiation and Spectra
36. What is the frequency of a helium-neon laser light with a wavelength of 632.8 nm?
The speed of light is 3.00 x 10 m/s.
a) 4.74 x 10
s
b) 4.74 x 10 s
c) 2.11 x 10
s
d) 1.58 x 10
s
m is necessary for a CO
37. The absorption of a photon of wavelength 4.67 x 10
molecule to pass from the lowest vibrational energy level to the next highest
vibrational level. If this higher vibrational level has an energy of 6.41 x 10
what is the energy of the lowest vibrational level?
h = 6.626 x 10
J s
a) 1.60 x 10
J
b) 2.15 x 10
J
c) 3.20 x 10
J
d) 4.26 x 10
J
J,
Section 5.5 Wavelike Properties of Matter
times that of a copper atom. Compare the de
38. An old copper penny has a mass 3 x 10
Broglie wavelength of a penny moving at 0.5 m/s to that of a copper atom moving 10
times as fast. The wavelength for the
a) copper atom is 3 x 10
times that of the penny.
b) copper atom is 3 x 10
times that of the penny.
c) penny is 3 x 10
times that of the copper atom.
d) penny is 3 x 10
times that of the copper atom.
Section 5.6 The Quantum Mechanical Description of the Hydrogen Atom
39. Which of the following is true?
a) The Bohr atom is the model currently accepted for electrons in atoms.
b) Electrons travel around the nucleus in circular orbits.
c) There is a 5% chance of finding an electron in an atom outside its orbital.
d) The square of the wave function gives the probability of finding the electron.
Section 5.7 Wave Functions and Quantum Numbers
40. Which of the following is not a valid set of quantum numbers?
a) n = 2, l = 1, m l = 0, and m s = -1/2
b) n = 2, l = 1, m l = -1, and m s = -1/2
c) n = 3, l = 0, m l = 0, and m s = 1/2
d) n = 3, l = 2, m l = 3, and m s = 1/2
41. How many h orbitals are allowed in a given shell?
a) 5
b) 6
c) 11
d) 13
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42. What is the maximum number of orbitals in the seventh shell?
a) 4
b) 15
c) 49
d) 98
Section 5.8 Atomic Spectra Revisited
43. What is the first ionization energy for a hydrogen atom in the ground state?
Rydberg constant is 1.097 x 10
nm .
a) 7.27 x 10
J
b) 1.63 x 10
J
c) 2.18 x 10
J
d) 0.00823 J
The
Section 5.9 Orbital Shapes
44. What is the number of spherical nodes in a 4s orbital?
a) zero
b) two
c) three
d) four
Sections 5.11 - 5.13 Electron Configurations of Multielectron Atoms
45. Which of the following orbital-filling diagrams could represent the ground state of
vanadium?
4s
3d
(A) [Ar]
(B) [Ar]
(C) [Ar]
(D) [Ar]
(E) [Ar]
a)
b)
c)
d)
all but (B)
all but (A) and (B)
(D) and (E)
only (D)
Section 6.1 Ionization Energy
46. Which element has the highest first ionization energy?
a) Ca
b) K
c) Li
d) Mg
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Section 6.3 Electron Affinity
47. What chemical process would liberate the most energy?
a) O(g) + e
O (g)
b) O (g) + e
O (g)
c) O (g) + e
O (g)
d) O(g)
O (g) + e
Section 6.4 Ionic Bonds and Formation of Ionic Solids - Lattice Energy
48. Which of the following pictures best represents an ionic compound with a very high
lattice energy?
a) A
b) B
c) C
d) D
49. In the reaction of sodium metal with chlorine gas which of the following processes
releases energy?
a) Cl (g)
2 Cl(g)
b) Cl(g) + e
Cl (g)
c) Na(s)
Na(g)
d) Na(g)
Na (g) + e
50. Calculate the energy change for the formation of MgBr (s) from its elements in their
standard states
Mg(s) + Br (l)
MgBr (s)
?
Mg(s)
Mg(g)
+147.1 kJ/mol
Mg(g)
Mg (g) + e
+737.8 kJ/mol
Mg (g)
Mg (g) + e
+1451 kJ/mol
Br (l)
Br (g)
+30.9 kJ/mol
1/2 Br (g)
Br(g)
+112.0 kJ/mol
Br(g) + e
Br (g)
-325.0 kJ/mol
MgBr (s)
Mg (g) + 2Br (g)
+2440 kJ/mol
a) -150.8 kJ/mol
b) -286.0 kJ/mol
c) -499.2 kJ/mol
d) -5682 kJ/mol
Page 10
Section 6.6 The Alkaline-Earth Metals (Group 2A)
51. What is not generally considered to be a chemical reaction of the alkaline earth
metal calcium?
a) Ca(s) + Cl (g)
CaCl (s)
b) 2 Ca(s) + 2 H O(l)
2 Ca(OH) (aq) + H (g)
c) 6 Ca(s) + 2 N (g)
2 Ca N (s)
d) Ca(s) + O (g)
CaO (s)
52. Calcium, strontium, and barium are all prepared commercially by the same method
which is
a) electrolysis of the molten metal oxides.
b) electrolysis of the molten metal halides.
c) chemical reduction of the metal oxides with aluminium.
d) chemical reduction of the metal halides with oxygen.
Section 6.9 The Noble Gases (Group 8A)
53. Group 8A elements He, Ne, Ar, Kr, Xe, and Rn are consistent with the following
a) gases, diamagnetic, ns np outer electron configuration, all display octet of
electrons except helium
b) gases, diamagnetic, ns np outer electron configuration, all display octet of
electrons except radon
c) gases, paramagnetic, ns np outer electron configuration, all display octet of
electrons except helium
d) gases, paramagnetic, ns np outer electron configuration, all display octet of
electrons
Section 6.10 The Octet Rule
54. How many electrons does barium
a) barium loses 2 and nitrogen
b) barium loses 2 and nitrogen
c) barium loses 3 and nitrogen
d) barium loses 3 and nitrogen
lose and nitrogen need to form Ba N ?
gains 2
gains 3
gains 2
gains 3
Sections 7.5-7.7 Electron-Dot Structures
55. How many lone pairs of electrons are on the P atom in PF ?
a) 0
b) 1
c) 2
d) 3
Section 7.9 Molecular Shapes: The VSEPR Model
56. What is the shape of IF ?
a) octahedral
b) see-saw
c) square pyramidal
d) trigonal bipyramidal
Page 11
Section 7.11-12 Hybrid orbitals
57. Which type of bond produces a charge cloud with a nodal plane containing the bond
axis?
a)
b)
c)
and
d) neither
nor
Section 8.8 Calorimetry and Heat Capacity
58. Water has an unusually high
a) heat of combustion.
b) heat of formation.
c) molar heat capacity.
d) specific heat.
Section 8.9 Hess's Law
SO (g)
H = - 296.1 kJ
59. Given: S(s) + O (g)
2 SO (g)
2 SO (g) + O (g)
H = 198.2 kJ
Find H for : 2 S(s) + 3 O (g)
2 SO (g)
a) -790.4 kJ
b) -394.0 kJ
c) -97.9 kJ
d) +97.9 kJ
Section 8.10 Standard Heats of Formation
60.
For which should the standard heat of formation,
H , be zero at
f
25 C?
a) O(g)
b) O (g)
c) O (g)
d) all the above
Section 8.12 Fuel Efficiency and Heat of Combustion
61. The heat of combustion per mole for acetylene, C H (g), is -1299.5 kJ/mol. Assuming
that the combustion products are CO (g) and H O(l), and given that the enthalpy of
formation is -393.5 kJ/mol for CO (g) and -285.8 kJ/mol for H O(l), find the
enthalpy of formation of C H (g).
a) -846.1 kJ/mol
b) -620.2 kJ/mol
c) -226.7 kJ/mol
d) +226.7 kJ/mol
Page 12
Section 8.13 An Introduction to Entropy
62. Determine the sign of S for
I. C H (s)
C H (l)
II. 2 SO (g) + O (g)
a) S should be negative for
b) S should be negative for
c) S should be positive for
d) S should be positive for
each of the following processes:
I
I
I
I
2 SO
and
and
and
and
(g)
negative
positive
negative
positive
for
for
for
for
II.
II.
II.
II.
Section 8.14 An Introduction to Free Energy
63. Methanol can be produced from carbon monoxide and hydrogen with suitable catalysts:
CO(g) + 2 H (g)
CH OH(l) at 25 C H = -128.1 kJ and S = -332 J/K.
Find G at 25 C.
a) -157.2 kJ
b) -29.1 kJ
c) 98.9 kJ
d) 157.2 kJ
Section 9.2 The Gas Laws
64. A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure. If the final pressure
is 1.15 atm, how many moles of gas were added to the bottle?
a) 0.128 mol
b) 0.630 mol
c) 1.19 mol
d) 1.28 mol
Section 9.3 The Ideal Gas Law
65. What is the volume of 10.0 g of argon gas at 157 C and 2.50 kPa pressure?
a) 1.29 L
b) 3.53 L
c) 131 L
d) 358 L
Section 9.4 Stoichiometric Relationships with Gases
66. How many grams of XeF are required to react with 0.579 L of hydrogen gas at 2.46
atm and 45 C?
XeF (s) + 3 H (g)
Xe(g) + 6 HF(g)
a) 3.73 g
b) 4.46 g
c) 12.8 g
d) 40.2 g
Page 13
Section 9.5 Partial Pressure and Dalton's Law
67. A 0.500 g sample containing Ag O and inert material is heated, causing the silver
oxide to decompose according to the following equation:
2 Ag O(s)
4 Ag(s) + O (g)
If 13.8 mL of gas are collected over water at 27 C and 1.00 atm external pressure,
what is the percentage of silver oxide in the sample? The partial pressure of water
is 26.7 mm Hg at 27 C.
a) 12.5%
b) 25.1%
c) 50.2%
d) 53.8%
Section 9.6 The Kinetic-Molecular Theory
68. Which of the following gases has the highest
a) CO
b) N O
c) SF
d) UF
average speed at 400K?
Section 9.7 Graham's Law: Diffusion and Effusion of Gases
69. Which one of the following gases will have the lowest
a) SF
b) SCl
c) S O
d) SO
rate of effusion?
Section 9.8 The Behavior of Real Gases
70. Which statement about real gases is TRUE?
a) The volume of the gas particles is zero.
b) The mass of the gas particles is zero.
c) Forces of attraction and repulsion exist between gas particles at close range.
d) The behavior of real gases can be exactly predicted using the ideal gas law.
Section 9.9 The Earth's Atmosphere
71. The principal cause of man-made ozone depletion in the stratosphere is due to
a) NO
b) CH
c) CO
d) Cl
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Section 10.1 Polar Covalent Bonds and Dipole Moments
72. The dipole moment of BrF is 1.29 D, and its bond length is 178 pm. What is the
percent ionic character of the Br-F bond?
a) 3.9%
b) 8.5%
c) 15%
d) 33%
Section 10.2 Intermolecular Forces
73. Which substance in each of the following pairs is expected to have the larger
dispersion forces?
I
Br
or I
H
I H
H
H
H
H
C
C
C
C
H
H H H
n-butane
H
or
H
H
H
C
H
H
C
C
C
H
H H H
isobutane
a)
b)
c)
d)
Br in set I and n-butane in set II
Br in set I and isobutane in set II
I in set I and n-butane in set II
I in set I and isobutane in set II
Section 10.4 Phase Changes
74. Bromine is one of only two elements that is a liquid at room temperature. Bromine
has a heat of vaporization of 30.91 kJ/mol and its boiling point is 59 C. What is
the entropy of vaporization for bromine?
a) -301 J/(mol K)
b) -93.1 J/(mol K)
c) 10.7 J/(mol K)
d) 93.1 J/(mol K)
75. How much heat is released when 75.0 g of steam at 100.0 C is cooled to ice at -15.0 C
? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for
water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol C),
and the molar heat capacity of ice is 36.4 J/(mol C).
a) 54.76 kJ
b) 158.5 kJ
c) 228.2 kJ
d) 652.6 kJ
Page 15
Section 10.5 Evaporation, Vapor Pressure, and Boiling Point
76. Hydroquinone is an antioxidant that is also used as a photographic reducer and
developer. The normal boiling point of hydroquinone is 310 C. Calculate the pressure
at which hydroquinone will boil at 200 C given that its H v a p is 73.38 kJ/mol.
a) 1.210 x 10
mm Hg
b) 1.35 mm Hg
c) 22.5 mm Hg
d) 757 mm Hg
77. From the plot of vapor pressure (in mm Hg) as a function of temperature shown below,
in the range 0 C to 100 C, the vapor pressure of t-butanol approximately doubles
every
a) 5 C.
b) 10 C.
c) 20 C.
d) 40 C.
Section 10.6 Kinds of Solids
78. Which of the following forms an ionic solid?
a) Ag
b) C H NH
c) RbI
d) SO
Page 16
Section 10.9 Packing of Spheres and the Structures of Metals
79. How many unit cells share an atom that is on the face of a cubic unit cell?
a) 1
b) 2
c) 4
d) 8
80. Iron crystallizes in a body-centered cubic cell having an edge length of 287 pm.
What is the density of iron in g/cm .
a) 1.99
b) 7.85
c) 11.9
d) 15.9
81. An element forms a body-centered cubic crystalline substance. The edge length of the
unit cell is 287 pm and the density of the crystal is 7.92 g/cm . Calculate the
atomic weight of the substance.
a) 45.0 amu
b) 48.0 amu
c) 56.4 amu
d) 63.5 amu
Page 17
Section 10.12 Phase Diagrams
82. Melting occurs along the
a) AC line.
b) CB line.
c) CD line.
d) all of the above.
Page 18
83. According to the diagram, the solid phase of this substance
a) has the same density as the liquid phase.
b) is less dense than water.
c) is less dense than the liquid phase.
d) is more dense than the liquid phase.
Page 19
84. The normal boiling point of this substance is approximately
a) 25 C.
b) 140 C.
c) 300 C.
d) 350 C.
Page 20
85. From the phase diagram above, the minimum pressure at which this substance can exist
in the liquid phase is
a) 0.25 atm.
b) 0.50 atm.
c) 1.0 atm.
d) 1.2 atm.
Section 11.1 Solutions
86. The rubbing alcohol sold in drug stores often is composed of 70% isopropyl alcohol
and 30% water. In this solution
a) isopropyl alcohol is the solvent.
b) water is the solvent.
c) both water and isopropyl alcohol are solvents.
d) neither water nor isopropyl alcohol is a solvent.
Section 11.2 Energy Changes and the Solution Process
87. When a particular solid begins to dissolve in water, the temperature rises
dramatically. For the dissolving of this solid in pure water
a) H s o l n is always negative and S s o l n may be negative or positive.
b) H s o l n is always negative and S s o l n is always positive.
c) H s o l n is always positive and S s o l n may be negative or positive.
d) H s o l n is always positive and S s o l n is always positive.
Page 21
88. In the process of dissolving ionic compounds, the cations and anions are separated
from the crystal lattice and surrounded by an ordered shell of solvent molecules. If
the solvent is water, the dissolved ions are said to be
a) halogenated.
b) homogenized.
c) hybridized.
d) hydrated.
89. Although there are exceptions, which is most likely
of a solid in a liquid?
a) H s o l n is positive
b) H s o l n is negative
c) S s o l n is positive
d) S s o l n is negative
to be true for the dissolving
90. When two similar liquids mix to form a solution, the entropy of solution ( S s o l n ) is
expected to be
a) negative.
b) zero.
c) positive.
d) negative at low temperatures but positive at high temperatures.
91. The change in the Gibbs free energy for dissolving more solute in a supersaturated
solution is
a) negative.
b) zero.
c) positive.
d) positive at low temperatures and negative at high temperatures.
92. Which should be least
a) H
soluble in water?
H
H
H
H
C
C
C
C
H
H
H
H
O
H
formic acid
O
H
methanol
H
methylamine
H
butane
H
b) O
C
H
c) H
C
H
d) H
H
H
N
C
H
Page 22
Section 11.3 Units of Concentration
93. A solution is prepared by dissolving 17.75 g sulfuric acid, H SO , in enough water
to make 100.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is
the mole fraction H SO in the solution?
a) 0.0181
b) 0.0338
c) 0.0350
d) 19.0
94. What is the weight percent of a caffeine solution made by dissolving 4.35 g of
caffeine, C H N O , in 75 g of benzene, C H ?
a) 0.055%
b) 0.058%
c) 5.5%
d) 5.8%
95. How much water must be added to 42.0 g of CaCl
wt% CaCl ?
a) 56.7 g H O
b) 78.0 g H O
c) 83.3 g H O
d) 120 g H O
96. To
a)
b)
c)
d)
to produce a solution that is 35.0
make a 2.00 m solution, one could take 2.00 moles of solute and add
1.00 L of solvent.
1.00 kg of solvent.
enough solvent to make 1.00 L of solution.
enough solvent to make 1.00 kg of solution.
97. How many grams of KBr are required to make 650. mL of a 0.115 M KBr solution?
a) 5.65 g
b) 7.48 g
c) 8.89 g
d) 74.8 g
98. A 2.00 M solution of CaCl
fraction of CaCl ?
a) 0.0348
b) 0.0360
c) 0.0366
d) 0.0380
in water has a density of 1.17 g/mL. What is the mole
99. A solution of LiCl in water has X L i C l = 0.0500. What is the molality?
a) 2.12 m LiCl
b) 2.60 m LiCl
c) 2.92 m LiCl
d) 5.26 m LiCl
100. Which concentration varies with temperature?
a) molality
b) molarity
c) mole fraction
d) wt %
Page 23
Section 11.4 Some Factors Affecting Solubility
101. Which of the following does not affect the solubility of a solute in a given
solvent?
a) polarity of the solute
b) polarity of the solvent
c) rate of stirring
d) temperature of the solvent and solute
Section 11.6 Vapor Pressure Lowering of Solutions: Raoult's Law
102. At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and
59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of
benzene and toluene with X b e n z e n e = 0.600.
a) 108 mm Hg
b) 121 mm Hg
c) 133 mm Hg
d) 242 mm Hg
Section 11.7 Boiling Point Elevation, Freezing Point
Depression
103. What is the freezing point of a solution of 1.43 g MgCl
K f = 1.86 C/m for water.
a) -0.028 C
b) -0.28 C
c) -0.56 C
d) -0.84 C
in 100. g of water?
Section 11.8 Osmosis and Osmotic Pressure
104. A solution is made by dissolving 13 g of sucrose, C 2H O , in 117 g of water,
producing a solution with a volume of 125 mL at 20 C. What is the expected osmotic
pressure at 20 C?
a) 7.3 atm
b) 10 atm
c) 14 atm
d) 58 atm
Section 12.2 Rate Laws and Reaction Order
105. Cerium(IV) ion reacts with thallium(I) ion in a one step reaction shown below:
2 Ce (aq) + Tl (aq)
2 Ce (aq) + Tl (aq).
If the rate law is: Rate = k[Ce ] [Tl ], what is the overall order of the reaction?
a) first
b) second
c) third
d) fourth
Page 24
Section 12.3 Experimental Determination of a Rate Law
106. The following set of data was obtained by the method of initial rates for the
reaction:
2 HgCl (aq) + C O
(aq)
2 Cl (aq) + 2 CO (g) + Hg Cl (s)
What is the rate law for the reaction?
a)
b)
c)
d)
[HgCl ],M
[C O
0.10
0.10
1.3 x 10
0.10
0.20
5.2 x 10
0.20
0.20
1.0 x 10
Rate
Rate
Rate
Rate
=
=
=
=
k[HgCl
k[HgCl
k[HgCl
k[HgCl
][C O
][C O
] [C O
][C O
], M
Rate, M/s
]
]
]
]
107. The following set of data was obtained by the method of initial rates for the
reaction:
2 HgCl (aq) + C O
(aq)
2 Cl (aq) + 2 CO (g) + Hg Cl (s)
What is the value of the rate constant, k?
a)
b)
c)
d)
1.4
1.3
1.4
1.3
[HgCl ],M
[C O
0.10
0.10
1.3 x 10
0.10
0.20
5.2 x 10
0.20
0.20
1.0 x 10
x
x
x
x
10
10
10
10
], M
Rate, M/s
M/s
M/s
M/s
M/s
108. The following set of data was obtained by the method of initial rates for the
reaction:
(H C) CBr + OH
(H C) COH + Br
What is the value of the rate constant, k?
[(H C) CBr],
M
a)
b)
c)
d)
[OH ],
M
Initial Rate,
M/s
0.25
0.25
1.1 x 10
0.50
0.25
2.2 x 10
0.50
0.50
2.2 x 10
8.8 x 10
M/s
4.4 x 10
M/s
1.8 x 10
M/s
none of these
Page 25
109. The following set of data was obtained by the method of initial rates for the
reaction:
BrO (aq) + 5 Br (aq) + 6 H (aq)
3 Br (aq) + 3 H O(l).
Calculate the initial rate when BrO
is 0.30 M, Br is 0.050 M, and H is 0.15 M.
Expt
a)
b)
c)
d)
[BrO
],M
[Br ],M
[H ],M
Rate, M/s
1
0.10
0.10
0.10
8.0 x 10
2
0.20
0.10
0.10
1.6 x 10
3
0.20
0.15
0.10
2.4 x 10
4
0.10
0.10
0.25
5.0 x 10
6.1
2.7
5.3
8.4
x
x
x
x
10
10
10
10
M/s
M/s
M/s
M/s
Section 12.4 Integrated Rate Law for a First-Order Reaction
SO + Cl , has a rate constant equal to 2.20 x
110. The first-order reaction, SO Cl
10
s
at 593 K. What percent of SO Cl will remain after 2.00 hours?
a) 1.00%
b) 14.7%
c) 17.1%
d) 85.4%
Section 12.5 Half-Life of a First-Order Reaction
111. The rate constant, k, for a first-order reaction is equal to 4.2 x 10
the half-life of the reaction?
a) 2.9 x 10
s
b) 1.5 s
c) 7.2 x 10 s
d) 1.7 x 10 s
s
. What is
Section 12.6 Second-Order Reactions
2 NO(g) + O (g).
112. The decomposition of nitrogen dioxide is second order: 2 NO (g)
If the half-life at 300 C is 11 seconds and the rate constant is 0.54 M
s , how
many moles of NO were in the 2.50 L container at the start of the reaction?
a) 0.17 mol
b) 0.42 mol
c) 5.9 mol
d) 15 mol
113. Which statement below regarding the half-life of a second-order reaction is true ?
a) Each half-life is half as long as the preceding one.
b) Each half-life is twice as long as the preceding one.
c) Each half-life is four times as long as the preceding one.
d) The length of the half-life remains unchanged throughout the course of the
reaction.
Page 26
Section 12.7 Reaction Mechanisms
114. The decomposition of ozone in the stratosphere can occur by the following two-step
mechanism:
Step 1: Br + O
BrO + O
Step 2: BrO + O
Br + O
Which species is an intermediate in this mechanism?
a) Br
b) BrO
c) O
d) O
Section 12.8 Rate Laws and Reaction Mechanisms
115. The slowest step in a reaction mechanism is called the _________ step.
a) activation
b) elementary
c) rate law
d) rate-determining
116. Which of the following statements are true about reaction mechanisms?
I.
A rate law can be written from the molecularity of the slowest elementary step.
II. The final rate law can include intermediates.
III. The rate of the reaction is dependent on the fastest step in the
mechanism.
IV. A mechanism can never be proven to be the correct pathway for a
reaction.
a) I, II, III
b) II, IV
c) I, III
d) I, IV
117. A three step mechanism has been suggested for the formation of carbonyl chloride:
Step 1: Cl
2 Cl (fast, equilibrium)
Step 2: Cl + CO
COCl (fast, equilibrium)
Step 3: COCl + Cl
COCl + Cl (slow)
What is the molecularity of the rate-determining step?
a) unimolecular
b) bimolecular
c) termolecular
d) none of these
Section 12.9 Reactions Rates and Temperature: The Arrhenius Equation
118. What is the mininum energy barrier that must be overcome for a chemical reaction to
occur?
a) activation energy
b) net energy
c) potential energy
d) rate limiting energy
Page 27
119. What factor affects the rate of a chemical reaction?
a) collision frequency
b) fraction of collisions with sufficient energy
c) orientation of molecules
d) all of the above
120. What fraction of collisions will have sufficient energy to react for a gas whose
activation energy is 68 kJ/mol at 25 C?
a) 1.2 x 10
b) 2.7 x 10
c) 0.96
d) 8.3 x 10
Section 12.10 Using the Arrhenius Equation
121. The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place
according to the equation:
Fe(phen)
+ 3 H O + 3 H O
Fe(H O)
+ 3 phenH
If the activation energy, E a , is 126 kJ/mol and the rate constant at 30 C is 9.8 x
10
min , what is the rate constant at 50 C?
a) 4.4 x 10
min
b) 2.2 x 10
min
c) 3.4 x 10 min
d) 2.3 x 10 min
Section 13.1 The Equilibrium State
122. Which one of the following statements does not describe the equilibrium state?
a) Equilibrium is dynamic and there is no net conversion to reactants and products.
b) The concentration of the reactants is equal to the concentration of the products.
c) The concentration of the reactants and products reach a constant level.
d) The rate of the forward reaction is equal to the rate of the reverse reaction.
Section 13.2 The Equilibrium Constant K
c
123. Write the equilibrium equation for the forward
2 CH (g) + 3 O (g)
2 CO(g) + 4 H O(g)
a) K c =
b) K c =
c) K c =
d) K c =
2 CO
+ 4 H O
2 CH
+ 3 O
2 CO
+ 3 O
2 CO
+ 4 H O
CO
H O
CH
H O
CH
O
CO
H O
reaction:
Page 28
124. Nitric oxide reacts with oxygen to form nitrogen dioxide:
2 NO(g) + O (g)
2 NO (g)
What is K c ' for the reverse reaction if the equilibrium concentration of NO is 0.300
M, O is 0.200 M, and NO is 0.530 M at 25 C?
a) 0.0340
b) 0.0641
c) 0.624
d) 15.6
2 NO (g), K c = 8.3 x 10
at 25 C. What is the
125. For the reaction: N (g) + 2 O (g)
concentration of N gas at equilibrium when the concentration of NO is twice the
concentration of O gas?
a) 2.08 x 10
M
b) 4.15 x 10
M
c) 2.4 x 10 M
d) 4.8 x 10 M
Section 13.3 The Equilibrium Constant K
p
126. A 1.50 L vessel contains an equilibrium mixture of 0.100 mol of NO, 0.150 mol of Br ,
and 0.250 mol of NOBr at 25 C. What is the value of K p for the reaction below?
2 NO(g) + Br (g)
2 NOBr(g)?
a) 2.56
b) 62.5
c) 1.28 x 10
d) 1.53 x 10
Section 13.4 Heterogeneous Equilibria
127. What is the equilibrium equation for the dissociation of formic acid in water?
HCOOH(aq) + H O(l)
H O (aq) + HCOO (aq)
a) K c =
b) K c =
c) K c =
d) K c =
H O
HCOO
HCOOH
H O
HCOOH
H O
H O
HCOO
H O
HCOO
HCOOH
HCOOH
H O
HCOO
Page 29
Section 13.5 Using the Equilibrium Constant
128. Cyclohexane (CH) undergoes a molecular rearrangement in the presence of AlCl to
form methylcyclopentane (MCP) according to the equation: CH
MCP. If K c = 0.143 at
25 C for this reaction, predict the direction the reaction will shift if the initial
concentrations of CH and MCP are 0.200 M and 0.100 M, respectively.
a) The reaction will shift left.
b) The reaction will shift right.
c) The reaction is already at equilibrium.
d) The reaction is at equilibrium but will then shift left.
129. Cyclohexane (CH) undergoes a molecular rearrangement in the presence of AlCl to
form methylcyclopentane (MCP) according to the equation: CH
MCP. If K c = 0.143 at
25 C for this reaction, find the equilibrium concentrations of CH and MCP if the
initial concentrations are 0.200 M and 0.100 M respectively.
a) [CH] = 0.0625 and [MCP] = 0.0625 M
b) [CH] = 0.138 and [MCP] = 0.162 M
c) [CH] = 0.262 M and [MCP] = 0.0375 M
d) [CH] = 0.283 and [MCP] = 0.0167 M
2 HI(g). Initially
130. K p is equal to 48.70 at 731 K for the reaction: H (g) + I (g)
the mixture contains 0.08592 atm each of H and I and 1.0000 atm of HI. What is the
pressure of HI at equilibrium?
a) 0.7955 atm
b) 0.9108 atm
c) 0.9140 atm
d) 0.9498 atm
131. Ammonium carbamate can dissociate into gases at 25 C according to the reaction:
NH COONH (s)
2 NH (g) + CO (g)
If sufficient ammonium carbamate is sealed in a flask, the total pressure will be
0.117 atm at equilibrium. What is the value of K p at 25 C?
a) 2.37 x 10
b) 2.00 x 10
c) 1.60 x 10
d) 3.42 x 10
132. Which of the following changes in reaction conditions will not alter the equilibrium
concentrations?
a) Addition of an inert gas to the reaction mixture.
b) Addition of reactants or products.
c) Decreasing the pressure or volume.
d) Increasing the temperature.
Sections 13.7-9 Altering an Equilibrium Mixture:
Changes in Concentration, Pressure, Volume, and
Temperature
133. Iron oxide ores are reduced to iron metal by exothermic reaction with carbon
monoxide: FeO(s) + CO(g)
Fe(s) + CO (g). Which of the following changes in
condition will cause the equilibrium to shift to the right?
a) Add FeO.
b) Add CO.
c) Add CO .
d) Raise the temperature.
Page 30
134. Calcium carbonate is relatively insoluble and the dissolution reaction is
endothermic: CaCO (s)
Ca (aq) + CO
(aq). Which change in reaction condition
below will shift the equilibrium to the right?
a) Add an acid to react with CO
ion.
b) Add an anion with which Ca
is even more soluble than calcium carbonate.
c) Increase the temperature.
d) All of the above will shift reaction to the right.
Section 13.11 The Link Between Chamical Equilibrium and Chemical
Kinetics
s
135. At 25 C, a certain first order reaction has a rate constant equal to 1.00 x 10
and an equilibrium constant, K c , equal to 4.18. What is the rate constant for the
reverse reaction?
a) 2.39 x 10
s
b) 4.18 x 10
s
c) 2.39 x 10 s
d) 4.18 x 10 s
136. The reaction below virtually goes to completion because cyanide ion forms very
stable complexes with Ni
ion:
[Ni(H O) ] (aq) + 4 CN (aq)
[Ni(CN) ] (aq) + 6 H O(l)
At the same time, incorporation of
C labelled cyanide ion ( CN ) is very rapid:
[Ni(CN) ] (aq) + 4
CN (aq) = [Ni( CN) ] (aq) + 4 CN (aq)
Which statement below is correct with regard to stability and rate of reaction?
a) Equilibrium is static.
b) Stable species can react rapidly.
c) Stable species do not react rapidly.
d) Unstable species react rapidly.
14.1 - 14.3 Hydrogen, Isotopes of Hydrogen, Synthesis of Hydrogen
137. Which is not an isotope of hydrogen?
a) hydrogen-1
b) hydrogen-2
c) hydrogen-3
d) hydrogen-4
138. If the molar mass of monoatomic deuterium (D) is 2.0141 grams then what is the
density of diatomic deuterium (D ) gas at 25.0 C and 1.00 atmosphere pressure?
a) 0.082 g/L
b) 0.165 g/L
c) 0.329 g/L
d) 12.2 g/L
139. Which individual is generally given credit for the discovery of hydrogen gas?
a) Cavendish
b) Davy
c) Lavoisier
d) Priestley
Page 31
14.5 Binary Hydrides
140. What is the Lewis electron dot structure for the hydride ion?
a) H
b) H:
c) H
d) H O
14.6 - 14.9 Oxygen, Preparation and Uses of Oxygen, Properties of
Oxygen, Oxides
141. How many mL of O gas at 25.0 C and 755 mmHg pressure can be obtained by thermal
decomposition of 0.300 grams of KClO ? The equation of interest is
2 KClO (s)
> 2 KCl(s) + 3 O (g).
a) 30.1 mL
b) 45.1 mL
c) 82.3 mL
d) 90.4 mL
142. How many grams of KCl are produced by the thermal decomposition of KClO that
produces 25.0 mL of O at 25.0 C and 1 atm pressure? The equation of interest is
2 KClO (s)
> 2 KCl(s) + 3 O (g).
a) 0.0508 g
b) 0.0762 g
c) 0.0835 g
d) 0.125 g
143. How many liters of oxygen at STP can be produced from the decomposition of 0.500 L
of 3.00 M H O if the equation of interest is
2 H O (l)
> 2 H O(l) + O (g)?
a) 16.8 L
b) 22.4 L
c) 33.6 L
d) 67.2 L
14.10 Peroxides and Superoxides
144. Indicate the trend in increasing bond length for molecular oxygen, the peroxide ion,
and superoxide ion.
a) O > O
> O
b) O > O
> O
c) O
> O
> O
d) O
> O > O
14.11 Hydrogen Peroxide
O,
O,
O and the major isotope of
145. Using the three different isotopes of oxygen
hydrogen, H. Determine the number of different types of isotopically substituted
hydrogen peroxide, H O , that could be formed.
a) 3
b) 5
c) 6
d) 9
Page 32
14.14 Hydrates
146. Which compound is not considered to be a hydrate?
a) [Mg(H O) ](ClO )
b) [Al(H O) ]Cl
c) CuSO H O
d) HOClO
147. When 3.00 grams of the anhydrous blue colored CoCl is exposed to moist air it forms
5.50 grams of the red-violet CoCl xH O hydrate. Determine the number of moles of
water that combine with one mole of CoCl .
a) 4
b) 6
c) 8
d) 10
14.15 Natural Waters
148. What are the
a) Cl , Na ,
b) Cl , Na ,
c) Cl , Na ,
d) Na , SO
four major ionic constituents of seawater?
Mg , HCO
SO
, Mg
SO
, HCO
, Mg , Ca
Section 15.1 Acid-Base Concepts: The Br
nsted-Lowry Theory
149. Which one of the following species acts as an acid in water?
a) NaH
b) NH
c) CH NH
d) C H
150. What are the Br nsted-Lowry acids in the following chemical reaction
HBr(sol) + CH CO0H(sol)
CH C(OH) (sol) + Br (sol)?
a) HBr, CH COOH
b) HBr, CH C(OH)
c) CH COOH, CH C(OH)
d) CH COOH, Br
151. Which one of the following can behave either as a Br nsted-Lowry acid or a Br nsted-L
owry base in an aqueous solution reaction?
a) HSO
b) NH
c) HI
d) H PO
Page 33
Section 15.2 Acid Strength and Base Strength
152. From the following chemical reactions determine the relative Br nsted-Lowry acid
strengths (strongest to weakest).
HCl(aq) + H O(l)
H O (aq) + Cl (aq)
HCN(aq) + H O(l)
H O (aq) + CN (aq)
a) HCl > HCN > H O
b) HCl > H O > HCN
c) H O > HCl > HCN
d) HCN > H O > HCl
153. From the following chemical reactions determine the relative Br nsted-Lowry base
strengths (strongest to weakest).
2 NaH(s) + H O(l)
2 NaOH + H (g)
NH (aq) + H O(l)
NH (aq) + OH (aq)
a) H > OH > NH
b) H > NH > OH
c) OH > H > NH
d) OH > NH > H
Sections 15.3 - 4 Hydrated Protons and Dissociation of Water
154. What is the hydroxide ion concentration for a solution that is 3.50 x 10
hydronium ion?
a) 2.86 x 10
M
b) 2.86 x 10
M
c) 2.86 x 10
M
d) 3.50 x 10
M
155. A solution with a hydroxide ion concentration of 4.15 x 10
hydrogen ion concentration of ______.
a) acidic, 2.41 x 10
M
b) acidic, 2.41 x 10
M
c) basic, 2.41 x 10
M
d) basic, 2.41 x 10
M
M in
M is ________ and has a
Section 15.6 Measuring pH
156. What is the approximate pH of a solution X that gives the following responses with
the indicators shown?
a)
b)
c)
d)
Indicators
HIn-In
pH range
Solution X
methyl orange
red-yellow
3.2-4.4
yellow
methyl red
red-yellow
4.8-6.0
yellow
bromthymol blue
yellow-blue
6.0-7.6
green
phenolphthalein
colorless-pink
8.2-10.0
colorless
3.2
4.8
6.0
8.2
-
4.4
6.0
7.6
10.0
Page 34
Section 15.7 The pH in Solutions of Strong Acids and Strong Bases
157. What is the pH of a 0.020 M HClO
a) 0.020
b) 0.040
c) 1.70
d) 12.30
solution?
158. What is the pH of a 0.020 M Ba(OH)
a) 1.40
b) 1.70
c) 12.60
d) 13.60
solution?
159. What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO , 50.0 mL of 0.20
M HCl, and 100.0 mL of water? Assume that the volumes are additive.
a) 0.30
b) 0.82
c) 1.00
d) 1.10
Section 15.8 Equilibria Solutions of Weak Acids
160. What is the equilibrium constant expression (K a ) for the acid dissociation of nitrous
acid HNO ? The equation of interest is
HNO (aq) + H O(l)
H O (aq) + NO (aq).
a) K a = ([H O ][NO ])/([HNO ][H O])
b) K a = ([H O ][NO ])/([HNO ])
c) K a = ([HNO ][H O])/([H O ][NO ])
d) K a = ([HNO ])/([H O ][NO ])
Section 15.9 Calculating Equilibrium Concentrations in Solutions of Weak
Acids
161. What is the hydronium ion concentration of a 0.100 M acetic acid solution with a K a =
1.8 x 10 ? The equation of interest is CH COOH(aq) + H O(l)
H O (aq) + CH CO (aq)
a)
b)
c)
d)
1.34
4.24
1.34
4.24
x
x
x
x
10
10
10
10
M
M
M
M
162. Potassium hydrogen phthalate (molar mass = 204.2 g/mol) is the most commonly used
acid for determining the molarity of a basic solution. The acid is monoprotic and
has a K a = 3.91 x 10 . What is the pH of 25.0 mL of a solution that contains 0.400 g
of potassium hydrogen phthalate?
a) 1.10
b) 3.26
c) 4.30
d) 5.41
Page 35
Section 15.10 Percent Dissociation in Solutions of Weak Acids
163. What is the percent dissociation of a benzoic acid solution with pH = 2.59? The acid
dissociation constant for this monoprotic acid is 6.5 x 10 .
a) 0.50%
b) 1.5%
c) 2.5%
d) 3.5%
164. The percent dissociation of acetic acid changes as the concentration of the acid
decreases. A 100-fold decrease in acetic acid concentration results in a ____ fold
_________ in the percent dissociation.
a) 10, increase
b) 10, decrease
c) 100, increase
d) 100, decrease
Section 15.11 Polyprotic Acids
165. Which of the following are weak diprotic acids?
a) carbonic acid - H CO , hydrosulfuric acid - H S, acetic acid - CH COOH
b) formic acid - HCOOH, acetic acid CH COOH, benzoic acid C H COOH
c) carbonic acid - H CO , oxalic acid - H C O , sulfurous acid - H SO
d) hydrocyanic acid - HCN, sulfuric acid - H SO , phosphoric acid - H PO
166. What is the second stepwise equilibrium constant expression for phosphoric acid H PO
?
a) K a
= ([H O ][H PO ])/([H PO ])
b) K a
= ([H O ]2[HPO 2 ])/([H PO ])
c) K a
= ([H O ]3[PO 3 ])/([H PO ])
d) K a
= ([H O ][HPO 2 ])/([H PO ])
167. Calculate the pH of a 0.020 M carbonic acid solution, H CO that has the stepwise
dissociation constants of K(a1) = 4.3 x 10
and K a
= 5.6 x 10
.
a) 1.70
b) 4.03
c) 6.39
d) 10.25
168. What is the selenide ion concentration [Se ] for a 0.100 M H Se solution that has
the stepwise dissociation constants of K a 1 = 1.3 x 10
and K a 2 = 1.0 x 10
?
a) 3.6 x 10
M
b) 1.3 x 10
M
c) 1.3 x 10
M
d) 1.0 x 10
M
Page 36
Section 15.12 Equilibria in Solutions of Weak Bases
169. How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH
of 9.00? The K b for pyridine is 1.9 x 10
and the equation of interest is C H N(aq)
+ H O(l)
C H NH (aq) + OH (aq).
a) 0.053 g
b) 0.42 g
c) 0.79 g
d) 7.9 g
Section 15.13 Relation Between K
a
and K
b
170. Acetic acid CH COOH, has an acid dissociation constant of 1.8 x 10 . What is the
conjugate base of acetic acid and what is its base dissociation constant?
a) CH C(OH) , 5.6 x 10
b) CH C(OH) , 5.6 x 10
c) CH COOH, 5.6 x 10
d) CH CO , 5.6 x 10
171. Dihydrogen phosphate H PO , has an acid dissociation constant of 6.2 x 10 . What
is the conjugate base of H PO
and what is its base dissociation constant?
a) H PO , 1.6 x 10
b) H PO , 1.6 x 10
c) HPO
, 1.6 x 10
d) HPO
, 1.6 x 10
Section 15.14 Acid-Base Properties of Salts
172. If
to
a)
b)
c)
d)
an equal number of moles of the weak acid HOCN and the strong base KOH are added
water, is the resulting solution acidic, basic, or neutral?
acidic
basic
neutral
more information is needed to answer the question
Section 15.16 Lewis Acids and Bases
173. Identify the Lewis acid that acts as a reactant in the following reaction
Co(H O)
(aq) + 6 NH (aq)
Co(NH )
(aq) + 6 H O(l).
a) Co(H O)
b) Co
c) NH
d) H O
174. Identify the set of Lewis acids.
a) BH , BF , Cu , CO
b) Cl , OH , NH , H O
c) H PO , H PO , HPO
, PO
d) CH , NH , OH , F
Page 37
Section 16.1 Neutralization Reactions
175. What is the approximate value of the equilibrium constant for the neutralization of
acetic acid with sodium hydroxide? The K a for acetic
acid is 1.8 x 10
and the reaction of interest is CH CO H(aq) + NaOH(aq) = H O(l) +
NaCH CO (aq).
a) 1.8 x 10
b) 5.6 x 10
c) 1.8 x 10
d) 1.8 x 10
176. What is the approximate value of the equilibrium constant for the neutralization of
pyridine with hydrochloric acid? The K b for pyridine is 1.8 x 10
and the equation
of interest is
HCl(aq) + C H N(aq)
C H NHCl(aq).
a) 5.6 x 10
b) 5.6 x 10
c) 1.8 x 10
d) 5.6 x 10
Section 16.2 The Common-Ion Effect
177. Indicate
a) HF, H
b) HF, H
c) HF, H
d) HF, H
the
O ,
O ,
O ,
O ,
major chemical species present in a solution of 0.10 HF and 0.10 M NaF?
F
F , Na
F , Na , H O
F , Na , H O, OH
178. What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH with 25.00 mL
of 0.10 M NH Cl? Assume that the volumes of solution are additive and that the K b for
ammonia is 1.8 x 10 ?
a) 7.00
b) 9.26
c) 9.56
d) 11.13
Section 16.3 Buffer Solutions
179. What is the [CH CO -]/[CH CO H] ratio necessary to make a buffer solution with a pH
of 4.44? The K a for acetic acid is 1.8 x 10 .
a) 0.30:1
b) 0.50:1
c) 1.07:1
d) 1.33:1
180. What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium
hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL
with water? The K a 2 for hydrogen phthalate is 3.1 x 10 .
a) 3.25
b) 5.08
c) 5.51
d) 5.94
Page 38
Section 16.4 The Henderson-Hasselbalch Equation
181. What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pK a
= 9.60?
a) 50%
b) 9%
c) 5%
d) 1%
Section 16.5 Titration Curves
182. What is the characteristic pH-titrant curve for the titration of a strong base by a
strong acid?
a) A
b) B
c) C
d) D
Page 39
183. Indicate the buffer region and the basic region from the titration curve of a weak
acid titrated with a strong base.
a) A and B
b) A and C
c) B and C
d) B and D
Page 40
184. Indicate the pH values at the equivalence point and halfway to the equivalence point
in the titration of a weak acid with a strong base.
a) A and B
b) B and C
c) C and B
d) C and E
Section 16.6 - 8 Titrations of Strong and Weak Acids and Bases
185. What is the pH at the equivalence point of a weak base-strong acid titration if
20.00 mL of NaOCl requires 28.30 mL of 0.500 M HCl? The K a for HOCl is 3.0 x 10
a) 0.30
b) 3.76
c) 4.03
d) 6.06
.
186. What is the pH of a solution made by mixing 30.00 mL of 0.100 M acetic acid, CH CO H,
with 40.00 mL of 0.100 M NaOH? The K a for acetic acid is 1.8 x 10 .
a) 8.44
b) 9.26
c) 11.13
d) 12.16
Page 41
Section 16.9 Polyprotic Acid - Strong Base Titrations
187. The dissociation equilibrium constants for the protonated form of alanine (a
diprotic amino acid, H X ) are K a 1 = 4.6 x 10
and K a 2 = 2.0 x 10
. What is the pH
of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been
added?
a) 4.85
b) 6.02
c) 7.39
d) 9.70
Section 16.10 Solubility Equilibria
188. What is the chromium ion concentration for a saturated solution of Cr(OH)
for Cr(OH) is 6.7 x 10
?
a) 8.19 x 10
M
b) 1.26 x 10
M
c) 2.17 x 10
M
d) 3.76 x 10
M
if the K s p
Section 16.12 Factors That Affect Solubility
189. Which solution will cause the greatest change in the solubility of PbCl
a) 0.1 M HCl
b) 0.1 M NaCl
c) 0.1 M CaCl
d) 0.1 M KNO
at 25
C?
190. Which of the following metal hydroxides are amphoteric?
a) Al(OH) , Zn(OH) , Cr(OH) , Sn(OH)
b) Cu(OH) , Mn(OH) , Fe(OH) , Fe(OH)
c) Be(OH) , Ca(OH) , Ba(OH) , Sr(OH)
d) LiOH, NaOH, KOH, RbOH
Section 16.13 - 14 Precipitation of Ionic Compounds and Separation of
Ions by Selective Precipitation
191. Potassium chromate is slowly added to a solution containing 0.20 M AgNO and 0.20 M
Ba(NO ) . Describe what happens if the K s p for Ag CrO is 1.1 x 10
and the K s p of
BaCrO is 1.2 x 10
.
a) The BaCrO precipitates first out of solution.
b) The Ag CrO precipitates first out of solution and then BaCrO precipitates.
c) Both BaCrO and Ag CrO precipitate simultaneously out of solution
d) Neither BaCrO nor Ag CrO precipitates out of solution.
Page 42
192. Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn
, Pb
and Cu
and 0.10 M in H S at a pH of 1.0?
a)
b)
c)
d)
Metal
Sulfide
Ks p
MnS
3 x 10
ZnS
3 x 10
PbS
3 x 10
CuS
6 x 10
, Zn
MnS
CuS
PbS, CuS
ZnS, PbS, CuS
193. Which
a) Ag
b) Cu
c) Ag
d) Na
metal ions can be precipitated out of solution as chlorides?
, Hg , Co
, Cd , Bi
, Hg
, Pb
, K , Mg
Section 17.1 Spontaneous Processes
194. Which of the following is a nonspontaneous process?
a) the expansion of a gas into a vacuum
b) N (g) + 3 H (g)
2 NH (g) if p H = p N = 1 atm, p N H = 0, and
K p = 4 x 10
c) 2 NH (g)
N (g) + 3 H (g) if p N H = 1 atm, p H = p N = 0, and
K p = 2 x 10
d) none of the above
Section 17.3 Entropy and Probability
195. Assume a heteronuclear diatomic molecule, AB, forms a one-dimensional crystal by
lining up along the x-axis. Also assume that each molecule can only have one of six
possible orientations, corresponding to atom A facing in either the positive or
negative direction along the x-,
y-, or z-axis. If the molecules are arranged randomly in the six directions, the
molar entropy at absolute zero should be
a) R ln 6.
b) R ln 6 .
c) R ln 6!
d) 0.
Page 43
Section 17.4 Entropy and Temperature
196. Which provides the greatest increase
a) H O (s, 0 C)
H O (l, 0 C)
b) H O (l, 0 C)
H O (l, 25 C)
c) H O (g, 0.1 C)
H O (s, 0.1 C)
d) H O (l, 100 C)
H O (g, 100 C)
in entropy?
Section 17.5 Standard Molar Entropies and Standard Entropies of Reaction
197. Calculate S for the following reaction.
N (g) + 2 O (g)
2 NO (g)
Species
a)
b)
c)
d)
S , J/(K mol)
N (g)
191.5
O (g)
205.0
NO (g)
240.0
-156.5 J/K
-121.5 J/K
15.5 J/K
636.5 J/K
198. Calculate S for the formation of one mole of solid sodium bromide from the
elements at 25 C.
Species
S , J/(K mol)
NaBr(s)
86.8
Na(s)
51.3
Br (l)
a)
b)
c)
d)
152.2
-116.7 J/K
-81.2 J/K
-40.6 J/K
86.8 J/K
199. Which should have the highest standard molar entropy at 25 C?
a) Al(s)
b) Al(l)
c) Al(g)
d) All three should have a standard molar entropy of zero.
Page 44
Section 17.7 Free Energy
200. At 25 C, H = 1.895 kJ and S = -3.363 J/K for the transition
C(graphite)
C(diamond)
Based on these data
a) graphite cannot be converted to diamond at 1 atm pressure.
b) diamond is more stable than graphite at all temperatures at 1 atm.
c) diamond is more stable than graphite below 290 C and graphite is more stable than
diamond above 290 C.
d) graphite is more stable than diamond below 290 C and diamond is more stable than
graphite above 290 C.
(c) 1998 Prentice-Hall, Inc. All rights reserved.
ANSWER KEY FOR TEST final review
Page 1
1. d)
Chapter: 1
QUESTION:
14
Chapter: 1
QUESTION:
21
Chapter: 1
QUESTION:
36
Chapter: 1
QUESTION:
47
Chapter: 1
QUESTION:
58
Chapter: 1
QUESTION:
60
Chapter: 1
QUESTION:
73
Chapter: 2
QUESTION:
2
Chapter: 2
QUESTION:
3
Chapter: 2
QUESTION:
19
Chapter: 2
QUESTION:
30
Chapter: 2
QUESTION:
35
Chapter: 2
QUESTION:
46
Chapter: 2
QUESTION:
58
Chapter: 2
QUESTION:
63
Chapter: 2
QUESTION:
65
Chapter: 2
QUESTION:
68
2. b)
3. b)
4. a)
5. c)
6. b)
7. a)
8. a)
9. a)
10. b)
11. c)
12. a) periodic table required
13. d)
14. b)
15. d)
16. d) periodic table required
17. c)
ANSWER KEY FOR TEST final review
Page 2
18. c)
Chapter: 2
QUESTION:
69
Chapter: 2
QUESTION:
73
Chapter: 3
QUESTION:
5
Chapter: 3
QUESTION:
15
Chapter: 3
QUESTION:
24
Chapter: 3
QUESTION:
28
Chapter: 3
QUESTION:
30
Chapter: 3
QUESTION:
33
Chapter: 3
QUESTION:
39
Chapter: 3
QUESTION:
64
Chapter: 3
QUESTION:
66
Chapter: 3
QUESTION:
72
Chapter: 3
QUESTION:
74
Chapter: 4
QUESTION:
4
Chapter: 4
QUESTION:
15
Chapter: 4
QUESTION:
50
Chapter: 4
QUESTION:
56
19. c)
20. d)
21. b)
22. c)
23. d)
24. b)
25. c)
26. d)
27. d)
28. c)
29. d)
30. c)
31. c)
32. d)
33. d)
34. b)
ANSWER KEY FOR TEST final review
Page 3
35. c)
Chapter: 4
QUESTION:
74
Chapter: 5
QUESTION:
6
Chapter: 5
QUESTION:
11
Chapter: 5
QUESTION:
18
Chapter: 5
QUESTION:
21
Chapter: 5
QUESTION:
30
Chapter: 5
QUESTION:
33
Chapter: 5
QUESTION:
34
Chapter: 5
QUESTION:
37
Chapter: 5
QUESTION:
41
Chapter: 5
QUESTION:
53
Chapter: 6
QUESTION:
4
Chapter: 6
QUESTION:
14
Chapter: 6
QUESTION:
26
Chapter: 6
QUESTION:
28
Chapter: 6
QUESTION:
36
Chapter: 6
QUESTION:
47
36. a)
37. b)
38. a)
39. d)
40. d)
41. c)
42. c)
43. c)
44. c)
45. c)
46. d)
47. a)
48. d)
49. b)
50. c)
51. d)
ANSWER KEY FOR TEST final review
Page 4
52. c)
Chapter: 6
QUESTION:
52
Chapter: 6
QUESTION:
71
Chapter: 6
QUESTION:
76
Chapter: 7
QUESTION:
23
Chapter: 7
QUESTION:
58
Chapter: 7
QUESTION:
73
Chapter: 8
QUESTION:
37
Chapter: 8
QUESTION:
41
Chapter: 8
QUESTION:
47
Chapter: 8
QUESTION:
58
Chapter: 8
QUESTION:
63
Chapter: 8
QUESTION:
76
Chapter: 9
QUESTION:
21
Chapter: 9
QUESTION:
34
Chapter: 9
QUESTION:
46
Chapter: 9
QUESTION:
54
Chapter: 9
QUESTION:
60
53. a)
54. b)
55. b)
56. c)
57. b)
58. d)
59. a)
60. b)
61. d)
62. c)
63. b)
64. a)
65. d)
66. b)
67. c)
68. a)
ANSWER KEY FOR TEST final review
Page 5
69. b)
Chapter: 9
QUESTION:
68
Chapter: 9
QUESTION:
74
Chapter: 9
QUESTION:
80
Chapter: 10
QUESTION:
4
Chapter: 10
QUESTION:
15
Chapter: 10
QUESTION:
25
Chapter: 10
QUESTION:
27
Chapter: 10
QUESTION:
40
Chapter: 10
QUESTION:
43
Chapter: 10
QUESTION:
48
Chapter: 10
QUESTION:
55
Chapter: 10
QUESTION:
56
Chapter: 10
QUESTION:
61
Chapter: 10
QUESTION:
73
Chapter: 10
QUESTION:
74
Chapter: 10
QUESTION:
76
Chapter: 10
QUESTION:
80
70. c)
71. d)
72. c)
73. c)
74. d)
75. c)
76. c)
77. c)
78. c)
79. b)
80. b)
81. c)
82. b)
83. d)
84. c)
85. b)
ANSWER KEY FOR TEST final review
Page 6
86. a)
Chapter: 11
QUESTION:
4
Chapter: 11
QUESTION:
11
Chapter: 11
QUESTION:
12
Chapter: 11
QUESTION:
16
Chapter: 11
QUESTION:
17
Chapter: 11
QUESTION:
19
Chapter: 11
QUESTION:
25
Chapter: 11
QUESTION:
30
Chapter: 11
QUESTION:
37
Chapter: 11
QUESTION:
40
Chapter: 11
QUESTION:
42
Chapter: 11
QUESTION:
45
Chapter: 11
QUESTION:
53
Chapter: 11
QUESTION:
54
Chapter: 11
QUESTION:
56
Chapter: 11
QUESTION:
59
Chapter: 11
QUESTION:
69
87. a)
88. d)
89. c)
90. c)
91. c)
92. a)
93. b)
94. c)
95. b)
96. b)
97. c)
98. c)
99. c)
100. b)
101. c)
102. c)
ANSWER KEY FOR TEST final review
Page 7
103. d)
Chapter: 11
QUESTION:
77
Chapter: 11
QUESTION:
87
Chapter: 12
QUESTION:
19
Chapter: 12
QUESTION:
24
Chapter: 12
QUESTION:
25
Chapter: 12
QUESTION:
27
Chapter: 12
QUESTION:
29
Chapter: 12
QUESTION:
33
Chapter: 12
QUESTION:
38
Chapter: 12
QUESTION:
47
Chapter: 12
QUESTION:
50
Chapter: 12
QUESTION:
55
Chapter: 12
QUESTION:
58
Chapter: 12
QUESTION:
59
Chapter: 12
QUESTION:
61
Chapter: 12
QUESTION:
63
Chapter: 12
QUESTION:
64
104. a)
105. c)
106. d)
107. d)
108. b)
109. b)
110. d)
111. d)
112. b)
113. b)
114. b)
115. d)
116. d)
117. b)
118. a)
119. d)
ANSWER KEY FOR TEST final review
Page 8
120. a)
Chapter: 12
QUESTION:
69
Chapter: 12
QUESTION:
78
Chapter: 13
QUESTION:
1
Chapter: 13
QUESTION:
5
Chapter: 13
QUESTION:
8
Chapter: 13
QUESTION:
12
Chapter: 13
QUESTION:
25
Chapter: 13
QUESTION:
28
Chapter: 13
QUESTION:
41
Chapter: 13
QUESTION:
48
Chapter: 13
QUESTION:
53
Chapter: 13
QUESTION:
55
Chapter: 13
QUESTION:
63
Chapter: 13
QUESTION:
69
Chapter: 13
QUESTION:
73
Chapter: 13
QUESTION:
80
Chapter: 13
QUESTION:
83
121. b)
122. b)
123. c)
124. b)
125. d)
126. a)
127. c)
128. a)
129. c)
130. b)
131. a)
132. a)
133. b)
134. d)
135. a)
136. b)
ANSWER KEY FOR TEST final review
Page 9
137. d)
Chapter: 14
QUESTION:
1
Chapter: 14
QUESTION:
7
Chapter: 14
QUESTION:
8
Chapter: 14
QUESTION:
11
Chapter: 14
QUESTION:
35
Chapter: 14
QUESTION:
36
Chapter: 14
QUESTION:
37
Chapter: 14
QUESTION:
45
Chapter: 14
QUESTION:
57
Chapter: 14
QUESTION:
68
Chapter: 14
QUESTION:
77
Chapter: 14
QUESTION:
79
Chapter: 15
QUESTION:
5
Chapter: 15
QUESTION:
9
Chapter: 15
QUESTION:
13
Chapter: 15
QUESTION:
22
Chapter: 15
QUESTION:
26
138. b)
139. a)
140. b)
141. d)
142. a)
143. a)
144. c)
145. c)
146. d)
147. b)
148. b)
149. b)
150. b)
151. a)
152. b)
153. a)
ANSWER KEY FOR TEST final review
Page 10
154. c)
Chapter: 15
QUESTION:
30
Chapter: 15
QUESTION:
32
Chapter: 15
QUESTION:
43
Chapter: 15
QUESTION:
46
Chapter: 15
QUESTION:
47
Chapter: 15
QUESTION:
52
Chapter: 15
QUESTION:
55
Chapter: 15
QUESTION:
60
Chapter: 15
QUESTION:
65
Chapter: 15
QUESTION:
66
Chapter: 15
QUESTION:
69
Chapter: 15
QUESTION:
70
Chapter: 15
QUESTION:
71
Chapter: 15
QUESTION:
72
Chapter: 15
QUESTION:
76
Chapter: 15
QUESTION:
81
Chapter: 15
QUESTION:
85
155. d)
156. c)
157. c)
158. c)
159. d)
160. b)
161. c)
162. b)
163. c)
164. a)
165. c)
166. d)
167. b)
168. d)
169. b)
170. d)
ANSWER KEY FOR TEST final review
Page 11
171. d)
Chapter: 15
QUESTION:
86
Chapter: 15
QUESTION:
89
Chapter: 15
QUESTION: 109
Chapter: 15
QUESTION: 114
Chapter: 16
QUESTION:
4
Chapter: 16
QUESTION:
5
Chapter: 16
QUESTION:
9
Chapter: 16
QUESTION:
13
Chapter: 16
QUESTION:
24
Chapter: 16
QUESTION:
25
Chapter: 16
QUESTION:
31
Chapter: 16
QUESTION:
36
Chapter: 16
QUESTION:
39
Chapter: 16
QUESTION:
40
Chapter: 16
QUESTION:
49
Chapter: 16
QUESTION:
53
Chapter: 16
QUESTION:
59
172. b)
173. b)
174. a)
175. d)
176. c)
177. c)
178. c)
179. b)
180. b)
181. b)
182. c)
183. d)
184. c)
185. c)
186. d)
187. d)
ANSWER KEY FOR TEST final review
Page 12
188. b)
Chapter: 16
QUESTION:
64
Chapter: 16
QUESTION:
73
Chapter: 16
QUESTION:
78
Chapter: 16
QUESTION:
81
Chapter: 16
QUESTION:
83
Chapter: 16
QUESTION:
85
Chapter: 17
QUESTION:
2
Chapter: 17
QUESTION:
18
Chapter: 17
QUESTION:
22
Chapter: 17
QUESTION:
27
Chapter: 17
QUESTION:
29
Chapter: 17
QUESTION:
30
Chapter: 17
QUESTION:
48
189. c)
190. a)
191. b)
192. d)
193. c)
194. d)
195. a)
196. d)
197. b)
198. c)
199. c)
200. a)
(c) 1998 Prentice-Hall, Inc. All rights reserved.