alexa Removal of Crystal Violet and Hexavalent Chromium using TiO2-Bentonite under Sunlight: Effect of TiO2 Content | Open Access Journals
ISSN: 2157-7048
Journal of Chemical Engineering & Process Technology
Like us on:
Make the best use of Scientific Research and information from our 700+ peer reviewed, Open Access Journals that operates with the help of 50,000+ Editorial Board Members and esteemed reviewers and 1000+ Scientific associations in Medical, Clinical, Pharmaceutical, Engineering, Technology and Management Fields.
Meet Inspiring Speakers and Experts at our 3000+ Global Conferenceseries Events with over 600+ Conferences, 1200+ Symposiums and 1200+ Workshops on
Medical, Pharma, Engineering, Science, Technology and Business

Removal of Crystal Violet and Hexavalent Chromium using TiO2-Bentonite under Sunlight: Effect of TiO2 Content

Ridha Djellabi1*, Mohamed Fouzi Ghorab1, Claudia Letizia Bianchi2, Giuseppina Cerrato3 and Sara Morandi3
1Laboratory of Water Treatment and Valorization of Industrial Wastes, Chemistry Department, Faculty of Sciences, Badji-Mokhtar University, BP12 2300, Annaba, Algeria
2Università degli Studi di Milano, Dip. Chimica and INSTM-UdR Milano, Milano, Italy
3Università degli Studi di Torino, Dipartimento di Chimica and NIS Interdepartmental Centre and Consorzio INSTM-UdR Torino, Italy
*Corresponding Author : Ridha Djellabi
Università degli Studi di Milano
Dip. Chimica and INSTM-UdR Milano
Milano, Italy
Tel: 213774662262
E-mail: [email protected]
Received: February 09, 2016; Accepted: February 25, 2016; Published: February 29, 2016
Citation: Djellabi R, Ghorab MF, Bianchi CL, Cerrato G, Morandi S (2016) Removal of Crystal Violet and Hexavalent Chromium using TiO2-Bentonite under Sunlight: Effect of TiO2 Content. J Chem Eng Process Technol 7:276. doi:10.4172/2157-7048.1000276
Copyright: © 2016 Djellabi R, et al. This is an open-access article distributed under the terms of the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original author and source are credited.

Visit for more related articles at Journal of Chemical Engineering & Process Technology


The main objective of this study was to investigate the correlation between TiO2 content in photoactive bentonite (B-TiO2) and the pathway by which crystal violet (CV) and hexavalent chromium (Cr (VI)) are removed from water under sunlight. B-TiO2 samples were prepared by impregnation with TiCl4 with different weight ratios (g/g) (namely, 5, 10, 20 and 30%). Materials were characterized using different techniques, among which: SEM, FT-IR, XRD, HRTEM, EDX and Zeta potential measurements. Results show that, only the anatase TiO2 polymorph was formed in the bentonite and the porosity of materials decreases with the increase of TiO2 content. Furthermore, zeta potential measurements indicate that, when TiO2 content increases, the negative charge of materials decreases. On the other hand, experimental results show that these materials combine both adsorption and photocatalytic reactions to remove CV molecules from water. As the TiO2 content increases, the adsorption capacity decreases, while the photocatalytic activity is more important. In the case of Cr (VI) species, all samples show a few adsorption because of the repulsion effect between these species and the negative charge of the bentonite. Therefore, under sunlight, the Cr (VI) removal occurred mainly by the photoreduction reaction that is more efficient when the TiO2 content increases.

Bentonite-TiO2; TiO2 content; Water remediation; Photoactivity; Sunlight
Among the challenges that our world is nowadays facing, water resources and their scarceness could be considered as important for the human, particularly with the increase of the world population. In this respects, the remediation of both water and wastewaters has become a global strategy in order to decrease the dependency from natural water resources. Moreover, industrial effluents are the main causes of water pollution by different pollutants, such as heavy metals and dyes.
Several technologies are available for the treatment of wastewaters. Among these, the Advanced Oxidation Processes (AOPs) have been and are still extensively investigated [1]. Among these techniques, photocatalysis is an efficient method, environmentally friendly and low cost point-of-use treatment technology for wastewater purification. It focuses on the production of high oxidizing species which can mineralize organics in water [2]. Furthermore, it can reduce heavy metal species to low or metallic states by electrons coming from the conduction band [3-5]. TiO2 is usually used in photocatalytic remediation for both oxidation and reduction of different pollutant species due to its excellent chemical and optical properties [5,6]. The efficiency rate of the photocatalytical treatment by TiO2 depends on pollutant concentration in the TiO2 vicinity, optical proprieties, adsorptive capacity as well as both the number of electrons and radicals produced. Many researcher groups have developed novel generation of photocatalysts in order to overcome different drawbacks of the commercial ones. One of the most applied strategies to enhance the photoeffeciecy is the immobilization of TiO2 on porous adsorbent materials [7-9]. Accordingly, economic reasons explain why the development of re-usable natural clays as TiO2 supports is attracting increasing interest [10-12]. Among these applied clay minerals, montmorillonite is frequently used. It possesses a layered structure, large external and internal surface area, high cation exchange capacities and it can adsorb organics/cations either on its external surface or within its interlaminar spaces by interaction or substitution [13,14]. In general, the dispersion of TiO2 particles into layered montmorillonite improves the photoactivity performance because such composite structure can stabilize TiO2 particles and maintain most of the surface of TiO2 crystals for access by various species. Forthermore, adsorption capacity of this material can participate to adsorb molecules and by-products.
In our previous work, we investigated the preparation of TiO2- Montmorillonite composite (B-TiO2) by impregnation of a local sodium-bentonite (B-Na) with TiCl4 for the decomposition of different dyes under UV irradiation [15]. Results showed that this material involves both adsorption and photocatalytic action for the removal of dyes from water, while both adsorption effectiveness and photocatalytic degradation were more pronounced for cationic dyes.
In the present work, we studied the effect of TiO2 loading in the TiO2-Montmorillonite composite on the degradation of a cationic dye (crystal violet) and the reduction of hexavalent chromium under natural sunlight. A series of TiO2-Montmorillonite composites have been prepared with different TiO2 content. Photocatalyst materials were characterized using different methods such as SEM, FT-IR, XRD, HR-TEM, EDX and Zeta potential measurements.
Materials and Methods
The montmorillonite used in this study is a natural sodiumexchanged bentonite (Na-B) from the Roussel deposit in Maghnia (Algeria) and was used without any further treatment or purification. Its cation-exchange capacity was determined by the methylene blue method and is 89.30 mmol/100 g. Solutions were prepared using double-distilled water. Crystal violet (Fluka), a cationic dye, was used in this study. Hexavalent chromium solution was prepared from potassium dichromate (Sigma-Aldrich, ≥ 99.0%). Adjustment of the pH solution was achieved with H2SO4 (Sigma-Aldrich) and monitored by a pH meter (HANNA HI 9812-5). Tartaric acid (Sigma-Aldrich, ACS reagent, ≥ 99.5%) was used as a holes scavenger for Cr (VI) reduction.
Synthesis of titania-montmorillonite
Titania-montmorillonite (B-TiO2) samples were prepared by B-Na impregnation with TiCl4 (Aldrich, 99.99%) at different weight ratios (g/g) (5, 10, 20 and 30%). The experimental synthesis procedure was reported in our previous paper [15].
Characterization methods
Fourier transform infrared (FT-IR) spectra of Na-M and TiO2-M (as self-supporting pellets, ~20 mg cm-2) were recorded at room temperature at a 2 cm-1 resolution in the 4000-400 cm-1 spectral range using a PerkinElmer FT-IR System 2000 spectrophotometer, equipped with a Hg-Cd-Te cryo-detector. The self-supporting pellets were posed in a quartz cell equipped with KBr windows: before recording the FTIR spectra, all samples have been activated in vacuo at room temperature (RT) connecting the cell to a vacuum line (residual pressure < 10-4 mbar).
The XRD patterns were recorded on a diffractometer instrument (Philips PW3830/3020 X’Pert diffractometer, PANalytical) using monochromatized CuKα radiation (λ=1.54 Å). The inter-layer d-spacing reflection was calculated using the Bragg equation [16]. The crystallite size of anatase TiO2 was calculated using Scherrer’s formula.
The morphology of samples particles was determined by field emission scanning electron microscopy (FEG LEO 1525, Zeiss Company, Germany) and (High-resolution) Transmission electron microscopy (HR-TEM) images were obtained employing a JEOL JEM 3010UHR (300 kV) microscope (300 kV acceleration, single crystal LaB6 filament) fitted with an Oxford INCA Energy TEM 200 energy dispersive X-ray (EDX) detector. Before inspection, all samples were dry deposited on Cu “holey” carbon grids (200 mesh).
Zeta potential measurements of samples were carried out using a Zetasizer 2000 instrument equipped with a microprocessor at a temperature of 25°C. The zeta meter automatically calculates the electrophoretic mobility of the particles and converts it to the zeta potential using the Smoluchowski equation as follow:
image (1)
Where ζ is zeta potential, EM is electrophoretic mobility at actual temperature, νt is the viscosity of the suspending distilled water, and Dt is dielectric constant.
Photocatalytic tests
The photocatalytic experiments were performed using a static batch reactor, consisting of Pyrex beakers open to air under natural sunlight at sea level (in front of the Chemistry Department without any obstacle) on sunny days (at Annaba University) and were started at 10:00 am for a duration of 4 h. 250 mL Solutions of crystal violet ([CV]: 10-4M, pH: 6.5) and hexavalent chromium ([Cr (VI): 30 ppm, pH: 2.2) were exposed to natural sunlight under a constant stirring. Adsorption experiments were performed under the same conditions without irradiation. During the experiments, samples (4 mL) were collected at selected time intervals. The photocatalyst was removed by filtration (0.45 μm, Whatman). The residual concentration of Cr (VI) species was determined at a wavelength of 540 nm via the 1,5-diphenylcarbazide (DPC) method [17]. Furthermore, the residual concentration of CV was determined at a wavelength of 590 nm. The intensity of sunlight radiation at 365 nm was measured using a VLX-3W radiometer (Vilber Loumart, France) with a cell diameter of 1 cm2: it always was in the 16 to 18 W/m2 range during the experimental period. The extent of water evaporation during the solar photocatalysis experimental was in average of 6.0% in volume after 4 h of irradiation and was considered to be within the experimental errors.
Results and Discussion
Characterization of photocatalysts
SEM: Figure 1 reports SEM images of Na-B, B-TiO2 (10%) and B-TiO2 (30%) samples. Both porosity and integrated flakes-like structure of the B-Na material are evident: see the top images in Figure 1. Porosity of bentonite, including intra-particles, interparticles and inter-aggregates, is a suitable feature for the intercalation of TiO2 particles. Furthermore, pollutants can be accumulated inside pores and onto the surface. However, images of B–TiO2 (10%) and B–TiO2 (30%) show a clear changing of the bentonite morphology, evidencing the appearance of TiO2 spheroids. In the case of B-TiO2 (30%), the high concentration of TiO2 causes the formation of aggregates (Figure 1, section “a” at bottom) which can reduce the porosity of this material. This observation will be confirmed by XRD analysis.
XRD: Figure 2 reports the XRD results obtained for all samples, also compared with those typical of a commercial pure anatase TiO2 (Kronos 1077). TiO2 in this form is well evident in samples B-TiO2 (10%), B-TiO2 (20%) and B-TiO2 (30%). On the contrary, the sample containing 5% of TiO2 exhibits no peaks related to the presence of TiO2: this may be reasonably due to the fact that the amount of TiO2 is under the detection limit of the technique.
The pure bentonite B-Na shows the peculiar peak located at 5.8° and related to the basal spacing reflection of montmorillonite. On the other hand, all the B-TiO2 samples exhibit two components in this region. As already reported in our previous paper [15], the two components are a clear indication that the introduction of TiO2 could bring about a decreasing of the basal spacing of a part of the montmorillonitic material. It is worth of note that the sample with the lowest amount of TiO2 shows the highest relative intensity of the component at higher angles, i.e., the peak arising from the TiO2 insertion in the basal spaces of montmorillonite. As far as the TiO2 content increases, the relative intensity of this component decreases. This result can reasonably suggest that only a small part of TiO2 is introduced in the basal spaces and this amount is inversely proportional to the TiO2 loading in the sample.
Moreover, the basal space related to the peak at the highest angles is about 14 Å and the mean particle size of TiO2, calculated by the Scherrer’s equation on the main peak (101), is quite coherent with the basal space, being in the range 14-20 Å for all the B-TiO2 samples.
FTIR spectra: Figure 3 reports the FTIR spectra of all the samples under investigation. As already reported in our previous work [15], after outgassing at RT, spectra of B-Na and B-TiO2 samples exhibit bands in the 3700-3000 cm-1 range that can be assigned to the stretching vibration modes of all (either structural and/or surface) OH groups interacting by H-bonding. The spectroscopic counterpart of these modes can be observed at ∼1630 cm-1 (bending mode of undissociated H2O molecules). Moreover, in the 2000-1700 cm-1 range a complex envelope of bands is present for all the B-TiO2 materials: it can be assigned to the typical overtones of the SiO2-like matrix. On the other hand, it is worth noting that B-Na exhibits a complex spectral component at ∼ 1490 cm-1: this component, totally absent in the case of all B-TiO2 samples, is ascribable to some modes typical of carbonate anions. The absence of this component can be related to the addition of TiO2, as reasonably in the synthetic step the anions, present in the interlayers of the montmorillonite material, are totally substituted by the anions formed by titanium-containing species. In the calcination step, the presence of the latter species brings about the formation of TiO2 and leads to the retaining of a higher amount of water, as evidenced in B-TiO2 spectra: the envelope assigned to the OH stretching mode(s) and the component located at 1630 cm-1 are larger/more intense in the case of all B-TiO2 samples than in the case of pure B-Na.
HR-TEM-EDX: As far as the general morphology of the particles is concerned, the indications coming from XRD/FTIR for both B-TiO2 (5%) and B-TiO2 (20%) are confirmed: in the case of B-TiO2 (5%) powder the typical features of a interlayered system are evident, whereas almost no trace of the presence of TiO2 particles is observable, even at high magnification (see the inset in the TEM images, Figure 4). Nevertheless, the presence of TiO2 is confirmed by the EDX spectrum, see Figure 5: this apparent contradiction is not unexpected, as the TiO2 particles can be very small (under the detection limit of the TEM technique) or, more likely, they are present in very limited extent due to the very low TiO2 amount. The presence of all the other elements in the EXD spectrum confirms the montmorillonitic nature of the powder.
In the case of the 20% TiO2 montmorillonite powder, the morphological features are totally different (Figure 6): even though large areas ascribable to the native interlayered system are still observable (see the left-hand section of Figure 6), the general morphology is totally upset, if compared to the 5% TiO2-containing system. In fact, a lot of small highly ordered crystalline particles are now present (see both central and right-hand sections). The average sizes of these newly formed particles, characterized by rather sharp edges and being very thin and closely packed, fall in the 5-20 nm range and the detailed inspection of the fringe patterns indicate the presence of the (101) family planes of the anatase TiO2 polymorph (ICDD card no. 21-1272).
A further proof of the upsetting of the interlayered system comes from the EDX spectrum of this sample (Figure 7): the Ti peak (being present in the form of TiO2) is now the prevalent component, whereas the other typical species connected to montmorillonite are present to a limited extent.
Zeta potential: Zeta potential mesurements of all samples, which reflect the electrical potential in the double layer at the interface between a bentonite particle and the surrounding liquid, are reported in Figure 8 and Table 1. The magnitude of this parameter is often used as a measure of the strength of the attractive/repulsive interactions between particles and to have information about the surface property of the particles in suspension. It is worth to note that all photocatalyst samples have negative zeta potentials, which indicate that these materials are negatively charged in water. This behaviour is not unusual for the bentonite. It is known that the permanent negative charge is very high in bentonite accounting for 90-95% of the total charges [18]. This is due to the high degree of isomorphic substitution where the Al (III) element in the octahedral sheet are substituted by either Fe (II) or Mg(II), in addition to some Si(IV) in the tetrahedral layer being substituted by Al(III). These permanent charges located on the basal face account for most of the surface charge density of the bentonite. This explains the strong tendency of smectite (or montmorillonite) particles to adsorb cations in order to balance the high negative charge. As can be seen, zeta potential values decrease in absolute value with increasing the amount of TiO2 in B-TiO2 composites. This result was expected because the screening effects of sheets charges of bentonite with TiO2 particles will make the number of negative charges less important. Furthermore, the decrease of zeta potential in absolute value correlates to the creation of clusters of bridging flocculation at high TiO2 content, which leads to B-TiO2 composites having less mobility in water.
Effect of TiO2 content on the removal of crystal violet and hexavalent chromium
Removal of crystal violet: The results of the decolorization of crystal violet using different B-TiO2 samples with different TiO2 ratios under natural sunlight irradiation compared with dark adsorption are represented in Figure 8 and summarized in Table 2. The experiences of CV decolorization were carried out in pH range around 6.5 based on the results of our previous work [2]. As discussed in our previous paper [15], the morphology of this composite allows to combine both adsorption and photocatalytic reaction to remove dyes from water. In order to evaluate the contribution of adsorption and photocatalysis on the total removal for each photocatalyst, we supposed that the total removed quantity of crystal violet (under irradiation) is equal to the sum of: the adsorbed quantity in dark, the removed quantity by photolysis and the removed quantity by photocatalysis, while the latter may be calculated by subtraction.
Photolysis of CV solution at 10-4 M under sunlight was around 7% after 4 h that corresponds to a CV photolysed quantity of 0.017 × 10-4 moles. Adsorption results show that the adsorption rate of crystal violet and the adsorbed quantity (mol) decrease with the increase of TiO2 amount in the composite where sample of 5% of TiO2 has the highest adsorption values. This could be explained by the decrease of bentonite porosity by increasing TiO2 particles in the interlayers. According to SEM results, the surface of montmorillonite is less porous when the amount of TiO2 is high (at 30%). Furthermore, XRD analysis demonstrates that the intensity of basal spacing decreases with increasing on TiO2 content. Hence, adsorptive sites for crystal violet hosting decrease at high TiO2 content. On the other hand, zeta potential changing to less negative with TiO2 increasing has an important role in the adsorption of crystal violet, which is a cationic dye, where the electrostatic attractions between photocatalyst surface and dye molecules decrease.
Results of crystal violet removal under sunlight by different photocatalysts demonstrate the participation of the photocatalytic action to degrade crystal violet molecules. We used the term “removal” because it involves adsorption, photocatalysis and photolysis reactions. The rate of total removal show that samples of B-TiO2 (10%) and B-TiO2 (20%) exhibit the highest values. However, the removed amount of CV per mol by photocatalysis action increases with the increase of TiO2 content. It is worth to mention that, in the case of B-TiO2 (10%), the removal process under sunlight is very fast in the first few minutes (62.3% at 5 minutes). This is due to a good suitability between photocatalyst properties including high porosity, negative surface charge and TiO2 particle distribution leading to a fast removal behavior as a synergistic effect of direct adsorption and photocatalytic degradation. The same manner for B-TiO2 (20%) during the first minutes, nevertheless, the process is less faster with the time.
If we compare the behavior of B-TiO2 (5%) and B-TiO2 (30%), we can conclude that the processes of adsorption and photocatalysis are inversed. ∼91% as a total removed rate by B-TiO2 (5%) corresponds to ∼62% by adsorption, ∼7% by direct photolysis and only ∼22% by photocatalysis action. The scarce performance of this sample is most likely due to the low TiO2 content. However, ∼95% as a total removed rate by B-TiO2 (30%) corresponds to ∼41% by adsorption, ∼7% by direct photolysis and ∼47% by photocatalysis action. In this case, photocatalysis reaction is predominant to remove CV molecules. Furthermore, for B-TiO2 (30%) we note that the removal process at the beginning (after ∼30 minutes) is too slow if compared to the other samples, because the attraction and the adsorption of molecules onto its surface take place with a very slow speed, reflecting its properties.
At the B-TiO2 surface, two mechanisms can alternatively take place (i): CV molecules directly access to bentonite sheets following by simple adsorption or further degradation by hydroxyls produced by TiO2. During the degradation reaction, the adsorption plays a determinate role as a first step for accruing the photocatalytic action as the adsorbed molecules have an intrinsically higher priority to be reacted with hydroxyl radicals than molecules in the solution. This removal process is very fast because the attraction/adsorption between cationic dye molecules and negative bentonite is very quick. (ii): CV molecules directly adsorb/depose onto the TiO2 particles to induce the photocatalytic degradation. This mechanism is observed when the material surface is covered by TiO2. As the attraction between crystal violet molecules and TiO2 is less important than that with bentonite, in this case the removal process may be slower than the first mechanism.
However, both mentioned mechanisms can take place at the same time: therefore, for small TiO2 content (10%), mechanism (i) is more pronounced, whereas for high TiO2 content (30%), mechanism (ii) may be the predominant pathway.
Removal of hexavalent chromium: The reduction of Cr (VI) was studied in acidic medium (at pH: 2.2) based on the results of our previous work [9]. This is necessary in order to ensure a high difference between the energy level of the conduction band (ECB) of TiO2 and the redox potential for Cr (VI) species (E0 Cr (VI)/Cr (III)). Tartaric acid was used as whole scavenger with a concentration of 40 ppm. Its principal role is the separation of pairs (electron/hole) by scavenging the photogenerated holes, thus (i) decreasing the chance of charges (electron/hole) recombination and (ii) setting free more electrons in the conduction band available to reduce Cr (VI) ions. Furthermore, it reacts with produced •OH which possesses a high oxidizing potential and therefore limits the oxidation of the produced Cr (III) species to Cr (VI) species. Experimental results of dark adsorption and photoreduction in the presence of tartaric acid under sunlight are reported in Figure 9.
Direct photolysis of Cr (VI) species in the presence of tartaric acid was negligible (around 1.3% after 4 h). In addition, Cr (VI) adsorption rates were few and similar for all B-TiO2 photocatalysts at ∼ 12%, because the repulsive effects between negative charge of Cr (VI) species and the negative charge of bentonite. Even if the increasing of the TiO2 content brings about changes in both zeta potential and porosity of the materials, it does not affect the adsorption of Cr (VI) anionic species. However, it is worth to mention that the positive edges charges accounting from 5 to 10% of the total charges of bentonite can participate to bond Cr (VI) species. Besides, tartaric acid molecules may chelate Cr (VI) leads to fix into the bentonite surface.
On the other hand, under sunlight, the efficiency of Cr (VI) removal is more pronounced with the increase of TiO2 content. Sample of B-TiO2 (30%) ensures a total removal of Cr (VI) at 30 ppm after 3 h, while both B-TiO2 (10%) and B-TiO2 (20%) samples achieved a total removal after 4 h. Surprisingly, the B-TiO2 (5%) sample ensures a removal rate of ∼ 80%. This result was not expected because of the very small TiO2 content. However, this low TiO2 content might lead to form TiO2 particles of very small size possessing such a good distribution on the bentonite surface, thus leading to a relatively high photocatalytic activity.
From Table 3, it can be seen that the photocatalysis action is the main reaction for reducing Cr (VI) species, while the participation of adsorption and photolysis is almost negligible.
As Cr (VI) adsorb very slight onto the bentonite surface, the removal of Cr(VI) species from the solution occurred mainly by a reduction reaction through two principal steps: (i) negatively charged species (Cr2O72-, HCrO4-) are reduced to positive species (Cr (III)) by electrons coming from the conduction band of TiO2 particles deposited on the bentonite material; (ii) the second important step caused by the montmorillonite support is the transfer of Cr (III) cations from the TiO2 particles to the negative inter-layer pores where binding strength can take place between Cr (III) and the negative charge of montmorillonite sheets. This positive effect avoids the penetration of Cr (III) species in the solution and ensures a continuous contact of Cr (VI) species with photocatalytic TiO2 sites.
The present work shows the effect of TiO2 content in photoactive bentonite-TiO2 on the removal of crystal violet and hexavalent chromium from water under natural solar light. In general, TiO2 content affects both the physico-chemical properties and the photocatalytic activity of synthesized photocatalysts. On one hand, on increasing the TiO2 content the CV adsorption rate decreases: this is due to the decrease of both porosity and negative charges present at the surface. On the other hand, Cr (VI) species adsorb slightly onto all B-TiO2 samples, because the high negative charge of bentonite leads to a repulsive effect with Cr (VI) species. However, under sunlight, the amount of CV molecules degraded by photocatalysis action increases as a function of the TiO2 content. Being the total removal of CV the sum of adsorption, photocatalysis and photolysis, B-TiO2 (10%) exhibits the highest rate of removal because of a good compromise between adsorption capacity and photo-catalytic activity. Furthermore, the removal of Cr (VI) occurred mainly by a photoreduction reaction via electrons generated from TiO2 under sunlight. The process of Cr (VI) reduction is more efficient and faster with TiO2 increasing amounts.
The authors acknowledge the financial support of the Ministry of Higher Education (Algeria). The authors would like to thank Prof G. Cerrato and and Dr. S. Morandi, Università degli Studi di Milano (Torino), extending their characterization facilities and for useful discussions.

Tables and Figures at a glance

Table icon Table icon Table icon
Table 1 Table 2 Table 3


Figures at a glance

Figure Figure Figure Figure Figure
Figure 1 Figure 2 Figure 3 Figure 4 Figure 5
Figure Figure Figure Figure
Figure 6 Figure 7 Figure 8 Figure 9
Select your language of interest to view the total content in your interested language
Post your comment

Share This Article

Recommended Conferences

Article Usage

  • Total views: 7911
  • [From(publication date):
    February-2016 - Jun 26, 2017]
  • Breakdown by view type
  • HTML page views : 7837
  • PDF downloads :74

Post your comment

captcha   Reload  Can't read the image? click here to refresh

Peer Reviewed Journals
Make the best use of Scientific Research and information from our 700 + peer reviewed, Open Access Journals
International Conferences 2017-18
Meet Inspiring Speakers and Experts at our 3000+ Global Annual Meetings

Contact Us

© 2008-2017 OMICS International - Open Access Publisher. Best viewed in Mozilla Firefox | Google Chrome | Above IE 7.0 version