ABSTRACT
FEI, XIUZHU. Towards Closed Loop Recycling of Polyester Fabric. (Under the direction of Dr. Harold S. Freeman and Dr. David Hinks).
Polyethylene terephthalate (PET) is extensively used in various types of apparel, home textiles, and outdoor products that are regularly placed in landfills after use. But unlike natural fibers,
PET is not readily biodegradable. In view of sustainability, research regarding the recycling of textiles derived from PET fibers is of interest, and effective color removal has been recognized as a crucial step towards recycling of colored PET fabrics. To this end, a decolorization process was developed using sodium formaldehyde sulfoxylate (SFS) as the reducing agent. Disperse dye decolorization studies were conducted in water and acetone media, and an optimized combination of treatment time (30 min), water to acetone ratio (1:2),
SFS concentration (10g/L), temperature (100oC), and liquor ratio (1:50) was found effective for decolorizing various commercial disperse dyes as well as basic dyes. Results in terms of intrinsic viscosity of decolorized PET showed that the optimized SFS decolorization method has no significant effect on fiber strength.
The goal of this work was to study the recyclability of bath and fabric after decolorization, investigate the ecotoxicity of the decolorization process, study the life cycle assessment of the closed-loop recycling process, characterize dyes from commercial fabrics and study their decolorization properties.
Fabric decolorization using the optimized SFS method followed by re-dyeing using Disperse
Yellow 42, Disperse Orange 30, Disperse Red 60, and Disperse Blue 79 was conducted on cationic dyeable PET. It was found that fabrics containing nitro and anthraquinone dyes,
Disperse Yellow 42 and Disperse Red 60, respectively, have better decolorization efficiency than those containing azo Disperse Orange 30 and Disperse Blue 79 dyed fabrics.
Bearing in mind that ecotoxicity testing is of increasing importance in the screening of newly developed substances or treatment processes, solutions of six high volume disperse dyes and one basic dye were decolorized using SFS, and the resultant solutions were tested with
Daphnia similis and Parhyale hawaiensis to observe the acute toxicity to the two species. The control sample, which is the SFS solution without dyes, showed that EC50 to Daphnia similis is 1.83%, and LC50 to Parhyale hawaiensis is 9.0%. EC50 and LC50 were expressed in percentage of dye solution. Decolorized dye solutions differed in the toxicity, however, the differences were not significant. The toxicity observed in the acute tests is probably mainly related to SFS decolorization medium. Converting EC50 and LC50 of decolorized solution to equivalent concentration, the effluents were considered relatively harmful to Daphnia similis.
Control SFS solution and decolorized Disperse Blue 56 were moderately toxic to Parhyale hawaiensis, whereas decolorized Disperse Orange 30 was relatively nontoxic to Parhyale hawaiensis.
A closed loop recycling of PET fabric was proposed beginning with collection of post- consumer PET fabrics/garments, followed by chemical decolorization, mechanical reprocessing, and ending with production of recycled PET fibers. A life cycle assessment was conducted to compare the innovative closed loop recycling process and virgin PET production process. Results suggest that recycled PET production has less environmental impacts than the virgin system in six categories, namely, exotoxicity, eutrophication, human health- carcinogenics, human health-non-carcinogenics, ozone depletion, and respiratory effects, but
also shows higher impact results in four categories, which are acidification potential, global warming potential, photochemical ozone formation potential, and fossil fuels resource depletion. Contribution analysis shows higher impacts in those four categories result from the consumption of acetone. Sensitivity analysis also shows that overall impact is sensitive to acetone consumption, which means environmental benefits of the recycling method are highly dependent on the acetone consumptions. This life cycle assessment is conducted based on a hypothetical closed-loop scenario. Further work on obtaining specific data in innovative recycling processing for more reliable analysis would be beneficial.
© Copyright 2018 by Xiuzhu Fei
All Rights Reserve Towards Closed Loop Recycling of Polyester Fabric
by Xiuzhu Fei
A dissertation submitted to the Graduate Faculty of North Carolina State University in partial fulfillment of the requirements for the degree of Doctor of Philosophy
Fiber and Polymer Science
Raleigh, North Carolina
2018
APPROVED BY:
______Dr. David Hinks Dr. Harold S Freeman Co-chair of Advisory Committee Co-chair of Advisory Committee
______Dr. Nelson Vinueza Dr. Joseph DeCarolis ii
DEDICATION
I dedicate my dissertation work to Dr. Harold S. Freeman and Dr. David Hinks for their guidance and support over the years.
I also dedicate this work to my parents, my sister, brother in law, and my beloved, Ju Dong.
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BIOGRAPHY
Xiuzhu Fei was born in Shaoxing, Zhejiang Province of China in 1991. Shaoxing is a medium size city that relied heavily on textile industry 15 years ago. Many of her relatives were working for textile companies. However, due to the increasing regulations and restrictions, the traditional labor-intensive textile plants and mills lost their competitiveness in recent years.
She chose the Dyeing and Finishing Engineering as her major in Jiangnan University, because she wanted to learn more about textiles and bring some benefits to her hometown. Later she was enrolled to North Carolina State University in August 2013 as a master student majoring in Textile Chemistry. Afterwards she was enrolled in the Fiber and Polymer Science Program to pursue a PhD degree. She believes sustainable textiles are the future of the textile world.
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ACKNOWLEDGMENTS
Writing this note of thanks is the finishing touch on my dissertation. It has been several years of learning in North Carolina State University, Raleigh, not only in the scientific area, but also on a personal level. I would like to express my sincere acknowledgements to the people who have supported and helped me so much throughout this period.
I would first like to thank Dr. David Hinks for founding me throughout my research career. I have never imaged I could study abroad before I received an offer letter from Dr. Hinks 5 years ago. I am deeply grateful for the opportunity. He covered me all the time so I could focus on the research. Without his support, this PhD work would not have been achievable.
My greatest appreciation goes to Dr. Harold S. Freeman for all the guidance, instruction and encouragement he gave me during the time I spent at the NC State. He is a very patient and responsible professor. I will always keep every piece of hand-written feedback he gave to me about my thesis and manuscripts. He pointed me to the right direction so that I can successfully complete my dissertation. He is also a considerate person which inspires me a lot in my personality.
I would also like to thanks Dr. Nelson Vinueza and Dr. Joseph DeCarolis for their excellent cooperation as kindly being my committee members. I sincerely appreciate the helpful suggestions and comments I received from them.
A very special thanks to previous and current group members in Dr. Hinks’s and Dr. Freeman’s research group, especially Dr. Malgorzata Szymczyk, for their help in the lab work and for their companionship in my life. v
Finally, many thanks go to my parents, sister and brother in law, for believing in me and supporting me all the time; to all my dear friends for bringing me happiness and joy; and to my dear boyfriend Ju, for his selfless love.
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TABLE OF CONTENTS
LIST OF TABLES ...... x
LIST OF FIGURES ...... xii
1. INTRODUCTION ...... 1
2. LITERATURE REVIEW ...... 3
2.1 Polyethylene terephthalate ...... 3
2.1.1 Introduction to polyethylene terephthalate ...... 3
2.1.2 Properties of polyesters ...... 5
2.2 Coloration of polyester ...... 7
2.2.1 Disperse dyes ...... 8
2.2.2 Basic dyes ...... 14
2.3 Dye characterization ...... 16
2.3.1 Ultraviolet-visible spectroscopy ...... 16
2.3.2 Chromatography ...... 17
2.3.3 Mass spectrometry ...... 18
2.4 Toxicity ...... 19
2.7.1 Dye structure property relationships ...... 20
2.4.2 Methods used ...... 25
2.5 Decolorization treatment ...... 29
2.5.1 Wastewater decolorization treatment ...... 29
2.5.2 Decolorization of textiles ...... 37
2.6 Recycling method ...... 40
2.6.1 Conventional polymer recycling ...... 41
2.6.2 Fabric reuse ...... 42 vii
2.7 Preliminary study - development of SFS decolorization method ...... 45
2.7.1 Effect of treatment conditions on fabric decolorization ...... 48
2.7.2 Fabric strength assessment ...... 57
2.7.3 Conclusions from preliminary study...... 58
3. PRESENT RESEARCH ...... 59
3.1 Objectives ...... 59
3.2 Rational ...... 59
4. REUSE OF DECOLORIZATION BATH AND DECOLORIZED FABRICS ...... 61
4.1 Introduction ...... 61
4.2 Experimental ...... 64
4.2.1 Material ...... 64
4.2.2 Batch fraction distillation ...... 65
4.2.3 Application of disperse dyes to decolorized fabrics ...... 65
4.2.4 Decolorization of laboratory-dyed fabrics using acetone distillate ...... 66
4.2.5 Color evaluation ...... 66
4.2.6 Fabric strength evaluation ...... 67
4.3 Results and discussion ...... 67
4.3.1 Solvent recovery and reuse ...... 67
4.3.2 Re-dyeing decolorized cationic dyeable PET ...... 68
4.3.3 Burst pressure measurement ...... 74
4.4 Conclusion ...... 74
5. THE ECOTOXICITY OF SODIUM FORMALDEHYDE SULFOXYLATE DECOLORIZATION MEDIUM ...... 75
5.1 Introduction ...... 75
5.2 Experiment ...... 80 viii
5.2.1 Materials and organisms ...... 80
5.2.2 Decolorization of commercial dyes ...... 80
5.2.3 Ecotoxicity testing ...... 81
5.3 Results ...... 81
5.3.1 SFS decolorization of commercial dyes...... 81
5.3.2 Daphnia similis test ...... 85
5.3.3 Parhyale hawaiensis test ...... 88
5.4 Conclusion ...... 91
6. LIFE CYCLE ASSESSMENT OF CLOSED-LOOP RECYCLING OF PET FABRICS ...... 92
6.1 Goal and scope ...... 92
6.2 Introduction ...... 93
6.3 Methodology ...... 95
6.3.1 Goal and scope, functional unit and system boundary ...... 95
6.3.2 Data collections and assumptions ...... 98
6.3.3 Weight and normalization ...... 100
6.4 Closed-loop recycling of polyester fabric ...... 103
6.5 Life-cycle assessment results ...... 104
6.5.1 Comparative analysis ...... 104
6.5.2 Contribution analysis ...... 106
6.6 Sensitivity and uncertainty analysis ...... 109
6.7 Conclusion ...... 111
7. COMMERCIAL BLACK DYE COMPOSITION AND THEIR DECOLORIZATION PROPERTIES ON POLYESTER FABRIC ...... 112
7.1 Introduction ...... 112 ix
7.2 Experimental ...... 114
7.2.1 Materials ...... 114
7.2.2 Decolorization of commercial black fabrics ...... 115
7.2.3 Fabric color evaluation...... 115
7.2.4 Chemical analysis ...... 115
7.2.5 Preparation of disperse dyes ...... 117
7.2.6 Decolorization of commercial dye solutions ...... 119
7.3 Results and discussion ...... 119
7.3.1 Analytical results ...... 119
7.3.2 Comparison with synthesized disperse dyes ...... 128
7.3.2 Decolorization results ...... 130
7.4 Conclusion ...... 134
8. FUTURE WORK ...... 135
9. REFERENCES...... 138
10. APPENDIX ...... 157
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LIST OF TABLES
Table 1. Relationship between polyester molecular weight and spinnability 3...... 5
Table 2. Abrasion resistance of polyester and other synthetic fibers...... 7
Table 5. Absorption of visible light and color seen ...... 16
Table 6. Disperse dyes considered a health risk to consumers...... 21
Table 7. Interpretation of LC50 values...... 27
Table 6. K/S values of commercial PET fabrics before and after SFS (40g/L) treatment in acetone/water (1:1) at 100°C...... 47
Table 7. Intrinsic viscosity (IV) Vs viscosity-average molecular weight for control PET fabric and PET fabric after SFS (40g/L) treatment in acetone/water (1:1) at 100 ˚C...... 57
Table 8. C.I. names, classes, and structures of dyes used in this study...... 64
Table 9. Acetone recovery percentage from lab-scale fractional distillation...... 67
Table 10. K/S values from lab-dyed cationic dyeable PET fabrics using virgin and recovered acetone for SFS (40g/L) decolorization in water/acetone (1:2) at 100 °C...... 68
Table 11. Color difference values of cationic dyeable PET fabrics between once decolorized fabrics and virgin white fabrics dyed by corresponding original colors...... 69
Table 12. Color difference values of cationic dyeable PET fabrics between twice decolorized fabrics and virgin white fabrics dyed by corresponding original colors...... 71
Table 13. Color difference values of cationic dyeable PET fabrics between three-time decolorized fabrics and virgin white fabrics dyed by Disperse Yellow 42...... 73
Table 14. C.I. names, classes, and structures of dyes used in this study...... 79
Table 15. EC50 (%) values of SFS decolorized solution tested with Daphnia similis...... 87
Table 16. Global harmonized system criteria for classification of a substance in acute categories ...... 88
Table 17. LC50 (%) values of decolorized solutions tested with Parhyale hawaiensis...... 89 xi
Table 18. Physico-chemical parameters of Parhyale hawaiensis acute toxicity test...... 89
Table 19. Globally harmonized system criteria for classification of hazardous to the aquatic environment...... 91
Table 20. Basis of the comparative life cycle assessment study...... 97
Table 21. Data source of this study...... 101
Table 22. Impact categories and TRACI normalization factors (US 2008) used in LCA analysis ...... 102
Table 23. Normalized LCA results for producing 1 metric ton of PET fiber by virgin and recycled fiber production methods...... 105
Table 24. Processes contributing to acidification potential in recycled PET fiber production ...... 107
Table 25. Processes contributing to acidification potential in virgin PET fiber production ...... 107
Table 26. Retention time, area, and percentage area of peaks ...... 122
Table 27. Identification of disperse dyes...... 125
Table 28. H-NMR spectral results of the Orange, Blue1 and Red dyes...... 128
Table 29. K/S values and WI of commercial black fabrics before and after SFS (10g/L) treatment in acetone/water (2:1) at 100°C...... 131 xii
LIST OF FIGURES
Figure 1. Simplified two-step PET manufacturing process...... 4
Figure 2. Structure of cationic dyeable polyester...... 5
Figure 3. Structures of various chromophores...... 9
Figure 4. General structure of aminoazobenzene disperse dye...... 10
Figure 5. Disperse dye structure based on aminoazobenzene...... 11
Figure 6. Structural skeleton of most anthraquinone disperse dyes...... 12
Figure 7. Disperse dye structure based on anthraquinone...... 13
Figure 8. Chemical structure of two heterocyclic disperse dyes...... 14
Figure 9. Colorless compound liberated from reaction of basic dye with alkali...... 15
Figure 10. Structure and color index specification of some basic dyes...... 15
Figure 11. Chemical structures of some bladder carcinogens...... 20
Figure 12. Chemical structure of 6BT and 4PhDAB...... 23
Figure 13. Electrophilic nitrenium ion from amino-containing compounds...... 24
Figure 14. Carcinogenic CI Disperse Orange 11 and CI Disperse Blue 1, and mutagenic CI Disperse Violet 1...... 24
Figure 15. Metabolic pathway for polycyclic aromatic hydrocarbons...... 25
Figure 30. Proposed initial pathway for degradation of commercial DR1 dye by photo- Fenton oxidation35...... 28
Figure 17. Production of reactive species in hydrogen peroxide (1), ...... 31
Figure 18. Proposed degradation pathway for the dye RB 171 by ozonation53...... 33
Figure 19. Chemical structures of some important reducing agent...... 34
Figure 20. Reductive degradation of azo dye under anaerobic condition...... 35
Figure 21. General overview of the fate of azo dyes during anaerobic-aerobic treatment. .. 36
Figure 22. Reduction of aromatic aldehyde to alcohol by SFS in aqueous media72...... 39 xiii
Figure 23. Reductive dehalogenation of phenacyl halide in ethanol medium by SFS...... 40
Figure 24. SFS decomposition reaction upon heated...... 40
Figure 25. Preparation of benzothiazole from BHET (a) and synthesis of dyes (b)81...... 44
Figure 26. Color photographs of polyester fabric dyed with synthesized dyes...... 45
Figure 27. Changes in the UV-visible spectrum of (A) Disperse Blue 56, (B) Disperse Orange 30, (C) Disperse Yellow 42, and (D) Basic Yellow 28 after SFS (25g/L) treatment in water/acetone (1:1) medium...... 46
Figure 28. Commercial PET fabrics before and after SFS (40g/L) treatment in acetone/water (1:1) at 100°C...... 48
Figure 29. Effect of (a) treatment time, (b) water to acetone ratio, (c) SFS concentration, (d) Temperature, and (e) liquor ratio on K/S value of black commercial fabrics after decolorization...... 54
Figure 30. Visualized effect of (a) treatment time, (b) water to acetone ratio, (c) SFS concentration, (d) Temperature, and (e) liquor ratio on K/S value of black commercial fabrics after decolorization...... 55
Figure 31. Diagram of experimental device for lab-scale fractional distillation. (1) Digital hot plate, (2) round-bottom flask, (3) condenser used as fractionating column, (4) two-way adapter, and (5) condenser...... 65
Figure 32. Cationic dyeable PET fabrics showing the color difference between virgin (left) and once decolorized fabrics (right) after dyeing in the same bath. (a) Disperse Red 60, (b) Disperse Orange 30, (c) Disperse Yellow 42, and (d) Disperse Blue 79...... 70
Figure 33. Cationic dyeable PET fabrics showing the color difference between virgin (left) and twice decolorized fabrics (right) after standard dyeing in same bath...... 71
Figure 34. Disperse Yellow 42 on three-time decolorized cationic dyeable PET fabrics originally dyed by (1) virgin-standard, (2) Disperse Yellow 42, (3) Disperse Orange 30, (4) Disperse Red 60, and (5) Disperse Blue 79...... 73
Figure 35. Preparation of sodium formaldehyde sulfoxylate through (1) reaction of formaldehyde with dithionite, and (2) reaction of bisulfite and formaldehyde with zinc...... 75
Figure 36. Reduction of aromatic aldehyde to alcohol by SFS in aqueous media72...... 76
Figure 37. Reductive dehalogenation of phenacyl halide in ethanol medium by SFS...... 77 xiv
Figure 38. SFS decomposition reaction upon heated...... 78
Figure 39. UV-Vis absorption spectra of commercial dyes (100mg/L) and SFS decolorized (SFS=10g/L, 95 °C, 45min) solutions...... 83
Figure 40. Comparison of decolorization percentage after SFS decolorizaton treatment (10g/L, 95 °C, 45min)...... 85
Figure 41. EC50 (%) values and confident intervals of SFS decolorized solution tested with Daphnia similis...... 87
Figure 42. LC50 (%) values and confident intervals of SFS decolorized solutions tested with Parhyale hawaiensis...... 90
Figure 43. Cradle-to-gate system boundaries of virgin PET fiber production system (left), and recycling PET fibers from waste PET textile products (right)...... 98
Figure 44. The closed-loop recycling process...... 104
Figure 45. Comparison of environmental impacts for producing 1 metric ton of PET fiber by virgin (Black) and recycled (Red) fiber production system using TRACI method...... 106
Figure 46. Sensitivity of the acetone consumption to acidification, global warming, photochemical ozone formation, and resource depletion...... 110
Figure 47. Disperse Black 9 formation inside textiles...... 113
Figure 48. TLC analysis of black fabric extract using chloroform: acetone (19:1)...... 120
Figure 49. UV-vis spectra of orange, blue1, red and blue2 fractions in chloroform/acetone (19/1, v/v) obtained by UV-vis spectroscopy...... 120
Figure 50. Chromatographic separation of the sample extracted from commercial black fabric at 515 nm...... 122
Figure 51. UV-vis spectra obtained by photodiode array detection of peak 1 obtained at 3.167 min, peak 2 at 3.383 min, peak 3 at 4.133 min, and peak 4 at 5.483 min...... 123
Figure 52. High resolution mass spectra and possible structures characterizing commercial black dye components (Orange, Blue, and Red Dye)...... 126
Figure 53. High-resolution mass spectrum of synthesized orange disperse dye...... 129
Figure 54. High-resolution mass spectrum of synthesized blue disperse dye...... 129 xv
Figure 55. TLC chromatogram compassion of A: black fabric extraction; B: synthesized orange disperse dye; and C: synthesized blue disperse dye using hexane/ethyl acetate (1/20)...... 130
Figure 56. Commercial black fabric before and after SFS (10g/L) treatment in water/acetone (1:2) at 100 ˚C for 30 min...... 131
Figure 57. Commercial disperse dye solution of SFS (10g/L) treatment in water/acetone (1:2) at 100 ˚C in different treatment times: A=0 min, B=5 min, C= 10 min and D=15 min...... 133
Figure 58. Absorption spectra changes during the SFS decolorization ([SFS] =10g/L, water/acetone=1/2, 100 ˚C) of black dye mixture solution...... 133
Figure 60. SEM pictures of SFS decolorized polyester fabrics...... 136
Figure 61. Microscopic pictures of (a) blue fiber and (b) decolorized blue fiber...... 137
Figure 62. Full 1H-NMR spectrum of synthesized orange disperse dye...... 158
Figure 63. Full 1H-NMR spectrum of synthesized blue disperse dye...... 159 1
1. INTRODUCTION
Polyethylene terephthalate (PET) fiber, commonly known as polyester fiber, has become the fiber of choice within textile industry due to its unique set of advantages. The overall demand for polyester fiber is increasing year-by-year. The low price of the virgin polyester fiber accounts significantly for this growing trend. One major application of polyester fiber is the production of fabrics, which are extensively used in all kinds of apparel, home furnishings, and other finished textile goods that are regularly disposed and ended in landfills. However, disposing PET products in landfills creates significant environmental issues, because of the durability of the polymer involved. In addition, the manufacture of PET is an energy-intensive process requiring large amounts of crude oil. One-time use of PET fabric is regarded as a waste of valuable polymer derived from non-renewable petroleum resources. Efforts have been devoted to recycle PET beverage bottles and liquid containers. However, methods that have been developed to recycle PET bottles are not applicable to recycle PET fabrics due to the presence of dyes.
Removing dyes from textile wastewater has been widely studied in recent years. Physical methods, including adsorption and membrane filtration, chemical methods, such as bleaching and ozonation, and biological methods have been reported. However, there is no systematic study on removing dyes from fabric in order to achieve fabric recycling. Bearing this in mind, an innovative approach is proposed in this work to decolorize dyes from fabrics.
This project will achieve the following objectives:
(1) Develop an efficient decolorization method for removing dyes from PET fabrics.
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(2) Determine the scope of disperse dyes that can be removed by the decolorization
method.
(3) Study the recyclability of the decolorized fabric.
(4) Study the ecotoxicity of the decolorization process.
(5) Understand the Life Cycle Assessment (LCA) of the recycling process.
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2. LITERATURE REVIEW
2.1 Polyethylene terephthalate
2.1.1 Introduction to polyethylene terephthalate
Polyethylene terephthalate, commonly abbreviated PET, is the most common form of polyester used commercially. PET has wide range of applications. It is spun into fibers for the production of fabric, blow-molded into disposable beverage bottles, and extruded into photographic film and magnetic recording tape. The history of polyester fiber dates back to the early 1940s when British scientists Whinfiled and Dickson firstly synthesized PET from a combination of terephthalic acid and ethylene glycol and found it was well suited for forming fiber. The first marketed polyester fiber was patented as Terylene by Imperial Chemical
Industries Ltd, and later DuPont manufactured another polyester fiber using modified nylon technology, which they named Dacron. Subsequent to the development of Terylene and
Dacron, a whole range of trademarked products as Kodel and Mylar were rapidly produced during 1960s and 1970s 1.
When carboxylic groups from terephthalic acid react with OH groups from ethylene glycol, esterification occurs at the ends of the bifunctional compounds and PETs with a liner structure are produced2. In large-scale practice, a two-step process, transesterification followed by polycondensation reaction using dimethyl terephthalate and excess ethylene glycol with the aid of catalysts, has achieved some importance on a production basis. This manufacturing process is based on the original patent of Whinfield and Dickosn. Figure 1 shows the linear structure of PET and the simplified two-step reaction process.
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Figure 1. Simplified two-step PET manufacturing process.
According to Carothers, the pioneer of thermoplastic polyesters, PET used in the production of fibers must possess a certain molecular weight range and must be capable of orientation when stretched. Table 1 gives the results achieved by Carothers and Van Natta3 in their investigation of the relationship between the molecular weight of polyester and its fiber formation including spinnability. Observations obtained by Meehan 4 are consistent with this results. In general, polyester with a number average molecular weight of 15,000 ~ 20,000 shows good spinnability, as well as other mechanical properties.
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Table 1. Relationship between polyester molecular weight and spinnability 3.
Molecular weight Spinnability Extensibility Fiber Strength (number average) (kg/mm2) 780 None N/A N/A 4,170 None N/A N/A 5,670 Short fibers None N/A 7,330 Long fibers None Minute 9,330 Long fibers Possible Minute 16,900 Good Good 13.1 20,700 Difficult Good 12.3
Apart from the conventional polyester fiber, there are cationic dyeable polyesters (CDP) that also became popular. CDP is a special polyester having anionic sites in the main chain5. The schematic structure of CDP is shown in Figure 2. It is worth mentioning that in a CDP polymer chain, the number of sections containing anionic sites are much less than the number of normal ester sections.
Figure 2. Structure of cationic dyeable polyester.
2.1.2 Properties of polyesters
Many new synthetic fibers have been developed within the last decades, including rayon, acetate, spandex, etc., but it is still hard to claim that polyester has been replaced by other fibers
6 in the textile market. In fact, in 2014, world production of polyester reached 46.1 million tons, which is greater than production of all the other synthetic fibers6. Distinguished properties of
PET take credit for its success. The presence of aromatic rings in the main chain gives PET notable stiffness and strength. When heated above its glass-transition temperature, PET turns from a rigid glass-like form into a rubbery elastic state, where the polymer molecular chain can be stretched and aligned in one direction to form polyester fibers7. Polyester fibers exhibit high elastic modulus, which indicates that polyester fibers possess superb elastic recovery8.
This capacity of recovering rapidly imparts polyester fibers with excellent crease resistance and very good dimensional stability. When used in textiles, PET also has many other attractive properties, like good abrasion and heat resistance9. Abrasion is an undesirable but inevitable effect of exposure to normal use. The abrasion of resistance of PET fiber is not as excellent as polyamide fibers, but almost equals to or surpasses the values of viscose and acetate fibers10.
Table 2 presents a comparison. Good thermal stability of PET is attributed to the presence of aromatic phenyl groups as well. The recorded glass transition temperature (Tg) ranges from
11 67 to 81 °C, and the experimental melting temperature (Tm) is between 255-260 °C .
Therefore, polyester textile products can withstand treatment at 170-180 °C without any damages. Polyester fibers exhibit good resistance to combustion and flammability. When a polyester fiber is contacted with a flame, the end of the fiber will contract and melt with formation of a droplet or a pill that is difficult to ignite12. It is interesting that when polyesters are blended with other readily flammable fibers that promote combustion, such as cotton, they become flammable as well and will continue to burn together with the other fibers12. In addition, polyester shows good resistance to atmospheric and biological agents13, due to the orientation and high crystallinity of polyester fibers. In accordance with the chemical structure
7 of PET, the ester linkages should undergo hydrolysis attacked by acids and alkalis. However, polyester fiber shows chemical resistance better than expected. Because the attack of these chemical agents is limited essentially to the surface, since water-soluble acids and alkalis cannot diffuse insider the nonpolar polymer phase. For the same reason, polyester fibers show an outstanding resistance to oxidants and reducing agents. CDP, the modified polyester, possesses similar properties with fibers of normal PET. However, the meta substitution in the anionic section increases segmental mobility, resulting in lower glass transition temperature and lower thermal stability of the CDP14. Also the CDP is more readily hydrolyzed.
Table 2. Abrasion resistance of polyester and other synthetic fibers.
Type of fiber Number of rubs up to breaking point Dry Wet Polyester 1980 1870 Polyamide 8800 3890 Polyacrylonitrile 135 139 Viscose 880 28 Acetate 409 58
2.2 Coloration of polyester
Due to the lack of water solubilizing group in polymer chain, polyester has limited affinity, especially at low temperatures, towards most of the water-soluble dyes, such as reactive and acid dyes15. Hence, polyester requires the use of disperse dyes, which are non-ionic chemicals with sparing solubility in water. Upon dyeing of polyesters, disperse dye particles are dissolved in the fiber material. A diffusion equilibrium is established between fiber and liquor until saturation concentration is attained16,17. However, due to the hydrophobicity and the
8 compact structure of polyester fibers, only pale to medium shades can be obtained under atmospheric conditions. For darker shades it is necessary to employ various carriers or raise dyeing temperature to increase the disperse dye diffusion. Cationic dyeable polyester fibers is a special polyester fiber that can be dyed with both disperse dye and cationic dye.
2.2.1 Disperse dyes
The name of disperse dye was derived for its sparing water-soluble properties and the need to apply it from a fine aqueous dispersion. Dyes are transferred in the molecular state from bath to fiber through a process of surface adsorption and diffusion. For the sake of efficient diffusion inside the fiber, disperse dye particles should be as small as possible, typically ranging from 0.5-2.0 micron, which necessitated designing disperse dye comprising low molecular weight in the range of 250-60015. Based on their unique sublimation fastness and dyeing properties, disperse dyes can be classified into four categories, named A to D. In dyes
A to D, the molecular weight increases along with the sublimation fastness, whereas ease of dyeing decreases18. Category A contains dyes that have excellent dyeing properties due to their molecular size but poor sublimation fastness. These dyes usually find use on acetate and nylon fiber. Category B dyes possess excellent carrier-dyeing behavior and moderate sublimation fastness. These dyes are suitable for the dyeing of texturized polyester fabric and yarn, on which they can provide a degree of heat fastness adequate for the mild heat setting treatments used on these materials. Dyes in category C have higher sublimation fastness than category B, and moderate carrier-dyeing properties and good high-temperature dyeing properties. Category D dyes have very high sublimation fastness and poor carrier-dyeing properties. They are used in cases when the highest standard of heat fastness is required, e.g.
9 for permanent press finishing treatments. They are not generally suitable for the carrier dyeing of polyester at the boil. From a dye chemist’s perspective, a classification by chromophore is very useful. The Color Index listed around 1,150 disperse dyes in 1992 by chemical class, and the categories include but not limit azo (1), anthraquinone (2), nitrodiphenylamine (3), methine
(4), quinoline (5), coumarin (6), and aminoketone (7). The corresponding chemical structures of the chromophores are demonstrated in Figure 3.
Figure 3. Structures of various chromophores.
Azo dyes are by far the most important class and account for more than 50% of the total commercialized disperse dyes in the world. The general method used to make an azo dye requires a coupling component and a diazo component. Therefore, various combinations of coupling components and diazo components should give an enormous range of possible dyes.
In theory, azo dyes can supply a complete range of rainbow colors, from yellow to blue-green and even black hues. However, commercially azo disperse dyes tend to supply more yellows, oranges and reds instead of dark hues. There are mono-azo, and disazo structures. However, in order to facilitate satisfactory molecular size, mono-azo structures are exceptionally
10 important. Aminoazobenzene is a typical structure in mono-azo disperse dye, which is presented by the structure in Figure 4. The characteristics of the product is controlled by the chemical nature of the substituents.
Figure 4. General structure of aminoazobenzene disperse dyes.
In this structure, X, Y, and Z are usually ring deactivating groups, such as, -NO2, -CN, -Br, and CF3. R1 to R4 include groups such as –CH3, -C2H5, -OCH3, -OC2H5, -C2H4CN, and
C2H4OCOCH3. Different combinations of substituents result in enormous numbers of aminoazobenzene based disperse dyes, creating colors from yellows to reds, and in some conditions, blues. In general, the greater the tendency of groups X, Y and Z to accept electrons and the groups R1 to R4 to donate electrons, the further the hue of the molecule will lie along the line from yellow, orange, red, violet, to blue19. Movement along the line in the direction yellow to black is an increase in the maximum absorption wavelength of the dye, which in a precise term is called a bathochromic shift. Figure 5 shows how the substituents affect the color of azo disperse dyes. The dyes from (8) to (11) are presented in a bathochromic series.
Other than the benzonoid mono-azo structures, heterocyclic diazo components are also used in preparation of azo disperse dyes to produce brighter and greener shades of yellow.
11
Figure 5. Disperse dye structure based on aminoazobenzene.
There are some deficiencies in azo dyes, which dye chemist should pay attention to during application, such as duller shades and lower light fastness than anthraquinone dyes, and the potential to breakdown into carcinogenic amines derived from the cleavage of the azo linkage20. However, the cost effectiveness compensates for the drawbacks mentioned above, which makes azo dyes still the largest class of synthetic organic dyes.
Another important group of disperse dyes are anthraquinone derivatives, accounting for 25% of the commercialized disperse dyes. Complementing the colors produced by the azo chemical class, anthraquinone disperse dyes often generate reds, violets, blues and blue-greens. While yellow and orange colors can be synthesized based on anthraquinone structure, they have been proved to be less competitive with yellows and oranges based on other chromophores20. Figure
6 presents the general structural of most anthraquinone disperse dyes.
12
Figure 6. Structural skeleton of most anthraquinone disperse dyes.
Like azo dyes, substituents R1 to R6 have wide range of options. The hue is largely controlled by substituents R1, R4, R5 and R6, rather than R2 and R3, and these groups are usually hydroxyl, amino and secondary amino groups, -NHR. The –R in the secondary amino groups also has various possibilities, such as –CH3, -C2H4OH, a benzene ring (Ar), and a benzene ring that is itself substituted by other groups. The more powerful the effect of the electron donor substituents, the further the hue of the dye will lie in the bathochromic shift direction. The approximate order of electron donating effect follows the list: -NHAr > -NHAlk > NH2 > OH, while substitution in both rings is more powerful than substitution in only one. Substituents in the R2 and R3 positions have less effect on the color of the anthraquinone disperse dyes.
Because they are less likely to form intramolecular hydrogen bonding with carbonyl group.
19 However, R2 and R3 can have a significant effect on the fastness properties of the product .
The effects of different substituents are shown in Figure 7.
13
Figure 7. Disperse dye structure based on anthraquinone.
Generally, anthraquinone dyes give brighter colors than azo dyes, and have better light fastness and wash fastness properties. They also have advantages such as good stability in dyeing and levelling. On the other hand, they are expensive to synthesize and pose the potential to cause pollution problems, which make them gradually replaced by other type of disperse dyes, except for some bright pinks and blues17. Newer disperse dyes are increasing based on the use of heterocyclic components; i.e., aromatic rings containing five or six membered atoms which include nitrogen, sulfur and oxygen in place of one or more of the normal carbon atoms. These heterocyclic components may appear at either side of the azo chromophore. Examples are CI
Disperse Green 9 and CI Disperse Yellow 8, which are shown in Figure 8.
14
Figure 8. Chemical structure of two heterocyclic disperse dyes.
2.2.2 Basic dyes
Concerning cationic dyeable polyesters, it literally means that they can be dyed by a cationic dye, which is also known as basic dye. Meanwhile, being dyeable by basic dyes does not prevent them being dyeable by disperse dyes as well. The consumption of CDP accounts for less than 10% of the polyester market, and they are often blended with other fibers to achieve certain properties. For example, when CDP is blended with polypropylene, the resulting mixed fiber shows reduced crystallinity, which favors the dyeability of the fibers21.
Basic dyes also have various chemical classes defined by their chromophores. Figure 10 shows structure and color index specification of several important basic dyes belonging to various classes.
Compared to disperse dyes, basic dyes have larger molecular extinction coefficients and higher build-up property, so they can give brighter and deeper colors, and some dyes even exhibit fluorescent properties. Basic dyes are very sensitive to alkali and upon hydrolysis produce colorless substances15. An example is illustrated in Figure 9. Therefore, acids should be added for the sake of storage. In addition, dyes form a sticky mass on storage posing difficulty in solubilization, adding a little acid can facilitate solubilization in water. Basic dyes possess
15 advantages like wide shade range, good brightness and relatively economical. However, they also have marked disadvantages, such as poor shade stability, very poor light fastness, high acid content, and color backwaters, making them not as wide spread as disperse and other dyes.
Figure 9. Colorless compound liberated from reaction of basic dye with alkali.
Figure 10. Structure and color index specification of some basic dyes.
16
2.3 Dye characterization
2.3.1 Ultraviolet-visible spectroscopy
Color of a substrate is determined by the light reflected from the surface of a solid or passing through a liquid. Sunlight has uniform white color, but it is actually composed of a broad range of wavelengths in the ultraviolet (UV), visible and infrared (IR) portions if the spectrum.
Visible wavelengths cover a range from approximately 400 to 700 nm, among which the shortest is violet and the longest is red. When a beam of sunlight or other white light is illuminated at a red dye, a portion of mixed wavelengths is absorbed, leaving the red light to be reflected. The remaining red light is the complementary color to the wavelengths absorbed.
Ultraviolet-visible (UV-Vis) spectrophotometer is used to measure the absorbed light22. The relationship between the wavelength absorbed, colored absorbed and the color seen by human eye is demonstrated in Table 3.
Table 3. Absorption of visible light and color seen
Wavelength Absorbed (nm) Color Absorbed Color Seen 400-435 Violet Yellow-Green 435-480 Blue Yellow 480-490 Green-Blue Orange 490-500 Blue-Green Red 500-560 Green Purple 560-580 Yellow-Green Violet 580-595 Yellow Blue 595-605 Orange Green-Blue 605-700 Red Blue-Green
17
For dye solution, other than measuring the absorbed wavelength of the sample, concentration of the dye solution can also be obtained by UV-Vis measurement. Because the absorption of light by a dye in solution is directly proportional to its concentration; i.e., the greater the concentration of the dye, the greater of the amount of light is absorbed. The equation for the absorption is known as Beer-Lambert Law, which is:
� = ���
Where A is the observed absorption, b is the path length of the sample cell, c is the concentration of the sample, and ε is the absorptivity or molar extinction coefficient, which is specific for each species23. Typical ε values for mono-substituted anthraquinone disperse dyes are in the range of 4,000-7,000, and for di-substituted anthraquinone disperse dyes are about
10,000-17,000.
2.3.2 Chromatography
The concept of chromatography was firstly introduced by Michael Tswett24. It is an analytical technique for the separation of a mixture. There are many types of chromatography, such as thin layer chromatography, column chromatography, and high performance liquid/gas chromatography, but all of these follow the same basic principles. The mixture is dissolved in a solvent called the mobile phase, which carries it through a fixed material called the stationary phase. From the same initial zone, different components in the mixture shows varying migration rates, causing them to separate. In another word, the separation is based on the different partition coefficient of the solute between the mobile and stationary phases. The mobile phase may be either a liquid or a gas, and can be manipulated to accommodate a variety of chemical compositions. Stationary phase can be either a solid or a liquid with different
18 choice of materials, e.g. cellulose, silica, alumina, inert gas, etc. High performance liquid chromatography (HPLC) is an improved form of column or thin layer chromatography. It uses material with very small particle size for column packing, which gives a larger surface area for interactions between the stationary phase and the molecules flowing through it. Moreover, there are two phases in use in HPLC depending on the relative polarity of the solvent. One is normal phase, the column of which is filled with polar materials as same as normal thin layer chromatography. The other is reversed phase HPLC. In this case, the column is filled with modified silica gels to make it non-polar. Although it is described as “reversed”, it is the most commonly used form of HPLC. In addition, the detection method is also improved by using highly automated and extremely sensitive technologies.
2.3.3 Mass spectrometry
Mass spectrometry is a highly sensitive technique used to detect and identify molecules based on their mass-to-charge ratios (m/z)25. In order to measure the characteristics of individual molecules, they are converted to ions so that they can be sorted and separated by external magnetic fields according to their mass-to-charge ratios. The ions are then detected and analyzed electronically by mass analyzer. The analytes can be ionized by various methods, such as electrons, photons, excited atoms, or electrostatically charged droplets. Harsh method results in more fragmentation patterns of the analyte, while soft method allows less fragmentation during ionization. It is common to couple HPLC to a mass spectrometer. When the detector from HPLC is showing a peak, the substance passing through the detector at that time is transferred to a mass spectrometer, at which it will finally be analyzed for its m/z and give a mass ion pattern for the sample. It can be compared against a computer database of
19 known patterns or other referrals, which means LC-MS can identify a wide range of compounds without having to know their retention times.
2.4 Toxicity
Toxicology is the study of adverse effects of chemicals on living organisms and their environment. Before the discovery of the first synthetic dye in 1856, people obtained colorants from nature, mainly from plants and some portion from insects and molluscs. It was relative safe for workers to produce dyes from nature. However, the efficiency was below expectation because large amounts of raw materials were required in order to just obtain a tiny amount of impure dyes. Since the historical development in 1856, dyes, chemical intermediates, and later pigments were produced on a large scale with less labor intensity. Unfortunately, several years later, the incidence of bladder cancer became higher between workers who involved in the manufacture of certain dyes and intermediates26, such as CI Basic Violet 14, CI Basic Yellow
2, benzidine and 2-naphthylamine (see Figure 11), which drew researchers’ attention to study the toxicity and structure-carcinogenic relationship of synthetic dyes and their intermediates.
Later it was proved that both benzidine and 2-naphthylamine are indeed bladder carcinogens in humans. Nowadays, for registration of a textile dye, the toxicological studies and eco- toxicological studies are required in the registration package.
20
Figure 11. Chemical structures of some bladder carcinogens.
2.7.1 Dye structure property relationships
The toxicological aspects of textiles dyes can be divided into acute, also known as short-term effects and chronic, or long-term effects. Acute toxicity is a result from an acute exposure to potential toxic dyes through oral ingestion, inhalation, skin and eye irritation, and skin sensitization. Caliskaner27 studied a case of a 35-year-old woman who was referred for a recurred lesion over the incision scar of right total hip replacement surgery. They found out that Disperse Blue 106 and Disperse Blue 124 from her dark-colored synthetic panties were the potential cause of the contact dermatitis. Textile dermatitis is actually not uncommon.
Other than the aforementioned two disperse blue dyes, which are the two mostly reported dye allergens, dermatologists also have reported textile-related skin reactions thought to be caused by Disperse Blue 1, Disperse Yellow 3, Disperse Orange 1, Disperse Orange 3, Disperse Red
1 and Disperse Red 1728, listed in Table 4.
21
Table 4. Disperse dyes considered a health risk to consumers.
C.I. Name Chemical structure Disperse Blue 106
Disperse Blue 124
Disperse Blue 1
Disperse Yellow 3
Disperse Orange 1
Disperse Orange 3
Disperse Red 1
Disperse Red 17
The sweat-fastness properties of the dyes are important as to whether an allergic response is caused or not. Disperse dyed polyester is not problematic since the sweat-fastness is high.
However, polyamide or cellulous acetate dyed with disperse dyes poses problems since the low sweat-fastness allows the dyes to migrate to the skin, which increases the sensitizing
22 potential. Besides, disperse dyes containing anthraquinone or azo structures are more likely to cause contact dermatitis28.
Certain reactive dyes have been implicated in causing acute effects on plant workers who manufacture or handle the dyes29. Reactive dyes for cotton are water-soluble and readily hydrolyzed. Once the dye has been used to color the cotton fabric, the dye structure is modified, i.e., a covalent bond is formed between the dye and the hydroxyl group in the fiber.
Any reactive dye left on the surface should be hydrolyzed in the wet dyeing process and can be easily removed through washing and rinsing. That is the reason why reactive dyes should poses no problems in consumers but mainly in plant workers.
Genotoxicity is the major long-term potential health hazard of certain textile dyes. Genotoxic chemicals include mutagens, carcinogens and teratogens. Some azo dyes have been found to be both mutagenic and carcinogenic, e.g., 6-dimethylaminophenylazobenzothiazole (6BT) is a potent carcinogen and mutagen in rat following dietary administration30. In stark contrast, some other azo dyes are neither mutagenic nor carcinogenic, e.g., 4’-phenyl-4- dimethylaminozaobenzene (4PhDAB) shows low azoreductase activity in the Salmonella bacterial tester assay in the presence of an induced rat-liver S9 mix31. Teratogens are agents that cause malformation of an embryo. Teratogenicity is very uncommon in textile dyes and will not be discussed.
23
Figure 12. Chemical structure of 6BT and 4PhDAB.
The underlying principle for dyes to induce genotoxic effects on living organisms is that the dyes need to penetrate the cell membranes and attack the DNA function. Therefore, physical factors of dyes such as solubility and molecular size are essential in determining whether the dye penetration occurs. In general, molecules with small size are more readily transported across the cell membranes than larger molecules. Above a certain molecular size, MW > 800, chemicals become too large to transport across the membranes. Thus, producing dyes with large molecular size is a potential way to prevent genotoxic effects. Indeed, this approach was adopted to produce non-toxic food dyes. Solubility is also of importance in determining the toxicity of dyes. Majority of pigments are non-carcinogenic because the nature of large pigment particles does not allow them to pass the cell membranes. Dyes with high water solubility are often non-carcinogenic. Because water-soluble molecules are generally excreted rapidly, bioaccumulation of such dyes is less likely to occur in a living organism32.
The active species of carcinogens or mutagens should be an electrophile, E, since the DNA is a nucleophile compound. The ultimate attack forms a covalent bond between the E and DNA.
Therefore, molecules containing electron-deficient carbon, nitrogen, or oxygen atom are possible to be genotoxic. Such molecules may be the dyes themselves, or may be metabolites of the dyes. Carcinogens related with textile dyes are most chemicals possessing one or more electron-deficient nitrogen atom, among which the most important type is the amino-
24 containing dye. Figure 13 shows the general process for these compounds to produce an ultimate electrophilic nitrenium ion33. This pathway occurs at primary or secondary amino groups, and at methylamino- or dimethylamino-groups via oxidative demethylation. As earlier mentioned, half of these compounds increasing the bladder cancer incidence are large depots for the nitrenium ion. Anthraquinone structure does not contain azo bond, but also follows the similar reaction mechanisms. Anthraquinone dyes having one or more primary amino- or methylamino- groups tend to be genotoxic. For instance, in Figure 14, CI Disperse Orange 11, and CI Disperse Blue 1 are carcinogens, and CI Disperse Violet 1 is a mutagen. Cationic dyes have been reported to be carcinogenic, such as CI Basic Violet 14 and CI Basic Yellow 14, as shown in Figure 11.
Figure 13. Electrophilic nitrenium ion from amino-containing compounds.
Figure 14. Carcinogenic CI Disperse Orange 11 and CI Disperse Blue 1, and mutagenic CI Disperse Violet 1.
25
Carcinogens from carbon and oxygen electrophiles are not as common as nitrogen electrophiles. However, they are encountered in the synthesis or chemical modification of dyes. They are usually chemicals containing alkyl substituents bearing a leaving group, such as chlorine and bromine, or a strained small ring system, which open to generate an electrophilic center. Some agents used in the synthesis of dyes produce electrophilic carbon by the polarization induced by the electron-withdrawing group. Typical examples are vinyl chloride, acrylamide and acrylonitrile. Many compounds having four or more fused benzene rings are believed to be carcinogenic. Because they tend to generate an electrophilic carbon center via epoxide formation, as illustrated in Figure 1534.
Figure 15. Metabolic pathway for polycyclic aromatic hydrocarbons.
2.4.2 Methods used
Whether dyeing and finishing or decolorization treatment, textile activities are often wet processes, thus generating considerable amount of effluent discharged to the environment.
Therefore, studying the effects of compounds to organisms living in the water, which is also known as aquatic toxicity, is of extreme importance. Toxicity tests are based on the principle that the response of living organisms to the exposure of the toxic agents is dependent upon the exposure level (dose) of the toxic agent. Therefore, aquatic toxicity tests are designed to demonstrate a dose-response relationship, referred to as the dose-response curve when the
26 measured effect is plotted graphically with the concentration. The endpoint for acute toxicity is usually survival, whereas endpoints for chronic studies are sub-lethal effects such as growth, reproduction, behavior.
2.7.2.1 Acute toxicity tests
Acute toxicity is the toxicity elicited immediately following short-term exposure to a chemical.
It may be the result from a single exposure or from multiple exposure in a short period, and the adverse effects should occur within 24- to 96-hour period. There are standard guides on how to perform acute toxicity tests published by the American Society for Testing and Material
(ASTM), Environment Canada, and the U.S. EPA. Particular species are used for different tests, environmental compartments, and regulations. The relationship is generally established by exposing groups of organisms to various concentrations of the chemical. A well-defined concentration-response curve should select concentrations that elicit >0% effect but <100% effect during the course of the experiment. Then it can be used to calculate the LC50 for the toxicant, which is defined as the exposure concentration of the toxicant that is lethal to 50% of the exposed population. Clearly, the LC50 value is not indicative of an acceptable level of the chemical in the environment, rather the LC50 is just an indicator of relative acute toxicity. LC50 values are often interpreted as follows, shown in Table 5. Besides, EC50 is also used to characterize the acute toxicity, which is defined as the concentration of a toxicant at which
50% if its maximum response is observed. The response may be lethal or sub lethal effects.
27
Table 5. Interpretation of LC50 values.
LC50 (mg/L) Toxicity rating >100 Relatively nontoxic 10-100 Moderately toxic 1-10 Very toxic <1 Extremely toxic
Much research has been conducted to investigate the ecotoxicity of some commercially available disperse dyes and their main degradation products by either reduction or oxidation.
For example, ecotoxicity of Disperse Red 1 (DR1), an azo dye, and the degradation products generated during photo-Fenton degradation has been assessed by measuring acute toxicity with microcrustacean Daphnia similis35. The tests were performed with Daphnia similis in 48 h, and EC50 values were reported. By real-time monitoring the photo-Fenton degradation process, it was found that toxicity increased after 10 min as a consequence of generation of degradation products of higher toxicity than DR1. After 45 min reaction, acute toxicity of DR1 azo dye to
Daphnia similis was completely removed. LC/MS results detected most of the intermediates formed in the reaction. A possible degradation mechanism was proposed and is depicted in
Figure 16. The attack of hydroxyl radical, which is a very reactive species generated by photo-
Fenton reaction, includes the hydroxyl addition to an aromatic ring and cleavage of the azo bond.
28
Figure 16. Proposed initial pathway for degradation of commercial DR1 dye by photo-Fenton oxidation35.
2.7.2.2 Chronic toxicity tests
Aquatic chronic toxicity study is used to assess potential hazards to aquatic species resulting from prolonged and repeated exposure over a significant portion of the organism’s life span, typically one tenth or more of the organism’s lifetime. Chronic studies evaluate the sub-lethal effects of toxicants on reproduction, growth, and behavior due to physiological and biochemical disruptions. Effects on survival are also evaluated, but they are not always the main objective of a chronic study. Aquatic toxicity studies often conducted on species includes brook trout, fathead and sheepshead minnow, daphnids, oligochate, midge, freshwater amphipod, zebrafish, and mysid shrimp36. Algal species reproduce so rapidly that several
29 generations are exposed during a typical study, and therefore chronic tests should not use these species. As acute toxicity tests, chronic toxicity tests also have standard testing methods regulated by environmental agencies. Important information derived from the concentration- response curve tells the NOEC (no observable effect concentration), LOEC (lowest observable effect concentration), and MATC (maximum allowable toxicant concentration) values of the chemical.
2.5 Decolorization treatment
According to the treatment object, decolorization can be classified into two categories: decolorization of solid phase and decolorization of liquid phase. The latter is well known as wastewater decolorization treatment. Decolorization of solid phase, which means stripping colors from a solid substrate, has been less investigated.
2.5.1 Wastewater decolorization treatment
Over the past two decades, manufactures and users of synthetic colorants have faced increasing stringent regulations regarding the safety our environment, which promoted tremendous research programs and technologies to comply with the regulations. A significant portion of the research was conducted to analyze and remove priority pollutants from wastewater effluents. Wastewater from the textile industry contains unfixed dyes along with other components like salts, acids, surfactants and even metals. In terms of its environmental impact, wastewater discharged is polluting to some extent. Colorful textile effluent also causes aesthetic issues. In general, the composition of a particular wastewater, in addition to site- specific conditions, dictates the most appropriate wastewater treatment method. Huge successes have been achieved to remove colors from wastewater37–44. However, the research
30 on the decolorization of textile dyes has mainly been focused on water-soluble dyes, while decolorization of disperse dyes has received only scant attention.
2.5.1.1 Chemical methods
Chemical decolorization methods use chemical agents to break down dye structure through oxidation or reduction reactions. In view of oxidation technologies, hydrogen peroxide and hypochlorite are reported as widely used oxidation agents. Hydrogen peroxide (H2O2) has low environmental impact and is relatively economic. Owing to its mild nature, H2O2 is heavily used as the bleaching agent to remove yellowish colors from cotton fabric. However, it may fail or take an extremely long time to decolorize dark hues. Chlorine-containing substances such as sodium hypochlorite, calcium hypochlorite, chlorine and chlorine dioxide are also well known bleaching agents for cellulosic fabric. The equipment required for hypochlorite decolorization is simple and the treatment process can be finished in a short time scale. On the other hand, they are of relatively high toxicity compared with other decolorization agents, and generate large amount of salt as secondary contamination. Ozone is also reported effective for azo disperse dyes decomposition in textile wastewaters38. Ozone fading of dyes occurs by the oxidative cleavage of the conjugated system of the dye molecule. The ozonization of molecules, such as azobenzene, phenylazonaphthalene, and azonaphthalene dyes, is very complicated so that the products have not been fully identified. Decolorization of Disperse
Blue 3 on nylon carpet via ozone fading has been reported to give phthalic acid45. It is suggested that aromatic rings are more reactive toward ozone than an azo linkage46. Ozone was used to decolorize wastewater containing Acid Red 158, a bisazo acid dye47. Results confirmed that ozone decolorization is an effective color removal method, and the rates of
31 ozone reaction are not sensitive to pH and only mildly affected by temperature. In that study, researchers also found that ozone does not react preferentially with uncolored organic compounds. In practice, ozone alone is usually utilized for the treatment of drinking water.
At present, Advanced Oxidation Process (AOP) 39,48–52 has been developed to oxidize organic compounds to harmless products with high reaction rate as well as low environmental emissions. The AOP is mainly a catalyst-driven process, using UV light or metal catalyst with an oxidizer such as H2O2 and/or ozone to generate highly reactive hydroxyl radicals, which can attack organic compounds non-selectively. For example, Fenton’s reagent, which is a combination of H2O2 and an iron catalyst, is able to generate free radicals automatically without UV light or heating42. Equation (1) in Figure 17 is the process of conventional hydrogen peroxide releasing reactive species HOO-. Equations (2) and (3) show how the hydroxyl radicals are produced from Fenton’s reagent, and how the ferric iron is reduced back to ferrous ion, indicating Fe2+ can be recycled after treatment.
Figure 17. Production of reactive species in hydrogen peroxide (1), and Fenton’s reagent (2), (3)
Szpyrkowicz et al. 42 made a comparison study on oxidation of disperse dyes (mixture of
Disperse Yellow 126, Disperse Red 74, and Disperse Blue 139) by chemical oxidation using ozone, hypochlorite, Fenton’s reagent and electrochemical oxidation. They found that the least
32 satisfactory result was obtained by hypochlorite oxidation, while the best treatment result was obtained with Fenton process, and the performance of ozone and electrochemical oxidation are between the two extremes, as judged by color removal and chemical oxygen demand (COD) removal.
Namata and co-workers53 reported a study regarding the decolorization of Reactive Blue 171
(RB 171) using ozonation and UV/H2O2. The found RB 171 with 50 mg/L can be completely decolorized using ozonation by modifying operational conditions such as pH, temperature, and concentration of the oxidants, while UV/H2O2 showed poor decolorization efficiency. Based on the GC-MS analysis, they proposed a possible fate of metabolism of intact RB 171 molecular by ozone, which is demonstrated in Figure 18. They assumed that the dye molecular was attacked by OH·, leading to an asymmetric cleavage and yielded intermediate a, and another reactive intermediate (1). Compound (1) was further attacked by OH· giving two intermediates b and (2), which the author described as an azo bond cleavage process. However, it seems other reactions occurred since the intermediates lost an -SO3Na group in b and an –
NH2 group in (2). These compounds were detected in (3) as other fragments. Oxidation cleavage between N and C of the triazine ring in (2) led to the formation of c and (4).
33
Figure 18. Proposed degradation pathway for the dye RB 171 by ozonation53.
For many dyes, particularly azo dyes, chemical reduction is an effective decolorization technique, and options for reducing agent are less complicated. Most reducing agent used in textile applications are compounds that can slowly decompose and release sulfur dioxide under specific conditions. These agents belong to the group of hydroxyl- and aminoalkanesulfinates
(rongalite, thiourea dioxide, and their analogs, see Figure 19). The reducing properties of these
34
2- compounds are mainly due to the cleavage of C-S bond and the formation of intermediate SO2
- 2- 54,55 anions of sulfoxylic acid, radical ions SO2 , and S2O4 dithionite ions .
Figure 19. Chemical structures of some important reducing agent.
When evaluating the reduction of dyes in wastewater, it is also important to investigate the potential reversal of the reaction upon exposure to oxygen, since color may reappear when the treated wastewater is discharged to the environment. A study was conducted to evaluate the effectiveness of three reducing agents in decolorizing Navy 106 (a mixture of three azo dyes)56.
In this study, the reduction process was the chemical pretreatment, followed by aerobic biological treatment. Three reducing agents were evaluated: 225 ppm sodium hydrosulfite,
225 ppm thiourea dioxide, and 150 ppm sodium borohydride. The chemical pretreatments were effective in removing color. However, they were not effective in removing BOD, and did not enhance the biodegradation when used in tandem with aerobic biological treatment.
2.5.1.2 Biological methods
Biological decolorization treatment is a complex process at the intersection of biology and biochemistry. Biological methods rely on microorganisms, such as white rot fungi, bacteria, nematodes, yeast and so on, to break down organic wastes. Due to the complex structure of dyes and their molecular design, many dyes are difficult to decolorize and decompose through simple exposure to biological agents. Aerobic biological treatment used to be very popular to
35 treat wastewater generated from textile dyeing operations. However, the ineffectiveness of aerobic biological treatment in reducing color has caused aesthetic issues. Azo disperse dyes, for example, are highly resistance to biodegradation under aerobic conditions. It has been reported that azo dyes undergo reductive splitting of the azo bond relatively easily under anaerobic microbial conditions, resulting in the formation of aromatic amines. The anaerobic treatment takes place in the absence of oxygen and converts various organic compounds to methane and carbon dioxide57. This process is considered to be microbiologically a nonspecific process, as presented in Figure 20.
Figure 20. Reductive degradation of azo dye under anaerobic condition.
However, some of the resultant aromatic amines have been demonstrated to be carcinogenic and mutagenic to aquatic life and even to mammals37. Therefore, the aerobic treatment seems to be a more practical and safe method for the biodegradation of textile dyes. In fact, sequential anaerobic-aerobic biological treatment has been reported capable of decolorizing textile
58–60 dyes . Regarding azo dyes, anaerobic-aerobic treatment (Figure 21) may generate CO2,
H2O, and NH3 as the final products.
36
Figure 21. General overview of the fate of azo dyes during anaerobic-aerobic treatment.
Textile wastes containing reactive, disperse and vat dyes were reported successfully decolorized and detoxified in a full scale combined anaerobic-aerobic system60. This study showed that the color derived from reactive and disperse dyes was largely removed in the pre- acidification basin and the anaerobic reactor. Anthraquinone vat dyes were also anaerobically decolorized, indicating that this system is capable of effective removing the color both soluble and insoluble dyes with various structures. The effluent after sequential anaerobic-aerobic treatment showed no toxicity towards Vibrio fisheri. In yet another report, the two-stage system was employed on decolorization of azo reactive dye, CI Reactive Black 5 (RB5), and its analog61. It has been reported that an overall color removal of 65% was found for both fully and partially hydrolyzed RB5 dyes. One metabolite (substituted hydroxylnaphthalene) remained in the aerobic stage effluent, causing the effluent to be colored even though no RB5 was present. Study on degradation of azo dye Disperse Red 1 in a pilot scale anaerobic-aerobic reactor has also been reported62. The results confirmed the capacity of the anaerobic-aerobic system to degrade azo dyes, as judged by 80% dye decolorization and 92% COD removal. In addition, both toxicity and mutagenicity were reduced significantly. Overall, the idea that
37 dyestuffs undergo anaerobic reduction generating organic amines that are more amenable to aerobic biodegradation than the original dyes is supported by these results.
2.5.1.3 Other methods
There are also other wastewater treatment methods that have been widely discussed, such as physical and physical-chemical wastewater treatment methods. Physical methods may not be dye-specific, but can be used to remove undissolved chemicals and particulate matter present in wastewater. Adsorption, for example, is one of the most effective, economically feasible techniques to remove textile dyes. Carbon-based adsorbent materials have been used for adsorption of various types of dyes, ranging from acid, direct, basic, and reactive to disperse dyes63,64. In general, low adsorption has been observed for acid and reactive dyes with low molecular weight, whereas high adsorption occurs with basic and direct dyes which are usually of higher molecular weight, and medium to high adsorption for disperse dyes which are hydrophobic in nature57. A major disadvantage of activated carbon adsorption is its high price, which calls for regeneration. Carbon adsorption is considered as neither an efficient nor economical decolorization treatment method. Therefore, it is recommended as a finishing and polishing step after a chemical or biological process65. Ion exchange, coagulation-flocculation, and membrane technologies are also reported for textile wastewater treatment66,67. However, they have disadvantages either high cost or secondary salt and sludge formation, which make them not a promising application for commercial treatment.
2.5.2 Decolorization of textiles
Many reactive dyes, basic dyes and disperse dyes used for textiles were designed to be stable to high temperature and UV light. In this case, decolorization of textile fiber will require strong
38 chemical agents to decompose the dye structure. There are limited efforts on fiber and fabric decolorization specifically. Hydrogen peroxide was patented to bleach hair fibers68.
Reduction clearing of disperse on the surface of polyester fabric may also be considered as a decolorization process. Disperse dyes adsorbed on surfaces are broken down into smaller and more water-soluble fragments by reduction clearing agents, usually made up of sodium dithionite and sodium hydroxide. Oxidative clearing of polyester fabric, is an alternative method to remove disperse dyes from polyester surface. Comparable wash fastness results to conventional reduction clearing and lower chemical oxygen demand values were reported by oxidative clearing process using hydrogen peroxide or ozone as the oxidation agent69.
SFS and its analog zinc formaldehyde sulfoxylate (ZFS) were largely used in discharge resist printing on polyesters fabrics70. SFS, also known as Rongalit (Rongal-registered trademark of
+ - BASF), is represented by the chemical formula Na HOCH2SO2 ·2H2O. Discharge printing is realized through destroy the background color by discharging agent, usually reducing agent such as SFS/ZFS, stannous chloride, and thiourea dioxide. Thus, compared to direct printing, discharge printing can print lighter colors on deeper background. Besides, SFS was also used to bleach dyed hair fibers and decolorize blue dyed denim fabric71. SFS has found applications in many other branches of industry of science, such as the paper industry and the organic synthesis, due to the excellent reducing properties of SFS. Like aforementioned sulfur- contained reducing agent, the reactions involving SFS occur through cleavage of C-S bond and
2- the formation of SO2 anions of sulfoxylic acid, which shows potential to selectively reduce aromatic aldehydes, benzils, ketones, and other carbonyl compounds without destroying the
72 - carbon frame . In addition, HOCH2SO2 anion also possesses relative reduction potential.
2- Aromatic carbonyl compounds can be destroyed by nucleophilic attack of either SO2 anions
39
- (Path A in Figure 22) or initial HOCH2SO2 anions (Path B in Figure 22). Considered that the reduction rate of some carbonyl compounds by sodium dithionite is more rapid than that by
SFS, Path B seems to be more favored.
Path A Path B
Figure 22. Reduction of aromatic aldehyde to alcohol by SFS in aqueous media72.
SFS also serves as an efficient reagent for the reductive dehalogenation of aldehydes and ketones. In Figure 23, a phenacyl halide was reduced in ethanol medium slowly (24 h) at room temperature or rapidly (<1 h) at reflux temperature to achieve the corresponding product73.
2- Addition of SO2 anion to ketone was also proposed as another possible mechanistic pathway.
- However, the nucleophilic displacement of halide by HOCH2SO2 anion, followed by loss of formaldehyde and SO2, was still more favored, because of the pronounced tendency of α- haloketones to undergo halogen displacement.
40
Figure 23. Reductive dehalogenation of phenacyl halide in ethanol medium by SFS.
Regarding physical properties, SFS is readily soluble in water, but is not stable in aqueous solution at high temperature. It contains large, transparent, and tubular crystals. It is a heavily hygroscopic substance and should be stored in a dry, cool and dark place, protected from moisture. SFS is odorless or possesses a faint leek smell. The loss of reactivity is indicated if a fishy smell is produced. It liberates toxic gases (H2S and SO2) upon heated, as the equation in Figure 24 shows74. Nevertheless, SFS is a powerful reducing agent, is inexpensive and commercially available, and can be handled without any special precautions, which make it a great candidate for decolorizing polyesters.
Figure 24. SFS decomposition reaction upon heated.
2.6 Recycling method
Many polymers like PET are inexpensive and durable materials, which can readily be converted to variety of products that find use in a range of applications. Current levels of polymer usage and disposal generate several environmental problems. Recycling is an
41 important action to reduce these impacts. Recycling provides opportunities to reduce oil usage and the quantities of landfilling wastes.
2.6.1 Conventional polymer recycling
Currently, recycling technologies for polymers including PET can be divided into primary, secondary, tertiary, and quaternary approaches75. Primary recycling approach only applies mechanical methods to achieve products with equivalent properties. It involves the re- introduction of clean products. From the textile perspective, primary recycling is simply reusing wearable polyester clothes that are donated to others who need them. Secondary recycling approach involves mechanical processes resulting in products with lower properties, therefore secondary recycling is often referred to as downgrading recycling. Examples are absorption composites recovered from polyester and polypropylene nonwoven selvages76, molded automotive carpets recovered from recycled fibers from PET bottle wastes77. In the former case, polyester and polypropylene nonwoven selvages were shredded, mixed, and compressed by molding techniques to produce functional sound absorption composites. While in the latter case, reclaimed PET bottles were melting extruded into fibers and further molded into automotive carpet. Both examples involve mechanical processes, but no chemical treatment. Tertiary recycling is the depolymerization process to convert polymers into constituent monomers or into oligomers that may be suitable for reforming original polymers.
Depolymerization of PET has been studied for many years. The initial patents78,79 regarding the depolymerization of PET by glycolysis in an excess diol, such as ethylene glycol and propylene glycol, were aimed to industrially produce polyols and unsaturated polyesters.
Satish and Wong initially developed the chemical recycling application of the reclaimed PET
42 for the purpose of sustainability. In their work, post-consumer soft-drink bottles were depolymerized by excess ethylene glycol in the presence of a metal acetate as catalyst. The resulting monomers and oligomers could be used as raw material to synthesize PET. Since then, the research of recycling PET bottles has been achieved significant progress. There are commercial approaches that have been well-established to recycle the PET bottles, either chemically or mechanically. However, recycling technology for dyed PET fabrics is limited, making incineration the predominant method of textile waste processing excluding landfilling.
Incineration, which is a way of quaternary recycling, only involves energy recovery and poses potential environmental problems, such as toxic ash emissions. Energy recovery from polymer wastes requires complete or partial oxidation of the material, producing heat, power and/or gaseous fuels, oils and chars. Each method provides a unique set of advantages that make it particularly beneficial for specific locations, applications or requirements.
2.6.2 Fabric reuse
Fabric reuse is different from primary recycling, which is a simply donating and transferring process. It involves chemical decolorization and re-dyeing the fabrics, producing products with new colors. Since polyester is a durable material, it is hard to damage the clothes by normal use. Decolorizing old-fashioned fabric and re-dyeing seem to be a good option to meet the continuously changing fashion markets and extend the life cycles of polyester fabrics.
Unfortunately, there is little literature regarding this type effort. When referring to fabric reuse, it is more likely to be quilting, re-purposing, and donating.
Guan et al. conducted a decolorization study of PET fabric using Fenton’s reagent80, which is known to be effective for wastewater decolorization. In their work, a full factorial design was
43 conducted to optimize the PET decolorization using Fenton’s reagent, and the optimal conditions involved using FeSO4 (0.18mM), H2O2 (1235mM), in water/acetone mixture
(1:1,v/v), at 120°C for 15 min. They found the use of acetone as a co-solvent with water was the key factor in providing efficient PET fabric decolorization. The efficiency of the optimized method was examined for a variety of disperse dyes, including azo dyes (Disperse Orange 30 and Disperse Blue 79), nitrodiphenylamine dyes (Disperse Yellow 42 and Disperse Yellow
86), anthraquinone dyes (Disperse Blue 56 and Disperse Red 60), a quinoline dye (Disperse
Yellow 54), and a basic dye (Basic Yellow 28). Result showed that PET fabric dyed by such colorants differ in ease of decolorization by Fenton’s reagent. Disperse Blue 79, Disperse Blue
56, Disperse Red 60 and Disperse Yellow 54 were successfully decolorized using the optimum conditions, while Disperse Orange 30, Disperse Yellow 42 and Disperse Yellow 86 were not fully decolorized using the same method.
An interesting study has been published by Shukla and co-workers for converting PET fabric waste into hydrophobic textile dyestuffs81. In their study, PET waste was chemically depolymerized using excess ethylene glycol, giving the product bis(2-hydroxyethylene terephthalate) (BHET). BHET was reacted with p-nitrobenzoyl chloride, which was prepared from p-nitrobenzoic acid, to give compound 2. Compound 2 was reduced to the amino derivative, and then reacted with bromine and potassium thiocyanate to get a benzothiazole derivative, which is the compound 4 shown in Figure 25 (a). Using the 2 diazo components,
2 disperse dyes were synthesized, which are the bright orange disperse Dye A and dull orange disperse Dye B in Figure 25 (b). These dyes were applied to polyester fabrics by standard dyeing, and depth of dyeing, levelness, and performance characteristics were found to be promising, which is shown in Figure 26.
44
(a)
(b)
Figure 25. Preparation of benzothiazole from BHET (a) and synthesis of dyes (b)81.
45
Figure 26. Color photographs of polyester fabric dyed with synthesized dyes.
2.7 Preliminary study - development of SFS decolorization method
Before the design of experiment, solutions of three disperse dyes and one basic dye with different types of chromophores (anthraquinone, azo, nitro, and methine) were treated with
SFS in water/acetone (1:1) medium and color changes were monitored by absorption spectroscopy. The anthraquinone dye (Disperse Blue 56) was not completely decolorized whereas the azo dye (Disperse Orange 30), nitro dye (Disperse Yellow 42) and methine dye
(Basic Yellow 28) underwent a much greater color loss. The changes of the four samples in
UV-visible spectra are displayed in Figure 27. The spectrum of Disperse Blue 56 showed a decrease in intensity at λmax and the color of the solution underwent a considerable hypsochromic shift, exemplified by a shift from 630 nm to 525 nm.
46
2.5 2.5 2 2 1.5 1.5 1 1 Absorbance Absorbance 0.5 0.5 0 0 330 430 530 630 730 330 430 530 630 730 Wavelength Wavelength
0 min 30 min 0 min 30 min
A B
2.5 3 2 2.5 2 1.5 1.5 1 1 Absorbance Absorbance 0.5 0.5 0 0 330 430 530 630 730 330 430 530 630 730 Wavelength Wavelength
0 min 30 min 0 min 30 min
C D
Figure 27. Changes in the UV-visible spectrum of (A) Disperse Blue 56, (B) Disperse Orange 30, (C) Disperse Yellow 42, and (D) Basic Yellow 28 after SFS (25g/L) treatment in water/acetone (1:1) medium.
In addition, several commercial fabrics were decolorized using SFS in water/acetone (1:1) solution. Kebelka-Munk (K/S) values were measured to characterize color remaining on treated fabrics. In these examples, the treated fabrics possessed only a faint amount of their original color. The color value of each sample was measured before and after treatment, the results of which are summarized in Table 6. The untreated samples were all deeply dyed, which
47 was reflected in their high K/S values, except for the grey sample. Dyes used for the commercial fabrics were not revealed to us. Results from decolorization of the commercial fabrics were coincident with that from decolorization of disperse dye solutions. After treatment, their colors were reduced dramatically and only a small amount of color remained on the fabric, as shown in Figure 28. The fluorescent yellow sample became slightly grey after
SFS reduction. The grey and blue fabrics samples possessed a beige tint. The black fabric was also well decolorized, becoming off-white. Decolorization of the red sample was somewhat less effective than the others, with a red stain left on the treated fabric. The green sample was decolorized efficiently, becoming nearly white.
Table 6. K/S values of commercial PET fabrics before and after SFS (40g/L) treatment in acetone/water (1:1) at 100°C.
K/S Values Fabric Color Before Treatment After Treatment Yellow 53.6 1.6 Grey 13.2 1.6 Blue 41.8 2.5 Black 532.6 6.1 Red 240.6 2.8 Green 220.7 1.9
Both from the visual assessment of these samples and statistical measurement of K/S values, it was clear that SFS decolorization is a promising method for treating dyed PET fabrics as well as dye solutions, since most of these fabrics and solutions were decolorized to a high degree.
48
Yellow Grey Blue
Before After Before After Before After
Black Red Green
Before After Before After Before After
Figure 28. Commercial PET fabrics before and after SFS (40g/L) treatment in acetone/water (1:1) at 100°C.
2.7.1 Effect of treatment conditions on fabric decolorization
2.7.1.1 Treatment time
Having confirmed that disperse dyes could be decolorized by SFS in solution and in PET fibers, the next set of experiments pertained to optimizing the decolorization process using a commercial garment fabric. Figure -(a) shows the effects of SFS treatment time on K/S values of the commercial black fabric, over the 5-60 min timeframe, and Figure 30-(a) shows samples of the treated PET fabrics themselves. It can be seen that longer treatment time gives better decolorization performance. To help establish the lower limit of the treatment time, 5 min and
10 min SFS treatment were considered. However, from the K/S values, it is clear that more
49 color persisted at both time intervals. In general, the sample treated for 30 min appears to have a comparable decolorization level to the one treated for 60 min.
2.7.1.2 Water to acetone ratio
The treatment procedure was the same as used to investigate the effects of treatment time, except for using baths of different water to acetone ratios, and the temperature was lowered to
110oC. If the reaction vessel was heated to 120oC, the pressure inside beaker led to significant bumping. With this in mind, the treatment temperature was lowered to 110oC.
The effects of water to acetone ratio on the depth of shade (K/S) of decolorized polyester fabric are illustrated in Figure -(b) and Figure 30-(b). The results show that decolorization took place in all media but higher ratios of water to acetone (4:1 and 3:1) had a negative effect on decolorization efficiency. It can be concluded that the higher proportion of water is unfavorable for the extraction of sparingly water soluble disperse dyes from PET fabric to the reducing medium. However, significantly increasing the amount of organic solvent (acetone) reduced decolorization efficiency as well. This is because SFS is soluble in water, but not in acetone. Solubility of reducing agent decreases as acetone content increases, which results in a decrease in decolorization performance. In summary, the most acceptable decolorization resulted when the ratio of water to acetone was 1 to 2.
2.7.1.3 SFS concentration
Results from assessing the effects of SFS concentration on fabric decolorization are illustrated in Figure -(c) and Figure 30-(c), and can be divided into three parts. First, the K/S value decreased when increasing SFS concentration from 5 to 10g//L, which indicates that more dye
50 was reduced by increasing the amount of reducing agent. Then K/S increased as SFS concentration increased further, and reached a peak at 30g/L. Subsequently, K/S value dropped back to a low level when SFS concentration was increased to 40g/L. These results suggest the conversion of initially uncolored products or intermediates to secondary colors followed by secondary color degradation. A large excess of SFS (40g/L or more) does not improve dye degradation. Sufficient decolorization performance can be achieved with concentrations as low as 10 g/L.
2.7.1.4 Temperature
Results from this set of experiments are presented in Figure -(d) and Figure 30-(d) where a strong temperature relationship on PET decolorization is observed, which means temperature is a very important parameter that will have a significant influence on decolorization. At 80˚C, little dye was extracted and decolorized, with decolorization at 100 ˚C and 110˚C much more effective. This emphasizes that SFS decolorization involves dye transfer from PET fibers to the liquid medium (extraction), and after dye arrives in the medium, it will be more readily decolorized, and thus driving more dye out of fiber. In the dyeing process, disperse dye molecules can only penetrate the amorphous region, and the diffusion of dye molecules from the fibers surface into the body of polymer can only occur when temperature is above the glass transition temperature (Tg) of polyester. When enough heat is applied, polyester changes from rigid structure to a flexible structure. Then the dye molecules have the opportunity to slip between the movable chain segments into the pores of the fiber. By the same token, decolorization takes place more effectively at elevated temperatures. As an energy conservation measure, 100 ˚C was deemed suitable for this decolorization process.
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2.7.1.5 Liquor ratio
Liquor ratio is an important parameter in batch process, and is defined as the weight of ratio between the total dry material and the bath volume. The effects of the liquor ratio on the K/S values of decolorized polyester fabric were investigated. The amount of SFS was constant as liquor ratio changed. The results obtained are shown in Figure -(e) and Figure 30-(e), which show that K/S decreased with increasing liquor ratio. The difference of decolorization performance between various liquor ratios was not significant, and 1:50 gave substantial color removal in the Ahiba lab dyeing machine. The relative higher K/S value at low liquor ratio
(1:10 or 1:20) is likely due to insufficient coverage of fabric samples, resulting in poor dye extraction and therefore decreased decolorization performance. However, the minimum liquor ratio needed differs greatly between machine types. Mechanical factors of wet processing equipment, such as bath and fabric turnover rate, turbulence and physical/flow characteristics could influence the liquor ratio significantly. Using low-liquor ratio equipment, the weight of bath used to dye and/or decolorize a given weight of goods can be reduced as a result.
52
Temperature=120°C (a) Water: acetone=1:1 [SFS]=40g/L Liquor ratio=50:1
Temperature=110°C Time=30min [SFS]=40g/L Liquor ratio=50:1 (b)
Figure 29. Effect of (a) treatment time, (b) water to acetone ratio, (c) SFS concentration, (d) Temperature, and (e) liquor ratio on K/S value of black commercial fabrics after decolorization.
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Temperature=110°C Water: acetone=1:2 (c) Time=30min Liquor ratio=50:1
Time=30min Water: acetone=1:2 [SFS]=10g/L (d) Liquor ratio=50:1
Figure 29 (continued).
54
Temperature=100°C (e) Water: acetone=1:2 [SFS]=10g/L Time=30min
Figure 29 (continued).
55
5 10 15 20 30 40 50 60
(a)
4:1 3:1 2:1 1:1 1:2 1:3 1:4
(b)
Figure 30. Visualized effect of (a) treatment time, (b) water to acetone ratio, (c) SFS concentration, (d) Temperature, and (e) liquor ratio on K/S value of black commercial fabrics after decolorization.
56
g/L 5 10 15 20 25 30 35 40
(c)
80 ˚C 90 ˚C 100 ˚C 110 ˚C
(d)
1:10 1:20 1:30 1:40 1:50
(e)
Figure 30 (continued).
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2.7.2 Fabric strength assessment
To determine whether fiber degradation occurred when dye PET fabrics were subjected to SFS decolorization at elevated temperature, intrinsic viscosity was measured using an Ubbelohde viscometer and viscosity-average molecular weight was calculated using the Mark-Houwink equation:
[η] = 3.72×10-4 M0.73
In this investigation, the control was untreated 100% PET warp knit fabric, while the test samples were decolorized PET fabrics that had been dyed by C.I Disperse Orange 30 and C.I
Disperse Blue 60. Intrinsic viscosity and molecular weight results from these three fabrics are recorded in Table 7, where it can be seen that these properties were essentially unchanged.
Although this analysis did not provide information pertaining to the shapes of the molecular weight distribution, it gave us a general indication that degradation of PET fibers did not occur during SFS treatment.
Table 7. Intrinsic viscosity (IV) Vs viscosity-average molecular weight for control PET fabric and PET fabric after SFS (40g/L) treatment in acetone/water (1:1) at 100 ˚C.
Fabric IV (dL/g) MW Untreated 0.50 19,400 Decolorized Orange 30 0.50 19,300 Decolorized Blue 60 0.50 19,350
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2.7.3 Conclusions from preliminary study
As an initial step in the recycling of PET-based textiles, it has been shown that sodium formaldehyde sulfoxylate (SFS) can be used to decolorize dyed PET in water/acetone media.
While a treatment time of 60 min gives better decolorization, 30 min is sufficient. A water to acetone ratio of 1:2 gives the best decolorization performance, as higher levels of water or acetone reduce decolorization effectiveness. Sufficient decolorization can be achieved with an SFS concentration as low as 10 g/L and there is a significant temperature dependence for decolorizing polyesters but 100oC is deemed suitable. On a laboratory scale, the best liquor ratio is 1:50, which gives substantial color removal. Organic solvent used during decolorization process can be efficiently recovered and reused. It is also clear that SFS decolorization does not affect the mechanical properties of PET fibers. This method has other advantages. It is very easy, a one-step process, and only one chemical (sodium formaldehyde sulfoxylate) is needed. Secondly, it is applicable to regular PET and cationic dyeable PET.
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3. PRESENT RESEARCH
3.1 Objectives
The present work had following objectives:
(1) Study the recyclability of the decolorization bath and the decolorized fabrics. Solvent-
based decolorization bath should be recovered and reused in order to reduce the effluent
emission. Decolorized fabrics should be re-dyed as virgin PET fabrics with acceptable
color differences.
(2) Characterize the dye compounds in commercial fabrics by UV-vis, TLC, HPLC, and
MS.
(3) Investigate the toxicity of the decolorized solution. Azo, anthraquinone, and nitro
disperse dyes are decolorized by SFS, and the toxicity data of the remaining solution
should be obtained.
(4) Conduct a life cycle assessment of the closed loop recycling process, and compare with
the life cycle assessment impacts of virgin PET production system.
3.2 Rational
In 2011, Aizenshtein predicted that the PET fiber production would be twice as high as the annual cotton harvest in a few years, making it the main and most reliable raw material base within the global textile industry82. It is a synthetic material derived from non-renewable petroleum sources and its hydrophobic nature and high resistance to biodegradation make disposing worn-out PET textiles in land field sites a potential environmental problem. Further, continuous disposal of PET following a single lifetime of use is a waste of valuable resources.
60
With environmental stewardship in mind, an efficient approach to recycling colored polyester textiles has come to the forefront in the textile industry. Many studies have been conducted to investigate the recycling of PET bottles. However, the recycling of PET fabrics is limited.
PET bottles are usually clear and transparent but PET apparel contains various dyes. The dyes inside the fiber will reduce the degree of polymerization of the fiber during recycling process.
Besides the remaining dyes in the recycled PET will cause uniformity issues. In this regard, it seems clear that dye removal from colored products is a crucial step in the recycling process.
This study involved the selection of a group of structural diverse and widely used dyes to develop an efficient PET decolorization method. Dyes chosen included azo, anthraquinone, quinoline, and nitro disperse dyes, and sodium formaldehyde sulfoxylate was used as the decolorizing agent. A medium containing an organic solvent combined with water facilitated simultaneous dye extractraction and decolorization. Considering sustainability, a toxicity study and life cycle assessment were conducted.
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4. REUSE OF DECOLORIZATION BATH AND DECOLORIZED FABRICS
4.1 Introduction
The worldwide production of polyethylene terephthalate (PET) was around 49 million tons in
2008, having overtaken cotton since 2002, and a majority (79%) of the PET produced was used in the textile industry 82,83. PET fabrics are extensively used in a wide variety of apparel, home furnishings and automotive products, which find their way to landfills at the end of their useful life84. As a semicrystalline thermoplastic polyester, PET has high mechanical strength and low permeability to gases, which means it has high resistance to atmospheric and biological agents
13. Disposing the slowly degradable PET fabrics in landfills is creating a significant environmental concern 85. In addition, the manufacture of PET is an energy-intensive process, requiring large amounts of crude oil 86. Thus, a one-time use of PET fabric can be regarded as a waste of a valuable polymer derived from non-renewable petroleum resources. Although a fraction of PET bottles are recycled 88, the technology needed to reuse the PET fabrics is limited.
Currently, recycling technologies for PET and other polymers can be divided into primary, secondary, tertiary, and quaternary approaches 89. Primary recycling approach applies mechanical methods to achieve products with equivalent properties. From the textiles perspective, primary recycling is simply reusing wearable polyester clothes that are donated to others who need them. Secondary recycling approach involves mechanical processes resulting in products with lower properties, therefore secondary recycling is often referred to as downgrading recycling. Examples are sound absorption composites recovered from polyester and polypropylene nonwoven selvages 76, molded automotive carpets recovered from recycled
62 fibers from PET bottle wastes 77. Tertiary recycling is the depolymerization process to convert polymers into constituent monomers or into oligomers which may be suitable for reforming original polymers 90. Depolymerization of PET has been studied for many years. The initial patents78,91 regarding the depolymerization of PET by glycolysis in an excess diol, such as ethylene glycol, propylene glycol, were aimed to industrially produce polyols and unsaturated polyesters. The chemical recycling application of the reclaimed PET with the purpose of sustainability was initially developed by Satish and Wong79. In their work, post-consumer soft-drink bottles were depolymerized by excess ethylene glycol in the presence of a metal acetate as catalyst. The resulting monomers and oligomers can then be used as raw material to synthesize PET again. PET can be depolymerized to the corresponding monomers by hydrolysis, aminolysis 92, methanolysis, and glycolysis 81,90. Ever since then, the research of recycling PET bottles has been achieved significant progress. There are commercial approaches that have been well-established to recycle the PET bottles, either chemically or mechanically87,93. However, these approaches are not suitable for recycling most PET based textiles due to the presence of dyes. Disperse dyes are used to dye PET fabric and basic or disperse dyes are employed to dye cationic dyeable PET, which is a specialty fiber produced by adding small amounts of the sodium salt of dimethyl ester of 5-sulfoisophthalic acid when manufacturing PET94. If disperse dyes are not removed before recycling the fabric, their presence could cause a reduction in degree of polymerization during the melting process 95, as well as uniformity issues. Since recycling technology for dyed PET fabrics is limited, making incineration the predominant method of textile waste processing excluding landfilling96.
Incineration, which is a way of quaternary recycling, only involves energy recovery and also poses potential environmental problems, such as toxic ash emissions 97.
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While solvent extraction methods can be used to remove dyes from textiles, the dye concentration inside and outside the fibers will eventually reach a thermodynamic equilibrium.
In another words, extraction cannot make the textiles fully colorless, without removing the dyes from the solvent medium continuously. Physical methods, including adsorption using granular activated carbon 98 and membrane filtration99, chemical methods such as bleaching
100, ozonation 101 and Fenton oxidation102, and biological methods 103 have been reported for decolorizing dyes from textile wastewater but normally not from dyed textiles.
The presence of colorful dyes makes PET fabric attractive, but brings about challenges when it comes to recycling. With this in mind, a decolorization method was developed in our previous studies to remove disperse dyes from PET fabric for enhanced recyclability. Sodium formaldehyde sulfoxylate (SFS) was employed as the reducing agent to help remove disperse dyes. The decolorization process was carried out in water/acetone mixture solution since disperse dyes are hydrophobic and cannot be substantially extracted using water as the only solvent. Elevated temperature is required to increase desorption of the dyes by reducing cohesion between polymer chains. The decolorization behavior is strongly influenced by SFS concentration, treatment time, and liquor ratio. By considering the decolorization performance as well as the cost effectiveness, the optimized procedure was found to be water/acetone media
(v/v=1:2) at elevated temperature (100˚C) with the liquor ratio of 50:1 using SFS (10g/L) for
30 min. This method was effective for decolorizing a variety range of colorants104.
In the present work, SFS decolorization was further investigated. The goal was to reduce acetone consumption without decreasing decolorization performance. In addition, the strength of the decolorized fabric was tested using a standard method, burst pressure measurement, and
64 the re-dyeability of decolorized PET fabrics was assessed. Dyes used in this study included those listed in Table 8.
Table 8. C.I. names, classes, and structures of dyes used in this study.
Color Index Name Chemical Class Molecular Structure Disperse Orange 30 Azo
Disperse Blue 79 Azo OC2H5 Br
N N(CH2CH2OCOCH3)2 O2N N HN NO 2 COCH3 Disperse Yellow 42 Nitro
Disperse Red 60 Anthraquinone O NH2 OC6H5
O OH
4.2 Experimental
4.2.1 Material
Dyed commercial polyester knit leisure wear and white cationic dyeable polyester fabric were kindly donated by Nike, Inc. (Beaverton, OR, USA). Reducing agent sodium formaldehyde sulfoxylate dihydrate (SFS) was purchased from Arcos Organics, and HPLC grade acetone was purchased from Fisher Scientific. The disperse dyes and dyeing auxiliaries were obtained from our internal pilot plant inventory. All chemicals were used without further purification.
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4.2.2 Batch fraction distillation
After each fabric decolorization, the treatment bath (47~48 mL of acetone/water) was collected. Lab-scale fractional distillation apparatus was assembled (Figure 31). The bath was transferred to a 100-mL round-bottom flask containing a boiling stone. Heat was applied from a digital hot plate and maintained for a distillation rate of one drop per second. When the liquid stopped boiling, heat was removed and the distillate was re-used in decolorization experiments.
Figure 31. Diagram of experimental device for lab-scale fractional distillation. (1) Digital hot plate, (2) round-bottom flask, (3) condenser used as fractionating column, (4) two-way adapter, and (5) condenser.
4.2.3 Application of disperse dyes to decolorized fabrics
A stock solution (1g/L) of each disperse dye was prepared, with the addition of 1 mL of the dispersing agent Novadye NT 9. The dyebath consisted of stock solution at a 1% (o.w.f.) level, and glacial acetic acid (50 µL). Tap water was used to bring the bath to final volume needed for a liquor ratio of 20:1. Dyeing was conducted in an Ahiba lab dyeing machine. The dyebath was increased from room temperature to 130 ˚C at a ramp rate of 4˚C/min. The bath was held at 130 ˚C for 30 min and allowed to cool for 30 min. The fabric was rinsed with water,
66 reduction cleared using sodium dithionite (0.5 g/L) and sodium hydroxide (0.5 g/L), rinsed again with water, and allowed to air-dry.
4.2.4 Decolorization of laboratory-dyed fabrics using acetone distillate
The collected acetone distillate from section 4.2.2 was used to decolorize cationic dyeable PET fabrics that were dyed using Disperse Blue 79, Disperse Yellow 42, and Disperse Red 60 at
1% (o.w.f.). Water and distilled acetone were mixed at the ratio of 1:2. For each run, 1 g of fabric was treated in 50 mL of the solvent medium. SFS (0.5 g) was used as the reducing agent. The bath chamber was sealed and heated to 100 ˚C at rate of 4°C/min, and held for 30 min. The bath was cooled, and fabrics were removed, rinsed with running tap water for 2 min, and allowed to air-dry.
4.2.5 Color evaluation
A calibrated Datacolor Spectraflash 600X Reflectance Spectrophotometer equipped with iMatch software from X-Rite was used to determine the K/S and Whiteness Index values of the PET fabrics. The software was set to use illuminant D65 with the UV light included, and the CIE 10-degree supplemental standard observer. The sample being tested was folded twice and measured two times by rotating the sample at 90 degrees between measurements. The average value was recorded. The K/S value of each sample was calculated by adding the K/S value of each 10 nm from 400 nm to 700 nm as follows: