WO2016192755A1

WO2016192755A1 - Titanium dioxide-catalysed oxidation method and use thereof

Info

Publication number: WO2016192755A1
Application number: PCT/EP2015/061991
Authority: WO
Inventors: Luis Domínguez SÁNCHEZ; Martin Sebastian Walter
Original assignee: Sánchez Luis Domínguez; Martin Sebastian Walter
Priority date: 2015-05-29
Filing date: 2015-05-29
Publication date: 2016-12-08

Abstract

The invention refers to a method for the oxidation of organic or inorganic substrates in the presence of a heterogeneous titanium dioxide catalyst, an organic peroxide or hydrogen peroxide and an acid, wherein the pKa of the acid is 3 or lower. The method of the invention may advantageously be employed in the degradation of contaminants in fluids, in the desulfurization and denitrogenation of oils and fuels, in the bleaching of fibres, in the improvement of the whiteness and/or appearance of food, etc. No external irradiation or electric energy is needed.

Description

TITANIUM DIOXIDE-CATALYSED OXIDATION METHOD AND USE

THEREOF

FIELD OF THE INVENTION

The present invention relates to a method for oxidizing a substrate by means of a heterogeneous Titanium dioxide (TiO₂) catalyst in accordance with claim 1 and a use of said method.

BACKGROUND

Methods for oxidising substrates, such as pollutants, are vastly known and vary greatly in their nature, finding widespread applications in industry, e.g. in the purification of wastewater, desulfurization and denitrogenation of oils and fuels or bleaching of fibres, among others.

Out of said methods of oxidation, those based on transition-metal catalysis represent an important subgroup of particular interest.

Classical transition-metal catalysed oxidations make use of homogenous iron catalysts and hydrogen peroxide. The industrial applicability of these classical reactions is however somewhat limited for a number of reasons, for example in that the oxidation requires high amounts of iron to be effective, which in most cases implies a further iron-removal treatment of the decontaminated solution.

Alternative oxidation methods for overcoming the drawbacks of classical systems are continuously being studied in view of their great potential industrial applicability in the above mentioned fields. Alternatives to said classical systems include the use of heterogeneous catalysts consisting of non-iron transition metal species alone or in combination with iron, or the use of external energy sources such as UV-visible radiation or ultrasounds to promote oxidation.

TiO₂ is the natural oxide of titanium. TiO₂ is commonly used in the oxidation of substrates as a catalyst activated in presence of UV light and often in the presence of an oxidizing agent such as H₂O₂.

Reported methods of oxidation employing TiO₂ as a catalyst are generally described to be most efficient in neutral or basic media. Singh et al. (Iranian Journal of Environmental Health, Science & Engineering, 2013, 10: 13) explore the effect of pH in the degradation of wastewater pollutants employing TiO₂ and H2O2 among other reaction conditions, and conclude that the optimal pH for the TiO2-catalysed oxidation is in the alkaline range. This observation is reinforced by the findings of Gota et al. (International Journal of Current Engineering and Technology, 2014, 4 (1 ), 156-1 59), Jain et al. (Journal of Environmental Management, 2007, 85(4), 956-964) and several others.

In accordance with the above, the use of acids in TiO₂-catalysed oxidations is generally limited to specific purposes such as catalyst doping, as described in WO201 1080080, or to increasing the solubility of substrates to be oxidised, e.g. the mixture H2O2/acetic acid has been employed to solubilise lignin in delignification processes.

The adsorption of water on TiO₂ surface, which has a strong influence on its Lewis acid behavior, can be classified as molecular or dissociative adsorption. This last one is considered as the most favorable for the low coordination states of Ti sites [ Bourikas, K., C. Kordulis, and A. Lycourghiotis, Titanium Dioxide (Anatase and Rutile): Surface Chemistry, Liquid-Solid Interface Chemistry, and Scientific Synthesis of Supported Catalysts. Chemical reviews, 2014. 114(19): p. 9754-9823.].

The Lewis acidity of Ti sites in TiO₂ anatase surface has been described and classified in the work of Hadjiivanov and co-worker [Hadjiivanov, K. , J. Lamotte, and J.-C. Lavalley, FTIR study of low-temperature CO adsorption on pure and ammonia-precovered Ti0₂ (anatase). Langmuir, 1997. 13(13): p. 3374-3381 ].

The most acidic Ti sites in TiO₂, named as a and β-sites, were described as tetra and penta coordinated titanium atoms. Besides, it was assigned an IR signal of adsorption of CO at low temperature with a peak around 2210 cm^"1 for a sites and a broader region from 2191 to 2179 cm^"1 for β ones.

In this regard, the pivotal role of tetracoordinate titanium atoms in titanosilicate (TS-1 ) to catalyze the oxidation of organic compounds in presence of H2O2/H2O underlines the importance of this coordinative structure as active site. In fact, the study of this catalyst has shown that the hexacoordination of titanium atoms is not active in comparison with the tetrahedral one [Bordiga, S., et al., Reactivity of Ti (iv) species hosted in TS-1 towards H2O2-H2O solutions investigated by ab initio cluster and periodic approaches combined with experimental XANES and EXAFS data: a review and new highlights. Physical Chemistry Chemical Physics, 2007. 9(35): p. 4854-4878]. However, the signal of tetracoordinate titanium sites in TS-1 and TiO₂ is not equal according to identification system of Hadjiivanov et al. due to the distorsions provoked by the matrix of the active sites (Si0₂ or Ti0₂) and therefore, an easy identification of tetracoordinate titanium sites has been remained elusive for Ti0₂ [Bonelli, B., et al., Study of the surface acidity of Ti0₂/Si0₂ catalysts by means of FTIR measurements of CO and NH3 adsorption. J Catal, 2007. 246(2): p. 293-300], Recent works of Deiana et al. [Deiana, C, et al., Shape-controlled Ti0₂ nanoparticles and Ti0₂ P25 interacting with CO and H₂0₂ molecular probes: a synergic approach for surface structure recognition and physico-chemical understanding. Physical Chemistry Chemical Physics, 2013. 15(1 ): p. 307-315; and Mino, L, et al., Particles morphology and surface properties as investigated by HRTEM, FTIR, and periodic DFT calculations: from pyrogenic Ti0₂ (P25) to nanoanatase. The Journal of Physical Chemistry C, 2012. 116(32): p. 17008- 17018] related these alpha sites to 3 and 4 fold coordinated titanium atoms located on defects with a more precise peak around 2008 cm^"1. Besides, these works pointed out the signal assigned to β sites as an overlapping between pentacoordinated titanium atoms present at (101 ) face (peak at 2179 cm^"1) and tetracoordinate titanium atoms present at (1 10) face (peak at 2185 cm^"1) of anatase Ti0₂. Finally, it is also important to underline that under certain conditions (001 ) face can also contain tetracoordinate titanium atoms to form the (1 x4) reconstruction. Since the presence of water during crystallization prevents the appearance of this reconstruction [BOURIKAS et al. 2014], it can be considered that such reconstruction can only be present at particles eluding this circumstance like P25, which is fabricated via flame method.

On the other hand, the Lewis acidity in rutile surface was also studied with the same methodology used by Hadjiivanv et al. The first results showed a total absence of 4 or 3 fold coordinated titanium atoms [Ferretto, L. and A. Glisenti, Surface acidity and basicity of a rutile powder. Chemistry of materials, 2003. 15(5): p. 1 181 -1188]. However, Mino et al. [Mino, L, et al., Rutile surface properties beyond the single crystal approach: new insights from the experimental investigation of different polycrystalline samples and periodic DFT calculations. The Journal of Physical Chemistry C, 2013. 117(21 ): p. 1 1 186- 1 1 196] presented recently a more accurate experiments with different ΤΊΟ2 rutile samples where it was proved the presence of tetracoordinate titanium atoms in some of them due to sites located at edges and/or the presence of (001 ) face formed by Ti(4c). The work also suggests that the presence of tetracoordinated titanium sites on rutile Ti0₂ depends on fabrication method like T1O2 anatase.

Furthermore, WO 97/13554 A2 discloses a process for catalytically decomposing stable organic pollutants in a liquid medium by irradiation, in particular for treating clarification sludges contaminated with organic pollutants such as polychlorinated dibenzo-p-dioxines and furans. An aqueous suspension is prepared with products which contain the stable organic pollutants, as well as a TiO₂ catalyst added to the suspension, which have specific conversion properties for converting the electronic radiation into a radiation capable of specifically splitting the chemical bond in question or active substances in the suspension which carry at their surface such radiation-converting catalysts, radical initiators such as hydrogen peroxide, and a lower carboxylic acid such as formic acid and acetic acid. As an example, a 0.1 to 10 cm thick layer of the thus prepared suspension is then stirred and irradiated in an acid medium with an electromagnetic radiation in form of an electron radiation with an energy in a range from 0.5 to 20 MeV.

Other oxidation catalysts, related to Fenton reaction with iron ions and H₂O₂ are known for example from WO 201 1/1 1 1052 A1 and WO 2013/132294 A1 . A cleaning and bleaching agent based on photocatalyticaly activated titanium dioxide, produced by optical irradiation is described in US 2004/171505 A1 . Thus, starting form the prior art of WO 97/13554 A2, it is the object of the present invention to provide alternative, efficient methods of oxidation of organic compounds under heterogeneous T1O2 catalysis, which are independent of any requirement of additional irradiation by an external source. This object is solved by a method for oxidizing a substrate in accordance with claim 1. In particular, the present invention in a first aspect relates to a method for oxidizing a substrate, said method comprising the use of:

- a heterogeneous titanium dioxide catalyst;

- hydrogen peroxide or an organic peroxide; and

- an acid, wherein the pK_a of the acid is about 3 or lower,

wherein the oxidation takes place in the absence of electromagnetic any kind of radiation and/or electric energy; and wherein at least about 0,1 % of the surface of the titanium dioxide catalyst represents low coordination sites, in which the Titanium atoms in said titanium dioxide catalyst are coordinated 3- to 4-fold.

Further aspects of the present inventions lie in uses of the method according to the present invention for different purposes.

For example, the present invention relates to a use for the degradation of organic and/or inorganic compounds in wastewater.

Another use in accordance with the present invention is one for oxidative desulfurization or denitrogenation. Additionally the method of the present invention can be used for bleaching organic and/or inorganic fibers.

A further aspect of the present invention is the use of the described method for improving the whiteness and/or appearance of food.

Another interesting aspect of the invention's method is a use for improving the whiteness and/or appearance of teeth.

Additionally, the method of the present invention is useful for carrying out a selective oxidation of hydrocarbons.

Finally, the method of the present invention is useful as a compounding additive or coating in antibacterial and/or antiseptic materials and/or surfaces. BRIEF DESCRIPTION OF THE INVENTION

The present inventors have surprisingly found a method for oxidizing substrates in the presence of a heterogeneous Ti0₂-catalyst under acidic conditions, particularly by strongly acidic conditions, said oxidation method being useful inter alia for the removal of organic and/or inorganic pollutants from fluids.

In particular, one aspect of the present invention relates to a method for oxidizing a substrate, said method comprising the use of:

- a heterogeneous titanium dioxide catalyst;

- a hydrogen peroxide or an organic peroxide; and

- an acid, wherein the pK_a of the acid is about 3 or lower.

Additionally, the method of oxidation of the present invention does not require necessarily the presence of any kind of radiation or electric energy. Therefore, in accordance with the present invention, the oxidation takes place in the absence of any external irradiation.

Advantageously, the method of oxidation of the present invention allows achieving good oxidation rates even when employing small quantities of hydrogen peroxide or the organic peroxide, or even when employing small amounts of catalyst in the system.

The next statements related to the range of amounts of catalyst in the system will be applied in the present document unless it will be indicated the opposite:

-Since the amount of active sites depends on fabrication method and crystal structure of T1O2, all the amounts of catalyst in the system will be related to Aeroxide Ti0₂ P90 (Evonik Industries AG Silica, May 2015). That entails that the oxidative activity of the catalyst will be related to the amount of active sites of this specific type of Ti0₂ and therefore, it could be increased or decreased if the used catalyst has more or less actives sites than Aeroxide Ti0₂ P90.

-For dispersed particles, the surface exposed could be lowered due to the agglomeration effect, which depends on several factors. Thus, the amounts of catalyst in the system will be consider effectives and therefore, free of agglomeration.

In accordance with this, in a further embodiment of the present invention, the amount of titanium dioxide catalyst, expressed as surface area in the system, may be even in the range from 1 1 to 5000 m²/L. In other embodiments, large amounts of catalyst are needed and then the use of dispersing agents may allow increasing the surface area without agglomeration, it thus being possible to reach amounts of titanium dioxide in the system in the range from 5,000 to 1 ,000,000 m²/L

In accordance with this, in a further embodiment of the present invention, the amount of titanium dioxide catalyst, expressed as surface area in the system, may be even in the range from 1 1 to 5000 m²/L. In other embodiments, large amounts of catalyst are needed, reaching amounts of catalyst in the system in the range from 5,000 to 1 ,000,000 m²/L.

In a preferred embodiment of the present invention, the amount of actives sites per gram, volume or relative surface of catalyst will be at least equal or larger to that present in Aeroxide ΤΊΟ2 P90.

According to a preferred embodiment, the acid with a pK_a of about 3 or lower is a mineral acid (also known as inorganic acid). Said mineral acid is preferably selected from the group consisting of hydrochloric acid, sulphuric acid and nitric acid.

The inventors have further observed that the method of oxidation of the present invention is enhanced under systems which are highly oxygen- saturated. Therefore, in a particular embodiment, the oxidation takes place in a system which is from 80% to 100% oxygen-saturated.

Another aspect of the present invention refers to the use of the oxidation method of the invention for the degradation of organic and/or inorganic compounds in wastewater.

Another aspect of the invention refers to the use of the oxidation method of the invention for oxidative desulfurization or denitrogenation.

Yet another aspect of the invention refers to the use of the oxidation method of the invention for bleaching organic and/or inorganic fibres.

Another aspect of the invention refers to the use of the oxidation method of the invention for improving the whiteness and/or appearance of food.

Yet another aspect of the invention refers to the use of the oxidation method of the invention for selective oxidation of hydrocarbons.

Yet another aspect of the invention refers to the use of the oxidation method of the invention for improving the whiteness and/or appearance of teeth.

Another aspect of the invention refers to the use of the oxidation method of the invention as a compounding additive or coating in antibacterial and/or antiseptic materials and/or surfaces. The above aspects and preferred embodiments thereof are additionally defined hereinafter in the detailed description, as well as in the claims.

BRIEF DESCRIPTION OF THE FIGURES

Figure 1 : Comparative study of dissolved 0₂ influence on kinetics of reaction. Rhodamine B degradation when not supplying O2 to the reaction mixture vs Rhodamine B degradation when supplying 0₂ via pipetting. Conditions: 5% H₂0₂, 10g/L Ti0₂ (aeroxide P90), pH=3 (HCI), 0.025 mM Rhodamine B.

Figure 2: Whiteness of paper according to a blank test compared to paper obtained after applying the method of the invention.

Figure 3: FTIR spectrum of sulfur-containing samples treated with: a) H₂0₂ + HNO₃ + Ti0₂; b) H₂0₂ + Ti0₂; c) no treatment. Figure 4 shows the rate constants for degradation kinetics of 0.005 mM

Rhodamine B in the presence of 15% H₂0₂ solution in the absence of acid for two different Ti0₂ samples with the same exposed area (Sigma-Aldrich rutile;

8,45g and Degussa P25;0,4g) and similar pH 0*2,95).

DETAILED DESCRIPTION OF THE INVENTION

As noted previously, the present invention relates to a method for oxidizing a substrate, said method comprising the reaction of a heterogeneous titanium dioxide catalyst, a hydrogen peroxide or an organic peroxide, and an acid, wherein the pK_a of the acid is about 3 or lower.

In the context of the present invention, the following terms have the meaning detailed below.

As used herein, the term "about" means a slight variation of the value specified, preferably within 10 percent of the value specified. Nevertheless, the term "about" can mean a higher tolerance of variation depending on for instance the experimental technique used. Said variations of a specified value are understood by the skilled person and are within the context of the present invention. Further, to provide a more concise description, some of the quantitative expressions given herein are not qualified with the term "about". It is understood that, whether the term "about" is used explicitly or not, every quantity given herein is meant to refer to the actual given value, and it is also meant to refer to the approximation to such given value that would reasonably be inferred based on the ordinary skill in the art, including equivalents and approximations due to the experimental and/or measurement conditions for such given value.

As used herein, a ΤΊΟ2 catalyst refers to any catalyst, in powder or structured, containing ΤΊΟ2 molecules alone or in combination with other catalytic or non-catalytic particles.

Illustrative non-limiting examples of other catalytic particles include metals, oxides, sulfurs, perovskites, zeolites and salts of elements of group IB, MB, 1MB, IVB, VB, VIB, VIIB and VIIIB of the periodic table.

A Ti0₂ catalyst according to present invention also refers to doped Ti0₂ catalysts. It is contemplated by the present invention that two or more individual metals or metal complexes may be used to dope the Ti0₂ catalyst. Examples of dopants suitable for use as part of the Ti0₂ catalysts include, but are not limited to, metals from groups IVB, VB, VIB, VIIB, VIIIB and IVA of the periodic table, lanthanoids such as Lanthanum (La) and Cerium (Ce), metal oxides of hafnium (Hf), zirconium (Zr), cerium (Ce), titanium (Ti), vanadium (V), tungsten (W), molybdenum (Mo), manganese (Mn), iron (Fe), osmium (Os), rhodium (Rh), ruthenium (Ru), iridium (Ir), palladium (Pd), platinum (Pt), lead (Pb), tin (Sn) or silicon (Si), carbon (C), nonmetals such as phosphorus (P), nitrogen (N), selenium (Se), sulfur (S) or halides, homopolymers or copolymers of defined, block or random composition which comprise microcrystalline cellulose, polyolefins, polysaccharides, polyamides, polyurethanes, siloxanes, polythiophene, polynitrile, polyesters, graphite or graphene.

Methods to dope Ti0₂ catalysts include, but are not limited to, acid treatment, ion-assisted sputtering, ion-implantation, chemical vapor deposition, sol-gel or plasma techniques or a combination thereof.

The Ti0₂ catalyst of the present invention may be used as a dispersed or film catalyst. The Ti0₂ catalyst of the present invention may also be used supported on an inorganic material such as silica gel, alumina, silica-alumina, zeolites, activated carbon, graphene, graphene oxide or combinations of the same. The Ti0₂ catalyst of the present invention may also be supported on polymers such as polysulfone, polyacrylonitrile, polystyrene, polyester terephthalate, polyurethane, polyaniline or combinations of the same. Τί0₂ catalysts with different specific surface areas are available and may be used in the present invention. In a particular embodiment, the Ti0₂ catalyst may have a specific surface area in the range from 10 to 1 ,000 m²/g.

Although all three crystalline mineral forms of Ti0₂, i.e. anatase, rutile and brookite, as well as amorphous TiO_2i or mixtures thereof may be used for the purposes of the present invention, preferably the Ti0₂ is predominantly in the anatase or rutile form cristalline. By predominantly it is meant that at least about 40% of the Ti0₂ particles are in a particular form. According to preferred embodiments, at least about 50%, 60%, 70%, 80% or 90% of the Ti0₂ particles are crystalline. More preferably, over about 99% of the Ti0₂ is crystalline.

Additionally, the crystalline form of Ti0₂ preferably predominantly displays a hydroxylated surface. The term hydroxilated surface refers to the capability of some Ti0₂ surfaces to adsorb H₂0 dissociatively. By predominantly it is meant that at least about 10% of the Ti0₂ surface is hydroxylated. According to preferred embodiments, at least about 50%, 60%, 70%, 80% or 90% of the catalyst surface is hydroxylated. More preferably, over about 99% of the catalyst surface is hydroxylated.

Additionally, the crystalline form of Ti0₂ can display a surface with Lewis- acid sites, i.e. the sites on the catalyst act as Lewis acids. According to preferred embodiments, at least about 10%, 20%, 30% or 40% of the catalyst surface represents Lewis-acid sites. More preferably, over about 99% of the catalyst surface represents Lewis-acid sites.

Additionally, the crystalline form of Ti0₂ can display a surface with low coordination sites. A low coordination site refers to sites on the catalyst, primarily Ti atoms, which exist in a low coordination state and may therefore coordinate further atoms or ligands.

For the purpose of the present invention, the term "low coordination site of a Titanium dioxide catalyst" refers to sites on the catalyst, primarily Ti atoms, which are coordinated with four or less atoms or ligands.

Ti0₂ catalysts displaying different percentages of a surface with low coordination sites or Lewis-acid sites or hydroxylated surface or mixtures thereof are commercially available. The methods for growing Ti0₂ anatase or rutile crystals which predominantly display low coordination sites or Lewis-acid sites or hydroxylated surface or mixtures thereof are known to the person skilled in the art. The Ti0₂ catalyst used in the present invention may also be in the form of nanocrystals, although microcrystals and larger crystals are also contemplated herein.

The quantity of catalyst employed can vary over a wide range but in general it includes a catalytically effective quantity of T1O2, herein expressed as surface area in the system, which gives a suitable and reasonable reaction rate. The Ti0₂ catalyst of the present invention may have a surface area in the system in the range from 1 1 to 1 ,000,000 m²/L, particularly in the range from 100 to 10,000 m²/L, and more particularly in the range from 500 to 5000 m²/L Generally, the use of a small amount of catalyst is desired.

Advantageously, the rate of oxidation of the present invention is greatly influenced by the pH of the reaction medium, such that under acidic, particularly strongly acidic conditions a good level of oxidation may be achieved even when employing small amounts of catalyst or oxidizing agent. The oxidation method of the present invention therefore does not solely rely on increasing concentrations of catalyst and/or oxidizing agent to achieve increased oxidation.

Accordingly, advantageously, in a particular embodiment of the present invention, the T1O2 catalyst may have a surface area in the system in the range from 1 1 to 10,000 m²/L, preferably in the range from 1 1 to 1000 m²/L, or even in the range from 11 to 100 m²/L.

In a particular embodiment of the present invention, the rate of oxidation is increased by reducing the pH of the oxidation with an acid with a pK_a of about 3 or lower without altering the amount of catalyst and peroxide (hydrogen peroxide or organic peroxide).

However, in other cases, the use of large amounts of catalyst may be needed. Then, the use of dispersing agents may allow increasing the surface area without agglomeration of the catalyst particles, Therefore, advantageously, in a particular embodiment of the invention the method of oxidation additionally comprises the use of a dispersing agent and the surface area of titanium dioxide catalyst in the system is in the range from 1 1 to 1 ,000,000 m²/L.

As mentioned above, dispersing agents may additionally be employed in the oxidation of the invention in order to avoid agglomeration of the Ti02 particles and a reduction or standstill in the rate of oxidation upon increasing the amount of catalyst. Exemplary dispersing agents suitable for use in the oxidation of the present invention include, but are not limited to, tetrahydrofuran (THF), sodium hexametaphosphate (SHMP), sodium dodecyl sulfate (SDS), polyacrylic acid or any of its salts, ethylene glycol, polyethylene glycol, polyethylene pyrrolidone, 4,5-dihydroxy-1 ,3-benzenedisulfonic acid disodium salt, sodium citrate, sodium ascorbate and commercial dispersants such as Dolapix CA, Dalais PC21 , Reotan LA, PEI, Dolapix A88, KV9021, Dolapix ET85, Dolapix PC80, Dolapix CE64, Tiron or combinations thereof. The Ti0₂ catalyst may also include activated titanium particles in order to improve the catalytic properties of the catalyst before the addition of the hydrogen peroxide or the organic peroxide. "Activated" as used herein means that at least part of the titanium particles on the surface of the catalyst has undergone the formation of radicals. Non-limiting examples of activated titanium particles include titanium-p-peroxide complexes, titanium-r)-peroxide complexes or titanium-r)²-peroxide complexes. Methods of catalyst activation include, but are not limited to, treatment of the catalyst with ultraviolet light (UV), ultrasounds, microwaves, gamma radiation or liquid phase plasma treatment, cavitation, or combinations thereof.

However, advantageously, in the present invention the catalyst may be activated solely by treating it with H₂0₂ or the organic peroxide, i.e. activation of the catalyst takes place in the absence of any external source of radiation or electric energy for example electromagnetic irradiation, in particular, ultraviolet light (UV), ultrasounds, microwaves, gamma radiation, electron radiation or any other means of catalyst surface activation.

Additionally, the Ti0₂ of the present invention may be reused to minimize costs.

The method of oxidation of the present invention takes place in the presence of H₂0₂ or an organic peroxide, which are the oxidizing agents of the reaction. Illustrative non-limiting examples of organic peroxides are methyl ethyl ketone peroxide, t-butyl peroxide, dicumyl peroxide, dibenzoyl peroxide, di-t- butyl peroxide, lauryl peroxide, t-butyl perbenzoate, hydroperoxides (such as t- butyl hydroperoxide, cumyl hydroperoxide, ethylbenzene hydroperoxide). Use of a combination of more than one peroxide is advantageous in certain circumstances, although generally just one peroxide is used.

The quantity of H₂0₂ or organic peroxide employed can vary over a wide range but in general it includes an effective quantity which gives a suitable and reasonable oxidation rate. However, advantageously, the rate of oxidation of the present invention is greatly influenced by the pH of the reaction medium, such that under acidic, particularly strongly acidic conditions a good level of oxidation may be achieved even when employing small amounts of H₂0₂ or an organic peroxide, as opposed to oxidative systems based on Ti0₂ catalysis which rely on increasing concentrations of catalyst and/or oxidizing agent to achieve increased oxidation. Additionally, high amounts of peroxide may not be desirable due to the explosive nature of peroxides, which is a factor which is taken into account particularly when carrying out oxidations at an industrial level, in addition to the cost of the peroxide. Therefore, the quantity of H₂0₂ or organic peroxide used for the purposes of the present invention can be as low as 0.001 % H₂0₂ or organic peroxide by volume. Preferably, the quantity of H₂0₂ or organic peroxide is between 1 and 50 % Η₂0₂ or organic peroxide by volume.

H₂0₂ or organic peroxide can be dosed to the reaction mixture. Specifically, the dose may be applied via small addition of the H₂0₂ or organic peroxide to solution at fixed intervals, or it may be obtained through continuous feeding of the H₂0₂ or organic peroxide to the solution.

The oxidation of the present invention may work in parallel to or together with additional oxidative systems and therefore may include additional oxidizing agents. Exemplary additional oxidizing agents include, but are not limited to, permanganates, dichromates, hypochlorous acid and its salts, sodium chlorite and chlorine dioxide, chlorate, peroxides, nitric acid and nitrogen tetroxide, nitrobenzene, ferric salts, copper salts, agents for alkaline fusion (e.g. Na₂0₂), arsenic acid, potassium ferricyanide, fuming sulfuric acid (oleum), ozone or combinations thereof.

Acids suitable for use in the oxidation of the present invention include organic or inorganic acids with a pK_a of about 3 or lower. The use of acids with a pK_a higher than 3 would in general require large amounts of acid to attain a desired acidic pH, especially when the pH of the reaction is strongly acidic, which would have several disadvantages: higher costs due to the higher consumption of acid; a higher concentration of the acid, which may lead to a higher probability of side-reactions competing with the oxidation reaction or which may be toxic to living organisms or detrimental for products subjected to the oxidation, not due to acidity but to reactivity of the acid species and in particular of the anion of the acid species. In line with these arguments, the inventors of the present invention have found and shown that the use of acids with a pK_a higher than 3 leads to a lesser extent of oxidation when compared to the level of oxidation attained when acids with a pK_a of about 3 or lower are employed, both oxidations being carried out at the same pH.

The term pK_a as used herein is that generally recognised in the art, i.e. the pK_a of an acid is the negative logarithm of the acid dissociation constant of the acid. The pK_a value of different acids is known to the person skilled in the art. The present patent application refers only to pK_a values of acids as measured in water. Polyprotic species with different pK_a values, wherein at least one of the pK_a values is about 3 or lower, also fall within the scope of the present invention.

Additionally, in the sense of the present invention, the acid may be a Bnzmsted-Lowry acid or a Lewis acid.

Illustrative non-limiting examples of acids suitable for use in the oxidation of the present invention are trifluoromethanesulfonic acid (pK_a -14), perchloric acid (pK_a -10), hydrochloric acid (pK_a -8.0), sulfuric acid (pK_a -3.0), nitric acid, (pK_a -1 .3), trifluoroacetic acid (pK_a -0.25), chromic acid (pK_a -0.1 ), sulfurous acid (pK_a 1 .9) or phosphoric acid (pK_a 2.1 ).

Preferably, the acid is a mineral acid such as perchloric acid, sulfuric acid, hydrochloric acid, nitric acid, or phosphoric acid. More preferably, the acid is sulfuric acid, nitric acid or hydrochloric acid.

The oxidation of the present invention may include one or more acids, which may be independently either oxidizing acids or non-oxidizing acids.

The quantity of acid added to the reaction mixture is generally the amount necessary for achieving the desired reaction pH. Preferably, the reaction pH is between 1 and 6. More preferably, the reaction pH is between 2 and 4. Specific pH values in the present oxidation method are about 2, about 3 or about 4. These preferred values refer to cases in which catalyst leaching is undesired. Catalyst leaching is enhanced at low pH values. Preferably, the quantity of acid may be added to the reaction mixture before the presence of the pollutant.

However, in cases in which catalyst leaching is not an issue, the preferred pH of the reaction will be as low as possible. As shown in Example 1 , oxidation rates in the method of the invention increase with decreasing pH. In a particular embodiment of the present invention, the reaction pH is between about 0.5 and about 3. Preferably the reaction pH is between about 1 .5 and about 2.5 specific preferred pH values are about 2.5, about 2, about 1 .5, about 1 and about 0.5.

The oxidation of the present invention may be carried out in mild conditions of pressure and temperature. In other cases, however, said process may also be carried out at high pressure and temperature conditions. Preferably, the oxidation reaction takes place at a pressure range of from about 50 mbar to about 40 bar. More preferably, the oxidation reaction takes place at a pressure range of from about 1 to about 10 bar. Preferably, the oxidation reaction takes place at a temperature range of from about 0° to about 400°C. More preferably, the oxidation reaction takes place at a temperature range of from about 0° to about 200°C. Even more preferably, the oxidation reaction takes place at a temperature range of from about 15° to about 50°C. Most preferably, the oxidation reaction takes place at room temperature (between about 20°C and about 23.5°C).

The oxidation of the present invention may be applied to fluids, including liquids, gases, plasmas, ionic liquids and, to some extent, plastic solids.

The oxidation of the present invention may be carried out under stirring, preferably under vigorous stirring. According to the Reynolds (Re) number, the fluid may flow in a laminar, transition or turbulent manner.

The oxidation of the present invention can take place in different polar and apolar solvents. Non-limiting exemplary polar solvents suitable for use in the oxidation system include water, acetic acid, acetonitrile or formic acid, carbon disulfide, pyridine, dimethyl sulfoxide (DMSO), n-propanol, ethanol, n- butyl alcohol, propylene glycol, ethylene glycol, triethylene glycol, dimethylformamide (DMF), methanol or any mixture thereof. Exemplary apolar solvents suitable for use in the oxidation system include, but are not limited to, decane, nonane, pentane, cyclopentane, benzene, toluene, 1 ,4-dioxane, chloroform, diethyl ether or any mixture thereof.

The oxidation of the present invention can be carried out in the presence of light, preferably in the presence of UV light, or in partial or complete darkness.

It has been found that high levels of oxygen greatly enhance the rate of oxidation in the method of the present invention. Therefore, the oxidation of the present invention preferably takes place in a system which is from about 80% to about 100% oxygen-saturated.

Substrates that may be oxidized through the present method include, but are not limited to, organic and inorganic pollutants such as dyes, pesticides, pharmaceuticals, herbicides, tire waste, oil and petroleum derivates, mine waste, battery waste, vegetable and animal by-products and other waste with hazardous properties. As regards the chemical structure of compounds that may be oxidized through the present method, these include, but are not limited to, alkanes, alkenes, alkynes, polyunsaturated compounds, alcohols, ketones, aldehydes, esters, acids, epoxides, cyclic compounds, aromatic compounds and heteroatom containing compounds such as compounds containing a halogen, a non-metal, or a transition metal from groups 3 to 12 of the periodic table of elements, or combinations thereof.

Preferably, the substrate to be oxidized through the method of the present invention is an unsaturated compound, partially oxidized compound or a compound with a non-metal element. More preferably, the substrate to be oxidized through the method of the present invention is a nitrogen or sulfur containing compound or an olefin. Exemplary compounds of the preferred substrates include, but are not limited to, amines, sulfides, sulfoxides, thiols and cyclic or short-chain olefins.

The oxidation method of the present invention may therefore be used in synthetic pathways to achieve the oxidation of starting materials or intermediates.

The oxidation method of the present invention may alternatively be used in the separation of at least a reaction product or by-product from a reaction mixture.

The present invention additionally relates to the use of the oxidation method of the invention to achieve an economical, effective and rapid treatment of industrial or urban wastewater contaminated with organic and/or inorganic substances, so as to destroy said substances or reduce the same preferably to a level below that which is considered detrimental to human use. Contaminants found in wastewater are varied and numerous. Exemplary contaminants present in wastewater are pharmaceuticals, pathogens, ammonia, pesticides and endocrine disruptors, all of which may be suitable substrates in the present invention, however the use of the oxidation method of the present invention is not limited to said contaminants.

The present invention further relates to the use of the oxidation method of the invention for oxidative desulfurization or denitrogenation, in particular for recovering sulfur and nitrogen from hydrocarbons present in petroleum and petroleum based products. Exemplary sulfur compounds present in hydrocarbon contaminants include sulfides, disulfides, mercaptans, as well as aromatic molecules such as thiophenes, benzothiophenes, dibenzothiophenes, as well as alkyl derivatives of said compounds. Exemplary, nitrogen compounds present in hydrocarbon contaminants include indoles, carbazoles, anilines, quinolones, acridines as well as alkyl derivatives of said compounds. All of said exemplary compounds may be suitable substrates in the present invention, however the use of the present invention is not limited to said compounds.

The present invention additionally relates to the use of the oxidation method of the invention for bleaching foodstuffs and improving the whiteness thereof. Furthermore, the oxidation method of the invention may be applied to reduce microbial and fungus contamination on food. The present invention also relates to a deodorant composition for sulfides, specifically on food, more specifically on meat. The oxidation method of the invention is further advantageous in that it comprises the use of titanium dioxide, a clear, generally white powder which does not itself negatively affect the whiteness of the foodstuffs and which is biocompatible.

The present invention further relates to the use of the oxidation method of the invention to bleach organic and/or inorganic fibers. The method of the invention is carried out at low pH, thus avoiding the disadvantages and drawbacks of bleaching processes that employ chlorinated compounds. In particular, the oxidation method of the invention can be used to improve wood and non-wood pulp brightness. Illustrative, non-limiting examples of pulps are groundwood pulps, bleached groundwood pulps, thermomechanical pulps, bleached thermomechanical pulps, chemi-thermomechanical pulps, deinked pulps, kraft pulps, bleached kraft pulps, sulfite pulps, and bleached sulfite pulps. The oxidation method of the invention is further advantageous in that it comprises the use of titanium dioxide, a clear, generally white powder which does not itself negatively affect the whiteness of the fiber.

The present invention additionally relates to the use of the oxidation method of the invention for improving the whiteness and/or appearance of teeth. In particular, the method of the present invention is applied to oxidize discoloring substances in food, beverages, tobacco, and salivary fluid that have penetrated the tooth enamel, particularly organic chromogenic substances. The oxidation method of the invention is further advantageous in that it comprises the use of titanium dioxide, a clear, generally white powder does not itself negatively affect the whiteness of the whitened teeth and which is biocompatible.

The present invention further relates to the use of the oxidation method of the invention for selective oxidation of hydrocarbons. The method of the invention provides a high reaction rate in mild and/or eco-friendly conditions, without pore limitations and reducing fouling problem, thus avoiding the disadvantages and drawbacks of other processes that employ titanium silicates or β-zeolite catalysts. In particular, the oxidation method of the invention is further advantageous in that it comprises the use of titanium dioxide, an extensive and easy to produce oxide, with low or no toxicity and reusable.

Having described the present invention in general terms, it will be more easily understood by reference to the following examples which are presented as an illustration and are not intended to limit the present invention. EXAMPLES

Example 1. Degradation of Rhodamine B

Recalcitrant ink Rhodamine B, an organic compound difficult to oxidize by common AOPs (Advanced Oxidative Processes), was chosen as a representative substrate for the oxidation method of the invention. The degradation of said ink is of particular interest as it represents one of the main challenges encountered during the bleaching of recycled paper.

In order to fully demonstrate the potential of the oxidation of the invention, the oxidation of Rhodamine B was carried out in the absence of light. The walls of a beaker (0 = 10 cm) were covered with aluminum foil to prevent any light exposure to the inside. A magnetic stirrer was introduced in a smaller beaker (0 = 6.5 cm), which was then covered on the top with parafilm and a small hole was punched thereon. The smaller beaker was introduced concentrically into the larger one. To immobilize the inner beaker, a foam was placed between the walls of the two vessels. A cover of the same foam (0 = 10 cm, 1 .5 cm thick) was placed on the top of the larger beaker. In the cover, a hole (0 = 0.5 cm) close to the inside wall of the inner beaker facilitated sample collection in the vortex formed during the agitation of the reaction mixture. A second hole situated on the opposite side of the first one was punched in order to facilitate pH measurements.

The catalytic reactor was placed on the stirrer (VMS-C4, VWR) at around 750 rpm. Then, the inner beaker was filled with the help of a funnel with the required amount of TiO₂. Immediately afterwards, the appropriate amount of 9.8 M H2O2 and deionised water, in each case, for a total volume of 20 mL, was introduced. The mixture was stirred for 1 minute, and 20 mL of the required concentration of Rhodamine B were then added. In the cases where an acid was employed, the corresponding amount of acid to achieve a particular pH was introduced in the reaction mixture before the addition of Rhodamine B. After 3 minutes stirring, an aliquot of 1 mL was taken through a plastic Pasteur pipette and was introduced in an Eppendorf tube (1.5 mL). The sample was centrifugated (Mikro 120, Hettich Zentrifugen) at 14000 rpm for 1 minute. The supernatant was centrifugated again under the same conditions and the remaining supernatant was placed in a 1 .5 mL cuvette for analysis in a spectrophotometer (Du 730, Beckman Coulter). The analyzed peaks, the intensity of which correlates to the amount of Rhodamine B present in the mixture, are situated at 554 and 520 nm. Finally, the TiO₂ and the liquid were reintroduced into the inner beaker. The procedure, starting with the 1 mL aliquot extraction, was repeated (at least) every 3 min for a maximum of 2 h. The experiment was repeated 4 times for every imposed condition. Fluctuations in pH throughout the experiments were in no case larger than ±0.1 units.

The time needed to degrade 90% of Rhodamine B and the kinetic constant at order 1 were the parameters used to compare the oxidative capacity of the different oxidation conditions in the method of the invention.

Table 1 shows the time needed to degrade 90% of the sample for a method of oxidation including no acid and for the method of oxidation of the present invention in the presence of different acids. Amounts of acid added were in each case those necessary to achieve a pH of 2.0 throughout the reaction.

Table 1 . Time needed to remove 90% of 0.025 mM Rhodamine B in the presence of 30g/L of Ti0₂ (aeroxide P90) and 5% H_?0₂ solution in the absence of acid and in the presence of different acids at a pH of 2. Example 2. Comparative effects of acids on reaction kinetics

In a further experiment, the effect on reaction kinetics of acids with a ρΚ_ε of 3 or lower was compared to that of acids with a pK_a of above 3 at a given pH.

Table 2. Rate constants for degradation kinetics of 0.025 mM Rhodamine B in the presence of 10g/L of T1O2 (aeroxide P90), 5% H₂0₂ solution and different acids at a pH of 2.

*lt was not possible to reach the desired pH due to side-reactions between H2O2 and acetic acid. The final pH in this case was 2.5.

Higher oxidation rates are achieved at a pH of 2 when employing acids with a pK_a of 3 or lower. Although acids with a pK_a over 3 may also be employed to still achieve good oxidation kinetics, as shown in Table 3 for formic acid (pK_a of 3.7), these acids generally require addition of large amounts thereof in order to achieve low pH values, which leads to unacceptable higher reagent consumption costs, especially at the industrial scale. Additionally, the use of large quantities of acid can lead to undesired side-reactions that compete with the oxidation reaction, as noted above for acetic acid (pK_a 4.7). In other cases, the pK_a of the acid is not strong enough to even attain a desired low pH.

Example 3. Effect of oxygen saturation on reaction kinetics

The inventors have surprisingly found that the amount of oxygen present in the reaction mixture affects the rate of the oxidation of the present invention. Analysed reaction mixture samples according to the procedure described in Example 1 are reintroduced in the reaction mixture by pipetting, which occurs with a concomitant introduction of air into the reaction system. Figure 1 shows the percentage of Rhodamine B degradation after 60 minutes for two differently treated reaction mixtures. The absorbance of Rhodamine B present in the mixture at each time point was employed to determine the percentage of degradation. The first mixture was supplied with oxygen throughout the reaction at regular intervals by extracting samples and reintroducing them into the reaction mixture. The second mixture was not supplied with oxygen throughout the reaction, i.e. only samples of the initial and final mixture were taken. The pH of both reactions was equal during all the kinetics. The degradation percentage for the reaction supplied with oxygen was about 7% greater than that of the reaction not supplied with oxygen.

Example 4. Paper bleaching

The oxidation method of the invention was applied to pulp samples in order to prove the usefulness of said method in the paper bleaching industry.

Pulp samples obtained from the bleaching industry were pre-treated to remove any CaC0₃ present in the samples that could interfere with the oxidation of the pulp.

The oxidation reaction was performed in a plastic vessel (1 L). The pre- treated pulp was added, followed by 162 ml_ H₂0 and 1 g Ti0₂ UV 100 (Sachtleben). The mixture was then stirred for a few minutes with a hydraulic stirrer at 300 rpm until the mixture was homogeneous. Once the mixture was homogeneous, 34 ml_ H₂O₂ 30% (Prolabo) and the amount of HNO₃ needed to attain a final pH of about 3 in dissolution were added. The mixture was stirred for 30 or 60 minutes. The blank test was carried out according to this same procedure, but substituting the H₂O₂ with water.

Once the oxidation reaction reached completion, the mixture was transferred to a fiber disintegrator (Lhomargy Dl 01 ) and diluted with water up to a volume of 0.5 L. The reaction mixture was disintegrated at 3000 rpm. Sheets of paper of a particular grammage (in this case 100 g/m²) were then formed from the disintegrated mixture. Each sheet obtained was dried and the whiteness percentage of the dried sheet was measured employing a Paperlab (Metso) machine. Whitening results are shown in Figure 2. As can be observed, pulp treated with the oxidation method of the present invention leads to sheets of paper of a greater whiteness as compared to sheets of paper obtained from pulp treated according to the blank test.

Example 5. Oxidative desulfurization

The oxidation method of the invention was applied to hydrocarbon samples polluted with sulfur compounds in order to prove the usefulness of said method in the petroleoum industry. A hydrocarbon solution (100 ml_) containing a known amount of sulfur compounds (R₂S0₂ and RS0₂OH; determined by Fourier-transform infrared spectroscopy (FTIR)) was mixed with 4g of Ti0₂ (aeroxide P 90, catalyst amount determined according to the amount of sulfur compounds present in the sample), and the reaction mixture was stirred until homogeneous. 1.78 μΙ_ of a previously prepared solution containing 5 μΙ_ HNO3 65%_w and 9mL H₂0₂ (Prolabo) 30%_w were then added and the oxidation reaction was allowed to proceed for 60 minutes. Samples from the reaction mixture were then placed in two tubes (50 mL) and centrifugated at 9000 rpm for 1 minute. After the operation, the catalyst particles were found agglomerated at the bottom of the tubes and were separated from the hydrocarbon liquid. Finally, the sample was analyzed again by FTIR. The analyzed peaks observed were the following (see Figure 3):

- Asymmetric stretch (around 1303 cm^"1). R2SO2.

- Symmetric stretch (around 1 126 cm^"1). R₂S0₂.

- Symmetric stretch (around 1 153 cm^"1). RS0₂OH.

It was observed that hydrocarbon samples oxidized through the method of the present invention contained a greater amount of oxidized sulfur compounds (Figure 3, a) when compared to samples oxidized in the absence of acid (Figure 3, b). Samples without treatment i.e. not subjected to oxidizing conditions (Figure 3, c) accordingly showed the least amount of oxidized sulfur compounds.

EXAMPLE 6

The present inventors have found that low coordinated titanium atoms present on the Ti0₂ surface are the active sites of the catalyst in accordance with the present invention. In this regard, it is important to underline the following documents which support the previous statement.

Deiana et al. 2013 performed successfully an experiment which prove the importance of the tetracoordinate titanium sites in the decomposition of H₂0₂ under UV light. However, the blank test to check the activity of a-sites with H₂0₂ in dark was not performed.

In this sense, the work of Martra [Martra, G., Lewis acid and base sites at the surface of microcrystalline Ti0₂ anatase: relationships between surface morphology and chemical behaviour. Applied Catalysis A: General, 2000. 200(1 ): p. 275-285] also described the different acidic behavior of P25 and anatase Merck samples related to IR spectra of CO adsorbed at low temperature. The spectrum extracted from P25 underlines the conclusions from Deiana et al. On the other hand, Merck anatase nanoparticles shows a completely different spectrum where it can be affirmed the completely lack of low coordinated sites.

Taking into account what it was mentioned before, the comparison between these samples can be considered analogous to that done in Deiana et al. where P25 was compared with TiO₂ samples with an almost null amount of low coordinated sites.

The catalytic activity of Merck anatase nanoparticle with H₂O₂ in dark at pH<3 was tested by Singh et al. [Singh, O, R. Chaudhary, and K. Gandhi, Preliminary study on optimization of pH, oxidant and catalyst dose for high COD content: solar parabolic trough collector. Iran J Environ Health Sci Eng, 2013. 10(1 ): p. 1 -10], showing a null catalytic effect. On the other hand, P25 has shown the opposite effect at similar conditions [Random, C, S. Wongnawa, and P. Boonsin, Bleaching of methylene blue by hydrated titanium dioxide. ScienceAsia, 2004. 30: p. 149-156]. Therefore, it can be concluded that the tetra-coordination of titanium sites is the primary factor which explains the different behavior of the samples.

On the other hand, it was checked the activity of TiO₂ rutile provided by Sigma-Aldrich, which was classified in the work of Mino et al. as a TiO₂ rutile with Ti(4c) sites, comparing its degradative effects on Rhodamine B with TiO₂ P25. The results show an almost identical behavior in connection with its acidity and catalytic effect remarking the strong connection between Lewis acid sites and catalyst activity.

The samples were analyzed according to the procedure described in Example 1 except for addition of acids and the number of experiments for Sigma-aldrich sample (n=1 ). In order to keep equal conditions, the amount of catalyst was set to maintain the same catalyst surface exposed at 500m²/L.

Figure 4 shows the rate constants for degradation kinetics of 0.005 mM Rhodamine B in the presence of 1 5% H₂O₂ solution in the absence of acid for two different TiO₂ samples with the same exposed area (Sigma-Aldrich rutile; 8,45g and Degussa P25;0,4g

Finally, Bonelli et al. [Bonelli, B., et al., Study of the surface acidity of Ti0₂/Si0₂ catalysts by means of FTIR measurements of CO and NH₃ adsorption. Journal of Catalysis, 2007. 246(2): p. 293-300] estimated the maximum amount of active sites of TS-1 in around 2,2 sites/nm² for a percentatge of titanium in silica matrix around 5%. A higher loading of titanium provokes the hexacoordination of titanium cations and therefore, the inactivation of these sites. Since Ti0₂ has not this limitation in active sites, it could be considered 5% of active as the minimum amount in Ti0₂ to get a real improvement in connection with TS-1 catalyst. However, it must be remarked that the active sites in titanosilicate TS-1 are located in the vicinities of the pores and therefore, the oxidation of some compounds can be affected due to steric hindrance. Besides, the lixiviation in this type of catalyst becomes a pivotal problem since it entails the total inactivation of the active sites. For this reason, the minimum amount of actives sites of Ti0₂ catalyst to get an improvement with respect TS-1 can be lowered to 0,1 % of the surface since due to the characteristics of Ti0₂, its active sites can avoid this problems.

Claims

A method for oxidizing a substrate, said method comprising the use of:

- a heterogeneous titanium dioxide catalyst;

- hydrogen peroxide or an organic peroxide; and

- an acid, wherein the pK_a of the acid is about 3 or lower, characterized in that the oxidation takes place in the absence of any source of radiation or electric energy; and

wherein at least about 0.1 % of the sites on the titanium dioxide surface of the titanium dioxide catalyst represents low coordination sites, in which the Titanium atoms in said titanium dioxide catalyst are coordinated 3- to 4-fold.

A method according to claim 1 , wherein the titanium dioxide catalyst has a surface area in the system in the range from 1 1 to 10.000 m²/L.

A method according to any of claims 1 or 2, wherein the method additionally comprises the use of a dispersing agent and wherein the titanium dioxide catalyst has a surface area in the system in the range from 1 1 to 1 ,000,000 m²/L.

A method according to any of the preceding claims, wherein at least about 10% of the surface of the titanium dioxide catalyst is a hydroxylated surface.

A method according to any of the preceding claims, wherein at least about 10% of the surface of the titanium dioxide catalyst represents Lewis-acid sites.

A method according to any of the preceding claims, wherein the titanium dioxide catalyst has, at least, an equal amount of active sites per volume, weight or relative surface than Aeroxide ΊΠ02 P90 (Evonik Industries AG Silica, May 2015)

A method according to any of the preceding claims, wherein the acid is sulfuric acid, nitric acid or hydrochloric acid.

8. A method according to any of the preceding claims, wherein the oxidation takes place in a system which is from about 80% to about 100% oxygen-saturated.

9. Use of the method according to any one of the preceding claims for the degradation of organic and/or inorganic compounds in wastewater.

10. Use of the method according to any one of claims 1 to 8 for oxidative desulfurization or denitrogenation.

1 1. Use of the method according to any one of claims 1 to 8 for bleaching organic and/or inorganic fibers.

12. Use of the method according to any one of claims 1 to 8 for improving the whiteness and/or appearance of food.

13. Use of the method according to any one of claims 1 to 8 for improving the whiteness and/or appearance of teeth.

14. Use of the method according to any one of claims 1 to 8 for selective oxidation of hydrocarbons.

15. Use of the method according to any one of claims 1 to 8, wherein the oxidative system is used as a compounding additive or coating in antibacterial and/or antiseptic materials and/or surfaces.