Kinetics and Mechanism of Interaction between Chromium ( III ) and Ethylenediaminetetra-3-Propinate in Aqueous Acidic Media

The kinetics of the formation of 1:1 complex of chromium(III) with ethylenediaminetetra-3-propinate (EDTP) was followed spectrophotometrically at max = 557 nm. The reaction was found to be first order in chromium(III) and was accelerated by EDTP. Increasing the pH from 3.3 to 4.7 accelerated the reaction rate, the reaction rate was retarded by increasing ionic strength and dielectric constant of the reaction medium. A mechanism was suggested to account for the results obtained which involves ion pair formation between the various species of the reactants. Values of the activation parameters obtained indicate an associative mechanism.


Introduction
Synthetic chelating agents are used in many industrial applications because of their capability to bind and mask metal ions (such as Cr(III), Co(III), Fe(III)).Amongst these, ethylenediaminetetra-3-propinate is a synthetic organic metal chelating agent whose metal binding properties are exploited in a wide range of applications.These include detergent, food, pharmaceutical, cosmetic, metal finishing, photographic, textile and paper industries [1][2][3].It is also used as a component in decontamination formulation of nuclear reactors and in nuclear waste processing [4,5].
Although the experimental system and reaction studied here is very simple in nature, elucidation of the mechanism in this model system has implications for a variety of more complex homogeneous and heterogeneous phenomena involving metal-organic complexes (e.g., metal ion transport, bioavailability, and toxicity).
In this study, the reaction of chromium(III) and ethylenediaminetetra-3-propinate in weak acid solution is investigated.Factors affecting the rate of reaction were the goal of this study.

Reagents and Solutions
All chemicals were of pure grade and were used without further purification.All solutions were prepared using bidistilled water.The ethylenediaminetetra-3-propinate was prepared using a previously described procedure [6].Stock solution of (0.1 mol•dm −3 ) of hexaaquachromium (III) was prepared by dissolving CrCl 3 in bidistilled water and leaving the solution for 48 hours at 45˚C, where upon green color of CrCl 3 changed to blue color of aquachromium(III) [7].

Instrumentals
The absorbance measurements were performed using thermostatted 292 Cecil spectrophotometer and pH measurements were conducted with Griffin pH meter fitted with glass-calomel electrode standardized by potassium hydrogen phthalate.

Kinetic Measurements
Kinetic experiments were conducted by mixing thermostatted solutions of chromium(III) and the ethylenediaminetetra-3-propinate and adjusting hydrogen ion concentration to the required value with potassium hydroxide or perchloric acid.Ionic strength was adjusted by sodium perchlorate solution.The solution was then introduced into the reaction vessel, which was previously thermostatted to the desired temperature and the reaction was followed spectrophotometrically at  max = 557 nm for the complex formed.The reaction rate was followed under pseudo first order conditions where at least ten fold excess of the ligand concentration over the reactant chromium(III) concentration was always ensured.Values of the observed first order rate constant, k obs , were determined graphically for each run by plotting log (A  -A t ) versus time, t, where A denotes the measured absorbance and the subscripts refer to time of reaction.The absorbance (A  ) was obtained directly after ensuring completion of the reaction.First order plots were linear for more than 85% of the reaction progress.

Dependence on [Cr(III)] T
The reaction was found to be first order in chromium(III), the observed first order rate constants, k obs , did not vary with chromium(III) concentration, (Table 1) ensuring first order kinetics in chromium(III).

Dependence on [EDTP] T
The effect of varying ethylenediaminetetra-3-propinate concentration, on the rate of reaction was also studied at different pH values (Table 1) and a plot of the first order rate constant, k obs , against EDTP concentration was nonlinear, (Figure 1), indicating formation of ion pair [8,9].

Dependence on Ionic Strength
Increasing the ionic strength, I, of the reaction medium from 0.6 to 1.5 mol•dm −3 (adjusted by sodium perchlorate) the reaction rate (Table 1).Applying Bronsted Bjerrum equation [10,11], a linear relationship was obtained by plotting log k obs versus √I, (Figure 2) indicating that reaction involves ion pairing formation.

Dependence on Dielectric Constant
The effect of the dielectric constant on the rate of reaction was studied using different ratios of ethanol-water mixtures.The values of the observed first order rate con- stant, k obs increased with decreasing the dielectric constant of the reaction medium, ε, (Table 1).Applying Bjerrum's equation [10], a plot of log k obs versus 1/ε was linear with positive slopes, (Figure 3) indicating that the reaction is an ion pair type [12].

Dependence on pH
The effect of pH on the rate of reaction was studied in the range from 3.0 to 4.7 at various temperatures, (Table 2).The results obtained show that the reaction is accelerated by lowering hydrogen ion concentration.
The dependence of k obs on hydrogen ion concentration can be explained by in following equilibriums between the various species of each reactant which are present in the reaction medium [13,14]. (2)
The results obtained can be explained by the following mechanism for the interaction between the predominant species of chromium(III) with the predominant species of EDTP in the pH range under investigation where IP 1 -IP 4 are the hexaaquo and pentaaquohydroxy ion pair complexes of chromium(III) and EDTP.
The rate of exchange of the first ligand molecule, in the inner coordination sphere of the metal center is slow and therefore the rate determining Equations ( 7)-( 10) [19][20][21].As soon as one carboxyl group of the ligand enters into the inner sphere, the electron density on the chromium center increases owing to the inductive effect and as results the remaining ligands are labilized easily and its substitution is rapid.From the previous mechanism, the first order rate constant is derived as by inversing Equation ( 11) we get equation EDTP  and a plot of 1/k obs versus 1/[EDTP] gave s straight line with slopes and intercepts, I and The values of the ion pair formation constants, K IP and the rate constants of the rate determining steps, k, were calculating by plotting 1/k obs versus 1/[EDTP] at different pH, (Figure 4).Values 7.11,14.78,10.15and 16.81 mol −1 •dm 3 for the ion pair formation constants, KIP and 1.83, 4.81, 2.97 and 5.23 × 10 −3 s −1 for the rate determining steps, k, respectively were calculating by applying Equations ( 13)-( 15) at different hydrogen ion concentrations and taking the values of K 1 , K 2 and K h from Equations ( 1) and (2).The unexpected values of ion pair formation constants, K IP , ( .

K 
) indicate the mechanism is not only via electrostatic attraction but also include hydrogen bonding between the acetate groups and the first coordination sphere H 2 O.
The effect of temperature on the rate reaction was also studied at different hydrogen ion concentrations (Table 2).The activation parameters were calculating using Arrhenius plots values and the Eyring equation and were found to be 57.2 ± 3 kJ•mol −1 for the energy of activation and −128 ± 8 J•K −1 •mol −1 for the entropy of activation.

Conclusion
In the Present study, the kinetics of the reaction between chromium(III) and EDTP in weak acid aqueous solutions was investigated.The reaction was found to be first order in chromium(III).The reaction rate accelerated with in-creasing the EDTP concentration, pH, temperature, decreasing ionic strength and dielectric constant of the reaction medium.An associative mechanism was suggested to account for the results obtained

Figure 5 .
Figure 5. Plot of log k 1 with long k 2 for the substitution of water in [Cr(H 2 O) 6 ] 3+ by different ligands.and EDTP (this work).