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12) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic
equation is ________.
A) Ag+ (aq) + (aq) → AgI (s)
B) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
C) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
D) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)
E) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
13) When aqueous solutions of Pb(NO3)2 and NaCl are mixed, PbCl2 precipitates. The balanced net ionic
equation is ________.
A) Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s)
B) Pb2+ (aq) + 2NO3- (aq) → Pb(NO3)2 (s)
C) Pb2+ (aq) + 2NO3- (aq) → Pb(NO3)2 (aq)
D) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)
E) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (aq) + 2NaNO3 (s)
14) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
B) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
C) H+ (aq) + OH- (aq) → H2O (l)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)
15) The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide
are ________.
A) OH- and ClO4-
B) H+, OH- , ClO4-, and Ba2+
C) H+ and OH-
D) H+ and Ba2+
E) ClO4- and Ba2+
16) The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are
________.
A) OH- and ClO3-
B) H+, OH-, ClO3-, and Ba2+
C) H+ and OH-
D) H+ and Ba2+
E) ClO3- and Ba2+
17) The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide
are ________.
A) OH-, F-, and Ba2+
B) F- and Ba2+
C) OH- and F-
D) Ba2+ only
E) H+, OH-, F-, and Ba2+
18) The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are
________.
A) H+ and NH3
B) H+, Cl-, NH3, and NH4+
C) Cl- and NH4+
D) H+, Cl-, and NH4+
E) Cl- only
19) Which of the following are strong acids?
HI
HNO3
HF
HBr
A) HF, HBr
B) HI, HNO3, HF, HBr
C) HI, HF, HBr
D) HNO3, HF, HBr
E) HI, HNO3, HBr
20) Which hydroxides are strong bases?
Sr(OH)2
KOH
NaOH
Ba(OH)2
A) KOH, Ba(OH)2
B) KOH, NaOH
C) KOH, NaOH, Ba(OH)2
D) Sr(OH)2, KOH, NaOH, Ba(OH)2
E) None of these is a strong base.
21) A neutralization reaction between an acid and a metal hydroxide produces ________.
A) water and a salt
B) hydrogen gas
C) oxygen gas
D) sodium hydroxide
E) ammonia
22) Of the metals below, only ________ will not dissolve in an aqueous solution containing nickel ions.
aluminum
chromium
barium
tin
potassium
A) aluminum
B) chromium
C) barium
D) tin
E) potassium
23) Which of these metals is the least easily oxidized?
Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag
24) Which of these metals is the most easily oxidized?
Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag
25) Of the following elements, ________ is the only one that cannot be found in nature in its elemental
form.
Cu
Hg
Au
Ag
Na
A) Cu
B) Hg
C) Au
D) Ag
E) Na
26) Of the following elements, ________ is the most easily oxidized.
oxygen
fluorine
nitrogen
aluminum
gold
A) oxygen
B) fluorine
C) nitrogen
D) aluminum
E) gold
27) Of the following elements, ________ is the least easily oxidized.
zinc
iron
hydrogen
aluminum
lead
A) zinc
B) iron
C) hydrogen
D) aluminum
E) lead
28) Based on the equations below, which metal is the most active?
Pb(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Pb (s)
Pb(NO3)2 (aq) + Ag (s) → No reaction
Cu(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Cu (s)
A) Ni
B) Ag
C) Cu
D) Pb
E) N
29) In the following reaction, which species is reduced?
Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)
H+
N+5
O2-
H2O
Au
A) H+
B) N+5
C) O2-
D) H2O
E) Au
28
30) What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient
water to give 350 mL of solution?
A) 18
B) 0.16
C) 0.45
D) 27
E) 2.7 × 10-2
31) How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
A) 2.00
B) 0.500
C) 0.160
D) 0.0800
E) 0.0400
32) How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?
A) 0.436
B) 0.871
C) 1.31
D) 3.70
E) 11.1
33) How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?
A) 0.436
B) 1.31
C) 0.145
D) 3.70
E) 11.1
29
34) What are the respective concentrations (M) of Na+ and SO42- afforded by dissolving 0.500 mol
Na2SO4 in water and diluting to 1.33 L?
A) 0.665 and 0.665
B) 0.665 and 1.33
C) 1.33 and 0.665
D) 0.376 and 0.752
E) 0.752 and 0.376
35) What are the respective concentrations (M) of K+ and PO43- afforded by dissolving 0.800 mol K3PO4
in water and diluting to 1.63 L?
A) 0.800 and 0.800
B) 0.491 and 0.491
C) 0.800 and 0.491
D) 1.44 and 0.491
E) 0.489 and 0.163
36) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M
solution of sodium sulfide to a total volume of 250.0 mL.
A) 0.175
B) 4.37
C) 0.525
D) 0.350
E) 0.874
37) An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The
concentration of the original solution was ________ M.
A) 0.400
B) 0.200
C) 2.00
D) 1.60
E) 4.00
38) The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was
30
diluted to 0.800 L is ________.
A) 0.800
B) 0.200
C) 0.500
D) 0.400
E) 8.00
39) The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of
solution is ________.
A) 0.0657
B) 1.85 ×
C) 1.85
D) 3.52
E) 0.104
40) The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of
solution is ________.
A) 5.46
B) 1.48
C) 0.104
D) 4.32
E) 1.85
41) The molarity (M) of an aqueous solution containing 22.5 g of glucose (C6H12O6) in 35.5 mL of
solution is ________.
A) 3.52
B) 0.634
C) 0.197
D) 0.125
E) 1.85
42) The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is
31
________.
A) 1.85
B) 2.12
C) 0.197
D) 3.52
E) 11.8
43) How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium
chloride?
A) 0.105
B) 6.11
C) 3.21
D) 6.11 × 103
E) 12.2
44) How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium
chloride?
A) 61.1
B) 1.05
C) 30.5
D) 6.11 × 104
E) 122
45) The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is
________.
A) 0.0879
B) 87.9
C) 0.0218
D) 0.0115
E) 0.870
46) The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500. mL is
________.
A) 57.2
B) 0.0044
C) 0.438
D) 0.0879
E) 0.870
47) The concentration of chloride ions in a 0.193 M solution of potassium chloride is ________.
A) 0.0643 M
B) 0.386 M
C) 0.0965 M
D) 0.579 M
E) 0.193 M
48) The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is ________.
A) 0.699 M
B) 0.233 M
C) 0.466 M
D) 0.0777 M
E) 0.155 M
49) The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.
A) 0.193 M
B) 0.386 M
C) 0.0965 M
D) 0.579 M
E) 0.0643 M
33
50) The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium
ion and ________ M sulfate ion.
A) 2.104, 1.052
B) 2.104, 2.104
C) 2.104, 4.208
D) 1.052, 1.052
E) 4.208, 2.104
51) When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the
concentration of HC2H3O2 is ________ M.
A) 3.33
B) 1.67
C) 0.835
D) 0.00167
E) 0.150
52) In a titration of 35.00 mL of 0.737 M H2SO4, ________ mL of a 0.827 M KOH solution is required for
neutralization.
A) 35.0
B) 1.12
C) 25.8
D) 62.4
E) 39.3
53) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a
0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.
A) 48.89
B) 97.78
C) 28.59
D) 1.086
E) 22.83
54) Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by
34
mass, then a 0.6543-g sample of that solid will require ________ mL of 0.3483 M NaOH for neutralization.
A) 11.19
B) 97.78
C) 28.59
D) 1.119
E) 22.39
55) A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for
neutralization. The concentration of acetic acid was ________ M.
A) 0.158
B) 0.423
C) 134
D) 6.88
E) 0.214
56) A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took
51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
A) 1.02
B) 0.114
C) 0.454
D) 0.113
E) 0.227
57) A 31.5 mL aliquot of HNO3 (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) 0.0051
C) 0.0204
D) 0.227
E) 1.02
58) A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It
