announcements - university of california,...
TRANSCRIPT
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Announcements• This is a learning experience for us all Thank you for understanding (kinetics, quiz, etc.) Read the book (and handouts on website)!
• Science clarifications Electrons can be in a beaker (solvated electrons) versus protons in a beaker (solvated protons = hydroniums and beyond), but protons are energetically easier to solvate
Salt bridges have spectator ions only
Course websitehttp://faculty.sites.uci.edu/chem2l/chem-h2lcm3lc/
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Button cell
CATHODE CAP
MOST COMMON BATTERIES – CLARIFICATION
Separator is the salt bridge; it contains an inert, redox inactive
salt solution (electrolyte)
Dendrites = Shunts
intercalated
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Week 6 Objectives
By the end of the week, you will be able to:
• Understand everything that I flew through before
• Use alpha fractions for electrochemical reactions
• Explain how ion‐selective electrodes and pH meters work
• Explain how the solubility product is pertinent to electrochemical reactions
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can be; but they are not. Use SHE!
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Electrochemical Alpha Fractions
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= Ideally polarizable electrodes
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –
Pt(s)‐Hg(l) Hg2Cl2(s)
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –
Pt(s)‐Hg(l) Hg2Cl2(s)
Eo(Cu2+/Cu) = +0.1 V vs. SCE
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –
Pt(s)‐Hg(l) Hg2Cl2(s)
Eo(Cu2+/Cu) = +0.1 V vs. SCE
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –Eo(Cu2+/Cu) = +0.1 V vs. SCE
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)
Pt(s)‐Hg(l) Hg2Cl2(s)+ Cl–(aq)
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –Eo(Cu2+/Cu) = +0.1 V vs. SCE
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s)‐Hg(l) Hg2Cl2(s)+ Cl–(aq)
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Write and explain the line notation for the redox reactionbetween Cu/Cu2+ and an SCE electrode, where Cu2+ is CuSO4(0.1 M), and KCl (1 M) is present in all cells.
Cu SCE
Cu2+(aq) Cu(s)
– –Eo(Cu2+/Cu) = +0.1 V vs. SCE
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
Pt(s)‐Hg(l) Hg2Cl2(s)+ Cl–(aq)
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Cu SCE
Cu2+(aq) Cu(s)
– –
Pt(s)‐Hg(l) Hg2Cl2(s)+ Cl–(aq)
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)
Eo(Cu2+/Cu) = +0.1 V vs. SCE
Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
(a) What is Ecell in this case?
(b) What is Ecell if [KCl] = 0.1 M?
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(a) What is Ecell in this case?
(b) What is Ecell if [KCl] = 0.1 M?Eo(Cu2+/Cu) = +0.1 V vs. SCE
ln
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
(a)
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(a) What is Ecell in this case?
(b) What is Ecell if [KCl] = 0.1 M?Eo(Cu2+/Cu) = +0.1 V vs. SCE
ln
0.0592Vlog
1
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
(a)
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(a) What is Ecell in this case?
(b) What is Ecell if [KCl] = 0.1 M?Eo(Cu2+/Cu) = +0.1 V vs. SCE
ln
0.1V0.0592V
2 log10.1
0.1V 0.0296V 0.0704V
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
(a)
0.0592Vlog
1
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(a) What is Ecell in this case?
(b) What is Ecell if [KCl] = 0.1 M?Eo(Cu2+/Cu) = +0.1 V vs. SCE
ln
0.1V0.0592V
2 log10.1
0.1V 0.0296V 0.0704V
Pt(s) | Hg(l) | Hg2Cl2(s) | KCl(1M, aq) | KCl(1M, aq) | KCl(1M, aq), CuSO4 (0.1M, aq) | Cu(s)Pt(s) | Hg(l) | Hg2Cl2(s) | Cl–(1M, aq) | | Cu2+ (0.1M, aq) | Cu(s)
Pt(s) | Hg(l) | Hg2Cl2(s) | | | Cu2+ | Cu(s)
0.1V0.0592V
2 log1
0.1
0.1V 0.0888V 0.0112V
(a)
(b)
0.0592Vlog
1
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EoxEred
Donnan Potential(not a liquid junction
potential)
Frederick G. Donnan(1870–1956)(from Wiki)
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Other Types of Electrodes
Membrane and Ion Selective Electrodes (ISEs)
pH Electrode
Ca2+ Electrode
NO3- Electrode
Corning glass membrane
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(from Prof. Penner’s Electrochemistry graduate‐level course)
Arnold Orville Beckman(1900–2004)(from Wiki)
porousglass frit
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(from Prof. Penner’s Electrochemistry graduate‐level course)
forms a Donnan Potential
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ALSO forms a Donnan Potential
(from Prof. Penner’s Electrochemistry graduate‐level course)
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ALSO forms a Donnan Potential
(from Prof. Penner’s Electrochemistry graduate‐level course)
(indicator electrode) (reference electrode)
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ALSO forms a Donnan Potential
(from Prof. Penner’s Electrochemistry graduate‐level course)
SCE electrode(ideally non-polarizable)
(indicator electrode) (reference electrode)
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Other Types of Electrodes
Membrane and Ion Selective Electrodes (ISEs)
pH Electrode
Ca2+ Electrode
NO3- Electrode
Polymer (PVC)membrane electrode containing a calcium ionophore
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Other Types of Electrodes
Membrane and Ion Selective Electrodes (ISEs)
pH Electrode
Ca2+ Electrode
NO3- Electrode
Polymer (PVC)membrane electrode containing a nitrate ionophore
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General ion-selective-electrode specifics
Ca2+ electrode NO3– electrodeIon Range 5x10-6 – 1 M 7x10-6 – 1 MpH Range 3 – 10 2.5 – 11
Interfering Ions various M2+ various A–
Electrode slope +28 mV/decade -56 mV/decade
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General ion-selective-electrode specifics
For nitrate
Thermo Scientific, ISE Manuals
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General ion-selective-electrode specifics
Thermo Scientific, ISE Manuals
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General ion-selective-electrode specifics
Ca2+ electrode NO3– electrodeIon Range 5x10-6 – 1 M 7x10-6 – 1 MpH Range 3 – 10 2.5 – 11
Interfering Ions various M2+ various A–
Electrode slope +28 mV/decade -56 mV/decade
How can we deal with interfering ions? Remove them!
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General ion-selective-electrode specifics
Ca2+ electrode NO3– electrodeIon Range 5x10-6 – 1 M 7x10-6 – 1 MpH Range 3 – 10 2.5 – 11
Interfering Ions various M2+ various A–
Electrode slope +28 mV/decade -56 mV/decade
How can we deal with interfering ions? Remove them!
Why is the electrode slope +28 and -56 mV per decade?The Nernst equation
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General ion-selective-electrode specifics
For nitrate1–
Thermo Scientific, ISE Manuals
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General ion-selective-electrode specifics
For calcium2+
Thermo Scientific, ISE Manuals
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Potentiometric Titrations and Solubility Equilibria/Product
Berger, J. Chem. Educ., 2012, 89, 812–813
Reduction: Ag+ Ago
Oxidation: Cuo Cu2+Ag indicator electrode
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Potentiometric Titrations and Solubility Equilibria/Product
Berger, J. Chem. Educ., 2012, 89, 812–813
Reduction: Ag+ Ago
Oxidation: Cuo Cu2+Ag indicator electrode
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Potentiometric Titrations and Solubility Equilibria/Product
Berger, J. Chem. Educ., 2012, 89, 812–813
Reduction: Ag+ Ago
Oxidation: Cuo Cu2+Ag indicator electrode
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Potentiometric Titrations and Solubility Equilibria/Product
Berger, J. Chem. Educ., 2012, 89, 812–813
Reduction: Ag+ Ago
Oxidation: Cuo Cu2+Ag indicator electrode
Excess Cl–
Excess Ag+
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Potentiometric Titrations and Solubility Equilibria/Product
Berger, J. Chem. Educ., 2012, 89, 812–813
Reduction: Ag+ Ago
Oxidation: Cuo Cu2+Ag indicator electrode
Excess Cl–
Excess Ag+
1 23
(1) Ksp = (tiny) (large)(2) Ksp = (large) (tiny)(3) Ksp = (tiny) (tiny) = (tiny)2
Thus, Ksp = [Ag+]2
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DISCUSSION TIME!Pourbaix diagrams are useful for identifying which material is present/stable
from Wiki
Marcel Pourbaix(1904–1998)
http://corrosion‐doctors.org/Biographies/PourbaixBio.htm
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DISCUSSION TIME!Pourbaix diagrams are useful for identifying which material is present/stable
from Wiki
RHE
Eo(O2/H2O)
Marcel Pourbaix(1904–1998)
http://corrosion‐doctors.org/Biographies/PourbaixBio.htm
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DISCUSSION TIME!Pourbaix diagrams are useful for identifying which material is present/stable
from Wiki
RHE
Eo(O2/H2O)
(1) What is the electrocatalyst for O2 evolution through water oxidation?(2) At what pH values is an electrocatalyst for H2 evolution stable?
Marcel Pourbaix(1904–1998)
http://corrosion‐doctors.org/Biographies/PourbaixBio.htm
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DISCUSSION TIME!Pourbaix diagrams are useful for identifying which material is present/stable
from Wiki
(1) What is the electrocatalyst for O2 evolution through water oxidation? MnO2(2) At what pH values is an electrocatalyst for H2 evolution stable?
RHE
Eo(O2/H2O)
Marcel Pourbaix(1904–1998)
http://corrosion‐doctors.org/Biographies/PourbaixBio.htm
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DISCUSSION TIME!Pourbaix diagrams are useful for identifying which material is present/stable
from Wiki
(1) What is the electrocatalyst for O2 evolution through water oxidation? MnO2(2) At what pH values is an electrocatalyst for H2 evolution stable? pH > 7.5
RHE
Eo(O2/H2O)
Marcel Pourbaix(1904–1998)
http://corrosion‐doctors.org/Biographies/PourbaixBio.htm
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Week 6 Objectives
By the end of the week, you will be able to:
• Understand everything that I flew through before
• Use alpha fractions for electrochemical reactions
• Explain how ion‐selective electrodes and pH meters work
• Explain how the solubility product is pertinent to electrochemical reactions
LectureWeek6-SAA.pdfLectureWeek6-SAA.pdfBinder4.pdfUpdates for LectureWeek6.pdfLectureWeek6-SAA.pdfLectureWeek5-SAA.pdfLectureWeek5-SAA.pdfUpdates for LectureWeek5.pdfLectureWeek5-SAA.pdfLectureWeek5-SAA.pdfLectureWeek5-SAA.pdfUpdates for LectureWeek5.pdfLectureWeek5-SAA.pdfLectureWeek5-SAA.pdfUpdates for LectureWeek5.pdfLectureWeek5-SAA.pdfUpdates for LectureWeek5.pdfLectureWeeks5and6-SAA.pdfLectureWeeks5and6-SAA.pdfLectureWeeks5and6-SAA.pdfUpdates for LectureWeek5.pdf
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