Ozonation of azo dye acid black 1 under the suppression effect by chloride ion

ARTICLE

Ozonation of azo dye acid black 1 under the suppression effect by chloride ion

Alexandre Paprocki; Heldiane S. dos Santos; Marta E. Hammerschitt; Marçal Pires; Carla M. N. Azevedo^*

Faculdade de Química, Pontifícia Universidade Católica do Rio Grande do Sul, Av. Ipiranga, 6681, 90619-900 Porto Alegre-RS, Brazil

ABSTRACT

The aim of this study is to determine the kinetics of the Acid Black 1 dye by oxidizing action of ozone and to evaluate the influence of chloride ion contamination on the dye degradation. Pseudo-first order kinetics was observed for both decolorization (620 nm) and aromatic structure (321 nm) degradations. A complete color removal was verified in 25 min ([dye]₀ = 1.8 × 10^-5 mol L^-1), while aromatic structures degraded at slower rates. The presence of chloride ion, the principal impurity of the solid dye reagents, influences significantly the ozonation rate (-42%), even at low chloride concentration (5.6 × 10^-4 mol L^-1). The most probable mechanism for the chloride suppression effect involves a direct reaction between O₃ and Cl^- generating HOCl, among other by-products. In despite of that, ozonation could be a competitive degradation process for this dye.

Keywords: azo dye, ozonation, salt additives, chloride ion, suppression effect

RESUMO

O objetivo deste estudo é determinar a cinética degradação do corante Acid Black 1 por ação oxidante do ozônio e avaliar a influência da contaminação de íons cloreto na degradação deste corante. Foram observadas cinéticas de pseudo-primeira ordem, tanto para a degradação das estruturas cromóforas (620 nm), quanto das aromáticas (321 nm). A completa remoção da coloração foi verificada em 25 min ([corante]₀ = 1,8 × 10^-5 mol L^-1), enquanto que as estruturas aromáticas foram degradadas com menor velocidade. A presença de íon cloreto, principal impureza do reagente sólido, influencia significantemente a velocidade de ozonização (-42%), mesmo em baixa concentração (5,6 × 10^-4 mol L^-1). O mecanismo mais provável para o efeito supressor do íon cloreto envolve a direta reação entre O₃ e Cl^- gerando HOCl, dentre outros subprodutos. Apesar deste aspecto, a ozonização pode ser um processo de degradação competitivo para este corante.

Introduction

The Acid Black 1 (C.I. 20470) is an important azo dye widely used in the textile industry. This compound is used not only to dye or to print on synthetic and natural fibers, but also as intermediate in the synthesis of other azo dyes. Another application of the Acid Black 1 is as indicator to assist in the protein separation for chromatography and electrophoresis analyses.¹

Textile effluents, when not correctly treated, can cause high impact to the environment. Azo dyes are considered as harmful compounds due to their mutagenic and carcinogenic characteristics. The toxicity of theses dyes is often related to the amines employed or formed in their syntheses.²

Dye wastewaters can be treated by conventional processes, such as activated carbon absorption or coagulation, or by alternative technologies including electrochemical treatment,^3,4 absorption using new materials and advanced oxidative processes (AOPs).⁵ Despite the fact that ozonation in acid medium is not an AOP, O₃ proved to yield excellent results on dye effluents treatment.^6-9 Some studies have been reported about destruction of Acid Black 1 by ozonation.^10-13 However, none of these studies concerned the by-products formation during ozone attack.

The possible interferences on ozonation efficiency by the presence of additives have been reported for the treatment of the dyes,^9,11,14,15 as well as for other class of compounds.^16,17 However, the available information concerning the role of these dye additives on the kinetics and by-product formation is scarce.¹⁶ The inorganic salts are the most common additives used, as exhausting and retarding agents, during textiles dyeing processes and its quantity varies from 5 to 60 g L^-1.¹⁸ Gahr et al.¹⁹ mentioned the effect of salt during ozone decoloration of reactive dye effluent and reported that, at higher levels, the presence of salt lowers the decomposition of reactive dyes.

Muthukumar et al.¹¹ observed that the ozonation kinetics of the Acid Black 1 is affected by the presence of some sodium salts (carbonate, chloride and sulfate). These authors explained the influence of added salts by side-reaction with O₃, which becomes less available for dye degradation. However, with respect to chloride ion, Gunten²⁰ stated that inorganic chlorine-derived by-products are only formed during ozonation if Cl^- aqueous solution is pretreated with chlorine or chlorine dioxide.

The influence of the impurities, commonly encountered in commercial dyes, is less studied. According to Lyon,²¹ these impurities present in dyes are: (i) diluents such as inorganic salts, starch and dispersing agents; (ii) by-products formed during manufacture and (iii) dyes of different constitution and color that are added for shading. Zhang and co-workers¹⁴ investigated the effects of impurities on the ozonation degradation of the azo dye C.I. Reactive Red 120. These authors compared the results obtained for unpurified (75%) and purified (90%) dyes, and concluded that the presence of impurities affects mostly the biodegradability of the dye. Zhang et al.¹⁴ also suggested that dyes need to be purified before ozonation treatment if detailed information on the oxidative processes and by-production formation are required.

In this context, special attention has been given to chloride ion that is additive as well as impurity for textile dyes.^{9,11,14,15,18,19,22} When present as additive, at relatively high concentration (0.5-5 g L^-1), Cl^- seems to play an important role on dyes degradation processes.^9,11,15,18 The possible influence of the low chloride concentration (< 50 mg L^-1, as an impurity) on dye ozonation has not been reported in literature. Despite the importance of chloride in this system, the mechanism of its action on dye ozonation is not completely understood.

The aim of this study is to determine the kinetics and by-products formation on the Acid Black 1 ozonation and to evaluate the influence of sodium chloride impurity on dye degradation. The reaction between O₃ and Cl^- was also investigated for a better understanding of the chloride suppression effect. Finally, the literature data about Acid Black 1 degradation processes as well as the chloride suppression effect on dye ozonization are discussed.

Experimental

Materials

The Acid Black 1 reagent (C.I. 20470) was obtained as a commercial dye from two suppliers Acros (purity 63.2%) and Sigma (> 80%). In Figure 1 the chemical structure of the dye, which has a molecular formula C₂₂H₁₄N₆Na₂O₉S₂ (616.48 g mol^-1) and solubility less than 0.1 g L^-1 in water, is shown. The reagents were used as received and Acros dye reagent was also purified to verify the possible influence of impurities on degradation process.²² The aqueous solutions containing nominal concentrations of the 5, 10 and 20 mg L^-1 on dye reagent were used in kinetic tests. All solutions were prepared with ultra pure water (MilliQPlus, Millipore; < 18 MΩ cm). Chloride ion work solutions were prepared using NaCl (Merck, 99.5%) or HCl (Merck 37%). All other reagents used were of analytical grade.

Dye purification was performed following Lankin procedure,²² which consists of the several sequential washings with sodium chloride and aqueous isopropanol solutions. In this way, 5 g of dye was weighed into centrifuge bottle and 10 mL of 6% sodium chloride solution was added and shaken vigorously for 20 min and centrifuged (2,000 rpm) for 10 min. The supernatant was separated and the treatment was repeated one more time with 6% sodium chloride solution and twice with aqueous isopropanol (100:20, isopropanol:water, v/v). For these washings the period of stirring was 10 min and then the dye was filtered using a Buchner funnel and dried in an oven at 110 ºC. Next the dye content on solid was estimated by its absorbance (λ_max 620 nm) on aqueous solutions using Lankin absorption coefficient ( 921).

Experimental set-up

The experimental set-up consisted of a prototype corona discharge generator (OZ Engenharia, Brazil) which uses dried atmospheric air to generated ozone, driven by air pump with flow rate of 1.32 ± 0.04 L min^-1. Production rate was 35 mg O₃ h^-1, determined by iodometric and spectrophotometric methods. ^6,23 The on-line O₃ absorbance was measured by UV-visible spectrophotometer (Micronal, B382) using a quartz flow cell (path length 10 mm) at 254 nm. Dye solutions (0.15 L) were ozonized in a cylindrical glass reactor (volume 0.2 L) by bubbling ozone/air mixture into the solution through a sinterized glass filter (pore size 50-80 µm). Due to the small reactor volume, 0.15 L fresh dye solution was used for each reaction time period studied (1 up to 25 min). Excess ozone leaving the reactor was trapped by two sequential bubblers containing KI aqueous solution (2%). After ozonation the samples were purged for 5 min with N₂ to remove residual ozone. All experiments were conducted at room temperature (295 ± 1 K).

Analyses

The optical absorption of dye solutions was determined and recorded by a UV-Vis spectrophotometer (Hewlett Packard 8453) through a 10 mm path length. In order to calculate the kinetics, the concentrations of the dye in solution were determined by its absorbance at maximum absorption wavelengths in the visible (620 nm) and UV (321 nm) regions following standard procedure.²⁴

Organic and inorganic anions and inorganic cations were determined by ion chromatography (Dionex DX500) operated in autosuppression recycle mode and equipped with a conductivity detector, detailed methods are described elsewhere.⁶ Ion chromatography technique (IC) allowed separation and quantification of most important low molecular carboxylic acids (formic, acetic and oxalic), inorganic anions (fluoride, chloride, nitrite, bromide, nitrate, phosphate and sulfate) and cations (sodium, potassium, calcium and magnesium). The detection limits, for all compounds, were < 5 µg L^-1. Chloride ion present as impurity on dye solutions was also determined by Ion Selective Electrode (ISE) using sensing (Orion, Model 96-17B) and double-junction reference (Orion Model 90-02) electrodes following standard procedure.²⁰ Conductivity (Digimed DM-41) and pH (Digimed DM-21) were also determined in some tests.

Due to the possible chloride interference on dye ozonation reaction,^9,11,14,15 some experiments were performed with O₃ and Cl^- solutions, without the presence of Acid Black 1. For theses tests, chloride ion was supplied from either NaCl or HCl solutions (2.8×10^-4 mol L^-1) and its concentration was monitored by IC and ISE techniques.^6,25 Chloride solutions were ozonized, following the procedure described previously, and the UV-Vis spectra were obtained at different reaction times, using 10 and 100 mm path length cells. For comparison, the individual spectra of the sodium hypochlorite and ozone (in 0.25 mol L^-1 H₂SO₄) were obtained in same conditions.

Results and Discussion

Dye purification

Since the efficiency of ozonation might be affected by salt additives and/or dye reagent impurities, preliminary tests were performed to assess dye purity and the presence of possible contaminants on purified and unpurified reagents.

The purity information about dye reagents were obtained from supplier catalog and in the certificates of analysis. For Acros reagent a purity of 63.2% is mentioned while a higher content is indicated to Sigma reagent (> 80%) both on dry basis. However, the measured dye contents for unpurified reagents indicated different values, 61.2 ± 0.5% (moisture 12.1 ± 0.3%) for Acros and 86.6 ± 0.8% (moisture 8.7 ± 0.6%) for Sigma on dry basis. The higher purification level was obtained for Acros reagent with dye purity increasing from 61.2 to 86.3%. Same tests were performed using the purified reagent (Acros ca. 86%).

In Figure 2 the spectra of Acid Black 1 solutions from unpurified Acros and Sigma reagents and purified Acros reagent, prepared in the same conditions (20 mg L^-1, natural pH) is shown. The three spectra presented in this figure are similar in all wavelength range studied (190-800 nm). The obtained data is also in good agreement with literature data.¹ These results indicate that the presence of possible contaminants does not interfere on dye absorption.

The IC and ISE analyses (not shown) indicated that chloride ion is the most important impurity identified on dye reagents (not ozonized). Unpurified Acros and Sigma reagents presented chloride contaminations of 6.8 and 2.0% (m/m on dry basis), respectively. Phosphate ion was also identified at average level ca. 0.5% in both unpurified dye reagents, while other anions (potential identifiable by IC) were not detected. The most abundant cations were found in the following order: Na⁺ >> Ca²⁺ >> K⁺ > Mg²⁺ for unpurified dyes. These results were expected because the probable chloride counter ion is sodium.²² On the other hand, purified Acros dye presents a significant decrease on Ca²⁺ (-98%) and Na⁺ (-42%) contents, while K⁺ and Mg²⁺ levels did not change with the purification process. The inorganic impurities on the Acros reagent correspond to ca. 30% of the dye contamination while organic species, such as starch or other dye synthesis by-products, are responsible for 70% of the impurities.²

Ozonation kinetics

Preliminary tests were performed using the Acros unpurified reagent (61%), for comparison with literature data. In Figure 3 the absorption spectra of Acid Black 1 solution (1.8×10^-5 mol L^-1) during the ozonation process are shown. A quick decrease in absorption band at 620 nm was observed, resulting in a decolorized solution, suggesting a rapid destruction of the dye chromophore structure (-N=N-) directly by ozone. Under these conditions decolorization was completed in 25 min reaction time. On the other hand, the absorbance at 321 nm, wavelength generally attributed to aromatic structures, presented a less intense diminution. These results indicated that chromophore group seems to be less recalcitrant to ozone attack compared to aromatic dye moiety.

Similar results were observed for other dye concentrations studied, prepared with the same dye reagent (Acros 61%). Complete color removal (λ_max 620 nm, A < 0.001) was observed after reaction times of 6 and 11 min for initial dye concentration of the 4.5×10^-6 and 8.9×10^-6 mol L^-1, respectively.

Kinetic parameters were obtained following dye degradation at their maxima visible and UV absorption bands (620 and 321 nm). The reproducibility of these calculations was evaluated by replicate tests and errors were in the range of 4.3-5.0%. According to previous studies the ozonation in a continuous purging mode could be formulated by equation (1), considering only direct oxidation by molecular ozone.^10,13,24 The indirect oxidation by hydroxyl free radicals can be neglected because the low hydroxide ion concentration in solution at pH used (< 5.3).

where [dye] and [O₃] are the concentrations of Acid Black 1 and ozone, and k₀ is the corresponding kinetic rate constant. In addition, ozone concentration in the solution can be assumed to be constant through the continuous ozone supply thus the term k₀[O₃] is constant, therefore the equation (1) can be simplified to,

where k is the overall pseudo-first-order rate constant. Finally, as dye concentration is proportional to absorbance (at specific l), the equation (2) becomes:

In Figure 4 the calculated logarithmic absorption ratio (at λ_max 620 nm) for ozonation at three different initial dye concentrations is shown. These results confirmed pseudo-first order kinetics. Several authors have also reported pseudo first-order kinetics for reactions between different dyes and ozone.^7,8,13,14,22 The similar result was observed at 321 nm (not shown) which suggests the same kinetics behavior, but at lower ozonation rate (four times slower) for aromatic degradation. A summary of the kinetics data, pH and conductivity measurements, obtained during Acid Black 1 ozonation, is presented in Table 1. The inverse relation between the dye concentration and the ozonation rate was observed, in accordance with literature.^4,5,8,20 The decrease of pH was expected, due to the formation of inorganic and organic acids during ozonation, confirmed by a significant conductivity increase, more pronounced for high dye concentrations.

By-products formation

To achieve detailed information on the dye degradation by O₃, complementary studies about ionic by-products generation were performed for ozonized solutions of the unpurified Acros dye reagent. The data presented in Table 2 shows that sulfate and carboxylic acids (formic, oxalic and acetic) were the main oxidation by-products (chloride is also present but as a dye impurity). These species were not observed as dye contaminants (initial concentrations < LD) but were actually formed during dye ozonization in all concentration conditions studied (4.5×10^-6 to 1.8×10^-5 mol L^-1). Nitrite and phosphate (not shown) were also detected but at lower concentrations (< 1 µmol L^-1). Formic acid is the principal organic compound formed, corresponding 40-49% of total identified short chain carboxylic acids. Oxalic acid was the second most abundant acid (34 up to 40%), with acetic acid presenting lower concentrations (0.8-4.5 µmol L^-1). These organic acids correspond to 8-10% of the initial dye concentration expressed in carbon basis.

The molecule of Acid Black 1 also contains six nitrogen atoms in the form of azo (4), amino (1) and nitro (1) groups and two sulfur atoms in the form of sulphonic groups (Figure 1). These heteroatoms react in different ways with ozone due to their specific reactivity and process conditions (O₃ dose, pH etc), being converted in several intermediates and end-products.²² A partial transformation (5-10%) of nitrogen atoms into nitrate and nitrite were observed. The remaining nitrogen atoms could still be in amino form or be converted into nitro-compounds, more recalcitrant to ozone attack. On the other hand, sulfonic groups seem to be easily converted to sulfate with high yields (up to 60%). It is also observed a raise of sulfur conversion with increase of the dye concentration (from 47 to 60%). These preliminary results and the presence of the small organic fragments (carboxylic acids) indicated that the dye structure was not completely mineralized under the prevailing oxidation conditions.

Comparison with other degradation processes

In Table 3 a summary of the literature data about Acid Black 1 degradation processes is shown.^{10,11,13,22-29} Only three works concerning Acid Black 1 ozonation kinetics were found and unfortunately in some studies important experimental conditions were not cited (pH, temperature, O₃ concentration etc). Shu and co-workers^10,13 also obtained pseudo first-order kinetics for unpurified Acid Black 1 ozonation. A rate constant of the 0.45 min^-1 was calculated for a reagent dye concentration of 20 mg L^-1. In these conditions a t_1/2 = 1.6 min was obtained, indicating a faster kinetics compare to our system (t_1/2ca. 3 min). This behavior is probably due to higher ozone doses used by these authors. It is difficult to draw a comparison of these data with results obtained by Muthukumar et al.¹¹ due to different experimental conditions used (basic medium with higher O₃ and dye concentrations).

Only two degradation processes (Table 3) present faster kinetics than ozonation: UV/H₂O₂ (power density 700 W L^-1) and Fenton with t_1/2ca. 0.6 min.^26,27 All other processes have similar or lower kinetic rates compared to O₃ treatment. However, generic conclusion must be made with caution due to the different experimental conditions used in some studies.

Another important aspect is the stated initial Acid Black 1 concentrations in Table 3, which in fact represent the dye reagent concentration. As shown in the present study, very different purities of the Acid Black 1 reagents could be found, 61 and 87% which rate constants of the 0.26 and 0.21 min^-1, respectively. As consequence, significant differences on actual dye concentration are obtained by using the same reagent concentration from different suppliers. For instance, a reagent concentration of 20 mg L^-1 resulting in dye concentrations of the 1.8×10^-5 mol L^-1 (unpurified Acros 61%) and 2.4×10^-5 mol L^-1 (for unpurified Sigma 87%). If a correct dye concentration is not taken into account, kinetics data could be misinterpreA further problem is the role that those reagent impurities (for instance: 13 up to 39% in the dye reagents used in this work) could play on the dye degradation processes. Special attention has been given to the inorganic salts, normally present on dyestuff wastes from dye impurities and/or salt added during textile processing.^15,19 Among these impurities, sodium chloride is a key species due to its wide use on dye synthesis and purification processes.¹⁹ Thus, the dye impurities, especially chloride ions, could be responsible for some discrepancies observed in literature data presented in Table 3.

Influence of chloride ion on dye ozonation

In Table 4 the kinetics data of Acid Black 1 ozonation in presence of the different added chloride concentrations (1.4×10^-6 up to 2.8×10^-2 mol L^-1) is shown. The dye decay always followed pseudo-first-order kinetics no matter the NaCl was involved or not. However, reaction rate significantly decreased (6 up to 42%) with chloride addition. This effect was observed for both purified and unpurified reagent (Figure 5), but in different ways. The most important influence was observed for Acros 86% (-42%) at 5.6×10^-4 mol L^-1 of the added chloride. A less intense, but significant decrease (-35%) on rate variation, was observed for unpurified Acros dye at highest chloride concentration tested (2.8×10^-2 mol L^-1).

These results were not expected because other authors have reported a chloride suppression effect at higher Cl^- concentrations.^9,11,15,16 Muthukumar et al.^11,15 working with concentrated chloride solutions (1.4×10^-1 to 2.6×10^-1 mol L^-1) observed an increasing of ca. 60% on reaction time for complete color removal. Soares et al.⁹ also observed a negative effect in decolorisation of Acid Blue 113 by O₃ in the presence of NaCl (1.4×10^-2 to 1.4×10^-1 mol L^-1) and verified a non linear behavior on color removal by ozone with the addition of higher chloride concentration.

The observed chloride suppression on dye ozonation rate constant is complex and indicates a possible inhibition effect at high Cl^- levels. In Figure 5, logarithmic correlations between k and [Cl^-] are obtained for three studied conditions (Acros 61 and 86%, Sigma 87%). These results sugested that chloride suppression is not a linear effect in our system. A more detailed discussion about this behavior is presented in the next section.

The influence of added salt on ozonation dye kinetics could be related to a simple decreasing of O₃ solubility (salting effect). To test this hypothesis an empirical relation was used to account for ionic strength influence on ozone partition between gas and water phases (Henry constant).²² For higher chloride concentration (2.6×10^-1 mol L^-1), an important reduction on O₃ solubility (16%) was calculated. This fact could in part explain the decrease on dye degradation rate observed by Muthukumar et al.¹¹ On the other hand, for low chloride concentration (< 2.8×10^-2 mol L^-1) an insignificant decrease on ozone solubility was estimated (< 2%). These calculations indicated that salting effects seem to remain marginal in our conditions.

Azevedo et al.¹⁷ suggested that the bromide ion, normally present as a contaminant of NaCl, reacts with O₃ faster then Cl^- generating brominated compounds. However, in the conditions tested the bromide ion was neither identified in dye solutions (LOD < 2 µg L^-1) nor in the NaCl solid reagent (< 0.02%) used. Thus, the influence of chloride on Acid Black 1 degradation should take place from different mechanism, neither related to the presence of bromide nor due to a salting effect.

Reaction between chloride ion and ozone

The possible mechanism explaining the Cl^- suppression effect could be a direct reaction between O₃ and chloride. Yeatts and Taube³⁰ firstly indicated that chlorine can be formed in ozone/chloride solutions in acid media as indicated in reaction A (Table 5). More recent works confirm the second order rate constant for this reaction as well as the catalytic effect of the H⁺.^31-33 Levanov et al.^32,33 proposed the mechanism indicated by reactions B-D for this system. Siddiqui suggested that hypochlorite could react with ozone generating chloride and chlorite ions. In addition, chlorite ion could also react with O₃ and produces chlorate ion by pathway shown in reactions E to G.³⁴

Levanov et al.^32,33 suggested that Cl₂ formation and its release into a gas phase result from a rapidly established equilibrium. Unfortunately it is very difficult to identify chlorine gas in the presence of the ozone, especially at low reactants concentration used. On the other hand, a decrease in the chloride level in ozonized solutions, with a concomitant hypochlorite generation, could be an alternative form to confirm the proposed mechanism.

Our experimental results indicated a significant decrease on Cl^- concentration (-20%) for ozonized hydrochloric acid solutions (2.8×10^-4 mol L^-1 in Cl^-, pH 1) without the presence of dye. As expected, this effect was not observed in sodium chloride solution (2.8×10^-4 mol L^-1 in Cl^-, pH 6) probably due to low [H⁺]. In order to verify the possible formation of the hypochlorous acid (HOCl), UV spectra of these solutions were recorded. For dilute HCl concentration (< 0.1 mol L^-1) only the peaks of ozone (254 nm) and chloride (ca. 200 nm) were detected. However, on increasing HCl concentration up to 0.5 mol L^-1, a new peak around 230 nm appears, while ozone peak (254 nm) is no longer observed (Figure 6). This new peak is close to the HOCl λ_max (230 nm) one, as could be observed in the spectrum obtained from a NaOCl acidic solution (in 0.25 mol L^-1 H₂SO₄) also shown in Figure 6.

Similar behavior was observed by Vinals et al.³⁵ studying the influence of chloride ion on the ozone assisted leaching of gold and palladium from metallic scraps. These authors verified the presence of a peak around 230 nm and attributed to the presence of HOCl, for chloride concentration up to 0.5 mol L^-1.

It is possible that hypochlorous acid formation could also take place in slight acid solutions (pH 4) and at low O₃ and chloride concentrations, such as the ones used in this study. If true, the direct reaction between O₃ and chloride could compete with dye ozonation and explain, at least in part, the observed Cl^- suppression effect on Acid Black 1 degradation. However, the global mechanism is probably more complex than that considered in this work. The presence of dye could directly influence the chloride reaction with ozone and their by-products also could interact among them, generating different products. Thus, for a best elucidation of the involved mechanism and to a precise estimation of chloride suppression effect further tests must be performed using more sensitive analytical techniques, free of interference.

Conclusions

Experimental results show that ozonation of Acid Black 1 solutions is very efficient in the destruction of the dye chromophore structures. Ozonation treatment leads to a complete decolorization of the dye solution (1.8×10^-5 mol L^-1) in few minutes (< 25 min). In addition, the aromatic structures are also attacked but at slower rates. Pseudo first-order rate kinetics were obtained, with an inverse relation between initial dye concentration and rate constant.

The ozonized unpurifed dye solutions showed the presence of short chains carboxylic acids (formic, oxalic and acetic) and inorganic anions (sulfate, nitrate and nitrite) as degradation by-products. The calculated conversions on molar ratios suggest that dye structure was not completely mineralized under used conditions.

The dye purity is a very important parameter not just to state the real dye concentration but also to indicate the presence of impurities which could be reactive towards O₃. The main identified contaminant (chloride ion) affects significantly the dye ozonation kinetics. Interference studies indicated that rate constants decrease up to 42% in the presence of 5.6×10^-4 mol L^-1 added chloride. However, the presence of other impurities could also interfere in the dye degradation. The mechanism of the chloride suppression effect seems to involve a direct reaction between O₃ and Cl^- generating HOCl, among other by-products.

Acknowledgments

The authors thank FAPERGS and CNPq for financial support.

References

1. Green, F. J.; The Sigma-Aldrich Handbook of Stains, Dyes and Indicators, Aldrich Chemical Co.: Milwaukee, Wisconsin, 1991.

2. Borrós, S.; Barbera, G.; Biada, J.; Agulló, N.; Dyes Pigm. 1999, 43, 189.

3. Carneiro, P. A.; Boralle, N.; Stradiotto, N. R.; Furlan, M.; Zanoni, M. V. B.; J. Braz. Chem. Soc. 2004, 15, 587.

4. Catanho, M.; Malpass, G. R. P.; Motheo, A. J.; Quim. Nova. 2006, 29, 983.

5. Almeida Filho, C.; Zarbin, J. G.; J. Braz. Chem. Soc. 2006, 17, 1151.

6. Martins, A. O.; Canalli, V. M.; Azevedo, C. M. N.; Pires, M.; Dyes Pigm. 2006, 68, 227.

7. Alaton, I. A.; Balcioglu, I. A.; Bahnemann, D. W.; Water Res. 2002, 36, 1143.

8. Sarayu, K.; Swaminathan, K.; Sandhya, S.; Dyes Pigm. 2007, 75, 362.

9. Soares, O. S. G. P.; Órfão, J. J. M.; Portela, D.; Vieira, A.; Pereira, M. F. R.; J. Harzard. Mater. B. 2006, 137, 1664.

10. Shu H. Y; Chang M. C.; Dyes Pigm. 2005, 65, 25.

11. Muthukumar, M.; Sargunamani, D.; Selvakumar, N.; Nedumaran, D.; Indian J. Chem. Technol. 2004, 11, 612.

12. Tosik R.; Wiktorowski, S.; Ozone Sci. Eng. 2001, 23, 295.

13. Shu H. Y.; Huang C. R.; Chemosphere 1995, 31, 3813.

14. Zhang, F. F.; Yediler, A.; Liang, X. M.; Kettrup, A.; Dyes Pigm. 2004, 60, 1.

15. Muthukumar, M.; Selvakumar, N.; Dyes Pigm. 2004, 62, 221.

16. Chu, W.; Lau, T. K.; J. Hazard. Mater. 2007, 144, 249.

17. Azevedo, E. B.; Neto, F. R. D.; Dezotti, M.; J. Hazard. Mater. 2006, 128, 182.

18. Dong, Y.; Chen, J.; Li, C.; Zhu H.; Dyes Pigm. 2007, 73, 261.

19. Gahr, F.; Hermanutz F.; Oppermann W.; Water Sci. Technol. 1994, 30, 255.

20. Gunten U.; Water Res. 2003, 37, 1469.

21. Lyon, H. O.; Biotechnic Histochem. 2002, 77, 57.

22. Lankin, A. L.; Chem. Ind. 1970, 38, 1227.

23. Standard Methods for the Examination of Water and Wastewater - APHA, 20^th ed.; American Public Health Association/American Water Works Association/Water Environment Federation, Washington DC, 1998.

24. Langlais, B.; Reckhow, D. A.; Brink, D. R.; Ozone in Water Treatment Applications and Engineering, AWWARF and Lewis Publishers, Inc.: Denver, 1991.

25. Evans, A.; Potentiometry and Ion Selective Electrodes, J. Wiley:, London, 1991.

26. Shu, H. Y.; Chang, M. C.; Fan, H. J.; J. Hazard. Mater. 2004, 113, 201.

27. Wang, S.; Dyes Pigm. 2008, 76, 714.

28. Yip, A. C. K.; Lam, F. L. Y.; Hu, X.; Chem. Eng. Sci. 2007, 62, 5150.

29. Grzechulska, J.; Morawski, A. W.; Appl. Catal. B - Environ. 2002, 36, 45.

30. Yeatts, L. R. B.; Taube, H.; J. Am. Chem. Soc. 1949, 71, 4100.

31. Hoigne, J.; Bader, H.; Haag, W. R.; Staehelin, J.; Water Res. 1985, 19, 993.

32. Levanov, A. V.; Kuskov, I. V.; Zosimov, A. V.; Antipenko, E. E.; Lunin, V. V.; Kin. Catal. 2003, 44, 740.

33. Levanov, A. V.; Kuskov, I. V.; Koiaidarova, K. B.; Zosimov, A. V.; Antipenko, E. E.; Lunin, V. V.; Kin. Catal. 2005, 46, 147.

34. Siddiqui, M.; Water Res. 1996, 30, 2160.

35. Vinals, J.; Juan, E.; Ruiz ,M.; Ferrando, E.; Cruells, M.; Roca, A.; Casadao, J.; Hydrometal. 2006, 81, 142.

Received: July 17, 2009

Web Release Date: December 3, 2009

Publication Dates

• Publication in this collection
  06 May 2010
• Date of issue
  2010

History

• Received
  17 July 2009
• Accepted
  03 Dec 2009