ResearchArticle RealWastewaterUsingC/PbO -,Pb+Sn/PbO +SnO -,and...

Hindawi Publishing CorporationJournal of ChemistryVolume 2013 Article ID 691763 9 pageshttpdxdoiorg1011552013691763

Research ArticleElectrochemical Degradation of Reactive Yellow 160 Dye inRealWastewater Using CPbO2- Pb+ SnPbO2 + SnO2- andPbPbO2 Modied Electrodes

Mohamed Gaber1 Nasser Abu Ghalwa2 Abdalla M Khedr1 andMunther F Salem1

1 Chemistry Department Faculty of Science Tanta University Tanta 31111 Egypt2Department of Chemistry Faculty of Science Al Azhar University Gaza Gaza Strip Palestine

Correspondence should be addressed to Nasser Abu Ghalwa drnassergalwahotmailcom

Received 3 June 2012 Revised 1 July 2012 Accepted 17 July 2012

Academic Editor Davide Vione

Copyright copy 2013 Mohamed Gaber et al is is an open access article distributed under the Creative Commons AttributionLicense which permits unrestricted use distribution and reproduction in any medium provided the original work is properlycited

ree modied electrodes (CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2) were prepared by electrodeposition and used as anodesfor electrochemical degradation of Reactive Yellow 160 (RY160) dye in aqueous solution Different operating conditions andfactors affecting the treatment process including current density temperature initial concentration of (RY160) pH conductiveelectrolyte and time of electrolysis were studied and optimizede best degradation occurred in the presence of NaCl (4 g Lminus1) as aconductive electrolyte Aer 15min nearly complete degradation of RY160 was achieved (979 9665 and 9535 using CPbO2Pb+SnPbO2 +SnO2 and PbPbO2 electrodes resp) at pH 713 Higher degradation efficiency was obtained at 25∘Ce optimumcurrent density for the degradation of RY160 on all electrodes was 50mA cmminus2 e prepared CPbO2 Pb+SnPbO2 + SnO2 andPbPbO2 electrodes were found to be highly efficient in the treatment of effluents obtained from dyeing factory which containRY160 dye with very slight matrix effect

1 Introduction

e electrochemical performance and stability of the PbO2lm are related to substrate preparation and electrodeposi-tion conditions as well as to the organic- and inorganic-doping species that might be used [1 2] Newmethodologieshave led to improved adhesion of the PbO2 lm onto thesubstrate [3] and also to an oxidation power of the PbO2anode comparable to that of the boron-doped diamond(DDB) anode [2] however the most used substrate is stillthe Ti-Pt [1ndash6] Comninellis and Chen [7] point the possiblerelease of Pb2+ ions especially in basic solutions as the maindrawback of PbO2 anodes inmany instances a short lifetimemight be another important drawback [8]edegradation ofreactive dyewas studied bywet-air oxidation (WAO) [9] wet-peroxide oxidation (WPO) [10] photooxidation [11ndash13]electro-fenton (EF) advanced oxidation [14 15] ozonation[16 17] H2O2UV [18 19] catalytic electro-oxidation [20]

and electrocoagulation [21 22] e performances of the Ti-Pt120573120573-PbO2 and the boron-doped diamond (BDD) electrodesin the electro-oxidation of simulated wastewaters containing85mg Lminus1 of the Reactive Orange 16 and Blue Reactive 19dye were investigated using a lter-press reactor [1 4] eelectrochemical characterization of TiSnO2-Sb-Pt anodesprepared by thermal decomposition was researched usingdifferent techniques ese results were also compared tothose obtained for the TiSnO2 TiSnO2-Sb and deactivatedTiSnO2-Sb-Pt anodes COD HPLC UV-Vis and potentialcontrol measurements were also used to verify the viability ofthese anodes to degrade and decolorize wastewater solutionscontaining a reactive dye CI Reactive Orange 4 [23 24]e electrochemical degradation of CI Reactive Red 195(RR195) and 4-chloro-3-methyl phenol (CMP) in aqueoussolution on a TiSnO2-SbPbO2 electrode was investigatede inuence of operating variables on the mineralizationefficiency was studied as a function of the current density

2 Journal of Chemistry

the initial pH the initial concentration of the dye and theaddition of NaCl [25] Basic Yellow 28 (SLY) and ReactiveBlack 5 (CBWB) which are respectively methane andsulfoazo textile dyes were individually exposed to electro-chemical treatment using diamond- aluminum- copper-and iron-zinc alloy electrodes Four different electrodicmaterials were tested and presented 95 color removal andCOD removal of up to 65ndash67 in the case of CBWB dyesolution treated with the copper and iron electrodes [26]Electrochemical degradation experiments were conductedto degrade a textile dye namely Reactive Blue 19 (RB-19)e oxidation of RB-19 using titanium-based dimensionallystable anode (DSA) takes place in the bulk solution withelectrolytically generated chlorinehypochlorite Increasingthe initial pH and increasing the reaction temperaturedecreases the de-colorization efficiency At the same timeincreasing the chloride concentration and increasing thecurrent density showed an increase in the color removale complete removal of color was achieved within a shortperiod of electrolysis for different concentrations of RB-19 However the removal of COD and TOC was 558and 156 respectively for 400mg Lminus1 RB-19 with 15 g Lminus1sodium chloride concentration [27] e electrochemicaloxidation of simulated textile wastewater was studied on ironelectrodes in the presence of NaCl electrolyte in a batchelectrochemical reactore simulated textile wastewater wasprepared from industrial components based on the real mer-cerized and nonmercerized cotton and viscon process [28]Electrochemical oxidation of O-Toluidine (OT) was studiedby galvanostatic electrolysis using lead dioxide (PbO2) and(BDD) as anodes e inuence of operating parameterssuch as current density initial concentration of OT andtemperature were investigated [29]

In this study an electrodegradation method was appliedon Reactive Yellow 160 (RY160) dye (Scheme 1) by usingthree modied electrodes (CPbO2 Pb + SnPbO2 + SnO2and PbPbO2) Different factors including the pH concen-tration of electrolyte conductive electrolyte type currentdensity time of electrolysis initial concentration of RY160solution and temperature were studied and optimized for itsremoval from water Two main parameters were measuredto evaluate the electrochemical treatment efficiency theremaining pollutant concentration and the chemical oxygendemand (COD)

2 Experiments

21 Chemicals and Instrumentation Sodium chloride so-dium uoride sodium carbonate sodium sulphate cal-ciumchloride potassium chloride sodium hydroxide sulphuricacid and potassium dichromate silver sulfate were of ana-lytical grade and purchased from Merck Distilled water wasused for the preparation of solutions Standard solutions ofpotassium dichromate sulfuric acid reagent with silver sul-fate and potassiumhydrogen phthalate (KHP)were preparedto measure the COD Different standard solutions of RY160with concentration from 20ndash200mg Lminus1 were prepared to

SS

S

N

N O

O O

OO

O

NHHN

NO

N

NHN

S

OO

O O

O

S

Na+

Na+

Na+

Na+

Ominus

Ominus

Ominus

minusO

H2N

Cl

S 1 e structure formula of RY160

measure its degradation at different conditions e double-beam UV-Vis spectrophotometer is from Shimadzu the DCpower supply is model GP4303D LG Precision CO Ltd(Korea) a pH meter model AC28 TOA electronics Ltd(Japan) to adjust pH of the solutions and a digital multimeteris kyoritsu model 1008 (Japan) for reading out the currentand potential values A closed reux titrimetric unit was usedfor the COD determination [30]

22 Electrodeposition of Doped Lead Dioxide atDifferent Substrates

221 Preparation of PbPbO2odied Electrode

Lead Surface Treatment Pretreatments of the lead substratewere carried out before anodization to ensure good-adhesionlead dioxide lm Lead was rst roughened to increasethe adhesion of PbO2 deposit via subjecting its surface tomechanical abrasion by sand papers of different grades downto 400 en it was cleaned by acetone to remove sandparticles or any other particles lodged in the metal surfaceis process has a great application and good penetratingpower en it was treated with an alkali solution a mix-ture of sodium hydroxide (50 g Lminus1) and sodium carbonate(20 g Lminus1) to remove any organic materials in the surfaceand tri-sodium orthophosphate (20 g Lminus1) and sulphuric acid

Journal of Chemistry 3

(2 g Lminus1) to remove any oxides Uniform and well-adhesivedeposit necessitates a smooth surface with no oxide or scalesTo conrm our preparation the lead substrate was soakedfor 2min in a pickling solution consisting of nitric acid(400 g Lminus1) and hydrouoric acid (5 g Lminus1) and then chem-ically polished in boiled oxalic acid solution (100 g Lminus1) for5min [31]

Electrochemical Deposition of 1198751198751198751198751198751198752 PbO2 was depositedgalvanostatically on the pretreated lead substrate by elec-trochemical anodization of lead in oxalic acid solution(100 g Lminus1) is acid solution was electrolyzed galvanostat-ically for 30min at ambient temperature using an anodiccurrent density of 100mA cmminus2 e cathode was stainlesssteel (austenitic type) and the two electrodes were concentricwith the lead electrode axially is arrangement gave theformation of a regular and uniform deposit [31]

222 Preparation of Pb + SnPbO2+ SnO2-Modied Electrode

Preparation and Fabrication of Pb-Sn Alloy Electrodes BinaryPb-Sn alloy with concentration (1 1 ww) were preparedaccording to the standard following procedure and thefabrication of the electrodes as discussed in detail elsewhereAnodic oxidation of alloy electrodes was carried out and thelm was characterized for its structure [32]

Electrochemical Deposition of 1198751198751198751198751198751198752 + 1198781198781198781198781198751198752ree electrodesassembly was used for making thin lms in which theworking alloy electrodes was of 1 cm2 area with Pt (4 cm) asthe counter-electrode and saturated calomel electrode (SCE)as the reference Prior to oxidation the working electrodesurface was successively polished on 1000sim grit paper onroughing stone using water as lubricant and nally withmethanol-acetic acidmixturee alloy substratewas cleanedby acetone to remove greases or oils lodged in the metalsurface treated with an alkali solution a mixture of sodiumhydroxide (50 g Lminus1) and sodium carbonate (20 g Lminus1) toremove any organic materials in the surface and tri-sodiumorthophosphate (20 g Lminus1) sulphuric acid (2 g Lminus1) to removeany oxides To conrm our preparation the alloy substratewas soaked for 2min in a pickling solution consisting of nitricacid (400 g Lminus1) and hydrouoric acid (5 g Lminus1) and thenchemically polished in boiled oxalic acid solution (100 g Lminus1)for 5min Potentiodynamic anodization of Pb-Sn alloy wascarried out at 80∘C in the potential range from minus125 Vto +235 V with a sweep rate 200mV sminus1 Aer 20min ofcontinuous anodization [32] the electrode was taken outof the electrolysis bath and washed thoroughly in doublydistilled water followed by drying in air at 120∘C for 2 h

223 Preparation of Modied CPbO2 Electrode

Carbon Surface Treatment Pretreatment of carbon rod(8mm times 25 cm) was carried out following the procedureapplied by Narasimham and Udupa [33]e carbon rod wassoaked in 5 NaOH solution washed with distilled water

dried in furnace at 105∘C and cooked with linseed oil toreduce the porosity of rod Aer that the electrode was readyto receive doped PbO2

Electrochemical Deposition of 1198751198751198751198751198751198752 e electrodepo-sition of PbO2 was performed at constant anodic currentof 20mA cmminus2 in 12 (wv) Pb(NO3)2 solution containing5 (wv) CuSO4sdot5H2O and 3 surfactant e role of thesurfactant is to minimize the surface tension of the solutionElectrodeposition was carried out for 60min at 80∘C withcontinuous stirring [33]

23 Electrolysis of Reactive Yellow 160 Degradation Gal-vanostatic electrolyses were carried out at CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2 electrodes with current den-sity ranging from 0 to 400mA cmminus2 and electrical potentialranging from 1ndash12 volts Runs were performed at 10ndash40∘CSolutions of 100mg Lminus1 of pure RY160 solution were usede investigations of this study were carried out in thepresence of sodium chloride (05ndash20 g Lminus1) and 4 g Lminus1 ofdifferent conductive electrolytes such as NaCl CaCl2 KClNa2CO3 NaF NaPO4 and Na2SO4 with pH between 15and 12 e electrolysis duration ranges from 0ndash30mine electrochemical degradation of the RY160 solutions wascarried out in a 100mL Pyrex glass cell where the preparedelectrodes CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2work as anode and austenitic stainless steel as cathode eelectrodes were connected to a DC power supply while thecurrent and potential measurements were read out using thedigital multimeter

24 Analysis Two main parameters were measured to eval-uate the electrochemical treatment efficiency remainingpollutants (RY160) concentration was measured with thedouble-beam UV-visible spectrophotometer from Shimadzuat 120582120582max = 415 nm using calibration curve with standard errorplusmn05 and the COD was determined using a closed reuxtitrimetric method [30]

25 Cost Calculation of RY160 Degradation e cost ofelectrochemical degradation of RY160 per literwas calculatedas follows

Cost = Electrical energy consumption

times price in dollars

Electrical energy consumption 10076501007650kwsminus110076661007666 = 119868119868119868119868119868119868(1000 times 3600)

(1)

where 119868119868 applied current density (A) 119868119868 duration (h) and 119868119868applied volt (V) Price in dollar = 102 times 10minus4 $

3 Results and Discussion

31 Mechanism of Electrochemical Oxidation of OrganicPollutants e electrochemical oxidation of many organicpollutants in aqueous solutions on anode could take place bydirect electron transfer or oxygen-atom transfer In addition


to direct oxidation organic pollutants can also be treatedby an indirect electrolysis generating chemical reactant toconvert them into less deleterious products Oxidation ofthese pollutants might go further to carbon dioxide andwater via successive reactions Each of them could proceedthrough several steps such as mass transport adsorptionand direct or indirect reaction at the anode surface [31]e direct electrochemical oxidation of organic compoundscould generally occur through the following mechanism inwhich the rst step is the oxidation of water molecules onthe electrode surface (MO119909119909) is process may give rise toformation of hydroxyl radicals according to the followingequation

MO119909119909 +H2O119896119896119896⟶ MO119909119909 [OH

bull] +H+ + eminus (2)

e produced hydroxyl radicals can be oxidized to a higherstate forming the so-called higher oxide as follows

MO119909119909 [OHbull]1198961198962⟶ MO119909119909 [O] +H

+ + eminus (3)

e role of the formed higher oxide is the participation in theformation of selective oxidation of the organic pollutants (R)without complete incineration (4)

MO119909119909 [O] + R119896119896119896⟶ RO +MO119909119909 (4)

e above route can take place only if the transition ofthe underlying oxide to a higher oxidation state occurrede electrodes of this class are called ldquoactive electrodesrdquo[34] However if the product of (4) is not obtained theelectrogenerated hydroxyl radicals could directly oxidize theorganic compound to carbon dioxide and water predom-inantly causing the combustion of the organic compoundthrough hydroxylation of these compounds as follows

MO119909119909 [OHbull] + R 119896119896119896⟶ O119909119909 + 119898119898CO2 + 119899119899H2O +H

+ + eminus (5)

and this class of electrodes are called ldquononactive electrodesrdquo[35] On the basis of the abovementioned mechanism thelead dioxide anode employed in this investigation is char-acterized by high oxygen overvoltage on which (OHbull) isgenerated from the oxidation of water Hydroxyl radicals(OHbull) are electrosynthesized in aqueous solutions and canreact rapidly with aromatic pesticides leading to a polyhy-droxylation reaction followed by complete mineralizationof the initial pollutants [35] However PbO2 does not havea higher oxidation state consequently it is classied asa ldquononactive electroderdquo It was reported that lead dioxideelectrode is hydrated one and the electrogenerated hydroxylradicals are expected to be more strongly adsorbed on itssurfaceis behaviormakes lead dioxide anode very reactivetowards organic oxidation e degradation of the organicpollutants is completed by reaction with adsorbed hydroxylradicals forming carbon dioxide and water Indirect electro-chemical oxidation of organic pollutants occurs through theldquoin siturdquo electrogeneration of catalytic species with powerfuloxidizing property is process is capable of eliminating

0

5

10

15

20

25

30

35

40

45

50

1783187139871125

pH (value)

0

10

20

30

40

50

60

70

80

90

100

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

Conc (CPbO2)

Conc (PbPbO2)Conc (Pb + SnPbO2 + SnO2)

COD (CPbO2)

COD (PbPbO2)COD (Pb + SnPbO2 + SnO2)

F 1 e effect of pH on RY160 and COD removal usingCPbO2 Pb + SnPbO2 + SnO2 and PbPbO2 electrodes

the detrimental pollutants from their solutions by convertingthem into harmless compound

Although a large number of electrogenerated oxidantscan be used such as Fentonrsquos reagent and ozone thehypochlorite ion is the most widely employed oxidant inwastewater treatment [36] e mechanism of electrogener-ation from a solution containing chloride ions involves twosteps e rst one is primary oxidation of chloride ions tochlorine at the anode surface according to [36] the followingequation

2Clminus 119896119896119896⟶ Cl2 + 2eminus (6)

e second step is formation of hypochlorous acid as follows

Cl2 +H2O119896119896119896⟶ HClO + Clminus +H+ (7)

e HClO undergoes dissociation into hypochlorite andhydrogen ions as follows

HClO 119896119896119896⟶ ClOminus +H+ (8)

32 Effect of Various Factors on the Rate of Degradatione effect of different operating conditions such as typeof conductive electrolyte current density pH of simulatedsolution temperature time interval of treatment initialconcentration and NaCl concentration were studied eremaining concentration (mg Lminus119896) and COD removal ()were illustrated in Figures 1ndash7

321 Effect of pH Value e pH of the solution was variedwhile the other conditions where kept constant As shownin Figure 1 maximum removal of RY160 and COD wasachieved at pH 713 for CPbO2 Pb+SnPbO2+SnO2 and


Conc (CPbO2)


COD (CPbO2)


120

100

80

60

40

20

010 5 4 2 1 05 0

NaCl concentration (gLminus1)

120

100

80

60

40

20

0

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 2 e effect of NaCl concentration on RY160 and CODremoval using CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2electrodes

PbPbO2 respectively e pH values of the solutions wereadjusted by adding drops of H2SO4 andNaOHe reactionswere carried out for 15min for three electrodes under thefollowing conditions the initial concentration of 100mg Lminus1a current density of 50mA cmminus2 a temperature of 25∘Cand NaCl concentration of 4 g Lminus1 e distance betweenthe two electrodes was adjusted to 1 cm It was found thatthe maximum rate of degradation using CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2 electrodes was achieved inneutral medium as the optimal medium

322 Effect of the NaCl Concentration Different concen-trations of NaCl were applied to study their effect on theremoval of RY160 and the corresponding COD eliminationas indicated in Figure 2 e results indicate that an increaseof the electrolyte concentration up to 4 g Lminus1 leads to increasein the RY160 degradation rate and COD removal for threeCPbO2 Pb + SnPbO2 + SnO2 and PbPbO2 electrodese NaCl solution liberates Cl2 gas which is considered asthe active species for the degradation of organic compoundFurther increase of the NaCl concentration has slight effecton the degradation rate of RY160 and COD removal

323 Effect of Current Density As shown in Figure 3 RY160degradation and COD removal increase with increasing theapplied current density up to 50mA cmminus2 by using CPbO2Pb + SnPbO2 + SnO2 and PbPbO2 electrodes Furtherincrease of the current density was followed by gradualdecrease in RY160 degradation and COD removal due toincrease in temperature Above a temperature 35∘C sodium

120

100

80

60

40

20

100 80 60 50 40 20 100

120

100

80

60

40

20

00

Current density (mAcmminus2)

Conc (CPbO2)


COD (CPbO2)


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 3e effect of current density on RY160 and COD removalusing CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2 electrodes

hypochlorite tends to chemically decompose to sodiumchlorate as follows

3NaClO⟶ NaClO3 + 2NaCl (9)

So when temperature rises higher than 35∘C productionof NaClO falls But at higher current densities the rateof hypochlorite decomposition increases with increase incurrent density

324 Effect of Type of Electrolyte Electrolytes of 4 g Lminus1 ofthe following salts NaCl CaCl2 KCl Na2CO3 NaF Na3PO4and Na2SO4 were studied by three electrodes As appears inFigure 4 e NaCl KCl and CaCl2 were the most effectiveconductive electrolytes for the electrocatalytic degradation ofthe investigated RY160 and COD removal e Clminus anionis a powerful oxidizing agent It enhances the degradationof pollutants erefore addition of NaCl KCl and CaCl2provides the effective Clminus ion is behavior may be due tothe small ionic size of K+ and Na+ which increases the ionmobilities and the loss ability of Clminus ion Na2SO4 and NaFelectrolytes showed the least efficiency in the degradationof pollutant is may be attributed to the formation ofan adherent lm on the anode surface which poisons theelectrode surface Also these electrolytes do not containchloride ions (Clminus) in their structures and may form stableintermediate species that could not be oxidized by directelectrolysis ese observations were also conrmed in otherstudies [31]

325 Effect of the Electrolysis Time To assess the effect ofelectrolysis time experiments were conducted with oper-ating treatment conditions that were consistent with thosedescribed for CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2


or

CO

D (

)

110

90

70

50

30

10

minus10NaCl CaCl2 KCl Na2CO3 Na3PO4 Na2SO4 NaF

Conductive electrolyte type (gLminus1)

Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 4e effect of the conductive electrolyte type on RY160 andCOD removal using CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2electrodes

electrodes e maximum removal of RY160 was achievedusing CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2electrodesaer at least 15min erefore this was taken as optimaldegradation time for the removal of RY160 e optimaltime for COD removal for three electrodes was 270 340 and360min respectively

326 Effect of Temperature It is well known that the rateof diffusion of ions increases with increasing temperatureFigure 5 represents the correlation between the concentra-tion of the remaining RY160 dye and COD residual as afunction of the solution temperature e rate of the RY160degradation and COD removal increase signicantly withincreasing the solution temperature until 25∘C erefore25∘C was xed as optimal electrolysis temperature for thenext experiments

327 Effect of Initial RY160 Concentration Figure 6 showsthe effect of different initial RY160 concentrations on therate of RY160 degradation and corresponding COD removalTotal removal of the RY160 and COD can be achieved in thepresence of initial RY160 load up to 100mg Lminus1 Howeverincreasing the RY160 concentration above this level resultsin a decrease in the electrocatalytic rate of degradation eremoval efficiency of the RY160 by using CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2 electrodes at 100mg Lminus1was the optimum concentration for the initial load con-centration of RY160 As the initial RY160 concentrationincrease the degradation efficiency decrease is evidencethat the generation of the powerful oxidizing agent Clminus ionson electrode surface was not increased in constant currentdensity e optimum operating conditions for degradation

Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 5 e effect of temperature on RY160 and COD removalusing CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2 electrodes

RY160 dye for each electrode were determined and summa-rized in Table 1 At optimized conditions the percentagesof RY160 degradation and COD removal for CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2 are 979 9665 and 9535respectively e results indicate that the CPbO2 electrodeis more adequate than Pb + SnPbO2 + SnO2- and thanPbPbO2-modied electrode for the degradation of RY160eir behavior may be attributed to the color and structureof tested electrodes CPbO2modied electrodes have a blackcolor while Pb + SnPbO2 + SnO2 and PbPbO2 modiedelectrodes have a brown color It was reported that PbO2lm has two structures 120572120572-structure (brown color) and 120573120573-structure (black color) [31] e black one has a tetrahedralcrystal structure which is close-packed and more disorderedin comparison with the close-packed structure of the brown120572120572-form (orthorhombic)erefore the surface area in case oftetrahedral structure is more than that of the orthorhombicone and hence the 120573120573-PbO2 form will be more effectivethan 120572120572-PbO2 form Because the overpotential for oxygenevolution of 120573120573-PbO2 is higher than that of 120572120572-PbO2 it isexpected that the electrocatalytic properties for CPbO2-modied electrodes are more efficient than that of PbPbO2-modied electrode [34] In this work the degradation rateof RY160 was nearly completed and reached 979 9665 and9535 percentage using CPbO2 Pb + SnPbO2 + SnO2 andPbPbO2 electrodes respectively aer 15min

328 Effect of Distance between the Cathode and Anodee effect of distance between the two electrodes of thecell was studied It was found from Figure 7 that there wasan increase of hypochlorite generation by decreasing thedistance between the two electrodes up to 1 cm for CPbO2Pb + SnPbO2 + SnO2 and PbPbO2 electrodes erefore


T 1 Percentage of CODand concentration removal of RY160 onCPbO2 Pb + SnPbO2 + SnO2 and PbPbO2 electrodes in the optimumconditions

Type of electrode Removal percent of RY160 at 15min Removal percent of COD Removal percent of COD for real samplesCPbO2 979 100 at 270min 100 at 300minPb + SnPbO2 + SnO2 9665 100 at 340min 100 at 380minPbPbO2 9535 100 at 360min 100 at 400min

Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20

Initial concentration of dye (mgLminus1)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 6 e effect of initial concentration on RY160 and CODremoval using CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2electrodes

Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05

Distance between the electrodes (cm)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

F 7 e effect of distance between the cathode and anode onRY160 and COD removal using CPbO2 Pb + SnPbO2 + SnO2 andPbPbO2 electrodes

1 cm was chosen as optimum distance between electrodesfor sodium hypochlorite generation e experiments werecarried out under the following conditions current density50mA cmminus2 pH of 713 temperature of 25∘C and theconcentration of NaCl 4 g Lminus1 e time of electrolysis was15min It is clear that the sodium hypochlorite productionincrease with decreasing distance down to 1 cmis is due todrop of electrolyte ohmic potential and hence the cell voltage[37] e highest hypochlorite production was achieved withnarrow distance between the cell electrodes of 1 cm

33 Application of the Treatment Process in Real Wastew-ater Samples e treatment of RY160 effluents obtainedfrom dyeing factory was carried out by using the preparedCPbO2- Pb+SnPbO2- + SnO2 and PbPbO2-modiedelectrodes e treatment was performed rst by collectingactual waste samples from the wastewater effluents of theRY160 dyeing bath e initial dye-load concentration ofthese samples was 170mgL taken from Hubbub dyeingfactory located in the industrial area at Biet Hanon GazaStrip PNA e dyestuff solutions were treated by theelectrocatalytic oxidation technique using the same methodas applied to the treatment of RY160 in aqueous solutionto investigate the optimum condition for real wastewatercontaining the dye Aer the treatment process the removalpercentages of RY160 dye at 15min using CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2 electrodes were 979 9665and 9535 respectively e removal percentages of CODwere 100 at 300 380 and 400min for the above elec-trodes respectivelyese results indicated that the suggestedmodied electrodes are highly ecient in the treatment ofeffluents containing RY160 dye with very slight effect ofmatrix

4 Conclusion

In this work three modied electrodes (CPbO2 Pb +SnPbO2 + SnO2 and PbPbO2) were prepared by ele-crodeposition and used as anodes for electrodegradation ofRY160 in aqueous solution at different parameters includingconductive electrolyte current density temperature initialconcentration of RY160 pH and time e optimum con-ditions for three electrodes are NaCl (4 g Lminus1) temperatureat 25∘C degradation time of 15min initial concentrationof 100mg Lminus1 current density equals 50mA cmminus2 and 1 cmdistance between the three electrodes of the cell e degra-dation of RY160 was nearly completed (979 9665 and9535) using CPbO2 Pb + SnPbO2 + SnO2 and PbPbO2electrodes at pH 713 respectively e obtained results


indicated high eciency of the suggestedmodied electrodesin the treatment of effluents containing RY160 dye with veryslight matrix effect

References

[1] L S Andrade L AM Ruotolo R C Rocha-Filho et al ldquoOn theperformance of Fe and FeF doped Ti-PtPbO2 electrodes in theelectrooxidation of the Blue Reactive 19 dye in simulated textilewastewaterrdquo Chemosphere vol 66 no 11 pp 2035ndash2043 2007

[2] G Zhao Y Zhang Y Lei et al ldquoFabrication and electrochem-ical treatment application of a novel lead dioxide anode withsuperhydrophobic surfaces high oxygen evolution potentialand oxidation capabilityrdquo Environmental Science and Technol-ogy vol 44 no 5 pp 1754ndash1759 2010

[3] I Sireacutes C T J Low C Ponce-de-Leoacuten and F C Walsh ldquoedeposition of nanostructured 120573120573-PbO2 coatings from aqueousmethanesulfonic acid for the electrochemical oxidation oforganic pollutantsrdquo Electrochemistry Communications vol 12no 1 pp 70ndash74 2010

[4] L S Andrade T T Tasso D L da Silva R C Rocha-Filho NBocchi and S R Biaggio ldquoOn the performances of lead dioxideand boron-doped diamond electrodes in the anodic oxidationof simulated wastewater containing the Reactive Orange 16dyerdquo Electrochimica Acta vol 54 no 7 pp 2024ndash2030 2009

[5] L S Andrade R C Rocha-Filho N Bocchi et al ldquoDegradationof phenol using Co- and CoF-doped PbO2 anodes in electro-chemical lter-press cellsrdquo Journal of Hazardous Materials vol153 no 1-2 pp 252ndash260 2008

[6] L Ciriacuteaco C Anjo J Correia M J Pacheco and A LopesldquoElectrochemical degradation of Ibuprofen on TiPtPbO2 andSiBDD electrodesrdquo Electrochimica Acta vol 54 no 5 pp1464ndash1472 2009

[7] C Comninellis and G Chen Electrochemistry for the Environ-ment Springer New York NY USA 2010

[8] J M Aquino G F Pereira R C Rocha-Filho N Bocchi andS R Biaggio ldquoElectrochemical degradation of a real textileeffluent using boron-doped diamond or 120573120573-PbO2 as anoderdquoJournal of Hazardous Materials vol 192 no 3 pp 1275ndash12822011

[9] M Zhou and J He ldquoDegradation of azo dye by three cleanadvanced oxidation processes Wet oxidation electrochemicaloxidation and wet electrochemical oxidation-A comparativestudyrdquo Electrochimica Acta vol 53 no 4 pp 1902ndash1910 2007

[10] B Goumlzmen B Kayan A M Gizir and A Hesenov ldquoOxidativedegradations of reactive blue 4 dye by different advancedoxidation methodsrdquo Journal of Hazardous Materials vol 168no 1 pp 129ndash136 2009

[11] R A Damodar S J You and S H Ou ldquoCoupling of membraneseparation with photocatalytic slurry reactor for advanced dyewastewater treatmentrdquo Separation and Purication Technologyvol 76 no 1 pp 64ndash71 2010

[12] E M El-Maghraby ldquoEffect of Sn ratio on the photocatalyticdegradation of methylene blue and soot of ink by TiO2-SnO2nanostructured thin lmsrdquo Physica B vol 405 no 10 pp2385ndash2389 2010

[13] P Bansal and D Sud ldquoPhotodegradation of commercial dyeProcion BlueHERD from real textile wastewater using nanocat-alystsrdquo Desalination vol 267 no 2-3 pp 244ndash249 2011

[14] G Zhang F Yang and L Liu ldquoComparative study ofFe2+ H2O2 and Fe3+ H2O2 electro-oxidation systems in the

degradation of amaranth using anthraquinonepolypyrrolecomposite lm modied graphite cathoderdquo Journal of Electro-analytical Chemistry vol 632 no 1-2 pp 154ndash161 2009

[15] H S El-Desoky M M Ghoneim R El-Sheikh and N MZidan ldquoOxidation of Levax CA reactive azo-dyes in industrialwastewater of textile dyeing by electro-generated Fentonrsquosreagentrdquo Journal of Hazardous Materials vol 175 no 1ndash3 pp858ndash865 2010

[16] G Moussavi and M Mahmoudi ldquoDegradation and biodegrad-ability improvement of the reactive red 198 azo dye using cat-alytic ozonation withMgOnanocrystalsrdquoChemical EngineeringJournal vol 152 no 1 pp 1ndash7 2009

[17] M T F Tabrizi D Glasser and D Hildebrandt ldquoWastewatertreatment of reactive dyestuffs by ozonation in a semi-batchreactorrdquo Chemical Engineering Journal vol 166 no 2 pp662ndash668 2011

[18] M Riera-Torres and M C Gutieacuterrez ldquoColour removal ofthree reactive dyes by UV light exposure aer electrochemicaltreatmentrdquo Chemical Engineering Journal vol 156 no 1 pp114ndash120 2010

[19] Ş Guumll and Ouml Oumlzcan-Yildirim ldquoDegradation of reactive red194 and reactive yellow 145 azo dyes by O3 and H2O2UV-Cprocessesrdquo Chemical Engineering Journal vol 155 no 3 pp684ndash690 2009

[20] L Du Y Wang S Dai J Pei S Qin and C Hu ldquoComparativestudy on the catalytic electrooxidative abilities of RuOx-PdO-TiO2Ti and RuOx-PdOTi anoderdquo Journal of Hazardous Mate-rials vol 185 no 2-3 pp 1596ndash1599 2011

[21] A Aouni C Fersi M Ben Sik Ali and M DhahbildquoTreatment of textile wastewater by a hybrid electrocoagula-tionnanoltration processrdquo Journal of Hazardous Materialsvol 168 no 2-3 pp 868ndash874 2009

[22] C Phalakornkule S Polgumhang W Tongdaung B Karakatand T Nuyut ldquoElectrocoagulation of blue reactive red disperseand mixed dyes and application in treating textile effluentrdquoJournal of Environmental Management vol 91 no 4 pp918ndash926 2010

[23] A I del Riacuteo J Fernaacutendez J Molina J Bonastre and FCases ldquoOn the behaviour of doped SnO2 anodes stabilized withplatinum in the electrochemical degradation of reactive dyesrdquoElectrochimica Acta vol 55 no 24 pp 7282ndash7289 2010

[24] A I del Riacuteo J Molina J Bonastre and F Cases ldquoInuenceof electrochemical reduction and oxidation processes on thedecolourisation and degradation of CI Reactive Orange 4solutionsrdquo Chemosphere vol 75 no 10 pp 1329ndash1337 2009

[25] S Song J Fan Z He et al ldquoElectrochemical degradation ofazo dye CI Reactive Red 195 by anodic oxidation on TiSnO2-SbPbO2 electrodesrdquo Electrochimica Acta vol 55 no 11 pp3606ndash3613 2010

[26] M Ceroacuten-Rivera M M Daacutevila-Jimeacutenez and M P Elizalde-Gonzaacutelez ldquoDegradation of the textile dyes Basic yellow 28 andReactive black 5 using diamond and metal alloys electrodesrdquoChemosphere vol 55 no 1 pp 1ndash10 2004

[27] D Rajkumar B J Song and J G Kim ldquoElectrochemicaldegradation of Reactive Blue 19 in chloride medium for thetreatment of textile dyeing wastewater with identication ofintermediate compoundsrdquoDyes and Pigments vol 72 no 1 pp1ndash7 2007

[28] B K Koumlrbahti and A Tanyolaccedil ldquoElectrochemical treatment ofsimulated textile wastewater with industrial components andLevax Blue CA reactive dye optimization through response


surface methodologyrdquo Journal of Hazardous Materials vol 151no 2-3 pp 422ndash431 2008

[29] E Hmani S Chaabane Elaoud Y Samet and R Abdel-heacutedi ldquoElectrochemical degradation of waters containing O-Toluidine on PbO2 and BDD anodesrdquo Journal of HazardousMaterials vol 170 no 2-3 pp 928ndash933 2009

[30] A E Greenberg L S Clesceri and L S A D Eaton StandardMethods for the Examination of Water and Wastewater vol 518th edition 1992

[31] H S Awad and N A Galwa ldquoElectrochemical degradation ofAcid Blue and Basic Brown dyes on PbPbO2 electrode in thepresence of different conductive electrolyte and effect of variousoperating factorsrdquo Chemosphere vol 61 no 9 pp 1327ndash13352005

[32] I Mukhopadhyay P Selvam M Sharon P Veluchamy andH Minoura ldquoSurface characterisation of anodic lms of Pb-Snalloy electrodes e effect of Sn on the photoelectrochemicalpropertiesrdquo Materials Chemistry and Physics vol 49 no 2 pp169ndash173 1997

[33] K C Narasimham and H V K Udupa ldquoPreparation andapplications of graphite substrate lead dioxide (Gsld) anoderdquoJournal of the Electrochemical Society vol 123 no 9 pp1284ndash1298 1976

[34] R L Pelegrino R A Di Iglia C G Sanches L A Avaca and RBertazzoli ldquoComparative study of commercial oxide electrodesperformance in electrochemical degradation of organics inaqueous solutionsrdquo Journal of the Brazilian Chemical Societyvol 13 no 1 pp 60ndash65 2002

[35] M Panizza C Bocca and G Cerisola ldquoElectrochemical treat-ment of wastewater containing polyaromatic organic pollu-tantsrdquoWater Research vol 34 no 9 pp 2601ndash2605 2000

[36] M Panizza and G Cerisola ldquoRemoval of organic pollu-tants from industrial wastewater by electrogenerated FentonrsquosreagentrdquoWater Research vol 35 no 16 pp 3987ndash3992 2001

[37] G H Kelsall ldquoHypochlorite electro-generation I A parametricstudy of a parallel plate electrode cellrdquo Journal of AppliedElectrochemistry vol 14 no 2 pp 177ndash186 1984

Submit your manuscripts athttpwwwhindawicom

Chromatography Research International

Hindawi Publishing Corporationhttpwwwhindawicom Volume 2013


Carbohydrate Chemistry

International Journal of

Hindawi Publishing Corporationhttpwwwhindawicom


Analytical ChemistryVolume 2013

ISRN Chromatography


Hindawi Publishing Corporation httpwwwhindawicom Volume 2013Hindawi Publishing Corporation httpwwwhindawicom Volume 2013

The Scientific World Journal

Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2013


CatalystsJournal of

ISRN Analytical Chemistry


ElectrochemistryInternational Journal of

Hindawi Publishing Corporation httpwwwhindawicom Volume 2013


Advances in

Physical Chemistry

ISRN Physical Chemistry


SpectroscopyInternational Journal of


ISRN Inorganic Chemistry



Journal of

Chemistry


Inorganic ChemistryInternational Journal of


International Journal ofPhotoenergy


Analytical Methods in Chemistry

Journal of

Volume 2013

ISRN Organic Chemistry



Journal of

Spectroscopy


the initial pH the initial concentration of the dye and theaddition of NaCl [25] Basic Yellow 28 (SLY) and ReactiveBlack 5 (CBWB) which are respectively methane andsulfoazo textile dyes were individually exposed to electro-chemical treatment using diamond- aluminum- copper-and iron-zinc alloy electrodes Four different electrodicmaterials were tested and presented 95 color removal andCOD removal of up to 65ndash67 in the case of CBWB dyesolution treated with the copper and iron electrodes [26]Electrochemical degradation experiments were conductedto degrade a textile dye namely Reactive Blue 19 (RB-19)e oxidation of RB-19 using titanium-based dimensionallystable anode (DSA) takes place in the bulk solution withelectrolytically generated chlorinehypochlorite Increasingthe initial pH and increasing the reaction temperaturedecreases the de-colorization efficiency At the same timeincreasing the chloride concentration and increasing thecurrent density showed an increase in the color removale complete removal of color was achieved within a shortperiod of electrolysis for different concentrations of RB-19 However the removal of COD and TOC was 558and 156 respectively for 400mg Lminus1 RB-19 with 15 g Lminus1sodium chloride concentration [27] e electrochemicaloxidation of simulated textile wastewater was studied on ironelectrodes in the presence of NaCl electrolyte in a batchelectrochemical reactore simulated textile wastewater wasprepared from industrial components based on the real mer-cerized and nonmercerized cotton and viscon process [28]Electrochemical oxidation of O-Toluidine (OT) was studiedby galvanostatic electrolysis using lead dioxide (PbO2) and(BDD) as anodes e inuence of operating parameterssuch as current density initial concentration of OT andtemperature were investigated [29]

In this study an electrodegradation method was appliedon Reactive Yellow 160 (RY160) dye (Scheme 1) by usingthree modied electrodes (CPbO2 Pb + SnPbO2 + SnO2and PbPbO2) Different factors including the pH concen-tration of electrolyte conductive electrolyte type currentdensity time of electrolysis initial concentration of RY160solution and temperature were studied and optimized for itsremoval from water Two main parameters were measuredto evaluate the electrochemical treatment efficiency theremaining pollutant concentration and the chemical oxygendemand (COD)

2 Experiments

21 Chemicals and Instrumentation Sodium chloride so-dium uoride sodium carbonate sodium sulphate cal-ciumchloride potassium chloride sodium hydroxide sulphuricacid and potassium dichromate silver sulfate were of ana-lytical grade and purchased from Merck Distilled water wasused for the preparation of solutions Standard solutions ofpotassium dichromate sulfuric acid reagent with silver sul-fate and potassiumhydrogen phthalate (KHP)were preparedto measure the COD Different standard solutions of RY160with concentration from 20ndash200mg Lminus1 were prepared to

SS

S

N

N O

O O

OO

O

NHHN

NO

N

NHN

S

OO

O O

O

S

Na+

Na+

Na+

Na+

Ominus

Ominus

Ominus

minusO

H2N

Cl

S 1 e structure formula of RY160

measure its degradation at different conditions e double-beam UV-Vis spectrophotometer is from Shimadzu the DCpower supply is model GP4303D LG Precision CO Ltd(Korea) a pH meter model AC28 TOA electronics Ltd(Japan) to adjust pH of the solutions and a digital multimeteris kyoritsu model 1008 (Japan) for reading out the currentand potential values A closed reux titrimetric unit was usedfor the COD determination [30]

22 Electrodeposition of Doped Lead Dioxide atDifferent Substrates

221 Preparation of PbPbO2odied Electrode

Lead Surface Treatment Pretreatments of the lead substratewere carried out before anodization to ensure good-adhesionlead dioxide lm Lead was rst roughened to increasethe adhesion of PbO2 deposit via subjecting its surface tomechanical abrasion by sand papers of different grades downto 400 en it was cleaned by acetone to remove sandparticles or any other particles lodged in the metal surfaceis process has a great application and good penetratingpower en it was treated with an alkali solution a mix-ture of sodium hydroxide (50 g Lminus1) and sodium carbonate(20 g Lminus1) to remove any organic materials in the surfaceand tri-sodium orthophosphate (20 g Lminus1) and sulphuric acid

















(1)






MO119909119909 +H2O119896119896119896⟶ MO119909119909 [OH



MO119909119909 [OHbull]1198961198962⟶ MO119909119909 [O] +H

+ + eminus (3)


MO119909119909 [O] + R119896119896119896⟶ RO +MO119909119909 (4)



+ + eminus (5)


0

5

10

15

20

25

30

35

40

45

50

1783187139871125

pH (value)

0

10

20

30

40

50

60

70

80

90

100

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

Conc (CPbO2)


COD (CPbO2)









HClO 119896119896119896⟶ ClOminus +H+ (8)




Conc (CPbO2)


COD (CPbO2)


120

100

80

60

40

20

010 5 4 2 1 05 0


120

100

80

60

40

20

0

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





120

100

80

60

40

20

100 80 60 50 40 20 100

120

100

80

60

40

20

00


Conc (CPbO2)


COD (CPbO2)


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)








or

CO

D (

)

110

90

70

50

30

10



Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)







Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy

















(1)






MO119909119909 +H2O119896119896119896⟶ MO119909119909 [OH



MO119909119909 [OHbull]1198961198962⟶ MO119909119909 [O] +H

+ + eminus (3)


MO119909119909 [O] + R119896119896119896⟶ RO +MO119909119909 (4)



+ + eminus (5)


0

5

10

15

20

25

30

35

40

45

50

1783187139871125

pH (value)

0

10

20

30

40

50

60

70

80

90

100

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

Conc (CPbO2)


COD (CPbO2)









HClO 119896119896119896⟶ ClOminus +H+ (8)




Conc (CPbO2)


COD (CPbO2)


120

100

80

60

40

20

010 5 4 2 1 05 0


120

100

80

60

40

20

0

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





120

100

80

60

40

20

100 80 60 50 40 20 100

120

100

80

60

40

20

00


Conc (CPbO2)


COD (CPbO2)


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)








or

CO

D (

)

110

90

70

50

30

10



Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)







Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy



MO119909119909 +H2O119896119896119896⟶ MO119909119909 [OH



MO119909119909 [OHbull]1198961198962⟶ MO119909119909 [O] +H

+ + eminus (3)


MO119909119909 [O] + R119896119896119896⟶ RO +MO119909119909 (4)



+ + eminus (5)


0

5

10

15

20

25

30

35

40

45

50

1783187139871125

pH (value)

0

10

20

30

40

50

60

70

80

90

100

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)

Conc (CPbO2)


COD (CPbO2)









HClO 119896119896119896⟶ ClOminus +H+ (8)




Conc (CPbO2)


COD (CPbO2)


120

100

80

60

40

20

010 5 4 2 1 05 0


120

100

80

60

40

20

0

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





120

100

80

60

40

20

100 80 60 50 40 20 100

120

100

80

60

40

20

00


Conc (CPbO2)


COD (CPbO2)


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)








or

CO

D (

)

110

90

70

50

30

10



Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)







Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy


Conc (CPbO2)


COD (CPbO2)


120

100

80

60

40

20

010 5 4 2 1 05 0


120

100

80

60

40

20

0

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





120

100

80

60

40

20

100 80 60 50 40 20 100

120

100

80

60

40

20

00


Conc (CPbO2)


COD (CPbO2)


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)








or

CO

D (

)

110

90

70

50

30

10



Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)







Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy


or

CO

D (

)

110

90

70

50

30

10



Conc (CPbO2)


COD (CPbO2)


Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)





Conc (CPbO2)


COD (CPbO2)


40

30

20

10

0

40

30

20

10

040 30 25 18 10 5

Temprature (∘C)

CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)







Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy




Conc (CPbO2)


COD (CPbO2)


100

90

80

70

60

50

40

30

20

10

0

70

60

50

40

30

20

10

0200 150 100 75 50 20


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)


Conc (CPbO2)


COD (CPbO2)


20

15

10

5

0

0minus5

7

6

5

4

3

2

1

2 15 1 05


CO

D (

)

Rem

ain

ing

con

cen

trat

ion

(mgLminus1

)




4 Conclusion




References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy



References


















































ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy





















ISRN Chromatography






CatalystsJournal of






Advances in

Physical Chemistry








Journal of

Chemistry







Journal of

Volume 2013




Journal of

Spectroscopy

ResearchArticle RealWastewaterUsingC/PbO -,Pb+Sn/PbO +SnO -,and...

Documents

Transcript of ResearchArticle RealWastewaterUsingC/PbO -,Pb+Sn/PbO +SnO -,and...