Azo compounds contain an azo group (-N=N-) bridge and have recently been used in many fields [1, 2]. These compounds have many advantages, including the ease of preparation, high purity, and abundant product. These facts motivated scientists to concentrate on researching this class of chemicals and the potential for using them in various applications. In addition, it has been utilized as an anti-cancer chemical and has successfully treated a variety of cancers . Azo compounds are coordination complexes containing transition elements that may attach to the DNA bases via their coordination with nitrogen atoms to create a chelating ring, making them useful in medicine [4, 5]. Furthermore, Azo compounds are anti-bacterial and anti-fungal materials [6, 7].
Zinc was one of the earliest discovered metals. It was referred to as brass when alloyed with copper (40% Zinc and 60% copper) . Zinc is resistant to attack in dry air at normal temperatures, but loses its luster in the moist air, creating basal carbonate, which functions as a protective cover, preventing further corrosion . It is an essential component of human, animal, and plant life, as well as a common biological component of nature . This ion is found in a few types of medicines . Zinc has a boiling point of 904 °C and shines white at 424 °C. However, it loses its shine after a short time because of the exospheric condition . Zn+2 has been characterized in several methods, including Flow Injection and Sequential Injection Techniques , Atomic Absorption Spectrophotometry , Cloud Point Extraction, Spectrophotometric Detection , Electrochemically , and development of HPLC method .
Materials and Methods
High-purity analytical materials were employed to make the solvents and compounds in this investigation. Zinc chloride was supplied by ROMIL and had a purity of 98 percent. Osteocare, Ferglobin, Zainc, Vitadex, and Calcipare were the utilized drugs. The majority of these medications are manufactured by German firms Fluka, BDH, Merck, and Sigma Aldrich. On a Bruker MHZ spectrophotometer, H-NMR spectra were captured by using DMSO-d6 as the solvent and TMS as the internal reference. The infrared spectra of Azo ligand were obtained as KBr discs by using a Shimadzu 8400 S FT-IR spectrophotometer in the 400 to 4000 cm-1 range.
Synthesis of thiazolyl azo dye ligand
The azo dye ligand was synthesized to use it in the same method [18, 19] with some modifications. 6-methylbenzo[d]thiazol-2-amine (1.64 g, 0.01 mol) was mixed with 3 mL of HCl, and 20 mL distilled water and diazotized below 4 °C with NaNO2 (0.75 g, 0.01 mol), dissolved in 35 mL. The diazonium salt was combined with (1.388 g, 0.01 mol) of 4-ethoxyphenol in alkaline media within 4 °C. The solution had a reddish-orange tint. Therefore, it was stirred for 60 minutes at 0 to 5 °C. Later, the solution was filtered, washed with distilled water several times, crystallized with 100% ethanol, and dried in an oven at 45 °C for a few hours. Scheme 1 displays the process of diazotase coupling.
Preparation of standard stock solution
Preparation of zinc ion for complexity
A 100 mg/L stock solution was prepared by dissolving 0.0209 g of water in 25 mL capacity Baker. The solution was then transferred to a 100 mL bottle, completed the size to the mark limit with pH=6.5 to 7, and adjusted by using the regulator solution to attend various concentrations by using the mitigation law.
Preparation of complex solution
A 1.5 mL of 5 mg/L and pH of 6.5 to 7 ion stock solution were mixed with 1.5 mL of the new organic reagent at 1×10-4 M concentration. Afterwards, the absorption was measured at 620 nm wavelength. The experiment was repeated under the same conditions, and average values were considered.
A.3. Positive ions interferences solutions
A 100 mg/L stock solution containing positive ions was prepared by dissolving certain weights of each substance in 100 mL distilled water and attended concentrations of positive ions for successive dilution.
Scheme1: A heterogeneous synthesis of the new Azo ligand (E)-4-ethoxy-2-((6-methylbenzo[d]thiazol-2-yl)diazenyl)phenol
Results and Discussion
Spectroscopic study for characterization of new hetrocyclic azo Ligand
As displayed in Figure 1, the spectra of azo ligand were measured by using (DMSO-d6) as a solvent in (TMS). The azo ligand was used as an internal reference (500 MHz). The parameters recorded for the ligand are illustrated in Table 1 [10, 20].
Figure 1: Spectrum 1H-NMR for azo ligand
Table 1: 1H-NMR spectra of azo ligand
|ligand (H atoms-peak-assignment)
1.32-1.35 (5H, t, 21)
2.4 (3H, S, 19)
2.52 solvent proton
3.99-4.03 (5H, q, 20)
6.00-7.10 (3H, S, 10, 11, 13)
7.13-7.20 (3H, S, 15, 17, 18)
10.30 (1H, S, 14)
Infrared spectra (FT-IR) for azo ligand
Table 2 presents the vibration bands stretching for functional groups in ligand and [Zn(L)Cl] in the 400-4000 cm-1 range of measurement [21, 22].
Study of precise analysis of reagent elements CHNS
The accurate analysis technique was used to characterize the new reagent by calculating the proportions of carbon, hydrogen, sulfur, and nitrogen elements, as summarized in Table 3. When comparing the values listed in the above table that were obtained in practice with the theoretically calculated values, the great convergence between them is clearly evident, that confirms the correctness of the formation of the solid reagent.
The electronic spectra measurement
The spectra of azo ligand were measured at room temperature at 1×10-4 M absolute ethanol. The results are listed in Table 4 and Figure 2.
Figure 2: UV-Visible spectra of azo dye ligand and complex zinc ion
Study the optimal conditions of complexity
Effect of reagent concentration
This study was conducted at a pH of 6.5 to 7- and 1-mL zinc solution. The 5 mg/L concentration was blended with a 1 mL reagent to form a series of 1×10-3 to 1×10-5 M concentrations. The absorption increases rapidly with increasing reagent concentration in the reagent concentration of 1×10-5 to 1×10-4 M where the best (optimum) reagent's concentration is achieved at wavelength 620 nm, as depicted in Figure 3. After the optimum concentration, the absorption declines, reaching about 0. 005 M. The increase of the reagent after concentration 0.0005 M does not affect the absorption.
Optimal reagent volume
The study was carried out through complex conditions, consisting of 1 mL ion size, 5 mg/L concentration, a series of 0.5 to 3 mL reagent at 1×10-4 M concentration, 620 nm wavelength, room temperature, and pH 6.5 to 7, as indicated in Figure 4. The maximum absorption is reached when the reagent volume is 1.5 mL. The absorption rises with increasing reagent volume. After reaching this concentration, the absorption starts to decline and eventually approaches 0.04 in the vicinity of reagent volume 3 mL.
Figure 3: Effect of reagent concentration
Figure 4: The optimal reagent volume
Optimal zinc ion volume
The optimal ion volume was studied by taking a series of ion volume from 0.5 to 2.5 mL at 5 mg concentration. Increasing the volume of zinc ions increases the absorption ability. The result shows that increasing volume zinc ions from 0.5 to 1 increased the absorption 10 times. The maximum absorption was achieved at 1.5 mL zinc ions volume at 1 ×10-4 M concentration of reagent and when increasing zinc ions volume more of 1.5 ml decreases the absorption ability, as demonstrated in Figure 5.
Effect of time on Zn(II) complex formation
This study was carried out in the best above mentioned conditions and at 25 to 40 °C. In these conditions, the complex has a good stability in the time frame between 0.5 to 120 min, as demonstrated in Figure 6.
Calibration curve to complex Zn(II)
After obtaining the best conditions, a series of ion metal concentrations were performed 0.01 to 30 mg/L. A linear relation was obtained in the range of (0.3 to 20 mg/L). The results outcomes were 0.1754 μg.cm-2. Sandal sensitivity was 0.2632 mg/L LOD, 0.8772 mg/L LOQ, respectively, as illustrated in Figure 7. The R2 value was 0.9997, indicating that the experimental data on absorption and Zinc(II) concentration were well fit by the linear equation.
Figure 5: Optimal zinc ion volume
Figure 6: Effect of time on the Zn(II) complex formation
Figure 7: Calibration curve to complex Zn(II)
Figure 8: Mole ration method
Determination of possible composition
Mole ration method
The molar ratio of the reagent to the metal ion was studied extensively and illustrated in Figure 8. The results show that the crossing of the two fitting lines was at reagent/ion of 1:1 ratio.
Stability Constant (β) for Complexes Zn+2 ion
To find out the stability of the formed zinc compound (II) and the possibility of its study by spectroscopic methods, the dissociation degree and its stability constant were calculated according to the following equations:
Study of interference
The positive and negative ions that may interfere with the zinc ion during its complexity were studied with the new reagent (Cu, Ni, Co, Fe, Mg, Mn, Cd, F, So4, I, CH3Coo, and Br). At the end of the experiment, it was found that all ions did not interfere except copper and iron and the interference was removed by using a blocking agent S2O3 .
The analytical method used to determination the Zinc(II) ion was applied to different drug samples at a concentration of 5 mg/L and comparing its results with the results of the FAAS technique for the same drug samples. The results outcomes are listed in Table 5. Based on Table 5, we deduced the recovery rate for Spec. technique (95-104) %, while for FAAS technique (94 -106%).
Statistical values for applications at technical Spec and FAAS
Table 6 shows the statistical values of different drug samples in the two techniques Spec. and FAAS.
According to the above mathematical equations, we deduce that since t calculated value is less than t scheduled value, the zero theorem is accepted.
The analytical method is straightforward and achieves high results, as it is easy to prepare and diagnose the new organic reagent, the ease of spectral estimation of the zinc binary complex, and its complexity with a group of other metal ions such as Ni and Cu, after fixing the optimal conditions of concentration and size of the reagent, acidity function, time, temperature, and molar ratio. After estimating the ion under study, we obtained high stability, control, efficiency, and accuracy at the greatest absorption wavelength of the zinc ion complex 620 nm under the optimal conditions. Except for the copper and iron ions that interfere with the metal ion and are blocked by S2O3, the recovery rate of the drug for the proposed method ranged from 95% to 104% when compared with the flame atomic absorption spectrum in which the recovery rate ranged between 94-106%. The results of the technique under study showed that it has a higher sensitivity compared with FAAS. Moreover, the complex stability constant is K=2.59×105, and when studying the statistical values for both techniques, it turns out. The t calculated value is less than the t scheduled value. Thus, the zero theorem is accepted.
This research did not receive any specific grant from funding agencies in the public, commercial, or not-for-profit sectors.
All authors contributed to data analysis, drafting, and revising of the paper and agreed to be responsible for all the aspects of this work.
Conflict of Interest
We have no conflicts of interest to disclose.
HOW TO CITE THIS ARTICLE
Thekrayat Joodi Jassim, Haider M. Hessoon, Faiq F. Karam. Preparation and Characterization of New Hetrocyclic Azo Thiozal Dye Ligand and Its Use As a Reagent for Determination of Zn+2 Ion in Drug by New Analytical Method. J. Med. Chem. Sci., 2023, 6(4) 857-867