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Presentation on theme: "ELECTROANALISIS (Elektrometri)"— Presentation transcript:

1 ELECTROANALISIS (Elektrometri)
Potensiometri, Amperometri and Voltametri

2 Electroanalysis Mengukur berbagai parameter listrik (potensial, arus listrik, muatan listrik, konduktivitas) dalam kaitannya dengan parameter kimia (reaksi ataupun konsentrasi dari bahan kimia) Konduktimetri, Potensiometri (pH, ISE), Koulometri, Voltametri, Amperometri

3 Potensiometri Pengukuran potensial listrik dari suatu Sel Elektrokimia untuk mendapatkan informasi mengenai bahan kimia yang ada pada sel tsb (conc., aktivitas, muatan listrik) Mengukur perbedaan potensial listrik antara 2 electroda: Elektroda Pembanding (E constant) Elektroda Kerja/Indikator(sinyal analit)

4 Elektroda Pembanding Ag/AgCl: Ag(s) | AgCl (s) | Cl-(aq) || .....

5 Elektroda Pembanding SCE: Pt(s) | Hg(l) | Hg2Cl2 (l) | KCl(aq., sat.) ||.....

6 Elektroda Pembanding Reaksi/Potensial setengah selnya diketahui
Tidak bereaksi/dipengaruhi oleh analit yang diukur Reversible dan mengikuti persamaan Nernst Potensial Konstan Dapat kembali ke potensial awal stabil Elektroda Calomel Hg in contact with Hg(I) chloride (Hg/Hg2Cl2) Ag/AgCl

7 Electroda Kerja Inert: Pt, Au, Carbon. Tidak ikut bereaksi.
Contoh: SCE || Fe3+, Fe2+(aq) | Pt(s) Elektroda Logam yang mendeteksi ion logamnya sendiri (1st Electrode) (Hg, Cu, Zn, Cd, Ag) Contoh: SCE || Ag+(aq) | Ag(s) Ag+ + e-  Ag(s) E0+= 0.799V Hg2Cl2 + 2e  2Hg(l) + 2Cl- E-= 0.241V E = log [Ag+] V

8 Electroda Kerja 1st kind Ecell=Eindicator-Ereference Metallic
1st kind, 2nd kind, 3rd kind, redox 1st kind respond directly to changing activity of electrode ion Direct equilibrium with solution

9 2nd kind 3rd kind Precipitate or stable complex of ion Ag for halides
Ag wire in AgCl saturated surface Complexes with organic ligands EDTA 3rd kind Electrode responds to different cation Competition with ligand complex

10 Metallic Redox Indictors
Inert metals Pt, Au, Pd Electron source or sink Redox of metal ion evaluated May not be reversible

11 Membrane Indicator electrodes
Non-crystalline membranes: Glass - silicate glasses for H+, Na+ Liquid - liquid ion exchanger for Ca2+ Immobilized liquid - liquid/PVC matrix for Ca2+ and NO3- Crystalline membranes: Single crystal - LaF3 for FPolycrystalline or mixed crystal - AgS for S2- and Ag+ Properties Low solubility - solids, semi-solids and polymers Some electrical conductivity - often by doping Selectivity - part of membrane binds/reacts with analyte

12 Glass Membrane Electrode

13 Ion selective electrodes (ISEs)
A difference in the activity of an ion on either side of a selective membrane results in a thermodynamic potensial difference being created across that membrane

14 ISEs

15 Combination glass pH Electrode

16 Proper pH Calibration E = constant – constant.0.0591 pH
Meter measures E vs pH – must calibrate both slope & intercept on meter with buffers Meter has two controls – calibrate & slope 1st use pH 7.00 buffer to adjust calibrate knob 2nd step is to use any other pH buffer Adjust slope/temp control to correct pH value This will pivot the calibration line around the isopotensial which is set to 7.00 in all meters Slope/temp control pivots line around isopotensial without changing it mV mV Calibrate knob raises and lowers the line without changing slope pH pH

17 Liquid Membrane Electrodes
Persamaan nikolsky untuk pengukuran sampel campuran dengan kurva kalibrasi dan standard adisi

18 Solid State Membrane Electrodes
Ag wire Solid State Membrane Chemistry Membrane Ion Determined LaF3 F-, La3+ AgCl Ag+, Cl- AgBr Ag+, Br- AgI Ag+, I- Ag2S Ag+, S2- Ag2S + CuS Cu2+ Ag2S + CdS Cd2+ Ag2S + PbS Pb2+ Filling solution with fixed [Cl-] and cation that electrode responds to Ag/AgCl Solid state membrane (must be ionic conductor)

19 Solid state electrodes

20 VOLTAMETRI Pengukuran arus sebagai fungsi perubahan potensial
POLAROGRAFI: Heyrovsky (1922): melakukan percobaan voltametri yang pertama dengan elektroda merkuri tetes (DME) Cu2+ + 2e → Cu(Hg)


22 Mengapa elektron berpindah
Reduction Oxidation EF Eredox Eredox E E EF

23 Steps in an electron transfer event
O must be successfully transported from bulk solution (mass transport) O must adsorb transiently onto electrode surface (non-faradaic) CT must occur between electrode and O (faradaic) R must desorb from electrode surface (non-faradaic) R must be transported away from electrode surface back into bulk solution (mass transport)

24 Mass Transport or Mass Transfer
Migration – movement of a muatan listrik listrik particle in a potensial field Diffusion – movement due to a concentration gradient. If electrochemical reaction depletes (or produces) some species at the electrode surface, then a concentration gradient develops and the electroactive species will tend to diffuse from the bulk solution to the electrode (or from the electrode out into the bulk solution) Convection – mass transfer due to stirring. Achieved by some form of mechanical movement of the solution or the electrode i.e., stir solution, rotate or vibrate electrode Difficult to get perfect reproducibility with stirring, better to move the electrode Convection is considerably more efficient than diffusion or migration = higher arus listriks for a given concentration = greater analytical sensitivity

25 Nernst-Planck Equation
Diffusion Migration Convection Ji(x) = flux of species i at distance x from electrode (mole/cm2 s) Di = diffusion coefficient (cm2/s) Ci(x)/x = concentration gradient at distance x from electrode (x)/x = potensial gradient at distance x from electrode (x) = velocity at which species i moves (cm/s)

26 Diffusion I = nFAJ Fick’s 1st Law
Solving Fick’s Laws for particular applications like electrochemistry involves establishing Initial Conditions and Boundary Conditions

27 Simplest Experiment Chronoamperometri

28 Simulation

29 Recall-Double layer

30 Double-Layer charging
Charging/discharging a capacitor upon application of a potensial step Itotal = Ic + IF

31 Working electrode choice
Depends upon potensial window desired Overpotensial Stability of material Conductivity contamination

32 electron transfer to the electroactive species.
The polarogram points a to b I = E/R points b to c electron transfer to the electroactive species. I(reduction) depends on the no. of molecules reduced/s: this rises as a function of E points c to d when E is sufficiently negative, every molecule that reaches the electrode surface is reduced.

33 Dropping Mercury Electrode
Renewable surface potensial window expanded for reduction (high overpotensial for proton reduction at mercury)

34 Polarography A = 4(3mt/4d)2/3 = 0.85(mt)2/3
Density of drop Mass flow rate of drop We can substitute this into Cottrell Equation i(t) = nFACD1/2/ 1/2t1/2 We also replace D by 7/3D to account for the compression of the diffusion layer by the expanding drop Giving the Ilkovich Equation: id = 708nD1/2m2/3t1/6C I has units of Amps when D is in cm2s-1,m is in g/s and t is in seconds. C is in mol/cm3 This expression gives the arus listrik at the end of the drop life. The average arus listrik is obtained by integrating the arus listrik over this time period iav = 607nD1/2m2/3t1/6C

35 Polarograms E1/2 = E0 + RT/nF log (DR/Do)1/2 (reversible couple)
Usually D’s are similar so half wave potensial is similar to formal potensial. Also potensial is independent of concentration and can therefore be used as a diagnostic of identity of analytes.



38 Other types of Polarography
Examples refer to polarography but are applicable to other votammetric methods as well all attempt to improve signal to noise usually by removing capacitive arus listriks

39 Normal Pulse Polarography

40 NPP advantage

41 Differential pulse voltametri

42 DPP vs DCP Ep ~ E1/2 (Ep= E1/2±DE/2) s = exp[(nF/RT)(DE/2)]
where DE=pulse amplitude s = exp[(nF/RT)(DE/2)] Resolution depends on DE W1/2 = 3.52RT/nF when DE0 Improved response because charging arus listrik is subtracted and adsorptive effects are discriminated against. l.o.d M

43 Resolution

44 Stripping voltametri Preconcentration technique.
1. Preconcentration or accumulation step. Here the analyte species is collected onto/into the working electrode 2. Measurement step : here a potensial waveform is applied to the electrode to remove (strip) the accumulated analyte.

45 Deposition potensial

46 ASV

47 ASV or CSV



50 Multi-Element

51 Standard Addition

52 Cyclic voltametri Cyclic voltametri is carried out at a stationary electrode. This normally involves the use of an inert disc electrode made from platinum, gold or glassy carbon. Nickel has also been used. The potensial is continuously changed as a linear function of time. The rate of change of potensial with time is referred to as the scan rate (v). Compared to a RDE the scan rates in cyclic voltametri are usually much higher, typically 50 mV s-1

53 Cyclic voltametri Cyclic voltametri, in which the direction of the potensial is reversed at the end of the first scan. Thus, the waveform is usually of the form of an isosceles triangle. The advantage using a stationary electrode is that the product of the electron transfer reaction that occurred in the forward scan can be probed again in the reverse scan. CV is a powerful tool for the determination of formal redox potensials, detection of chemical reactions that precede or follow the electrochemical reaction and evaluation of electron transfer kinetics.

54 Cyclic voltametri

55 Cyclic voltametri For a reversible process Epc – Epa = 0.059V/n

56 The Randles-Sevcik equation Reversible systems

57 The Randles-Sevcik equation Reversible systems
n = the number of electrons in the redox reaction v = the scan rate in V s-1 F = the Faraday’s constant 96,485 coulombs mole-1 A = the electrode area cm2 R = the gas constant J mole-1 K-1 T = the temperature K D = the analyte diffusion coefficient cm2 s-1

58 The Randles-Sevcik equation Reversible systems
As expected a plot of peak height vs the square root of the scan rate produces a linear plot, in which the diffusion coefficient can be obtained from the slope of the plot.

59 Cyclic voltametri

60 Cyclic voltametri

61 Cyclic voltametri

62 Cyclic voltametri – Stationary Electrode
Peak positions are related to formal potensial of redox process E0 = (Epa + Epc ) /2 Separation of peaks for a reversible couple is 0.059/n volts A one electron fast electron transfer reaction thus gives 59mV separation Peak potensials are then independent of scan rate Half-peak potensial Ep/2 = E1/2  0.028/n Sign is + for a reduction

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