Ferrate(VI) enhanced photocatalytic oxidation of pollutants in aqueous TiO2 suspensions.
OBJECTIVE
Photocatalytic oxidation using UV irradiation of TiO(2) has been studied extensively and has many potential industrial applications, including the degradation of recalcitrant contaminants in water and wastewater treatment. A limiting factor in the oxidation process is the recombination of conduction band electrons (e(-)(cb)) with electron holes (h(vb)(+)) on the irradiated TiO(2) surface; thus, in aqueous conditions, the presence of an effective electron scavenger will be beneficial to the efficiency of the oxidation process. Ferrate (FeO(4)(2-)) has received much recent attention as a water treatment chemical since it behaves simultaneously as an oxidant and coagulant. The combination of ferrate [Fe(VI)] with UV/TiO(2) photocatalysis offers an oxidation synergism arising from the Fe(VI) scavenging of e(-)(cb) and the corresponding beneficial formation of Fe(V) from the Fe(VI) reduction. This paper reviews recent studies concerning the photocatalytic oxidation of problematic pollutants with and without ferrate.


METHODS
The paper reviews the published results of laboratory experiments designed to follow the photocatalytic degradation of selected contaminants of environmental significance and the influence of the experimental conditions (e.g. pH, reactant concentrations and dissolved oxygen). The specific compounds are as follows: ammonia, cyanate, formic acid, bisphenol-A, dibutyl- and dimethyl-phthalate and microcystin-LR. The principal focus in these studies has been on the rates of reaction rather than on reaction pathways and products.


RESULTS
The presence of UV/TiO(2) accelerates the chemical reduction of ferrate, and the reduction rate decreases with pH owing to deprotonation of ferrate ion. For all the selected contaminant substances, the photocatalytic oxidation rate was greater in the presence of ferrate, and this was believed to be synergistic rather than additive. The presence of dissolved oxygen in solution reduced the degradation rate of dimethyl phthalate in the ferrate/photocatalysis system. In the study of microcystin-LR, it was evident that an optimal ferrate concentration exists, whereby higher Fe(VI) concentrations above the optimum leads to a reduction in microcystin-LR degradation. In addition, the rate of microcystin-LR degradation was found to be strongly dependent on pH and was greatest at pH 6.


CONCLUSIONS
The initial rate of photocatalytic reduction under different conditions was analysed using a Langmuirian form. Decrease in rates in the presence of dissolved oxygen may be due to competition between oxygen and ferrate as electron scavengers and to non-productive radical species interactions. The reaction between ferrate(VI) and microcystins-LR in the pH range of 6.0-10.0 is most likely controlled by the protonated Fe(VI) species, HFeO(4)(-).


CONCLUSIONS
The photocatalytic oxidation of selected, recalcitrant contaminants was found to be significantly greater in the presence of ferrate, arising from the role of ferrate in inhibiting the h(vb)(+)-e(-)(cb) pair recombination on TiO(2) surfaces and the corresponding generation of highly oxidative Fe(V) species. The performance of the ferrate/photocatalysis system is strongly influenced by the reaction conditions, particularly the pH and dissolved oxygen concentration, arising from the complex nature of the interactions between the catalyst and the solution. Overall, the treatment performance of the Fe(VI)-TiO(2)-UV system is generally superior to alternative chemical oxidation methods.


CONCLUSIONS
The formation of intermediate Fe(V) species in the photocatalytic reduction of ferrate(VI) requires confirmation, and a method involving electron paramagnetic resonance spectroscopy could be applied for this. The reactivity of Fe(V) with the selected contaminants is required in order to better understand the role of ferrate in the Fe(VI)-TiO(2)-UV oxidation system. To increase the practical utility of the system, it is recommended that future studies involving the photocatalytic oxidation of pollutants in the presence of ferrate(VI) should focus on developing modified TiO(2) surfaces that are photocatalytic under visible light conditions.
Sharma
Virender K
VK
Chemistry Department, Florida Institute of Technology, 150 West University Boulevard, Melbourne, FL 32901, USA. vsharma@fit.edu
Graham
Nigel J D
NJ
Li
Xiang-Zhong
XZ
Yuan
Bao-Ling
BL
D000641:Ammonia / Q000032:analysis / Q000737:chemistry; D001559:Benzhydryl Compounds; D002384:Catalysis; D003485:Cyanates / Q000032:analysis / Q000737:chemistry; D052918:Environmental Restoration and Remediation; D005561:Formates / Q000032:analysis / Q000737:chemistry; D007501:Iron / Q000032:analysis / Q000737:chemistry*; D008387:Marine Toxins; D052998:Microcystins / Q000032:analysis / Q000737:chemistry; D010084:Oxidation-Reduction; D010636:Phenols / Q000032:analysis / Q000737:chemistry; D055668:Photochemical Processes; D010795:Phthalic Acids / Q000032:analysis / Q000737:chemistry; D014025:Titanium / Q000032:analysis / Q000737:chemistry* / Q000528:radiation effects; D014874:Water Pollutants, Chemical / Q000032:analysis / Q000737:chemistry*; D000098826:Bisphenol A Compounds
D000641:Ammonia; D001559:Benzhydryl Compounds; D003485:Cyanates; D005561:Formates; D007501:Iron; D008387:Marine Toxins; D052998:Microcystins; D010636:Phenols; D010795:Phthalic Acids; D014025:Titanium; D014874:Water Pollutants, Chemical; C030544:formic acid; C009495:titanium dioxide; C017311:ferrate ion; C057862:cyanoginosin LR; C006780:bisphenol A; D000098826:Bisphenol A Compounds