Ch 13 Solutions
STUDY GUIDE
Name___________________________________
Accelerated Chemistry
SCANTRON
No-Calculators Allowed
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MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) The tragedy at Lake Nyos in Cameroon, West Africa, was caused by:
A) the release of excessive amounts of carbon dioxide that had been dissolved in the water at
the bottom of the lake.
B) the release of excess water stored in the volcanic lake which flooded the village below.
C) the release of excessive amounts of nitrogen gas that had been dissolved in the water at
the bottom of the lake.
D) the release of excessive amounts of oxygen gas that had been dissolved in the water at the
bottom of the lake.
1)
2) Which of the following substances is NOT a solution?
A) brass
B) vodka
C) copper
2)
3) Which of the following substances is NOT a solution?
A) humid air
B) oxygen
C) beer
D) air
3)
D) steel
4) Which of the following substances is NOT a solution?
A) sea water
B) soda
C) homogenized milk
D) bronze
4)
5) Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink
composed of water. What is the solute in this type of martini?
A) alcohol
B) olive
C) ice
D) water
5)
6) The oxygen in the air we breath is classified as:
A) the solvent in a homogeneous gas mixture.
B) the solute in a homogeneous gas mixture.
C) the solute in a heterogeneous gas-liquid mixture.
D) the solvent in a simple mixture.
6)
7) Hexane, a nonpolar solvent, will dissolve which of the following substances?
A) ammonium acetate
B) oil
C) sodium chloride
D) none of the above
7)
8) Which of these compounds would you expect to be least soluble in water?
A) NH3
B) CH3 O H
C) N 2
8)
9) In order for a solute to dissolve in solution:
A) the solute-solvent forces must equal the solute-solute forces.
B) the polarity of the solute and solvent must be opposite.
C) the solute-solute forces must be greater than the solute-solvent forces.
D) the solute-solvent forces must be greater than the solute-solute forces.
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D) NaCl
9)
10) If the solubility of sodium acetate (Molar mass = 82 g/mol) is 76 grams per 100 grams of water,
which of the following solutions would be considered supersaturated?
A) 8.5 moles of sodium acetate dissolved in 1 L of water
B) 1.2 moles of sodium acetate dissolved in 200 mL of water
C) 5.5 moles of sodium acetate dissolved in 500 mL of water
D) 1.8 moles of sodium acetate dissolved in 300 mL of water
10)
11) If the solubility of sodium chloride is 36 grams per 100 grams of water, which of the following
solutions would be considered unsaturated?
A) 3.25 moles of NaCL dissolved in 500 ml of water
B) 5.8 moles of NaCl dissolved in 1 L of water
C) 1.85 moles of NaCl dissolved in 300 ml of water
D) none of the above
11)
12) The solubility of Pb(NO3 ) 2 is 55 grams per 100 g H2 O at 20°C. Which term would properly
12)
describe a solution where 44 grams of Pb(NO3 ) 2 is added to 100 grams of water at this
temperature?
A) saturated
B) unsaturated
C) supersaturated
D) insoluble
13) If you prepare a solution by adding sufficient amount of solute so that after heating and
cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the
solution would be considered ________.
A) unsaturated.
B) thermally saturated.
C) saturated.
D) supersaturated.
13)
14) Which of the following compounds is a strong electrolyte?
A) NaCl
B) NaC 2 H 3 O2
C) NH 4 Cl
14)
15) Which of the following compounds is a strong electrolyte?
A) NaC 2 H 3 O2
B) C 6 H 12O6
C) C 7 H 14O5
16) The solubility of solids in water:
A) decreases with increasing temperature.
C) increases with increasing temperature.
D) all of the above
15)
D) C 4 H 8 O2
16)
B) is independent of the temperature.
D) none of the above
17) The solubility of solids in water:
A) increases with increasing pressure above solution.
B) is independent of pressure above solution.
C) decreases with increasing pressure above solution.
D) Solids are not soluble in water.
E) none of the above
17)
18) When an ionic compound dissolves in water:
A) the negative end of water dipoles attract the positive ions.
B) the positive end of water dipoles attract the negative ions.
C) the solvent-solute attractive forces overcome the solute-solute attractions.
D) all of the above (A, B, and C) occurs.
18)
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19) Which among the following is NOT true about the solubility of a solid in water?
A) Solid crystallizes when a saturated solution is prepared at a higher temperature and then
cooled.
B) A saturated solution prepared at a lower temperature becomes unsaturated when heated
to a higher temperature.
C) The solubility generally increases as temperature increases.
D) none of the above
19)
20) 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) none of the above
20)
21) The solubility of gases in water:
A) decreases with increasing temperature.
C) is independent of temperature.
21)
B) increases with increasing temperature.
D) gases are not soluble in water.
22) The solubility of a gas in a liquid can always be increased by:
A) decreasing the polarity of the solvent.
B) increasing the temperature of the solvent.
C) decreasing the pressure of the gas above the solvent.
D) increasing the pressure of the gas above the solvent.
22)
23) A solution is saturated in both nitrogen gas (N2 ) and sodium iodide (NaI) at 50°C. When the
23)
solution is cooled to 25°C, which of the following is most likely to occur?
A) Some nitrogen gas bubbles out of solution.
B) Some sodium iodide will precipitate out of solution.
C) Both A) and B) will happen.
D) Nothing will happen.
24) When preparing sodium hydroxide solution, it is best to use water that does not contain any
dissolved carbon dioxide as it reacts with the sodium hydroxide. Removing the carbon dioxide
can be accomplished by:
A) using water fresh out of the purification system.
B) vigorously stirring the solution.
C) boiling the water.
D) Nothing can be done to remove dissolved gases.
24)
25) We dissolve 2.45 g of sugar in 200.0 g water. What is the mass percent of sugar in the solution?
A) 1.21%
B) 2.42%
C) 1.23%
D) 123%
25)
26) A solution contains 100.0 g water, 10.0 g NaCl, and 15.0 g methanol. What is the weight
percent of methanol in the solution?
A) 8.00%
B) 15.0%
C) 10.0%
D) 12.0%
26)
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27) What is the mass percent of a solution prepared by dissolving 18.9 grams of solid into
39.5 grams of water?
A) 32.4%
B) 47.8%
C) 58.4%
D) The identity of the compound must be known.
E) none of the above
27)
28) What is the mass percent of an ammonium carbonate solution prepared by dissolving
33.2 grams of solid into 39.5 grams of water?
A) 84.1%
B) 45.7%
C) 54.3%
D) 72.7%
28)
29) What is the mass percent of a sodium fluoride solution prepared by dissolving 0.64 moles of
sodium fluoride into 63.5 grams of water?
A) 42.3%
B) 70.3%
C) 29.7%
D) none of the above
29)
30) How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of
NaF?
A) 239
B) 55.9
C) 31.1
D) none of the above
30)
31) How many moles of NaF are in 34.2 grams of a 45.5% by mass NaF solution?
A) 0.371
B) 75.2
C) 0.814
D) 15.6
31)
32) What is the molarity of a solution prepared by dissolving 10.7 g NaI in 0.250 L?
32)
A) 0.286
B) 42.8
C) 0.0714
D) 2.86 × 10-4
33) You need to prepare 2.00 L of 0.100 M Na2 CO3 solution. The best procedure is to weigh out
A) 21.2 g Na2 CO3 and add 2.00 L of water to it.
B) 21.2 g Na2 CO3 and add water until the final solution has a volume of 2.00 L.
C) 10.6 g Na2 CO3 and add 2.00 L of water to it.
D) 10.6 g Na2 CO3 and add water until the final solution has a volume of 2.00 L.
33)
34) Given that you wished to use exactly 0.325 mole of NaCl to prepare a 2.50 M NaCl solution,
how many milliliters of solution must you prepare?
A) 0.130 mL
B) 130. mL
C) 7.69 mL
D) 0.813 mL
34)
35) How many moles of KOH are contained in 750. mL of 5.00 M KOH solution?
A) 6.67 mol
B) 3.75 × 103 mol
C) 3.75 mol
D) 56.1 mol
35)
36) What is the molarity of a solution prepared by dissolving 54.3 g of Ca(NO3 ) 2 into 355 mL of
water?
A) 0.331 M
B) 0.117 M
C) 0.932 M
D) 1.99 M
36)
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37) A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final
volume of 3.00 liters. The molarity of the final solution is ________.
A) 1.00 M
B) 0.500 M
C) 2.25 M
D) 0.750 M
37)
38) How many grams of KCl are needed to make 50.0 mL of 2.45 M KCl?
A) 0.123
B) 91.3
C) 9.13
D) none of the above
38)
39) How many grams of LiF would be present in 575 mL of 0.750 M LiF solution?
A) 19.9
B) 11.2
C) 0.0338
D) 33.8
39)
40) How many liters of a 2.18 M solution can be made from 200.0 g K2 S?
A) 1.20
B) 0.252
C) 1.81
40)
41) A 0.15 M solution of BaCl2 contains:
D) 0.832
41)
A) 0.30 M Ba2+ ions and 0.30 M Cl- ions.
C) 0.15 M Ba2+ ions and 0.30 M Cl- ions.
B) 0.15 M Ba2+ ions and 0.15 M Cl- ions.
D) 0.30 M Ba2+ ions and 0.15 M Cl- ions.
42) What are the ion concentrations in a 0.12 M solution of AlCl3 ?
A) 0.12 M Al3+ ions and 0.040 M Cl- ions
C) 0.040 M Al3+ ions and 0.040 M Cl- ions
42)
B) 0.12 M Al3+ ions and 0.36 M Cl- ions
D) 0.36 M Al3+ ions and 0.12 M Cl- ions
43) Which solution below contains the highest total quantity of dissolved sodium ions?
A) 50.0 mL of 8.0 M NaOH
B) 100. mL of 4.0 M NaCl
C) 50.0 mL of 2.0 M Na3 PO4
43)
D) 75.0 mL of 3.0 M Na2 SO4
44) After you have completed the task of diluting a solution, which statement below must be
TRUE?
A) The new solution has more volume but has a lower concentration than before.
B) The new solution has less volume but has a lower concentration than before.
C) The new solution has less volume but has a higher concentration than before.
D) The new solution has more volume but has a higher concentration than before.
44)
45) Oftentimes solubility of a compound limits the concentration of the solution that can be
prepared. Use the solubility data given with each compound shown below to determine which
compound would allow the preparation of a 10.0 Molar solution.
A) NaNO3 (solubility = 89.0 g/100 g H2 O)
B) NH4 Cl (solubility = 41.1 g/100 g H2 O)
45)
C) KCl (solubility = 34.0 g/100 g H2 O)
D) AgNO3 (solubility = 122 g/100 g H2 O)
46) What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a
final volume of 1.20 L?
A) 0.350 M
B) 3.50 M
C) 0.504 M
D) 0.420 M
46)
47) What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
A) 0.560 mL
B) 560. mL
C) 257 mL
47)
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D) 21.9 mL
48) What volume of 9.00 M nitric acid is needed to make 6.50 L of 1.25 M solution?
A) 903 mL
B) 1.10 L
C) 1.73 L
D) 748 mL
48)
49) What molarity should the stock solution be if you want to dilute 25.0 mL to 2.00 L and have
the final concentration be 0.103 M?
A) 4.12 M
B) 8.24 M
C) 0.243 M
D) 0.206 M
49)
50) If you add 4.00 mL of pure water to 6.00 mL of 0.750 M NaCl solution, what is the
concentration of sodium chloride in the diluted solution?
A) 1.13 M
B) 0.250 M
C) 0.500 M
D) 0.450 M
50)
51) How many grams of barium sulfate are produced if 25.34 mL of 0.113 M BaCl2 completely
51)
react given the reaction:
BaCl2 (aq) + Na 2 SO4 (aq)
A) 0.668
BaSO4 (s) + 2NaCl (aq)
B) 1039
C) 26.3
D) 5.90
52) What is the concentration of sodium chloride in the final solution if 25.34 mL of 0.113 M BaCl2
52)
completely reacts and the total volume of the reaction is 110.4 mL, given the reaction:
BaCl2 (aq) + Na 2 SO4 (aq)
A) 0.0259
BaSO4 (s) + 2NaCl (aq)
B) 0.667
C) 0.0519
D) 0.226
53) How many mL of 0.218 M sodium sulfate react with exactly 25.34 mL of 0.113 M BaCl2 given
the reaction:
BaCl2 (aq) + Na 2 SO4 (aq)
A) 5.52
BaSO4 (s) + 2NaCl (aq)
B) 2.86
C) 13.1
D) 24.6
54) How many milliliters of 0.755 M H2 SO4 solution is needed to react with 55.0 mL of 2.50 M
KOH solution?
Given: 2 KOH (aq) + H2 SO4 (aq)
2 H2 O (l) + K2 SO4 (aq)
A) 51.9 mL
53)
B) 182 mL
C) 17200 mL
55) Which of the following statements about colligative properties is FALSE?
A) The identity of the solute is not a factor.
B) The freezing point of a solution is lowered by the addition of salt.
C) The boiling point of a solution is increased by the addition of salt.
D) All of the above statements are true.
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54)
D) 91.1 mL
55)
56) In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl2 solution,
A) the CaCl2 solution has the higher boiling point and the lower freezing point.
56)
B) both solutions have the same boiling point and the same freezing point.
C) the NaCl solution has the higher boiling point and the CaCl2 solution has the lower
freezing point.
D) the CaCl2 solution has the higher boiling point and the NaCl solution has the lower
freezing point.
E) the NaCl solution has the higher boiling point and the lower freezing point.
57) What is the molality of a solution made by dissolving 14.7 g of C 6 H 12O6 into 150.0 ml of
57)
water? Assume the density of water is 1.00 g/mL.
A) 0.0816
B) 10.2
C) 0.544
D) 0.980
E) none of the above
58) What is the change in the boiling point of a solution made by dissolving 14.7 g of C6 H 12O6
into 150.0 ml of water? The density of water is 1.00 g/mL and Kb = 0.512°C/m.
58)
A) 5.22°C
B) 0.0418°C
C) 0.502°C
D) 0.279°C
E) none of the above
59) What is the change in the freezing point of a solution made by dissolving 14.7 g of C6 H 12O6
into 150.0 ml of water? The density of water is 1.00 g/mL and Kf = 1.86°C/m.
59)
A) 0.152°C
B) 1.01°C
C) 1.82°C
D) 18.97°C
E) none of the above
60) Why is NOT a good idea to drink seawater when people are lost at sea?
A) The semipermeable membrane protecting your stomach is ruptured during osmosis.
B) The seawater has fish urine in it and who wants to drink that?
C) The osmotic pressure builds up in the cells of your intestine until they potentially
rupture.
D) The high concentration of salt forces water out of the cells lining your stomach and
intestine.
E) none of the above
60)
61) What will happen if a healthy red blood cell is placed into a container of pure water?
A) The cell will remain unchanged.
B) The cell will totally dissolve in the water.
C) The cell will become swollen.
D) The cell will shrink.
E) none of the above
61)
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62) Solution A has a concentration of 0.10 M sugar and Solution B has a concentration of 0.20 M
sugar. If the two solutions are separated by a semipermeable membrane, which of the
following occurs during osmosis?
A) Sugar molecules move from B into A.
B) Solvent molecules move from B into A.
C) The molarity of A increases.
D) The molarity of B increases.
E) none of the above
62)
63) An osmosis cell is constructed of a "U" shaped tube with a semipermeable membrane
separating the two arms of the tube. Suppose a concentrated solution is placed in the left arm
of the U-tube, and a dilute concentration of the same substance is poured into the other arm to
the same height. After a period of time has elapsed, you would expect to find that
A) the level of the liquid in the right arm is now higher.
B) the level of liquid in the left arm is now higher.
C) the levels in both arms stay at the same height.
D) no molecules of any type cross the membrane.
E) none of the above
63)
64) Osmotic pressure is:
A) the pressure required to reverse the flow of solvent through a semipermeable membrane
during osmosis.
B) the pressure required to stop the flow of solvent from a region of high solute
concentration to a region of low solute concentration.
C) the pressure required to stop the rupture of the semipermeable membrane.
D) the pressure required to stop the flow of solvent from a region of low solute
concentration through a semipermeable membrane into a region of high solute
concentration.
E) none of the above
64)
65) Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL
of pure water.
A) 72.3
B) 47.0
C) 27.3
D) 37.6
E) none of the above
65)
66) Calculate the molarity of a KCl solution prepared by dissolving 0.525 moles of KCl in
250. mL of water.
A) 0.00210
B) 2.10
C) 2.02
D) 0.476
E) none of the above
66)
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67) Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of
500. mL.
A) 6.04
B) 0.331
C) 0.166
D) 0.663
E) none of the above
67)
68) How many moles of KCl are present in 95.3 mL of 2.10 M KCl?
A) 20.0
B) 0.200
C) 5.00
D) 0.0500
E) none of the above
68)
69) How many grams of KCl are present in 75.0 mL of 2.10 M KCl?
A) 117
B) 2.66
C) 11.7
D) 5.59
E) none of the above
69)
70) What volume (L) of 2.00 M KCl solution contains 25.0 g of KCl?
A) 0.335
B) 0.672
C) 1.49
D) 0.168
E) none of the above
70)
71) What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl
solution to a volume of 0.500 L?
A) 0.0167
B) 3.0
C) 0.600
D) 1.67
E) none of the above
71)
72) How many mL of 0.112 M Pb(NO3 ) 2 are needed to completely react with 25.0 mL of
72)
0.105 M KI?
Given: Pb(NO3 ) 2 (aq) + 2KI(aq)
PbI 2 (s) + 2KNO3 (aq)
A) 11.7
B) 5.85
C) 23.4
D) 0.147
E) none of the above
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73) Calculate the molality of a solution prepared by dissolving 19.9 g of KCl in 750.0 mL of water.
A) 0.267
B) 4.99
C) 0.356
D) 0.200
E) none of the above
73)
74) Given that the freezing point depression constant for water is 1.86°C kg/mol, calculate the
change in freezing point for a 0.907 m sugar solution.
A) 0.592°C
B) 2.05°C
C) 1.69°C
D) 0.488°C
E) none of the above
74)
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