1) Which one of the following solutions will have the greatest concentration of
hydroxide ions?
A) 1.10 M rubidium hydroxide
B) 0.368 M calcium hydroxide
C) 0.368 M ammonium hydroxide
D) 0.368 M potassium hydroxide
E) 0.368 M sulfuric acid
2) How many moles of B are present at 30 s?
A) 2.4 x 10-3
B) 0.15
C) 0.073
D) 1.7 x 10-3
E) 0.051
3) A 0.1 M aqueous solution of ________ will have a pH of 7.0 at 25.0 oC.
LiF
RbBr
NaClO4
NH4Cl
A) RbBr and NaClO4
B) LiF and RbBr
C) NaClO4 only
D) LiF only
E) NH4Cl only
4) According to VSEPR theory, if there are three electron domains in the valence shell
of an atom, they will be arranged in a(n) ________ geometry.
A) tetrahedral
B) octahedral
C) linear
D) square planar
E) bent
5) Of the species below, only ________ is not an electrolyte.
A) HCl
B) Rb2SO4
C) Ar
D) KOH
E) NaCl
6) A 11.5 mL aliquot of 0.162 M H3PO4 (aq) is to be titrated with 0.229 M NaOH (aq).
What volume (mL) of base will it take to reach the equivalence point?
A) 24.4
B) 1.28
C) 8.14
D) 2.71
E) 103
7) There should be ________ significant figures in the answer to the following
computation.
A) 1
B) 2
C) 3
D) 4
E) 5
8) In what year was Fritz Haber awarded the Nobel Prize in chemistry for his
development of a process for synthesizing ammonia directly from nitrogen and
hydrogen?
A) 1954
B) 1933
C) 1918
D) 1900
E) 1912
9) Which one of the following pairs cannot be mixed together to form a buffer solution?
A) NH3, NH4Cl
B) NaC2H3O2, HCl (C2H3O2
– = acetate)
C) RbOH, HBr
D) KOH, HF
E) H3PO4, KH2PO4
10) Of the species below, only ________ is not an electrolyte.
A) HBr
B) LiCl
C) Ne
D) KOH
E) NaNO3
11) Which one of the following is a triprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
12) The volume of 1.26 mol of gas at 69.4 kPa and 25.30 °C is ________ L.
A) 45.1
B) 633
C) 3.82
D) 0.445
E) 0.439
13) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The combustion of ethane in the presence of excess oxygen yields carbon dioxide and
water:
2C2H6 (g) + 7O2 (g) –> 4CO2 (g) + 6H2O (l)
The value of S o for this reaction is ________ J/K mol.
A) +718.0
B) -620.1
C) -718.0
D) -151.0
E) +151.0
14) Consider the following chemical reaction:
CO (g) + 2H2(g) CH3OH(g)
At equilibrium in a particular experiment, the concentrations of CO and H2 were 0.15
M and 0.36, M respectively. What is the equilibrium concentration of CH3OH? The
value of Keq for this reaction is 14.5 at the temperature of the experiment.
A) 14.5
B) 7.61 x 10-3
C) 2.82 x 10-1
D) 3.72 x 10-3
E) 1.34 x 10-3
15) Which equation correctly represents the reaction between silica and hydrofluoric
acid?
A) SiCl4 + 4HF –> SiF4 + 4HCl
B) SiO2 + 6HF –> H2SiF6 + 2H2O
C) SiCl2 + 2HF –> SiF2 + 2HCl
D) SiH4 + 4HF –> SiF4 + 4H2
E) none of the above
16) For a given arrangement of ions, the lattice energy increases as ionic radius
________ and as ionic charge ________.
A) decreases, increases
B) increases, decreases
C) increases, increases
D) decreases, decreases
E) This cannot be predicted.
17) The rate law of a reaction is rate = k[D][X]. The units of the rate constant are
________.
A) mol L-1s-1
B) L mol-1s-1
C) mol2 L-2s-1
D) mol L-1s-2
E) L2 mol-2s-1
