1
Substance
State at room
Melting Point (C)
Boiling Point (C)
temperature
CO2
Gas
NA
NA
CS2
Liquid
-111.6
46.5
CSe2
Liquid
-45.5
125
a) Draw the Lewis Dot structure for CO2. Properly label each atom with a partial charge. Does
this molecule have a dipole moment? Explain your answer.
b) Are CS2 and CSe2 polar or non-polar molecules? Explain your answer.
c) Explain in detail the differences in physical properties among the substances listed in the
chart. In your discussion be sure to include intermolecular forces and polarity.
2 The vapor pressure of a liquid is
a)
b)
c)
d)
directly related to temperature.
inversely related to intermolecular forces.
the pressure of vapor above a pure liquid at its boiling point.
directly proportional to the enthalpy of fusion.
3
The molarity of a solution is defined as the
a. moles of solute per kilogram of solvent.
b. moles of solute per liter of solution.
c. moles of solute per liter of solvent.
d. grams of solute per liter of solution.
e. grams of solute per kilogram of solvent.
4
What mass of 40.0% glucose, C H O , solution contains 75.0 g of water?
6 12 6
a. 40.0 g
b. 50.0 g
c. 125 g
d. 150. g
e. 175 g
5
What is the molarity of an NaI solution that contains 3.00 g of NaI in 40.0 mL of solution?
a. 0.100 M
b. 0.500 M
c. 1.00 M
d. 2.00 M
e. 5.00 M
6
In order to prepare a standard 1.00 M solution of oxalic acid from H C O • 2H O (molar mass = 127.07
2 2 4
2
g/mol), 3.152 g of oxalic acid dihydrate should be dissolved in
a. 25.0 cm3 of water.
b. 25.0 g of water.
c. 22.7 g of water.
d. enough water to make 25.0 g of solution.
e. enough water to make 25.0 mL of solution.
7
A 60.0-g sample of NaOH is dissolved in water, and the solution is diluted to give a final volume of 3.00
L. The molarity of the final solution is
a. 0.500 M.
b. 0.750 M.
c. 1.00 M.
d. 2.00 M.
e. 3.00 M.
8
To obtain 12 g of sucrose (MM = 342) from a solution labeled 8.0% C 12H22O11 by mass, we would
need to weigh out _______ g of solution.
a. 25 g
b. 50 g
c. 100 g
d. 150 g
e. 200 g
9
A 12.0% sucrose solution has a density of 1.05 g/cm3. The number that gives the best value for the
mass of sugar in 55 mL of this solution is
a. 6.6 g.
b. 6.60 g.
c. 6.9 g.
d. 6.93 g.
e. 58 g.
10
Which of the following aqueous solutions can be prepared by making only mass measurements?
1.
2.
3.
a.
b.
c.
d.
e.
0.10 mole fraction of a solution of NaCl
10.0% solution of NaCl
1.0 molar solution of NaCl
1 only
2 only
3 only
1 and 2 only
1 and 3 only
11
The number of grams of oxalic acid dihydrate, H2C2O4 • 2H2O, that is required to prepare 250.0 mL of
1.25 M solution is
a. 28.1 g.
b. 39.4 g.
c. 43.6 g.
d. 48.2 g.
e. 90.0 g.
12
13
14
Calculate the molarity of a solution that contains 85.0 g of HCl in 275 mL of solution. (MW HCl = 36.5
g/mol.)
a. 7.23 M
b. 7.92 M
c. 8.47 M
d. 8.81 M
e. 9.25 M
3
–3
What is the mass of H SO in a 50.0-cm sample of sulfuric acid that has a density of 1.55 g cm and
2 4
which consists of 65.0% H SO ?
2 4
a. 27.1 g
b. 32.5 g
c. 50.4 g
d. 77.5 g
e. 119 g
Which of the following affect the solubility of gases in solvents?
1.
2.
3.
a.
b.
c.
d.
e.
15
the nature of the gas (polarity)
the density of the solvent
the temperature of the solvent
1 only
2 only
3 only
1 and 3 only
1, 2, and 3
Which of the following increases the solubility of a gas in a given solvent?
a. increasing the partial pressure of the gas
b. increasing the temperature of the solvent
c. decreasing the partial pressure of the gas
d. increasing the temperature of the solvent and decreasing the partial pressure of the gas
simultaneously
e. both a and b
16
Which of the following would become more soluble in water at 20°C if the pressure were increased?
a.
b.
c.
d.
e.
17
1.
2.
SO2
TiO2
3.
CO2
1 only
2 only
3 only
1 and 3 only
1, 2, and 3
All the following gases have appreciable solubility in water except
a. CO2.
b. N2O3.
c. O .
2
d. H2S.
e.
HCN.
18 Which of the following compounds (each as a liquid) would be expected to be the best solvent for carbon
disulfide?
a. HBr(l)
b. CH OH(l)
3
c. C H (l)
6 6
d. H O(l)
2
e. NH (l)
3
The following data pertain to Questions 19 through 12.21.
A concentrated sulfuric acid solution is 74.0% H SO by mass and has a density of 1.66 g/mL at 20°C. (MW of
2 4
H SO is 98.0 g/mol.)
2 4
19
20
A liter of sulfuric acid weighs
a. 1000 g.
b. 1660 g.
c. 1660 g x 0.740.
d. 1000 g x 0.740.
1660 g  0.740
e.
.
98
The mass of H SO in each liter of concentrated H SO is
2 4
2 4
a. (1660 X 0.740) g.
b. (1660 – 1000) g.
c. 1660 g.
d. (1660 X 0.740 – 1000) g.
e. 740 g.
21
22
23
The molarity of the H SO solution is
2 4
a. 2.3 M.
b. 6.7 M.
c. 7.6 M.
d. 12.5 M.
e. 16.9 M.
How many grams of Na CO are contained in 0.400 L of 0.250 M Na CO solution?
2 3
2 3
a. 5.30 g
b. 10.6 g
c. 15.3 g
d. 20.8 g
e. 24.2 g
The vapor pressure of ethylene glycol, HOCH2CH2OH, depends primarily
on the
a. volume of the container.
b. atmospheric pressure.
c. molar mass of the liquid.
d. intramolecular forces of the liquid.
e. temperature of the liquid.
24
Which of the following has the highest vapor pressure at room temperature?
a. Ethylene glycol, b.p. = 198°C
b. Ethanol, b.p. = 78°C
c. Water, b.p. = 100°C
d. Benzene, b.p. = 80°C
e. Carbon disulfide, b.p. = 46°C
25
Which of the following solutions contains the largest number of moles of solute?
a. 50. mL of 1 M hydrochloric acid
b. 25. mL of 5 M sodium chloride
c. 100. mL of 0.5 M nitric acid
d. 25. mL of 2 M sulfuric acid
e. 200. mL of 0.1 M sodium hydroxide
26
Which of the following solutes dissolved in 1,000 g of water would provide the greatest number of
particles?
a. 0.030 mole urea, CO(NH )
22
b. 0.030 mole acetic acid, CH COOH
3
c. 0.030 mole ammonium nitrate, NH NO
4 3
d. 0.030 mole calcium sulfate, CaSO
4
e. 0.030 mole barium chloride, BaCl
2
27
When solid NH NO is dissolved in a nearly saturated solution of NH NO , the solution becomes
4 3
4 3
colder. This information indicates that if the temperature of a solution is raised,
a. ∆H will become negative.
b. ∆H will become zero.
c. the solubility of NH NO will decrease.
4 3
d. the solubility of NH NO will increase.
4 3
e. the solubility of NH NO will not change.
4 3
28
Which substance would produce three moles of particles per mole of solute when dissolved in water?
a.
CH2O
b.
SO2
c.
CO2
d. K CrO
2
4
e.
Al(NO3)3