electroanalysis measure the variation of an electrical parameter (potential, current, charge,...
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Electroanalysis
measure the variation of an electrical parameter (potential, current, charge, conductivity) and relate this to a chemical parameter (the analyte concentration)
Selectivity: by choice of operating parameters (potential, current etc…) and/or the electrode material
applications– environmental analyses– quality control– biomedical analyses etc
Electrochemical Cells
galvanic:spontaneous chemical reactions to produce
electrical energy (ΔG = -nFE, negative)
• applications: batteries, potentiometry (pH, ISE)
electrolytic:utilisation of energy (ex: applied V) to force a chemical rxn
to take place (ΔG +)
• applications: coulometry, voltammetry
Galvanic Cells- +
CathodeAnode
Cd(s) --> Cd 2+(aq) +2e -
Cd
e-
AgSalt bridge
Cl - K+
Cd2+
AgNO3(aq)
NO3-
V
CdCl2
2Ag +(aq) + 2e - -->2Ag(s)
line notation (shorthand)| interface between two phases. || salt bridge
Cd(s) | CdCl2(aq, M) || AgNO3(aq, M) | Ag(s)
Half-Reactions
(aq)Cd+2Ag(s)Cd(s)+(aq)2Ag :net
_____________________________
2e+(aq)Cd(s) Cd :
2Ag(s)2e+(aq)2Ag :
+2+
-+2
-+
anode
cathode
Ecell= Ecathode (+) - Eanode(-)
Standard Potentials
To predict the reactivity of oxidants or reductants we need to measure the potential of each half-reaction.impossible!!....for every oxidation we have a reduction reaction
• Define a standard half-cell of potential = 0V against which all other half-cell reduction potentials are measured (with the std half-cell attached to the negative terminal of the potentiometer). Each component in these standard cells having unit activity (pressure, conc.)
Standard Hydrogen Electrode
- +e-
AgSalt bridge
AAg+=1
V=+0.799V
AH+=1
AH2=1
Pt(s) | H2(g, A=1) | H+(aq, A=1) || Ag+(ag, A=1) |_________________________|
NHEH+(aq, A=1) + e- 1/2H2(g, A=1) E0=0 V
Electrochemical Series
Reduction half-reactions oxidant reducing agent E0 (V)
stronger oxidant F2(g) + 2e- 2F- 2.890 Ce4+ + e- Ce3+ 1.720 Ag+ + e- Ag(s) 0.799 Fe3+ + e- Fe2+ 0.771 O2 + 2H+ + 2e- H2O2 0.695 Cu2+ + 2e- Cu(s) 0.339 2H+ + 2e- H2(g) 0.000 Cd2+ + 2e- Cd(s) -0.402 Zn2+ + 2e- Zn(s) -0.762 K+ + e- K(s) -2.936 Li+ +e- Li(s) -3.040 stronger reducer
Nernst Equationfor a half-rxn
aOx + ne- bRed
R= gas constant T= temperature in Kelvinn= no. of electrons in half-rxnF= Faraday constant (96485 C/mol)A= activity (= 1 for a pure solid, liquid or solvent and expressed in mol/L for solutes and in bar for gases)
)ln( Re0
a
b
Ox
d
A
A
nF
RTEE
Nernst Equation
Converting ln to log10 (x 2,303) and at 25oC (298.15K)
)log(0592.0 Re0
a
b
Ox
d
A
A
nEE
Potentiometry
the measure of the cell potential to yield chemical information (conc., activity, charge)
Measure difference in potential between two electrodes:
reference electrode (E constant)indicator electrode (signal α analyte)
Reference electrodes
Ag/AgCl:Ag(s) | AgCl (s) | Cl-(aq) || .....
- +
Ag/AgClSalt bridge
KCl
Pt
Fe2+, Fe3+
- +
Ag
Soln. aq. satdin KCl + AgCl
Pt
Fe2+, Fe3+AgCl + KCl
AgCl
Porous glass
AgCl(s) + e - <=> Ag(s) + Cl -
E0=0.222V
Fe3+ + e - <=> Fe2+
E0=0.771VE(KCl sat.)=0.197V
Reference Electrodes
SCE:
Pt(s) | Hg(l) | Hg2Cl2 (l) | KCl(aq., sat.) ||.....
Hg(l)
Soln. sat. in KCl
Pt
KCl
Hg, Hg2Cl2 et KCl
Porous glass
E0=0.268V
E(KCl sat.)=0.241VGlass wool
Hg2Cl2 + 2e - <=> 2Hg(l) + 2Cl -
Indicator Electrodes
• Inert:Pt, Au, Carbon. Don’t participate in the reaction.
example: SCE || Fe3+, Fe2+(aq) | Pt(s)
• Certain metallic electrodes: detect their ions(Hg, Cu, Zn, Cd, Ag)example SCE || Ag+(aq) | Ag(s)Ag+ + e- Ag(s) E0
+= 0.799VHg2Cl2 + 2e- 2Hg(l) + 2Cl- E0
-= 0.241V
E = 0.799 + 0.05916 log [Ag+] - 0.241 V
Ion selective electrodes (ISEs)
A difference in the activity of an ion on either side of a selective membrane results in a thermodynamic potential difference being
created across that membrane
C a 2 + C a 2 + 0 . 0 1 M C a 2 +
0 . 0 2 M C l -
0 . 1 M C a 2 +
0 . 2 M C l -
( 0 . 1 + ) M C a 2 + ( 0 . 1 - ) M C a 2 +
0 . 0 2 M C l - 0 . 2 M C l -
+
+
+
+
-
-
-
-
Calcium selective molecular recognition ligand
Combination glass pH Electrode
Ag
Soln. aq. satdin KCl + AgCl
AgCl(s) + KCl(s)
AgCl porousglass
+ -
0.1M HCl inAgCl sat.
Combination glass pH Electrode
int ref
int+H
analyte
ext ref
Ag(s)|AgCl(s)|(aq)-Clint),(aq,Hext)(aq,H||(aq)-Cl|AgCl(s)|Ag(s)
β~ 1, constant = asymmetric potential (2 sides are not identical)
)log()0592.0(constantint
H
H
A
AE ext
Other ISEs
• by changing the composition of the glass, ISE selective for different ions can be fabricated
• By replacing the glass with a perm-selective barrier incorporating a selective binding agent (ion-exchanger, host, doped crystal) ISEs for different ions can be fabricated
Voltammetry
The measurement of variations in current produced by variations of the potential applied to a working electrode
polarography:• Heyrovsky (1922): first voltammetry experiments using a
dropping mercury working electrode
In voltammetry, once the applied potential is sufficiently negative, electron transfer occurs between the electrode and the electroactive species: Cu2+ + 2e → Cu(Hg)
• Hg liquid metal (surface can be renewed)
The polarogrampoints a to b
I = E/Rpoints b to c
electron transfer to the electroactive species.
I(reduction) depends on the no. of moecules
reduced/s: this rises as a function of Epoints c to d
when E is sufficiently negative, every molecule that reaches the electrode
surface is reduced.
Reactions that can be studied using voltammetry
amalgam-forming metallics;reducible metallic ions e.g. Fe(III) → Fe(II);reducible anions e.g. chromate, iodate...reduction of molecular oxidants e.g. NO2, O2, H2O2...reduction of organics, e.g. ketones, quinones, aldehydes, peroxides...
Glucose Monitoring and Diabetes
Diabetes is a serious disease, and, with its complications, is the fourth leading cause of death by disease in the
United States. Its causes are unknown, and there is no cure.
Testing: A Crucial ToolBlood tests, done by pricking the finger for a drop of blood, are recommended by most doctors because they give the
exact amount of blood sugar at any given moment.There are an estimated 14 million diabetics in the U.S.
It is recommended to test blood glucose levels at least 4 times daily.
Market of 56 millions disposable tests per day!!
Voltammetric Blood Glucose Monitors
An example of a test is the use of the immobilised enzyme glucose oxidase, which releases electrons on interaction with glucose. A sensor of this type could detect the level of glucose in the blood.
E le c tro ns
R ed u ced M ed ia to rO x id is ed M ed ia to r
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