Questions-on-chapter-4-aqueous

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Selected Questions on Chapter 4
Reactions in Aqueous Solutions
Circle the correct answer:
1) The reaction HNO3(aq) + KOH(aq) → KNO3 (aq) + H2O(l) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) exchange reaction.
2) The reaction 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3 )2 (aq) + 2 H2O(l) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) exchange reaction.
3) The reaction Pb(NO3)2(aq) + K2 SO4(aq) → PbSO4(s) + 2 KNO3(aq) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) single replacement reaction.
4) The reaction Na3PO4(aq) + 3 AgNO3(aq) → Ag3 PO4(s) + 3 NaNO3(aq) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) single replacement reaction.
5) The reaction Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) is best classified as a(n)
A) acid-base neutralization reaction.
B) double replacement reaction.
C) oxidation-reduction reaction.
D) precipitation reaction.
6) The reaction C6H12 O6(s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O(l) is best classified as a(n)
A) acid-base neutralization reaction.
B) double replacement reaction.
C) oxidation-reduction reaction.
D) precipitation reaction.
7) The combustion reaction CH4(g) + 2 O2(g) → CO2 (g) + 2 H2O(l) can be classified as a(n)
A) acid-base neutralization reaction.
B) double replacement reaction.
C) oxidation-reduction reaction.
D) precipitation reaction.
8) HBr, HCl, HClO4, KBr, and NaCl are all classified as
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A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
9) Acetic acid (CH3CO2 H), formic acid (HCO2H), hydrofluoric acid (HF), ammonia (NH3), and
methylamine (CH3 NH2) are commonly classified as
A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
10) Methyl alcohol (CH3OH), ethyl alcohol (CH3CH2 OH), ethylene glycol (HOCH2CH2 OH), and
sucrose (C12H22 O11) are commonly classified as
A) bases.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
11) In a solution prepared by mixing CH3 OH with H2O the major species present are
A) CH3 OH and H2 O
B) CH3OH, H+, and OHC) CH3+, OH-, and H2O
D) CH3 O-, H+, and H2O
12) What is the molar concentration of sodium ions in a 0.350 M Na3PO4 solution?
A) 0.117 M
B) 0.350 M
C) 1.05 M
D) 1.40 M
13) What is the molar concentration of sulfate ions in a 0.150 M Na2SO4 solution?
A) 0.075 M
B) 0.150 M
C) 0.300 M
D) 0.450 M
14) Write a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq).
A) Pb(NO3)2 (aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)
B) Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) → Pb2+(aq) + 2 I-(aq) + 2 Na+(aq) + 2 NO3 -(aq)
C) Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2 I-(aq) → PbI2 (s) + 2 Na+(aq) + 2 NO3-(aq)
D) Pb2+(aq) + 2 I-(aq) → PbI2(s)
15) Write a balanced net ionic equation for the reaction of H2SO4 (aq) with Ba(OH)2 (aq).
A) H2 SO4(aq) + Ba(OH)2 (aq) → BaSO4 (s) + 2 H2O(l)
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B) 2 H+(aq) + SO42-(aq) + Ba2+(aq) + 2 OH-(aq) → BaSO4(s) + 2 H2O(l)
C) H+(aq) + OH+(aq) → H2O(l)
D) Ba2+(aq) + SO42-(aq) → BaSO4(s)
16) Write a balanced net ionic equation for the reaction of Na2 CO3(s) and HCl(aq).
A) Na2CO3 (s) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g)
B) 2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) + H2 O(l) + CO2(g)
C) Na2CO3 (s) + 2 H+(aq) → 2 Na+(aq) + H2O(l) + CO2(g)
D) CO3 2-(aq) + 2 H+(aq) → H2O(l) + CO2(g)
17) Write a balanced net ionic equation for the reaction of AgNO3 (aq) with Cu(s).
A) AgNO3(aq) + Cu(s) → Ag(s) + CuNO3(aq)
B) Ag+(aq) + Cu(s) → Ag(s) + Cu+(aq)
C) 2 AgNO3(aq) + Cu(s) → 2 Ag(s) + CuNO3(aq)
D) 2Ag+(aq) + Cu(s) → 2 Ag(s) + Cu2+(aq)
18) Write a balanced net ionic equation for the reaction of AgNO3 (aq) with KBr(aq).
A) AgNO3(aq) + KBr(aq) → AgBr(aq) + KNO3 (s)
B) Ag+(aq) + NO3 -(aq) + K+(aq) + Br-(aq) → Ag+(aq) + Br-(aq) + KNO3(s)
C) Ag+(aq) + NO3 -(aq) + K+(aq) + Br-(aq) → AgBr(s) + K+(aq) + NO3 -(aq)
D) Ag+(aq) + Br-(aq) → AgBr(s)
19) Write a balanced net ionic equation for the reaction of CdCl2(aq) with Na2S(aq).
A) CdCl2 (aq) + Na2S(aq) → CdS (aq) + 2 NaCl(aq)
B) Cd2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + S2-(aq) → CdS(s) + 2 NaCl(aq)
C) Cd2+(aq) + S2-(aq) → CdS(s)
D) Cd 2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + S2-(aq) → CdS(s) + 2 Na+(aq)
20) Write a balanced net ionic equation for the reaction of NiBr2(aq) with (NH4)2S(aq).
A) NiBr2(aq) + (NH4)2S(aq) → NiS(s) + 2 NH4 Br(aq)
B) Ni2+(aq) + 2 Br-(aq) + 2 NH4+(aq) + S2-(aq) → NiS(s) + 2 NH4+(aq) + 2 Br-(aq)
C) Ni2+(aq) + 2 Br-(aq) + 2 NH4+(aq) + S2-(aq) → NiS(s) + 2 NH4Br(s)
D) Ni2+(aq) + S2-(aq) → NiS(s)
21) In the reaction AgNO3 (aq) + HI(aq) → AgI(s) + HNO3(aq) the spectator ions are
A) Ag+ and NO3–
B) Ag+ and I–
C) H+ and I–
D) H+ and NO3–
22) Which one of the following compounds is insoluble in water?
A) K2 SO4
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B) NaNO3
C) PbSO4
D) Rb 2CO3
23) Which pair of compounds is insoluble in water?
A) AgNO3 and KNO3
B) Na2S and CuS
C) (NH4)2SO4 and AgI
D) PbSO4 and Pb3(PO4)2
24) Which one of the following compounds is soluble in water?
A) Ag3PO4
B) CuS
C) Pb(NO3)2
D) ZnCO3
25) Which pair of compounds is soluble in water?
A) AgBr and AgI
B) CdS and (NH4)2S
C) KI and Ba(NO3)2
D) NaNO3 and CuCO3
26) A 31.5 mL aliquot of H2 SO4 (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
27) The mixing of which pair of reactants will result in a precipitation reaction?
A) CsI(aq) + NaOH(aq)
B) HCl(aq) + Ca(OH)2 (aq)
C) K2 SO4(aq) + Ba(NO3)2(aq)
D) NaNO3(aq) + NH4Cl(aq)
28) The mixing of which pair of reactants will result in a precipitation reaction?
A) Cu(NO3 )2 (aq) + Na2CO3(aq)
B) K2 SO4(aq) + Cu(NO3)2(aq)
C) NaClO4(aq) + (NH4)2S(aq)
D) NH4 Br(aq) + NaI(aq)
29) What reagent could be used to separate Br- from NO3- when added to an aqueous solution
containing both?
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A) AgNO3(aq)
B) Ba(OH)2(aq)
C) CuSO4(aq)
D) NaI(aq)
30) What reagent could not be used to separate Cl- from OH- when added to an aqueous solution
containing both?
A) AgNO3(aq)
B) Ca(NO3)2 (aq)
C) Cu(NO3 )2 (aq)
D) Fe(NO3)3 (aq)
31) Predict the products of a reaction between AgNO3(aq) and KBr(aq).
A) Ag(s) and NO(g)
B) Ag(s) and Br2 (l)
C) AgBr(s) and KNO3(aq)
D) AgNO3(aq) and KBr(aq)
32) Predict the products of a reaction between Ba(NO3 )2(aq) and K2SO4 (aq).
A) Ba(s), KNO3(aq) and K2 SO3(aq)
B) BaSO3(s) and KNO2(aq)
C) BaSO3(s) and KNO3(aq)
D) BaSO4(s) and KNO3(aq)
33) Which pair of reactants will produce a precipitate when mixed together?
A) HCl(aq) and NaOH(aq)
B) HCl(aq) and Na2CO3 (aq)
C) HCl(aq) and Na2S(aq)
D) HCl(aq) and Pb(NO3 )2 (aq)
34) When K2 SO4(aq) and Pb(NO3)2(aq) are mixed, a white colored precipitate forms which is
A) KNO3.
B) K2 SO3.
C) Pb.
D) PbSO4.
35) When Na2CrO4(aq) and AgNO3(aq) are mixed, a red colored precipitate forms which is
A) Ag.
B) Ag2CrO4.
C) AgNO3.
D) NaNO3.
36) What reagent would distinguish between Ba2+ and Pb2+?
A) NaCl
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B) NaNO3
C) Na2SO4
D) Na2S2 O3
37) What reagent would distinguish between Ag+ and Fe3+?
A) NaClO3
B) NaI
C) NaNO3
D) NaOH
38) Which of the following compounds is not an Arrhenius acid?
A) CH3 CO2H
B) CH3NH2
C) HNO3
D) H2 SO4
39) What ion is provided when Arrhenius bases dissolve in water?
A) H+
B) Na+
C) ClD) OH40) When dissolved in water, LiOH behaves as
A) an acid that forms Li+ and OH- ions.
B) an acid that forms LiO- and H+ ions.
C) a base that forms Li+ and OH- ions.
D) a base that forms LiO- and H+ ions.
41) Which of the following compounds is an Arrhenius base in water?
A) C6 H12O6
B) HOClO2
C) H2 SO4
D) NH3
42) Which of the following compounds is an Arrhenius base in water?
A) CH3 OH
B) CH3CO2H
C) HOCl
D) KOH
43) Which one of the following compounds behaves as an acid when dissolved in water?
A) BaO
B) CH4
C) HBr
D) KOH
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44) When dissolved in water, of HClO4, Ca(OH)2, KOH, HI, which are acids?
A) Ca(OH)2 and KOH
B) HClO4 and HI
C) only HI
D) only KOH
45) When dissolved in water, of HClO4 , Ca(OH)2, KOH, HI, which are bases?
A) Ca(OH)2 and KOH
B) HClO4 and HI
C) only HI
D) only KOH
46) Which of the following is not a strong acid?
A) HF
B) HCl
C) HBr
D) HI
47) How many H+ ions can the acid, H2CO3, donate per molecule?
A) 0
B) 1
C) 2
D) 3
48) How many H+ ions can the acid H3 PO4 donate per molecule?
A) 0
B) 1
C) 2
D) 3
49) How many H+ ions can the acid CH3CO2H donate per molecule?
A) 1
B) 2
C) 3
D) 4
50) Write a net ionic equation for the neutralization reaction of HCN(aq) with NaOH(aq).
A) HCN(aq) + NaOH(aq) → NaCN(aq) + H2O(l)
B) HCN(aq) + Na+(aq) + OH-(aq) → Na+(aq) + CN-(aq) + H2O(l)
C) HCN(aq) + OH-(aq) → CN-(aq) + H2 O(l)
D) H+(aq) + OH-(aq) → H2 O(l)
51) Write a net ionic equation for the neutralization reaction of H3 PO4(aq) with Ba(OH)2(aq).
A) 2 H3 PO4(aq) + 3 Ba(OH)2 (aq) → Ba3(PO4)2(s) + 6 H2O(l)
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B) 2 H3 PO4(aq) + 3 Ba2+(aq) + 6 OH-(aq) → Ba3(PO4 )2 (s) + 6 H2O(l)
C) 6 H+(aq) + 2 PO43-(aq) + 3 Ba2+(aq) + 6 OH-(aq) → Ba3 (PO4 )2 (s) + 6 H2O(l)
D) H+(aq) + OH-(aq) → H2 O(l)
52) What is the oxidation number of the sulfur atom in S8?
A) –2
B) 0
C) +6
D) +8
53) What is the oxidation number of the sulfur atom in H2SO4?
A) -2
B) +2
C) +4
D) +6
54) What is the oxidation number of the chromium atom in K2 Cr2 O7?
A) -2
B) +2
C) +6
D) +7
55) What is the oxidation number of the oxygen atom in H2O2?
A) -2
B) -1
C) +1
D) +2
56) In which compound is the oxidation number of oxygen not –2?
A) MgO
B) Li2O
C) Na2O2
D) Al2O3
57) In which compound is the oxidation number of hydrogen not +1?
A) H2 O
B) H2 O2
C) NaH
D) Na2HSO4
58) What is the oxidation number change (final- initial) for the manganese atom in the following
unbalanced reduction half reaction?
MnO4 -(aq) + H+(aq) → Mn2+(aq) + H2O(l)
A) -7
B) -5
C) +5
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D) +7
59) What is the oxidation number change (final- initial) for the iron atom in the following reaction?
2 Fe2 O3(s) + 3 C(s) → 4 Fe(s) + 3 CO2(g)
A) -6
B) -3
C) +3
D) +6
60) Which species functions as the oxidizing agent in the following reduction-oxidation reaction? Use
the activity series
Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)
A) Cu(s)
B) Cu2+(aq)
C) Zn(s)
D) Zn 2+(aq)
61) Which species functions as the oxidizing agent in the following reduction-oxidation reaction?
5 Fe2+(aq) + MnO4 -(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2 O(l)
A) Fe2+(aq)
B) H+(aq)
C) Mn2+(aq)
D) MnO4 -(aq)
62) Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4 ), by
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
63) A 17.5 mL sample of an acetic acid (CH3 CO2H) 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
64) 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
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D) 0.113
E) 0.227
65) 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
66) Which species functions as the reducing agent in the following reduction-oxidation reaction?
2 P(s) + 3 Br2(l) → 2 PBr3(l)
A) Br-(aq)
B) Br2(l)
C) P(s)
D) P3+(aq)
67) Which species functions as the reducing agent in the following reduction-oxidation reaction?
ZnO(s) + C(s) → Zn(s) + CO(g)
A) C(s)
B) CO(g)
C) Zn(s)
D) ZnO(s)
68) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2 O4) 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
69) In the reaction 2 H2O2 (l) → 2 H2 O(l) + O2(g) oxygen is
A) both oxidized and reduced.
B) neither oxidized nor reduced.
C) only oxidized.
D) only reduced.
70) Using the following portion of the activity series for oxidation half-reactions, determine which
combination of reactants will result in a reaction.
Na(s) → Na+(aq) + eCr(s) → Cr3+(aq) + 3eA) Na(s) with Cr(s)
B) Na(s) with Cr3+(aq)
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C) Na+(aq) with Cr3+(aq)
D) Na+(aq) with Cr(s)
71) Using the following portion of the activity series for oxidation half reactions
K(s) → K+(aq) + eAl(s) → Al3+(aq) + 3eFe(s) → Fe2+(aq) + 2eSn(s) → Sn2+(aq) + 2edetermine which reaction will occur.
A) Al3+(aq) with Fe(s)
B) Al(s) with Sn(s)
C) K+(aq) with Fe2+(aq)
D) K(s) with Sn2+(aq)
72) Using the following portion of the activity series for oxidation half reactions
Ca(s) → Ca2+(aq) + 2eMg(s) → Mg2+(aq) + 2eZn(s) → Zn2+(aq) + 2eCu(s) → Cu2+(aq) + 2edetermine which reaction will not occur.
A) Ca(s) with Cu2+(aq)
B) Ca(s) with Zn2+(aq)
C) Zn(s) with Cu2+(aq)
D) Zn(s) with Mg2+(aq)
73) Using the following portion of the activity series for oxidation half reactions
Mg(s) → Mg2+(aq) + 2eZn(s) → Zn2+(aq) + 2eCu(s) → Cu2+(aq) + 2eindicate which pairs of reactions will occur.
A) Cu(s) with Zn2+(aq) and Zn(s) with Mg2+(aq)
B) Mg(s) with Cu2+(aq) and Zn2+(aq) with Mg2+(aq)
C) Mg(s) with Cu(s) and Zn(s) with Cu(s)
D) Mg(s) with Zn2+(aq) and Zn(s) with Cu2+(aq)
74) Using the following portion of the activity series for oxidation half reactions
K(s) → K+(aq) + eAl(s) → Al3+(aq) + 3eFe(s) → Fe2+(aq) + 2eSn(s) → Sn2+(aq) + 2edetermine which pairs of reactions will occur.
A) Al(s) with Fe2+(aq) and Sn(s) with K+(aq)
B) Fe(s) with Al(s) and Al3+(aq) with Sn2+(aq)
C) Fe(s) with Sn2+(aq) and Al(s) with Sn2+(aq)
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D) K(s) with Al3+(aq) and Fe(s) with Al3+(aq)
75) When 0.500 mol of HC2 H3O2 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
76) 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
77) Coinage metals are metals that are not easily oxidized. Based on the activity series, which metal
would be least desirable as a coinage metal?
A) Al
B) Au
C) Mg
D) Mn
78) Based on the activity series, which metal dissolves in hydrochloric acid to produce hydrogen gas?
A) Ag
B) Au
C) Co
D) Cu
79) Which elements will react rapidly with aqueous H+ ions and also with liquid H2O?
A) Al, Cr, Fe, Mn, Zn
B) Au, Co, Cu, Ni, Sn
C) Au, Li, K, Ni, Sn
D) Ba, Ca, Li, K, Na
80) Which elements will not react with liquid water but will react with aqueous H+ ions?
A) Ag, Cu, Hg, Pt
B) Al, Cr, Mn, Zn
C) Ba, Ca, Li, Na
D) Ag, Au, Ca, K
81) Which elements will not react with liquid water or with aqueous H+ ions?
A) Ag, Au, Hg, Pt
B) Ba, Ca, Li, K
C) Co, Cu, Ni, Sn
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D) Cr, Fe, Mn, Zn
82) 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
83) 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
84) 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
85) 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
86) The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12 H22 O11) in 35.5 mL of
solution is __________.
A) 0.0657
B) 1.85 ×
C) 1.85
D) 3.52
E) 0.104
87) The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12 H22 O11) in 35.5 mL of
solution is __________.
A) 5.46
B) 1.48
C) 0.104
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D) 4.32
E) 1.85
88) 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
89) The molarity of an aqueous solution containing 75.3 g of glucose (C6 H12 O6) in 35.5 mL of solution
is __________.
A) 1.85
B) 2.12
C) 0.197
D) 3.52
E) 11.8
90) 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
91) 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
92) 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
93) 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
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C) 0.438
D) 0.0879
E) 0.870
94) 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
95) 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
96) 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
97) 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
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