1) Which of the following ions will act as a weak base in water?
A) OH–
B) Cl–
C) NO3
–
D) ClO–
E) None of the above will act as a weak base in water.
2) Tetraboric acid, H2B4O7, is prepared by heating boric acid, H3BO3 (a condensation
reaction involving water loss). If 400.0 mmol H3BO3 are used, what mass (g) of H2O is
formed, assuming quantitative stoichiometric conversion?
A) 5.77
B) 0.500
C) 0.320
D) 7.21
E) 9.01
3) The molecular geometry of each carbon atom in an alkane is ________.
A) octahedral
B) square planar
C) trigonal planar
D) tetrahedral
E) trigonal pyramidal
4) Radiation in the infrared portion of the spectrum is absorbed by ________ found in
the atmosphere.
A) N2
B) O2
C) CO2
D) Ar
E) He
5) What is the order of the reaction with respect to OH–?
A) 0
B) 1
C) 2
D) 3
E) 4
6) The hybridization of orbitals on the central atom in a molecule is sp. The
electron-domain geometry around this central atom is ________.
A) octahedral
B) linear
C) trigonal planar
D) trigonal bipyramidal
E) tetrahedral
7) Using the data in the table, which of the conjugate bases below is the weakest base?
A) OAc–
B) C7H5O2
–
C) NO2
–
D) F–
E) OAc– and C7H5O2
–
8) A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134
M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The
concentration (M) of the acid was ________.
A) 0.0102
B) 0.00508
C) 0.0204
D) 0.102
E) 0.227
9) Which elemental halogen(s) can be used to prepare I2 from NaI?
A) F2 only
B) Cl2 only
C) Br2 only
D) both Cl2 and Br2, but not F2
E) F2, Cl2, and Br2
10) Based on the crystal-field strengths F– < CH2CN < NH3 < NO2
– < CN–, which Co
(III) complex is most likely high-spin?
A) [Co(NH3)6]3+
B) [Co(NO2)6]3-
C) [Co(CN)6]3-
D) [CoF6]3-
E) [Co(CH3CN)6]3+
11) An aqueous solution contains 0.050 M of methylamine. The concentration of hydro
xide ion in this solution is ________ M. Kb for methylamine is 4.4 x 10-4.
A) 0.050
B) 2.2 x 10-5
C) 2.9 x 10-3
D) 4.5 x 10-3
E) 4.7 x 10-3
12) The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin
C9H8O4) in 0.250 L of water at 25 oC is ________ atm.
A) 24.5
B) 2.05 x 10-3
C) 0.0245
D) 4.41
E) 2.48
13) According to kinetic-molecular theory, if the temperature of a gas is raised from 100
°C to 200 °C, the average kinetic energy of the gas will ________.
A) double
B) increase by a factor of 1.27
C) increase by a factor of 100
D) decrease by half
E) decrease by a factor of 100
14) Predict the empirical formula of the ionic compound that forms from aluminum and
oxygen.
A) AlO
B) Al3O2
C) Al2O3
D) AlO2
E) Al2O
15) Components of AirMole Fraction
Nitrogen 0.781
Oxygen 0.209
Argon 0.010
What is the partial pressure or argon (in torr) in the atmosphere when the atmospheric
pressure is 750.0 torr?
A) 157
B) 586
C) 611
D) 7.50
E) 760
16) Which one of the following is the correct formula for potassium
diaquatetrachloromolybdate (III)?
A) K2[Mo(H2O)2Cl4]
B) K[Mo(H2O)2Cl2]Cl2
C) K[Mo(H2O)2Cl4]
D) Mo[K(H2O)2]Cl4
E) K3[Mo(H2O)2Cl4]
17) Consider the following types of compounds:
(i)amino acid
(ii)nitrogen-containing organic base
(iii)phosphoric acid
(iv)five-carbon sugar
From which of the above compounds are the monomers of nucleic acids, called
nucleotides, formed?
A) none
B) (i) and (ii)
C) (ii) and (iv)
D) (ii), (iii), and (iv)
E) all
18) The average atomic weight of copper, which has two naturally occurring isotopes, is
63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of
the copper isotopes. The other isotope has an abundance of 30.9%. The atomic weight
(amu) of the second isotope is ________ amu.
A) 63.2
B) 63.8
C) 64.1
D) 64.8
E) 28.1