Chem II test chapter 4
____
1) Aqueous potassium chloride will react with which one of the following in an exchange
(metathesis) reaction?
A) calcium nitrate
B) sodium bromide
C) lead nitrate
D) barium nitrate
E) sodium chloride
____
2) Which of the following is soluble in water at 25 °C?
A) Fe3 (PO4)2
B) Fe(OH)2
C) Fe(NO3)2
D) FeCO3
E) FeS
____
3) When aqueous solutions of __________ are mixed, a precipitate forms.
A) NiBr2 and AgNO3
B) NaI and KBr
C) K2SO4 and CrCl3
D) KOH and Ba(NO3)2
E) Li2CO3 and CsI
____
4) Which one of the following compounds is insoluble in water?
A) Na2CO3
B) K2SO4
C) Fe(NO3)3
D) ZnS
E) AgNO3
____
5) Which combination will produce a precipitate?
A) NH4OH (aq) and HCl (aq)
B) AgNO3 (aq) and Ca(C2H3O2)2 (aq)
C) NaOH (aq) and HCl (aq)
D) NaCl (aq) and H C2H3O2 (aq)
E) NaOH (aq) and Fe(NO3)2 (aq)
____
6) Which combination will produce a precipitate?
A) Pb(NO3)2 (aq) and HCl (aq)
B) Cu(NO3)2 (aq) and KC2H3O2 (aq)
C) KOH (aq) and HNO3 (aq)
D) AgC2H3O2 (aq) and HC2H3O2 (aq)
E) NaOH (aq) and Sr(NO3)2 (aq)
____
7) With which of the following will the ammonium ion form an insoluble salt?
A) chloride
B) sulfate
C) carbonate
D) sulfate and carbonate
E) none of the above
____
8) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide
is __________.
A) H+ (aq) + HSO4- (aq) + 2OH- (aq)  2 H2O (l) + NO3- (aq)
B) HNO3 (aq) + NaOH (aq)  NaNO3 (aq) + H2O (l)
C) H+ (aq) + OH- (aq)  H2O (l)
D) HNO3 (aq) + OH- (aq)  NO3- (aq) + H2O (l)
E) H+ (aq) + Na+ (aq) +OH- (aq)  H2O (l) + Na+ (aq)
____
9) Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
____
10) A compound was found to be soluble in water. It was also found that addition of acid to an
aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the
following cations would form a precipitate when added to an aqueous solution of this compound?
A) NH4+
B) K+
C) Cr3+
D) Rb+
E) Na+
____
11) Which hydroxides are weak bases?
A) KOH, Ba(OH)2
B) Sr(OH)2, KOH, NaOH, Ba(OH)2
C) KOH, NaOH
D) KOH, NaOH, Ba(OH)2
E) None of these is a weak base.
____
12) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is
__________.
A) HNO3 (aq) + Sr(OH)2 (aq)  Sr(NO3)2 (aq) + H2 (g)
B) HNO3 (aq) + Sr(OH)2 (aq)  H2O (l) + Sr(NO3)2 (aq)
C) HNO3 (aq) + SrOH (aq)  H2O (l) + SrNO3 (aq)
D) 2HNO3 (aq) + Sr(OH)2 (aq)  2 H2O (l) + Sr(NO3)2 (aq)
E) 2HNO3 (aq) + Sr(OH)2 (aq)  Sr(NO3)2 (aq) + 2 H2 (g)
____
13) In which reaction does the oxidation number of oxygen increase?
A) Ba(NO3)2 (aq) + K2SO4 (aq)  BaSO4 (s) + 2 KNO3 (aq)
B) HCl (aq) + NaOH (aq)  NaCl (aq) + H2O (l)
C) MgO (s) + H2O (l)  Mg(OH)2 (s)
D) 2 SO2 (g) + O2 (g)  2 SO3 (g)
E) 2 H2O (l)  2 H2 (g) + O2 (g)
____
14) In which species does nitrogen have the highest oxidation number?
A) N2
B) NH3
C) HNO2
D) NO2E) NaNO3
____
15) Of the choices below, which would be the best for the lining of a tank intended for use in storage
of hydrochloric acid?
A) copper
B) zinc
C) nickel
D) iron
E) tin
____
16) Which of these metals will be oxidized by the ions of cobalt?
A) nickel
B) tin
C) iron
D) copper
E) silver
____
17) Of the reactions below, only __________ is not spontaneous.
A) Mg (s) + 2HCl (aq)  MgCl2 (aq) + H2 (g)
B) 2Ag (s) + 2HNO3 (aq)  2AgNO3 (aq) + H2 (g)
C) 2Ni (s) + H2SO4 (aq)  Ni2SO4 (aq) + H2 (g)
D) 2Al (s) + 6HBr (aq)  2AlBr3 (aq) + 3 H2 (g)
E) Zn (s) + 2HI (aq)  ZnI2 (aq) + H2 (g)
____
18) Based on the activity series, which one of the reactions below will occur?
A) Fe (s) + ZnCl2 (aq)  FeCl2 (aq) + Zn (s)
B) Mn (s) + NiCl2 (aq)  MnCl2 (aq) + Ni (s)
C) Pb (s) + NiI2 (aq)  PbI2 (aq) + Ni (s)
D) SnBr2 (aq) + Cu (s)  CuBr2 (aq) + Sn (s)
E) None of the reactions will occur.
____
19) Oxidation is the __________ and reduction is the __________.
A) gain of oxygen, loss of electrons
B) loss of oxygen, gain of electrons
C) loss of electrons, gain of electrons
D) gain of oxygen, loss of mass
E) gain of electrons, loss of electrons
____
20) Oxidation and __________ mean essentially the same thing.
A) activity
B) reduction
C) metathesis
D) decomposition
E) corrosion
____
21) Which solution has the same number of moles of KCl as 75.00 mL of 0.250M solution of KCl?
A) 20.0 mL of 0.200M solution of KCl
B) 25.0 mL of 0.175M solution of KCl
C) 129 mL of 0.145M solution of KCl
D) 50.0 mL of 0.125M solution of KCl
E) 100 mL of 0.0500M solution of KCl
____
22) What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in
water and diluting to 725 mL?
A) 0.276 and 0.828
B) 0.828 and 0.276
C) 0.276 and 0.276
D) 0.145 and 0.435
E) 0.145 and 0.0483
____
23) What are the respective concentrations (M) of Cu+2 and Cl- afforded by dissolving 0.200 mol
CuCl2 in water and diluting to 345 mL?
A) 0.200 and 0.200
B) 0.580 and 1.16
C) 0.200 and 0.400
D) 1.16 and 2.32
E) 0.580 and 0.290
____
24) Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a __________.
A) crystallization
B) neutralization
C) twofold dilution
D) tenfold dilution
E) titration
____
25) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to
350. mL to make a 2.75 M solution of magnesium chloride?
A) 2.75
B) 50.0
C) 45.0
D) 107
E) 350
____
26) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to
200.0 mL to make a 0.880 M solution of sodium hydroxide?
A) 2.64
B) 176
C) 26.4
D) 29.3
E) 50.0
____
27) What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an
iodide ion concentration of 0.193 M?
A) 9.44
B) 18.9
C) 0.024
D) 0.048
E) 37.7
____
28) What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of
aqueous hydrobromic acid?
A) 1.44
B) 1.23
C) 53.6
D) 34.5
E) 188
____
29) What mass (g) of CaF2 is formed when 47.8 mL of 0.334 M NaF is treated with an excess of
aqueous calcium nitrate?
A) 1.25
B) 0.472
C) 2.49
D) 0.943
E) 0.623
____
30) What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5
g of NaOH in 350 mL of water?
A) 50.0
B) 0.44
C) 1.75
D) 0.070
E) 1.75  10-3
____
31) The point in a titration at which the indicator changes is called the __________.
A) setpoint
B) indicator point
C) standard point
D) endpoint
E) volumetric point
____
32) Which one of the following substances is produced during the reaction of an acid with a metal
hydroxide?
A) H2
B) H2O
C) CO2
D) NaOH
E) O2
____
33) A 13.8 mL aliquot of 0.176 M H3PO4 (aq) is to be titrated with 0.110 M NaOH (aq). What volume
(mL) of base will it take to reach the equivalence point?
A) 7.29
B) 22.1
C) 199
D) 66.2
E) 20.9
____
34) What volume (mL) of 7.48  10-2 M phosphoric acid can be neutralized with 115 mL of 0.244 M
sodium hydroxide?
A) 125
B) 375
C) 750
D) 188
E) 75.0
____
35) A strong electrolyte is one that __________ completely in solution.
A) reacts
B) associates
C) disappears
D) ionizes
____
36) What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
A) K+ and H+
B) H+ and OHC) K+ and NO3D) H+ and NO3E) OH- only
____
37) What are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?
A) K+ and Ag+
B) Ag+ and ClC) K+ and NO3D) Ag+ and NO3E) K+ only
____
38) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) Mg+2 and H+
B) H+ and OHC) Mg+2 and ClD) H+ and ClE) OH- only
____
39) Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s)
is/are spectator ions in the reaction?
A) Ba2+ only
B) Na+ only
C) Ba2+ and SO42-
D) Na+ and IE) SO42- and I____
40) The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and
CaCl2 are mixed is __________.
A) 2Na+ (aq) + CO32- (aq)  Na2CO3 (aq)
B) 2Na+ (aq) + 2Cl- (aq)  2NaCl (aq)
C) Na+ (aq) + Cl- (aq)  NaCl (aq)
D) Ca2+ (aq) + CO32- (aq)  CaCO3 (s)
E) Na2CO3 (aq) + CaCl2 (aq)  2NaCl (aq) + CaCO3 (s)
____
41) 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)  2 H2O (l) + SO42- (aq)
E) 2H+ (aq) + 2NaOH (aq)  2 H2O (l) + 2Na+ (aq)
____
42) The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide
are __________.
A) OH- and ClO4B) H+, OH-, ClO4-, and Ba2+
C) H+ and OHD) H+ and Ba2+
E) ClO4- and Ba2+
____
43) 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
____
44) 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
____
45) Which of these metals is the most easily oxidized?
Na
Au
Fe
Ca
Ag
A)
B)
C)
D)
E)
____
Na
Au
Fe
Ca
Ag
46) 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)
B)
C)
D)
E)
Ni
Ag
Cu
Pb
N
____
47) When gold dissolves in aqua regia, what is reduced?
A) H+
B) N+5
C) ClD) H2O
E) Au
____
48) 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
____
49) 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
____
50) The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was
diluted to 0.800 L is __________.
A) 0.800
B) 0.200
C) 0.500
D) 0.400
E) 8.00
____
51) The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of
solution is __________.
A)
B)
C)
D)
E)
5.46
1.48
0.104
4.32
1.85
____
52) 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
____
53) 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
____
54) 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
____
55) The total concentration of ions in a 0.625 M solution of HCl is __________.
A) 0
B) 0.500 M
C) 0.625 M
D) 1.25 M
E) 1.50 M
____
56) How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 1.0 M
CH3OH?
A) 0.15
B) 430
C) 2.4
D) 4.8
E) 4.3
____
57) There are __________ mol of bromide ions in 0.500 L of a 0.100 M solution of AlBr3.
A) 0.0500
B)
C)
D)
E)
0.450
0.150
0.167
0.500
____
58) What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in
sufficient water to give exactly 230. mL of solution?
A) 11.9
B) 1.59
C) 0.00159
D) 3.17
E) 0.0841
____
59) How many grams of H3PO4 are in 175 mL of a 2.50 M solution of H3PO4?
A) 0.438
B) 20.0
C) 42.9
D) 4.90
E) 612
60) How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?
61) What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in
sufficient water to give 425 mL of solution?
____
62) Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.
A) 148
B) 1.68
C) 5.30  103
D) 5.30
E) 1.68  10-3
63) When gold dissolves in aqua regia, into what form is the gold converted?
____
64) Ca(OH)2 is a strong base.
____
65) The compound HClO4 is a weak acid.
____
66) HNO2 is a strong acid.
____
67) The compound NH4Cl is a weak acid.
____
68) Ammonia is a strong base.
AP chem test chapter 4
Answer Section
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C
C
A
D
E
A
E
C
E
C
E
D
E
E
A
C
B
B
C
E
C
A
B
C
D
D
A
B
E
C
D
B
D
A
D
C
C
C
D
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1
1
1
1
1
1
1
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1
1
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1
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1
1
1
1
1
1
1
1
1
1
1
1
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1
1
1
1
1
1
1
1
1
1
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2
2
1
3
3
1
3
2
4
2
2
3
4
5
5
4
4
2
2
4
4
4
2
2
2
3
4
4
4
1
2
4
4
2
2
2
2
2
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Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.3
Sec. 4.3
Sec. 4.3
Sec. 4.3
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.4
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.6
Sec. 4.6
Sec. 4.6
Sec. 4.6
Sec. 4.6
Sec. 4.6
Sec. 4.6
Sec. 4.1
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
40)
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45)
46)
47)
48)
49)
50)
51)
52)
53)
54)
55)
56)
57)
58)
59)
60)
D
C
E
E
A
D
A
B
D
B
C
D
A
B
A
D
D
C
B
C
PTS:
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1
1
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1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
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PTS: 1
61) ANS:
0.29
DIF:
3
REF: Sec. 4.5
PTS: 1
62) ANS: D
63) ANS:
AuCl4- (aq)
DIF:
PTS:
3
1
REF: Sec. 4.5
DIF: 2
REF: Sec. 4.5
PTS:
ANS:
ANS:
ANS:
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ANS:
DIF:
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3
1
1
1
1
1
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64)
65)
66)
67)
68)
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39.0
1
T
F
F
T
F
3
2
3
2
2
3
3
4
3
3
2
3
3
3
4
1
3
3
3
3
Sec. 4.5
1
2
1
2
1
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Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.2
Sec. 4.3
Sec. 4.4
Sec. 4.4
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.6
Sec. 4.1
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.5
Sec. 4.3
Sec. 4.3
Sec. 4.3
Sec. 4.3
Sec. 4.3