Chemistry Journal <strong>of</strong> Moldova. N. Secara/Chem.J.Mold. General, Industrial and 2008, Ecological 3 (1), 127-128 Chemistry. 2008, 3 (1), 127-128DIHYDROXYFUMARIC ACID TRANSFORMATIONIntroductionSecara NataliaInstitute <strong>of</strong> Chemistry, 3, Academy st., Chisinau, Republic <strong>of</strong> MoldovaEmail: natalia_secara@yahoo.com, Phone: (+373 22) 72 97 61Abstract: This short communication presents several preliminary results obtained during kineticinvestigation <strong>of</strong> dihydroxyfumaric acid decarboxylation. The reaction order towards the hydrogenions concentration has been established, the correlation between the decarboxylation velocity andtemperature has been found, the Arrhenius equation for the decarboxylation constant has been drawn.Keywords: dihydroxyfumaric acid, decarboxylation, activation energyThe papers [1, 2] have demonstrated that in solid form, the dihydroxyfumaric acid (DFH 4) has the structure <strong>of</strong>the tautomeric ketonic form. Researches conducted by Souchay et al. [3] have shown that in solution this equilibriumin greatly influenced by the pH value <strong>of</strong> the medium, i.e., the equilibrium is totally shifted towards the ketonic form atpH < 0,5 and at pH>12 – towards the enolic form. Fleury [4] has shown that dihydroxyfumaric acid decarboxylationcan only take place through the formation <strong>of</strong> the ketonic form – oxaloglycolic acid, transparent for spectrometricmeasurements (>200 nm). The mechanism proposed in [4] for the primary decarboxylation is shown below:ExperimentalThe following reagents were used during the research: dihydroxyfumaric acid hydrate 98% purchased fromAldrich, sodium hydroxide, hydrochloric acid, EDTA – titration standards. All solutions were prepared using bidistilledwater. Freshly prepared dihydroxyfumaric acid solution was used in each experiment. The investigated solutioncontained: [DFH 4] 0= 1·10 -4 M, [EDTA] = 5·10 -3 M. The anaerobic medium was created by purging argon through thesolution. Spectrometric measurements have been made using a Perkin Elmer Lambda 25 Spectrometer at =290 nm,the established value <strong>of</strong> dihydroxyfumaric acid absorption maximum.Resultslg [H+]-7,8-7 -6 -5 -4 -3 -2-8y = 0,4894x - 6,0381R 2 = 0,9964-8,2-8,4lg v-8,6-8,8-9-9,2Fig. 1. The decarboxylation velocity <strong>of</strong> the dihydroxyfumaricacid, as function <strong>of</strong> the pH value <strong>of</strong> the solution, t=30°CAccording to [4], for values <strong>of</strong> pH > 3, the rate <strong>of</strong> decrease <strong>of</strong> the enolic form concentration is equivalentwith the velocity <strong>of</strong> decarboxylation <strong>of</strong> the dihydroxyfumaric acid, therefore making it possible to investigate thedecarboxylation reaction by the decrease in absorbance at 290 nm.127
N. Secara/Chem.J.Mold. 2008, 3 (1), 127-128Investigations allowed finding the dependence <strong>of</strong> the decarboxylation velocity on the pH value <strong>of</strong> the solution(for pH > 3), the decarboxylation velocity and the rate constant which describe this reaction have been calculated (Table1 and Figure 1). It was found that the reaction order towards [H + ] equals to 0,49.Table 1The decarboxylation velocity <strong>of</strong> the dihydroxyfumaric acid, as function <strong>of</strong> the pH value <strong>of</strong> the solution, t=30°CpHv r, mol/l·s3,9 1,2·10 -84,8 3,71·10 -95,8 1,33·10 -96,2 8,79·10 -10During current investigations, the influence <strong>of</strong> temperature on the rate <strong>of</strong> the decarboxylation process wasestablished. The decarboxylation rates and the rate constants have been calculated for the temperature range 20°C –60°C. The obtained results are shown in Table 2.Table 2The decarboxylation rate <strong>of</strong> the dihydroxyfumaric acid, as function <strong>of</strong> the temperature <strong>of</strong> the solution at pH 4,8t, °C v r, mol/l·s k T, s -120 5,43·10 -10 0,000460630 3,71·10 -9 0,002072740 4,29·10 -9 0,002763650 1,15·10 -8 0,007660 1,68·10 -8 0,011515Figure 2 illustrates how the rate constant <strong>of</strong> the decarboxylation reaction depends on the temperature <strong>of</strong> theinvestigated solution.00,0029-0,50,003 0,0031 0,0032 0,0033 0,0034 0,0035lg k-1-1,5-2y = -3294,6x + 8,0147R 2 = 0,9561-2,5-3-3,5-41/TFig. 2. The rate constant <strong>of</strong> the decarboxylation, asfunction <strong>of</strong> the temperature <strong>of</strong> the solution at pH 4,8Using the graphical method, the activation energy and the pre-exponential factor have been determined. Therewere obtained the following values: for the pre-exponential factor – 1,034·10 8 , for the activation energy calculated bythe graphical method - 63,08 kJ/mol, and by the analytical method – 65,3 kJ/mol.Therefore, we propose the Arrhenius equation which describes the variation <strong>of</strong> the rate constant with temperature,<strong>of</strong> the following form:3 7.58 10T8k 1.034 10 e .Aknowledgements: I would like to express my sincere gratitude to my scientific adviser, Acad. Gh. Duca, who helpedand guided me through the entire work, and Pr<strong>of</strong>. Maria Gonta, who encouraged me from the beginning.References:[1]. Syciov A., Scutaru Yu., Duca Gh., Journal <strong>of</strong> structural <strong>chemistry</strong> (Russia), 1986, Vol. 27, nr. 5, pp. 142.[2] Duca Gh., Catalysis <strong>of</strong> oxidation <strong>of</strong> tartaric and Dihydroxyfumaric acids, PhD thesis, Chisinau, 1979.[3]. Souchay P., Fleury D., Fleury M., C.R. Acad. Sci. Paris, 1967, Vol. 264, pp.2130.[4]. Fleury D., Bull. de la Soc. Chimique de France, 1970, Nr.1, pp.370.128
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