1. Introduction

L-Trp or D-Trp; sold for medical use as Tryptan (fig. 1)[1] is one of the 20 standard amino acids, as well as an essential amino acid in the human diet. It is encoded in the standard genetic code as the codon UGG. Tryptophan (Trp) is considered exceptional in its diversity of biological functions[2]. It is a vital constituent of proteins and indispensable in human nutrition for establishing and maintaining a positive nitrogen balance[3]. Besides, some of its derivatives are potent drugs[4]. Trp is widely used in food industry. It is sometimes added to dietary and feed products as a food fortifier in order to maintain the amino acid balance of the food and correct possible dietary deficiencies. Trp can also be used to study structure and dynamics of the proteins because of its indole moiety[5]. In particular, Trp is the precursor of the neurotransmitter serotonin and plays an important role in brain function and related regulatory mechanisms[6]. In addition, Trp is an important and frequently used starting material in the chemical synthesis of a range of pharmaceuticals[7].

The distinguishing structural characteristic of tryptophan is that it contains an indole functional group. It is an essential amino acid as demonstrated by its growth effects on rats. Now it is interesting to investigate the complex bilding of ternary systems with Trp. We would like to determine the

thermodynamic constants of ternary complexes such as Cu(Har)(Trp).

Figure 1. Chemical formula of L-Tryptophan

2. Experimental

2.1. Materials

Chemicals were purchased from Merck. Copper(II) nitrate trihydrated, sodium nitrate, potassium hydrogen phthalate and standard solutions of sodium hydroxide (titrasol), 2,2'- bipyridyl, 1,10-phenanthroline, nitric acid, EDTA and of the buffer solutions of pH 4.0, 7.0 and 9.0 were from Merck. All the starting materials were pro analysis and used without further purification. Water was purified by Mili-Q water purification system, deionized and distillated.

2.2. pH titrations

Reagents: Carbonate-free sodium hydroxide 0.03 M was preparated and standardized against sodium hydrogen phthalate and a standard solution of nitric acid 0.5 mM. Copper (II) nitrate solution (0.03 M) was prepared by dissolving the above substance in water and was standardized with standard solution of EDTA 0.1 M (triplex).

2.3. Apparatus

All pH titrations was performed using a Metrohm 794 basic automatic titrator (Titrino), coupled with a Hero thermostating bath at 25℃ (±0.1℃) and a Metrohm combined glass electrode (Ag/AgCl). The pH meter was calibrated with Merck standard buffer solutions (4.0, 7.0 and 9.0).

2.4. Procedure

For the determination of acid dissociation constants of the ligand Trp an aqueous solution (0.3 mM) of the protonated ligand was titrated with 0.03 M NaOH at 25℃ under nitrogen atmosphere and ionic strength of 0.1 M, NaNO₃. For the determination of binary (one ligand and Cu²⁺) and ternary systems (Cu²⁺, one of the other L ligand (Har) and Trp), the ratios used were 1:1, 1:2 Cu(II) : ligand and 1:1:1, Cu(II) : Trp : Har, 0.3 mM. This solution was titrated with 0.03 M NaOH under the same conditions mentioned above. Each titration was repeated seven times in order to check the reproducibility of the data.

Calculation

The acid dissociation constants, and for H₂(Trp) were calculated by an algebraic method. The equilibria involved in the formation of 1:1 complex of Trp and a divalent metal ion may be expressed as equations (3) & (4).

3. Results and Discussion

In this section we would discuss the resulted data.

3.1. Acidity Constants

Tryptophan (Trp) can accept one proton on carboxylic group, for which the following deprotonation equilibria hold:

(1a)

(1b)

Trp can release one other proton from amine group according following deprotonation equilibria:

(2a)

(2b)

Also the two protons in H₂(Trp) are certainly bound at the terminal acetate group and amine group, i.e., it is released from −CO₂H or –NH₂ according to equilibrium (1) & (2). These values are, as accepted, close to the pKa values of –CO₂H which is 2.22[8].

3.2. Stability of Binary and Ternary Complexes

If we abbreviate for simplicity Cu²⁺, Cu(Bpy)²⁺, and Cu(Phen)²⁺ with M²⁺, one may write the following two equilibria (3) & (4):

(3a)

(3b)

(4a)

(4b)

The experimental data of the potentiometric pH titrations may be completely by considering the above mentioned equilibria (1) through (4), if the evaluation is not carried into the pH range where hyrdoxo complex formation occurs.

The stability of ternary complexes may be evaluated by the following equilibrium:

(5a)

where M is the metal ion, H is the proton, A and B are the ligand. The global stability constant for the ternary complexes may be represented as following:

(5b)

It is possible to define the stability constants for ternary complexes in relation to their binary ones[9], represented by the equilibrium (6) & (7).

(6a)

(6b)

(7a)

(7b)

Differences between the stability constants of the ternary and binary complexes show the tendency of the formation of ternary species[10]. This could be expected by Eq. (8):

(8)

The difference between the constant refined from experimental data and those calculated statistically using Eq. (8) indicates the possibility of ligand-ligand interaction.

3.3. Potentiometric Analyses

The model of species for this ternary system that was used in superquad program includes all the species of table 1 as well as the hydrolysis of Cu²⁺[11,12]. The stability constants of the binary complexes were refined separately using the titration data of this system in a 1:1 and 1:2 ligand:Cu²⁺ ratio in the same conditions of temperature and ionic strength. They were fixed and, consequently, only ternary species were refined in ternary model of the species. The results are summarized in Table 1.

Table 1. Logarithm of the stability constants of binary and ternary complexes of M2+ at 25℃, 0.1 M, NaNO3* =2.22±0.08 =9.14±0.03 No. Species logKa Δlog Kb Ref. 1 Cu2+ 8.05±0.05 - [13] 2 Cu(Bpy)2+ 9.02±0.06 0.97±0.08 - 3 Cu(Phen)2+ 9.36±0.08 1.31±0.09 -

The order of the resulted stability constants are Cu²⁺ < Cu(Bpy)²⁺ < Cu(Phen)²⁺. Figure 2 shows Schematic structures of the species with interactions according to equilibrium (4) & (7) for Cu (Phen)(Trp). The results of the acidity constants show good agreement with reported values[13]. The reported stability constant of Cu(Trp) complex is similar to our results (tab. 1).The difference between stability constants according eq. (8) show that mixed ligand complexes[14-17] formed by a divalent 3d ion, a heteroaromatic N base and an O donor ligand possess increased stability. Now one can calculate the free energy ΔG, used ΔlogK received from eq. 8 (tab. 1). We receive for Δlog 5.441 kJ/mol and for Δlog 7.349 kJ/mol, which are considerable high. This means that interaction between Cu(Har)²⁺ and trp²− is relative strong and the observed increased stability indicate strong complex bilding of ternary systems.

Figure 2. Schematic structures of the species with interactions according to equilibrium (4) & (7) for Cu(Phen)(Trp). The structure in the right part of the figure was drawn with the program CS Chem 3D, version 3.5, from Cambridge Software Corporation

Notes

1. Trp: L-Tryptophan

2. Bpy: 2,2'-Bipyridyl

3. Phen: 1,10-phenanthroline

4. Har: Heteroaromatic ligand such as Bpy or Phen