# Recent Overview of Solar Photocatalysis and Solar Photo-Fenton Processes for Wastewater Treatment

Authors: A. G. Gutierrez-Mata; S. Velazquez-Martínez; Alberto Álvarez-Gallegos; M. Ahmadi; José Alfredo Hernández-Pérez; F. Ghanbari; S. Silva-Martínez
Journal: International Journal of Photoenergy
 (2017)

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## Abstract

This literature research, although not exhaustive, gives perspective to solar-driven photocatalysis, such as solar photo-Fenton andTiO2 solar photocatalysis, reported in the literature for the degradation of aqueous organic pollutants. Parameters that influence the degradation and mineralization of organics like catalyst preparation, type and load of catalyst, catalyst phase, pH, applied potential, and type of organic pollutant are addressed. Such parameters may also affect the photoactivity of the catalysts used in the studied solar processes. Solar irradiation is a renewable, abundant, and pollution-free energy source for low-cost commercial applications. Therefore, these solar processes represent an environmentally friendly alternative mainly because the use of electricity can be decreased/avoided.


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## Body

## 1. Introduction

The use of solar irradiation to detoxify contaminated effluents has recently increased and become of utmost importance for saving energy and to improve the performance of several degradation aqueous processes. Solar photocatalysis and solar photo-Fenton technologies are classified into advanced oxidation processes (AOP). The AOP involve the in situ generation of highly oxidizing radical species such asOH• by using different energy sources like chemical, natural (solar), and artificial light energy. The hydroxyl radicals, OH•, are capable of transforming toxic and persistent organic compounds into harmless end products (CO2 and mineral acids) [1]. The interaction of solar irradiation with catalysts such as iron ions (Fe3+), in photo-Fenton, and TiO2, in photocatalysis, increases the rate of pollutant degradation by the photochemical reactions produced within these processes.These two AOP have proved to be very effective for degrading a vast aqueous organic contaminants such as emerging [2, 3], persistent [4–9], textiles [10–13], and bacteria [14–16] pollutants.This literature research, although not exhaustive, gives perspective to solar photo-Fenton, solar photoelectro-Fenton, andTiO2 solar photocatalytic processes reported in the literature for the degradation of aqueous organic pollutants. Solar irradiation is a renewable, abundant, and pollution-free energy source for low-cost commercial applications. Parameters that influence the degradation and mineralization of organics that may also affect the photoactivity of the catalysts used in the studied solar processes are addressed.


## 2. Fenton Processes

Fenton oxidation process consists of the reaction betweenH2O2 and Fe2+ (1) in acidic solution to produce hydroxyl radicals OH•, highly oxidant species responsible for pollutant degradation [17–19]:
(1)H2O2+Fe2+→Fe3++OH•+OH−k=63M−1s−1.Following a chain reaction [20–26]:
(2)Fe3++H2O2→Fe2++HO2•+H+k=1×10−2M−1s−1,(3)OH•+H2O2→HO2•+H2Ok=2.7×107M−1s−1,(4)OH•+Fe2+→Fe3++OH−k=3.2×108M−1s−1,(5)Fe3++HO2•→Fe2++O2+H+k=3.1×105M−1s−1,(6)Fe2++HO2•+H+→Fe3++H2O2k=1.2×106M−1s−1,(7)HO2•+HO2•→H2O2+O2k=8.3×105M−1s−1,(8)HO2•+H2O2→OH•+H2O+O2k=3M−1s−1.However, according to Pignatello and collaborators [19], reaction (8) is very slow compared to those involving HO2• species and can be neglected.The reaction betweenH2O2 and Fe3+ (2), referred to as Fenton-like reaction, produces less oxidant radical species (HO2•); nevertheless, both ferric and ferrous ion species are present simultaneously in the chain reaction (reactions (1)–(7) regardless of which is used to initiate the reaction. Thus, the H2O2 can be catalytically decomposed by Fe3+/Fe2+ into oxidant radical species [19]. The homogeneous catalytic decomposition of H2O2 by ferric ions may be also represented by [27–29]
(9)Fe3++H2O2↔FeHO22++H+k=3.1×10−3,FeHO22+↔Fe2++HO2•k=2.7×10−3s−1.The photo-Fenton process increases the amount ofOH• radicals with Fe2+ regeneration (11) by the photoreduction of FeOH2+, produced in (reaction (10)) which maxima concentration is at pH ~3.1 [28, 30]:
(10)Fe3++H2O→FeOH2++H+K=2.89×10−3M−1,(11)FeOH2++hvλ<400nm→Fe2++OH•Thus, solar light irradiation (UV/visible irradiation) promotes photochemical reactions with light active intermediate species, such asFeOH2+; reaction (11) produces hydroxyl radicals and regenerates Fe2+ which close the catalytic cycle of OH• generation via reaction (1). This light enhancement has been explained mainly by photolysis of hydroxide complexes of Fe3+ (reaction (11)) and photochemical reactions of ligand complexes formed between Fe3+/Fe2+ and organic acids (ferric carboxylic complexes) such as oxalic citric acids [31, 32]. Nevertheless, the rate of photolysis of ferric carboxylic complexes can be several orders higher than that of hydrated ferric ions, FeOH2+ (reaction (11)) [33, 34]. Enhancement of the photo-Fenton reaction with the use of these ligand complexes was attributed to their higher solubility and higher stability constant than that of iron-organic pollutant complexes and high photoactivity under UV-visible light by increasing the quantum yield for Fe2+ production [35].Table1 summarizes the experimental degradation of several organic contaminants by solar photo-Fenton. It is shown that the oxidation degree, or mineralization, depends on several parameters like the type of reactor used, pH, initial concentration of the organic contaminant, degradation time, among some others. The oxidation of the organic matter with time was followed by parameters like DOC, TOC, COD, and organic concentration decrease.Table 1
Solar photo-Fenton treatment.
Contaminant (concentration interval)
Experimental conditions
Reactor type (volume)
Best degradation conditions
Reference
Catalyst (pH)
Percentage (time)
Herbicide 2,4-dichlorophenoxy acetic acid (0.13 mM L−1)
1 mg L−1 Fe3+ (3.0)
The nonconcentrating solar photoreactor (35 L)
Total organic carbon conversion of 98.9% (at 210 min)
[100]
Reactive blue 4 (RB4) (25 mg L−1)
9.4 mg L−1 Fe2+ (2.0)
CPC (50 L)
Total discoloration, 82% and 23% of COD and TOC removal, respectively (at 60 min)
[52]
Reactive blue 4 (RB4), (25 mg L−1)
7 mg L−1 Fe2+ and 10 mg L−1 of oxalic acid (2.5)
CPC (50 L)
Total discoloration and COD removal were achieved whereas 66% of TOC was eliminated (at 50 min)
[52]
Emerging contaminants such as acetaminophen, antipyrine, atrazine, caffeine, carbamazepine, diclofenac, flumequine, hydroxybiphenyl, ibuprofen, isoproturon, ketorolac, ofloxacin, progesterone, sulfamethoxazole, and triclosan (100μg L−1 each, dissolved in methanol at 2.5 g L−1; this was the mother solution)
5 mg L−1 Fe2+ (no pH adjustment)
CPC (35 L)
~25% TOC mineralization (300 min)
[2]
Electro-optical industry wastewater (563–593 mg L−1 of COD)
256 mg L−1 Fe2+ (3.0)
Fresnel lens assisted inclined plate curvature channel reactor (8 L)
The COD of the wastewater could reach a reduction of 85–90% (at 60 min)
[101]
Hierbamina or 2,4 dichlorophenoxyacetic acid, 2,4-D and gesaprim or 90% atrazine, ATZ (80 mg L−1 of TOC, 90 mg L−1 ATZ, and 50 mg L−1 2,4-D)
10 mg L−1 Fe2+ (2.7–2.9)
CPC (40 L)
~60% mineralization, 20 mg L−1 remainingTOC (at 120 min)
[82]
Alachlor, atrazine, chlorfenvinphos, diuron, and isoproturon (80 mg L−1 of TOC or 30 mg/L each)
10 mg L−1 Fe2+ (2.7–2.9)
CPC (75 L)
~80% TOC mineralization (at 100 min)
[184]
Ofloxacin-OFX and trimethoprim-TMP (100μg L−1 each produce no more than 0.1 mg L−1 of DOC)
5 mg L−1 Fe2+ (2.8–2.9)
CPC (250 L)
~21% DOC removed and ~50% COD abatement (at 180 min)
[102]
Water from a natural source (Pance River in Cali, Colombia) and spiked withE. coli (5.5 mg L−1 of TOC and E. coli 106 CFU mL−1)
0.6 mg L−1 Fe3+ (6.5)
CPC (20 L)
~55% TOC reduction and totalE. coli inactivation (at 6 h)
[103]
Azo dye orange II (20 mg L−1)
2 mg L−1 Fe2+ and 60 mg L−1 oxalic acid [H2C2O4] (3.0)
CPC (50 L)
100% decoloration of dye solution and 95% TOC removal (at 80 W h of accumulated solar energy)
[185]
Herbicide tebuthiuron (THB) (0.5 mmol L−1)
0.5 mmol L−1 of potassium ferrioxalate K3Fe(C2O4)3 3H2O (2.5)
Shallow pond type solar flow reactor (20 L)
~58% TOC removal (at 60 min)
[186]
Pesticide 3-chloropyridine (40 mg L−1)
0.88 mM L−1 Fe2+ (2.8)
CPC (30 L)
Complete mineralization (at 150 min)
[187]
Herbicide tebuthiuron-TBH (0.5 mM L−1 or 54 mg L−1 of TOC)
Fe(NO3)3 and citric acid at the same molar iron-to-ligand ratio 1 : 1 at 1.0 mM L−1 (2.5–7.5)
Open dark-glass vessels 4.5 cm deep (250 mL)
20% and 85% of TOC were removed at pH 7.5 and 2.5, respectively (at 45 min)
[104]
Phenol (50 mg L−1)
0.07 g L−1impure bismuth ferrite (BiFeO3) nanoparticles (2.5)
Erlenmeyer flask with mixing rate of 400 rpm (100 mL)
~97% was removed (60 min)
[188]
Antibiotic sulfamethoxazole (SMX) (50 mg L−1 or 23.75 mg C L−1 of DOC)
5.2 mg L−1 Fe2+ (2.5–2.8)
CPC (39 L)
SMX was completely decomposed. ~80% DOC removal or 5 mg C L−1 residual (16 min)
[189]
Vydate®—10% oxamyl, Metomur®—20% methomyl, Couraze®—20% imidacloprid, Ditimur-40®—40% dimethoate, and Scala®—40% pyrimethanil, (200 mg L−1 of DOC or 40 mg L−1 of each commercial pesticide)
20 mg L−1 Fe3+ (2.7–2.9)
CPC (75 L)
~50% DOC mineralization (180 min)
[105]
Citrus wastewater (CODinitial of 10,000 mg O2 L−1)
510 mg L−1 Fe3+ (3.6–4.5)
Batch systems in quartz flasks (100 mL)
COD and DOC removal 76.9% and 53.3%, respectively (at 30 min)
[190]
Pesticide acetamiprid (ACTM) (100μg L−1)
0.095 mM L−1 Fe2+ (2.8)
Fiberglass raceway pond reactor (360 L)
90% ACTM removal expressed in concentration, from 4.49 · 10−4 mM to 4.49 · 10−5 mM (90 min)
[191]
Inactivation ofFusarium solani spore (spore concentration greater than 103 CFU mL−1)
10 mg L−1 Fe2+ (3.0)
Sterile glass bottles (250 mL)
To achieve over 99.9% ofF. solani inactivation (at 4.20 kJUV L−1 of accumulated energy)
[192]
Enterococcus faecalis model (microorganism concentration of 106 CFU mL−1)
20 mg L−1 Fe2+ (8.0)
Jacketed stirred tank reactors (1.25 L)
Complete water disinfection (100 min)
[106]
Synthetic cotton-textile dyeing wastewater (100 mg C L−1 of DOC or 250 mg O2 L−1 of COD)
40 mg L−1 Fe3+ iron/oxalate molar ratio 1 : 3 (4.0)
CPC (40 L)
98.3% of colour removal, 14.2 mg C L−1 of residual DOC and 57 mg O2 L−1 of remnant COD are achieved (at 3.2 kJUV L−1 of accumulated energy)
[53]
Metronidazole (MTZ) (960 mg L−1 COD0)
1 mmol L−1 Fe2+ (3.0)
A rectangular mirror glass (50 × 80 cm) on which is placed in parallel at 5 mm a glass plate of the same size (1 L)
~96% COD removal (12 min)
[83]
Synthetic aqueous wastes polluted with safflower oil (70 mg L−1)
1 mM L−1 (2.6)
System with five DuranTM tubes, a Pyrex glass reservoir, a recirculation pump, and a planar aluminum surface under solar radiation (2.5 L)
The COD was abated smoothly up to 68% COD decrease after 90 min of Fenton reaction (1.6 h)
[193]The main disadvantages of the Fenton process are (i) the pH of the solution (its optimum conditions is obtained at pH 2.8), (ii) sludge formation which depends on the amount and type of iron used, and (iii) H2O2 storage and handling and its associated cost.


### 2.1. The Electrochemical Fenton-Based (EF) Processes

The electrochemical Fenton-based (EF) processes, included in the electrochemical advanced oxidation processes, were developed to overcome the drawbacks of the classical Fenton (CF) process. These processes in situ generate the Fenton reagents (H2O2 and/or Fe2+) to yield OH• radicals [36, 37]. The EF processes such as Fered-Fenton (EF-FeRe) [38, 39], electrochemical peroxidation/anodic Fenton (EF-FeOx) [40–42], electro-Fenton (EF-H2O2-FeRe) [38, 43], and peroxi-coagulation (EF-H2O2-FeOx) [44, 45] increase the efficiency of pollutant degradation. The efficiency of pollutant degradation is enhanced when UV light or solar irradiation is used in combination with CF (photo-Fenton or solar photo-Fenton) and EF (photoelectro-Fenton or solar photoelectro-Fenton) processes. Figure 1 schematically shows CF and EF processes: (1) CF: addition of both reagents to the solution, (2) EF-FeRe: addition of both reagents to the solution with the regeneration of Fe2+ from reaction (13), (3) EF-FeOx: generation of iron anions using a sacrificial iron anode with the addition of hydrogen peroxide, (4) EF-H2O2-FeRe (the most common electrochemical Fenton-based process, known as electro-Fenton): generation of hydrogen peroxide and regeneration of initially added Fe2+ catalyst, (5) EF-H2O2-FeOx: in situ generation of both hydrogen peroxide and iron anions, and finally, (6) CF and EF combined with UV light or solar irradiation.Figure 1
Classical Fenton (CF) and electrochemical Fenton (EF) oxidation processes: (1) CF, (2) Fered-Fenton (EF-FeRe), (3) electrochemical peroxidation/anodic Fenton (EF-FeOx), (4) electro-Fenton (EF-H2O2-FeRe), (5) peroxi-coagulation (EF-H2O2-FeOx), and (6) UV-CF/UV-EF.The hydrogen peroxide is generated in situ from the two-electron oxygen reduction on cathodes such as reticulated vitreous carbon [46], gas diffusion electrodes [47], carbon felt [48, 49], pristine graphene [50], and boron-doped diamond [51] from reaction (12), and Fe2+ can be electrochemically regenerated, if it was initially added to the solution (reaction (13)) or electrochemically generated from a sacrificial iron anode (reaction (14)).
(12)O2+2H++2e−→H2O2(13)Fe3++e−→Fe2+(14)Fe−2e−→Fe2+


### 2.2. Solar Photoelectro-Fenton

The conventional photo-Fenton reaction showed a limited efficiency in the mineralization of real textile wastewater mainly associated to three factors [10, 35, 52–55]: (i) formation of iron-organic pollutant complexes with low solubility at acidic pH values (2.8), leading to iron precipitation and abatement of dissolved organic carbon, cannot be associated with mineralization; (ii) low photoactivity of the iron-organic pollutant complexes under UV-visible light; and (iii) photoreduction via a ligand-to-metal charge mechanism, which occurs on the surface of the iron precipitates, is very slow.The photo-Fenton reaction can be enhanced by the following:(1)
The use of different iron(III)-organic ligand complexes such as Fe(III)-oxalate, Fe(III)-citrate and Fe(III)-EDDS (EDDS: S,S′-ethylenediamine-N,N′-disuccinic acid tri-sodium salt). These ligand complexes have higher solubility and higher stability constant than iron-organic pollutant complexes which prevent iron precipitation that allows to achieve proper mineralization. The superiority of Fe(III)-oxalate over Fe(III)-citrate and Fe(III)-EDDS complexes can be mainly associated to the different quantum yield values for Fe(II) production and the half-life of the Fe(III)-organic ligand complexes under UVA radiation. The photo-Fenton reaction mediated by ferricarboxylates was characterized by an initial fast reaction rate, mainly associated to the fast regeneration ofFe3+ to Fe2+, enhanced by the photodecarboxylation of ferricarboxylate complexes under UV-visible light, followed by a very slow reaction rate with a low consumption of H2O2 due to the disappearance of oxalic acid and free iron species complex with other organic oxidation by-products which reduced substantially the dissolved iron concentration and consequently the reaction rate [35].(2)
The use of electricity to drive the photo-Fenton process electrochemically (photoelectro-Fenton (PEF)) under sunlight [56]. The PEF process accelerates the degradation of pollutants because of (a) the enhancement of Fe2+ regeneration and OH• production by the photolytic reaction (11) and (b) the photolysis of Fe-complexes with generated intermediates like carboxylic acids by reaction (15) [57–59]:(15)FeOOCR2+→hvFe2++R•+CO2An interesting comparison of the performance of solar photo-Fenton and solar photoelectro-Fenton experiments, at laboratory scale, was carried out by Serra and collaborators [60]. These authors studied the degradation of the amino acid a-methylphenylglycine (a soluble and nonbiodegradable target pollutant) and observed that the solar-driven photo-Fenton is the most environmentally friendly alternative, mainly because of the use of electricity in the solar photoelectro-Fenton experiments [60]. Indeed, the solar photoelectro-Fenton (SPEF) process can be driven by a photovoltaic system when scale up to a pilot plant or solar plant to decrease the costs associated with the consumption of electricity, which may make sustainable the whole process. Having this in mind, a self-sustainable SPEF, driven by a photovoltaic cell, was designed to study the oxidation of the antibiotic trimethoprim (TMP), producing a high degree of mineralization. Tenaromatic intermediates generated from hydroxylation, carbonylation, and demethylation reactions were identified together with three carboxylic acids (oxamic, oxalic, and formic acids) and two inorganic ions (NH4+ and NO3−). This study is a cost-effective approach for TMP degradation and demonstrated that the sunlight can provide the electric power (for mechanical systems) and the UV radiation for SPEF process [61].Almeida and coworkers [62] studied the degradation of paracetamol by solar photoelectro-Fenton using a flow plant with a Pt/carbon-PTFE air-diffusion electrochemical cell (one-compartment filter-press reactor) coupled with a compound parabolic collector. The H2O2 was electrogenerated from the cathodic O2 reduction at the carbon-PTFE air-diffusion electrode (ADE). These authors reported 75% of total organic carbon (TOC) decrease with an energy cost of 93 kWh kg−1 TOC (7.38 kWh m−3) and 71% removal efficiency. 80% TOC removal was the maximum value acquired at 150 min, with conversion of 79% of initial N into NH4+ ion. Thus, according to these authors, total mineralization of paracetamol was not attained because of the formation of N− derivatives and other undetected products that cannot be destroyed by radical OH• and UV light. The same solar flow plant used by Almeida et al. was employed to oxidize azo dyes [63] and the antibiotic metronidazole [64] by electro-Fenton (EF) and solar photolectro-Fenton (SPEF) processes. Ruiz and coworkers observed that the EF process yielded rapid decolorization with poor TOC removal, and Pérez et al. also reported very weak mineralization of the antibiotic. These results were attributed to the formation of persistent carboxylic acids like oxalic acid as the major component of final electrolyzed solutions; conversely, quick photolysis of Fe(III)-oxalate complexes by UV light of solar irradiation explained the higher oxidation power of SPEF that gave almost total mineralization of the organic contaminants under study. It was described that the incident UV light played an important role in the photodecomposition of several N-derivatives that favored the release of ammonium ions and the loss of volatile N-compounds. Espinoza and coworkers [65] reported that the elimination of an diazo dye (acid yellow 42 dye) and its organic intermediates was due to hydroxyl radicals formed both at the anode surface from water oxidation and in bulk solution from Fenton reaction between electrogeneratd H2O2 and added Fe2+. The application of solar radiation in the photolectro-Fenton process yielded higher current efficiencies and lower energy consumptions than electro-Fenton (EF) and electro-oxidation, with electrogenerated H2O2 by the additional production of hydroxyl radicals from the photolysis of Fe(III)-hydrated species (reaction (11)), and the photodecomposition of Fe(III)-complexes with organic intermediates (ferric carboxylic complexes, like ferric oxalate) that pass through an excitation state under the influence of photons of UV/vis wavelengths. This reaction is called the ligand-metal charge transfer reaction [66–68]:
(16)FeC2O4n3−2n+→hvFe2++n−1C2O42−+C2O4•−Table2 summarizes the experimental degradation of several organic contaminants by solar photoelectro-Fenton. It is shown that the oxidation degree, or mineralization, depends on several parameters like the type of reactor used, pH, initial concentration of the organic contaminant, degradation time, among some others. The oxidation of the organic matter with time was followed by parameters like DOC, TOC, COD, and organic concentration decrease.Table 2
Solar photoelectro-Fenton.
Contaminant (concentration interval)
Experimental conditions
Reactor type (volume)
Best degradation conditions
Reference
Catalyst (pH)
Electrochemical cell (current density)
Percentage (time)
Paracetamol (157 mg L−1)
0.4 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (50 mA cm−2)
CPC (10 L)
~80% TOC removal (at 150 min)
[62]
Acid yellow (AY9) azo dye (200 mg L−1 TOC)
0.5 mM L−1 Fe2+ (3.0)
Boron-doped diamond (BDD)/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom and inclined 30° (2.5 L)
~93% TOC removal (at 360 min)
[63]
Salicylic acid (165 mg L−1 or 100 mg L−1 of TOC)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (3.0 L)
~59% TOC removal (at 360 min)
[194]
Monoazo acid orange 7 (50 mg L−1 of DOC)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (55.4 mA cm−2)
CPC (10 L)
~97% DOC abatement (at 180 min)
[69]
o-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~90% TOC removal (at 120 min)
[195]
m-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~89% TOC removal (at 120 min)
[195]
p-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~87% TOC removal (at 120 min)
[195]
Heterocyclic antibiotic metronidazole (1.39 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
Pt/air-diffusion (55.4 mA cm−2)
CPC (10 L)
~53% DOC removal (at 300 min)
[64]
Disperse red 1 (DR1) (0.520 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
BDD/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC abatement of 84% (at 240 min)
[84]
Disperse yellow 3 (DY3) (0.558 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
BDD/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC abatement of 86% (at 240 min)
[84]
Ibuprofen (41 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
BDD anode/O2-diffusion cathode (33.3 mA cm−2)
Open-cell compartment (0.1 L)
88% DOC removal (at 120 min)
[43]
Acid orange 7 (AO7) (150 mg L−1 of TOC)
0.75 mM L−1 Fe2+ (3.0)
Pt sheet and a carbon-PTFE air-diffusion electrode. (40 mA cm−2)
CPC (10 L)
TOC was reduced by 96% (at 360 min)
[196]
Acid yellow 42 (AY42) (100 mg L−1 of TOC)
1.0 mM L−1 Fe2+ (3.0)
Boron-doped diamond (BDD) anode and an air diffusion cathode (ADC) (50 mA cm−2)
CPC (8 L)
~80% TOC removal (at 270 min)
[65]
Organic matter present in slaughterhouse wastewater (52 mg L−1 of TOC)
1.0 mM L−1 Fe2+ (3.0)
Si/BDD thin-film anode and carbon-PTFE air-diffusion cathode (50 mA cm−2)
Open-cell compartment (0.1 L)
4 mg L−1 of total organic carbon (TOC) (at 240 min)
[91]
Pharmaceutical ranitidine (112.6 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt sheet anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
67% TOC removal (at 360 min)
[197]
Antibiotic trimethoprim (200 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
RuO2/Ti mesh electrodes (18 mA cm−2)
Cylindrical quartz cell (125 mL)
80% TOC decay (at 360 min)
[61]
Allura red AC azo dye (460 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt sheet anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
A planar solar photoreactor (2.5 L)
97% TOC decay (at 180 min)
[85]
Sulfanilic acid (240 mg L−1 or 100 mg L−1 of TOC)
0.5 mM L−1 Fe2+ (4.0)
Pt/air-diffusion (100 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC was reduced by 76% (at 120 min)
[56]
Chloramphenicol (2,2-dicloro-N-[1,3-dihydroxy-1-(4-nitrophenyl)propan-2-yl] acetamide) (245 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion filter-press cell (100 mA cm−2)
CPC (10 L)
DOC was reduced by 89% (at 180 min)
[86]
Sunset yellow FCF azo dye (290 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/carbon-PTFE air-diffusion cell (77.6 mA cm−2)
CPC (10 L)
TOC was reduced by 94% (at 150 min)
[198]
Sulfanilamide (239 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/carbon-PTFE air-diffusion cell (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
DOC decay of 91% (at 180 min)
[199]
Tebuthiuron (0.18 mM L−1)
0.5 mM L−1 Fe2+(3.0)
BDD anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
Solar flow plant (2.5 L)
75% TOC removal (at 360 min)
[200]
A sanitary landfill leachate previously subjected to biological and coagulation processes (337–430 mg L−1 of DOC)
60 mg L−1 Fe3+ and oxalic acid to get Fe(III)-to-oxalate molar ratio of 1 : 3 (2.8)
BDD anode and a carbon-PTFE air-diffusion cathode (200 mA cm−2)
Lab-scale flow plant (2.2 L)
DOC decay of 80% (at 300 min)
[201]
Atrazine (20 mg L−1)
0.1 mM L−1 Fe2+ (3.0)
BDD thin-film electrode on Nb (13.33 mA cm−2)
In an open, undivided and cylindrical tank reactor (200 mL)
TOC reduction of 70% (at 300 min)
[202]


### 2.3. Influencing Parameters on the Degradation of Organic Compounds by Solar Photoelectro-Fenton Process

Complete transformation of organic compounds toCO2 by the solar photoelectro-Fenton process depends directly on the applied current density, the concentration of catalyst, organic concentration, and the solar radiation intensity [65, 69, 70]. There are other parameters like pH of the solution, temperature, and electrode materials that are important too in the photoelectro-Fenton process; however, Fenton reaction is efficient at the pH interval of 2.5 < pH < 3 [7, 71–73], oxygen is needed to produce H2O2, and its solubility is affected by the temperature [74]; thus, it is better to perform the experiment at room temperature, and the electrode materials like carbonaceous cathodes [46, 48–50] and BDD anodes [56, 75] have been proved to be the best materials (to reduce oxygen and to produce OH• radicals, resp.) so far.


#### 2.3.1. Current Density Influence

The current density (or voltage cell) applied to the electrochemical cell forH2O2 production in the photoelectro-Fenton process influences the electrode surface reaction kinetics and the extension of electrode reactions. Hydroxyl radicals are in situ generated in the photoelectro-Fenton process. Such oxidant species can be produced simultaneously via oxygen cathodic reduction (reaction (12)) in the presence of catalyst (reactions (1) and (8)) and on the anode boron-doped diamond (BDD) [75]:
(17)BDD+H2O→BDDOH•+H++e−B
D
D
O
H
• enhances the destruction of aromatic pollutants and their aliphatic intermediates such as short-linear carboxylic acids [56]. Thus, the oxidation power of the solar photoelectro-Fenton is additionally enhanced by reactions (11) and (15) under the solar radiation.Garcia-Segura and collaborators [76] claimed that at current densities > 33.3 mA cm−2, the removal rate of oxalic and oxamic acids was not improved because of the occurrence of parasitic reactions, such as nonorganic oxidizing reactions with hydroxyl radicals, which led to an efficiency, decrease at higher current densities. According to these authors, the parasitic reactions limited the mass transport of acids to the electrodes and increased largely the electric charge consumption. A drop-in TOC mineralization of the antibiotic sulfamethoxazole by photoelectro-Fenton which was observed when the current density reached 25 mA cm−2 was also reported [61, 77]. This drop was attributed to (i) an increase in the degree of cathode polarization as the current density increased, resulting in H2O2 decomposition to H2O on the anode [59]; (ii) reduction of H2O to H2 [78]; and (iii) Fe2+ present in the solution is anodically oxidized to Fe3+, and OH• is dimerized to H2O2 (reaction (18)) [59]. It should be noted that the dimerization generally occurs at higher concentration of hydroxyl radicals, and such higher concentration is possible with the higher voltage (or current) applied [79].
(18)2OH•→H2O2Additionally, to these parasitic reactions, there is the oxidation ofBDDOH• to O2 (reaction (19)) together with reactions (3), (4), and (18) [65].
(19)2BDDOH•→2BDD+O2+2H++2e−The quantity ofBDDOH• may also decrease because of the increase in the formation rate of other weaker oxidants at the BDD anode, such as the peroxodisulfate (S2O82−) ion by oxidation of SO42− from the electrolyte (reaction (20)) and ozone generation (reaction (21)) [75]:
(20)2HSO4−→S2O82−+2H++2e−(21)3H2O→O3+6H++6e−Thus, using an appropriated current density can prevent such side reactions and also avoid using high energy consumption.


#### 2.3.2. Effect of the Concentration of Ferrous Ions

TheFe2+ catalyst concentration is an important parameter that limits the rate of Fenton reaction (1) to produce hydroxyl radicals and, therefore, affects the degree of mineralization of the organic contaminants. The decrease in the oxidation power of Fenton reaction is related to the competitive reaction between Fe2+ and OH• (4) which can also be photolyzed [80], reaction (11).There are experimental evidences that the decolorization rate of azo dyes dropped gradually with increasing the initial ferrous ion content [65, 70]. Espinoza et al. [65] observed that concentration of Fe2+ ≥ 2 mmol L−1 decreased the decolorization which was attributed to reaction (4); also, there were produced colored compounds that decreased the effect of solar radiation, and therefore, the removal of the dye was disfavored. Furthermore, there might have been the generation of unwanted reactions like the formation of Fe3+ complexes ((22) and (23)) that would have prevented the regeneration of Fe2+ or slowed the process [65, 70]:
(22)Fe3++OH•→FeOH3+(23)2Fe3++2n−1C2O42−→2FeC2O4n3−2n+Feng and collaborators [81] reported that the degradation rate of the anti-inflammatory drug ketoprofen decreased with increasing Fe2+ concentration up to 1.0 mmol L−1. Fast degradation rate of ketoprofen by electro-Fenton was achieved at concentration of 0.1 mmol L−1Fe2+. Further increase in catalyst concentration resulted in the decrease of oxidation rate due to the competitive reaction between Fe2+ and OH• (4).


#### 2.3.3. Influence of Initial Concentration of the Organic Compound

Generally, an increase in contaminant concentration produces a decrease in the extent of the organic compound mineralization. The oxidation of high amounts of contaminant molecules by the hydroxyl radical species becomes slower since a number of intermediate species are also produced that demand moreOH• [61, 82–89], but a constant amount of hydroxyl radicals is produced during fixed experimental conditions used. Fryda and coworkers [90] claimed that the chemical oxygen demand (COD) reduction is a highly suitable parameter for wastewater treatment, in most cases independent of the class or organic pollutants. These authors stated that a COD content between 100 mg L−1 to 25 g L−1 is a cost-effective and efficient range for advanced oxidation processes.Ammar and collaborators reported that slower abatement of the target compound was observed as its content increased [83]. This was attributed to the following: (i) the amount of OH• generated continuously into the reactor was constant, and thus, it limited the disappearance of the organic pollutant, and (ii) when the organic matter in the solution is sufficiently high, a minor quantity of hydroxyl radicals attacks the pollutant molecules because more amounts of them destroy its intermediates. Similar results were reported by Samet et al., in which the removal of COD decreased as the initial COD content increased in the treated solution [89]; such results were observed using different H2O2/Fe2+ molar ratios under solar photo-Fenton process.


#### 2.3.4. Influence of Solar Radiation

The naturally occurring wavelengths from the solar radiation, mainly those from the UV and visible radiation wavelengths, produce different photochemical reactions. The solar light is expected to improve the performance of artificial UVA lamps since it provides photons in the UV range of 300–400 nm, as well as in the visible range of 400–650 nm which can also be absorbed by reactants in reactions (11) and (15), respectively [43, 65, 91–94]. There are several designs of solar reactors to concentrate and use efficiently the solar irradiation in the solar photo-Fenton and solar photoelectro-Fenton processes.


### 2.4. Combination of Solar Photo-Fenton and Solar Photoelectro-Fenton with Other Treatment Processes

The advanced oxidation processes (AOP) are environmentally friendly technologies and have shown the capability of mineralizing organic pollutants [9, 19, 35, 95–98]. Inside the AOP, the electrochemical advanced oxidation processes (EAOP) are versatile processes, like solar photoelectro-Fenton, that can produce hydroxyl radical species under controlled optimal conditions with the application of an electric current that enables high hydroxyl radical production [43, 61, 64, 65]. Hence, the hydroxyl radicals, produced by the solar photoelectro-Fenton, can be used initially to oxidize recalcitrant organics and transform them into nontoxic biodegradable species; then, such intermediate compounds can be treated by the biological treatment used as posttreatment process. An anaerobic biological treatment followed by solar photoelectro-Fenton process to oxidize organic matter present in slaughterhouse wastewater from a Chilean meat company was investigated [91]. It was observed that the combination of both processes produced a totally clarified, odorless effluent, without solids in suspension and higher chemical oxygen demand removal than the one from the separate processes.It has also been shown that the solar photo-Fenton can be used as a pretreatment for the secondary treatment process. Ballesteros and coworkers [88] proposed a strategy for treating water with high pesticide concentrations to overcome the low biodegradability of solar photo-Fenton intermediates; such strategy consisted of mixing the contaminated water with a biodegradable carbon source before biological oxidation. Hence, this combination of photo-Fenton and acclimatized activated sludge in several SBR cycles led to complete biodegradation of a concentrated pesticide solution of 500 mg L−1 dissolved organic carbon (DOC) in ∼5 h with a carbon removal efficiency of 90%. According to García-Montaño and coworkers [99], the Fenton process at pilot plant can be used as a biological pretreatment. Since after certain time and under experimental conditions, treated dye solutions became enough biocompatible to be fully biodegraded in the IBR reactor, attaining residual DOC values close to the 20 mg L−1 corresponding to biomass metabolites.There are several papers devoted to oxidize many organic contaminants (like microcontaminants, herbicides, textile dyes, landfill leachates, and emergent contaminants) by solar photo-Fenton and solar photoelectro-Fenton (as depicted in Tables1 and 2) using solar compound parabolic collectors and solar pilot reactors [2, 52, 53, 82, 88, 100–108]. Most of these studies claimed that photo-Fenton enhanced the degradation of the organic compounds achieving over 50% TOC removal. Also, bacteria inactivation by solar photo-Fenton at near-neutral pH using a CPC solar reactor led to a simultaneous decrease of TOC (55%) and total E. coli inactivation with the absence of bacterial regrowth during 24 h in the dark [103].The solar photo-Fenton degradation of the 2,4-dichlorophenoxyacetic acid (2,4-D) herbicide in solar pilot-plant reactors was carried out by Conte et al. [100]. These authors proposed a kinetic model to predict the reactant concentrations during the degradation and reported that the solar reactor was able to reach complete degradation of both the 2,4-D and the main intermediate (2,4-dichlorophenol) at 60 min with 98.9% of total organic carbon (TOC) conversion at 210 min.Durán and collaborators [52] observed that the solar photo-Fenton in the presence of oxalic acid (solar photo-Fenton-ferrioxalate) increased the degradation rate of reactive blue 4 since ferrioxalates strongly absorb a higher portion of the solar spectrum. The addition of oxalic acid increased the operational costs but reduced the pH of the solution. Thus, under optimum conditions, a 66% of TOC elimination with total discoloration and total chemical oxygen demand (COD) removal was achieved. High enhancement of the biodegradability of textile synthetic wastewater with the use of oxalic acid in the solar photo-Fenton process (ferrioxalate) was also reported [53]; in such study, the iron precipitated when over 70% of the initially added oxalic acid was photodecarboxylated. Clearly, the ferric-organic ligand complexes prevent iron precipitation, produce a higher amount of hydroxyl radicals (allowing to use efficiently the solar irradiation), and permit to achieve proper mineralization [35].Table3 summarizes the degradation of several organic contaminants at pilot scale using sand filter and microfiltration as pretreatment for the solar photo-Fenton process. Also, it reports the solar photo-Fenton process as pretreatment of the secondary treatment process. It is interesting to note that the volume treated was relatively high and that the mineralization achieved depended on the initial experimental conditions, degradation time, type of contaminants, and their initial concentration. The oxidation of the organic matter with time was followed by parameters like DOC, TOC, and organic concentration decrease.Table 3
Solar photo-Fenton coupled with other treatment processes.
Contaminant (concentration interval)
Experimental conditions
Reactor type (volume)
Best degradation conditions
Coupled treatment
Reference
Catalyst (pH)
Percentage (time)
Procion Red H-E7B (25 mg L−1)
2 mg L−1 Fe2+ (2.8–3.0 for SPF and neutral for BT)
CPC (35 L)
30% DOC removal in photo-Fenton pre-treatment (13 min only photo-Fenton process)
The photo-Fenton process precedes an aerobic biological treatment carried out in an immobilised biomass reactor (IBR).
[99]
Cibacron Red FN-R (250 mg L−1)
5 mg L−1 Fe2+ (2.8–3.0 for SPF and neutral for BT)
CPC (35 L)
67% DOC removal in photo-Fenton pretreatment (22 min only photo-Fenton process)
The photo-Fenton process precedes an aerobic biological treatment carried out in an immobilised biomass reactor (IBR).
[99]
Pesticides: Vydate, Metomur, Couraze, Ditumur, and Scala (500 mg L−1 DOC)
20 mg L−1 Fe2+ (2.7–2.9 for SPF and neutral for BT)
CPC (50 L)
Carbon removal efficiency of the combined process was as high as 90%. activated sludge acclimatization with several SBR cycles led to complete biodegradation in less than 5 h
The photo-Fenton process precedes a biotreatment with acclimatized activated sludge in several sequencing batch eactor (SBR) cycles
[88]


## 2.1. The Electrochemical Fenton-Based (EF) Processes

The electrochemical Fenton-based (EF) processes, included in the electrochemical advanced oxidation processes, were developed to overcome the drawbacks of the classical Fenton (CF) process. These processes in situ generate the Fenton reagents (H2O2 and/or Fe2+) to yield OH• radicals [36, 37]. The EF processes such as Fered-Fenton (EF-FeRe) [38, 39], electrochemical peroxidation/anodic Fenton (EF-FeOx) [40–42], electro-Fenton (EF-H2O2-FeRe) [38, 43], and peroxi-coagulation (EF-H2O2-FeOx) [44, 45] increase the efficiency of pollutant degradation. The efficiency of pollutant degradation is enhanced when UV light or solar irradiation is used in combination with CF (photo-Fenton or solar photo-Fenton) and EF (photoelectro-Fenton or solar photoelectro-Fenton) processes. Figure 1 schematically shows CF and EF processes: (1) CF: addition of both reagents to the solution, (2) EF-FeRe: addition of both reagents to the solution with the regeneration of Fe2+ from reaction (13), (3) EF-FeOx: generation of iron anions using a sacrificial iron anode with the addition of hydrogen peroxide, (4) EF-H2O2-FeRe (the most common electrochemical Fenton-based process, known as electro-Fenton): generation of hydrogen peroxide and regeneration of initially added Fe2+ catalyst, (5) EF-H2O2-FeOx: in situ generation of both hydrogen peroxide and iron anions, and finally, (6) CF and EF combined with UV light or solar irradiation.Figure 1
Classical Fenton (CF) and electrochemical Fenton (EF) oxidation processes: (1) CF, (2) Fered-Fenton (EF-FeRe), (3) electrochemical peroxidation/anodic Fenton (EF-FeOx), (4) electro-Fenton (EF-H2O2-FeRe), (5) peroxi-coagulation (EF-H2O2-FeOx), and (6) UV-CF/UV-EF.The hydrogen peroxide is generated in situ from the two-electron oxygen reduction on cathodes such as reticulated vitreous carbon [46], gas diffusion electrodes [47], carbon felt [48, 49], pristine graphene [50], and boron-doped diamond [51] from reaction (12), and Fe2+ can be electrochemically regenerated, if it was initially added to the solution (reaction (13)) or electrochemically generated from a sacrificial iron anode (reaction (14)).
(12)O2+2H++2e−→H2O2(13)Fe3++e−→Fe2+(14)Fe−2e−→Fe2+


## 2.2. Solar Photoelectro-Fenton

The conventional photo-Fenton reaction showed a limited efficiency in the mineralization of real textile wastewater mainly associated to three factors [10, 35, 52–55]: (i) formation of iron-organic pollutant complexes with low solubility at acidic pH values (2.8), leading to iron precipitation and abatement of dissolved organic carbon, cannot be associated with mineralization; (ii) low photoactivity of the iron-organic pollutant complexes under UV-visible light; and (iii) photoreduction via a ligand-to-metal charge mechanism, which occurs on the surface of the iron precipitates, is very slow.The photo-Fenton reaction can be enhanced by the following:(1)
The use of different iron(III)-organic ligand complexes such as Fe(III)-oxalate, Fe(III)-citrate and Fe(III)-EDDS (EDDS: S,S′-ethylenediamine-N,N′-disuccinic acid tri-sodium salt). These ligand complexes have higher solubility and higher stability constant than iron-organic pollutant complexes which prevent iron precipitation that allows to achieve proper mineralization. The superiority of Fe(III)-oxalate over Fe(III)-citrate and Fe(III)-EDDS complexes can be mainly associated to the different quantum yield values for Fe(II) production and the half-life of the Fe(III)-organic ligand complexes under UVA radiation. The photo-Fenton reaction mediated by ferricarboxylates was characterized by an initial fast reaction rate, mainly associated to the fast regeneration ofFe3+ to Fe2+, enhanced by the photodecarboxylation of ferricarboxylate complexes under UV-visible light, followed by a very slow reaction rate with a low consumption of H2O2 due to the disappearance of oxalic acid and free iron species complex with other organic oxidation by-products which reduced substantially the dissolved iron concentration and consequently the reaction rate [35].(2)
The use of electricity to drive the photo-Fenton process electrochemically (photoelectro-Fenton (PEF)) under sunlight [56]. The PEF process accelerates the degradation of pollutants because of (a) the enhancement of Fe2+ regeneration and OH• production by the photolytic reaction (11) and (b) the photolysis of Fe-complexes with generated intermediates like carboxylic acids by reaction (15) [57–59]:(15)FeOOCR2+→hvFe2++R•+CO2An interesting comparison of the performance of solar photo-Fenton and solar photoelectro-Fenton experiments, at laboratory scale, was carried out by Serra and collaborators [60]. These authors studied the degradation of the amino acid a-methylphenylglycine (a soluble and nonbiodegradable target pollutant) and observed that the solar-driven photo-Fenton is the most environmentally friendly alternative, mainly because of the use of electricity in the solar photoelectro-Fenton experiments [60]. Indeed, the solar photoelectro-Fenton (SPEF) process can be driven by a photovoltaic system when scale up to a pilot plant or solar plant to decrease the costs associated with the consumption of electricity, which may make sustainable the whole process. Having this in mind, a self-sustainable SPEF, driven by a photovoltaic cell, was designed to study the oxidation of the antibiotic trimethoprim (TMP), producing a high degree of mineralization. Tenaromatic intermediates generated from hydroxylation, carbonylation, and demethylation reactions were identified together with three carboxylic acids (oxamic, oxalic, and formic acids) and two inorganic ions (NH4+ and NO3−). This study is a cost-effective approach for TMP degradation and demonstrated that the sunlight can provide the electric power (for mechanical systems) and the UV radiation for SPEF process [61].Almeida and coworkers [62] studied the degradation of paracetamol by solar photoelectro-Fenton using a flow plant with a Pt/carbon-PTFE air-diffusion electrochemical cell (one-compartment filter-press reactor) coupled with a compound parabolic collector. The H2O2 was electrogenerated from the cathodic O2 reduction at the carbon-PTFE air-diffusion electrode (ADE). These authors reported 75% of total organic carbon (TOC) decrease with an energy cost of 93 kWh kg−1 TOC (7.38 kWh m−3) and 71% removal efficiency. 80% TOC removal was the maximum value acquired at 150 min, with conversion of 79% of initial N into NH4+ ion. Thus, according to these authors, total mineralization of paracetamol was not attained because of the formation of N− derivatives and other undetected products that cannot be destroyed by radical OH• and UV light. The same solar flow plant used by Almeida et al. was employed to oxidize azo dyes [63] and the antibiotic metronidazole [64] by electro-Fenton (EF) and solar photolectro-Fenton (SPEF) processes. Ruiz and coworkers observed that the EF process yielded rapid decolorization with poor TOC removal, and Pérez et al. also reported very weak mineralization of the antibiotic. These results were attributed to the formation of persistent carboxylic acids like oxalic acid as the major component of final electrolyzed solutions; conversely, quick photolysis of Fe(III)-oxalate complexes by UV light of solar irradiation explained the higher oxidation power of SPEF that gave almost total mineralization of the organic contaminants under study. It was described that the incident UV light played an important role in the photodecomposition of several N-derivatives that favored the release of ammonium ions and the loss of volatile N-compounds. Espinoza and coworkers [65] reported that the elimination of an diazo dye (acid yellow 42 dye) and its organic intermediates was due to hydroxyl radicals formed both at the anode surface from water oxidation and in bulk solution from Fenton reaction between electrogeneratd H2O2 and added Fe2+. The application of solar radiation in the photolectro-Fenton process yielded higher current efficiencies and lower energy consumptions than electro-Fenton (EF) and electro-oxidation, with electrogenerated H2O2 by the additional production of hydroxyl radicals from the photolysis of Fe(III)-hydrated species (reaction (11)), and the photodecomposition of Fe(III)-complexes with organic intermediates (ferric carboxylic complexes, like ferric oxalate) that pass through an excitation state under the influence of photons of UV/vis wavelengths. This reaction is called the ligand-metal charge transfer reaction [66–68]:
(16)FeC2O4n3−2n+→hvFe2++n−1C2O42−+C2O4•−Table2 summarizes the experimental degradation of several organic contaminants by solar photoelectro-Fenton. It is shown that the oxidation degree, or mineralization, depends on several parameters like the type of reactor used, pH, initial concentration of the organic contaminant, degradation time, among some others. The oxidation of the organic matter with time was followed by parameters like DOC, TOC, COD, and organic concentration decrease.Table 2
Solar photoelectro-Fenton.
Contaminant (concentration interval)
Experimental conditions
Reactor type (volume)
Best degradation conditions
Reference
Catalyst (pH)
Electrochemical cell (current density)
Percentage (time)
Paracetamol (157 mg L−1)
0.4 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (50 mA cm−2)
CPC (10 L)
~80% TOC removal (at 150 min)
[62]
Acid yellow (AY9) azo dye (200 mg L−1 TOC)
0.5 mM L−1 Fe2+ (3.0)
Boron-doped diamond (BDD)/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom and inclined 30° (2.5 L)
~93% TOC removal (at 360 min)
[63]
Salicylic acid (165 mg L−1 or 100 mg L−1 of TOC)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (3.0 L)
~59% TOC removal (at 360 min)
[194]
Monoazo acid orange 7 (50 mg L−1 of DOC)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion (55.4 mA cm−2)
CPC (10 L)
~97% DOC abatement (at 180 min)
[69]
o-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~90% TOC removal (at 120 min)
[195]
m-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~89% TOC removal (at 120 min)
[195]
p-Cresol (128 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
BDD anode and O2-diffusion cathode (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
~87% TOC removal (at 120 min)
[195]
Heterocyclic antibiotic metronidazole (1.39 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
Pt/air-diffusion (55.4 mA cm−2)
CPC (10 L)
~53% DOC removal (at 300 min)
[64]
Disperse red 1 (DR1) (0.520 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
BDD/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC abatement of 84% (at 240 min)
[84]
Disperse yellow 3 (DY3) (0.558 mmol L−1)
0.50 mmol L−1 Fe2+ (3.0)
BDD/air-diffusion (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC abatement of 86% (at 240 min)
[84]
Ibuprofen (41 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
BDD anode/O2-diffusion cathode (33.3 mA cm−2)
Open-cell compartment (0.1 L)
88% DOC removal (at 120 min)
[43]
Acid orange 7 (AO7) (150 mg L−1 of TOC)
0.75 mM L−1 Fe2+ (3.0)
Pt sheet and a carbon-PTFE air-diffusion electrode. (40 mA cm−2)
CPC (10 L)
TOC was reduced by 96% (at 360 min)
[196]
Acid yellow 42 (AY42) (100 mg L−1 of TOC)
1.0 mM L−1 Fe2+ (3.0)
Boron-doped diamond (BDD) anode and an air diffusion cathode (ADC) (50 mA cm−2)
CPC (8 L)
~80% TOC removal (at 270 min)
[65]
Organic matter present in slaughterhouse wastewater (52 mg L−1 of TOC)
1.0 mM L−1 Fe2+ (3.0)
Si/BDD thin-film anode and carbon-PTFE air-diffusion cathode (50 mA cm−2)
Open-cell compartment (0.1 L)
4 mg L−1 of total organic carbon (TOC) (at 240 min)
[91]
Pharmaceutical ranitidine (112.6 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt sheet anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
67% TOC removal (at 360 min)
[197]
Antibiotic trimethoprim (200 mg L−1)
1.0 mM L−1 Fe2+ (3.0)
RuO2/Ti mesh electrodes (18 mA cm−2)
Cylindrical quartz cell (125 mL)
80% TOC decay (at 360 min)
[61]
Allura red AC azo dye (460 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt sheet anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
A planar solar photoreactor (2.5 L)
97% TOC decay (at 180 min)
[85]
Sulfanilic acid (240 mg L−1 or 100 mg L−1 of TOC)
0.5 mM L−1 Fe2+ (4.0)
Pt/air-diffusion (100 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
TOC was reduced by 76% (at 120 min)
[56]
Chloramphenicol (2,2-dicloro-N-[1,3-dihydroxy-1-(4-nitrophenyl)propan-2-yl] acetamide) (245 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/air-diffusion filter-press cell (100 mA cm−2)
CPC (10 L)
DOC was reduced by 89% (at 180 min)
[86]
Sunset yellow FCF azo dye (290 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/carbon-PTFE air-diffusion cell (77.6 mA cm−2)
CPC (10 L)
TOC was reduced by 94% (at 150 min)
[198]
Sulfanilamide (239 mg L−1)
0.5 mM L−1 Fe2+ (3.0)
Pt/carbon-PTFE air-diffusion cell (50 mA cm−2)
Polycarbonate box built-up with a mirror at the bottom (2.5 L)
DOC decay of 91% (at 180 min)
[199]
Tebuthiuron (0.18 mM L−1)
0.5 mM L−1 Fe2+(3.0)
BDD anode and a carbon-PTFE air-diffusion cathode (100 mA cm−2)
Solar flow plant (2.5 L)
75% TOC removal (at 360 min)
[200]
A sanitary landfill leachate previously subjected to biological and coagulation processes (337–430 mg L−1 of DOC)
60 mg L−1 Fe3+ and oxalic acid to get Fe(III)-to-oxalate molar ratio of 1 : 3 (2.8)
BDD anode and a carbon-PTFE air-diffusion cathode (200 mA cm−2)
Lab-scale flow plant (2.2 L)
DOC decay of 80% (at 300 min)
[201]
Atrazine (20 mg L−1)
0.1 mM L−1 Fe2+ (3.0)
BDD thin-film electrode on Nb (13.33 mA cm−2)
In an open, undivided and cylindrical tank reactor (200 mL)
TOC reduction of 70% (at 300 min)
[202]


## 2.3. Influencing Parameters on the Degradation of Organic Compounds by Solar Photoelectro-Fenton Process

Complete transformation of organic compounds toCO2 by the solar photoelectro-Fenton process depends directly on the applied current density, the concentration of catalyst, organic concentration, and the solar radiation intensity [65, 69, 70]. There are other parameters like pH of the solution, temperature, and electrode materials that are important too in the photoelectro-Fenton process; however, Fenton reaction is efficient at the pH interval of 2.5 < pH < 3 [7, 71–73], oxygen is needed to produce H2O2, and its solubility is affected by the temperature [74]; thus, it is better to perform the experiment at room temperature, and the electrode materials like carbonaceous cathodes [46, 48–50] and BDD anodes [56, 75] have been proved to be the best materials (to reduce oxygen and to produce OH• radicals, resp.) so far.


### 2.3.1. Current Density Influence

The current density (or voltage cell) applied to the electrochemical cell forH2O2 production in the photoelectro-Fenton process influences the electrode surface reaction kinetics and the extension of electrode reactions. Hydroxyl radicals are in situ generated in the photoelectro-Fenton process. Such oxidant species can be produced simultaneously via oxygen cathodic reduction (reaction (12)) in the presence of catalyst (reactions (1) and (8)) and on the anode boron-doped diamond (BDD) [75]:
(17)BDD+H2O→BDDOH•+H++e−B
D
D
O
H
• enhances the destruction of aromatic pollutants and their aliphatic intermediates such as short-linear carboxylic acids [56]. Thus, the oxidation power of the solar photoelectro-Fenton is additionally enhanced by reactions (11) and (15) under the solar radiation.Garcia-Segura and collaborators [76] claimed that at current densities > 33.3 mA cm−2, the removal rate of oxalic and oxamic acids was not improved because of the occurrence of parasitic reactions, such as nonorganic oxidizing reactions with hydroxyl radicals, which led to an efficiency, decrease at higher current densities. According to these authors, the parasitic reactions limited the mass transport of acids to the electrodes and increased largely the electric charge consumption. A drop-in TOC mineralization of the antibiotic sulfamethoxazole by photoelectro-Fenton which was observed when the current density reached 25 mA cm−2 was also reported [61, 77]. This drop was attributed to (i) an increase in the degree of cathode polarization as the current density increased, resulting in H2O2 decomposition to H2O on the anode [59]; (ii) reduction of H2O to H2 [78]; and (iii) Fe2+ present in the solution is anodically oxidized to Fe3+, and OH• is dimerized to H2O2 (reaction (18)) [59]. It should be noted that the dimerization generally occurs at higher concentration of hydroxyl radicals, and such higher concentration is possible with the higher voltage (or current) applied [79].
(18)2OH•→H2O2Additionally, to these parasitic reactions, there is the oxidation ofBDDOH• to O2 (reaction (19)) together with reactions (3), (4), and (18) [65].
(19)2BDDOH•→2BDD+O2+2H++2e−The quantity ofBDDOH• may also decrease because of the increase in the formation rate of other weaker oxidants at the BDD anode, such as the peroxodisulfate (S2O82−) ion by oxidation of SO42− from the electrolyte (reaction (20)) and ozone generation (reaction (21)) [75]:
(20)2HSO4−→S2O82−+2H++2e−(21)3H2O→O3+6H++6e−Thus, using an appropriated current density can prevent such side reactions and also avoid using high energy consumption.


### 2.3.2. Effect of the Concentration of Ferrous Ions

TheFe2+ catalyst concentration is an important parameter that limits the rate of Fenton reaction (1) to produce hydroxyl radicals and, therefore, affects the degree of mineralization of the organic contaminants. The decrease in the oxidation power of Fenton reaction is related to the competitive reaction between Fe2+ and OH• (4) which can also be photolyzed [80], reaction (11).There are experimental evidences that the decolorization rate of azo dyes dropped gradually with increasing the initial ferrous ion content [65, 70]. Espinoza et al. [65] observed that concentration of Fe2+ ≥ 2 mmol L−1 decreased the decolorization which was attributed to reaction (4); also, there were produced colored compounds that decreased the effect of solar radiation, and therefore, the removal of the dye was disfavored. Furthermore, there might have been the generation of unwanted reactions like the formation of Fe3+ complexes ((22) and (23)) that would have prevented the regeneration of Fe2+ or slowed the process [65, 70]:
(22)Fe3++OH•→FeOH3+(23)2Fe3++2n−1C2O42−→2FeC2O4n3−2n+Feng and collaborators [81] reported that the degradation rate of the anti-inflammatory drug ketoprofen decreased with increasing Fe2+ concentration up to 1.0 mmol L−1. Fast degradation rate of ketoprofen by electro-Fenton was achieved at concentration of 0.1 mmol L−1Fe2+. Further increase in catalyst concentration resulted in the decrease of oxidation rate due to the competitive reaction between Fe2+ and OH• (4).


### 2.3.3. Influence of Initial Concentration of the Organic Compound

Generally, an increase in contaminant concentration produces a decrease in the extent of the organic compound mineralization. The oxidation of high amounts of contaminant molecules by the hydroxyl radical species becomes slower since a number of intermediate species are also produced that demand moreOH• [61, 82–89], but a constant amount of hydroxyl radicals is produced during fixed experimental conditions used. Fryda and coworkers [90] claimed that the chemical oxygen demand (COD) reduction is a highly suitable parameter for wastewater treatment, in most cases independent of the class or organic pollutants. These authors stated that a COD content between 100 mg L−1 to 25 g L−1 is a cost-effective and efficient range for advanced oxidation processes.Ammar and collaborators reported that slower abatement of the target compound was observed as its content increased [83]. This was attributed to the following: (i) the amount of OH• generated continuously into the reactor was constant, and thus, it limited the disappearance of the organic pollutant, and (ii) when the organic matter in the solution is sufficiently high, a minor quantity of hydroxyl radicals attacks the pollutant molecules because more amounts of them destroy its intermediates. Similar results were reported by Samet et al., in which the removal of COD decreased as the initial COD content increased in the treated solution [89]; such results were observed using different H2O2/Fe2+ molar ratios under solar photo-Fenton process.


### 2.3.4. Influence of Solar Radiation

The naturally occurring wavelengths from the solar radiation, mainly those from the UV and visible radiation wavelengths, produce different photochemical reactions. The solar light is expected to improve the performance of artificial UVA lamps since it provides photons in the UV range of 300–400 nm, as well as in the visible range of 400–650 nm which can also be absorbed by reactants in reactions (11) and (15), respectively [43, 65, 91–94]. There are several designs of solar reactors to concentrate and use efficiently the solar irradiation in the solar photo-Fenton and solar photoelectro-Fenton processes.


## 2.3.1. Current Density Influence

The current density (or voltage cell) applied to the electrochemical cell forH2O2 production in the photoelectro-Fenton process influences the electrode surface reaction kinetics and the extension of electrode reactions. Hydroxyl radicals are in situ generated in the photoelectro-Fenton process. Such oxidant species can be produced simultaneously via oxygen cathodic reduction (reaction (12)) in the presence of catalyst (reactions (1) and (8)) and on the anode boron-doped diamond (BDD) [75]:
(17)BDD+H2O→BDDOH•+H++e−B
D
D
O
H
• enhances the destruction of aromatic pollutants and their aliphatic intermediates such as short-linear carboxylic acids [56]. Thus, the oxidation power of the solar photoelectro-Fenton is additionally enhanced by reactions (11) and (15) under the solar radiation.Garcia-Segura and collaborators [76] claimed that at current densities > 33.3 mA cm−2, the removal rate of oxalic and oxamic acids was not improved because of the occurrence of parasitic reactions, such as nonorganic oxidizing reactions with hydroxyl radicals, which led to an efficiency, decrease at higher current densities. According to these authors, the parasitic reactions limited the mass transport of acids to the electrodes and increased largely the electric charge consumption. A drop-in TOC mineralization of the antibiotic sulfamethoxazole by photoelectro-Fenton which was observed when the current density reached 25 mA cm−2 was also reported [61, 77]. This drop was attributed to (i) an increase in the degree of cathode polarization as the current density increased, resulting in H2O2 decomposition to H2O on the anode [59]; (ii) reduction of H2O to H2 [78]; and (iii) Fe2+ present in the solution is anodically oxidized to Fe3+, and OH• is dimerized to H2O2 (reaction (18)) [59]. It should be noted that the dimerization generally occurs at higher concentration of hydroxyl radicals, and such higher concentration is possible with the higher voltage (or current) applied [79].
(18)2OH•→H2O2Additionally, to these parasitic reactions, there is the oxidation ofBDDOH• to O2 (reaction (19)) together with reactions (3), (4), and (18) [65].
(19)2BDDOH•→2BDD+O2+2H++2e−The quantity ofBDDOH• may also decrease because of the increase in the formation rate of other weaker oxidants at the BDD anode, such as the peroxodisulfate (S2O82−) ion by oxidation of SO42− from the electrolyte (reaction (20)) and ozone generation (reaction (21)) [75]:
(20)2HSO4−→S2O82−+2H++2e−(21)3H2O→O3+6H++6e−Thus, using an appropriated current density can prevent such side reactions and also avoid using high energy consumption.


## 2.3.2. Effect of the Concentration of Ferrous Ions

TheFe2+ catalyst concentration is an important parameter that limits the rate of Fenton reaction (1) to produce hydroxyl radicals and, therefore, affects the degree of mineralization of the organic contaminants. The decrease in the oxidation power of Fenton reaction is related to the competitive reaction between Fe2+ and OH• (4) which can also be photolyzed [80], reaction (11).There are experimental evidences that the decolorization rate of azo dyes dropped gradually with increasing the initial ferrous ion content [65, 70]. Espinoza et al. [65] observed that concentration of Fe2+ ≥ 2 mmol L−1 decreased the decolorization which was attributed to reaction (4); also, there were produced colored compounds that decreased the effect of solar radiation, and therefore, the removal of the dye was disfavored. Furthermore, there might have been the generation of unwanted reactions like the formation of Fe3+ complexes ((22) and (23)) that would have prevented the regeneration of Fe2+ or slowed the process [65, 70]:
(22)Fe3++OH•→FeOH3+(23)2Fe3++2n−1C2O42−→2FeC2O4n3−2n+Feng and collaborators [81] reported that the degradation rate of the anti-inflammatory drug ketoprofen decreased with increasing Fe2+ concentration up to 1.0 mmol L−1. Fast degradation rate of ketoprofen by electro-Fenton was achieved at concentration of 0.1 mmol L−1Fe2+. Further increase in catalyst concentration resulted in the decrease of oxidation rate due to the competitive reaction between Fe2+ and OH• (4).


## 2.3.3. Influence of Initial Concentration of the Organic Compound

Generally, an increase in contaminant concentration produces a decrease in the extent of the organic compound mineralization. The oxidation of high amounts of contaminant molecules by the hydroxyl radical species becomes slower since a number of intermediate species are also produced that demand moreOH• [61, 82–89], but a constant amount of hydroxyl radicals is produced during fixed experimental conditions used. Fryda and coworkers [90] claimed that the chemical oxygen demand (COD) reduction is a highly suitable parameter for wastewater treatment, in most cases independent of the class or organic pollutants. These authors stated that a COD content between 100 mg L−1 to 25 g L−1 is a cost-effective and efficient range for advanced oxidation processes.Ammar and collaborators reported that slower abatement of the target compound was observed as its content increased [83]. This was attributed to the following: (i) the amount of OH• generated continuously into the reactor was constant, and thus, it limited the disappearance of the organic pollutant, and (ii) when the organic matter in the solution is sufficiently high, a minor quantity of hydroxyl radicals attacks the pollutant molecules because more amounts of them destroy its intermediates. Similar results were reported by Samet et al., in which the removal of COD decreased as the initial COD content increased in the treated solution [89]; such results were observed using different H2O2/Fe2+ molar ratios under solar photo-Fenton process.


## 2.3.4. Influence of Solar Radiation

The naturally occurring wavelengths from the solar radiation, mainly those from the UV and visible radiation wavelengths, produce different photochemical reactions. The solar light is expected to improve the performance of artificial UVA lamps since it provides photons in the UV range of 300–400 nm, as well as in the visible range of 400–650 nm which can also be absorbed by reactants in reactions (11) and (15), respectively [43, 65, 91–94]. There are several designs of solar reactors to concentrate and use efficiently the solar irradiation in the solar photo-Fenton and solar photoelectro-Fenton processes.


## 2.4. Combination of Solar Photo-Fenton and Solar Photoelectro-Fenton with Other Treatment Processes

The advanced oxidation processes (AOP) are environmentally friendly technologies and have shown the capability of mineralizing organic pollutants [9, 19, 35, 95–98]. Inside the AOP, the electrochemical advanced oxidation processes (EAOP) are versatile processes, like solar photoelectro-Fenton, that can produce hydroxyl radical species under controlled optimal conditions with the application of an electric current that enables high hydroxyl radical production [43, 61, 64, 65]. Hence, the hydroxyl radicals, produced by the solar photoelectro-Fenton, can be used initially to oxidize recalcitrant organics and transform them into nontoxic biodegradable species; then, such intermediate compounds can be treated by the biological treatment used as posttreatment process. An anaerobic biological treatment followed by solar photoelectro-Fenton process to oxidize organic matter present in slaughterhouse wastewater from a Chilean meat company was investigated [91]. It was observed that the combination of both processes produced a totally clarified, odorless effluent, without solids in suspension and higher chemical oxygen demand removal than the one from the separate processes.It has also been shown that the solar photo-Fenton can be used as a pretreatment for the secondary treatment process. Ballesteros and coworkers [88] proposed a strategy for treating water with high pesticide concentrations to overcome the low biodegradability of solar photo-Fenton intermediates; such strategy consisted of mixing the contaminated water with a biodegradable carbon source before biological oxidation. Hence, this combination of photo-Fenton and acclimatized activated sludge in several SBR cycles led to complete biodegradation of a concentrated pesticide solution of 500 mg L−1 dissolved organic carbon (DOC) in ∼5 h with a carbon removal efficiency of 90%. According to García-Montaño and coworkers [99], the Fenton process at pilot plant can be used as a biological pretreatment. Since after certain time and under experimental conditions, treated dye solutions became enough biocompatible to be fully biodegraded in the IBR reactor, attaining residual DOC values close to the 20 mg L−1 corresponding to biomass metabolites.There are several papers devoted to oxidize many organic contaminants (like microcontaminants, herbicides, textile dyes, landfill leachates, and emergent contaminants) by solar photo-Fenton and solar photoelectro-Fenton (as depicted in Tables1 and 2) using solar compound parabolic collectors and solar pilot reactors [2, 52, 53, 82, 88, 100–108]. Most of these studies claimed that photo-Fenton enhanced the degradation of the organic compounds achieving over 50% TOC removal. Also, bacteria inactivation by solar photo-Fenton at near-neutral pH using a CPC solar reactor led to a simultaneous decrease of TOC (55%) and total E. coli inactivation with the absence of bacterial regrowth during 24 h in the dark [103].The solar photo-Fenton degradation of the 2,4-dichlorophenoxyacetic acid (2,4-D) herbicide in solar pilot-plant reactors was carried out by Conte et al. [100]. These authors proposed a kinetic model to predict the reactant concentrations during the degradation and reported that the solar reactor was able to reach complete degradation of both the 2,4-D and the main intermediate (2,4-dichlorophenol) at 60 min with 98.9% of total organic carbon (TOC) conversion at 210 min.Durán and collaborators [52] observed that the solar photo-Fenton in the presence of oxalic acid (solar photo-Fenton-ferrioxalate) increased the degradation rate of reactive blue 4 since ferrioxalates strongly absorb a higher portion of the solar spectrum. The addition of oxalic acid increased the operational costs but reduced the pH of the solution. Thus, under optimum conditions, a 66% of TOC elimination with total discoloration and total chemical oxygen demand (COD) removal was achieved. High enhancement of the biodegradability of textile synthetic wastewater with the use of oxalic acid in the solar photo-Fenton process (ferrioxalate) was also reported [53]; in such study, the iron precipitated when over 70% of the initially added oxalic acid was photodecarboxylated. Clearly, the ferric-organic ligand complexes prevent iron precipitation, produce a higher amount of hydroxyl radicals (allowing to use efficiently the solar irradiation), and permit to achieve proper mineralization [35].Table3 summarizes the degradation of several organic contaminants at pilot scale using sand filter and microfiltration as pretreatment for the solar photo-Fenton process. Also, it reports the solar photo-Fenton process as pretreatment of the secondary treatment process. It is interesting to note that the volume treated was relatively high and that the mineralization achieved depended on the initial experimental conditions, degradation time, type of contaminants, and their initial concentration. The oxidation of the organic matter with time was followed by parameters like DOC, TOC, and organic concentration decrease.Table 3
Solar photo-Fenton coupled with other treatment processes.
Contaminant (concentration interval)
Experimental conditions
Reactor type (volume)
Best degradation conditions
Coupled treatment
Reference
Catalyst (pH)
Percentage (time)
Procion Red H-E7B (25 mg L−1)
2 mg L−1 Fe2+ (2.8–3.0 for SPF and neutral for BT)
CPC (35 L)
30% DOC removal in photo-Fenton pre-treatment (13 min only photo-Fenton process)
The photo-Fenton process precedes an aerobic biological treatment carried out in an immobilised biomass reactor (IBR).
[99]
Cibacron Red FN-R (250 mg L−1)
5 mg L−1 Fe2+ (2.8–3.0 for SPF and neutral for BT)
CPC (35 L)
67% DOC removal in photo-Fenton pretreatment (22 min only photo-Fenton process)
The photo-Fenton process precedes an aerobic biological treatment carried out in an immobilised biomass reactor (IBR).
[99]
Pesticides: Vydate, Metomur, Couraze, Ditumur, and Scala (500 mg L−1 DOC)
20 mg L−1 Fe2+ (2.7–2.9 for SPF and neutral for BT)
CPC (50 L)
Carbon removal efficiency of the combined process was as high as 90%. activated sludge acclimatization with several SBR cycles led to complete biodegradation in less than 5 h
The photo-Fenton process precedes a biotreatment with acclimatized activated sludge in several sequencing batch eactor (SBR) cycles
[88]


## 3.TiO2 Solar Photocatalysis

T
i
O
2 has proven to be one of the most promising photocatalysts amongst several metal oxide semiconductors because of its high reactivity, chemical stability, low cost, and nontoxicity [109]. TiO2 photocatalyst has been mainly used widely in environmental remediation (i.e., wastewater detoxification) and solar energy conversion [96, 110]. TiO2 (band gap energy 3.2 eV) upon illumination with UV light (λ < 380 nm) produces excited high-energy states of electron (in the conduction band, ecb−) and hole (in the valence band, hvb+) pairs, reaction (24), capable of initiating chemical reactions [111], as shown in the photocatalysis mechanism (Scheme 1).
(24)TiO2+hv→ecb−+hvb+Scheme 1
Schematic representation of the photocatalysis mechanism.The holes are responsible for the degradation of organic compounds and can react with water (reaction (25)) or hydroxyl ions (reaction (26)) to produce hydroxyl radicals; though, the recombination of the ecb−/hvb+ pair (reaction (27)) and the reduction of OH• radicals (reaction (28)) produce large inefficiencies in the photocatalytic process [112].
(25)H2O+hvb+→OH•+H+(26)OH−+hvb+→OH•(27)hvb++ecb−→TiO2+heat(28)OH•+ecb−→OH−The oxidation of organic pollutants (R-H) can take place by a direct reaction with holes (reaction (29)) or indirectly via hydroxyl radicals (reaction (30)) or free organic radicals (reaction (31)) [109, 111]:
(29)R−H+hvb+→R+•+degradationproducts(30)R−H+OH•→R•+H2O(31)R•+O2→RO2•→CO2+intermediatesThe hydroxyl radicals, generated under ambient conditions in this process, are nonselective powerful oxidant species capable of converting organic pollutants (toxic and nonbiodegradable) into relatively innocuous end products such asCO2, H2O, and mineral acids [1].


### 3.1. Photocatalytic Activity of TiO2 under Sunlight

T
i
O
2 semiconductor is mainly photoactive with artificial UV lamps that increase the electrical cost of the photocatalytic process. The sunlight is expected to improve the performance of TiO2 photocatalysis since it provides photons in the UV range (300–400 nm); also, doping TiO2 extends its photoresponse capacity towards the sunlight visible range (400–700 nm). The chemical surface alteration of TiO2 (when doped or photodoped with transition metals, noble metals, nonmetals, organic dye sensitization, and coupled semiconductors) modifies its electronic structure producing changes in the electron densities in the conduction band [113] which enhances the solar efficiency of TiO2 under solar irradiation and, hence, influences the mechanism of the photocatalytic process. Dopants can act as electron (or hole) traps preventing charge recombination, create an intermediate energy level introduced between the conduction band and the valence band, lead to band bend gap narrowing or expansion, and induce band bending or conduction band edge shifts which occur due to disruption of the lattice structure of the dopants and formation of surface oxygen vacancies [113–116]. Introduction of such energy levels in the band gap induces the red shift in the band gap transition and the visible light absorption through a charge transfer between a dopant and conduction band (or valence band) [112]. Nevertheless, these changes depend on the nature of dopants, synthesis methods, annealing process, dopant concentration, and dopant distribution [11, 112, 113, 117–120].


### 3.2. Influencing Parameters on the Degradation of Organic Compounds by TiO2 Solar Photocatalysis

Mineralization of organic compounds (conversion toCO2 and mineral acids) by the TiO2 solar photocatalytic process depends directly on the synthesis method of the catalyst [121–126], type of doping materials [11, 112, 113, 117–120], annealing temperature [127–131], catalyst load [132–135], pollutant concentration [136–139], and pH of the aqueous solution [140–142]. There are other parameters like reaction temperature, reactor configuration (geometry), reactor material, air sparging in the reactor solution, and the solar radiation intensity (solar concentration ratio) [143] that are important too in the TiO2 solar photocatalytic process. Nevertheless, these last factors contribute in less extension to the degradation of the pollutants compared to the most commonly studied such as catalyst load, pollutant concentration, and pH of the aqueous solution.


#### 3.2.1. Effect of TiO2 Annealing Temperature

The influence of annealing temperature on the microstructure, surface morphology, and optical property ofTiO2 particles, TiO2 nanoparticles, and TiO2 thin films strongly depends on the synthesis methods [144–149]. Three different phases of TiO2 have been reported which depend on the heat treatment like anatase, rutile, and brookite, anatase and rutile phases being commonly prepared [8, 9, 11, 145, 149]. It has been reported that anatase is more photoactive than rutile [1, 109, 150, 151]; however, it has also been reported that synergistic effects of mixed phases of anatase and rutile enhances the photoactivity of the photocatalyst [152–155].


#### 3.2.2. Influence of Catalyst Concentration

Catalyst load is an important factor that can affect the degradation rate of the organic pollutants; the optimum amount depends on the nature of the organic compound and on the geometry of the photoreactor [156–158]. When TiO2 concentration increases from 0 to certain values, a significant enhancement of efficiency is recorded for the elimination and mineralization of organics. However, there is a loading range in which either no significant changes are observed or even a decrease in the elimination of organic compounds happens. The number of active surface sites increases with TiO2 concentration until certain loading since light penetration decreases and aggregation of TiO2 particles increases at relative high catalyst loading [159]. It has been reported that TiO2 photocatalysis combined with ultrasound can be benefited [72, 97, 159, 160] due to different factors like (a) an increase in the catalyst surface area due to the aggregation action of ultrasound, which enhances the performance of the photocatalytic system [161]; (b) an improvement of mass transfer of organic compounds between the liquid phase and the TiO2 surface [162, 163]; and (c) a reduction of charge recombination and promotion production of additional OH• due to the residual H2O2 generated [162, 163]. Also, the continuous cleaning of the TiO2 surface by acoustic cavitation [164] might also have some role in modifying the photocatalytic rate. Tables 4–6 show that different amounts of catalyst ranging from 10 mg L−1 to 4 g L−1 yielded different degrees of organic degradation during the photocatalytic oxidation process under the experimental conditions stated.Table 4
Slurry TiO2 solar photocatalysis.
Contaminant (concentration interval)
Catalyst
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Solution pH
Initial concentration
Type of reactor
Total volume
Percentage
Time
Amoxicillin
40 mg L−1
Degussa P-25 (7.5)
0.5 g L−1
CPC
15 L
70% of the residual DOC content in the form of low molecular weight
215 min
[167]
Methyl-orange, orange II
30 mg L−1
Degussa P-25 (6.4–6.7)
0.2 g L−1
CPC
39 L
90% of colour abatement and final TOC 0.11 ppm for both
—
[168]
Bisphenol A
100μg mL−1
TiO2 anatase, purity 99.9%, Wako Pure Chemical Industries (6.0)
10 mg L−1
Pyrex reaction vessel
50 mL
60% with light intensity: 1.3 m W cm−2
60 min
[98]
The commercial detergent (α-sodium fatty acid ester sulfonate, alkylaryl sulfonate, a sodium salt of a fatty acid, aluminosilicate, and sodium carbonate)
0.1 g L−1
TiO2 P-25 (4.9)
6.0 g L−1
A batch mode reactor exposed to sunlight using a mirror concentrator.
3 L
0.2 of Ct/Co
120 min
[203]
Remazol brill blue R (RBBR)
100 mg L−1
TiO2 by solution combustion method (natural pH conditions)
1 g L−1
Cylindrical borosilicate glass reactor
400 mL
0.26 of Ct/Co
150 min
[130]
Reactive yellow 17 (RY17)
Initial COD 476 mg L−1
TiO2 Degussa P25 (3.5)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 56 mg L−1 (88%)
8 h
[139]
Reactive red 2 (RR2)
Initial COD 225 mg L−1
TiO2 Degussa P25 (4.65)
4 g L−1
The cylindrical reactor
200 mL of capacity
COD 18 mg L−1 (92%)
8 h
[139]
Reactive blue 4 (RB4)
Initial COD 81 mg L−1
TiO2 Degussa P25 (4.2)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 15 mg L−1 (82%)
8 h
[139]
Escherichia coli K-12, ilitrelding
Concentration of 104 CFU mL−1
TiO2 Degussa P25 (no pH adjustment)
25 mg L−1
CPC collector
The photoreactor volume is 5.4 L
101 CFU mL−1
At 2 KJ L−1 of QUV
[169]
Reactive brilliant red K-2G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 82%
4 h
[204]
Reactive brilliant red K-BP
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 73%
4 h
[204]
Reactive yellow KD-3G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 42%
4 h
[204]
Cationic pink FG
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 61%
4 h
[204]
Methyl orange
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 52%
4 h
[204]
Humic acids
100 mg L−1
TiO2 Degussa P25 (natural pH)
1 g L−1
CPC
35 L
Removal of DOC 93%
Q
UV = 33 kJ L−1
[172]
Reactive yellow 14
5 × 10−4 mol L−1
TiO2 Degussa P25 (5.5)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Degradation 84.4%
60 min
[138]
Nitrobenzene
300 mg L−1
Degussa P-25 TiO2 (4.5)
0.3% (w/v of the solution)
Cylindrical reactor
465 mL of capacity
96% destruction of TOC
240 min
[205]
Propranolol
50 mg L−1
Degussa P-25 (no pH adjustment)
0.4 g L−1
Pilot plant (6 parallel CPCs) (concentration factor of 1, CCPC = 1)
10 L
81% of degradation
240 min
[133]
Reactive orange 4
5 × 10−4 mol L−1
Degussa P-25 (4.8)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Dye degradation 97%
150 min
[206]
Phenol
20 mg L−1
A home-made TiO2“TiEt-450” (between 5.2 and 6.2)
500 mg L−1
CPC
35 L
Smaller than 3 mg L−1
200 min
[207]
Diclofenac (DCF) and naproxen (NPX) 1 : 1 mixture
30 mg L−1
TiO2 P25 Aeroxide® (ambient pH)
0.1 g L−1
Immersion-well photoreactor
400 mL
Total COD reductions of 76%
360 min
[208]
Imazalil (IMZ), thiabendazole (TBZ), and acetamiprid (ACP)
9.0μg L−1 of IMZ, 12.6 μg L−1 of TBZ, and 20.4 μg L−1 of ACP
Evonik P25 TiO2 (7.2–8.0)
200 mg L−1
CPC
8 L
Removal 68% ACP and 85% TBZ and 100% of IMZ
20 kJ L−1
[173]
Synthetic sewage
200 mg L−1 DOC
TiO2 Degussa P25 and sodium peroxydisulfate (Na2S2O8) (3.3)
TiO2 = 200 mg L−1 Na2S2O8 = 4300 mg L−1
CPC
35 L
73% decrease in the initial DOC
5 h
[209]
Ferricyanide
4 × 10−3–10 × 10−3 mol L−1 of Fe(CN)63−, pH values tested were 10, 11, 12, 13, and 14
TiO2 Sigma-Aldrich 93% anatase and 7% rutile, particle size < 25 nm (pH values tested were 10, 11, 12, 13, and 14)
600 mg L−1
CPC
1.5 L
Sunlight exposure with TiO2 the total amounts of ferricyanide and cyanide decreased 94%, whereas only 4.8% was decreased with solar photolysis
24 h
[174]


#### 3.2.3. Influence of Initial Pollutant Concentration and pH of the Solution

The initial concentration of the organic compounds at constant pH and different initial pH of the solution are also important factors that affect the degradation rate of the organic pollutants and the efficiency of the photocatalytic oxidation process.As the initial concentration of organics increases, the photocatalytic efficiency decreases due to a decrease of the reaction rate, which is attributed to a decrease in the number of photons andTiO2 particles available, since the number of organic molecules adsorbed onto the catalyst may block catalyst activation. Also, the initial pH of the solution influences the rate of the degradation process. It has been reported that the adsorption of the organic compounds onto the TiO2 surface is affected by the pH of the solution [97, 160]. The pollutant and thus the rates of degradation will be maximum near the point of zero charge (pzc) of the catalyst [164]. The pzc of TiO2 surface is at pHpzc between 6.25 and 7.1 [1, 165, 166], depending on the ionic strength [166]. Tables 4, 5, and 6 show that different initial pollutant concentration and solution pH were used to degrade different organics during the photocatalytic oxidation process under the experimental conditions stated. Most of the experiments were carried out in the pH range of 2.0–14, and some were with no pH control, as depicted on Tables 4–6.Table 5
Immobilized TiO2 solar photocatalysis.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Method of synthesis
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Atrazine
20 mg L−1
Sol-gel method using titanium butoxide
180 spheres of TiO2-coated glass sustained by a nylon mesh (3.0)
0.3 g L−1
An open, undivided and cylindrical tank reactor
200 mL
Reduction of 30% of initial concentration
300 min
[202]
Methylene blue
50 mg L−1
Hydrothermal method
TiO2 Degussa P25 supported on black volcanic ashes TVA (no pH adjustment)
3 g L−1 TVA
Stirred photoreactors with parabolic sunlight irradiation concentrators
50 mL
95% degradation of wastewater pollutant
120 min
[210]
Salicylic acid
165 mg L−1
Sol-gel method using titanium butoxide
TiO2 coating onto borosilicate glass spheres of 5 mm diameter (3.0)
0.25 g TiO2 L−1
A polycarbonate box with a mirror at the bottom and tilted 41°
3.0 L
Reduction of 14% of initial concentration
360 min
[194]
Acetaminophen, thiabendazole, acetamiprid, and imazalil
100μg L−1 each
Sol-gel technique using titanium isopropoxide
Glass spheres (6 mmφ) were dip-coated with the TiO2 sol (6.2–8.4)
0.6 mg of TiO2 on the surface of each glass bead
CPC
8 L
Reduction of 100% of initial concentration
240 min
[122]Table 6
Solar photocatalysis using nitrogen-doped TiO2, carbon-doped TiO2, polypyrrole TiO2 nanocomposites, and a mix of TiO2 with persulfate ions.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Cefazolin
Concentration of 1.0 × 10−2 mol L−1
N-doped TiO2 (6.4)
2.0 g L−1
Batch-type photoreactor
600 mL
80% of cefazolin removed
30 min
[211]
Azo dye orange G
25 mg L−1
Nitrogen-doped TiO2 (2.0)
1.0 g L−1
Glass beaker
1000 mL
Efficiency of degradation greater than 95%
40 min
[212]
Methylene blue
20 mg L−1
Carbon-doped TiO2 nanoparticles (neutral pH)
1.0 g L−1
Batch-type photoreactor
200 mL of 10 mg/L methylene blue
Greater than 0.1 Ct/Co
60 min
[175]
Acid orange 7 in the concentration
0.2 mM L−1
Combination of TiO2 with potassium persulphate (3.0)
TiO2 (200 mg L−1) and 10 mM L−1of potassium persulphate
Photochemical reactor with recirculation
300 mL
90% of color removal COD removal depended on the persulfate ion concentration
120 min
[13]
Methyl orange
10 mg L−1
Polypyrrole-TiO2 nanocomposites (no pH adjustment)
0.45 g L−1 polypyrrole-TiO2 nanocomposites suspended
Glass beaker
450 mL
~90% initial concentration removal
160 min
[213]
4-Chlorophenol
20 mg L−1
Titania Degussa P-25 and activated carbon (no pH adjustment)
0.2 g L−1
Two CPC modules in connected in series
247 L
~100% initial concentration removal
At 2000 min W m−2
[176]


### 3.3. Organic Matter Degradation by TiO2 Solar Photocatalysis

The sunlight can be used efficiently in theTiO2 photocatalytic process with the use of solar reactors that concentrate the solar irradiation. Thereby, TiO2 solar photocatalysis is cost-effective and environmentally friendly alternative.The use of CPC solar photoreactors was shown to be effective forTiO2 solar photocatalytic degradation of several organic contaminants such as antibiotics [167], azo dyes [168], water disinfection [169, 170], pesticides [8, 171], humic acids [172], agro-food industry effluents [173], and ferricyanide [174].Pereira and coworkers [167] studied the TiO2 solar photocatalytic degradation of the antibiotic amoxicillin in aqueous solutions at neutral conditions (pH 7.5). These authors reported that the solar UV radiation alone was unable to attack the antibiotic molecules during the same treatment period as in the TiO2 solar photocatalysis. They observed that the antibiotic concentration was reduced from 40 to 3.1 mg L−1 (at 4.6 kJUV L−1 of UV accumulated energy in the CPC) by TiO2 solar photocatalysis which led to a considerable reduction of the antibacterial activity with 71% mineralization at the end of the treatment. They attributed such findings mainly to hydroxyl radicals, although singlet oxygen also played an important role in the antibiotic amoxicillin self-photosensitization under UV/visible solar light.The combination ofTiO2 solar photocatalysis with H2O2 and persulfate ions S2O82−, as electron acceptors, for the degradation of azo dyes using CPC reactors was studied [168]. It was reported that the presence of hydrogen peroxide did not affect appreciably the photodegradation rate of methyl-orange but the presence of S2O82− was strongly beneficial. It was also reported that the presence of both H2O2 and S2O82− was always beneficial for orange-II degradation. Complete decolourization was achieved in a few hours for both dyes but mineralization occurred after longer times with the formation of CO2, NO3−, and SO42− ions. Jiménez-Tototzintle and coworkers [173] added H2O2 to the solar photocatalytic CPC reactor to treat pesticides (biorecalcitrant compounds) for improving supported TiO2 photocatalysis efficiency. It was reported that nearly complete removal of pesticides was acquired avoiding expensive separation of TiO2 slurries from treated wastewater.Water disinfection byTiO2 solar photocatalysis in a solar reactor was also studied in simulated wastewater containing E. coli K-12 [169] and urban effluent contaminated with E. coli and F. solani spores [170]. Fernández et al. [169] observed that bactericidal deactivation by sunlight in a CPC solar collector occurred with and without catalyst. The total photocatalytic deactivation of pure E. coli suspensions was a consequence of the combined effect of sunlight and the oxidant species generated in the TiO2 in suspensions and or by supported TiO2. The slurry TiO2 was more efficient for bacteria deactivation than the supported TiO2 in the solar photocatalytic process. García-Fernández and collaborators [170] reported that the temperature and the dissolved oxygen, the most commonly used electron acceptor, were key factors for water disinfection. Thus, changes in temperature of photocatalytic reactors for water disinfection should be considered to evaluate the efficiency of the process. Also, air sparging caused improvements in the bacterial and spore photocatalytic inactivation, which was specifically manifested in F. solani spores. This was in line with the important role of dissolved oxygen in photocatalytic water disinfection.Arellano and Martínez [174] investigated the effects of pH on the degradation of aqueous ferricyanide by photolysis and photocatalysis in the solar CPC reactor. These authors revealed that upon sunlight exposure, the conversion of ferricyanide to ferrocyanide and the reverse reaction depended strongly on the pH of the solution whether or not the TiO2 catalyst was present. Thus, the pH of the solution dictated the type of redox reaction that would proceed under illumination. Additionally, the extent of the heterogeneous photocatalytic degradation of ferricyanide was influenced by pH, but the initial concentration of ferricyanide did not affect its degradation.Tables4 and 5 summarize the degradation of several organics by TiO2 solar photocatalysis in which suspended or immobilized TiO2 was used, respectively. As can be seen, the degradation and mineralization were taken place in several solar reactors under different experimental conditions in which the oxidation of the organic matter with time was followed by parameters like DOC, TOC, COD, and organic concentration decrease. Also, the efficiency of the TiO2 solar photocatalysis depended on the suspended or immobilized TiO2 catalyst phase, nature of organic contaminant, solution pH, reaction time, and the initial concentration of the organics. Thus, these studies have shown that sunlight was used efficiently in the TiO2 solar photocatalytic process acquiring high oxidation yields.In order to take advantage of the solar photons in the visible range (400–700 nm) and make the degradation process more efficient under the sunlight, some studies were conducted using dopedTiO2 catalyst, as shown in Table 6. Solar photocatalysis using nitrogen-doped TiO2, carbon-doped TiO2, polypyrrole-TiO2 nanocomposites, and TiO2 with persulfate ion addition were conducted to oxidize diverse organics. These studies have shown better performance of the solar photocatalytic process using doped TiO2 catalyst and higher organic mineralization. The efficiency of the solar photocatalysis using carbon-doped TiO2 was ascribed to the presence of oxygen vacancy state between the valence and the conduction bands because of the formation of Ti3+ species in the as-synthesized carbon-doped titania [175]. Herrmann and coworkers [176] degraded the 4-chlorophenol compound (4-CP) by solar photocatalysis using carbon-doped TiO2. These authors reported that the addition of a commercial activated carbon to titania under UV irradiation could have induced a substantial synergy effect in the photoefficiency of the photocatalyst. It had been explained by an important adsorption of 4-CP on activated carbon (AC) followed by a mass transfer to photoactive titania. According to these authors, such transfer occurred mainly via a spillover of 4-CP through the contact surface between AC and TiO2. This interface was spontaneously created by a mere mixture of both phases in suspension. The simple mixture of the two solids had permitted to avoid a preparation procedure which would have modified the surface of both constituents and prevented a direct comparison from their initial surface state. These authors stated that the synergy effect of the AC could be extrapolated to a large solar pilot plant scale, working in the near UV fringe of sunlight.


## 3.1. Photocatalytic Activity of TiO2 under Sunlight

T
i
O
2 semiconductor is mainly photoactive with artificial UV lamps that increase the electrical cost of the photocatalytic process. The sunlight is expected to improve the performance of TiO2 photocatalysis since it provides photons in the UV range (300–400 nm); also, doping TiO2 extends its photoresponse capacity towards the sunlight visible range (400–700 nm). The chemical surface alteration of TiO2 (when doped or photodoped with transition metals, noble metals, nonmetals, organic dye sensitization, and coupled semiconductors) modifies its electronic structure producing changes in the electron densities in the conduction band [113] which enhances the solar efficiency of TiO2 under solar irradiation and, hence, influences the mechanism of the photocatalytic process. Dopants can act as electron (or hole) traps preventing charge recombination, create an intermediate energy level introduced between the conduction band and the valence band, lead to band bend gap narrowing or expansion, and induce band bending or conduction band edge shifts which occur due to disruption of the lattice structure of the dopants and formation of surface oxygen vacancies [113–116]. Introduction of such energy levels in the band gap induces the red shift in the band gap transition and the visible light absorption through a charge transfer between a dopant and conduction band (or valence band) [112]. Nevertheless, these changes depend on the nature of dopants, synthesis methods, annealing process, dopant concentration, and dopant distribution [11, 112, 113, 117–120].


## 3.2. Influencing Parameters on the Degradation of Organic Compounds by TiO2 Solar Photocatalysis

Mineralization of organic compounds (conversion toCO2 and mineral acids) by the TiO2 solar photocatalytic process depends directly on the synthesis method of the catalyst [121–126], type of doping materials [11, 112, 113, 117–120], annealing temperature [127–131], catalyst load [132–135], pollutant concentration [136–139], and pH of the aqueous solution [140–142]. There are other parameters like reaction temperature, reactor configuration (geometry), reactor material, air sparging in the reactor solution, and the solar radiation intensity (solar concentration ratio) [143] that are important too in the TiO2 solar photocatalytic process. Nevertheless, these last factors contribute in less extension to the degradation of the pollutants compared to the most commonly studied such as catalyst load, pollutant concentration, and pH of the aqueous solution.


### 3.2.1. Effect of TiO2 Annealing Temperature

The influence of annealing temperature on the microstructure, surface morphology, and optical property ofTiO2 particles, TiO2 nanoparticles, and TiO2 thin films strongly depends on the synthesis methods [144–149]. Three different phases of TiO2 have been reported which depend on the heat treatment like anatase, rutile, and brookite, anatase and rutile phases being commonly prepared [8, 9, 11, 145, 149]. It has been reported that anatase is more photoactive than rutile [1, 109, 150, 151]; however, it has also been reported that synergistic effects of mixed phases of anatase and rutile enhances the photoactivity of the photocatalyst [152–155].


### 3.2.2. Influence of Catalyst Concentration

Catalyst load is an important factor that can affect the degradation rate of the organic pollutants; the optimum amount depends on the nature of the organic compound and on the geometry of the photoreactor [156–158]. When TiO2 concentration increases from 0 to certain values, a significant enhancement of efficiency is recorded for the elimination and mineralization of organics. However, there is a loading range in which either no significant changes are observed or even a decrease in the elimination of organic compounds happens. The number of active surface sites increases with TiO2 concentration until certain loading since light penetration decreases and aggregation of TiO2 particles increases at relative high catalyst loading [159]. It has been reported that TiO2 photocatalysis combined with ultrasound can be benefited [72, 97, 159, 160] due to different factors like (a) an increase in the catalyst surface area due to the aggregation action of ultrasound, which enhances the performance of the photocatalytic system [161]; (b) an improvement of mass transfer of organic compounds between the liquid phase and the TiO2 surface [162, 163]; and (c) a reduction of charge recombination and promotion production of additional OH• due to the residual H2O2 generated [162, 163]. Also, the continuous cleaning of the TiO2 surface by acoustic cavitation [164] might also have some role in modifying the photocatalytic rate. Tables 4–6 show that different amounts of catalyst ranging from 10 mg L−1 to 4 g L−1 yielded different degrees of organic degradation during the photocatalytic oxidation process under the experimental conditions stated.Table 4
Slurry TiO2 solar photocatalysis.
Contaminant (concentration interval)
Catalyst
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Solution pH
Initial concentration
Type of reactor
Total volume
Percentage
Time
Amoxicillin
40 mg L−1
Degussa P-25 (7.5)
0.5 g L−1
CPC
15 L
70% of the residual DOC content in the form of low molecular weight
215 min
[167]
Methyl-orange, orange II
30 mg L−1
Degussa P-25 (6.4–6.7)
0.2 g L−1
CPC
39 L
90% of colour abatement and final TOC 0.11 ppm for both
—
[168]
Bisphenol A
100μg mL−1
TiO2 anatase, purity 99.9%, Wako Pure Chemical Industries (6.0)
10 mg L−1
Pyrex reaction vessel
50 mL
60% with light intensity: 1.3 m W cm−2
60 min
[98]
The commercial detergent (α-sodium fatty acid ester sulfonate, alkylaryl sulfonate, a sodium salt of a fatty acid, aluminosilicate, and sodium carbonate)
0.1 g L−1
TiO2 P-25 (4.9)
6.0 g L−1
A batch mode reactor exposed to sunlight using a mirror concentrator.
3 L
0.2 of Ct/Co
120 min
[203]
Remazol brill blue R (RBBR)
100 mg L−1
TiO2 by solution combustion method (natural pH conditions)
1 g L−1
Cylindrical borosilicate glass reactor
400 mL
0.26 of Ct/Co
150 min
[130]
Reactive yellow 17 (RY17)
Initial COD 476 mg L−1
TiO2 Degussa P25 (3.5)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 56 mg L−1 (88%)
8 h
[139]
Reactive red 2 (RR2)
Initial COD 225 mg L−1
TiO2 Degussa P25 (4.65)
4 g L−1
The cylindrical reactor
200 mL of capacity
COD 18 mg L−1 (92%)
8 h
[139]
Reactive blue 4 (RB4)
Initial COD 81 mg L−1
TiO2 Degussa P25 (4.2)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 15 mg L−1 (82%)
8 h
[139]
Escherichia coli K-12, ilitrelding
Concentration of 104 CFU mL−1
TiO2 Degussa P25 (no pH adjustment)
25 mg L−1
CPC collector
The photoreactor volume is 5.4 L
101 CFU mL−1
At 2 KJ L−1 of QUV
[169]
Reactive brilliant red K-2G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 82%
4 h
[204]
Reactive brilliant red K-BP
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 73%
4 h
[204]
Reactive yellow KD-3G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 42%
4 h
[204]
Cationic pink FG
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 61%
4 h
[204]
Methyl orange
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 52%
4 h
[204]
Humic acids
100 mg L−1
TiO2 Degussa P25 (natural pH)
1 g L−1
CPC
35 L
Removal of DOC 93%
Q
UV = 33 kJ L−1
[172]
Reactive yellow 14
5 × 10−4 mol L−1
TiO2 Degussa P25 (5.5)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Degradation 84.4%
60 min
[138]
Nitrobenzene
300 mg L−1
Degussa P-25 TiO2 (4.5)
0.3% (w/v of the solution)
Cylindrical reactor
465 mL of capacity
96% destruction of TOC
240 min
[205]
Propranolol
50 mg L−1
Degussa P-25 (no pH adjustment)
0.4 g L−1
Pilot plant (6 parallel CPCs) (concentration factor of 1, CCPC = 1)
10 L
81% of degradation
240 min
[133]
Reactive orange 4
5 × 10−4 mol L−1
Degussa P-25 (4.8)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Dye degradation 97%
150 min
[206]
Phenol
20 mg L−1
A home-made TiO2“TiEt-450” (between 5.2 and 6.2)
500 mg L−1
CPC
35 L
Smaller than 3 mg L−1
200 min
[207]
Diclofenac (DCF) and naproxen (NPX) 1 : 1 mixture
30 mg L−1
TiO2 P25 Aeroxide® (ambient pH)
0.1 g L−1
Immersion-well photoreactor
400 mL
Total COD reductions of 76%
360 min
[208]
Imazalil (IMZ), thiabendazole (TBZ), and acetamiprid (ACP)
9.0μg L−1 of IMZ, 12.6 μg L−1 of TBZ, and 20.4 μg L−1 of ACP
Evonik P25 TiO2 (7.2–8.0)
200 mg L−1
CPC
8 L
Removal 68% ACP and 85% TBZ and 100% of IMZ
20 kJ L−1
[173]
Synthetic sewage
200 mg L−1 DOC
TiO2 Degussa P25 and sodium peroxydisulfate (Na2S2O8) (3.3)
TiO2 = 200 mg L−1 Na2S2O8 = 4300 mg L−1
CPC
35 L
73% decrease in the initial DOC
5 h
[209]
Ferricyanide
4 × 10−3–10 × 10−3 mol L−1 of Fe(CN)63−, pH values tested were 10, 11, 12, 13, and 14
TiO2 Sigma-Aldrich 93% anatase and 7% rutile, particle size < 25 nm (pH values tested were 10, 11, 12, 13, and 14)
600 mg L−1
CPC
1.5 L
Sunlight exposure with TiO2 the total amounts of ferricyanide and cyanide decreased 94%, whereas only 4.8% was decreased with solar photolysis
24 h
[174]


### 3.2.3. Influence of Initial Pollutant Concentration and pH of the Solution

The initial concentration of the organic compounds at constant pH and different initial pH of the solution are also important factors that affect the degradation rate of the organic pollutants and the efficiency of the photocatalytic oxidation process.As the initial concentration of organics increases, the photocatalytic efficiency decreases due to a decrease of the reaction rate, which is attributed to a decrease in the number of photons andTiO2 particles available, since the number of organic molecules adsorbed onto the catalyst may block catalyst activation. Also, the initial pH of the solution influences the rate of the degradation process. It has been reported that the adsorption of the organic compounds onto the TiO2 surface is affected by the pH of the solution [97, 160]. The pollutant and thus the rates of degradation will be maximum near the point of zero charge (pzc) of the catalyst [164]. The pzc of TiO2 surface is at pHpzc between 6.25 and 7.1 [1, 165, 166], depending on the ionic strength [166]. Tables 4, 5, and 6 show that different initial pollutant concentration and solution pH were used to degrade different organics during the photocatalytic oxidation process under the experimental conditions stated. Most of the experiments were carried out in the pH range of 2.0–14, and some were with no pH control, as depicted on Tables 4–6.Table 5
Immobilized TiO2 solar photocatalysis.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Method of synthesis
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Atrazine
20 mg L−1
Sol-gel method using titanium butoxide
180 spheres of TiO2-coated glass sustained by a nylon mesh (3.0)
0.3 g L−1
An open, undivided and cylindrical tank reactor
200 mL
Reduction of 30% of initial concentration
300 min
[202]
Methylene blue
50 mg L−1
Hydrothermal method
TiO2 Degussa P25 supported on black volcanic ashes TVA (no pH adjustment)
3 g L−1 TVA
Stirred photoreactors with parabolic sunlight irradiation concentrators
50 mL
95% degradation of wastewater pollutant
120 min
[210]
Salicylic acid
165 mg L−1
Sol-gel method using titanium butoxide
TiO2 coating onto borosilicate glass spheres of 5 mm diameter (3.0)
0.25 g TiO2 L−1
A polycarbonate box with a mirror at the bottom and tilted 41°
3.0 L
Reduction of 14% of initial concentration
360 min
[194]
Acetaminophen, thiabendazole, acetamiprid, and imazalil
100μg L−1 each
Sol-gel technique using titanium isopropoxide
Glass spheres (6 mmφ) were dip-coated with the TiO2 sol (6.2–8.4)
0.6 mg of TiO2 on the surface of each glass bead
CPC
8 L
Reduction of 100% of initial concentration
240 min
[122]Table 6
Solar photocatalysis using nitrogen-doped TiO2, carbon-doped TiO2, polypyrrole TiO2 nanocomposites, and a mix of TiO2 with persulfate ions.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Cefazolin
Concentration of 1.0 × 10−2 mol L−1
N-doped TiO2 (6.4)
2.0 g L−1
Batch-type photoreactor
600 mL
80% of cefazolin removed
30 min
[211]
Azo dye orange G
25 mg L−1
Nitrogen-doped TiO2 (2.0)
1.0 g L−1
Glass beaker
1000 mL
Efficiency of degradation greater than 95%
40 min
[212]
Methylene blue
20 mg L−1
Carbon-doped TiO2 nanoparticles (neutral pH)
1.0 g L−1
Batch-type photoreactor
200 mL of 10 mg/L methylene blue
Greater than 0.1 Ct/Co
60 min
[175]
Acid orange 7 in the concentration
0.2 mM L−1
Combination of TiO2 with potassium persulphate (3.0)
TiO2 (200 mg L−1) and 10 mM L−1of potassium persulphate
Photochemical reactor with recirculation
300 mL
90% of color removal COD removal depended on the persulfate ion concentration
120 min
[13]
Methyl orange
10 mg L−1
Polypyrrole-TiO2 nanocomposites (no pH adjustment)
0.45 g L−1 polypyrrole-TiO2 nanocomposites suspended
Glass beaker
450 mL
~90% initial concentration removal
160 min
[213]
4-Chlorophenol
20 mg L−1
Titania Degussa P-25 and activated carbon (no pH adjustment)
0.2 g L−1
Two CPC modules in connected in series
247 L
~100% initial concentration removal
At 2000 min W m−2
[176]


## 3.2.1. Effect of TiO2 Annealing Temperature

The influence of annealing temperature on the microstructure, surface morphology, and optical property ofTiO2 particles, TiO2 nanoparticles, and TiO2 thin films strongly depends on the synthesis methods [144–149]. Three different phases of TiO2 have been reported which depend on the heat treatment like anatase, rutile, and brookite, anatase and rutile phases being commonly prepared [8, 9, 11, 145, 149]. It has been reported that anatase is more photoactive than rutile [1, 109, 150, 151]; however, it has also been reported that synergistic effects of mixed phases of anatase and rutile enhances the photoactivity of the photocatalyst [152–155].


## 3.2.2. Influence of Catalyst Concentration

Catalyst load is an important factor that can affect the degradation rate of the organic pollutants; the optimum amount depends on the nature of the organic compound and on the geometry of the photoreactor [156–158]. When TiO2 concentration increases from 0 to certain values, a significant enhancement of efficiency is recorded for the elimination and mineralization of organics. However, there is a loading range in which either no significant changes are observed or even a decrease in the elimination of organic compounds happens. The number of active surface sites increases with TiO2 concentration until certain loading since light penetration decreases and aggregation of TiO2 particles increases at relative high catalyst loading [159]. It has been reported that TiO2 photocatalysis combined with ultrasound can be benefited [72, 97, 159, 160] due to different factors like (a) an increase in the catalyst surface area due to the aggregation action of ultrasound, which enhances the performance of the photocatalytic system [161]; (b) an improvement of mass transfer of organic compounds between the liquid phase and the TiO2 surface [162, 163]; and (c) a reduction of charge recombination and promotion production of additional OH• due to the residual H2O2 generated [162, 163]. Also, the continuous cleaning of the TiO2 surface by acoustic cavitation [164] might also have some role in modifying the photocatalytic rate. Tables 4–6 show that different amounts of catalyst ranging from 10 mg L−1 to 4 g L−1 yielded different degrees of organic degradation during the photocatalytic oxidation process under the experimental conditions stated.Table 4
Slurry TiO2 solar photocatalysis.
Contaminant (concentration interval)
Catalyst
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Solution pH
Initial concentration
Type of reactor
Total volume
Percentage
Time
Amoxicillin
40 mg L−1
Degussa P-25 (7.5)
0.5 g L−1
CPC
15 L
70% of the residual DOC content in the form of low molecular weight
215 min
[167]
Methyl-orange, orange II
30 mg L−1
Degussa P-25 (6.4–6.7)
0.2 g L−1
CPC
39 L
90% of colour abatement and final TOC 0.11 ppm for both
—
[168]
Bisphenol A
100μg mL−1
TiO2 anatase, purity 99.9%, Wako Pure Chemical Industries (6.0)
10 mg L−1
Pyrex reaction vessel
50 mL
60% with light intensity: 1.3 m W cm−2
60 min
[98]
The commercial detergent (α-sodium fatty acid ester sulfonate, alkylaryl sulfonate, a sodium salt of a fatty acid, aluminosilicate, and sodium carbonate)
0.1 g L−1
TiO2 P-25 (4.9)
6.0 g L−1
A batch mode reactor exposed to sunlight using a mirror concentrator.
3 L
0.2 of Ct/Co
120 min
[203]
Remazol brill blue R (RBBR)
100 mg L−1
TiO2 by solution combustion method (natural pH conditions)
1 g L−1
Cylindrical borosilicate glass reactor
400 mL
0.26 of Ct/Co
150 min
[130]
Reactive yellow 17 (RY17)
Initial COD 476 mg L−1
TiO2 Degussa P25 (3.5)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 56 mg L−1 (88%)
8 h
[139]
Reactive red 2 (RR2)
Initial COD 225 mg L−1
TiO2 Degussa P25 (4.65)
4 g L−1
The cylindrical reactor
200 mL of capacity
COD 18 mg L−1 (92%)
8 h
[139]
Reactive blue 4 (RB4)
Initial COD 81 mg L−1
TiO2 Degussa P25 (4.2)
2 g L−1
The cylindrical reactor
200 mL of capacity
COD 15 mg L−1 (82%)
8 h
[139]
Escherichia coli K-12, ilitrelding
Concentration of 104 CFU mL−1
TiO2 Degussa P25 (no pH adjustment)
25 mg L−1
CPC collector
The photoreactor volume is 5.4 L
101 CFU mL−1
At 2 KJ L−1 of QUV
[169]
Reactive brilliant red K-2G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 82%
4 h
[204]
Reactive brilliant red K-BP
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 73%
4 h
[204]
Reactive yellow KD-3G
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 42%
4 h
[204]
Cationic pink FG
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 61%
4 h
[204]
Methyl orange
20 mg L−1
TiO2 Beijing Chemical Industrial Company (no pH adjustment)
1 g L−1
Pyrex beakers
1 L
Removal of TOC 52%
4 h
[204]
Humic acids
100 mg L−1
TiO2 Degussa P25 (natural pH)
1 g L−1
CPC
35 L
Removal of DOC 93%
Q
UV = 33 kJ L−1
[172]
Reactive yellow 14
5 × 10−4 mol L−1
TiO2 Degussa P25 (5.5)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Degradation 84.4%
60 min
[138]
Nitrobenzene
300 mg L−1
Degussa P-25 TiO2 (4.5)
0.3% (w/v of the solution)
Cylindrical reactor
465 mL of capacity
96% destruction of TOC
240 min
[205]
Propranolol
50 mg L−1
Degussa P-25 (no pH adjustment)
0.4 g L−1
Pilot plant (6 parallel CPCs) (concentration factor of 1, CCPC = 1)
10 L
81% of degradation
240 min
[133]
Reactive orange 4
5 × 10−4 mol L−1
Degussa P-25 (4.8)
4 g L−1
Open borosilicate glass tube, 40 cm height and 20 mm diameter
50 mL capacity
Dye degradation 97%
150 min
[206]
Phenol
20 mg L−1
A home-made TiO2“TiEt-450” (between 5.2 and 6.2)
500 mg L−1
CPC
35 L
Smaller than 3 mg L−1
200 min
[207]
Diclofenac (DCF) and naproxen (NPX) 1 : 1 mixture
30 mg L−1
TiO2 P25 Aeroxide® (ambient pH)
0.1 g L−1
Immersion-well photoreactor
400 mL
Total COD reductions of 76%
360 min
[208]
Imazalil (IMZ), thiabendazole (TBZ), and acetamiprid (ACP)
9.0μg L−1 of IMZ, 12.6 μg L−1 of TBZ, and 20.4 μg L−1 of ACP
Evonik P25 TiO2 (7.2–8.0)
200 mg L−1
CPC
8 L
Removal 68% ACP and 85% TBZ and 100% of IMZ
20 kJ L−1
[173]
Synthetic sewage
200 mg L−1 DOC
TiO2 Degussa P25 and sodium peroxydisulfate (Na2S2O8) (3.3)
TiO2 = 200 mg L−1 Na2S2O8 = 4300 mg L−1
CPC
35 L
73% decrease in the initial DOC
5 h
[209]
Ferricyanide
4 × 10−3–10 × 10−3 mol L−1 of Fe(CN)63−, pH values tested were 10, 11, 12, 13, and 14
TiO2 Sigma-Aldrich 93% anatase and 7% rutile, particle size < 25 nm (pH values tested were 10, 11, 12, 13, and 14)
600 mg L−1
CPC
1.5 L
Sunlight exposure with TiO2 the total amounts of ferricyanide and cyanide decreased 94%, whereas only 4.8% was decreased with solar photolysis
24 h
[174]


## 3.2.3. Influence of Initial Pollutant Concentration and pH of the Solution

The initial concentration of the organic compounds at constant pH and different initial pH of the solution are also important factors that affect the degradation rate of the organic pollutants and the efficiency of the photocatalytic oxidation process.As the initial concentration of organics increases, the photocatalytic efficiency decreases due to a decrease of the reaction rate, which is attributed to a decrease in the number of photons andTiO2 particles available, since the number of organic molecules adsorbed onto the catalyst may block catalyst activation. Also, the initial pH of the solution influences the rate of the degradation process. It has been reported that the adsorption of the organic compounds onto the TiO2 surface is affected by the pH of the solution [97, 160]. The pollutant and thus the rates of degradation will be maximum near the point of zero charge (pzc) of the catalyst [164]. The pzc of TiO2 surface is at pHpzc between 6.25 and 7.1 [1, 165, 166], depending on the ionic strength [166]. Tables 4, 5, and 6 show that different initial pollutant concentration and solution pH were used to degrade different organics during the photocatalytic oxidation process under the experimental conditions stated. Most of the experiments were carried out in the pH range of 2.0–14, and some were with no pH control, as depicted on Tables 4–6.Table 5
Immobilized TiO2 solar photocatalysis.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Method of synthesis
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Atrazine
20 mg L−1
Sol-gel method using titanium butoxide
180 spheres of TiO2-coated glass sustained by a nylon mesh (3.0)
0.3 g L−1
An open, undivided and cylindrical tank reactor
200 mL
Reduction of 30% of initial concentration
300 min
[202]
Methylene blue
50 mg L−1
Hydrothermal method
TiO2 Degussa P25 supported on black volcanic ashes TVA (no pH adjustment)
3 g L−1 TVA
Stirred photoreactors with parabolic sunlight irradiation concentrators
50 mL
95% degradation of wastewater pollutant
120 min
[210]
Salicylic acid
165 mg L−1
Sol-gel method using titanium butoxide
TiO2 coating onto borosilicate glass spheres of 5 mm diameter (3.0)
0.25 g TiO2 L−1
A polycarbonate box with a mirror at the bottom and tilted 41°
3.0 L
Reduction of 14% of initial concentration
360 min
[194]
Acetaminophen, thiabendazole, acetamiprid, and imazalil
100μg L−1 each
Sol-gel technique using titanium isopropoxide
Glass spheres (6 mmφ) were dip-coated with the TiO2 sol (6.2–8.4)
0.6 mg of TiO2 on the surface of each glass bead
CPC
8 L
Reduction of 100% of initial concentration
240 min
[122]Table 6
Solar photocatalysis using nitrogen-doped TiO2, carbon-doped TiO2, polypyrrole TiO2 nanocomposites, and a mix of TiO2 with persulfate ions.
Contaminant (concentration interval)
Experimental conditions
Reactor
Best degradation conditions
Reference
Name
Initial concentration
Catalyst (pH)
Initial concentration
Type of reactor
Total volume
Percentage
Time
Cefazolin
Concentration of 1.0 × 10−2 mol L−1
N-doped TiO2 (6.4)
2.0 g L−1
Batch-type photoreactor
600 mL
80% of cefazolin removed
30 min
[211]
Azo dye orange G
25 mg L−1
Nitrogen-doped TiO2 (2.0)
1.0 g L−1
Glass beaker
1000 mL
Efficiency of degradation greater than 95%
40 min
[212]
Methylene blue
20 mg L−1
Carbon-doped TiO2 nanoparticles (neutral pH)
1.0 g L−1
Batch-type photoreactor
200 mL of 10 mg/L methylene blue
Greater than 0.1 Ct/Co
60 min
[175]
Acid orange 7 in the concentration
0.2 mM L−1
Combination of TiO2 with potassium persulphate (3.0)
TiO2 (200 mg L−1) and 10 mM L−1of potassium persulphate
Photochemical reactor with recirculation
300 mL
90% of color removal COD removal depended on the persulfate ion concentration
120 min
[13]
Methyl orange
10 mg L−1
Polypyrrole-TiO2 nanocomposites (no pH adjustment)
0.45 g L−1 polypyrrole-TiO2 nanocomposites suspended
Glass beaker
450 mL
~90% initial concentration removal
160 min
[213]
4-Chlorophenol
20 mg L−1
Titania Degussa P-25 and activated carbon (no pH adjustment)
0.2 g L−1
Two CPC modules in connected in series
247 L
~100% initial concentration removal
At 2000 min W m−2
[176]


## 3.3. Organic Matter Degradation by TiO2 Solar Photocatalysis

The sunlight can be used efficiently in theTiO2 photocatalytic process with the use of solar reactors that concentrate the solar irradiation. Thereby, TiO2 solar photocatalysis is cost-effective and environmentally friendly alternative.The use of CPC solar photoreactors was shown to be effective forTiO2 solar photocatalytic degradation of several organic contaminants such as antibiotics [167], azo dyes [168], water disinfection [169, 170], pesticides [8, 171], humic acids [172], agro-food industry effluents [173], and ferricyanide [174].Pereira and coworkers [167] studied the TiO2 solar photocatalytic degradation of the antibiotic amoxicillin in aqueous solutions at neutral conditions (pH 7.5). These authors reported that the solar UV radiation alone was unable to attack the antibiotic molecules during the same treatment period as in the TiO2 solar photocatalysis. They observed that the antibiotic concentration was reduced from 40 to 3.1 mg L−1 (at 4.6 kJUV L−1 of UV accumulated energy in the CPC) by TiO2 solar photocatalysis which led to a considerable reduction of the antibacterial activity with 71% mineralization at the end of the treatment. They attributed such findings mainly to hydroxyl radicals, although singlet oxygen also played an important role in the antibiotic amoxicillin self-photosensitization under UV/visible solar light.The combination ofTiO2 solar photocatalysis with H2O2 and persulfate ions S2O82−, as electron acceptors, for the degradation of azo dyes using CPC reactors was studied [168]. It was reported that the presence of hydrogen peroxide did not affect appreciably the photodegradation rate of methyl-orange but the presence of S2O82− was strongly beneficial. It was also reported that the presence of both H2O2 and S2O82− was always beneficial for orange-II degradation. Complete decolourization was achieved in a few hours for both dyes but mineralization occurred after longer times with the formation of CO2, NO3−, and SO42− ions. Jiménez-Tototzintle and coworkers [173] added H2O2 to the solar photocatalytic CPC reactor to treat pesticides (biorecalcitrant compounds) for improving supported TiO2 photocatalysis efficiency. It was reported that nearly complete removal of pesticides was acquired avoiding expensive separation of TiO2 slurries from treated wastewater.Water disinfection byTiO2 solar photocatalysis in a solar reactor was also studied in simulated wastewater containing E. coli K-12 [169] and urban effluent contaminated with E. coli and F. solani spores [170]. Fernández et al. [169] observed that bactericidal deactivation by sunlight in a CPC solar collector occurred with and without catalyst. The total photocatalytic deactivation of pure E. coli suspensions was a consequence of the combined effect of sunlight and the oxidant species generated in the TiO2 in suspensions and or by supported TiO2. The slurry TiO2 was more efficient for bacteria deactivation than the supported TiO2 in the solar photocatalytic process. García-Fernández and collaborators [170] reported that the temperature and the dissolved oxygen, the most commonly used electron acceptor, were key factors for water disinfection. Thus, changes in temperature of photocatalytic reactors for water disinfection should be considered to evaluate the efficiency of the process. Also, air sparging caused improvements in the bacterial and spore photocatalytic inactivation, which was specifically manifested in F. solani spores. This was in line with the important role of dissolved oxygen in photocatalytic water disinfection.Arellano and Martínez [174] investigated the effects of pH on the degradation of aqueous ferricyanide by photolysis and photocatalysis in the solar CPC reactor. These authors revealed that upon sunlight exposure, the conversion of ferricyanide to ferrocyanide and the reverse reaction depended strongly on the pH of the solution whether or not the TiO2 catalyst was present. Thus, the pH of the solution dictated the type of redox reaction that would proceed under illumination. Additionally, the extent of the heterogeneous photocatalytic degradation of ferricyanide was influenced by pH, but the initial concentration of ferricyanide did not affect its degradation.Tables4 and 5 summarize the degradation of several organics by TiO2 solar photocatalysis in which suspended or immobilized TiO2 was used, respectively. As can be seen, the degradation and mineralization were taken place in several solar reactors under different experimental conditions in which the oxidation of the organic matter with time was followed by parameters like DOC, TOC, COD, and organic concentration decrease. Also, the efficiency of the TiO2 solar photocatalysis depended on the suspended or immobilized TiO2 catalyst phase, nature of organic contaminant, solution pH, reaction time, and the initial concentration of the organics. Thus, these studies have shown that sunlight was used efficiently in the TiO2 solar photocatalytic process acquiring high oxidation yields.In order to take advantage of the solar photons in the visible range (400–700 nm) and make the degradation process more efficient under the sunlight, some studies were conducted using dopedTiO2 catalyst, as shown in Table 6. Solar photocatalysis using nitrogen-doped TiO2, carbon-doped TiO2, polypyrrole-TiO2 nanocomposites, and TiO2 with persulfate ion addition were conducted to oxidize diverse organics. These studies have shown better performance of the solar photocatalytic process using doped TiO2 catalyst and higher organic mineralization. The efficiency of the solar photocatalysis using carbon-doped TiO2 was ascribed to the presence of oxygen vacancy state between the valence and the conduction bands because of the formation of Ti3+ species in the as-synthesized carbon-doped titania [175]. Herrmann and coworkers [176] degraded the 4-chlorophenol compound (4-CP) by solar photocatalysis using carbon-doped TiO2. These authors reported that the addition of a commercial activated carbon to titania under UV irradiation could have induced a substantial synergy effect in the photoefficiency of the photocatalyst. It had been explained by an important adsorption of 4-CP on activated carbon (AC) followed by a mass transfer to photoactive titania. According to these authors, such transfer occurred mainly via a spillover of 4-CP through the contact surface between AC and TiO2. This interface was spontaneously created by a mere mixture of both phases in suspension. The simple mixture of the two solids had permitted to avoid a preparation procedure which would have modified the surface of both constituents and prevented a direct comparison from their initial surface state. These authors stated that the synergy effect of the AC could be extrapolated to a large solar pilot plant scale, working in the near UV fringe of sunlight.


## 4. Scaling-Up of the Solar Processes

The application of solar-powered photoreactors for wastewater treatment represent an environmental alternative specially for regions receiving strong sunlight throughout the year. The solar photoreactors decrease the operating, capital, and maintenance costs associated to photocatalytic reaction systems that are powered with UV lamps. Thus, an appropriate design of solar photoreactors is important to ensure efficient conversion of incident photons to oxidant reactive species such asOH• and holes, among some others [177]. According to Sagawe et al., several parameters need to be addressed for the design of field-scale photoreactors such as pollutant concentration (COD initial load), volumetric flow rate, light intensity, and solar irradiation area; also, the concentration of dissolved oxygen in water, in equilibrium with atmospheric air, defines the limits of all practical oxidizing processes for removing pollutants in photocatalytic reactors [178].The variability in both the composition and concentration of real wastewater effluents in addition to the solar photon flux variation during the degradation process makes more difficult the field-scale reactors and also increases the cost. Soares et al. made an economic assessment using UVA-vis radiation (solar light) or UVC radiation (lamps) based on the operation variables obtained for the treatment of 30,240 m3 per day of a textile wastewater after a biological preoxidation process (to achieve the values required by German regulations for discharge into water bodies); from this study, the following conclusions were withdrawn: (a) at acidic pH values, the addition of iron to the UVC/H2O2 reaction enhanced the decolourisation rates, resulting in a lower treatment cost when compared to neutral pH conditions; (b) the UVC/H2O2 system at natural wastewater pH is cheaper than at acid pH, mainly due to the need for acids and bases; (c) the use of solar radiation (UVA-vis) increases the treatment costs, mainly due to an increase in the capital spending associated with CPC; (d) the addition of oxalic acid to the photo-Fenton reaction decreases the capital spending (high reaction rates), but the cost of consumables increases significantly, making the treatment more costly; and (e) the photo-Fenton system mediated by ferrioxalate at near neutral pH using solar radiation is the most costly treatment process, due to the low decolourization rates and high consumption of reactants, especially oxalic acid [179].Silva et al. proposed a methodology for the treatment of landfill leachates, after aerobic lagooning and adjusted at pilot scale. Such methodology involved an aerobic activated sludge biological preoxidation, a coagulation/sedimentation step and a photooxidation through a photo-Fenton reaction combining solar and artificial light [108]. These authors reported that the H2O2 was the reactant that most contributed to the final treatment cost (~42%), while the sulphuric acid and the ferrous iron were the chemicals that contributed less (~1%). Finally, the combination of solar and artificial radiation, taking into account the energetic needs throughout the year, showed to be the best alternative to treat 100 m3/day of leachate targeting a COD value lesser than 150 ppm and 1000 mg O2/L.Jordá et al. performed an economic evaluation of the photo-Fenton process to degrade paracetamol in water to form biodegradable reaction intermediates which can be finally removed with a downstream biological treatment [180]. These authors observed that the key feature was to find the shortest chemical treatment time necessary to reach a sufficiently high biodegradability of the treated water which minimized the cost of the overall process.A comparison ofTiO2 solar photocatalysis and solar photo-Fenton for the treatment of pesticides from industrial wastewater was carried out to assess the viability of solar heterogeneous photocatalysis (UV/TiO2) and photo-Fenton (UV/Fe2+/H2O2) for the treatment of agrochemical industrial wastewater at lab scale using CPC reactors. Also, the operational conditions, kinetics, and treatment costs were estimated [181]. Their results showed that the cost of photo-Fenton process was more economical than (UV/TiO2) photocatalysis and (UV/TiO2/H2O2) processes. In addition, the maximum COD removal (90.7%) by photo-Fenton process was higher than that obtained by TiO2 photocatalysis (79.6%) and the cost was 34.8% more economical, which was considered the best solution concerning the process performance. Finally, these authors observed that the variation of operating costs mainly depends on the type and dosage of chemicals.Zapata et al. developed a strategy targeting the design of an industrial scale combined solar photo-Fenton/aerobic biological system for the decontamination of commercial pesticides [182] using CPC reactors. These authors recommended that for adequate design of this type of treatment, a detailed study should be done for each particular case using different analytical tools and bioassays, mainly dissolved organic carbon, chemical oxygen demand, toxicity, and biodegradability. It was demonstrated that the H2O2 dose was a critical parameter for the design and control of operation of the combined system. It also remarked the importance of the wide difference in efficiency found in the biological treatment stage when the integrated system was scaled up. Based on their results, these authors highlighted how decisive and restrictive (for the treatment of very specific and variable wastewater) start-up and growth could be in implementing a new biological reactor, especially when the biotreatment is performed in an immobilized biomass reactor which is much more resistant than a conventional sequencing batch reactor. Their observations highlighted the limitations of the results obtained in small laboratory devices and working with model wastewaters to design a proper treatment [182].Chong et al. [183] published an interesting review on the research and development progresses of engineered photocatalysts, photoreactor systems, and the process optimizations and modellings of the photooxidation processes for water treatment. These authors mentioned several key technical constraints ranging from catalyst development to reactor design and process optimization that have to be addressed, such as (a) catalyst improvement for a high photoefficiency that can utilize wider solar spectra, (b) catalyst immobilization strategy to provide a cost-effective solid/liquid separation, (c) effective design of solar photoreactors because of the low efficacy design of current solar collecting technology (0.04% capture of original solar photons), and (d) the need of a large scale, solar-driven, photocatalytic treatment process with high efficacy and low site area requirements with different possible pilot plant configurations.


## 5. Concluding Remarks

Solar-driven photocatalysis, as in the processes of solar photo-Fenton andTiO2 solar photocatalysis, is an environmentally friendly alternative mainly because the use of electricity can be decreased/avoided. Indeed, the solar-driven processes can be driven by a photovoltaic system when scale up to a pilot plant or solar plant to decrease the costs associated with electricity consumption. These two solar photocatalytic processes represent powerful tools for removing organic pollutants from aqueous solution. Total mineralization of diverse organics has been achieved under different experimental conditions. Mineralization of organics with these solar processes depends on the nature of the contaminants and on other parameters such as solution pH, catalyst amount, and initial concentration of organics. Thus, to yield high mineralization, each process requires optimal experimental conditions of such parameters. However, in order to take advantage of the solar light in these solar photocatalytic technologies, photoreactors need to be specifically designed for these purposes. The literature reports the use of different types of reactors to treat wastewater by these solar-driven processes, but some are difficult to scale up.



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*Source: 8528063-2017-07-09.xml*