M. Revenco et al./Chem.J. Mold. 2008, 3 (1), 44-47Preparation <strong>of</strong> the electrodesThe PVC membrane electrodes were prepared using a procedure similar to those described in [10].The mixture <strong>of</strong> PVC cocktail, prepared by dissolving 0,02 – 0,03 g ionophore, 0,3 g PVC, 0,3 g DOP, and 0,9 gnitrobenzene in 3 –5 ml <strong>of</strong> tetrahydr<strong>of</strong>uran (THF), was poured onto a glass dish (ca. 5 cm diameter) and allowed to dryat room temperature. A membrane (ca.16 mm diameter) was cut and glued to the polished end <strong>of</strong> a PVC tube by usinga PVC (ca. 5 %) – THF solution. According to the number <strong>of</strong> complexes used for preparation <strong>of</strong> the membrane the ionselective electrodes (ISE) are noted as (ISE1, ISE2 and ISE3). The Ag/AgCl electrode and 10 -1 M <strong>of</strong> NO 3-+ 5 . 10 -3 M <strong>of</strong>KCl solution were used as reference electrode and the internal filing solution, respectively.The assembled electrodes were conditioned by soaking into solution <strong>of</strong> sodium nitrate (10 -1 M) for 12 h beforethe electrodes have been used.Measurement <strong>of</strong> electromotive forceA nitrate-selective PVC electrode and saturated Ag/AgCl electrode were used as the indicating and the referenceelectrode, respectively. All potential measurements were performed at an ambient temperature (25 ± 1 0 C) using agalvanic cell <strong>of</strong> the following type:Ag/AgCl, KCl (5 . 10 -3 M) | internal filing solution (10 -1 M NO 3-) | PVC membrane || tested solution || KCl satd.AgCl/Ag.The behavior <strong>of</strong> each electrode was investigated in the concentration range <strong>of</strong> 1 . 10 -7 – 1 . 10 -1 M at a constant pH.-The data were plotted as the observed potential against the negative logarithm <strong>of</strong> the NO 3activity. The potentiometriccoefficients (KNO 3-/X - ) were determined according to the fixed interference method.Results and discussionInfl uence <strong>of</strong> the nature <strong>of</strong> the ligand in the apical position <strong>of</strong> the trinuclear cromium(III) pivalates on the sensorsparametersThe potentiometric response <strong>of</strong> the ISE1 was linear Nernstian in the concentration range 8 . 10 -5 – 1 . 10 -1 M witha slope 50 mV/decade. The detection limit was 3,2 . 10 -5 mol/l and the electrode lifetime – only one day. We explain thisshort lifetime, by the possible hydrolysis <strong>of</strong> the complex and loss <strong>of</strong> the charge by the complex species according to thescheme:[Cr 3O(C 5H 9O 2) 6(H 2O) 3] + + H 2O [Cr 3O(C 5H 9O 2) 6(H 2O) 2(OH)] + H 3O + .The substitution <strong>of</strong> the co-ordinated water by quinoline in ISE2 gives rise to an increase <strong>of</strong> the lipophilicproperties <strong>of</strong> the complex, extending his lifetime up to 7 day and diminishing the detection limit up to 2 . 10 -5 M, similarto the behavior <strong>of</strong> the electrodes described in [7, 8].Fig. 1. Calibration curve <strong>of</strong> ISE3Although the substitution <strong>of</strong> the water molecules by quinoline improves the parameters <strong>of</strong> the sensor, the lifetimeis short enough. A possible washing-out <strong>of</strong> the electroactive material could be the cause <strong>of</strong> this relatively short lifetime.To stabilize the ionophore in membrane, we have tried the polymerisation <strong>of</strong> the trinuclear cores using bridging ligands.45
M. Revenco et al./Chem.J. Mold. 2008, 3 (1), 44-47The 4,4’-bipiridil was suitable for this purpose. The interaction <strong>of</strong> pivalate I with 4,4’-bipyridil in stoechiometric ration2:3, leads to formation <strong>of</strong> a product III, which one is poorly soluble both in water and in the used for preparation themembrane solvents. Use <strong>of</strong> a saturate in nitrobenzene solution and incorporated in membrane, does not give rise to anitrates sensitive electrode. This behavior demonstrates the formation <strong>of</strong> a polymer with very low solubility, whichcannot assure a sufficient concentration to prepare a PVC membrane.To achieve the objective we have tried the synthesis <strong>of</strong> the active material in situ [8], directly in membraneduring its formation. The complex I, 4,4’-bipiridil and the other components used for preparation <strong>of</strong> the membrane <strong>of</strong>ISEI, all together, were mixed stirred and left for evaporation. During this time part <strong>of</strong> water molecules was substitutedby 4,4’- bipyridil, and a new polymeric structure has appeared and plays the role <strong>of</strong> ionophore. We suppose, that thepresence <strong>of</strong> the PVC does not allow the formation <strong>of</strong> the crystalline polymer, but it ensures the lacing <strong>of</strong> a number <strong>of</strong>trinuclear unities encapsulated by the solvent containing nitrate as counter ion.Washing-out <strong>of</strong> this compound from membrane is surely hindered. The potentiometric response <strong>of</strong> ISE3,containing the ionophore synthesized in situ, was linear with a Nernstian slope <strong>of</strong> 56 mV/decade within the NO 3-concentration range 2 . 10 -5 -1 . 10 -1 mol/l. Detection limit is 3,2 . 10 -6 mol/l (Fig. 1).The reponse time <strong>of</strong> the electrode was 15 s over the entire linear concentration range <strong>of</strong> the calibration plot.In order to study the effect <strong>of</strong> pH on the performance <strong>of</strong> ISE3, the responses <strong>of</strong> the sensor to NO 3-ion at differentconcentrations <strong>of</strong> H + ion were measured. It was observed that the sensor exhibite a stable behavior with a constantpotential in the pH range 2 –11. The Fig. 2 shows the variation <strong>of</strong> the potential <strong>of</strong> the sensors immersed in a solutionwith the concentration 0,001 M. To achieve stable parameters the preconditioning time must be close to 12 h in a 0,1mol/l solution <strong>of</strong> NaNO 3. The drift <strong>of</strong> the potential for a constant concentration is negligible. The electrodes preparedby this method show stable parameters during 4 months. During this period, the electrode was kept in a 0,1 mol/l NaNO 3solution and calibrated periodically. No significant change in the performance <strong>of</strong> the electrode was observed.320E, mV3002802600 1 2 3 4 5 6 7 8 9 10 11 12 13 14Fig. 2. Influience <strong>of</strong> pH on the response <strong>of</strong> the ISE3 immersed in a solution <strong>of</strong> NaNO 3(0,001 M)The performances <strong>of</strong> a selection <strong>of</strong> different electrodes published in literature are shown in the Table 1. As it canbe observed the parameters <strong>of</strong> the proposed electrode are comparable with <strong>of</strong> available nitrate-selective electrodes.Table 1Parameters <strong>of</strong> a selectoion <strong>of</strong> nitrate-selective electrodesConcentration range, mol/l Slope, mV/decade Detection limit, mol/l pH range Lifetime Reference1 . 10 -1 – 1 . 10 -6 3,4 . 10 -7 2 - 8 [1]1 . 10 -1 – 2 . 10 -5 58 5 - 11 [2]60 4,2 . 10 -6 1 year [3]54-55 5,0 . 10 -5 [4]1 . 10 -1 – 1 . 10 -5 54,7 2,3 . 10 -6 2 - 12 [5]1 . 10 -1 – 2 . 10 -5 56 3,2 . 10 -6 2 -11 4 months ISE3Selectivity <strong>of</strong> the electrode ISE3The potentiometric selectivity coefficients were determined by fixed interference method [10]. The potentiometricselectivity coefficients <strong>of</strong> the proposed electrode are summarized in table 2.Table 2Selectivity coefficients (-lgKNO 3-/X - ) <strong>of</strong> ISE3 determined using fixed interference methodX ClO 4-I - SCN - Br - BF 4-Cl - CH 3COO - SO 42-F --lgK NO3,X0,83 1,05 1,14 1,38 1,83 3,71 3,83 4,17 4,65pH46
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