1. Which graph represents the relationship between
solubility and temperature of most gases, such as NH
3 , in water?
A)
B)
C)
D)
3. In a beaker is a clear solution containing 20.g of
KClO 3 in 100 g of water at 20°C.
E)
This solution is
2. How many grams of solute are undissolved after 100.
grams of KNO 3 are added and mixed well with 100. g
of H2O at 40 ° C?
A) 36
B) 40
C) 64
D) 100
E) none
A) unsaturated
C) supersaturated
E) weak
B) saturated
D) strong
4. In a beaker is a clear solution containing 50.g of NH 4
Cl in 100 g of water at 50°C.
6. Which compound is the most soluble at 20°C?
A)
B)
C)
D)
E)
7. What is the net ionic equation for the reaction
between potassium iodide solution, KI (aq), and silver
nitrate solution, AgNO 3 (aq)?
This solution is
A) unsaturated
C) supersaturated
E) weak
B) saturated
D) strong
5. Which polyatomic ion combines with metallic ions to
form salts, all of which are soluble in water?
A) NO 3–
C) SO 42–
E) Cl –
Substance A
Substance B
Substance C
Substance D
It cannot be determined from the information
given.
B) NH 4+
D) CH 3COO–
A)
B)
C)
D)
E)
K+ (aq) + I –(aq) ® KI(s)
K+ (aq) + NO3–(aq) ® KNO3(s)
Ag+ (aq) + NO3–(aq) ® AgNO3(s)
Ag+ (aq) + I –(aq) ® AgI(s)
KI(aq) + AgNO 3(aq) ® AgI(s) + KNO 3(aq)
8. Note the chart of interactions of equal volumes of
various 0.100 M aqueous solutions. (Symbols of
elements or ions have been replaced by capital letters,
and soluble products are indicated.) What is the
formula of the precipitate?
A) AX
B) BY
C) CX
D) DY
E) XY
9. A white precipitate results when lead nitrate solution
reacts with sodium chloride solution. A similar
precipitate results when lead nitrate solution reacts
with hydrochloric acid. What is the formula of the
precipitate?
A) PbH 2
C) NaNO3
E) PbCl 2
B) HNO3
D) Pb(NO 3) 2
A) maximum number of grams of solute that can
be dissolved in 100 g of solvent at a specific
temperature
B) minimum number of grams of solute that can
dissolve in 100 g of solvent to produce an
unsaturated solution
C) minimum number of grams of solvent that can
dissolve 100 g of solute to produce an saturated
solution
D) ability of a solute to dissolve in various
solvents at a specified temperature
E) ability of a solvent to dissolve various solutes at
a specified temperature
g of water and
A)
B)
C)
D)
E)
raise the pressure
raise the temperature
evaporate some of the water
add a crystal of potassium nitrate
add a crystal of another salt
14. Which statements are correct?
10. Solubility is defined as the
11. A mixture of
well shaken.
13. How would a saturated solution of KNO 3 be made
unsaturated?
g of table salt is
I
II
Any solid dissolves readily in any liquid.
When a solute dissolves in a solvent, the
inter–ionic or–molecular forces of both have
to be overcome.
III
All solid solutes break down into molecules
when in solution.
IV
Some solids separate into molecules while
others separate into ions as they dissolve.
A) I and II only
C) II and III only
E) III and IV only
B) I and III only
D) II and IV only
15. At 20°C, 144 grams of KI dissolves in 100 cm 3 of
water, and 0.068 g of PbI 2 dissolves in this amount
of water. A solution containing
144 g KI/100 cm3 H2O at 20°C is
When stirring produces no more change, the total
mass of the solution phase in the container is
A)
C)
E)
B)
D)
12. A salt forms a saturated solution containing 15.0%
solute by mass. The solubility of the salt is
A)
B)
C)
D)
E)
11.3 g solute/100 g of solvent
12.8 g solute/100 g of solvent
15.0 g solute/100 g of solvent
17.6 g solute/100 g of solvent
19.2 g solute/100 g of solvent
A)
B)
C)
D)
E)
dilute and saturated
dilute and unsaturated
concentrated and saturated
concentrated and unsaturated
concentrated and supersaturated
16. The solubility of PbI2 in water at 20°C is 0.07 g/100
g H2O. When the temperature of the solution is
raised to 30°C, the solution becomes
A) dilute.
C) unsaturated.
E) supersaturated.
B) saturated.
D) concentrated.
17. Which solution is the most concentrated?
A) 1.0 mole of solute dissolved in 1.0 liter of
solution
B) 2.0 moles of solute dissolved in 3.0 liters of
solution
C) 4.0 moles of solute dissolved in 8.0 liters of
solution
D) 6.0 moles of solute dissolved in 4.0 liters of
solution
E) 8.0 moles of solute dissolved in 5.0 liters of
solution
18. All solutions are
A) liquids
C) heterogeneous
E) saturated
B) homogeneous
D) pure substances
19. The density of water, H 2O, is greater than that of
octane,
C8H18, because
A) water has a higher boiling point than octane.
B) the molecular mass of water is smaller than that
of octane.
C) there are no Van der Waals forces acting
among octane molecules.
D) intermolecular hydrogen bonding, present in
water, is absent in octane.
E) water is a polar molecule while octane is
nonpolar.
20. How many phases are in a reaction vessel which
holds a saturated solution of common salt in water
and excess salt?
A)
B)
C)
D)
E)
1
2
3
4
It cannot be determined.
22. What mass of HNO3 (MM = 63) is present in 50. mL
of a 1.5 M solution?
A) 2.1 g
C) 7.5 g
E) 18.9 g
B) 4.7 g
D) 15.0 g
23. A sample of 40. mL of 0.20 M NaI contains how
many moles of iodide ion?
A) 0.0080 moles
C) 0.20 moles
E) 8.00 moles
B) 0.040 moles
D) 0.40 moles
24. An aqueous solution of concentrated HBr contains
48% HBr (MM = 80.9) by mass. The density of the
solution is 1.50 g•mL –1. What is the molarity of the
HBr solution?
A) 5.9 M
C) 11.4 M
E) 40.0 M
B) 8.9 M
D) 18.5 M
25. What is the
in an aqueous solution prepared by
adding
of
to sufficient water to make
of solution?
A)
C)
E)
B)
D)
26. Which aqueous solution has the same ion molarity
as 1.0 M MgCl2?
A) 1.0 M FeSO4
C) 1.5 M KI
E) 1.0 M NaOH
B) 2.0 M KCl
D) 0.50 M NH 4Cl
27. How many grams of calcium are contained in 1000
grams of a 3 molal solution of calcium bromide
21. The graph is a plot of data obtained during the
distillation of a solution. How many components are
in the initial solution?
A) 40 g
C) 120 g
E) 600 g
B) 80 g
D) 300 g
28. A solution contains 58 grams of NaCl in 5.6 moles
of water, what is the solution's molality?
A) 1
B) 2
C) 3
D) 4
E) 5
A) 3.32 m
C) 9.92 m
E) 15.18 m
B) 5.80 m
D) 12.62 m
29. What would be the molality of a solution containing
119 g of KBr dissolved in 500 g of water?
A) .5 m
C) 1.5 m
E) 2.5 m
B) 1 m
D) 2 m
30. If a 750g solution of sodium bromide is 2 molal,
how many grams of NaBr does it contain?
A) 53 g
C) 103 g
E) 173 g
B) 69 g
D) 155 g
31. A solution contains 174 grams of lithium bromide in
360 grams of water, what is the mole fraction of
lithium bromide?
A) .05
B) .09
C) .10
D) .48
E) 11
32. If 116 g of sodium chloride are dissolved in 1800 g
of water, what is the mole fraction of NaCl?
A) 0.0098
B) 0.0143
C) 0.0196
D) 0.0230
E) none of the above
33. A solution contains 3 moles of CuBr 2 in 360 grams
of water. What is the mass percent concentration of
CuBr2?
A) 9.0%
C) 28.6%
E) 47.4%
B) 25.0%
D) 40.0%
34. If a solution contains 4 moles of MgCl 2 in 40 moles
of water, what is the mass percent concentration of
MgCl 2?
A) 17.6%
C) 27.0%
E) 34.6%
B) 21.2%
D) 31.5%
35. Which sugar solution has the highest boiling
temperature?
A)
B)
C)
D)
E)
0.50 mol sugar / 500. g H 2O
0.50 mol sugar / 2.0 kg H 2O
1.00 mol sugar / 500. g H 2O
4.00 mol sugar / 10.0 kg H 2O
50.0 mol sugar/ 100. kg H 2O
36. Water is boiling in a beaker. What might be done to
raise the boiling temperature?
A)
B)
C)
D)
Dissolve sugar in the water.
Use a wire gauze to distribute the heat.
Dissolve ethyl alcohol (ethanol) in the water.
Increase the heating rate with a more efficient
burner.
E) Increase the temperature of the flame with a
different fuel.
37. What is the boiling point of a solution of 93 grams of
the nonelectrolyte ethylene glycol, C2H4(OH)2,
(molar mass 62), mixed with 500 grams of water?
(The Molal boiling point elevation constant for
water is 0.52°C•m -1 )
A) 99.48°C
C) 100.78°C
E) 101.56°C
B) 100.26°C
D) 101.04°C
38. Mixtures are made, each of which has 1.0 mol of
solute added to 1.0 kg of water.
Which same solution has all of these attributes:
I) the highest boiling temperature,
II) the lowest freezing temperature,
III) the best conductor of electricity?
A) BaCO 3
C) Ag2CO 3
E) Na2CO 3
B) CaCO 3
D) NaNO3
39. What is the freezing temperature of a 2.0 molal
solution of KBr in water?
(The Molar freezing point deppresion constant for
water is 1.86°C•m –1)
A) –0.47°C
C) –1.86°C
E) –7.44°C
B) –0.93°C
D) –3.72°C
40. A solution consists of 200. g of a nonelectrolytic
solute dissolved in 500. g of water. It freezes at
–9.30°C. What is the molecular weight of the solute?
(The Molal freezing point depression constant for
water is 1.86°C•m –1)
A) 40.0 B) 80.0 C) 200. D) 400. E) 500.
41. I. Addition of antifreeze to water lowers the freezing
point of the solution
44. I. An aqueous salt solution is a good conductor of
electricity
BECAUSE
II. the addition of antifreeze lowers the vapor
pressure of the water.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
42. I. Water boils at a higher temperature at low
altitudes than at high altitudes
BECAUSE
II. the solution contains positive and negative ions.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
45. I. Addition of a non-volatile solute to a solvent
causes the freezing point of the solution to be
lowered
BECAUSE
II. the atmospheric pressure decreases as the altitude
increases.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
43. I. At standard pressure, water has a higher boiling
point than alcohol
BECAUSE
II. the solute is always molecular.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
46. I. Antifreeze dissolved in water elevates the boiling
point
BECAUSE
BECAUSE
II. water has stronger intermolecular bonds.
II. the antifreeze molecules prevent the water
molecules from escaping to the atmosphere.
A)
B)
C)
D)
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
47. I. Antifreeze dissolved in water elevates the freezing
point
49. I. Sugar dissolved in a polar solvent, such as water,
will be a good electrical conductor
BECAUSE
II. the antifreeze molecules prevent the water
molecules from crystallizing.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
48. I. Ammonia gas will escape from a saturated water
solution when heated
BECAUSE
II. sugar dissolves in water to form ions.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
50. I. Sodium chloride in water is considered a
non-electrolyte
BECAUSE
BECAUSE
II. the solubility of gases decreases when the
temperature increases.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
II. the solution of an electrolyte conducts an electric
current.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a
correct explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I