Next Article in Journal / Special Issue
Ion Selective PVC Membrane Electrode for the Determination of Methacycline Hydrochloride in Pharmaceutical Formulation
Previous Article in Journal / Special Issue
Calixarene-Based Molecules for Cation Recognition
Article Menu

Export Article

Sensors 2002, 2(10), 417-423; doi:10.3390/s21000417

Article
Sensor for Silver(I) Ion Based on Schiff-base-p-tertbutylcalix[4]arene
Department of chemistry, Guru Nanak Dev University, Amritsar 143005, India
*
Author to whom correspondence should be addressed.
Received: 16 September 2002 / Accepted: 1 October 2002 / Published: 18 October 2002

Abstract

:
The preparation of polymer membrane selective to silver ion and its application to ion-selective electrode is reported here. PVC membrane contain silver-selective calix[4]arene derivative as ionophore. The membrane electrode is highly selective to silver ion and exhibit good linear response over a wide concentration range of 1.0×10-1 to 1.0×10-5M AgNO3 with Nernstian slope of 58.9 mV per decade. The detection limit of electrode is 6.31×10-6 M .The calix[4]arene based membrane electrode exhibit enhanced selectivities for silver ion over other cations; log KPotAg,Na = -2.35, log KPotAg,K = -2.65, log KPotAg,Mg = -4.57, log KPotAg,Ba = -4.10, log KPotAg,Cd = -3.42, log KPotAg,Pb = -3.45. Even the strongest interferent Hg2+ do not interfere to great extent, log KPotAg,Hg = -2.0. The electrode response is stable over wide pH range of 1.0-6.0. The response time of the sensor is 30 seconds and the membrane can be used for more than 6 months without observing any divergence. The sensor can also be applied as an indicator electrode for potentiometric titration of Ag+ ions with Cl-. It is possible to determine Ag(I) in the natural water spiked with silver with this electrode assembly.
Keywords:
Sensor; Silver(I); Potentiometry

Introduction

Amongst the various analytical techniques available, the use of ion-selective membrane electrodes is well establish routine analytical technique. Good ion-selective electrodes(ISEs) possess many advantages over the traditional methods of analysis as they provide accurate, reproducible, fast and often selective determination of various ionic species. Not only this, the ion-selective electrodes(ISEs) allow non-destructive, on line monitoring of particular ion in small volume of sample without any pretreatment. Because of these merits, the use of ISEs is increasing day by day in medicinal, enviornmental, agricultural and industrial field. During last three decades, a number of ion-selective electrodes with polymeric membranes have been reported[1,2,3,4,5,6,7,8,9,10]. Among the various ligands available for ion-selective electrodes such as crowns, podands, cryptands and spherands, the calixarenes met many of the requirements that an ionophore should satisfy for the use in ion-selective electrodes[11]. A number of calixarene derivatives containing pendant ether, amide, ketonic and ester groups have been incorporated as neutral carriers into ion-selective electrodes sensitive to sodium, potassium and cesium ions[12,13,14,15]. Recently,we reported silver(I) and cesium ion-selective PVC membrane electrode based on bis(pyridine tetramide) macrocycle and calix crown ether ester,respectively[2,3,10].The present paper deals with Schiff-base-p-tert-butylcalix[4]arene derivative [I] based ISE for selective determination of silver. The silver ion selectivity may be due to electrostatic interaction between the metal ion and aza crown cavity composed of four highly preorganized soft binding units (imine units).
The silver(I) ion selective electrode exhibit a good response for silver ion over wide concentration range of 1.0×10-5-1.0×10-1M with a Nernstian slope of 58.9mV per decade. The proposed ion selective electrode incorporates PVC as supporting material to give a pseudo-solid sensing membrane and bis(2-ethylhexyl)sebacate as plasticizing agent. The performance of this electrode which involves linear range, detection limit, response time, slope etc is in agreement and in many respects better than those reported in literature [8,9].

Experimental

Reagents

Schiff-base–p-tert butylcalix[4]arene derivative was prepared as reported earliar[2]. High molecular weight poly(vinylchloride) PVC and bis(2-ethylhexyl)sebacate were obtained from Fluka. All other reagents used were of Analytical - Reagent grade.
Sensors 02 00417 i001

Electrode Preparation

The PVC based ion selective electrode membrane is prepared by dissolving 100.0mg of PVC, 211.0mg of bis(2- ethylhexyl) sebacate as plasticizer and 5.6mg of calix[4]arene as ionophore in 5 ml tetrahydrofuran(THF). The mixture so obtained was shaken vigorously and poured into 50 mm petridish after removing air bubbles. The solvent was allowed to evaporate at room temperature and the resulting membrane was cut to size, attached to pyrex tube with PVC glue and conditioned with AgNO3 solution of 1.0×10-1M for two days.

Potentiometric measurements

The potentiometric measurements were carried at room temperature with the following cell set up:
Ag/AgCl / 1.0×10-1 M AgNO3 / PVC membrane / test solution / Ag/AgCl
All the measurements were made with Elico LI Model-120 pH meter. Standard AgNO3 solutions for calibration were obtained by gradual dilution of 0.1M AgNO3 solution.

Results and Discussion

Schiff-base-p-tert-butylcalix[4]arene derivative[I] was employed as silver selective ionophore in the preparation of silver ion- selective electrode. The potentiometric response of the electrode is shown in Fig 1. The measurements were performed in the concentration range of 1.0×10-8-1.0×10-1M AgNO3. The electrode shows linear response in the concentration range from1.0×10-5to1.0×10-1M. The detection limit obtained from the intersection of the extrapolated linear regions in the plot, is 6.31×10-6 M. The sensor shows nearly Nerntian slope 58.7mV per decade. The response time of the sensor is 30 seconds which is quite short. In terms of lifetime of the PVC membrane electrodes, their response stability was observed for over more than six months.
Figure 1. Potential responses of silver ion sensors based on ionophore[I].
Figure 1. Potential responses of silver ion sensors based on ionophore[I].
Sensors 02 00417 g001
The pH dependance of the membrane potential was also examined at 1.0×10-2M silver(I) concentration. As shown in Fig. 2, the membrane electrode shows good stability in relation to pH changes over wide pH range i.e 1.0 -6.0, which may be taken as the functional pH range of the sensor. In this plot, the high variation of the potentiometric response corresponds to pH limit.This points towards the applicability of the developed electrode in the moderately acidic media. As the pH of silver nitrate solutions lies in the functional range of the sensor, do not need any pH adjustment.
Figure 2. Plot showing the variation of membrane potential with pH at 1.0×10-2 M Ag+ ions.
Figure 2. Plot showing the variation of membrane potential with pH at 1.0×10-2 M Ag+ ions.
Sensors 02 00417 g002
Selectivity is perhaps the single most important characteristic of any sensor which defines the nature of device and the extent to which it may be employed in the determination of a particular ion in the presence of other interfering ions. This is measured in terms of potentiometric selectivity coefficients (log KPotAg,M) which has been evaluated using fixed interference method at 1.0x10-2M concentration of interfering ions. The potentiometric selectivity coefficients (logKPotAg,M) measures the response of the electrode for the primary ion in the presence of foreign ions. Table 1 shows potentiometric selectivity coefficient data of Schiff-base–p-tert-butyl calix[4]arene based silver ion- selective electrode for interfering cations relative to Ag+. The selectivity coefficients data indicate that KPotAg,M values are of the order of 10-3 for monovalent and for divalent metal ions (except for the mercury(II)ions) the values are of the order of 10-4 and 10-5. Therefore, the electrode can be used for the determination of silver ions in the presence of interfering ions.
These results demonstrated that Schiff-base-p-tert-butylcalix[4]arene[I] acted primarily as a Ag+ selective ionophore and avoided interference from other cations when present at high concentration of 1.0×10-2M. Even the strongest interferent Hg2+ does not disturb the performance of sensor when present at the concentration less than 1.0×10-5M (Fig. 3).
In a comparison with PVC based Ag+ ion sensor having calix[4]arene derivatives with functional hetrocyclic group such as pyridyl[9] as ionophore, it is interesting to note that the interference from Hg2+ is much prominent in normal performance of the sensor, Log KPotAg,Hg = -1.80. Further, the slope and linear range, detection limit of the proposed sensor are comparable and better in many respects than that sensor. From another comparison with Ag+ ion selective electrode incorporating bis(3- pyridinecarboxylate)calix[4]arene as an ionophore[8] in which the Hg2+ act as an strongest interferent with Log KPotAg,Hg >+1.0.,we find the sensitivity and selectivity of the Ag+ selective electrode develops in this study are better than those of previous electrodes.
Table 1. The selectivity coefficients of diverse ions.
Table 1. The selectivity coefficients of diverse ions.
Diverse ionsKPotAg,MLog KPotAg,M
K+2.24×10-3-2.65
Na+4.47×10-3-2.35
NH4+4.47×10-3-2.35
Mg2+2.69×10-5-4.57
Ca2+3.80×10-4-3.42
Ba2+7.94×10-5-4.10
Ni2+5.01×10-5-4.30
Co2+2.51×10-4-3.60
Cu2+1.59×10-4-3.80
Pb2+3.55×10-4-3.54
Hg2+1.0×10-2-2.00
Zn2+1.51×10-4-3.82
Cd2+3.80×10-4-3.42
Figure 3. Plots showing E vs Log [Ag+] in the presence of Hg2+ ions at varying level of interference ( )1.0×10-2 , (∏)1.0×10-3, (⊄) 1.0×10-4 (;)1.0×10-5 and (•) 0.0 M.
Figure 3. Plots showing E vs Log [Ag+] in the presence of Hg2+ ions at varying level of interference ( )1.0×10-2 , (∏)1.0×10-3, (⊄) 1.0×10-4 (;)1.0×10-5 and (•) 0.0 M.
Sensors 02 00417 g003
The proposed sensor works well under laboratory conditions and can be successfully employed in the potentiometric tritrations of Ag+ solutions with sodium chloride and the resulting titration curve is shown in Fig. 4. The electrode assembly can also used to determine chloride ion concentration in the tap water by potentiometric titration.
Figure 4. Plot showing the potentiometric titration of 1.0×10-1M of AgNO3 with 1.0×10-1M NaCl solution.
Figure 4. Plot showing the potentiometric titration of 1.0×10-1M of AgNO3 with 1.0×10-1M NaCl solution.
Sensors 02 00417 g004
Table 2. Analysis of water sample spiked with silver(I).
Table 2. Analysis of water sample spiked with silver(I).
Sample No.[Ag+]AAS(ppm)/ SD(n=4)[Ag+]ISE(ppm)/ SD(n= 4)
140/ 0.339.5/ 0.2
229/ 0.429.1/ 0.3
319.5/ 0.319.3/ 0.3
The applicability of the sensor is illustrated by measuring the silver(I) ion potentiometrically in Doubly distilled deionised water (DDW) spiked with 40, 30 and 20ppm silver(I). The results obtained were compared with those obtained from atomic absorption spectrometric (AAS) analysis and were found in good agreement (Table 2).

Conclusion

The silver ion selective electrode based on Schiff-base-p-tert-butylcalix[4]arene is comparable and superior in many respects than those reported in literature. The proposed Ag+ ion selective electrode posess better linear range (1.0×10-5-1.0×10-1M) and detection limit 6.31×10-6M and short response time. The Ag+- ion selective electrode based on Schiff-base-p-tert-butylcalix[4]arene shows good selectivity for Ag+ ion over other alkali metal ions.

Acknowledgements

We are thankful to Council of Scientific and Industrial Research, New Delhi,India for financial assistance. One of us (I.K) is thankful to Guru Nanak Dev University, Amritsar, India for providing Research Fellowship.

References

  1. Srivastva, S.K.; Gupta, V.K.; Jain, S. Analyst 1995, 120, 495.
  2. Mahajan, R.K.; Kumar, M.; Sharma, V.; Kaur, I. Analyst 2001, 126, 505. [PubMed]
  3. Mahajan, R.K.; Parkash, O. Talanta 2000, 52, 691. [PubMed]
  4. Buhlmann, P.; Pretsch, E.; Bakker, E. Chem.Rev. 1998, 98, 1593. [PubMed]
  5. Shean, S.R.; Shih, L.S. Analyst 1992, 117, 1691.
  6. Srivastva, S.K.; Gupta, V.K.; Jain, S. Anal. Chem. 1996, 68, 1272.
  7. Assubaie, F.N.; Moody, G.J.; Thomas, G.J. Analyst 1989, 114, 1545.
  8. Liu, Y.; Zhao, B.-T.; Chen, L.-X.; He, X.-W. Microchemical Journal 2000, 65, 75.
  9. Chen, L.; Zeng, X.; Ju, H.; He, X.; Zhang, Z. Microchemical journal 2000, 65, 129.
  10. Mahajan, R.K.; Kumar, M.; Sharma, V.; Kaur, I. Talanta 2002, 58, 545.
  11. Diamond, D. Jouranal of Inclusion Phenomena and Molecular Recognition in chemistry 1994, 19, 149.
  12. Kimura, M.; Miura, T.; Matsuo, M.; Shona, T. Anal. Chem. 1990, 62, 1510.
  13. Cadogan, A.; Diamond, D.; Smyth, M.R.; Deasy, M.; Mckervey, M.A.; Harris, S.J. Analyst 1989, 114, 1551.
  14. Cadogan, A.; Diamond, D.; Cremin, S.; Mckervey, M.A.; Harris, S.J. Anal. Proc. 1991, 28, 13.
  15. Cadogan, A.; Diamond, D.; Smyth, M.R.; et al. Analyst 1990, 115, 1207.
  • Sample Availability: Available from the authors.
Sensors EISSN 1424-8220 Published by MDPI AG, Basel, Switzerland RSS E-Mail Table of Contents Alert
Back to Top