The complex-formation equilibria between copper(II), nickel(II), cobalt(II) and zinc(II) and cycloserine (n-s-amino-Svtsoxazolidone,
C3H602N2)were investigated potentimetrically. It was found that cycloserine forms 1: 1 and 1: 2 (metal ion: ligand)complexes. The ternary complex of Cu" with nitrilotriacetic acid and cycloserine was investigated potentiometrically and spectrophotometrically.
The probable bonding in the chelated compounds formed in aqueous solution was deduced. The formation constants follow the Irving- Williams series

Afkar K. Abdel Hadi

Mohamed M. Shoukry

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CROATICA CHEMICA ACTA CCACAA 62 (1) 67-72 (1989)CCA-1840YU ISSN 0011-1643UDC 541.122NoteEquilibrium Studies of Binary and Ternary Complexes ofCycloserineMohamed M. Shoukry and Afkar K. Abdel HadiDepartment of Chemistry, Faculty of Science, University of United Arab Emirates,AI-Ain, P. O. Box 15551, United Arab EmiratesReceived January 26, 1988The complex-formation equilibria between copper(II), nic-kel(II), cobalt(II) and zinc(II) and cycloserine (n-s-amino-Svtso-xazolidone, C3H602N2)were investigated potentimetrically. It wasfound that cycloserine forms 1: 1 and 1: 2 (metal ion: Iigand)complexes. The ternary complex of Cu" with nitrilotriacetic aeidand cycloserine was investigated potentiometrically and spectro-photometrically. The probable bonding in the chelated compo-unds formed in aqueous solution was deduced. The formationconstants follow the Irving- Williams series.INTRODUCTIONCycloserine (CS) has wide application in the pharmaceutical industryand is a drug commonly used in c1inical therapeutics being a broad-spectrumantibiotic, inhibitory for l\iIycobacterium tuberculosis, Escherichia coli, Sta-phylococcus aureus and other microorganisms belonging to Psittacosis-lympho-granulo ma group. It is known that the metal complexes of ligands whichhave biological activity are more active than the free Iigands.l-" The useof the drug as metal complex instead of the free molecule could representa better route of administration associated with a small risk of toxic reactionsand could be a good sustained-release pharmaceutical preparation. Copper(II)and palladium(II) complexes of cycloserine" have been synthesized and cha-racterized. However, no data on the complex-formation equilibria betweentransition metal ions, commonly existing in biological fluids, and cycloserineseems to have been reported.We have a particular interest in the study of nitrilotriacetic acid (NTA).4,5This stems from the resemblance of NTA coordination sites to those of proteins(e. g. Concanavalin)." As a continuation of our research work oriented towardthe study of binary and ternary complexes of biologically active ligands,7-12we present a further study. This investigation traces the formation and cha-racteristics of binary and ternary complexes of cycloserine and nitrilotriaceticacid.EXPERIMENTALl\iIaterials and ReagentsCycloserine was provided by Fluka Chem. Co. Disodium salt of nitrilotriaceticaeid was supplied by Merck. The metal salts were in the form of nitrate and68 M. M. SHOUKRY AND A. K. ABDEL HADIpro vid ed by BDH. All solutions were prepared in doubly distilled water. Themetal ion solutions were standardized by EDTA using suitable Indicators.PApparatusThe pH values were measured by means of 114D Pu sl Munchen2 pH meter(Karl Kolb) using a special vessel described previously." The pH-meter and electrodewere calibrated by using standard buffer solutions, prepared according to NBSspecifications.v The potentiometric titrations were carried out with a Metrohm645 titrator. Spectrophotometric measurements were taken on a Pye Unicam SP8-400spectrophotometer.ProcedureThe following mixtures were prepared for the determination of acid dissocia-tion constant of cycloserine and formation constants of the bin ary and ternarycomplexes.(A) 10 mL of 0.02 M (CS) + 30 mL of 0.13 M KN03(B) 20 mL of 0.02 M (CS) + 10 mL of 0.02 M metal ion !- 10 mL of 0.40 M KN03·(c) 10 mL of 0.02 M metal ion + 10 mL of 0.02 M (NTA) + 20 mL of 0.20 M KN03•(D) 10 mL of 0.02 M metal ion + 10 mL of 0.02 M (NTA) + 10 mL of '0.02 M (CS) ++ 10 mL of 0.40 M KN03•Mixtures A-D were titrated against 0.20 M NaOH solution, at 25°C in a purifiedN2 atmosphere.Formation constants, evaluated from titration data, are defined by Eq. 1 and 21M + P NTA + q CS + r H ~ M[(NTA)p(CS)qHr(JI = [MI(NTA)p(CS)qHr]pqr [M]'[NTA]P[CSl"[H],(1)(2)Calculations were made with the aid of the MINIQUAD-75 computer program-š onan IBM-4331 computer. The model selected was that which gave the best statisticalfit and consistent with chemical logic. The formation constant, K~:~~~~;cs,of themixed-ligand complex was calculated assuming the complex M(NTA) is undisso-ciated in the region of mixed-Jigand complex formation. The results are listed inTable 1.TABLE IFormation constants of metaL ion compLexes with cycLoserineSystem p q r" log {J" sc x.~d R"'"H+ O O 1 1 7.27(0.01) 1.0 X 10-7 6 0.006O O 1 2 11.70(0.01)Cu" 1 O 1 O 6.03(0.03) 1.1 X 10-6 53 0.D101 O 2 O 9.93(0.03)1 1 1 O 1.38(0.09) 4.9 X 10-6 40 0.030Ni" 1 O 1 O 3.99(0.03) 1.9 X 10-6 67 0.0221 O 2 O 6.52(0.06)Co" 1 O 1 O 3.10(0.03) 5.1 X 10-6 76 0.021Zn" 1 O 1 O 3.31(0.01) 4.5 X 10-7 3 0.0061 O 2 O 5.60(0.01)• 1, p, q and r are the stoichiometric coefficients corresponding to M", NTA,cycloserine and H+, respectively; o Standard deviations are given in parentheses;e Sum of square of residuals; d Chi square; e Hamilton's reliability factor.COMPLEXES OF CYCLOSERINE 69Spectrophotometric measurements of the complexes Cu(NTA), Cu(CS), CU(CS)2and Cu(NTA)CS were carried out. These complexes were prepared by mixing Cu"and ligand solution in the appropriate ratio and the pH is raised to pH 7.5. Theanalytical concentration of Cu" in these complexes was 0.004 M.The charges on all the complex species reported in this paper are omitted forclarity.RESULTS AND DISCUSSIONThe potentiometric titration curve of cycloserine, mixture A, shows aninflection at a = 1, (a = moles of base added per mole of ligand), Figure 1.The addition of an equivalent of RN03 to cycloserine yields a potentiometriccurve exhibiting inflections at a = 1 and a = 2. This could be ascribed to theproton dissociation from (N=COR) and (NR3+)groups according to the pro-posed equilibriaThe bin ary complexes of cycloserine were investigated by titrating mix-ture (B). The potentiometric data of CuII, NilI and ZnII complexes was fittedwell by considering the formation of 1: 1 and 1: 2 complexes. The resultsof Con system revealed the formation of 1 : 1 complex only. The formationpH2~ ~ ~ ~o 2Moles of base odded per mole of eu (II)3Figure 1. Potentiometric titration curves of Cu(II)-NTA cycloserine system. Curves:(1) Cycloserine; (2) Cu(II)-NTA; (3) Cu(II)-NTA-cycloserine and (4) Composite curve.'10 M. M. SHOUKRY AND A. K. ABDEL HAD!of protonated complexes with all metal ions was rejected. Therefore, thebinding sites are the amino group and the exocyclic oxygen atom.It is evident from Table I that the stability constants of the binary com-plexes follow the orderCo" < Ni" < CuTI > Zn"which is in accord with the Irving Williams order.!"The tendency of cycloserine to form mixed-ligand complexes with theabove mentioned metal ions and NTA was studied. The titration curves ofthe CulI complexes are presented in Figure 1. The CulI-NTA (1 : 1) mixturetitration curve starts at pR - 2 and has a low pR buffer region followed bya sharp inflection at a = 1, corresponding to complete formation of the 1: 1complex. The mixed CuII-NTA-cycloserine (1: 1 : 1) solution does not showa sharp inflection at a = 1. The formation of the mixed-ligand complex isascertained by comparison of the mixed ligand titration curve with the com-posite curve, obtained by graphical addition of the free cycloserine curveto the 1 : 1 CulI-NTA titration curve. The experimental titration curve of themixed ligand system is quite different from the composite curve betweena = 1 and a = 2, indicating the formation of the mixed-ligand complex.Based on the above finding and in view of the fact that the 1 : 1 CuII-NTAcomplex is appreciably more stable-? than the 1 : 1 CuICcycloserine complex,it can be assumed that in the presence of both ligands, the NTA will beprimarily liga ted to the CulI ion, with subsequent liga tion of the cycloserine.The tendency of the other metal ions to form mixed-ligand complexesseems rather poor. As amatter of fact, the experimental titration curves oftheir mixed ligand system coincide with the composite curve.The relative stability of the ternary complex as compared to that of thecorresponding bin ary complex can be quantitatively expressed in differentways. Arecent review-" of these methods has shown that for a variety ofreasons the most suitable comparison is in terms of 6. log K, given by Eq. 3.A 1 K loa KCu(XTA) 1 K CuL\ og = og. Cu(NTA)CS - og Cu(Cs) (3)The log K value of CulI ion was found to be - 4.65. This means that thecycloserine forms amore stable complex with the free CulI ion than withthe Cu-NTA complex.The concentration distribution of the binary and mixed-ligand complexspecies (as percentage of total metal) as a function of pR was obtained byMINIQUAD-75 computer program. The distribution curves are presented inFigure 2. The different magnitudes of stabilitv constants of the binary and'ternary complexes are manifested unequivocal1y in different concentrationsof the complex species.Spectral analyses of biriary and ternary complexes of the CuII systemwere performed under a specified condition (pR = 7.5), where it was assumedthat the formation of these complexes is complete. It is known that the spec-trum of aquated Cu!' ion consists of a broad, weak, asymmetric band (E = 11)with maximum wavelength at 833 nm, which has been attributed to the2T2g~ 2Eg transition.P The spectral bands of the binary and ternary CuIIcomplexes are quite different from that of the aquated CuII ion, both asregards the positions of the maximum wavelengths and their average molarCOMPLEXES OF CYCLOSERINE 71"00-CuL2 CoLpHFigure 2. Concentration distribution of the complexes formed with cycloserine asa function of pH. The ordinate units: 100· [M]/[M,o'].TABLE IIMaximum wavelengths of the spectral bands of Cu" complexesT X 10"Cu!l NTA CSAmax/nm c/cm2 mmol'4 4 790 2404 4 770 2454 8 750 2554 4 4 710 265T = molar concentration.absorptivities, Table II. There is a general hypsochromic shift with anincrease in the spectral band intensity of the binary and ternary complexes,relative to that of the aquated CuII ion. It is noteworthy that hypsochromicshift, relative to that of aquated CuII ion, of 1 : 2 Cu-I-cycloserine is greaterthan that of the 1 : 1 complex. This is due to the increase in electron densityin the vicinity of the metal ion dorbitals as second ligand molecule is added.The spectrum of the mixed-ligand complex exhibits a band at a much lowerwavelength than those of Cu(NTA), Cu(CS) and Cu(CS)z. This confirms theformation of mixed-ligand complexes in solution.REFERENCES1. S. Kr i s c h ner, Y. K. W e i, D. Fra n c i s, and J. G. B e r g man, J. Med.Chem. 9 (1966) 369.2. A. J. T h o m s o n, R. J. P. W i Il i a m s, and S. R e s lova, Structure andBonding 11 (1972) 1.3. C. Pre t i and G. T o s i, J. Coord. Che71'~.9 (1979) 125.4. M. M. S h o ukr s, M. M. K h ate r, and E. IVI. S h o ukr s, Indian J. Chem.25A (1986) 488.5. M. M. S h o ukr y and E. M. S h o ukr s, Indian J. Chem. 27A (1988) 364.6. K. D. Ha r d man, Nletal Ions in Biological Systems, Plenum Press, New York,1973.M. M. SHOUKRY AND A. K. ABDEL HAD I7. D. L. Rab e n ste i n, A. A. I s a b, and M. M. S h o ukr y, Inorg. Chem. 21(1982) 3234.8. D. L. Rab e n ste i n, S. A. Da i g n a u 1t, A. A. I s a b, A. P. Arn old,and M. M. S h o ukr s, J. Amer. Chem. Soc. 107 (1985) 6435.9. M. M. S h o ukr s. A. E. Mah g o u b, and W. M. H o s n s, Transition Met.Chem. 12 (1987) 77.10. M. M. S h o ukr s. N. A. Dar w i s h, and W. M. H o s n s, J. Chin. Chem.Soc. 33 (1986) 179.11. M. M. S h o ukr s, Egypt J. Chem. 28 (1985) 433.12. M. M. S h o ukr y, E. M. K hai r y, and A. S a e e d, J. Coord. Chem. 17(1988) 305.13. F. J. W e 1c h e r, The AnalyticaL Uses of EthyLenediaminetetraacetic Acid, VanNostrand, Princeton, 1965.14. R. G. Bat es, Determination of pH, Wiley-Interscience, New York, 1973.15. P. Ga n s, A. S a bat i n i, and A. Vac c a, Inorg. Chim. Acta 18 (1976) 237.16. H. Ir v i n g and R. P. W i Il i a m s, Nature (London) 162 (1948) 746.17. D. D. Per r i n, StabiLity Constants of Metal Ion Complexes, Part B, OrganicLigands. Pergamon Press, 1979.18. R. B. Mar t i n and R. J. Pra d o s, J. Inorg. nucl. Chem. 36 (1974) 1665.19. B. N. F i g g i s, Introduction to Ligands FieLds, Interscience, Publishers, NewYork, 1966.SAŽETARBinarni i ternarni kompleksi cikloserinaM. M. Shoukry i .A. K. AbdeL HadiMetodom potenciometrijske titracije proučavano je nastajanje kompleksa ba-kra(II), nikla(II), kobalta(II) i cinka(II) s cikloserinom (D-3-amino-3-izoksazolidom,i utvrđeno je da nastaju kompleksi sastava ML i ML2• Ternarni kompleks bakra(II)s nitrilotrioctenom kiselinom i cikloserinom proučen je potenciometrijski i spek-trofotometrijski, i izvedeni su zaključci o vjerojatnom načinu vezivanja u nastalimkelatima.

Equilibrium Studies of Binary and Ternary Complexes of Cycloserine

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