Visible Light-Driven Photocatalytic Degradation of Ciprofloxacin, Ampicillin and Erythromycin by Zinc Ferrite Immobilized on Chitosan
Visible Light-Driven Photocatalytic Degradation of Ciprofloxacin, Ampicillin and Erythromycin by...
Hassan Mohamed, Nehad Ahmed;Shamma, Rehab Nabil;Elagroudy, Sherien;Adewuyi, Adewale
2022-09-22 00:00:00
resources Article Visible Light-Driven Photocatalytic Degradation of Ciprofloxacin, Ampicillin and Erythromycin by Zinc Ferrite Immobilized on Chitosan 1 2 , 1 , 3 Nehad Ahmed Hassan Mohamed , Rehab Nabil Shamma * , Sherien Elagroudy 4 , 5 , and Adewale Adewuyi * Public Works Department, Faculty of Engineering, Ain Shams University, Cairo 11535, Egypt Department of Pharmaceutics and Industrial Pharmacy, Faculty of Pharmacy, Cairo University, Cairo 11561, Egypt Egypt Solid Waste Management Center of Excellence, Ain Shams University, Cairo 11535, Egypt Department of Chemical Sciences, Faculty of Natural Sciences, Redeemer ’s University, Ede 230, Osun State, Nigeria Yusuf Hamied Department of Chemistry, University of Cambridge, Lensfield Road, Cambridge CB2 1EW, UK * Correspondence: rehab.shamma@pharma.cu.edu.eg (R.N.S.); walexy62@yahoo.com (A.A.); Tel.: +20-111-930-1245 (R.N.S.); +2348035826679 (A.A.) Abstract: This study investigated the synthesis of zinc ferrite immobilized on chitosan (ZnFe O @Chitosan) 2 4 and its application in the photodegradation of ciprofloxacin (CIP), ampicillin (AMP) and erythromycin (ERY) in aqueous solution. Results from Fourier transform infrared spectroscopy (FTIR) revealed peaks suggesting its synthesis, while signals from X-ray diffraction (XRD) showed diffraction patterns confirming the synthesis of ZnFe O @Chitosan with a crystallite size of 35.14 nm. Scanning electron 2 4 2 1 microscopy (SEM) revealed a homogeneous morphology with a surface area of 12.96 m g from the Brunauer–Emmett–Teller (BET) analysis. The vibrating sample magnetometry (VSM) result revealed Citation: Hassan Mohamed, N.A.; a saturation magnetization of 2.38 emu g . The photodegradation study of CIP, AMP and ERY Shamma, R.N.; Elagroudy, S.; showed that both photodegradation and adsorption were taking place at the same time with the Adewuyi, A. Visible Light-Driven Photocatalytic Degradation of percentage degradation efficiency in the order CIP (99.80 0.20%) > AMP (94.50 0.10%) > ERY Ciprofloxacin, Ampicillin and (83.20 0.20%). ZnFe O @Chitosan exhibited high stability with capacity > 90% even at the 15th 2 4 Erythromycin by Zinc Ferrite regeneration cycle, suggesting a viable economic value of ZnFe O @Chitosan. 2 4 Immobilized on Chitosan. Resources 2022, 11, 81. https://doi.org/ Keywords: adsorption; antibiotics; catalysis; ferrite; photodegradation 10.3390/resources11100081 Academic Editor: Eveliina Repo Received: 21 August 2022 1. Introduction Accepted: 16 September 2022 Contamination of natural sources of drinking water by antibiotics is a global con- Published: 22 September 2022 cern [1]. The contamination is on the rise because of the unregulated use of antibiotics Publisher’s Note: MDPI stays neutral in some nations of the world [2]. The ease of purchasing antibiotics without medical with regard to jurisdictional claims in prescription in some countries has encouraged self-medication, resulting in the excessive published maps and institutional affil- use of antibiotics. The excessive use of antibiotics is one of the causes of their presence iations. in environmental natural water-like surface and underground water systems. These an- tibiotics may become persistent in the environment or may decompose to form products that are toxic to humans and the environment. Some of the decomposition products can cause serious health challenges like cancer. Apart from this, the presence of antibiotics in Copyright: © 2022 by the authors. the environmental natural water system has led to far more serious consequences like the Licensee MDPI, Basel, Switzerland. emergence of drug-resistant strains of pathogenic organisms [3], which, in turn, hampered This article is an open access article the efficacies of well-known antibiotics. Unfortunately, previously efficient antibiotics are distributed under the terms and now losing efficacy. It is important that these antibiotics are removed from water in order conditions of the Creative Commons to avoid the challenges associated with their presence in natural sources of drinking water. Attribution (CC BY) license (https:// creativecommons.org/licenses/by/ Many antibiotics have been detected in water [4,5], including ciprofloxacin (CIP), 4.0/). ampicillin (AMP) and erythromycin (ERY) reported in surface water as contaminants [6–9]. Resources 2022, 11, 81. https://doi.org/10.3390/resources11100081 https://www.mdpi.com/journal/resources Resources 2022, 11, 81 2 of 17 Their presence in water is of serious concern, although efforts have been made to remove them from water, but most of these efforts have shortcomings, like incomplete removal or being expensive. It is important to develop a process that can overcome such shortcomings with an affordable and sustainable approach. Photocatalysis is a green approach which has shown exceptional performance in the degradation of organic pollutants in water [10–12]. Photocatalysis has the potential of overcoming these shortcomings with the capacity for complete degradation of antibiotics in water [13]. Zinc oxide (ZnO) is an example of a photocatalyst that can be used in photocatalysis for the photocatalytic degradation of antibiotics. Unfortunately, ZnO is limited in its photocatalytic application, because it is photoactive in UV light due to its large bandgap energy. Previous studies have reported the use of ZnO particles for the degradation of amoxi- cillin, CIP, AMP and cloxacillin under UV light irradiation in aqueous solutions [14]. The study revealed a degradation efficiency of approximately 50% for CIP, creating the need for improvement. ZnO is active under UV light irradiation, which increases the process cost since there is a need to get a UV light source, unlike in the case of materials which are visible-light sensitive. A similar observation was also recorded recently using ZnO- functionalized fly-ash-based zeolite for the degradation of CIP which exhibited complete degradation [15]; despite the complete degradation, provision of UV light sources is an additional cost which eventually increases process cost. Developing ZnO into materials that are visible-light sensitive will go a long way in helping to reduce process cost. One of the ways of achieving this will be to incorporate ZnO into other particles, which reduces its bandgap energy. A good example of this is zinc ferrite (ZnFe O ). Ferrites are useful in this 2 4 regard because of their relatively narrow bandgap of approximately 2.0 eV, which makes it suitable for photocatalysis in the visible-light region. Spinel ferrites were recently reported for the degradation of tetracycline hydrochlo- ride [16]. Moreover, magnesium ferrite (MgFe O ) and manganese ferrite (Mn Fe O ) 2 4 x 3-x 4 have shown similar capacities against tetracycline [17] and sulfamethoxazole [18], respec- tively. Furthermore, high performance has been reported from the synergistic activity of MnFe O and molybdenum disulfide (MoS) for the degradation of tetracycline [19]. 2 4 Photocatalytic degradation of antibiotics by ferrite has proved to be a good solution for the treatment of antibiotic-contaminated water due to its soft magnetic properties, high catalytic activities and ease of recycling through magnetic separation [20]. However, a recent study revealed that the performance of a photocatalyst can be enhanced via a simple modification process. The current study proposes the modification of ZnFe O by organic molecule such 2 4 as chitosan. The use of chitosan will help stabilize the particles of ZnFe O by reducing 2 4 aggregation and helping to promote the recovery of ZnFe O particles from solution. A 2 4 previous study has shown that the efficiency of modified photocatalysts may be attributed to high light absorption, formation of step scheme heterojunction and interfacial charge sep- aration. Being a polysaccharide, chitosan contains random distribution of -(1–4)-linked D-glucosamine and N-acetyl-D-glucosamine. It is either neutral or negatively charged in acidic medium, which allows it to form electrostatic complexes or multilayer structure. Its nontoxicity, biocompatibility and biodegradability make it suitable for various applications such as in water treatment. This study aimed at investigating the preparation of ZnFe O via coprecipitation and 2 4 its immobilization on chitosan to further improve on its separation from aqueous solution when used as a photocatalyst for the photodegradation of antibiotics. ZnFe O @Chitosan 2 4 was proposed as a photocatalyst for the degradation of CIP, AMP and ERY in aqueous solution. Therefore, this study was aimed at the photodegradation of CIP, AMP and ERY under visible-light irradiation using ZnFe O @Chitosan. 2 4 2. Materials and Methods 2.1. Materials Zinc chloride hexahydrate (ZnCl .6H O), ferric chloride hexahydrate (FeCl .6H O), 2 2 3 2 chitosan, acetic acid, NaOH, C H OH, HCl, oleic acid, ciprofloxacin (CIP), ampicillin 2 5 Resources 2022, 11, 81 3 of 17 (AMP), erythromycin (ERY), isopropyl alcohol (IPA), ammonium oxalate (AO), chloro- form (CH), and all other chemicals used were purchased from the Aldrich Chemical Co., Gillingham, UK. 2.2. Synthesis of ZnFe O Particles 2 4 To prepare ZnFe O particles, mixtures of FeCl .6H O (0.4 M) and ZnCl .6H O (0.2M) 2 4 3 2 2 2 were continuously stirred for 60 min, after which oleic acid (15 mL) was added as a capping agent. The mixture was maintained at a temperature of 80 C and a pH range of 10–12 by dropwise addition of NaOH (2 M) until the appearance of precipitate while stirring for 2 h. The mixture was cooled to room temperature, filtered, and washed severally with water and ethanol. The residue obtained was oven-dried at 105 C for 12 h and transferred to the furnace at 550 C for 18 h. 2.3. Synthesis of ZnFe O @Chitosan Particles 2 4 To prepare ZnFe O @Chitosan, chitosan (1 g) was dissolved in acetic acid (50 mL, 2 4 2% v/v) and sonicated for 60 min. ZnFe O (2 g) was added to the solution and stirred 2 4 for 60 min. While maintaining room temperature, 30 mL of NaOH (1 M) were added and stirred for 40 min to form precipitates. The ZnFe O @Chitosan formed was filtered and 2 4 washed severally with deionized water. The residue obtained was oven-dried at 40 C for 12 h. 2.4. Characterization of ZnFe O @Chitosan Particles 2 4 The functional groups in ZnFe O @Chitosan were determined using FTIR (Agilent 2 4 Technologies); spectrum was recorded in the range of 400–4500 cm . The BET surface area was determined by N gas adsorption using Nova 3200 quanta chrome. TG analysis was carried out using a Mettler thermogravimetric analyzer (SDT Q600 V20.9 Build 20). The X-ray diffraction pattern was measured in 2 ranging from 5 to 90 using an X-ray diffractometer (Philip XRD-1390 PW model) with filtered Cu K radiation operated at 40 kV and 40 mA. The SEM image was recorded using SEM JSM-T25 (JOEL Co., Japan), while elemental composition was estimated on EDS. VSM was carried out on a magnetometer and UV-visible absorption spectra were recorded on a UV-visible spectrophotometer (UV-vis: Cary 60). 2.5. Photocatalytic Degradation of CIP, AMP and ERY by ZnFe O @Chitosan 2 4 The photodegradation study was carried out under visible light using a low-cost solar simulator (LSO1O6, 150 W Xe light source) with a filter holder and 90 beam turner. The degradation was achieved by contacting 100 mL of either CIP, AMP or ERY at a concentration of 5.00 mg L with 0.1 g of ZnFe O @Chitosan particle in a 150 mL beaker 2 4 for 180 min while stirring gently at 80 rpm under the simulated visible-light irradiation, ensuring a distance of 20 cm between the UV lamp and the test solution. Samples were withdrawn at different intervals to monitor the degradation rate. The concentrations of CIP ( = 271 nm), AMP ( = 420 nm) and ERY ( = 285 nm) were measured max max max using a UV-visible spectrophotometer (Perkin Elmer, Lambda 750 spectrometer). The effect of the ZnFe O @Chitosan weight on degradation was checked by varying the weight of 2 4 ZnFe O @Chitosan from 0.1 to 0.5 g, while the effect of concentration of CIP, AMP or 2 4 ERY on degradation capacity was evaluated by varying the concentration from 1.00 to 5.00 mg L (CIP, AMP or ERY), and the effect of pH was determined by varying the pH solution from 2 to 10. The experiment was repeated in the dark to establish the adsorption– desorption equilibrium. All the experiments were repeated three times and values were presented as mean value. The degradation efficiency was calculated as: Degradation E f f iciency (%) = 100 x (1 ) (1) o Resources 2022, 11, 81 4 of 17 where C is the initial concentration of CIP, AMP or ERY, and C is the concentration of CIP, o t AMP or ERY at time t. The adsorption capacity (q ) and the percentage removal (% removal) for the adsorption–desorption equilibrium experiment in the dark was calculated as: C C V ( ) o t q = (2) (C Ct) % removal = X 100 (3) Co Equation (4) was obtained by combining Equations (2) and (3) (% removal X C X V) q = (4) 100 X m 1 1 where C (mg L ) is the initial concentration of CIP, AMP or ERY, C (mg L ) is the o t concentration of CIP, AMP or ERY at time t; m is the weight (g) of ZnFe O @Chitosan used, 2 4 V represents the volume in litres (L) and q (mg g ) is the adsorption capacity. 2.6. Evaluation of Reactive Oxygen Species Scavenging Capacity In order to understand the mechanism of operation of ZnFe O @Chitosan, the role of 2 4 reactive oxygen species (ROS) in the photodegradation of CIP, AMP and ERY was inves- tigated using isopropyl alcohol (IPA) as a hydroxyl radical (OH) scavenger, ammonium oxalate (AO) as a scavenger for hole (h ) and the scavenger for superoxide ion radical (O ) being chloroform (CH). The scavengers were separately introduced into the photodegrada- tion process as a concentration of 1 mM. The process conditions (ZnFe O @Chitosan weight, 2 4 concentration of CIP, AMP or ERY, photodegradation time, and pH) for photodegradation with and without scavengers was kept constant. 2.7. Re-Useability and Stability of ZnFe O @Chitosan 2 4 To determine re-useability, the ZnFe O @Chitosan was recovered after the degrada- 2 4 tion time, washed with solvents (deionized water, 0.1 M HCl, ethanol or a mixture of ethanol and 0.1 M HCl (3:2)) and dried in the oven at 80 C for 5 h before it was reused for the photodegradation process. The treated aqueous solution was analyzed to check for the leaching of ZnFe O into solution using inductively coupled plasma–optical emission 2 4 spectroscopy (ICP–OES). The ICP–OES analysis was carried out at the end of each treat- ment cycle with ZnFe O @Chitosan. The photostability of the ZnFe O @Chitosan for the 2 4 2 4 photodegradation of CIP, AMP and ERY was evaluated in fifteen (15) successive cycles of operation. 3. Results and Discussion 3.1. Synthesis and Characterization of ZnFe O @Chitosan 2 4 The FTIR spectrum of ZnFe O @Chitosan revealed the functional groups it contained, 2 4 as shown in Figure 1a. The spectrum revealed a peak at 3420 cm , which was attributed to the O-H stretching, while the peak at 2892 cm was assigned to the C-H stretching of alkane. The -NH C stretch was observed at 2352 cm , while the signal corresponding to the C=O carbonyl stretch of amide was seen at 1612 cm . The N-H and C-H bending 1 1 appeared at 1584 and 1580 cm , respectively. The peak at 1432 cm was assigned to C-O stretch, while the anti-asymmetric stretching vibration of C-O-C appeared at 1027 cm . The signals appearing at 593 and 387 cm correspond to the stretching frequencies of Zn-O and Fe-O, respectively. The BET surface area of ZnFe O @Chitosan is shown in 2 4 2 1 Figure 1b, which revealed a surface area of 12.96 m g , total pore volume (at P/P = 0.900) 3 1 of 0.109 cm g and a mean pore diameter of 33.71 nm. The BET isotherm exhibited by ZnFe O @Chitosan is of type II, which suggests unrestricted monolayer–multilayer 2 4 adsorption that is common to mesoporous adsorbents [21]. The XRD diffraction (Figure 1c) showed the most intense peak at 2 = 35.61 with a plane spacing corresponding to Resources 2022, 11, 81 5 of 17 (311), which is the plane previously reported for ZnFe O particles [22] with other planes 2 4 corresponding to (110), (111), (134), (220), (222), (400), (422), (511), (440), (620), (533), (444), (642), (731) and (800), as seen in the pattern [22,23]. Equation (5) shows an expression from which the crystallite size of ZnFe O @Chitosan may be calculated considering its X-ray 2 4 line broadening from the reflections of (311) and Debye–Scherrer ’s formula [24]: Kl Resources 2022, 11, x FOR PEER REVIEW D = 6 of 19(5) b Cosq Figure 1. FTIR (a), BET (b), XRD (c) and TGA analysis (d) of ZnFe2O4@Chitosan. Figure 1. FTIR (a), BET (b), XRD (c) and TGA analysis (d) of ZnFe O @Chitosan. 2 4 The SEM micrograph is presented in Figure 2a, revealing district packs of particles on the surface of ZnFe2O4@Chitosan which may be seen to be homogeneous. The EDS result (Figure 2b) confirms the presence of carbon (c), oxygen (O), nitrogen (N), iron (Fe) and zinc (Zn) in the molecule of ZnFe2O4@Chitosan, while elemental surface mapping is shown in Figure 2c (C1–5). Resources Resources 2022 2022 , 11 , 11 , x FO , x FO R P R P EER EER R R E E VIEW VIEW 5 of 5 of 19 19 Resources 2022, 11, x FOR PEER REVIEW 5 of 19 −− 11 1b, which revealed a surface area of 12.96 m² g , total pore volume (at P/Po = 0.900) of 1b, which revealed a surface area of 12.96 m² g , total pore volume (at P/Po = 0.900) of −− 11 0. 0.10 109 cm 9 cm³³gg and and a me a mean an pore diame pore diametteerr of of 33.71 n 33.71 nm m. The BET . The BET iso isottherm exh herm exhiibited by bited by −1 1b, which revealed a surface area of 12.96 m² g , total pore volume (at P/Po = 0.900) of ZnFe ZnFe 22 O O 44@Chitosan is o @Chitosan is off type II, which type II, which suggests suggests uunnre ressttri rict cteedd monol monolaaye yer– r–mu multi ltillaayyeerr a add-- −1 0.109 cm³g and a mean pore diameter of 33.71 nm. The BET isotherm exhibited by sorp sorpttiion th on that at is com is comm mo on to n to m meesop sopo orous rous adsorb adsorben ents ts [2 [21] 1]. The X . The XR RD D dif difffrraact ction (F ion (Fiig gure ure 1c) 1c) ZnFe2O4@Chitosan is of type II, which suggests unrestricted monolayer–multilayer ad- showed the showed the most most in in tense tense peak peak at at 22θθ = 35 = 35 .6 .6 1° 1° wi wi tt h h a a p p ll aa n n e e sp sp aa cc ii n n g correspondi g correspondi ng t ng t o o ( ( 311 311 ), ), sorption that is common to mesoporous adsorbents [21]. The XRD diffraction (Figure 1c) which which is t is t h h e e pla pla n n e previously report e previously report ed for ZnFe ed for ZnFe 22 O O 44 particle particle s [22] with s [22] with oth oth ee r r p p ll anes anes corre corre -- showed the most intense peak at 2θ = 35.61° with a plane spacing corresponding to (311), sponding to (110), (111), (134), (220), (222), (400), (422), (511), (440), (620), (533), (444), (642), sponding to (110), (111), (134), (220), (222), (400), (422), (511), (440), (620), (533), (444), (642), which is the plane previously reported for ZnFe2O4 particles [22] with other planes corre- ((731 731)) aannd d (8 (800 00), as seen ), as seen iinn t thhe p e paattttern [2 ern [22, 2,2233]]. E . Eqquuaatition (5 on (5) ) shows shows an expr an express essiioonn from from sponding to (110), (111), (134), (220), (222), (400), (422), (511), (440), (620), (533), (444), (642), whi whicch t h thhe crysta e crystallllit ite siz e sizee of of ZnFe ZnFe 22 O O 44@ @C Chitosan m hitosan maay be c y be caalc lculated considerin ulated considering its X g its X--ray ray (731) and (800), as seen in the pattern [22,23]. Equation (5) shows an expression from line broadening from line broadening from the reflec the reflec tions o tions o ff (311) (311) and Deb and Deb y y e–Scherre e–Scherre r’s formula [24]: r’s formula [24]: which the crystallite size of ZnFe2O4@Chitosan may be calculated considering its X-ray Resources 2022, 11, 81 6 of 17 𝐾𝜆 𝐾𝜆 line broadening from the reflections of (311) and Debye–Scherrer’s formula [24]: (5 (5 )) 𝐷= 𝐷= 𝛽 𝛽 𝑜𝜃𝐶𝑠 𝑜𝜃𝐶𝑠 𝐾𝜆 (5) 𝐷= From Equation (5), D is the average crystallite size of ZnFe O @Chitosan, K represents From Equation (5), D is the average crystallite size of ZnFe2O 2 4@Chito 4 san, K represents From Equation (5), D is the average crystallite size of ZnFe2O4@Chitosan, K represents 𝛽 𝑜𝜃𝐶𝑠 a constant taken as 0.89. l is the X-ray wavelength (1.5406 Å), while and are the full aa cco ons nsta tant nt tak takeen n a ass 0. 0.89 89. . λλ is is the the X-r X-raay y wavelen waveleng gth th ( (11.5 .5440066 Å) Å), wh , while ile ββ and and θθ ar are e th the full e full From Equation (5), D is the average crystallite size of ZnFe2O4@Chitosan, K represents width of diffraction line at half of the maximum intensity (FWHM) and Bragg’s angle (at width width of diffr of diffr action line at ha action line at half of the lf of the m m aaxim xim u um in m inte tensity nsity (FW (FWH HM M)) an and Br d Bragg’ agg’ s s angle (at angle (at a constant taken as 0.89. λ is the X-r peak ay wavelen (311)), r gespectively th (1.5406 Å) [25 , wh ]. The ile β and crystallite θ are size the full for ZnFe O @Chitosan was found to 2 4 p peeak ak ( (3311 11)) )), , rreesp spect ectiiv veelly y [2 [25] 5]. The . The cr crys ysta talli llite te s siize ze for for Z Zn nFe Fe 22 O O 44@Chitosan @Chitosan w waas fo s found to und to be be width of diffraction line at half of the be m 35.14 axim nm. um in The tensity crystallite (FWHsize M) an isd Br important agg’s angle (at in understanding its diffusion properties. 35 35.1 .14 nm 4 nm. . Th The crys e crysttaalllliitte s e siize ze is is import importaan nt in t in unde unders rsttaandin nding i g ittss di diffffus usion proper ion propertie tiess. . Ap- Ap- Apparently, this can be expressed as [26,27]: peak (311)), respectively [25]. The crystallite size for ZnFe2O4@Chitosan was found to be parently, this can be expressed as [26,27]: parently, this can be expressed as [26,27]: 35.14 nm. The crystallite size is important in understanding its diffusion properties. Ap- 2 2 22 22 Ʈ Ʈ = r = r = r ᴫᴫD ( D ( D 66 (6))) parently, this can be expressed as [26,27]: where where Ʈ Ʈ i iss th the av e aveerraag ge e di diff ffusion usion tim timee of of charge charge c caarri rrier ers f s frrom om b bu ulk lk s so olu lution tion to to the the su surf rface ace 2 2 where Ʈ = r is the ᴫD ( average diffusion time of charge carriers6) from bulk solution to the surface of of ZnFe of ZnFe 22 O O 44 @ @ C C hitosan, hitosan, and and D represen D represen ts ts the d the d ii ffusion ffusion coefficien coefficien t o t o ff the ch the ch arge arge s. s. Accordin Accordin g g ZnFe O @Chitosan, and D represents the diffusion coefficient of the charges. According to 2 4 where Ʈ is the average diffusion time of charge carriers from bulk solution to the surface to the expression (Equation (6)), the larger the size of a catalyst, the longer the diffusion to the expression (Equation (6)), the larger the size of a catalyst, the longer the diffusion the expression (Equation (6)), the larger the size of a catalyst, the longer the diffusion time, of ZnFe2O4@Chitosan, and D represents the diffusion coefficient of the charges. According tim timee, wh , which ich m meeans ans th the m e moore s re su uscep sceptib tiblle e it it is is to to agg aggrrega egattion ion (rec (recombinat ombinatiion on eeffec ffectt)). Such . Such which means the more susceptible it is to aggregation (recombination effect). Such recombi- to the expression (Equation (6)), the larger the size of a catalyst, the longer the diffusion recom recomb bina inattio ion le n leads ads to to de decreas creaseed c d caattaally ytic tic p prrop oper erty ty [2 [27, 7,2288]. ]. It It is is i im mp po ortan rtant t th thaatt the cr the crys ys-- nation leads to decreased catalytic property [27,28]. It is important that the crystallite size time, which means the more susceptible it is to aggregation (recombination effect). Such ta tallllitite e si size ze i iss smal small.l. The The cr cryst ystaalllliittee s siize ze of ZnF of ZnFee 22 O O 44@ @C Chitos hitosaann f faallllss w wiith thing ing the the r raange nge of of is small. The crystallite size of ZnFe O @Chitosan falls withing the range of previously 2 4 recombination leads to decreased catalytic property [27,28]. It is important that the crys- p prrev evious iously ly rreep po orted rted ssiizes ( zes (37 to 4 37 to 455 nm nm) for ) for sp spin inel ferr el ferrite [ ite [2299]], sug , sugg geest sting a ing a good good cat cataalys lystt reported sizes (37 to 45 nm) for spinel ferrite [29], suggesting a good catalyst functional tallite size is small. The crystallite size of ZnFe2O4@Chitosan falls withing the range of func func tion tion al al s s ii zz ee for for ZnFe ZnFe 22 O O 44 @Chito @Chito san san . . size for ZnFe O @Chitosan. 2 4 previously reported sizes (37 to 45 nm) for spinel ferrite [29], suggesting a good catalyst The thermal degradation is shown in Figure 1d, which showed three major losses. The thermal degradation is shown in Figure 1d, which showed three major losses. The thermal degradation is shown in Figure 1d, which showed three major losses. The functional size for ZnFe2O4@Chitosan. The firs The first t loss loss at r at raang nge 0 e 0––118800 °C °C i iss ab abou out t 5. 5.58% 58%, which , which was was at attrib tribut uted to ed to a los a losss o off v voola lattile ile first loss at range 0–180 C is about 5.58%, which was attributed to a loss of volatile and The thermal degradation is shown in Figure 1d, which showed three major losses. and and adso adsorb rbed ed wa water m ter mo olec lecu ule les. Th s. This is is is ffo ollowed llowed b by y a a second m second maajor jor los losss a att ran rang gee 2 21100––415 415 adsorbed water molecules. This is followed by a second major loss at range 210–415 C, The first loss at range 0–180 °C is about 5.58%, which was attributed to a loss of volatile °C, wh °C, wh ich ich is is 11 77 .41% .41% of of tot tot aa ll mas mas ss and and wa wa s s at at trib trib ut ut ed ed tt o o the the decomp decomp osi osi tt ion ion of of the the chito chito ss an an which is 17.41% of total mass and was attributed to the decomposition of the chitosan and adsorbed water molecules. This is followed by a second major loss at range 210–415 str stru ucture w cture wiith loss o th loss off H H 22O, O, N NH H 33, CO , CO, CO , CO 22 and C and CH H 33C COOH, which OOH, which was considered to be was considered to be structure with loss of H O, NH , CO, CO and CH COOH, which was considered to be 2 3 2 3 °C, which is 17.41% of total mass and was attributed to the decomposition of the chitosan pyrrolic degradation of chitosan as previously reported [30,31]. Moreover, previous study ppyrr yrroli olic c degr degradation adation of ch of chitosan itosan aas s ppr rev eviou iouslsly y rep reported orted [3 [0, 30 3,1 31 ]. ]. Mor Mor eov eover er, p , pr rev evious ious ststudy udy structure with loss of H2O, NH3, CO, CO2 and CH3COOH, which was considered to be has has shown shown th that at the the degr degrad adat ation o ion off chi chitto ossan an can can ta take ke p pllace ace b by y ran rand dom om b brrea eaking king of of the the C C-- has shown that the degradation of chitosan can take place by random breaking of the pyrrolic degradation of chitosan as previously reported [30,31]. Moreover, previous study 1 −− 11 O- O- C C skel skel eta eta ll bond bond [30 [30 –33 –33 ]] , ,whi whi cc h h wa wa s s seen seen ii n n t t h h e FTIR e FTIR result result ( ( F F ii g g ure 1 ure 1 a a )) at at 10 10 27 cm 27 cm . The . The C-O-C skeletal bond [30–33], which was seen in the FTIR result (Figure 1a) at 1027 cm . has shown that the degradation of chitosan can take place by random breaking of the C- thir thir The d im d im thir p po d ort rt important aan nt los t losss in in loss the the range in range the 4 range 41155––1100 415–1000 00 00 °C °C acco accoun C unts fo accounts ts for 2 r 266.3 .3 for 0% 0% 26.30% loss o loss off the the lossto to of ttaal m the l maa total ss ss, , −1 O-C skeletal bond [30–33], which was seen in the FTIR result (Figure 1a) at 1027 cm . The which ma which ma mass, which y b y bee may a attr ttribu be ibu attributed tted ed ttoo loss loss to of C of C lossH H of 44 th th CH at w at w that aass co was consider nsider consider ed ed to h to h ed to aavv have ee ta taken p ken p takenlla place acce v e viia via a a a a third important loss in the range 415–1000 °C accounts for 26.30% loss of the total mass, dehydrogenation mechanism as previously reported [30,34,35]. dehydrog dehydrog enation m enation m ee chan chan ism as pr ism as pr evio evio usly repor usly repor tt ed ed [30,34,35]. [30,34,35]. which may be attributed to loss of CH4 that was considered to have taken place via a The SEM micrograph is presented in Figure 2a, revealing district packs of particles on dehydrogenation mechanism as previously reported [30,34,35]. the surface of ZnFe O @Chitosan which may be seen to be homogeneous. The EDS result 2 4 (Figure 2b) confirms the presence of carbon (c), oxygen (O), nitrogen (N), iron (Fe) and zinc (Zn) in the molecule of ZnFe O @Chitosan, while elemental surface mapping is shown in 2 4 Figure 2c (C ). 1–5 The magnetic property of ZnFe O @Chitosan was investigated using vibration sample 2 4 magnetometry and the results are presented in Figure 2d with magnetic hysteresis loop, indicating that ZnFe O @Chitosan is magnetic. The saturation magnetization is found 2 4 to be 2.38 emu g , which is large enough for magnetic separation for practical applica- tions. Previous study has reported a high saturation magnetization [22,36,37] for ZnFe O ; 2 4 however, the observed low saturation magnetization in ZnFe O @Chitosan compared to 2 4 previous reports may be due to the immobilization of ZnFe O on chitosan, which may 2 4 have altered the inversion degree of ZnFe O . 2 4 The UV-visible spectrum is shown in Figure 3a, revealing absorbance in the visible region, which suggests that ZnFe O @Chitosan may have photocatalytic activity in the 2 4 visible-light region. The optical bandgap was determined from the Tauc plot method, as shown in Figure 3b; this was determined as described for a transition-type semiconductor (Equation (7): (µ hv) = A hv E (7) where hv is the frequency of incident light, A represents the proportionality constant, E is the bandgap and is the absorption coefficient. The bandgap for ZnFe O @Chitosan was 2 4 found to be 2.98 eV, which further corroborates the fact that ZnFe O @Chitosan may be 2 4 active for photodegradation within the visible-light region. Resources 2022, 11, 81 7 of 17 Resources 2022, 11, x FOR PEER REVIEW 7 of 19 Figure 2. SEM (a), EDS (b), surface mapping (c) and VSM analysis (d) of ZnFe2O4@Chitosan. Figure 2. SEM (a), EDS (b), surface mapping (c) and VSM analysis (d) of ZnFe O @Chitosan. 2 4 The magnetic property of ZnFe2O4@Chitosan was investigated using vibration sam- 3.2. Photodegradation Study ple magnetometry and the results are presented in Figure 2d with magnetic hysteresis The time-dependent degradation of CIP, AMP and ERY by ZnFe O @Chitosan at a 2 4 loop, indicating that ZnFe 21 O4@Chitosan is magnetic. The saturation magnetization is concentration of 5.00 mg L is presented in Figure 4a. The percentage degradation was −1 found to be 2.38 emu g , which is large enough for magnetic separation for practical ap- in the following order of efficiency: CIP (99.80 0.20%) > AMP (94.50 0.10%) > ERY plications. Previous study has reported a high saturation magnetization [22,36,37] for (83.20 0.20%). The photodegradation reached equilibrium after 150 min of treatment. ZnFe2O4; however, the observed low saturation magnetization in ZnFe2O4@Chitosan com- The degradation efficiency exhibited by ZnFe O @Chitosan towards the antibiotics might 2 4 pared to previous reports may be due to the immobilization of ZnFe2O4 on chitosan, which be molecular weight-dependent since the highest efficiency was found in CIP having the may have altered the inversion degree of ZnFe2O4. lowest molecular weight and the least efficiency found in ERY having the highest molecular The UV-visible spectrum is shown in Figure 3a, revealing absorbance in the visible weight. The molecular weight is in the increasing order of CIP (331.347 g mol ) < AMP 1 1 region, which suggests that ZnFe2O4@Chitosan may have photocatalytic activity in the (349.406 g mol ) < ERY (733.930 g mol ). The molecular structures of the antibiotics are visible-light region. The optical bandgap was determined from the Tauc plot method, as shown in Figure 3c–e; the lower the molecular weight, the higher the degradation efficiency shown in Figure 3b; this was determined as described for a transition-type semiconductor expressed by ZnFe O @Chitosan. The dark experiment revealed that adsorption was tak- 2 4 ing (Equation ( place at7the ): same time with the photocatalytic degradation. Therefore, the adsorption capacities as well as the percentage removal with time are presented in Figure 4b–d. The (∝ ℎ