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?. Whic
Trang 1SC2 – 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?
9 Which is the descriptive term that indicates there is a large quantity of
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
12 When a solute is added to pure water, the vapor
pressure of the water will decrease
Because All solutes dissociate into positive and negative ions
14 A salt dissolved in an organic solvent will be a good
electrical conductor
Because Salts will not dissolve appreciably in an organic solvent
15 A super saturated solution of glucose in boiling water
crystallizes as it cools
Because The solubility increases as the temperature decreases
16 Salt dissolved in water lowers the freezing point Because The change in freezing point is given by: Tf = iKfm
17 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
Trang 230 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 D
2 A
3 A
4 D
5 B
6 E
7 D
8 C
9 B
10 A
11 B
12 T F
13 T T CE
14 F T
15 T F
16 T T CE
17 T T CE
18 B
19 B
20 D
21 D
22 C
23 D
24 D
25 B
26 C
27 C
28 C
29 B
30 C
31 E
32 B
33 E
34 B
35 B
36 E
37 C
38 C
39 B
40 A
41 C
42 B
43 C
44 B
45 C
46 D
47 B
48 D