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Summary of Potentiometry : pH and Ion Selective Electrodes Potentiometric Sensors

Summary of Potentiometry : pH and Ion Selective Electrodes Potentiometric Sensors I = controlled at 0 Amps E eq is measured In general E eq = const – 0.0592 log a X. Electrode Potentials (review). Electrochemical cell – two half cells Convention, write both as reductions

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Summary of Potentiometry : pH and Ion Selective Electrodes Potentiometric Sensors

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  1. Summary of Potentiometry: pH and Ion Selective Electrodes Potentiometric Sensors I = controlled at 0 Amps Eeq is measured In general Eeq = const – 0.0592 log aX

  2. Electrode Potentials (review) • Electrochemical cell – two half cells • Convention, write both as reductions • 2 AgCl (s) + 2 e-= 2 Ag (s) + 2 Cl-(cathode) • - [2 H+ + 2 e- =H2 (gas)] (Pt, NHE reference, anode) • Ecell = Ecathode-Eanode Cell reaction is the sum of the two above 2 AgCl (s) + H2 =2 Ag (s) + 2 Cl- + 2 H+ Ecell= EAg/AgCl – EH+/H2by convention EH+/H2 = 0 Ecell= EAg/AgCl = 0.46 V DG = - n F Ecell ; DG = positive, non-spontaneous, electrolytic cell

  3. Measurements in Potentiometry; I = 0 Amps; equilibrium Cell: working electrode + reference electrode (E half cell = const) Working or indicator Ecell= EWE – Eref - Ejunction

  4. Simple potentiometric measuring circuit Variable resistor V voltmeter galvanometer Move slidewire (arrow) until G shows I = 0, then V = Ecell= Eeq In practice this is all automatic in modern potentiometers or pH meters

  5. Reference electrodes: critical to both potentiometry and voltammetry They keep a nearly constant half cell potential during experiment Normal Hydrogen, Pt| H2 (1 atm), HCL (0.01 M), NHE THE STANDARD, E = 0 V, but not practical Standard Calomel Electrode Hg| Hg2Cl2 (s), KCl (sat’d.) SCE Set up as self-contained Half cell Contact to test solution

  6. Half cell potential of the SCE – serves as a reference against which other E’s are measured Hg2Cl2 (s) + 2 e-= 2 Hg (l) + 2 Cl- Use Nernst equation: E = Eo - [RT/nF] ln (aCl2aHg2/acalomel) ; but a of pure solids =1 only aClremains in the log term, and E = Eo’- [0.0592/2] log [Cl-]2 or E = Eo’- 0.0592 log [Cl-] ;sat’d KCl is ~3.5 M at 25 oC So ESCE = 0.244 V vs. NHE at 25 oC Alternative reference: Ag|AgCl (s), KCl (sat’d.) EAg/AgCl = 0.199 V vs. NHE at 25 oC

  7. Half cell potential of the SCE – serves as a reference against which other E’s are measured Hg2Cl2 (s) + 2 e-= 2 Hg (l) + 2 Cl- Use Nernst equation: E = Eo - [RT/nF] ln (aCl2aHg2/acalomel) ; but a of pure solids =1 only aClremains in the log term, and E = Eo’- [0.0592/2] log [Cl-]2 or E = Eo’- 0.0592 log [Cl-] ;sat’d KCl is ~3.5 M at 25 oC So ESCE = 0.2415 V vs. NHE Alternative reference: Ag|AgCl (s), KCl (sat’d.) EAg/AgCl = 0.2415 V vs. NHE

  8. Ion Selective Electrodes (ISE) - sensor surface usually a membrane That adsorbs the ions, Eeq measured at I = 0 Amps In pH electrode, the membrane is a very thin glass layer 0.1 M HCl Stand alone glass pH electrode must be used with reference Glass pH electrode combined with internal reference electrode Glass membranes are made of SiO2, Li2O (or Na2O) and BaO (or CaO)

  9. ISE’s obey Nernst-like equations (25 oC) E = const + [0.0592/z] log aionISE measure activity, not conc. if the ion Is H+, E = const - 0.0592 pH; pH = -log aH+ Fast response is important, < 1 sin buffer for most pH electrodes ISE Nernstian region, slope = 0.0591/z E, mV Most pH meters read pH directly, But must be calibrated daily Log aion

  10. How a glass pH electrode responds to H+ ions (must store in in water or buffer to maintain hydrated layer) Ag/AgCl 0.1 N HCl aH+ = const Inner hydrated layer outer hydrated layer Dry glass Test solution aH+ , soln a1 a2 0.1 mm 50 mm E2 E1 EM = E1 – E2 + Eint ref; or EB = E1 – E2 (boundary E) Ecell = const + EB Li+ in glass can exchange with H+ (both small ions), giving rise to E1 and E2 H+ DOES NOT cross the membrane

  11. EB is related to a1 and a2,but a2 is constant (0.1 M HCl) These ion activities control the membrane potentials, E1 and E2 and so control EB, at 25 oC EB = E1 – E2 = 0.0592 log (a1/a2) Ecell = const + 0.0592 log (a1) Ecell = const - 0.0592 pH In practice, pH meter incorporates these equations And relates them to measurements with standard buffer, And the output is a direct measurement of pH: pH = pHstd + F (Ecell- Estd)/2.303 RT, R = gas const, T = abs. temperature

  12. Errors and Interferences in pH electrode measurements Alkaline error: In basic solutions or high salt conc. NaCl, KCl, Na+ and K+ interfere by adsorbing to the glass membrane then pHobs < true pH e.g. 0.1 M NaOH, pH 13, [Na+] is 0.1 M, [H+]= 1 x 10-13 Large error due to high [Na+], low [H+] In general fprISEs, Nicolsky equation Ecell = const + 0.0592 log [a1 + ΣKjaj], j = 1….n interfering ions Kj = selectivity coefficient Acid error pH < 1, origin unknown pH electrodes reliable between pH 1 and 13 only

  13. ISE’s for ions other than H+ • glass membranes, Na+, K+, NH4+ - different composition than pH • solid state membranes, F-, S- • liquid membranes, Ca+ • gas sensitive electrodes CO2, H2S, NH3 • enzyme electrodes – biological molecules • can all be used with pH meter in mV-mode

  14. Fluoride ISE – Solid State FLUORIDE ISE Detection limit 10-9 M

  15. Impregnated with ion exchanger; Ca++ ISE, Ca(dodecylphosphate) + Polymer like PVC; Phosphate groups bind Ca++ Crystals or solid state have the analyte Ion present, e.g. LaF3 Detection limit ~10-8 to 10-6 M

  16. Urea Enzyme ISE (NH)2CO + 2 H2O + H+ Urease enzyme 2 NH4+ + HCO3- Detection limit ~10-6 M

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