SAT chem 07 solutions test review

SC2 – O’Malley

SAT II Review (Solutions)

For 1 – 2:
a. Molarity
b. Formality
c. Density
d. Molality
e. Normality
1.

Which is defined as moles of solute
per kilogram of solvent?

2.

Which is defined as moles of solute
per liter of solution?

For 3 – 6:
a. Solute
b. Solvent
c. Solubility
d. Aqueous solution
e. Solvation
3.

Which is present in a lesser
amount in a solution?

4.

Which describes a species in which
the solvent is water?

5.

Which is present in greater quantity
in solution?

6.

Which is the interaction between
the solute and the solvent
molecules?
For 7 – 9:
a. Dilute
b. Concentrated
c. Unsaturated
d. Saturated
e. Supersaturated
7.

Which is the condition, unrelated to
quantities, that indicates that the
rate going into solution is equal to
the rate coming out of solution?

8.

Which is the condition that exists
when a water solution that has
been at equilibrium is heated to a
higher temperature with a higher
solubility, but no additional solute is
added?

solute, compared with the amount
of solvent, in a solution?
For 10 – 11:
a. i, ii and iii
b. i and ii
c. ii and iii
d. i only
e. iii only
10. The ionization of salts in water is
useful in explaining
i. Their unusually large solubility
in water
ii. Their electrical conductivity in
solution
iii. The lowered freezing points
and increased boiling points
of their solutions
11. Which of the following describe
water?
i. Solvent for polar solutes
ii. Polar molecule
iii. Good conductor of electricity

9.

Q
12.
13.
14.
15.
16.
17.

Which is the descriptive term that
indicates there is a large quantity of
Statement I
Because
Statement II
When a solute is added to pure water, the vapor
Because
All solutes dissociate into positive and negative ions
pressure of the water will decrease
NaCl(aq) is an electrolyte
Because
It forms ions in solution
A salt dissolved in an organic solvent will be a good
Because
Salts will not dissolve appreciably in an organic solvent
electrical conductor
A super saturated solution of glucose in boiling water Because
The solubility increases as the temperature decreases
crystallizes as it cools
Salt dissolved in water lowers the freezing point

Because
The change in freezing point is given by: Tf = iKfm
Sodium chloride forms aqueous solution of ions
Because
The sodium has a +1 charge and the chloride has a -1 charge and
they are hydrated by the water molecules

18. What is the molarity if a 500 mL solution
contains 20 g of CaBr2?
a. 0.1 M
b. 0.2 M
c. 0.5 M
d. 1 M
e. 5 M
19. How many moles of sulfate ions are in 200
mL of a 2 M sodium sulfate solution?
a. 0.2 mol
b. 0.4 mol
c. 0.6 mol
d. 0.8 mol
e. 1.0 mol
20. A 0.5 m solution could be prepared by
dissolving 20 g NaOH in
a. 0.5 L water
b. 0.5 kg water
c. 1 L water
d. 1 kg water
e. 2 L water
21. What volume of water would be needed to
dilute 50 mL of a 3 M HCl solution to 1 M?

a. 25 mL
b. 50 mL
c. 75 mL
d. 100 mL
e. 150 mL

22. About how many grams of sodium chloride
would be dissolved in water to form a 0.5
M solution in 500 mL solution?
a. 7
b. 29
c. 14.5
d. 58
e. 112
23. A one liter solution of 2 M NaOH can be
prepared with
a. 20 g NaOH
b. 40 g NaOH
c. 60 g NaOH
d. 80 g NaOH
e. 100 g NaOH
24. What is the molarity of a 10 mL solution in
which 3.7 g KCl are dissolved?
a. 0.05 M
b. 0.1 M
c. 1 M
d. 5 M
e. 10 M
25. A solution of 10 M NaOH was used to
prepare 2 L of 0.5 M NaOH. How many

mL of the original NaOH solution are
needed?
a. 10 mL
b. 100 mL
c. 1000 mL
d. 200 mL
e. 2000 mL

26. A 1 molal solution of NaCl results when
58.5 g of sodium chloride is dissolved in
a. One liter of water
b. 100 mL of water
c. one kilogram of water
d. 100 g of water
e. one cubic meter of water
27. A small crystal of NaCl is added to a
sodium chloride solution resulting in the
precipitation of more than 1 gram of
sodium chloride. This solution had been
a. Unsaturated
b. Saturated
c. Supersaturated
d. Dilute
e. Concentrated
28. Sodium chloride would be most soluble in
a. Ether
b. Benzene
c. Water
d. Carbon tetrachloride
e. Gasoline

29. Which of the following would produce a
highly conductive aqueous solution?
a. Cyclohexane
b. Hydrochloric acid
c. Benzene
d. Sucrose
e. Acetic acid


30. A 10% solution of HNO3 would be
produced by dissolving 63 g HNO3 in how
many mL water?
a. 100
b. 300
c. 567
d. 630
e. 1000
31. What is the boiling point of an aqueous
solution containing 117 g NaCl in 1000 g
H2O? Kb = 0.52 oC kg/mol
a. 98.96 oC
b. 99.48 oC
c. 100.52 oC
d. 101. 04 oC
e. 102.08 oC
32. Which of the following sequences lists the
relative sizes of particles in a water mixture
from smallest to largest?
a. Solutions, suspensions, colloids
b. Solutions, colloids, suspensions

c. Colloids, solutions, suspensions
d. Colloids, suspensions, solutions
e. Suspensions, colloids, solutions
33. A compound which, when dissolved in
water, barely conducts electrical current
can probably be
a. A strong electrolyte
b. An ionic salt
c. A strong acid
d. A strong base
e. None of the above
34. How many grams of HCl must be added to
500 mL water to produce a solution that
freezes at -1.86 oC? (molal freezing
constant = 1.86 oC kg/mol)
a. 4.6
b. 9.1
c. 18.3
d. 36.5
e. 73.0
35. A solution can be both
a. Dilute and concentrated
b. Saturated and dilute
c. Saturated and unsaturated
d. Supersaturated and saturated
e. None of these
36. The solubility of a solute indicates
a. The temperature of the solution
b. The quantity of solvent
c. The quantity of solute

d. The nature of the solute & solvent
e. All of these
37. A 10% solution of NaCl means that in 100
g of solution there is
a. 5.85 g NaCl
b. 58.5 g NaCl
c. 10 g NaCl
d. 94 g NaCl
38. The molarity of a solution made by placing
98 g H2SO4 in sufficient water to make 500
mL of solution is
a. 0.5
b. 1
c. 2
d. 3

39. If 684 g sucrose (MM = 342 g) is dissolved
in 2000 g H2O (essentially 2 L), what will
be the freezing point of this solution?
a. -0.51 oC
b. -1.86 oC
c. -3.72 oC
d. -6.58 oC
40. Ten grams of sodium hydroxide dissolved
in 1 L of water makes a solution that is
a. 0.25 M
b. 0.5 M
c. 1 M
d. 1.5 M
e. 4 M

41. How much water, in liters, must be added
to 0.5 L of 6 M HCl to make it 2 M?
a. 0.33
b. 0.5
c. 1
d. 1.5
e. 2
42. How many grams of NaOH are needed to
make 100 g of a 5 % solution?
a. 2
b. 5
c. 20
d. 40
e. 95
43. What is the boiling point of water at the top
of a mountain?
a. 100 oC
b. > 100 oC since the pressure is less
than at ground level
c. < 100 oC since the pressure is less
than at ground level
d. > 100 oC since the pressure is greater
than at ground level
e. < 100 oC since the pressure is greater
than at ground level
44. 1 mol NaCl in 1000 g H2O will change the
boiling point of water to
a. 100.51 oC
b. 101.04 oC
c. 101.53 oC

d. 101.86 oC
e. 103.62 oC
45. To what volume, in mL, must 50.0 mL of
3.50 M H2SO4 be diluted in order to make
2 M H2SO4?
a. 25
b. 60.1
c. 87.5
d. 93.2
e. 101
46. What is the molar mass of a non-ionizing
solid if 10 g of this solid, dissolved in 100 g
of water, formed a solution that froze at 1.21 oC?
a. 0.65 g
b. 6.5 g
c. 130 g
d. 154 g
e. 265 g

47. What is the melting point of 0.2 L water
containing 6.20 g C2H6O2?
a. -1.86 oC
b. -0.93 oC
c. 0 oC
d. 0.93 oC
e. 1.86 oC
48. Which of the following are TRUE?
i. Adding a solute raises the vapor
pressure & boiling point
ii. The change in boiling & freezing point

depends on molality.
iii. The number of solute particles in a
solvent is an important factor in
determining the boiling point elevation
a. i only
b. ii only
c. i and ii
d. ii and iii
e. i, ii and iii
Answers:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.

21.
22.
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24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
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48.

D

A
A
D
B
E
D
C
B
A
B
TF
T T CE
FT
TF
T T CE
T T CE
B
B
D
D
C
D
D
B
C
C
C
B
C
E

B
E
B
B
E
C
C
B
A
C
B
C
B
C
D
B
D