AP® Chemistry Practice
Multiple Choice Questions
Background Information:
We wrote these questions to be as similar as possible to the type of questions that are
asked on the real test. You’ll get a sense of the strategies you need to use, and you’ll see
many of the common tricks and traps.
This set of questions is only a third as long as a real test (30 minutes instead of 90
minutes). You’ll be able to do it much more quickly. However, this also means we
weren’t able to include questions on every single topic. Still, the selections are very
representative.
Instructions:
We really recommend printing this packet out on paper, to make the experience as
realistic as possible. Take 30 minutes to complete these problems. Set a timer!
The test packet contains a periodic table, an equation sheet, and an answer sheet.
Remember to fill your answers into the answers sheet. On the real test, if the answers
aren’t bubbled in when the time ends, they don’t count!
Good luck!
For in-depth explanations of the answers and videos for each question,
check out: www.tdwscience.com/apchem-resources
AP® Chemistry is a trademark owned by the College Board, which is not affiliated
with, and does not endorse, these practice problems or any associated content.
© Bascom Science Incorporated, 2022
Multiple Choice Questions Mini Practice Test
Time: 30 minutes
1) 10.0 g of iron and 10.0 g of sulfur react to completion. Assuming a 100% yield, which of the
following describes the contents of the reaction vessel?
(A)
(B)
(C)
(D)
Fe, S, and FeS
Fe and FeS
S and FeS
FeS
2) Identify the Brønsted-Lowry acid/conjugate base pair:
(A)
(B)
(C)
(D)
H3O+ and OH–
H2SO4 and H2SO3
HNO3 and NO3–
H2PO4– and HPO42–
3) The following is a photoelectron spectrum of an element in its ground state. Which element
matches this spectrum?
(A)
(B)
(C)
(D)
Boron
Aluminum
Argon
Potassium
4) A saturated solution of (NH4)3PO4 has a concentration of ammonium ions [NH4+] = 1.50 M.
What is the concentration of ammonium phosphate?
(A)
(B)
(C)
(D)
0.50 M
1.00 M
1.50 M
4.50 M
1
5) An antacid tablet containing Ca(OH)2(s) (74.1 g/mol) is titrated with a 0.100 M solution of
HCl(aq). The equivalence point is determined by using an indicator. Based on the information
below, what was the mass of the Ca(OH)2(s) in the tablet?
Initial buret reading: 5.1 mL
Final buret reading: 25.1 mL
(A)
(B)
(C)
(D)
0.0741 g
74.1 g
0.1482 g
148.2 g
6) Which of the following 0.10 M solutions would experience the highest percent ionization?
(A)
(B)
(C)
(D)
HBrO
HBrO2
HBrO3
They are all the same
7) Given a constant temperature, which of the following reactions is most likely to proceed
spontaneously?
(A)
(B)
(C)
(D)
A(aq) + 2B(aq) → C(aq) + 2D(aq), ∆H = +75 kJ/mol
A(g) + B(g) → C(s), ∆H = +25 kJ/mol
A(aq) + B(s) → C(aq) + 2B(g), ∆H = –75 kJ/mol
2A(g) + B(g) → C(g) + D(g), ∆H = –80 kJ/mol
8) A student is performing a redox titration by oxidizing Fe2+ ions to Fe3+ ions using a solution
of 0.0010 M KMnO4(aq). The target solution is iron (II) sulfate. The balanced redox reaction is:
5Fe2+(aq) + MnO4–(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Assuming all glassware has been cleaned and thoroughly rinsed with distilled water, what is the
proper laboratory procedure before adding the KMnO4(aq) solution to the buret?
(A)
(B)
(C)
(D)
Perform an additional rinse using distilled water.
Rinse the buret with the KMnO4(aq) solution.
Rinse the buret with the FeSO4(aq) solution.
Add drops of sulfuric acid to acidify the KMnO4(aq) solution.
2
9) For a hypothetical reaction M + 2Q + X → Y+ Z, the following initial rate data were
obtained. The temperature remains constant.
Experiment
1
2
3
4
Initial
[M]o,
(mol.L-1)
0.10
0.10
0.20
0.10
Initial
[Q]o,
(mol.L-1)
0.20
0.40
0.20
0.20
Initial
[X]o,
(mol.L-1)
0.10
0.10
0.10
0.20
Initial Rate of
Formation of Z,
(mol.L-1.sec-1)
6.0 x 10-3
2.4 x 10-2
1.2 x 10-2
6.0 x 10-3
The rate law for this reaction would be:
(A) Rate = k[M][Q][X][Y][Z]
(B) Rate = k[M][Q][X]
(C) Rate = k[M]2[Q]
(D) Rate = k[M][Q]2
10) H2(g) + Cl2(g) ⇋ 2HCl(g), ∆H = –185 kJ/mol
The above gaseous reaction occurs and comes to equilibrium in a closed container. Which of the
following changes to the system would cause the reverse reaction to speed up?
(A)
(B)
(C)
(D)
Removing some HCl
Adding some H2
Lowering the temperature
Raising the temperature
11) Which of the following diagrams provides the best representation of an aqueous solution of
HNO3?
3
12) A 0.50 g sample of Zn(s) was placed in a solution of HCl(aq). The zinc reacted completely
with the acid. Which one of the following equations best represents the reacting species
described above?
(A)
(B)
(C)
(D)
Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
Zn(s) + 2HCl(aq) → Zn2+(aq) + Cl2(g) + H2(g)
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
Zn(s) + 2HCl(aq) → ZnCl2(aq) + 2H+(aq)
13) Beaker A contains 250 mL of pure, deionized water and Beaker B contains 500 mL of 1.0 M
KCl. AgCl crystals are added to each beaker. After stirring the contents of the beakers, some
solid AgCl remains at the bottom of each, as shown below. Which of the following is true?
(A)
(B)
(C)
(D)
Beaker A contains a greater [Ag+].
Beaker B contains a greater [Ag+].
[Ag+] is the same, but not zero, in each beaker.
[Ag+] is zero in each beaker.
14) Which of the following is a nonpolar molecule that still contains polar bonds?
(A)
(B)
(C)
(D)
N2
CO2
CH4
CH2F2
15) Which of the following statements is true regarding lithium and cesium?
(A)
(B)
(C)
(D)
Cesium has a higher ionization energy and a larger atomic radius.
Lithium has a higher ionization energy and a higher electronegativity.
Cesium has a higher ionization energy and a higher electronegativity.
Lithium has a larger atomic radius and a higher electronegativity.
4
16) A 1.0-liter sealed container contains equal masses of Ne and Ar. The total pressure of the
system is 12 atm. The temperature remains constant. What is the partial pressure of Ar?
(A)
(B)
(C)
(D)
2 atm
4 atm
6 atm
8 atm
17) Which of the following species has the electron configuration shown below?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
(A)
(B)
(C)
(D)
Ar
Sr2+
Br+
Pd
18) Magnesium has a specific heat capacity of 1.0 J/g°C. A sample of magnesium is heated to
80.0°C. It is placed in a calorimeter filled with 100.0 g of water at 19.0°C. The magnesium cools
and reaches thermal equilibrium with the water at 20.0°C. If the specific heat of water is 4.2
J/g°C, what is the approximate mass of the magnesium?
(A)
(B)
(C)
(D)
4.2 grams
7 grams
10 grams
21 grams
Questions 19-20 refer to the information below.
The diagram below represents a standard Pb|Pb2+ half-cell connected to a standard Fe3+| Fe2+
half-cell using a salt bridge and an external circuit. Electrode 1 represents the anode, and
Electrode 2 the cathode. The overall equation for the reaction is 2Fe3+ + Pb → 2Fe2+ + Pb2+.
Relevant reduction potentials are provided
in the table below:
Standard Reduction Potentials:
Fe3+ + e– → Fe2+
0.77 V
2+
–
Pb + 2e → Pb
–0.13 V
5
19) Which expression gives the standard cell potential in volts?
(A)
(B)
(C)
(D)
0.77 + 0.13
0.77 – 0.13
(2 x 0.77) + 0.13
(2 x 0.77) – 0.13
20) Which of the following accurately describes the change in mass occurring at the electrodes
during operation of the cell?
(A)
(B)
(C)
(D)
Electrode 1
Electrode 2
decreases
no change
increases
decreases
no change
decreases
no change
increases
6
Chemistry Practice Multiple Choice Questions
Your Name:
Last
Date:
First
M.I.
/
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Multiple Choice Answer Sheet
Completely darken bubbles with a No. 2 pencil. If you make a mistake, be sure to erase marks
completely. Erase all stray marks.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
A
B
C
D
A
B
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D
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D
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D
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B
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D
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B
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D
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D
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B
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D
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B
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D
A
B
C
D
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19.
20.
A
B
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D
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D
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D
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B
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D
A
B
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D
A
B
C
D
A
B
C
D
A
B
C
D
A
B
C
D
A
B
C
D
For an answer key and explanation videos for each question, check out:
www.tdwscience.com/apchem-resources
AP® Chemistry Practice
Free Response Questions
Background Information:
We wrote these questions to be as similar as possible to the type of questions that are
asked on the real test. You’ll get a sense of the strategies you need to use, and you’ll see
many of the common tricks and traps.
To create a test that was only about one-third as long as the real one, we altered the
length of questions slightly. The full AP® Chemistry free response section contains both
long and short questions. Our “long” question is a little shorter than the ones on the real
test, and our “short” questions are a little longer. This was so we could ask questions on
as many different topics as possible; otherwise, it shouldn’t matter much.
Instructions:
We really recommend printing this packet out on paper, to make the experience as
realistic as possible. Get a few sheets of blank paper, to write your answers on. Take 40
minutes to complete these problems. Set a timer!
The test packet contains a periodic table and an equation sheet.
Pay attention to significant figures,and show all your work to get maximum credit.
Good luck!
For in-depth explanations of the answers and videos for each question,
check out: www.tdwscience.com/apchem-resources
AP® Chemistry is a trademark owned by the College Board, which is not affiliated
with, and does not endorse, these practice problems or any associated content.
© Bascom Science Incorporated, 2022
AP® CHEMISTRY MINI-TEST
FREE-RESPONSE QUESTIONS
Please show all your work, otherwise you may be ineligible for partial credit. Pay attention to
significant figures.
Question 1
This question refers to the following compounds.
Formaldehyde (Methanal)
Formic acid (Methanoic acid)
Methane
Methanol
(a) Indicate the hybridization of the carbon atom in formaldehyde. (1 point)
(b) Indicate the approximate bond angle of the C–O–H bond in methanol. (1 point)
(c) The boiling points of the four compounds are shown in the table below. Use concepts of
intermolecular forces to explain why methanol has a higher boiling point than formaldehyde.
(1 point)
Compound Name Boiling Point (1 atm)
Formic Acid
Methanol
100.8 ºC
64.7 ºC
Formaldehyde
–19.3 ºC
Methane
–162.2 ºC
(d) A student argues that methane molecules experience no intermolecular forces. Explain why
the student is or is not correct. (1 point)
(e) Methanol can be used as a fuel for a variety of applications. The balanced equation for its
combustion is given below.
2CH3OH(g) + 3O2(g) ® 2CO2(g) + 4H2O(l)
Calculate the ∆H° for the reaction above, using the data from the table below. (2 points)
Compound
∆Hf° (kJ/mol)
CH3OH(g)
–201.0
O2(g)
0.0
CO2(g)
–393.5
H2O(l)
–285.8
(f) Methanol has a density of 0.792 g/mL and a molar mass of 32.04 g/mol. How much heat will
be released when a 150.0 mL sample of methanol is combusted with an excess of oxygen? (2
points)
AP® CHEMISTRY MINI-TEST
FREE-RESPONSE QUESTIONS
Please show all your work, otherwise you may be ineligible for partial credit. Pay attention to significant
figures.
Question 2
Formic acid (CHOOH) reacts with water according to the following equation:
CHOOH(aq) + H2O(l) ⇋ H3O+(aq) + CHOO–(aq)
Ka = 1.78 × 10-4 at 25°C
(a) Write the equilibrium constant expression, Ka, for formic acid. (1 point)
(b) Calculate the pH of a 0.150 M aqueous solution of formic acid. (2 points)
(c) To create a buffer solution, sodium formate (NaCHOO) can be added to formic acid. How
many moles of sodium formate would need to be added to 250 mL of a 0.10 M formic acid
solution to create a buffer with a pH of 3.90? (2 points)
AP® CHEMISTRY MINI-TEST
FREE-RESPONSE QUESTIONS
Please show all your work, otherwise you may be ineligible for partial credit. Pay attention to significant
figures.
Question 3
NO2(g) + CO(g) → NO(g) + CO2(g)
(a) Explain how the following graphs suggest the reaction above is second order with respect to
NO2. (1 point)
(b) Write a rate law for the full reaction, assuming it is zero-order with respect to CO. (1 point)
(c) The initial rate of reaction is 1.4 × 10–4 mol L-1 s-1. Using the graphs above, determine the
rate constant, k. (1 point)
(d) The reaction is expected to proceed according to the mechanistic steps below:
NO2 + NO2 → NO3 + NO (slow)
NO3 + CO → NO2 + CO2 (fast)
Explain whether this mechanism is consistent with your proposed rate law from part 2.
(1 point)
(e) The reaction proceeds spontaneously. Sketch a relative potential energy diagram for the
overall reaction. (1 point)