Exam
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) A solution containing a large concentration of dissolved ions can be classified as a(n) ________.
A) suspension
B) weak solution
C) unsaturated solution
D) solvent
E) electrolyte
1)
2) How many atoms of neon occupy a volume of 14.3 L at STP?
A) 9.45 × 1023 atoms
2)
B) 3.84 × 1023 atoms
C) 2.21 × 1025 atoms
D) 3.88 × 1024 atoms
E) 1.92 × 1025 atoms
3) Assuming that the pressure and quantity of a gas sample remain constant, what will be the final
volume of a 4.86 L sample of a gas at 281 °C which is cooled to 225 °C?
A) 2.92 L
B) 4.37 L
C) 5.19 L
D) 2.78 L
3)
4) An increase in the temperature of a solution usually
A) increases the solubility of a gas in the solution.
B) increases the boiling point.
C) decreases the solubility of a solid solute in the solution.
D) decreases the solubility of a liquid solute in the solution.
E) increases the solubility of a solid solute in the solution.
4)
5) How is the solubility of a solid affected by temperature?
A) As temperature goes up, the solubility goes up.
B) As temperature goes down, the solubility goes down.
C) As temperature goes up, the solubility goes down.
D) As temperature goes down, the solubility goes up.
E) both A and B
5)
6) Methanol, CH3 OH, can be classified as a __________.
6)
7) Which of the following interparticle attractions play a part in the formation of a solution?
A) answers A, B, and C play a part
B) solvent-solvent
C) solute-solute
D) solvent-solute
7)
A) solid
B) strong electrolyte
C) gas
D) weak electrolyte
E) nonelectrolyte
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8) In a solution, the solvent is ________.
A) always water
B) the substance present in the greatest amount
C) the substance being dissolved
D) always a liquid
8)
9) In a solution, solutes ________.
A) must be liquids
C) can be solids, liquids or gases
9)
B) cannot be solids
D) can be liquids or gases
10) Oil does not dissolve in water because
A) oil is hydrated.
B) oil is polar.
C) water is nonpolar.
D) water is saturated.
E) oil is nonpolar.
10)
11) The ideal gas equation cannot be written as ________.
11)
A)
B)
C) PV = nRT
D)
12) A gas under an initial pressure of 0.60 atm is compressed at constant temperature from 27 L to 3.0
L. The final pressure becomes ________.
A) 0.060 atm
B) 5.4 atm
C) 0.54 atm
D) 54 atm
12)
13) How is the solubility of a gas affected by temperature?
A) As temperature goes up, the solubility goes up.
B) As temperature goes up, the solubility stays the same.
C) As temperature goes down, the solubility goes up.
D) As temperature goes down, the solubility goes down.
E) both A and B
13)
14) What volume of 8.25 M HCl solution must be diluted to prepare 2.40 L of 0.500 M HCl solution?
A) 438 mL
B) 39.6 L
C) 145 mL
D) 0.256 L
14)
15) The volume of 2.3 g nitrogen gas at STP is ________.
A) 11.2 L
B) 22.4 L
15)
C) 1.8 L
D) 44.8 L
16) According to the kinetic theory of gases, particles of a gas
A) are very large.
B) lose their valence electrons.
C) move slowly.
D) decrease kinetic energy as temperature increases.
E) are very far apart.
17) As you rise higher in Earth's atmosphere, the atmospheric pressure
A) increases.
B) remains the same.
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16)
C) decreases.
17)
18) When KCl dissolves in water
A) the Cl- ions are attracted to dissolved K+ ions.
18)
B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule.
C) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.
E) the K+ ions are attracted to Cl- ions on the KCl crystal.
19) At 10°C, which is more concentrated a saturated solution of sodium nitrate, NaNO3 , or a
19)
saturated solution of sodium chloride? (See figure shown above )
A) At 10°C a saturated solution of sodium nitrate, NaNO3 , is more concentrated than a saturated
solution of sodium chloride, NaCl.
B) At 10°C a saturated solution of sodium chloride, NaCl, is more concentrated than a saturated
solution of sodium nitrate, NaNO3 .
C) At 25°C a saturated solution of sodium nitrate, NaNO3 , is more concentrated than a saturated
solution of sodium chloride, NaCl.
D) At 20°C a saturated solution of sodium nitrate, NaNO3 , is more concentrated than a saturated
solution of sodium chloride, NaCl.
20) Which solute graphed above has a solubility in water that does not markedly increase with
increasing temperature?
A) NaCl
B) NaNO3
C) KCl
D) LiCl
20)
21) Solubility of gases in water:
A) decreases with increasing pressure above solution.
B) is independent of pressure above solution.
C) increases with increasing pressure above solution.
D) Gases are not soluble in water.
E) none of the above
21)
22) Which type of compound is likely to dissolve in water?
A) all are correct
B) a highly polar compound
C) a salt
D) one with hydrogen bonds
22)
23) A solution in which the rate of crystallization is equal to the rate of dissolution is ________.
A) supersaturated
B) dilute
C) unsaturated
D) saturated
23)
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24) When the combined gas law is rearranged to solve for V2 , the following is the
24)
correct expression: V2 =
A) P1 V1 T2 /P2 T1
B) P1 V1 T1 /P2 T2
C) P2 T2 /P1 V1 T1
D) P1 V1 /T1 - P2 /T2
E) T2 T1 V1 /P2 P1
25) Salts incorporating all but one of the following ions are usually soluble in water. Which ion is the
exception?
A) PO4
B) CH3COO
C) K+
D) SO4
25)
26) In water, a substance that ionizes completely in solution is called a
A) nonconductor.
B) weak electrolyte.
C) semiconductor.
D) strong electrolyte.
E) nonelectrolyte.
26)
27) A solution is prepared by dissolving 2 g of KCl in 100 g of H2 O. In this solution, H2 O is the
27)
28) A tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?
A) 7.50 mmHg
B) 1.50 mmHg
C) 760 mmHg
D) 507 mmHg
E) 1 140 mmHg
28)
29) When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the
solution is
A) dilute.
B) unsaturated.
C) saturated.
D) nonpolar.
E) polar.
29)
30) How many equivalents are present in 5.0 moles of Al3+ ?
A) 1.3 Eq
B) 15 Eq
C) 3.0 Eq
30)
A) solvent.
B) solid.
C) solute.
D) solution.
E) ionic compound.
D) 0.67 Eq
E) 5.0 Eq
31) A student wishes to prepare 65.0 mL of 0.875 M HCl from 12.0 M HCl. What volume of the 12.0 M
HCl should he/she start with?
A) 4.74 mL
B) 9.28 mL
C) 18.2 mL
D) 4.65 mL
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31)
32) If the volume of a gas container at 32.0°C changes from 1.55 L to 755 mL, what will the final
temperature be?
A) 353°C
B) 273°C
C) -124°C
D) 149°C
E) none of the above
32)
33) A solution is made by dissolving 2.68 mole of KF in enough water to give a final volume of 1030
mL. What is the molarity of the solution?
A) 2.60 M
B) 0.125 M
C) 0.800 M
D) 1.52 M
33)
34) When solutions of KCl and Pb(NO3 ) 2 are mixed, a precipitate forms. Which of the following is the
34)
balanced equation for the double replacement reaction that occurs?
KNO3 (aq) + PbCl2 (s)
A) KCl(aq) + Pb(NO3 ) 2 (aq)
B) KNO3 (aq) + PbCl2 (s)
C) KCl(aq) + Pb(NO3 ) 2 (aq)
D) K+ (aq) + NO3 - (aq)
KCl(aq) + Pb(NO3 ) 2 (aq)
KNO3 (aq) + PbCl(s)
KNO3 (aq)
E) 2KCl (aq) + Pb(NO3 ) 2 (aq)
2 KNO3 (aq) + PbCl2 (s)
35) Which of the following is not soluble in water?
A) iron (III) hydroxide
C) ammonium sulfate
35)
B) potassium sulfide
D) iron (III) nitrate
36) 3.01 × 1023 molecules of methane gas will occupy ________ at STP.
A) 67.2 L
B) 11.2 L
C) 44.8 L
D) 22.4 L
36)
37) If the volume of a given gas sample doubles, what happens to the temperature of the gas? The
amount of gas and the pressure of the gas stay the same.
A) increase by a factor of 2
B) decrease by a factor of 2
C) stay exactly the same
37)
38) A gas occupies a volume of 480 mL at 127 °C and 140 mm Hg. What mathematical expression will
yield the correct volume at 177 °C and 400 mm Hg?
A) 480 × (140/400) × (400/450)
B) 480 × (400/140) × (450/400)
C) 480 × (400/140) × (400/450)
D) 480 × (140/400) × (450/400)
38)
39) Which one of the following compounds will NOT be soluble in water?
A) MgCl2
B) LiOH
C) NaNO3
D) BaSO4
39)
E) K2 S
40) Under which of the following conditions would you expect the highest solubility of oxygen gas in
water?
A) high temperature and low O2 pressure above the solution
B) The O2 solubility is independent of temperature and pressure.
C) low temperature and high O2 pressure above the solution
D) low temperature and low O2 pressure above the solution
E) high temperature and high O2 pressure above the solution
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40)
41) In a solution, the solvent
A) can be a solid, liquid, or gas.
B) is the substance present in the smallest concentration.
C) is a liquid.
D) is never a solid.
E) can be a liquid or gas.
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41)
Answer Key
Testname: EXAM 3 PRACTICE TEST
1) E
2) B
3) B
4) E
5) E
6) E
7) A
8) B
9) C
10) E
11) B
12) B
13) C
14) C
15) C
16) E
17) C
18) D
19) A
20) A
21) C
22) A
23) D
24) A
25) A
26) D
27) A
28) E
29) C
30) B
31) A
32) C
33) A
34) E
35) A
36) B
37) A
38) D
39) D
40) C
41) A
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