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Electrochemical Oxidation for Water Treatment and the Limitation of Hazardous Byproducts. AWRA Meeting Philadelphia, PA March 21, 2013 Adrienne Donaghue Brian P. Chaplin Villanova University Department of Civil & Environmental Engineering . Introduction. - PowerPoint PPT Presentation
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AWRA MeetingPhiladelphia, PAMarch 21, 2013
Adrienne DonaghueBrian P. ChaplinVillanova University
Department of Civil & Environmental Engineering
Electrochemical Oxidation for Water Treatment and the
Limitation of Hazardous Byproducts
Introduction
Electrochemical oxidation has become promising for treatment of recalcitrant and biorefractory waste streams
Advantages:• Easy installation and operation
• Cost effective
• Environmentally friendly
2
Oxineo ®
Environmental Applications
Electrochemical Oxidation Pilot plant for landfill leachate in Cantabria, Spain.
3
Electrochemical Reactions
Power Supply+ _
Anode Cathode
e-
OHH 0.5eOH 22H2O OH + H+ + e-
OH
OH
OH
OH
OH
OH
OH
4
Electrochemical OxidationDestruction of pollutants occurs through 2 mechanisms:
1. Direct electron transfer (DET)2. Indirect oxidation via hydroxyl radicals (OH●)
* Electrochemical material plays important role in the effectiveness of oxidation!
5
Indirect electrochemical oxidation
Anode Adsorbed •OH
current
•OH
Free •OH
R
ROR or RO
CO₂ + H₂O
Oxygen Evolution
Direct electrochemical oxidation
e-
Zhu et. al, 2008.
Boron Doped Diamond Electrode
• Boron-doped diamond (BDD) film grown on p-silicon substrate using CVD (Advanced Diamond Technologies).
• Boron doping @ ppm levels provides electrical conductivity.• Inert surface and low adsorption properties• Remarkable corrosion satiability• Produces large amount of OH●
(weakly adsorbed)
• Emerging AOP technology.• Can oxidize perfluorinated
compounds
Note! These compounds can not be degraded by
other AOP technologies 6
Farrell et al. (2008)
Perfluorooctane Sulfunate (PFOS)
(C₈F₁₇SO₃⁻)
7
By-product/Perchlorate (ClO4-) Formation
• Is a multi-step process• Hazardous to human health• EPA set an advisory limit of 15 ppb for drinking
water sources• CA and MA drinking water limits of 2 and 6 ppb
Cl- OCl- ClO₂- ClO₃- ClO₄-
8
Rate-limiting step
9
By-product/ClO4- Formation Cont.
Azizi et. al, 2011
2 step process:
Cl- OCl- ClO₂- ClO₃- ClO₄-
Rate-limiting step
Reaction Zone
Anod
e
ClO₃⁻
OH●
e-
ClO3●
ClO4-
1.
2.
Research Objectives
• Understand how the reactivity of certain organics effect perchlorate formation at the anode surface
• Use “model” p-substituted phenols to determine the importance of each step in the two step process of perchlorate formation.
• Model organic behavior with in the diffuse and reaction zones to understand mechanisms of inhibition of ClO4
- at the anode surface
10
1)
2)
Experimental Setup
11
Batch ReactorRotating Disk Electrode (RDE)
Organic compounds
p-nitrophenol (p-NP)
p-methoxyphenol (p-MP)
p-benzoquinone (p-BQ)
Oxalic acid (OA)
Solutions were tested at: Kinetically Control: 1.0 mA/cm² Mass-transfer Control: 2.4 mA/cm²,
10.0 mA/cm²
12
Results: ClO₄⁻ Formation
OH• Rate Constant* Log Kow
(L mol⁻¹ s⁻¹)
p-nitrophenol (p-NP) 3.8x10⁹ 1.91
p-benzoquinone (p-BQ) 6.6x10⁹ 0.2
p-methoxyphenol (p-MP) 2.6x10¹⁰ 1.34
oxalic acid (OA) 1.4x10⁶ -0.81
p-NP p-BQ p-MP OA0
20
40
60
80
100
12099.6 96.1 93.3
5.3
93.6 92.1
53.5
0.0
29.27
85.04
12.96
0.00
1.0 mA cm⁻² 2.4 mA cm⁻² 10 mA cm⁻²
Inhi
bitio
n of
ClO
₄⁻ F
orm
ation
(%)
* Buxton et al. 1988
Initial Organic Concentration = 250 μM
13
Results: Organic Reactivity
C
x/L
Anode Diffuse Layer
COMSOL ®
Anod
e Su
rface
OH●
ClO₃●
RB
Diffusion ZoneReaction Zone
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1-2.0E-03
5.2E-18
2.0E-03
4.0E-03
6.0E-03
8.0E-03
1.0E-02 High Current Density
p-NP p-BQp-pmeth
x/μm
Conc
entr
ation
(mol
/m³)
0 0.2 0.4 0.6 0.8 1 1.2 1.4 1.6 1.8 20
0.05
0.1
0.15
0.2
0.25Low Current Density
p-NP p-BQ p-pmeth
x/μm
Conc
entr
ation
(mol
/m³)
2 μm 5 μm
Results: ClO₄⁻ Formation
14
p-NP p-BQ p-MP OA0
20
40
60
80
100
12099.6 96.1 93.3
5.3
93.6 92.1
53.5
0.0
29.3
85.0
13.0
0.0
Experimental1.0 mA cm⁻²2.4 mA cm⁻²10 mA cm⁻²
Inhi
bitio
n of
ClO
₄⁻ F
or-
mati
on (%
)
p-NP p-BQ p-MP OA0
20
40
60
80
100
120
95 97 99
1
85 8696
16 5 5 1
Model1.0 mA cm⁻²
2.4 mA cm⁻²
10 mA cm⁻²
Inhi
bitio
n of
ClO
₄⁻
Form
ation
(%)
Conclusions:
15
Limiting ClO₄- formation• Rate limiting step is a
two step process• Reactions occur right at
surface• Organic reactivity is
importantFor Low Current Densities:
Scavenging occurs on surface
For High Current Density:Location becomes important
Anod
e
ClO₃⁻
OH●
e-
ClO3●
ClO4-
Step 1
Step 2
Conclusion Cont.
• Operating under MT conditions is the most effective means to limit ClO4
- formation.• In addition, operating at these conditions is
cost effective.• EC is viable technology for refractory organic
pollutants but in order for it to be integrated into environmental applications, ClO4
- must be inhibited below advisory levels.
16
Acknowledgements
This research was funded by Advanced Diamond Technologies (ADT) in Romeoville, IL via NSF SBIR Phase II grant.
Special thanks to my advisor Dr. Brian P. Chaplin
17
Questions?
Results: LSV of p-substituted phenols
19
0.50 1.00 1.50 2.00 2.50 3.00 3.500.00
0.20
0.40
0.60
0.80
1.00
1.20p-methoxyphenol
Potential (V/ SHE)
Curr
ent D
ensit
y (m
A/cm
^2)
0.50 1.00 1.50 2.00 2.50 3.000.00
0.20
0.40
0.60
0.80
1.00
1.20
p-nitrophenol
Potential (V/SHE)
Curr
ent D
ensit
y (m
A/cm
²)
0.50 1.00 1.50 2.00 2.50 3.00 3.50-0.30
0.20
0.70
1.20
1.70 p-benzoquinone
Potential (V/SHE)
Curr
ent D
ensit
y (m
A/cm
²)
Blank
Blank
Blank
0.50 1.00 1.50 2.00 2.50 3.00 3.500.00
0.20
0.40
0.60
0.80
1.00
1.20
Oxalic Acid
Potential (V/SHE)
Curr
ent D
ensit
y (m
A/cm
²)
Blank
1 mM
5 mM
10 mM
0.75 mM
1.0 mM
0.25 mM
0.50 mM
20
Measured Rates vs. Mass Transfer
0 200 400 600 800 10000.0E+005.0E+021.0E+031.5E+032.0E+032.5E+033.0E+033.5E+034.0E+03
p-NP
Conc (µM)
Rate
(µm
ole/
m³/
min
)
0 200 400 600 800 10000.0E+00
5.0E+02
1.0E+03
1.5E+03
2.0E+03
2.5E+03
3.0E+03
3.5E+03
4.0E+03 p-BQ
Conc. (µM)
Rate
(µm
ole/
m³/
min
)0 200 400 600 800 1000
0.0E+005.0E+021.0E+031.5E+032.0E+032.5E+033.0E+033.5E+034.0E+03
p-MP
Conc (µM)
Rate
(µm
ole/
m³/
min
)
OH●
OH●
OH●
OH●
R
R
RClO3
●
ClO3●
ClO3●
ClO₄⁻
ClO₄⁻
Anod
e
Reaction Zone
Anod
e
ClO₃⁻
OH●
e-
ClO3●
ClO4-