Appl. Sci. 2012, 2(1), 166-174; doi:10.3390/app2010166

Article
Reduction and Immobilization of Potassium Permanganate on Iron Oxide Catalyst by Fluidized-Bed Crystallization Technology
Guang-Xia Li 1, Yao-Hui Huaug 2,3,*, Teng-Chien Chen 2, Yu-Jen Shih 2 and Hui Zhang 1
1
Department of Environmental Engineering, Wuhan University, P.O. Box C319 Luoyu Road 129#, Wuhan 430079, China; Email: liguangxiamanman@gmail.com (G.-X.L.); eeng@whu.edu.cn (H.Z.)
2
Department of Chemical Engineering, National Cheng Kung University, Tainan 701, Taiwan; Email: joily@ceg.com.tw (T.-C.C.); mcdyessjin@gmail.com (Y.-J.S.)
3
Sustainable Environment Research Center, National Cheng Kung University, Tainan 701, Taiwan
*
Author to whom correspondence should be addressed; Email: yhhuang@mail.ncku.edu.tw; Tel.: +886-6-275-7575x626-36; Fax: +886-6-234-4496.
Received: 9 February 2012; in revised form: 21 February 2012 / Accepted: 23 February 2012 /
Published: 1 March 2012

Abstract

: A manganese immobilization technology in a fluidized-bed reactor (FBR) was developed by using a waste iron oxide (i.e., BT-3) as catalyst which is a by-product from the fluidized-bed Fenton reaction (FBR-Fenton). It was found that BT-3 could easily reduce potassium permanganate (KMnO4) to MnO2. Furthermore, MnO2 could accumulate on the surface of BT-3 catalyst to form a new Fe-Mn oxide. Laboratory experiments were carried out to investigate the KMnO4-reduction mechanism, including the effect of KMnO4 concentration, BT-3 dosage, and operational solution pH. The results showed that the pH solution was a significant factor in the reduction of KMnO4. At the optimum level, pHf 6, KMnO4 was virtually reduced in 10 min. A pseudo-first order reaction was employed to describe the reduction rate of KMnO4.
Keywords:
Fluidized-Bed Reactor (FBR); iron oxide; potassium permanganate

1. Introduction

Recently, numerous researches have focused on adsorptive arsenic removal, in which iron oxide was considered to be an appropriate adsorbent due to its high affinity [1,2,3,4,5,6,7]. However, the As(III) adsorption is less effective than the As(V) adsorption by adsorbents in natural water. Arsenite [As(III)] is much more toxic, soluble and mobile than arsenate [As(V)]. Manganese oxides have been extensively investigated as oxidizing agents for arsenite; the reaction is written as follows [8,9,10]:

MnO2 + H3AsO3 +2H+ = Mn2+ + H3AsO4 + H2O

Accordingly, a novel binary oxide concept in which the Mn-O catalyzed the As(III) pre-oxidation to As(V) and the Fe-O functioned as adsorbent, was therefore proposed [11,12]. To our knowledge, the Mn-Fe binary oxide materials was easily prepared by the co-precipitation methods, where the Mn reduction by ferrous is dependent on the solution pH [12,13]:

3Fe2+ + MnO4 + 4OH + 3H2O → 3Fe (OH) 3(s) + MnO2(s) + H+

However, the powder product of micrometers in size was difficul for solid-liquid separation. Based on the perspective of Mn-Fe binary oxide for arsenic removal, this study applied a millimeter scale iron oxide (BT-3) as support and aims at the synthesis of manganese oxides on its surface through the redox of potassium permanganate + in a fluidized bed reactor (FBR). The FBR technology could immobilize potassium permanganate onto BT-3, which was a waste iron oxide from real fluidized bed-Fenton (FBR-Fenton) instruments and was mainly composed of poorly crystallized goethite [14].

Therefore, the employment of BT-3 as the support had the advantages of being cost-efficient and facilitated easier separation and disposal during the synthetic process of binary oxide, and during the application for arsenic removal. Our previous studies have explored the ability of BT waste iron oxide as an excellent adsorbent for F, PO43−, Cu2+, and Pb2+ removal because of its high surface area and porosity nature [14,15,16]. In this study, we attempted to investigate the feasibility of Mn immobilization onto BT-3 without ferrous addition, and then to develop a novel Mn-Fe binary oxide using fluidized-bed crystallization technology. The characterization of BT-3 was examined first. Then, the Mn removal efficiency in solution was detected as a function of reaction time. Furthermore, the effect of KMnO4 concentration, BT-3 dosage, and initial solution pHi was studied through bench scale studies. The optimized parameters were also proposed. Finally, a possible mechanism to synthesize the novel Mn-Fe was rationally proposed via the kinetic study of Mn removal.

2. Material and Methods

The experimental set-up was composed of a 500 mL FBR and a pump which are shown in Figure 1. 40 g (or 100 g) of the fluidized media (BT-3) was placed into the reactor. The dimensions of the reactor were 480 cm3 at high 80 cm. The input flow rate was 60 mL/min and the reflux flow rate was 150 mL/min. The concentration of the potassium permanganate was around 20 mg/L to 70 mg/L. The potassium permanganate (KMnO4) in the aqueous solution was fresh prepared from KMnO4 (Merck), and the solution pHf was adjusted using NaOH and HClO4. At the selected time intervals, the samples were withdrawn from the top of the FBR by syringe. Each sample was filtrated immediately with a 0.45 mm membrane and measured the concentration of KMnO4 with a UV–vis detector. The UV-vis detector was scanning from 200 to 800 nm. The total iron ([Fe]) and manganese ([Mn]) content in samples without filtration were dissolved in concentrated HCl and then were measured with an atomic absorption spectrophotometer. The immobilizations of potassium permanganate defined as ([KMnO4]i − [KMnO4]a)/ [KMnO4]i indicated that the extent of Mn immobilized onto support media rather than through the formation of a precipitate in solution. Where i is the initial concentration, and a is the KMnO4 concentration after adsorption.

Applsci 02 00166 g001 200
Figure 1. Fluidized bed reactor.

Click here to enlarge figure

Figure 1. Fluidized bed reactor.
Applsci 02 00166 g001 1024

The physic-chemical characteristics of the BT-3 were examined using standard procedures. The morphology of the BT-3 was determined using a JEOL JSM-6700F HR-FESEM. An XRD powder diffraction measurement of BT-3 was performed on a powder diffractometer (Rigaku RX III) using Cu Kα radiation. The accelerating voltage and current were 40 kV and 30 mA. Brunauer-Emmett-Teller (BET) surface area and porosity of the adsorbents were obtained from the isotherms. The surface area of the adsorbents was calculated from the BET equation.

3. Results and Discussion

3.1. Characterization of BT-3

The properties of BT-3 are listed in Table 1. The average particle size is about 0.5–1 mm. Furthermore, the bulk density and true density are 1.56 and 2.38 g cm−1, respectively, which indicates that it is easy to separate from aqueous solutions. The BET specific surface area and pore volume of BT-3 are 174 m2/g-solid and 0.14 m2/g-solid, respectively, which reveals the high surface area of BT-3 adsorbent. Figure 2 displays four different magnifications of the morphology of BT-3. An oval shape with irregular surface morphology reveals its high surface area. Figure 3 shows the XRD patterns of BT-3. According to the diffraction files of the Joint Committee on Powder Diffraction Standards (JCPDS), the main diffraction peaks of BT-3 adsorbent at 2θ = 21.5°, 36.7°and 53.3° adsorbent was identified as the α-FeOOH phase.

Table Table 1. Physical properties of BT-3.

Click here to display table

Table 1. Physical properties of BT-3.
PropertiesBT-3
ColorBlack
MaterialIron oxide
Bulk density (g·cm−1)1.56
True density (g·cm−1)2.38
Total iron content (g·Kg−1)649
Specific surface area (BET) (m2/g-solid)174
Pore vol. (cm3/g)0.14
Average grain size (mm)0.5–1
Applsci 02 00166 g002 200
Figure 2. SEM-EDS images of (a) BT-3,(b) BT-3 covered by MnO2.

Click here to enlarge figure

Figure 2. SEM-EDS images of (a) BT-3,(b) BT-3 covered by MnO2.
Applsci 02 00166 g002 1024
Applsci 02 00166 g003 200
Figure 3. X-ray diffraction pattern of the (a) standard of αFeOOH (b) BT-3 adsorbent.

Click here to enlarge figure

Figure 3. X-ray diffraction pattern of the (a) standard of αFeOOH (b) BT-3 adsorbent.
Applsci 02 00166 g003 1024

3.2. Effect of KMnO4 Concentration

Figure 4 shows the effect of initial concentration of KMnO4 on its immobilization efficiency onto BT-3 (BT-3 = 100 g, pHi = 2.5), in which the reduction rate of KMnO4 decreased with increasing KMnO4 concentration from 20 to 70 mg/L. The time for complete decomposition of 20 mg/L KMnO4 is 1.5 h, and that with 70 mg/L KMnO4 is even longer than 6 h.

Applsci 02 00166 g004 200
Figure 4. The effect of initial concentration of KMnO4 on the immobilized efficiency onto BT-3.

Click here to enlarge figure

Figure 4. The effect of initial concentration of KMnO4 on the immobilized efficiency onto BT-3.
Applsci 02 00166 g004 1024

3.3. Effect of BT-3 Dosage

As shown in Figure 5, when the pHi, and the initial concentration of KMnO4 was 2.5 and 35 mg/L, the reduction rate increased with increasing the dose of adsorbent. The maximum removal rate was exhibited at a dosage of 100 g adsorbent when the initial concentration of KMnO4 was 35 mg/L. Reusing BT3 or higher reusing BT-3 dosage may be attributed to the limitation of catalytic activity sites the BT-3 could provide, which results in a decrease in reduction efficiency of KMnO4.

Applsci 02 00166 g005 200
Figure 5. Effect of dosage of BT-3 on the immobilization of KMnO4 in binary system.

Click here to enlarge figure

Figure 5. Effect of dosage of BT-3 on the immobilization of KMnO4 in binary system.
Applsci 02 00166 g005 1024

3.4. Effect of the Operational pH Level

The solution pH was a significant factor on the reduction of KMnO4. In this study, we applied four different operation pH levels which used the NaOH to adjust the operational pH level. Figure 6 indicated the effect of different PH level on the reduction and immobilization of KMNO4 in which the concentration of KMnO4 was 20 mg/L and the BT-3 dosage was 100 g.

Applsci 02 00166 g006 200
Figure 6. Effect of pHf on the reduction and immobilization of KMnO4.

Click here to enlarge figure

Figure 6. Effect of pHf on the reduction and immobilization of KMnO4.
Applsci 02 00166 g006 1024

The optimum pHi was about 6, at which KMnO4 could be virtually reduced to MnO2 in 10 min. Chen [17] discussed the reduction of KMnO4 in H2SO4 solution at temperature of 70–95 °C for 30 min, the chemical reaction between potassium permanganate and sulfuric acid can be formulated as:

MnO4− + 8H+ + 5e== Mn2+ + 4H2O

2MnO4− + 3Mn2+ + 2H2O == 5MnO2 + 4H+

It showed low pH of the reaction system would prohibit the formation of MnO2. Therefore, a neutral or weak acid system medium is preferable for such reaction.

3.5. The Possible Mechanism of KMnO4 Immobilization on BT-3

The probable reaction of KMnO4 reduction in weak acidic condition could be written as follows:

MnO4− + 4H++ 3e == MnO2+ 2H2O (1)

The MnO2 formed from the reduction of KMnO4 could be adsorbed on the BT-3. However, contrary to the reduction of KMnO4 with homogeneous catalytic oxidation, as shown in Equation (3), this study aimed to investigate the reduction of KMnO4 with heterogeneous catalysis by iron oxide, which is seldom discussed in the literature.

According to Ma and Lin [18,19], the reduction of KMnO4 could proceed in two possible stages. In the first stage, the BT-3 surface was positively charged via hydrolysis in acidic condition. MnO4 ions were absorbed, thereby producing a heterogeneous MnO4 film on the BT-3.

≡FeOOH + H+ Applsci 02 00166 i001 ≡FeOOH2+ (2)

≡FeOOH2+ + MnO4 Applsci 02 00166 i001 ≡FeOOH2-MnO4 (3)

Moreover, Chou et al. [20], proposed that iron is generated as Fe2+ by reductive dissolution of FeOOH. Therefore another possible mechanism is proposed for the acid condition.

FeOOH(s) + 3H+ + e Applsci 02 00166 i001Fe2++ 2H2O (4)

3Fe2+ + MnO4− + 4OH + 3H2O Applsci 02 00166 i001 3Fe (OH) 3(s) + MnO2(s) + H+ (5)

3.6. Kinetics of KMnO4 Decomposition

The results concerning the immobilization of KMnO4 at pHi = 2.5 in the presence of 100 g BT-3 particles are presented in Figure 7.

Applsci 02 00166 g007 200
Figure 7. First-order fit of KMnO4 decomposition for different concentrations of KMnO4.

Click here to enlarge figure

Figure 7. First-order fit of KMnO4 decomposition for different concentrations of KMnO4.
Applsci 02 00166 g007 1024

The logarithmic KMnO4 concentration is plotted as a function of the reaction time for different initial concentrations of KMnO4, ranging from 20 to 70 mg/L. The well fitted data to a straight line indicates that the decomposition of KMnO4 in the presence of BT-3 follows a first-order kinetic rate law:

−d [KMnO4]/dt = k [KMnO4]

thus ln[KMnO4]/[KMnO4]0 = −kt

where k is the observed first-order rate constant and [KMnO4] and [KMnO4]0 are the concentrations of KMnO4 in the solution at any time t and time zero, respectively. The lines were treated by linear regression, which produced correlation coefficients >0.982. Furthermore, the k is 2.34, 1.04 and 0.45 when the concentration of KMnO4 is 20, 35 and 70 mg/L, respectively.

Obviously, initially the first-order date did not intersect with the origin; this is probably due to the trace amounts of Fe2+ on the surface of BT-3 which could accelerate the reduction in the short term. To prove this, Fe2+ with a molar ratio Fe:Mn = 2:1, was added in the same experiment but without BT-3 (date not shown), the KMnO4 was reduced in 10 min, then almost maintained at the same level.

Conclusion

A new and novel Mn-Fe binary oxide was synthesized using a fluidized bed reactor. In the binary system, through in situ monitoring of the KMnO4 concentration, the decomposition of KMnO4 in the presence of BT-3 follows a first-order kinetic rate law. Low KMnO4 concentration is advantageous in increasing the reduction rate, which decreased from 2.34 to 0.45 when the KMnO4 concentration was 20 and 70 mg/L, respectively. High BT-3 dosage could also be favorable to the reduction rate. Furthermore, the optimum pHi condition for the immobilization of KMnO4 is 6, and KMnO4 could be virtually reduced in 10 min. Finally, a possible mechanism of KMnO4 immobilization, where the BT-3 was found to act as the substrate and reduction agent, was proposed.

References

  1. Banerjee, K.; Amy, G.L.; Prevost, M.; Nour, S.; Jekel, M.; Gallagher, P.M.; Blumenschein, C.D. Kinetic and thermodynamic aspects of adsorption of arsenic onto granular ferric hydroxide (GFH). Water Res. 2008, 42, 3371–3378, doi:10.1016/j.watres.2008.04.019.
  2. Chen, R.; Zhi, C.; Yang, H.; Bando, Y.; Zhang, Z.; Sugiur, N.; Golberg, D. Arsenic (V) adsorption on Fe3O4 nanoparticle-coated boron nitride nanotubes. J. Colloid Interface Sci. 2011, 359, 261–268, doi:10.1016/j.jcis.2011.02.071.
  3. Simeonidis, K.; Gkinis, T.; Tresintsi, S.; Martinez-Boubeta, C.; Vourlias, G.; Tsiaoussis, I.; Stavropoulos, G.; Mitrakas, M.; Angelakeris, M. Magnetic separation of hematite-coated Fe3O4 particles used as arsenic adsorbents. Chem. Eng. J. 2011, 168, 1008–1015, doi:10.1016/j.cej.2011.01.074.
  4. Tang, Y.; Wang, J.; Gao, N. Characteristics and model studies for fluoride and arsenic adsorption on goethite. J. Environ. Sci. 2010, 22, 1689–1694, doi:10.1016/S1001-0742(09)60307-7.
  5. Yang, W.; Kan, A.T.; Chen, W.; Tomson, M.B. pH-dependent effect of zinc on arsenic adsorption to magnetite nanoparticles. Water Res. 2010, 44, 5693–5701, doi:10.1016/j.watres.2010.06.023.
  6. Youngran, J.; Fan, M.; van Leeuwen, J.; Belczyk, J.F. Effect of competing solutes on arsenic(V) adsorption using iron and aluminum oxides. J. Environ. Sci. 2007, 19, 910–919, doi:10.1016/S1001-0742(07)60151-X.
  7. Zhang, J.S.; Stanforth, R.S.; Pehkonen, S.O. Effect of replacing a hydroxyl group with a methyl group on arsenic (V) species adsorption on goethite ([alpha]-FeOOH). J. Colloid Interface Sci. 2007, 306, 16–21, doi:10.1016/j.jcis.2006.10.004.
  8. Manning, B.A.; Fendorf, S.E.; Bostick, B.; Suarez, D.L. Arsenic(III) oxidation and Arsenic(V) adsorption reactions on synthetic birnessite. Environ. Sci. Technol. 2002, 36, 976–981, doi:10.1021/es0110170.
  9. Nesbitt, H.W.; Canning, G.W.; Bancroft, G.M. XPS study of reductive dissolution of 7Å-birnessite by H3AsO3, with constraints on reaction mechanism. Geochim. Gosmochim. Acta 1998, 62, 2097–2110, doi:10.1016/S0016-7037(98)00146-X.
  10. Scott, M.J.; Morgan, J.J. Reactions at oxide surfaces. 1. Oxidation of As(III) by synthetic birnessite. Environ. Sci. Technol. 1995, 29, 1898–1905, doi:10.1021/es00008a006.
  11. Zhang, G.S.; Qu, J.H.; Liu, H.J.; Liu, R.P.; Li, G.T. Removal mechanism of As(III) by a novel Fe-Mn binary oxide adsorbent: Oxidation and sorption. Environ. Sci. Technol. 2007, 41, 4613–4619, doi:10.1021/es063010u.
  12. Zhang, G.; Qu, J.; Liu, H.; Liu, R.; Wu, R. Preparation and evaluation of a novel Fe-Mn binary oxide adsorbent for effective arsenite removal. Water Res. 2007, 41, 1921–1928, doi:10.1016/j.watres.2007.02.009.
  13. Wu, K.; Wang, H.; Liu, R.; Zhao, X.; Liu, H.; Qu, J. Arsenic removal from a high-arsenic wastewater using in situ formed Fe-Mn binary oxide combined with coagulation by poly-aluminum chloride. J. Hazard. Mater. 2011, 185, 990–995, doi:10.1016/j.jhazmat.2010.10.003.
  14. Huang, Y.H.; Shih, Y.J.; Chang, C.C. Adsorption of fluoride by waste iron oxide: The effects of solution pH, major coexisting anions, and adsorbent calcination temperature. J. Hazard. Mater. 2011, 186, 1355–1359, doi:10.1016/j.jhazmat.2010.12.025.
  15. Huang, Y.H.; Hsueh, C.L.; Cheng, H.P.; Su, L.C.; Chen, C.Y. Thermodynamics and kinetics of adsorption of Cu(II) onto waste iron oxide. J. Hazard. Mater. 2007, 144, 406–411, doi:10.1016/j.jhazmat.2006.10.061.
  16. Huang, Y.H.; Hsueh, C.L.; Huang, C.P.; Su, L.C.; Chen, C.Y. Adsorption thermodynamic and kinetic studies of Pb(II) removal from water onto a versatile Al2O3-supported iron oxide. Sep. Purif. Technol. 2007, 55, 23–29, doi:10.1016/j.seppur.2006.10.023.
  17. Chen, Y.; Liu, C.; Li, F.; Cheng, H.M. Preparation of single-crystal [alpha]-MnO2 nanorods and nanoneedles from aqueous solution. J. Alloy. Compd. 2005, 397, 282–285, doi:10.1016/j.jallcom.2004.12.049.
  18. Ma, S.B.; Ahn, K.Y.; Lee, E.S.; Oh, K.H.; Kim, K.B. Synthesis and characterization of manganese dioxide spontaneously coated on carbon nanotubes. Carbon 2007, 45, 375–382, doi:10.1016/j.carbon.2006.09.006.
  19. Lin, S.S.; Gurol, M.D. Catalytic decomposition of hydrogen peroxide on iron oxide: Kinetics, mechanism, and implications. Environ. Sci. Technol. 1998, 32, 1417–1423, doi:10.1021/es970648k.
  20. Chou, S.; Huang, C.; Huang, Y.H. Heterogeneous and homogeneous catalytic oxidation by supported γ-feooh in a fluidized-bed reactor: Kinetic approach. Environ. Sci. Technol. 2001, 35, 1247–1251, doi:10.1021/es001129b.
Appl. Sci. EISSN 2076-3417 Published by MDPI AG, Basel, Switzerland RSS E-Mail Table of Contents Alert