Chapter 5 and 6
1. What is often the source of the
ammonium ion in waste water?
a) fish by-products
b) human and animal
waste
c) industrial plating
compounds
d) algae
0%
a)
0%
b)
0%
c)
0%
d)
2. In an alcoholic beverage with 10% alcohol
content by volume, how can the alcohol be
defined?
a)
b)
c)
d)
as a solvent
as a solute
as a solution
as a fluid
0%
a)
0%
b)
0%
c)
0%
d)
3.Blood plasma is considered what
component of a solution?
a)
b)
c)
d)
the solvent
the protein
the solute
the lipid
0%
a)
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b)
0%
c)
0%
d)
4.How are molecules described when they
contain both a positive and negative end?
a)
b)
c)
d)
planar
apolar
non-polar
polar
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a)
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b)
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c)
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d)
5.In general, when an aqueous solution is
heated, what happens to the solubility of ionic
compounds within it?
a) Solubility decreases.
b) Solubility increases.
c) Kinetic energy is
added by the solute.
d) Kinetic energy is
removed by the
solute.
0%
a)
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b)
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c)
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d)
6.What affects the rate at which
solutes dissolve?
a) temperature of the
solution
b) surface area of the
solute
c) concentration of the
solute
d) all of the above
0%
a)
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b)
0%
c)
0%
d)
7.Why does powdered sugar dissolve
in water more rapidly than a sugar
cube?
a) greater surface area of
the powder
b) more kinetic energy in
the powdered sample
c) greater concentration
in the sugar cube
d) greater density of the
sugar cube
0%
a)
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b)
0%
c)
0%
d)
8.What is an electrolyte?
a) a compound that
dissolves in water
b) a compound that
dissociates into ions in
water
c) a compound that
dissociates into molecules
in water
d) an ionic compound that
doesn't dissolve in water
0%
a)
0%
b)
0%
c)
0%
d)
9.What is a weak electrolyte?
a) a compound that
completely forms ions in
solution
b) a compound that only
partially forms molecules in
solution
c) a compound that
completely forms
molecules in solution
d) a compound that only
partially forms ions in
solution
0%
a)
0%
b)
0%
c)
0%
d)
10. Which compounds could be
electrolytes?
a)
b)
c)
d)
SO3
NO2
CH4
MgCl2
0%
a)
0%
b)
0%
c)
0%
d)
11.Which of these are electrolytes?
a)
b)
c)
d)
ICl
CO2
NaCl
CO
0%
a)
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b)
0%
c)
0%
d)
12. Which of the following are not
electrolytes?
a)
b)
c)
d)
NaI
CaCl2
KBr
NO2
0%
a)
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b)
0%
c)
0%
d)
13. What is a saturated solution?
a) one that contains the maximum
amount of solute that can be
dissolved.
b) one that contains the maximum
amount of solvent that can be
dissolved.
c) one that contains the maximum
amount of solution that can be
dissolved.
d) one that contains the maximum
amount of a salt that can be
0%
dissolved.
a)
0%
b)
0%
c)
0%
d)
14. What type of compound is
NH4NO3?
a)
b)
c)
d)
acidic
basic
insoluble
soluble
0%
a)
0%
b)
0%
c)
0%
d)
15. Molarity is what?
a) moles of solvent per
liters of solution
b) moles of solute per
liters of solution
c) moles of solute per
liters of solute
d) moles of solvent per
liters of solvent
0%
a)
0%
b)
0%
c)
0%
d)
16. What is the molarity of a solution made
from 54.9 g of NaCl in 0.75 L of water?
a)
b)
c)
d)
73.2 M
1.25 M
1.42 M
0.01 M
0%
a)
0%
b)
0%
c)
0%
d)
17. What is the molarity of a solution made
from 0.25 mol of KBr and 0.80 L of water?
a)
b)
c)
d)
0.31 M
3.20 M
0.20 M
1.05 M
0%
a)
0%
b)
0%
c)
0%
d)
18. An acid is any compound that
can release what?
a)
b)
c)
d)
O2–
H+
H–
O+
0%
a)
0%
b)
0%
c)
0%
d)
19. What do all weak acids have in
common?
a) They are weak
electrolytes.
b) They are non-electrolytes.
c) They are strongly acidic.
d) They are strong
electrolytes.
0%
a)
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b)
0%
c)
0%
d)
20. NaOH is classified as what kind
of compound?
a)
b)
c)
d)
weak base
strong acid
strong base
weak acid
0%
a)
0%
b)
0%
c)
0%
d)
21. How is a base defined?
a) as a compound that
produces hydroxide ions
b) as a compound that
produces H+ ions
c) as a compound with a pH
below 7
d) as a compound with pH = 7
0%
a)
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b)
0%
c)
0%
d)
22. What is lithium hydroxide?
a) LiOH, a strong base
b) LiOH, a weak base
c) Li(OH)2, a strong
base
d) Li(OH)2, a weak base
0%
a)
0%
b)
0%
c)
0%
d)
23. A solution with a pH = 3.5 is
said to be what?
a)
b)
c)
d)
acidic
basic
neutral
can't tell from the
information given
0%
a)
0%
b)
0%
c)
0%
d)
24. The pH of a solution with a [H+]
–8
= 1.0 x 10 is what?
a)
b)
c)
d)
4
8
12
can't be determined
0%
a)
0%
b)
0%
c)
0%
d)
25. What is a solution with a pH of
12?
a)
b)
c)
d)
neutral
acidic
basic
concentrated
0%
a)
0%
b)
0%
c)
0%
d)
26. Attractive forces that exist
between particles are called what?
1. intermolecular
forces
2. intramolecular
forces
3. heteromolecular
forces
4. intravenousmolecular forces
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1
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2
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3
0%
4
27. What is surface tension?
1. a measure of how much energy is needed to
decrease the surface volume of a liquid
2. a measure of how much surface is needed
to increase the energy within a liquid
3. a measure of how much energy is needed to
increase the surface area of a liquid
4. a measure of how much surface is needed
to decrease the energy within a liquid
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1
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2
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4
28. What takes place within the
electron cloud of an atom?
1. Electrons acquire
positive charge.
2. Electrons acquire
negative charge.
3. Electrons are fixed
in positions.
4. Electrons are in
constant motion.
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1
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2
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3
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4
29. How is an induced dipole
created?
1. by an electron positioning
next to it
2. by an electron inversion
near it
3. by dipoles placed on both
sides of it
4. by the presence of a dipole
0%
next to it
1
0%
2
0%
3
0%
4
30. Polarizability is defined how?
1. by how easily an atom
changes shape and charge
2. by how deformable an
atomic nucleus is
3. by how deformable an
electron cloud is
4. by how easily an electron
changes shape and charge
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1
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2
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3
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4
31. How would the following—HCl,
HF, and HBr—be ranked from least
to most polarizable?
1.
2.
3.
4.
HCl, HF, HBr
HF, HCl, HBr
HF, HBr, HCl
HBr, HCl, HF
0%
1
0%
2
0%
3
0%
4
32. Rank HCl, HI, and HBr from
least to most polarizable.
1.
2.
3.
4.
HCl, HBr, HI
HI, HBr, HCl
HBr, HCl, HI
HI, HCl, HBr
0%
1
0%
2
0%
3
0%
4
33. How would the following, Ne,
Kr, Ar, He, be ordered from lowest
to highest melting point?
1.
2.
3.
4.
He, Ne, Ar, Kr
Kr, He, Ar, Ne
He, Ar, Ne, Kr
Kr, Ar, Ne, He
0%
1
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2
0%
3
0%
4
34. To what is the positive region
of a polar molecule attracted?
1. a magnet
2. the positive region of a
neighboring molecule
3. the negative region of a
neighboring molecule
4. to a non-polar molecule, thus
inducing a dipole
0%
1
0%
2
0%
3
0%
4
35. Of the following choices, which
can form hydrogen bonds?
1.
2.
3.
4.
H2O
H2
H2S
HCl
0%
1
0%
2
0%
3
0%
4
36. When a solute is added to a solvent,
why does the boiling point increase?
1. Intermolecular attractions hold solute and solvent apart,
requiring more energy to make the solution boil.
2. Intermolecular attractions hold solute and solvent
together, requiring less energy to make the solution boil.
3. Intermolecular attractions hold solute and solvent
together, requiring more energy to make the solution
boil.
4. Intermolecular attractions hold solute and solvent apart,
requiring less energy to make the solution boil.
0%
1
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2
0%
3
0%
4
37. How does boiling an unknown sample of
water allow you to determine if it is pure water
or a salt solution?
1. In a salt solution, the b.p. should be
lower than 100°C.
2. In a salt solution, the b.p. should be
higher than 100°C.
3. In pure water, the b.p. should be
lower than 100°C.
4. In pure water, the b.p. should be
higher than 100°C.
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1
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2
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4
38. As the molecular mass of the compound
increases, the higher the melting point.
1. True
2. false
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1
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2
39. Which of the following aqueous
solution will have the lowest freezing
point?
1.
2.
3.
4.
1 M MgBr2
1 M KBr
2 M C6H12O6
2 M C12H22O11
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1
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2
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3
0%
4
40. When comparing the freezing point of pure water
and a salt solution, the best explanation would be:
1.
2.
3.
4.
When a salt is dissolved in a solvent, it blocks part
of the liquid solvent from interacting with the
molecules resulting in a decreased rate of binding
into a solid.
When a salt is dissolved in a solvent, it blocks part
of the liquid solvent from interacting with the
molecules resulting in a increased rate of binding
into a solid.
A salt solution would freeze much faster than pure
water because there are more molecules to bind to.
Pure water will not freeze because there are not
enough molecules to bind.
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1
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2
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3
0%
4
41. In general, ionic compounds have
1. High boiling points and low
melting points.
2. Low boiling points and high
melting points.
3. High boiling points and high
melting points.
4. Low boiling points and low
melting points.
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1
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2
0%
3
0%
4
42. Which of the following is most
likely to have a high boiling point?
1.
2.
3.
4.
NaCl
CO2
CH4
H2O
0%
1
0%
2
0%
3
0%
4
43. Place the following list of atoms
in order of increasing
polarizability:Ga, B, Al, In
1.
2.
3.
4.
B, Al, Ga, In
Al, Ga, B, In
Ga, B, Al, In
In, Al, B, Ga
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1
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2
0%
3
0%
4
44. What is the one factor upon which
boiling point elevation depends?
1.
2.
3.
4.
number of particles in solution
size of particles in solution
charges of particles in solution
types of particles in solution
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1
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2
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3
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4
45. A solution with pH = 3 has what
[H+] concentration?
a)
b)
c)
d)
1 x 10–3
1 x103
3 x 10–13
3 x 103
0%
a)
0%
b)
0%
c)
0%
d)
46. If equal molar amounts of two solutions, one with pH = 1, the
other with pH = 14, were mixed carefully and no solution was
lost, what would be the pH of the final solution?
a)
b)
c)
d)
15
13
7
not enough
information to tell
0%
a)
0%
b)
0%
c)
0%
d)
47. What is the pH of a completely
neutral solution?
a)
b)
c)
d)
0
14
1
7
0%
a)
0%
b)
0%
c)
0%
d)
48. The products that would be expected in the
neutralization reaction involving nitric acid and
barium hydroxide are:
a)
b)
c)
d)
BaO and H2O
BaO2 and 2H2O
BaNO3 and H2O
Ba(NO3)2 and 2H2O
0%
a)
0%
b)
0%
c)
0%
d)