AP Chemistry
Period 1
Name:____________________________
Multiple Choice Question Practice
1. In which of the following compounds does sulfur have
an oxidation state of +4?
a. H2S
b. SO3
c. MgSO4
d. H2SO3
e. H2SO4
In H2SO3, the H’s have a +1 state, the O’s have a -2
state. To cancel out a +2 and a -6 (the balance is 4) the S has to be +4.
2. You have two samples of the same gas in the same size
container, at the same pressure. The temperature in the
first container is -23oC and the temperature in the
second container is 227oC. What is the ratio of the
number of moles of gas in the first container compared
to that in the second container?
a. 4 : 1
b. 1 : 4
c. 1 : 1
d. 2 : 1
e. 1 : 2
V=V2, P=P2, T = -23+273, T2 = 227 + 273
N1 = T2 = 500 = 2
N2
T1
250
1
3. 435 mL of a 0.100 M HNO3 solution is mixed with 235
mL of 0.175M Ca(OH)2. Which of the following
statements are true?
1. Some HNO3 remains unreacted.
2. The solution is alkaline.
3. Water is a product.
4. The solution is acidic.
5. Some Ca(OH)2 remains unreacted.
a. 1 and 5
b. 3 and 4
c. 2 and 3
d. 1 and 4
e. 1, 4, and 5
2 HNO3 + Ca(OH)2  2H2O + Ca(NO3)2
435mL*0.100M = 43.5mmol HNO3 (LR)
235mL*0.175M = 41.1mmol Ca(OH)2



Excess calcium hydroxide makes solution
alkaline(basic)
Water IS a product
Statement 5 is also true, but there’s no
option for that! Pick the most true choice.
4. A valve separates two tanks, one containing 7.6 liters of
oxygen at 4.0 atmospheres and the other containing 4.0
liters of carbon dioxide at 11.0 atm. When the valve is
opened and the two gases are allowed to come together,
what is the final pressure?
a. 6.4 atm
b. 9.5 atm
c. 1.8 atm
d. 3.6 atm
e. 8.2 atm
Total V = 7.6 + 4.0 = 11.6 L
Use PV=nRT for gas one to find moles
Use PV=nRT for gas two to find moles.
Add moles, use total volume to find total pressure.
5. How many grams of sodium chloride are dissolved in
50.0 mL of 1.50 M solution?
a. 117 g
b. 4.38 x 103 g
c. 0.00324 g
d. 4.38 g
e. 23.4 g
0.050L * 1.50M = 0.075mol
0.075mol *58.44g/mol = 4.38 g
6. How many moles of gas would it take to fill an average
man’s lungs, total capacity of which is about 4.5 liters?
Assume 1.00 atm pressure and 37oC.
a. 0.75 mol
b. 37 mol
c. 1.24 mol
d. 11.2 mol
e. 0.18 mol
PV=nRT plug in and solve!!
7. Which of the following is the most soluble base?
a. Ca(OH)2
b. Mg(OH)2
c. Ba(OH)2
d. NaOH
e. Al(OH)3
Hydroxides are mostly soluble, sodium (alkalai
metal!) is extremely soluble.
8. 325 mL of a gas at STP has a mass of 0.805 grams.
What is the molar mass of the gaseous compound?
a. 9.04 g/mol
b. 55.5 g/mol
c. 0.0555 g/mol
d. None of these
e. 31.7 g/mol
Moles = 0.805(Molar Mass)
Plug into PV=nRT…
PV=(0.805)(MM)RT
9. In the balanced molecular equation for the
neutralization reaction between phosphoric acid and
potassium hydroxide, the products are:
a. KPO4 + H3OH
b. K3PO4 + 3H2O
c. K+(aq) + PO4-3(aq) + 3H+ + 3OHd. 3 H2O
e. None of these
H3PO4 + 3KOH  3H2O + K3PO4
10. An 8.25 L sample of oxygen is collected at 25oC and
1.022 atm pressure. What volume will the gas occupy
at 0.940 atm and -15oC?
a. 10.4 L
b. 8.76 L
c. 5.00 L
d. 7.77 L
e. 1.78 L
PV =P2V2 Plug in and solve
T
T2
11. NaCl + H2SO4 + MnO2  Na2SO4 + MnSO4 + H2O +
Cl2
In this reaction, the reducing agent is:
a. Mn4+
b. H+
c. O2d. Na+
e. ClCl-1  Cl2
and
MnO2 MnSO4
-1
0
+4
+2
Oxidized (red.ag.)
Reduced (Ox.Ag)
12. Which of the following is not a weak acid?
a. HClO
b. H2CO3
c. HF
d. H2S
e. HNO3
Nitric acid is a strong acid!
13. A chemist makes a stock solution of potassium
chromate solution by dissolving 97.1 grams of the
compound in 1.00 liter of solution. What volume of the
solution must be diluted with water in order to prepare
200. mL of 0.200 M solution?
a. 0.150 L
b. 0.0800 mL
c. 80.0 mL
d. 750. mL
e. 120 mL
(97.1g / (194.2g/mole))/1.00L = 0.5 M
M1V1 = M2V2
0.5(x) = (200)(0.2)
14. In which flask do the molecules have the highest
average velocity?
Flask 1: 1 Liter of NH3 at STP
Flask 2: 1 Liter of CH4 at STP
Flask 3: 1 Liter of O2 at STP
a.
b.
c.
d.
e.
Flask 2
Flask 2 and 3
Flask 1
Flask 3
All are the same
All are at the same temperature,
all have the same kinetic energy,
so all are at the same speed.
15. In which of the flasks from question 14 is the greatest
number of molecules?
a. Flask 1
b. Flask 3
c. Flask 2
d. Flasks 2 and 3
e. All are the same
CH4 has the lightest molar mass, so in an equal
volume under constant conditions, there are more
moles of CH4