Cadmium Succinate and Cadmium Malate Stability Constants Revisited

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  • Cadmium Succinate and Cadmium Malate Stability ConstantsRevisited

    Montserrat Filella*

    Department of Inorganic, Analytical and Applied Chemistry, University of Geneva, Quai Ernest-Ansermet 30,CH-1211 Geneva 4, Switzerland

    Raewyn M. Town

    School of Chemistry, David Keir Building, The Queens University of Belfast, Stranmillis Road,Belfast BT9 5AG, Northern Ireland

    Mercedes Garca Bugarn

    Departamento de Qumica Inorganica, Universidad de Vigo, Calle Torrecedeira 86, E-36208 Vigo, Spain

    The complexes formed in the cadmium(II) succinate (suc2-) hydrogen ion and in the cadmium(II) malate(mal2-) hydrogen ion systems in aqueous solution at 37 C and I ) 150 mmoldm-3 (NaCl) have beencharacterized by means of glass-electrode potentiometry. The succinate and malate protonation constantswere found to be 5.187 ( 0.001, 9.135 ( 0.002 and 4.618 ( 0.001, 7.804 ( 0.002, respectively. The formationconstants for the complexes Cdsuc, CdsucH+, and Cdmal were found to be 1.63 ( 0.02, 6.26 ( 0.06, and1.25 ( 0.05, respectively. Particular attention has been paid to the evaluation of the effect of possiblesystematic errors on the constant values determined. Reliable standard deviation estimations have beenmade by applying a Monte Carlo calculation technique. Cyclic voltammograms and differential pulsepolarograms for both cadmium(II) systems were consistent with formation of weak, labile complexes.


    Succinic acid (butanedioic acid, ethane dicarboxylic acid),HOOC-CH2-CH2-COOH, and malic acid (hydroxybu-tanedioic acid, monohydroxysuccinic acid), HOOC-CHOH-CH2-COOH, are naturally occurring ligands present inmany organisms. Succinic acid is an important intermedi-ate in the tricarboxylic acid cycle, where it is formed fromR-ketoglutaric acid. It is used via reactions in the tricar-boxylic cycle and in the glyoxylate cycle for the synthesisof amino acids and carbohydrates. The S-isomer of malicacid is also an intermediate both in the tricarboxylic acidcycle, being formed by hydration of fumaric acid andconverted into oxaloacetic acid by malate deshydrogenase,and in the glyoxylate cycle. Succinate is present, in free orbound form, especially as calcium and potassium succi-nates, in unripe fruits, algae, fungi, and lichens. Malateplays several metabolic roles in plants, for example in thediurnal acid rhythm of the Crassulaceae. Malic acid isfound free in sour apples, quinces, and berries. Succinateand malate are used in the preparation of drugs and inflavorings. Malic acid is also used to impregnate packingmaterials for foods.

    Despite their biological significance, values of the stabil-ity constants for metal succinate and malate systems inaqueous solution have rarely been determined underconditions of temperature and ionic strength close to thoserelevant for biological fluids.

    Determination of stability constants for weak complexes,as in the present case for the cadmium succinate and

    malate systems, is not straightforward because the ana-lytical signals are only slightly perturbed in the presenceof complex formation. This situation is common to manybiological, and environmental, systems. For such systems,the effect of experimental errors on model selection andon the constant values obtained can be very important andmust be carefully checked. Failure to adequately considerthese aspects may be a source of the disparity amongpublished stability constant values.

    In the present study, two different analytical techniquesare applied, glass potentiometry and voltammetry. Par-ticular attention is paid to the evaluation of the effect ofpossible systematic errors on the constant values deter-mined, and reliable standard deviation estimations aremade by applying a Monte Carlo calculation technique.Comparison of the values obtained with previously pub-lished values allows discussion of the validity and limita-tions of some of the existing values.

    Experimental SectionPotentiometric Studies. A. Reagents. Analytical grade

    reagents were used throughout. All solutions were preparedusing demineralized water (Millipore system), which hadbeen boiled and cooled under nitrogen, and stored underan atmosphere of purified nitrogen.

    Malic and succinic acids were purchased from Merck.They were potentiometrically assayed and found to besufficiently reliable to be used without further purification.Ligand solutions were freshly prepared daily by directweighing.

    Stock solutions of cadmium were prepared from theirchloride salts and were made slightly acidic by adding* Corresponding author. E-mail:

    1009J. Chem. Eng. Data 1999, 44, 1009-1019

    10.1021/je990048w CCC: $18.00 1999 American Chemical SocietyPublished on Web 08/18/1999

  • hydrochloric acid to prevent hydrolysis and adsorption ofcarbon dioxide. The metal content of the solutions wasdetermined against EDTA using xylenol orange as indica-tor (Vogel, 1971). Their mineral acid content was deter-mined by titration with standard alkali (Gran, 1988) andthe concentration verified by using the MAGEC program(May et al., 1982).

    Carbonate-free sodium hydroxide solutions were pre-pared from Merck standard volumetric solutions. Alkalititer and absence of carbonate were checked by means ofGran plots (Gran, 1988) using potassium hydrogen phtha-late (Merck) as the acid.

    B. Technique and Experimental Conditions. Forma-tion constants were determined from potentiometric titra-tions. A Radiometer PHM93 millivoltmeter was used tomonitor the emf of cells of the type

    where G.E. denotes a glass electrode (Orion 91-01) and R.E.a double-junction silver/silver chloride reference electrode(Orion 90-02). Successive aliquots of sodium hydroxide wereadded to the solution by means of a Metrohm Multi-dosimat 665 autoburet. A versatile computer-controlledsystem for data acquisition was used throughout. Allexperiments were carried out in a titration cell thermo-stated at (37 ( 0.02) C by circulating thermostated water.Titrations were performed in a nitrogen atmosphere.

    Sodium chloride (150 mmoldm-3) was used to maintainthe ionic strength constant and to ensure isotonicity withblood plasma. Although, from the thermodynamic view-point, the conditions used are not ideal due to the possibleassociation of chloride with metal ions (Daniele et al.,1985), the advantage is that constants obtained in this saltsolution implicitly account for the influence of the biologicalmedium.

    The electrode system was calibrated in terms of hydrogenion concentrations by performing strong acid versus strongbase titrations (Linder et al., 1984). The logarithm of theconcentration quotient for water dissociation under thesame experimental conditions was found to be -13.36, ingood agreement with literature values (Pettit and Powell,1997).

    The cadmium and ligand solutions used were acidifiedsuch that all the ligand donor groups were protonated atthe beginning of each titration. Titrations were performedover the wider range of metal-to-ligand ratios allowed bythe working ionic strength. Data were recorded over thewidest possible -log[H] range. Replicate titrations weredone to check reproducibility.

    Titration data used for calculating formation constantsare summarized in Table 1.

    C. Calculation Procedures. The general equilibriainvolving metal M2+, ligand L2- (i.e. deprotonated succinicacid ) suc, deprotonated malic acid ) mal), and H+ ionscan be written as

    Signs are omitted for simplicity. The overall formationconstant is denoted by pqr.

    The titration data were processed with the ESTA com-puter program library (May et al., 1985, 1988; May andMurray, 1988a, 1988b) by following our previously de-scribed approach (Filella et al., 1987a, 1987b; GarcaBugarn et al., 1989; Garca-Tasende et al., 1991a, 1991b)involving optimization and simulation in successive steps.The initial models were obtained from the experimental

    protonation, deprotonation and formation curves. Proto-nation curves are obtained by plotting the average numberof protons bound to each ligand, Zh H, as a function of-log[H]

    where TH, TL and TOH ) total concentrations of strong acid,ligand, and hydroxide, respectively and n ) number oftitratable protons of the ligand. Deprotonation curves areobtained by plotting Qh as a function of -log[H], Qh beingdefined as

    Table 1. Summary of Titration Data Used in theFormation Constant Calculations: Number of TitrationPoints, Initial Total Concentrations of Cadmium(II) (TM),and Ligand (TL) in mmoldm-3, and -log[H] RangeInvestigated

    system titrationno. ofpoints TM TL


    suc-H+ 1 48 5.1 2.30-8.502 46 5.1 2.30-6.063 50 9.6 2.29-6.544 50 9.6 2.29-6.555 48 14.9 2.28-6.496 49 14.9 2.28-8.677 45 15.39 2.28-6.958 59 15.39 2.29-6.529 53 19.25 2.28-6.22

    10 53 19.25 2.28-6.2211 55 19.86 2.28-6.3712 47 19.86 2.28-6.37

    mal-H+ 1 45 4.85 2.27-5.622 46 4.85 2.27-6.163 44 5.17 2.26-5.074 48 5.17 2.27-6.325 42 10.08 2.24-6.086 52 10.08 2.23-5.977 53 10.34 2.23-5.938 57 14.94 2.21-5.769 43 14.94 2.20-5.75

    10 63 19.98 2.18-7.0211 56 19.98 2.18-6.04

    Cd2+-suc-H+ 1 42 0.8554 12.36 2.79-5.372 42 0.8554 12.36 2.79-5.373 43 0.8554 16.29 2.74-5.504 42 0.8554 17.30 2.74-5.285 41 0.8554 17.30 2.73-5.236 51 0.8554 26.21 2.68-6.017 52 0.8554 26.21 2.68-6.188 44 1.711 7.616 2.68-5.509 51 1.711 17.40 2.61-5.84

    10 49 1.711 17.40 2.61-5.6511 49 1.711 26.03 2.56-5.7312 49 1.711 26.03 2.57-5.7413 52 3.421 7.62 2.44-5.7914 50 3.421 26.03 2.39-5.67

    Cd2+-mal-H+ 1 50 0.8554 16.17 2.46-5.952 45 0.8554 17.06 2.46-4.933 43 1.711 7.33 2.52-4.974 47 1.711 17.06 2.40-4.995 47 1.711 17.06 2.70-4.996 52 1.711 17.54 2.39-5.337 55 1.711 17.4 2.39-5.918 48 1.711 25.70 2.32-5.139 46 1.711 25.70 2.31-4.96

    10 51 3.421 7.33 2.38-5.2811 52 3.421 17.37 2.28-5.1412 53 3.421 17.37 2.29-5.2313 54 3.421 25.70 2.24-5.71