Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
Using a table of standard reductions potentials calculate the solubility product (Ksp) of the compound assigned to you. Write down the two balanced half-reactions and their voltages. Label the anode, the cathode, which cell is the oxidation and reduction and whether it is positive or negative. Indicate the direction of electron flow, the concentrations of all ionic species and the composition of the electrodes. Calculate the voltage of the cell and then, using the voltage, calculate the Ksp of your compound. MUST SHOW ALL WORK!
Calculation of the Ksp of Ag2CO3
Half reactions:
Overall Voltage:
![Thermochem
There are three tables for this electrochemical series. Each
table lists standard reduction potentials, E° values, at 298.15 K
(25 °C), and at a pressure of 101.325 kPa (1 atm) (not the standard
pressure of 1 bar). The activity of all soluble species is assumed
to be 1.000 mol/L. This is in particular important when pH (H+
or OH-) take part in the equilibrium. Table 1 is an alphabetical
listing of the elements, according to the symbol of the elements.
Thus, data for silver (Ag) precede those for aluminum (Al). Table
2 lists only those reduction reactions that have E° values posi-
tive in respect to the standard hydrogen electrode. In Table 2, the
reactions are listed in the order of increasing positive potential,
and they range from 0.0000 V to +3.4 V. Table 3 lists only those
reduction potentials that have Eº negative with respect to the
standard hydrogen electrode. In Table 3, the reactions are listed
in the order of decreasing potential and range from 0.0000 V to
TABLE 1. Alphabetical Listing
E°/V
-2.20
0.7996
1.980
0.643
0.07133
0.546
0.4647
0.22233
-0.017
0.47
0.4470
0.779
0.1478
-0.15224
0.354
0.4573
0.564
0.342
0.739
1.9
Ag³+ + e Ag²+
1.8
Ag₂O₂ + 4H+ + e = 2 Ag+ 2 H₂O
1.802
2 AgO + H₂O +2e= Ag₂O + 2OH- 0.607
AgOCN+eAg + OCN-
Ag₂S + 2 e 2 Ag + S²-
Ag₂S + 2 H+ + 2e = 2 Ag + H₂S
AgSCN+eAg + SCN-
0.41
-0.691
-0.0366
0.08951
0.3629
0.654
2 Ag + SeO₂²-
2 Ag + SO4²-
2 Ag+ WO₂²-
0.4660
-1.676
-2.30
-2.310
-2.33
-2.069
2.60
-1.9
Ac³+ + 3 e Ac
Ag+ + e
Ag2+ + e
Ag(ac) + e
Reaction
Ag
Ag+
5-78
Ag+ (ac)-
AgBr + e
AgBrO3 + e
Ag₂C₂O4 +2 e 2 Ag + C₂0,²-
AgCl +eAg + Cl-
AgCN + e Ag + CN-
Ag₂CO3 + 2 e 2 Ag+ CO₂²-
Ag + Br
Ag + BrO3-
Ag₂ CrO4 + 2 e 2 Ag + CrO₂²-
AgF+eAg + F-
Ag,[Fe(CN),]+4e 4Ag+[Fe(CN),]
Agle Ag+ I
AgIO3 +eAg + 10₂
Ag₂MoO4 + 2 e 2 Ag + MoO4²-
AgNO₂+ e Ag + 2 NO₂-
Ag₂O + H₂O + 2 e 2 Ag+ 2 OH-
Ag₂O3 + H₂O +2e=2 AgO+2OH-
Ag³+ + 2 e = Ag+
Ag₂SeO3 + 2 e
Ag₂SO4 + 2 e
Ag₂WO4 +2 e
Al³+ + 3 e = Al
Al(OH)3 + 3 e = Al + 3OH-
Al(OH)4 + 3e = Al + 4 OH-
H₂AlO3 + H₂O +3e Al +4 OH-
AlF³+3e Al + 6 F-
Am + e
Am³+
Am²+ + 2 e Am
ELECTROCHEMICAL SERIES
Petr Vanýsek
-4.10 V. The reliability of the potentials is not the same for all
the data. Typically, the values with fewer significant figures have
lower reliability. The values of reduction potentials, in particular
those of less common reactions, are not definite; they are subject
to occasional revisions.
Bi
Bit
Abbreviations: ac = acetate; bipy = 2,2'-dipyridine, or bipyri-
dine; en = ethylenediamine; phen = 1,10-phenanthroline.
Reaction
Am³+ + 3 e Am
Am³+ + e Am²+
As + 3 H + 3 e = AsH₂
As₂O3 + 6 H+ + 6 e 2 As + 3 H₂O
HASO₂ + 3H+ + 3 e As + 2 H₂O
AsO₂ + 2 H₂O + 3 e As + 4 OH-
H₂AsO4 + 2 H+ + 2e = HASO₂ + 2
H₂O
References
1. Milazzo, G., Caroli, S., and Sharma, V. K. Tables of Standard Elec-
trode Potentials, Wiley, 4th Edition, Chichester, 1978.
2. Bard, A. J., Parsons, R., and Jordan, J. Standard Potentials in Aque-
ous Solutions, Marcel Dekker, New York, 1985.
3. Bratsch, S. G. J. Phys. Chem. Ref. Data, 18, 1-21, 1989.
AsO³+2H₂O+2e AsO₂ +4OH-
At₂ + 2 e 2 At-
Aue Au
Au³+ + 2e Aut
Au³+ + 3e Au
Au²+ + e Au+
AuOH2+ + H+ + 2e
AuBr₂e Au + 2 Br
Aut + H₂O
AuBr + 3 e
Au + 4 Br
AuCl + 3 e
Au + 4 Cl
Au(OH)3 + 3 H+ + 3e Au +3
H₂O
H₂BO3 +5H₂O+8e BH₁+8OH-
H₂BO3 + H₂O + 3 e B+ 4 OH-
H₂BO3 + 3 H+ + 3e=B+ 3 H₂O
B(OH)3 + 7 H+ + 8e BH₂ + 3
H₂O
Ba2+ + 2 e Ba
Ba²+ + 2 e Ba(Hg)
Ba(OH)₂ + 2 e Ba + 2 OH-
Be²+ + 2 e Be
Be₂O32 + 3H₂O + 4e 2 Be +6 OH-
p-benzoquinone + 2 H+ + 2 e
hydroquinone
Bit + e Bi
Bi³+ + 3 e
Bi³+ + 2 e
Bi + 3 H + 3 e
BiH,
BiCl + 3 e Bi + 4 Cl
Bi₂O3 + 3 H₂O + 6 e
Eᵒ/V
-2.048
-2.3
-0.608
0.234
0.248
-0.68
0.560
-0.71
0.2
1.692
1.401
1.498
1.8
1.32
0.959
0.854
1.002
1.45
-1.24
-1.79
-0.8698
-0.481
-2.912
-1.570
-2.99
-1.847
-2.63
0.6992
0.5
0.308
0.2
-0.8
0.16
2 Bi + 6 OH- -0.46
Reaction
Bi₂O4 + 4 H+ + 2e = 2 BIO+ + 2
H₂O
BIO+ + 2 H+ + 3e Bi + H₂O
BIOCI + 2 H+ + 3 e Bi+ Cl +
H₂O
Bk++eBk³+
Bk2+ + 2 e Bk
Bk++eBk²+
Br₂(aq) + 2 e 2 Br
Br₂(1)+2 e 2 Br
HBrO + H+ + 2 e Br + H₂O
HBrO + H+ +e=1/2 Br₂(aq) +
H₂O
HBrO + H+ + e
BrO + H₂O +2 e
BrO3 +6 H+ + 5 e
H₂O
BrO₂ + 6 H+ + 6 e Br + 3 H₂O
BrO3 + 3 H₂O + 6 e Br +6 OH-
(CN)₂ + 2 H+ + 2e = 2 HCN
2 HCNO + 2 H+ + 2 e
H₂O
(CNS)₂ + 2 e 2 CNS-
CO₂ + 2 H+ + 2e = HCOOH
Cat + e = Ca
(CN)₂ + 2
Ca²+ + 2 e Ca
Ca(OH)₂ + 2 e Ca + 2 OH-
Calomel electrode, 1 molal KCI
1/2 Br₂(1) + H₂O
Br + 2OH-
1/2 Br₂ + 3
Calomel electrode, 1 molar KCl
(NCE)
Calomel electrode, 0.1 molar KCl
Calomel electrode, saturated KCI
(SCE)
Calomel electrode, saturated NaCl
(SSCE)
Cd²+ + 2 e
Cd²+ + 2 e
Cd
Cd(Hg)
Cd(OH)₂ + 2 e Cd(Hg) + 2 OH-
CdSO4 + 2 e Cd + SO4²-
Eᵒ/V
1.593
0.320
0.1583
1.67
-1.6
-2.8
1.0873
1.066
1.331
1.574
1.596
0.761
1.482
1.423
0.61
0.373
0.330
0.77
-0.199
-3.80
-2.868
-3.02
0.2800
0.2801
0.3337
0.2412
0.2360
-0.4030
-0.3521
-0.809
-0.246](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca2199f1-0096-4df2-b2ef-c79ddcec7676%2Fb39fce33-772a-4f6b-ac41-7dd3623230f1%2Fkckxcob_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Thermochem
There are three tables for this electrochemical series. Each
table lists standard reduction potentials, E° values, at 298.15 K
(25 °C), and at a pressure of 101.325 kPa (1 atm) (not the standard
pressure of 1 bar). The activity of all soluble species is assumed
to be 1.000 mol/L. This is in particular important when pH (H+
or OH-) take part in the equilibrium. Table 1 is an alphabetical
listing of the elements, according to the symbol of the elements.
Thus, data for silver (Ag) precede those for aluminum (Al). Table
2 lists only those reduction reactions that have E° values posi-
tive in respect to the standard hydrogen electrode. In Table 2, the
reactions are listed in the order of increasing positive potential,
and they range from 0.0000 V to +3.4 V. Table 3 lists only those
reduction potentials that have Eº negative with respect to the
standard hydrogen electrode. In Table 3, the reactions are listed
in the order of decreasing potential and range from 0.0000 V to
TABLE 1. Alphabetical Listing
E°/V
-2.20
0.7996
1.980
0.643
0.07133
0.546
0.4647
0.22233
-0.017
0.47
0.4470
0.779
0.1478
-0.15224
0.354
0.4573
0.564
0.342
0.739
1.9
Ag³+ + e Ag²+
1.8
Ag₂O₂ + 4H+ + e = 2 Ag+ 2 H₂O
1.802
2 AgO + H₂O +2e= Ag₂O + 2OH- 0.607
AgOCN+eAg + OCN-
Ag₂S + 2 e 2 Ag + S²-
Ag₂S + 2 H+ + 2e = 2 Ag + H₂S
AgSCN+eAg + SCN-
0.41
-0.691
-0.0366
0.08951
0.3629
0.654
2 Ag + SeO₂²-
2 Ag + SO4²-
2 Ag+ WO₂²-
0.4660
-1.676
-2.30
-2.310
-2.33
-2.069
2.60
-1.9
Ac³+ + 3 e Ac
Ag+ + e
Ag2+ + e
Ag(ac) + e
Reaction
Ag
Ag+
5-78
Ag+ (ac)-
AgBr + e
AgBrO3 + e
Ag₂C₂O4 +2 e 2 Ag + C₂0,²-
AgCl +eAg + Cl-
AgCN + e Ag + CN-
Ag₂CO3 + 2 e 2 Ag+ CO₂²-
Ag + Br
Ag + BrO3-
Ag₂ CrO4 + 2 e 2 Ag + CrO₂²-
AgF+eAg + F-
Ag,[Fe(CN),]+4e 4Ag+[Fe(CN),]
Agle Ag+ I
AgIO3 +eAg + 10₂
Ag₂MoO4 + 2 e 2 Ag + MoO4²-
AgNO₂+ e Ag + 2 NO₂-
Ag₂O + H₂O + 2 e 2 Ag+ 2 OH-
Ag₂O3 + H₂O +2e=2 AgO+2OH-
Ag³+ + 2 e = Ag+
Ag₂SeO3 + 2 e
Ag₂SO4 + 2 e
Ag₂WO4 +2 e
Al³+ + 3 e = Al
Al(OH)3 + 3 e = Al + 3OH-
Al(OH)4 + 3e = Al + 4 OH-
H₂AlO3 + H₂O +3e Al +4 OH-
AlF³+3e Al + 6 F-
Am + e
Am³+
Am²+ + 2 e Am
ELECTROCHEMICAL SERIES
Petr Vanýsek
-4.10 V. The reliability of the potentials is not the same for all
the data. Typically, the values with fewer significant figures have
lower reliability. The values of reduction potentials, in particular
those of less common reactions, are not definite; they are subject
to occasional revisions.
Bi
Bit
Abbreviations: ac = acetate; bipy = 2,2'-dipyridine, or bipyri-
dine; en = ethylenediamine; phen = 1,10-phenanthroline.
Reaction
Am³+ + 3 e Am
Am³+ + e Am²+
As + 3 H + 3 e = AsH₂
As₂O3 + 6 H+ + 6 e 2 As + 3 H₂O
HASO₂ + 3H+ + 3 e As + 2 H₂O
AsO₂ + 2 H₂O + 3 e As + 4 OH-
H₂AsO4 + 2 H+ + 2e = HASO₂ + 2
H₂O
References
1. Milazzo, G., Caroli, S., and Sharma, V. K. Tables of Standard Elec-
trode Potentials, Wiley, 4th Edition, Chichester, 1978.
2. Bard, A. J., Parsons, R., and Jordan, J. Standard Potentials in Aque-
ous Solutions, Marcel Dekker, New York, 1985.
3. Bratsch, S. G. J. Phys. Chem. Ref. Data, 18, 1-21, 1989.
AsO³+2H₂O+2e AsO₂ +4OH-
At₂ + 2 e 2 At-
Aue Au
Au³+ + 2e Aut
Au³+ + 3e Au
Au²+ + e Au+
AuOH2+ + H+ + 2e
AuBr₂e Au + 2 Br
Aut + H₂O
AuBr + 3 e
Au + 4 Br
AuCl + 3 e
Au + 4 Cl
Au(OH)3 + 3 H+ + 3e Au +3
H₂O
H₂BO3 +5H₂O+8e BH₁+8OH-
H₂BO3 + H₂O + 3 e B+ 4 OH-
H₂BO3 + 3 H+ + 3e=B+ 3 H₂O
B(OH)3 + 7 H+ + 8e BH₂ + 3
H₂O
Ba2+ + 2 e Ba
Ba²+ + 2 e Ba(Hg)
Ba(OH)₂ + 2 e Ba + 2 OH-
Be²+ + 2 e Be
Be₂O32 + 3H₂O + 4e 2 Be +6 OH-
p-benzoquinone + 2 H+ + 2 e
hydroquinone
Bit + e Bi
Bi³+ + 3 e
Bi³+ + 2 e
Bi + 3 H + 3 e
BiH,
BiCl + 3 e Bi + 4 Cl
Bi₂O3 + 3 H₂O + 6 e
Eᵒ/V
-2.048
-2.3
-0.608
0.234
0.248
-0.68
0.560
-0.71
0.2
1.692
1.401
1.498
1.8
1.32
0.959
0.854
1.002
1.45
-1.24
-1.79
-0.8698
-0.481
-2.912
-1.570
-2.99
-1.847
-2.63
0.6992
0.5
0.308
0.2
-0.8
0.16
2 Bi + 6 OH- -0.46
Reaction
Bi₂O4 + 4 H+ + 2e = 2 BIO+ + 2
H₂O
BIO+ + 2 H+ + 3e Bi + H₂O
BIOCI + 2 H+ + 3 e Bi+ Cl +
H₂O
Bk++eBk³+
Bk2+ + 2 e Bk
Bk++eBk²+
Br₂(aq) + 2 e 2 Br
Br₂(1)+2 e 2 Br
HBrO + H+ + 2 e Br + H₂O
HBrO + H+ +e=1/2 Br₂(aq) +
H₂O
HBrO + H+ + e
BrO + H₂O +2 e
BrO3 +6 H+ + 5 e
H₂O
BrO₂ + 6 H+ + 6 e Br + 3 H₂O
BrO3 + 3 H₂O + 6 e Br +6 OH-
(CN)₂ + 2 H+ + 2e = 2 HCN
2 HCNO + 2 H+ + 2 e
H₂O
(CNS)₂ + 2 e 2 CNS-
CO₂ + 2 H+ + 2e = HCOOH
Cat + e = Ca
(CN)₂ + 2
Ca²+ + 2 e Ca
Ca(OH)₂ + 2 e Ca + 2 OH-
Calomel electrode, 1 molal KCI
1/2 Br₂(1) + H₂O
Br + 2OH-
1/2 Br₂ + 3
Calomel electrode, 1 molar KCl
(NCE)
Calomel electrode, 0.1 molar KCl
Calomel electrode, saturated KCI
(SCE)
Calomel electrode, saturated NaCl
(SSCE)
Cd²+ + 2 e
Cd²+ + 2 e
Cd
Cd(Hg)
Cd(OH)₂ + 2 e Cd(Hg) + 2 OH-
CdSO4 + 2 e Cd + SO4²-
Eᵒ/V
1.593
0.320
0.1583
1.67
-1.6
-2.8
1.0873
1.066
1.331
1.574
1.596
0.761
1.482
1.423
0.61
0.373
0.330
0.77
-0.199
-3.80
-2.868
-3.02
0.2800
0.2801
0.3337
0.2412
0.2360
-0.4030
-0.3521
-0.809
-0.246
Transcribed Image Text:Cell Diagram:
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