Chapter 4: Chemical Reactions and Solutions Stoichiometry
1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent).
Molecules of what type are present in the substance?
A)
neither polar nor nonpolar
B)
polar
C)
either polar or nonpolar
D)
nonpolar
E)
none of these
2. The interaction between solute particles and water molecules, which tends to cause a salt to
fall apart in water, is called
A)
hydration
B)
polarization
C)
dispersion
D)
coagulation
E)
conductivity
3. Consider two organic molecules, ethanol and benzene. One dissolves in water and the other
does not. Why?
A)
They have different molar masses.
B)
One is ionic, the other is not.
C)
One is an electrolyte, the other is not.
D)
Ethanol contains a polar O–H bond, and benzene does not.
E)
Two of these are correct.
4. Polar molecules have an unequal distribution of charge within the molecule.
5. Which of the following is a strong acid?
A)
HF
B)
KOH
C)
HClO4
D)
HClO
E)
HBrO
6. All of the following are weak acids except
A)
HCNO
B)
HBr
C)
HF
D)
HNO2
E)
HCN
7. Which of the following is not a strong base?
A)
Ca(OH)2
B)
KOH
C)
NH3
D)
LiOH
E)
Sr(OH)2
8. Which of the following is paired incorrectly?
A)
H2SO4 – strong acid
B)
HNO3 – weak acid
C)
Ba(OH)2 – strong base
D)
HCl – strong acid
E)
NH3 – weak base
9. The man who discovered the essential nature of acids through solution conductivity studies
is
A)
Priestly
B)
Boyle
C)
Einstein
D)
Mendeleev
E)
Arrhenius
10. A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the
following is true?
I. II.
A)
In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong
acid.
B)
In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak
acid.
C)
In both cases, HX is acting like a strong acid.
D)
In both cases, HX is acting like a weak acid.
E)
HX is not soluble in water.
11. An acid is a substance that produces OH– ions in water.
12. A 16.4-g sample of HF is dissolved in water to give 2.0 102 mL of solution. The
concentration of the solution is:
A)
0.82 M
B)
0.16 M
C)
0.08 M
D)
4.1 M
E)
8.2 M
13. 1.00 mL of a 3.50 10–4 M solution of oleic acid is diluted with 9.00 mL of petroleum
ether, forming solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum
ether, forming solution B. What is the concentration of solution B?
A)
3.50 10–6 M
B)
9.72 10–6 M
C)
7.00 10–5 M
D)
7.78 10–5 M
E)
7.00 10–6 M
14. 1.00 mL of a 4.05 10–4 M solution of oleic acid is diluted with 9.00 mL of petroleum
ether, forming solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum
ether, forming solution B. How many grams of oleic acid are 5.00 mL of solution B? (Molar
mass for oleic acid = 282 g/mol)
A)
5.71 10–6 g
B)
1.59 10–5 g
C)
2.28 10–2 g
D)
1.14 10–5 g
E)
5.71 10–4 g
15. How many grams of NaCl are contained in 350. mL of a 0.287 M solution of sodium
chloride?
A)
16.8 g
B)
5.87 g
C)
11.74 g
D)
100.5 g
E)
none of these
16. Which of the following aqueous solutions contains the greatest number of ions?
A)
400.0 mL of 0.10 M NaCl
B)
300.0 mL of 0.10 M CaCl2
C)
200.0 mL of 0.10 M FeCl3
D)
200.0 mL of 0.10 M KBr
E)
800.0 mL of 0.10 M sucrose
17. What mass of calcium chloride, CaCl2, is needed to prepare 3.950 L of a 1.49 M solution?
A)
294 g
B)
5.89 g
C)
41.9 g
D)
111 g
E)
653 g
18. A 38.1-g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this
solution.
A)
27.0 M
B)
2.14 M
C)
53.7 M
D)
0.339 M
E)
none of these
19. What mass of solute is contained in 256 mL of a 0.838 M ammonium chloride solution?
A)
11.5 g
B)
175 g
C)
16.3 g
D)
215 g
E)
3.27 g
20. A 74.28-g sample of Ba(OH)2 is dissolved in enough water to make 2.450 liters of solution.
How many mL of this solution must be diluted with water in order to make 1.000 L of
0.100 M Ba(OH)2?
A)
565 mL
B)
177 mL
C)
17.7 mL
D)
4.34 mL
E)
231 mL
21. What volume of 18 M sulfuric acid must be used to prepare 2.30 L of 0.145 M H2SO4?
A)
19 mL
B)
0.33 mL
C)
1.1 103 mL
D)
2.9 mL
E)
6.0 mL
22. How many grams of NaOH are contained in 5.0 102 mL of a 0.74 M sodium hydroxide
solution?
A)
15 g
B)
74 g
C)
0.37 g
D)
30 g
E)
370 g
23. An analytical procedure requires a solution of chloride ions. How many grams of NaCl must
be dissolved to make 1.95 L of 0.0561 M Cl–?
A)
3.28 g
B)
0.595 g
C)
6.39 g
D)
1.64 g
E)
12.8 g
24. The concentration of a salt water solution that sits in an open beaker decreases over time.
25. You have two solutions of chemical A. To determine which has the highest concentration of
A in molarity, what is the minimum number of the following you must know?
I.
the mass in grams of A in each solution
II.
the molar mass of A
III.
the volume of water added to each
solution
IV.
the total volume of the solution
A)
0
B)
1
C)
2
D)
3
E)
You must know all of them.
26. Diabetics often need injections of insulin to help maintain the proper blood glucose levels in
their bodies. How many moles of insulin are needed to make up 45 mL of 0.0062 M insulin
solution?
A)
0.00056 mol
B)
0.14 mol
C)
7.3 mol
D)
0.28 mol
E)
0.00028 mol
27. You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M
solution. You have much more of the 4.00 M solution and you add the solutions together.
Which of the following could be the concentration of the final solution?
A)
2.70 M
B)
3.00 M
C)
3.50 M
D)
6.00 M
E)
8.10 M
28. You have equal masses of different solutes dissolved in equal volumes of solution. Which of
the solutes would make the solution having the highest molar concentration?
A)
NaOH
B)
KCl
C)
KOH
D)
LiOH
E)
all the same
29. Which of the following do you need to know to be able to calculate the molarity of a salt
solution?
I. the mass of salt added
II. the molar mass of the salt
III. the volume of water added
IV. the total volume of the solution
A)
I, III
B)
I, II, III
C)
II, III
D)
I, II, IV
E)
You need all of the information.
30. A 230.0-mL sample of a 0.275 M solution is left on a hot plate overnight; the following
morning the solution is 1.29 M. What volume of solvent has evaporated from the 0.275 M
solution?
A)
49.0 mL
B)
63.3 mL
C)
181.0 mL
D)
230. mL
E)
279.0 mL
31. For the reaction 4FeCl2(aq) + 3O2(g) → 2Fe2O3(s) + 4Cl2(g), what volume of a 0.760 M
solution of FeCl2 is required to react completely with 6.36 1021 molecules of O2?
A)
5.26 103 mL
B)
10.7 mL
C)
10.4 mL
D)
18.5 mL
E)
6.02 mL
32. Phosphoric acid, H3PO4, is a triprotic acid. What is the total number of moles of H+
available for reaction in 2.50 L of 0.700 M H3PO4?
A)
0.233 mole
B)
2.10 mole
C)
0.583 mole
D)
3.00 moles
E)
5.25 moles
33. The following reactions:
Pb2+ + 2I– → PbI2
2Ce4+ + 2I– → I2 + 2Ce3+
HOAc + NH3 → NH4+ + OAc–
are examples of
A)
acid-base reactions
B)
unbalanced reactions
C)
precipitation, acid-base, and redox reactions, respectively
D)
redox, acid-base, and precipitation reactions, respectively
E)
precipitation, redox, and acid-base reactions, respectively
34. The following reactions
2K(s) + Br2(l) → 2KBr(s)
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
HCl(aq) + KOH(aq) → H2O(l) + KCl(aq)
are examples of
A)
precipitation reactions
B)
redox, precipitation, and acid-base, respectively
C)
precipitation (two) and acid-base reactions, respectively
D)
redox reactions
E)
none of these
35. The following reactions
ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s)
KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
are examples of
A)
oxidation-reduction reactions
B)
acid-base reactions
C)
precipitation reactions
D)
A and C
E)
none of these
36. All of the following reactions
2Al(s) + 3Br2(l) → 2AlBr3(s)
2Ag2O(s) → 4Ag(s) + O2(g)
CH4(l) + 2O2(g) → CO2(g) + 2H2O(g)
can be classified as
A)
oxidation-reduction reactions
B)
combustion reactions
C)
precipitation reactions
D)
A and B
E)
A and C
37. You have exposed electrodes of a light bulb in a solution of H2SO4 such that the light bulb is
on. You add a dilute solution and the bulb grows dim. Which of the following could be in
the solution?
A)
Ba(OH)2
B)
NaNO3
C)
K2SO4
D)
Cu(NO3)2
E)
none of these
38. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which
statement is correct?
A)
Both NaCl and CuS precipitate from solution.
B)
No reaction will occur.
C)
CuS will precipitate from solution.
D)
NaCl will precipitate from solution.
E)
A gas is released.
39. Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which
statement is correct?
A)
Both KNO3 and NH4SO4 precipitate from solution.
B)
A gas is released.
C)
NH4SO4 will precipitate from solution.
D)
KNO3 will precipitate from solution.
E)
No reaction will occur.
40. Which of the following salts is insoluble in water?
A)
Na2S
B)
K2CO3
C)
Pb(NO3)2
D)
CaCl2
E)
All of these are soluble in water.
41. How many of the following salts are expected to be insoluble in water?
sodium sulfide
ammonium sulfate
A)
none
B)
1
C)
2
D)
3
E)
4
42. When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. Its formula is:
A)
Cu(NH)3
B)
Cu(NO3)2
C)
Cu(OH)2
D)
Cu(NH3)22+
E)
CuO
43. Which of the following ions is most likely to form an insoluble sulfate?
A)
K+
B)
Li+
C)
Ca2+
D)
S2–
E)
Cl–
44. Which of the following compounds is soluble in water?
A)
Ni(OH)2
B)
K3PO4
C)
BaSO4
D)
CoCO3
E)
PbCl2
45. Which pair of ions would not be expected to form a precipitate when dilute solutions of each
are mixed?
A)
Al3+, S2–
B)
Pb2+, Cl–
C)
Ba2+, PO43–
D)
Pb2+, OH–
E)
Mg2+, SO42–
46. A solution contains the ions Ag+, Pb2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and
Na2S are available to separate the positive ions from each other. In order to effect
separation, the solutions should be added in which order?
A)
Na2SO4, NaCl, Na2S
B)
Na2SO4, Na2S, NaCl
C)
Na2S, NaCl, Na2SO4
D)
NaCl, Na2S, Na2SO4
E)
NaCl, Na2SO4, Na2S
47. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium
phosphate. What is the formula of the solid formed in the reaction?
A)
Ca(PO4)2
B)
CaPO4
C)
Ca3(PO4)2
D)
Ca3(PO3)2
E)
none of these
48. The filtrate is the solid formed when two solutions are mixed.
49. The balanced molecular equation contains which one of the following terms?
A)
AgCl (s)
B)
2AgCl (s)
C)
2Ba(NO3)2 (aq)
D)
BaNO3 (aq)
E)
3AgCl (aq)
50. The balanced complete ionic equation contains which of the following terms?
A)
2Ba2+(aq)
B)
Cl–(aq)
C)
2Ag+(aq)
D)
NO3– (aq)
E)
AgCl(aq)
51. The net ionic equation contains which of the following terms?
A)
Ag+(aq)
B)
Ba2+(aq)
C)
NO3– (aq)
D)
H+ (aq)
E)
AgCl(aq)
52. In writing the complete ionic equation for the reaction (if any) that occurs when aqueous
solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as
ionic species?
A)
KOH
B)
Mg(NO3)2
C)
Mg(OH)2
D)
KNO3
E)
All of the above would be written as ionic species.
53. The net ionic equation for the reaction of calcium bromide and sodium phosphate contains
which of the following species?
A)
2Br–(aq)
B)
PO43–(aq)
C)
2Ca3(PO4)2(s)
D)
6NaBr(aq)
E)
3Ca2+(aq)
54. When sodium chloride and lead(II) nitrate react in an aqueous solution, which of the
following terms will be present in the balanced molecular equation?
A)
PbCl(s)
B)
Pb2Cl(s)
C)
NaNO3(aq)
D)
2NaNO3(aq)
E)
2PbCl2(s)
55. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium
phosphate. Write and balance the equation for this reaction to answer the following
question.What is the sum of the coefficients when the molecular equation is balanced in
standard form?
A)
4
B)
5
C)
7
D)
11
E)
12
56. When solutions of phosphoric acid and iron(III) nitrate react, which of the following terms
will be present in the balanced molecular equation?
A)
HNO3(aq)
B)
3HNO3(aq)
C)
2FePO4(s)
D)
3FePO4(s)
E)
2HNO3(aq)
57. When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms
will be present in the net ionic equation?
A)
CoCO3(s)
B)
H+(aq)
C)
2CoCO3(s)
D)
2Cl–(aq)
E)
two of these
58. When solutions of strontium chloride and sodium sulfate react, which of the following is a
spectator ion?
A)
strontium ion
B)
chloride ion
C)
sodium ion
D)
sulfate ion
E)
two of these
59. The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains
which of the following species?
A)
3Al3+(aq)
B)
OH–(aq)
C)
3OH–(aq)
D)
2Al3+(aq)
E)
2Al(OH)3(s)
60. Consider the reaction between 15.0 mL of a 1.00 M aqueous solution of AgNO3 and 10.0
mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed.
What is present in solution after the reaction is complete? Note: the solid is not considered
to be in solution.
A)
Ag+, NO3–, K+, CrO42–, water
B)
Ag+, NO3–, K+, water
C)
K+, CrO42–, water
D)
NO3–, K+, CrO42–, water
E)
water
61. You mix 275.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.85 M potassium iodide.
The lead(II) iodide is insoluble. Which of the following is false?
A)
The final concentration of Pb2+ ions is 0.0913 M.
B)
You form 128 g of lead(II) iodide.
C)
The final concentration of K+ is 0.965 M.
D)
The final concentration of NO3– is 0.965 M.
E)
All are true.