Unit 5 Study Guide
2.
In soda pop, CO2(g) is a ______________, and
water is the ______________.
A)
solute; solvent
B)
solvent; solute
C)
solution; solute
D)
solute; solution
E)
solvent; solution
Ans: A
3.
A mixture of sand and water is a(n)
______________.
A)
solution
B)
solvent
C)
solute
D)
aqueous solution
E)
none of these
Ans: E
4.
True or false? Approximately 38 g of NaCl can be
dissolved in 100 g of water at 25°C. A solution prepared by
adding 35 g of NaCl to 100 g of water at 25°C is
unsaturated.
A)
True
B)
False
Ans: A
6.
When a solvent has dissolved all the solute it can at
a particular temperature, it is said to be
A)
diluted
B)
unsaturated
C)
supersaturated
D)
saturated
E)
none of these
Ans: D
8.
An oven-cleaning solution is 40.0% (by mass)
NaOH. If one jar of this product contains 457 g of solution,
how much NaOH does it contain?
A)
1.14  103 g
B)
11.4 g
C)
183 g
D)
18.3 g
E)
none of these
Ans: C
9.
A nitric acid solution containing 71.0% HNO3 (by
mass) has a density of 1.42 g/mL. How many moles of
HNO3 are present in 2.02 L of this solution?
A)
64.1 mol
B)
32.3 mol
C)
22.8 mol
D)
3.09  10–2 mol
E)
none of these
Ans: B
13.
Determine the concentration of a solution made by
dissolving 24.8 g of sodium chloride in 750.0 mL of
solution.
A)
0.318 M
B)
33.1 M
C)
0.424 M
D)
0.566 M
E)
18.6 M
Ans: D
14.
If you mix 20.0 mL of a 3.00 M sugar solution with
30.0 mL of a 4.11 M sugar solution, you will end up with a
sugar solution of ________.
A)
3.55 M
B)
0.142 M
C)
6.11 M
D)
3.67 M
E)
9.17 M
Ans: D
15.
You have 250.0 mL of 4.00 M sugar solution. You
add 217.3 mL of water to this solution. Determine the
concentration of the sugar solution after the water has been
added.
A)
4.00 M
B)
2.39 M
C)
2.88 M
D)
2.14 M
E)
2.47 M
Ans: D
17.
Which of the following aqueous solutions contains
the greatest number of ions in solution?
A)
2.0 L of 1.50 M sodium phosphate
B)
2.0 L of 1.50 M magnesium chloride
C)
3.0 L of 1.50 M sodium chloride
D)
2.0 L of 2.00 M potassium fluoride
E)
1.0 L of 3.00 M sodium sulfate
Ans: A
19.
What is the minimum volume of a 2.42 M NaOH
solution needed to make 150.0 mL of a 0.800 M NaOH
solution?
A)
375 mL
B)
24.8 mL
C)
61.6 mL
D)
120. mL
E)
49.6 mL
Ans: E
22.
What volume of a 0.190 M Na2S solution contains
1.01 g of Na+ ions?
A)
0.231 L
B)
8.65 L
C)
4.32 L
D)
0.416 L
E)
0.116 L
Ans: E
35.
What volume of a 0.550 M solution of potassium
hydroxide can be made with 10.7 g of potassium hydroxide?
(Ignore significant figures for this problem.)
A)
19.5 mL
B)
347 mL
C)
191 mL
D)
2884 mL
E)
2.88 mL
Ans: B
24.
A 0.236-g sample of NaCl (molar mass = 58.44
g/mol) is dissolved in enough water to make 5.20 mL of
solution. Calculate the molarity of the resulting solution.
A)
0.777 M
B)
4.04  10–3 M
C)
1.29 M
D)
0.889 M
E)
0.633 M
Ans: A
37.
What mass of solute is contained in 417 mL of a
0.169 M magnesium fluoride solution?
A)
4.39 g
B)
70 g
C)
10.5 g
D)
1.13 g
E)
none of these
Ans: A
26.
A 54.5-g sample of SrCl2 is dissolved in 112.5 mL
of solution. Calculate the molarity of this solution.
A)
0.344 M
B)
3.06 M
C)
0.0387 M
D)
4.38 M
E)
none of these
Ans: B
38.
What mass of solute is contained in 30.0 mL of a
1.56 M potassium bromide solution?
A)
19.2
B)
5.57
C)
46.8
D)
2.54
E)
none of these
Ans: B
27.
A 86.17-g sample of NaCl is dissolved in 250.0 mL
of solution. Calculate the molarity of this solution.
A)
1.475 M
B)
344.7 M
C)
5.898 M
D)
7.131 M
E)
none of these
Ans: C
40.
A chemist needs 225 mL of 2.5 M HCl. What
volume of 12 M HCl must be dissolved in water to form this
solution? (Ignore significant figures for this problem.)
A)
10.8  102 mL
B)
15 mL
C)
7.5 mL
D)
21 mL
E)
47 mL
Ans: E
28.
Calculate the mass of silver nitrate (in grams) in a
145 mL solution of 4.71 M AgNO3. (Ignore significant
figures for this problem.)
A)
800 g
B)
0.800 g
C)
116 g
D)
30.8 g
E)
none of these
Ans: C
32.
The molarity of Cl– in 110. mL of a solution
containing 3.33 g of CaCl2 is
A)
0.273 M
B)
0.0300 M
C)
0.00330 M
D)
0.546 M
E)
0.366 M
Ans: D
43.
A 55.70-g sample of Ba(OH)2 is dissolved in
enough water to make 1.20 L of solution. How many
milliliters of this solution must be diluted with water in order
to make 1.00 L of 0.100 M Ba(OH)2? (Ignore significant
figures for this problem.)
A)
369 mL
B)
66.8 mL
C)
325 mL
D)
271 mL
E)
557 mL
Ans: A
44.
What volume of 18.0 M sulfuric acid must be used
to prepare 15.5 L of 0.188 M H2SO4? (Ignore significant
figures for this problem.)
A)
162 mL
B)
218 mL
C)
2.91 L
D)
82.4 mL
E)
none of these
Ans: A
46.
You have 3.00 L of a 2.31 M solution of NaCl(aq)
called solution A. You also have 2.00 L of a 2.00 M solution
of AgNO3(aq) called solution B. You mix these solutions
together, making solution C.
Calculate the concentration (in M) of Na+ ions in solution C.
A)
0M
B)
2.31 M
C)
3.47 M
D)
0.86 M
E)
1.39 M
Ans: E
48.
You have 3.00 L of a 3.74 M solution of NaCl(aq)
called solution A. You also have 2.00 L of a 2.00 M solution
of AgNO3(aq) called solution B. You mix these solutions
together, making solution C.
Calculate the concentration (in M) of Ag+ ions in solution C.
A)
0M
B)
1.44 M
C)
2.24 M
D)
0.800 M
E)
3.61 M
Ans: A
49.
You have 3.00 L of a 3.00 M solution of NaCl(aq)
called solution A. You also have 2.00 L of a 1.66 M solution
of AgNO3(aq) called solution B. You mix these solutions
together, making solution C.

Calculate the concentration (in M) of NO 3 ions in solution
C.
A)
0M
B)
0.664 M
C)
1.14 M
D)
1.66 M
E)
1.80 M
Ans: B
50.
You have two HCl solutions, labeled solution A
and solution B. Solution A has a greater concentration than
solution B. Which of the following statements is/are true?
A)
If you have equal volumes of both solutions,
solution B must contain more moles of HCl.
B)
If you have equal moles of HCl in both
solutions, solution B must have a greater volume.
C)
To obtain equal concentrations of both
solutions, you must add a certain amount of water
to solution B.
D)
Adding more moles of HCl to both solutions
will make them less concentrated.
E)
At least two of the above statements are
true.
Ans: B
52.
If you mix 40.0 mL of a 0.366 M solution of
K2CrO4 with 40.0 mL of a 0.366 M solution of AgNO3, what
mass of solid forms?
A)
4.86 g
B)
2.43 g
C)
2.84 g
D)
14.6 g
E)
7.32 g
Ans: B
54.
For the reaction between 200.0 mL of 0.100 M
silver nitrate and 95.00 mL of 0.100 M sodium chloride, the
concentration of silver ions in solution after the reaction is
complete is
A)
0.00 M. All of the silver ions are used up to
make the precipitate.
B)
0.100 M. The silver ions do not participate
in the chemical reaction and are considered
spectator ions.
C)
greater than 0.100 M. For every 1.0 mol of
silver nitrate there are 2.0 mol of silver ions in
solution.
D)
less than 0.100 M. Even though silver ions
do not react, they are diluted when mixed with the
sodium chloride solution.
E)
less than 0.100 M. Some, but not all, of the
silver ions are used to make the precipitate.
Ans: E
56.
Calculate the volume of 0.188 M HNO3 required to
neutralize 25.0 mL of 0.250 M NaOH.
A)
18.8 mL
B)
33.2 mL
C)
4.70 mL
D)
30.1 mL
E)
none of these
Ans: B
58.
In the following acid-base neutralization, 1.61 g of
the solid acid HC6H5O neutralized 11.61 mL of aqueous
NaOH solution base by the reaction
NaOH(aq) + HC6H5O(aq)
 H2O(l) + NaC6H5O(aq)
Calculate the molarity of the base solution.
A)
1.47 M
B)
17.1 M
C)
7.21 M
D)
0.139 M
E)
0.199 M
Ans: A
63.
Which of the following solutions contains the
smallest number of ions?
A)
555.7 mL of 1.0 M lithium nitrate
B)
386.4 mL of 2.0 M potassium hydroxide
C)
197.8 mL of 2.0 M iron(III) chloride
D)
233.4 mL of 1.0 M sodium sulfate
E)
At least two of the above contain the
smallest number of ions.
Ans: D
65.
How many moles of chloride ions are in 62.6 mL
of a 2.00 M aluminum chloride solution?
A)
0.125 mol
B)
0.0313 mol
C)
0.0417 mol
D)
0.751 mol
E)
0.376 mol
Ans: E
67.
15.0 mL of 0.30 M sodium phosphate solution
reacts with 20.0 mL of 0.23 M lead(II) nitrate solution. What
is the concentration of nitrate ions left in solution after the
reaction is complete?
A)
0.0 M
B)
0.13 M
C)
0.26 M
D)
0.066 M
E)
0.09 M
Ans: C
70.
You have three ammonium sulfate solutions on a lab
table in front of you. All of the solutions came from a 500.0mL volumetric flask containing 3.00 M ammonium sulfate.
Solution 1 contains 124.4 mL of the 3.00 M solution.
Solution 2 contains 55.8 mL of the 3.00 M solution.
Solution 3 contains 24.4 mL of the 3.00 M solution.
How many moles of ions does Solution 2 contain?
A)
0.167 mol
B)
1.17 mol
C)
0.502 mol
D)
0.335 mol
E)
0.251 mol
Ans: C
72.
You have three sodium carbonate solutions on a lab
table in front of you. All of the solutions came from a 500.0mL volumetric flask containing 3.00 M sodium carbonate.
Solution 1 contains 100.0 mL of the 3.00 M solution.
Solution 2 contains 50.0 mL of the 3.00 M solution.
Solution 3 contains 10.0 mL of the 3.00 M solution.
What is the new concentration of Solution 2 if 16.5 g of
solid sodium carbonate is added and dissolved? (Assume no
volume change.)
A)
3.11 M
B)
12.1 M
C)
1.91 M
D)
6.11 M
E)
0.611 M
Ans: D
74.
What mass of solute is contained in 50.0 mL of a
2.09 M potassium chloride solution?
A)
23.9 g
B)
1.78 g
C)
104.5 g
D)
7.79 g
E)
35.7 g
Ans: D