Chapter 7 Electrochemistry § 7.5 Theories for strong electrolyte + + + + + + + + + + + + +
Chapter 7 Electrochemistry
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Transcript of Chapter 7 Electrochemistry
![Page 1: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/1.jpg)
Chapter 7 Electrochemistry
§7.9 Electrode potential and electromotive forces
H2O
O2
H2
pH
/
V
2 4 6 8 10 12 14
0.401
-0.828
0.000
1.229
0
![Page 2: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/2.jpg)
1) emf’s and rGm of a reaction in different forms
reaction:
H2 + Cu2+ Cu + 2H+ G1, E1
1/2 H2 + 1/2 Cu2+ 1/2 Cu + H+ G2, E2
Cu + 2H+ H2 + Cu2+ G3, E3
7.9.1. Influential factors for electrode potential
Exercise: Compare G1, G2, G3 and E1, E2, E3.
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2) between different oxidation states
Fe3+ Fe2+ Fe1y
2y
3y
Give the relationship between
Exercise
Initial state and final state
![Page 4: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/4.jpg)
AgCl = Ag+ + Cl-
Ag(s)|AgNO3(c1) ||KCl(c2) |AgCl(s)|Ag(s)
3) of relevant electrodes + AgCl/AgAg /Ag y y
+AgCl/Ag Ag /AgE y y y
splnRT
E KnF
y y
+AgCl/Ag spAg /Agln
RTK
nF y y y
-2Ag(CN) /Ag
y+Ag /Ag
y
Exercise:
deduce the relationship between
and
![Page 5: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/5.jpg)
7.9.2. Concentration-dependence of
Nernst equation ox
red
lnaRT
nF a y
for Ag+/Ag electrode
+ + +Ag /Ag Ag /Ag Ag Ag /Ag Ag
0.05916ln ln
RTa a
nF n y y
(Ag+/Ag) depends on [Ag+] , or (Ag+/Ag) responds to [Ag+].
The relationship between (Ag+/Ag) and [Ag+] can be used
for quantitative electroanalysis of Ag+.
![Page 6: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/6.jpg)
Can we use hydrogen
electrode for measuring the
pH of the solution?
Give the principle of the
measurement.
Exercise:
why electrode Hg(l)Hg2SO4(s)CaSO4(s)Ca2+(m) can be used to measure the concentration of Ca2+ in a solution?
Normal and italic
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7.9.3. pH-dependence of : Pourbaix diagram
For electrode reaction with H+ or OH- participating in, the electrode potential will depend on pH.
O2 + 4H+ + 4e- 2H2O
= ⊖ + 0.05916 lgaH+
= 1.229 - 0.05916 pH
= ⊖ + 0.05916 lgaH+
= 0.000 - 0.05916 pH
2H+ + 2e- H2
pH-potential diagram/Pourbaix diagram
H2O
O2
H2
pH
/ V
2 4 6 8 10 12 14
0.401
-0.828
0.000
1.229
0
![Page 8: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/8.jpg)
Application of Pourbaix diagram
Cu2+ Cu(OH)2
Cu
pH
/ V
2 4 6 8 10 12 140
CuO22
Cu2O
![Page 9: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/9.jpg)
Pourbaix diagram of iron-water system
Equilibrium line
Stable zone
Fe2+
Fe2O3
Fe
pH
/ V
2 4 6 8 10 12 140
Fe3O4
Fe3+
FeO22
Stable state
Reaction
Product
Protection, passivation,
active dissolution,
electroplating,
electrosynthesis
![Page 10: Chapter 7 Electrochemistry](https://reader036.fdocuments.in/reader036/viewer/2022062408/56813868550346895da01795/html5/thumbnails/10.jpg)
Group discussion -2
1) How can you measure the liquid-liquid junction potential of a HCl/KCl interface? Write out the notation of the cell you use to conduct your measurement.
2) A potential is usually established across the cell membrane due to the concentration difference of K+ inside and outside a cell, which is named as membrane potential. This potential is crucial for sensation of any living thing. Can you design an experimental apparatus for measuring the membrane potential of a cell? State the principle you use.