1) The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0 oC is 2.03.
What is the value of Ka for HF?
A) 2.0 x 10-9
B) 1.1 x 10-9
C) 6.0 x 10-5
D) 3.5 x 10-4
E) none of the above
2) Aluminum reacts with a certain nonmetallic element to form a compound with the
general formula Al2X3. Element X must be from Group ________ of the Periodic Table
of Elements.
A) 3A
B) 4A
C) 5A
D) 6A
E) 7A
3) The species ________ contains 16 neutrons.
A) 31P
B) 34S2-
C) 36Cl
D) 80Br–
E) 16O
4) Which of the following liquids will have the lowest freezing point?
A) pure H2O
B) aqueous glucose (0.050 m)
C) aqueous CoI2 (0.030 m)
D) aqueous FeI3 (0.030 m)
E) aqueous NaI (0.030 m)
5) The standard Gibbs free energy of formation of ________ is zero.
(a) H2O (l)
(b) O (g)
(c) Cl2 (g)
A) (a) only
B) (b) only
C) (c) only
D) (b) and (c)
E) (a), (b), and (c)
6) The missing product in this reaction combines with o x ygen to form a compound
with the formula ________.
K –> e + _____
A) M2O
B) MO
C) MO2
D) M2O3
E) M3O2
7) The two allotropic forms of phosphorus are ________ and ________.
A) black, red
B) white, black
C) white, yellow
D) white, red
E) black, yellow
8) A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough
water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at
25.0 oC. What is the molecular weight (g/mol) of the unknown solute?
A) 16.4
B) 196
C) 110
D) 30.6
E) 5.12 x 10-3
9) An electron in a Bohr hydrogen atom has an energy of -1.362 X 10-19 J. The value of
n for this electron is ________.
A) 1
B) 2
C) 3
D) 4
E) 5
10) When the following equation is balanced, the coefficient of H2 is ________.
CO (g) + H2 (g) → H2O (g) + CH4 (g)
A) 1
B) 2
C) 3
D) 4
E) 0
11) Which of the following substances is least likely to dissolve in water?
A) HOCH2CH2OH
B) CHCl3
C) O
CH3(CH2)9CH
D) CH3(CH2)8CH2OH
E) CCl4
12) All of the orbitals in a given electron shell have the same value as the ________
quantum number.
A) principal
B) angular momentum
C) magnetic
D) spin
E) psi
13) Sulfur forms an ion with a charge of ________.
A) 2+
B) 2-
C) 3+
D) 6-
E) 6+
14) What type(s) of intermolecular forces exist between Br2 and CCl4?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces and dipole-dipole
D) dispersion forces, ion-dipole, and dipole-dipole
E) None. Since both are gases at room temperature, they do not interact with each other.
15) ________ is the energy required to expand the surface area of a liquid by a unit
amount of area.
A) Viscosity
B) Surface tension
C) Volatility
D) Meniscus
E) Capillary action
16) The value of G o at 181.0 oC for the formation of calcium chloride from its
constituent elements:
Ca (s) + Cl2 (g) –> CaCl2 (s)
is ________ kJ/mol. At 25.0 oC for this reaction, H o is -795.8 kJ/mol, G o is -748.1
kJ/mol, and S o is -159.8 J/K.
A) -868.4
B) -723.2
C) 7.18 x 104
D) -766.9
E) 2.81 x 104
17) In which of the following reactions would increasing pressure at constant
temperature change the concentrations of reactants and products, based on Le Ch
¢teliers principle?
A) N2 (g) + 3H2 (g) 2NH3 (g)
B) N2O4 (g) 2NO2 (g)
C) N2 (g) + 2O2 (g) 2NO2 (g)
D) 2N2 (g) + O2 (g) 2N2O (g)
E) all of the above
18) A certain mass of carbon reacts with 128 g of oxygen to form carbon monoxide.
________ grams of oxygen would react with that same mass of carbon to form carbon
dioxide, according to the law of multiple proportions.
A) 25.6
B) 64.0
C) 128
D) 1280
E) 256
19) Which of the following aqueous solutions has the highest [OH–]?
A) a solution with a pH of 3.0
B) a 1 x 10-4 M solution of HNO3
C) a solution with a pOH of 12.0
D) pure water
E) a 1 x 10-3 M solution of NH4Cl