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Electroanalytical chemistry

Electroanalytical chemistry. Potentiometry, Voltammetry and Polarography. Electroanalysis. measure the variation of an electrical parameter (potential, current, charge, conductivity) and relate this to a chemical parameter (the analyte concentration)

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Electroanalytical chemistry

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  1. Electroanalytical chemistry Potentiometry, Voltammetry and Polarography

  2. Electroanalysis • measure the variation of an electrical parameter (potential, current, charge, conductivity) and relate this to a chemical parameter (the analyte concentration) • Conductimetry, potentiometry (pH, ISE), coulometry, voltammetry

  3. 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)

  4. Reference electrodes Ag/AgCl: Ag(s) | AgCl (s) | Cl-(aq) || .....

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

  6. 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+= 0.799V Hg2Cl2 + 2e  2Hg(l) + 2Cl- E-= 0.241V E = 0.799 + 0.05916 log [Ag+] - 0.241 V

  7. 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

  8. ISEs

  9. Combination glass pH Electrode

  10. 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 isopotential which is set to 7.00 in all meters Slope/temp control pivots line around isopotential without changing it mV mV Calibrate knob raises and lowers the line without changing slope 4 7 4 7 pH pH

  11. Liquid Membrane Electrodes

  12. Solid State Membrane Electrodes Ag wire Filling solution with fixed [Cl-] and cation that electrode responds to Ag/AgCl Solid state membrane (must be ionic conductor)

  13. Solid state electrodes

  14. 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)

  15. EF Eredox Why Electrons Transfer Reduction Oxidation Eredox E E EF • Net flow of electrons from M to solute • Ef more negative than Eredox • more cathodic • more reducing • Net flow of electrons from solute to M • Ef more positive than Eredox • more anodic • more oxidizing

  16. 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)

  17. Mass Transport or Mass Transfer • Migration – movement of a charged particle in a potential 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 currents for a given concentration = greater analytical sensitivity

  18. Diffusion Migration Convection Nernst-Planck Equation 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 = potential gradient at distance x from electrode (x) = velocity at which species i moves (cm/s)

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

  20. Simplest ExperimentChronoamperometry

  21. Simulation

  22. Recall-Double layer

  23. Double-Layer charging • Charging/discharging a capacitor upon application of a potential step Itotal = Ic + IF

  24. Working electrode choice • Depends upon potential window desired • Overpotential • Stability of material • Conductivity • contamination

  25. 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.

  26. Dropping Mercury Electrode • Renewable surface • Potential window expanded for reduction (high overpotential for proton reduction at mercury)

  27. 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 current at the end of the drop life. The average current is obtained by integrating the current over this time period iav = 607nD1/2m2/3t1/6C

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

  29. 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 currents

  30. Normal Pulse Polarography • current measured at a single instant in the lifetime of each drop. • higher signal because there is more electroactive species around each drop of mercury. • somewhat more sensitive than DC polarography. • data obtained have the same shape as a regular DCP.

  31. NPP advantage • IL = nFAD1/2c/(ptm)1/2 • (tm = current sampling t) • IL,N.P./IL,D.C. = (3t/7tm)1/2 • Predicts that N.P.P. 5-10 X sensitive than D.C.P.

  32. Differential pulse voltammetry

  33. DPP • current measured twice during the lifetime of each drop difference in current is plotted. • Results in a peak-shaped feature, where the top of the peak corresponds to E1/2, and the height gives concentration • This shape is the derivative of the regular DC data. • DPP has the advantage of sensitive detection limits and discrimination against background currents. Traditionally, metals in the ppm range can be determined with DPP. • Derivative improves contrast (resolution) between overlapping waves

  34. DPP vs DCP Ep ~ E1/2 (Ep= E1/2±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 current is subtracted and adsorptive effects are discriminated against. l.o.d. 10-8M

  35. Resolution

  36. Square wave voltammetry

  37. SWV

  38. SWV Response

  39. SWV • advantage of square wave voltammetry is that the entire scan can be performed on a single mercury drop in about 10 seconds, as opposed to about 5 minutes for the techniques described previously. SWV saves time, reduces the amount of mercury used per scan by a factor of 100. If used with a pre-reduction step, detection limits of 1-10 ppb can be achieved, which rivals graphite furnace AA in sensitivity. • data for SWV similar to DPP • height and width of the wave depends on the exact combination of experimental parameters (i.e. scan rate and pulse height

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

  41. Deposition potential

  42. ASV

  43. ASV or CSV

  44. Adsorptive Stripping Voltammetry • Use a chelating ligand that adsorbs to the WE. • Can detect by redox process of metal or ligand.

  45. Multi-Element

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