RISKeLearning Nanotechnology – Applications and Implications … · • According to some...
Transcript of RISKeLearning Nanotechnology – Applications and Implications … · • According to some...
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SBRP/NIEHS
William Suk
Heather Henry
Claudia Thompson
Beth Anderson
Kathy Ahlmark
EPA
Michael Gill
Jayne Michaud
Warren Layne
Marian Olsen
Charles Maurice
Nora Savage
Barbara Walton
Randall Wentsel
Mitch Lasat
Martha Otto
MDB
Maureen Avakian
Larry Whitson
Larry Reed
Organizing Committee:
Nanotechnology –Applications and Implications for Superfund
RISKeLearning
February 13, 2007Session 2:
“Nanotechnology – Metal Remediation”
Dr. Mason Tomson, Rice UniversityDr. Shas Mattigod, Pacific
Northwest National Laboratory
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Contaminant Removal and Water Reuse: Research Opportunities with Nanotechnology
Mason TomsonVicki Colvin
Amy T. Kan, Heather Shipley, Sujin Yean, Xuekun Cheng, Lili Cong, Ping Zhang, Wei Chen and John Czarnik
Center for Biological and Environmental Nanotechnology&
Department of Civil and Environmental EngineeringRice University
Houston, TX
Arsenic Adsorption on Nanoscale Magnetite
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Overview of Arsenic
• Widely distributed in earth’s crust• In water by dissolution of ores/minerals• Concentrated in areas by erosion• Human Activities sources
– Residue from alloys and treatments– Burning of fossil fuels
• Largest threat to humans– Inorganic As(III) and As(V)– In drinking water
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These are the most general and important “first” points to know about Arsenic. The particularly important point, highlighted in green, is that it is As(III) that is the largest threat to humans.
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Arsenic Mobility Profile
• Arsenates-As(V) – Usually occurs as ions: H2AsO4
- and HAsO42-
• predominates in aerobic soils
• Arsenites – As(III)– Occurs as H3AsO3 (pH below 9.2)– Exists in slightly reduced soils– Larger concern than As(V) because of
• higher toxicity • greater mobility
• Arsenic in water– rather than solubility equilibrium controlling the mobility of
arsenic, it is usually controlled by redox conditions, pH, biological activity, and adsorption/desorption reactions.
• Arsenic immobilization through ionic adsorption can be controlled within normal oxidizing Eh/pH conditions to varying degrees
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Redox conditions, pH, biological activity and specific chemical reaction are keys to distribution – NOT A GENERAL SOLUBILITY BALANCE!
The last statement is a “soft” way of saying “without normal oxidizing and acid conditions, we have a problem!”
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Source: Polizzotto, M., Scott Fendorf, S., Harvey, C., Badruzman., B., Ali, A.(2005) Influxes and Near-surface Processes Governing Arsenic in Aquifers of Bangladesh
Arsenic Deposition and Transport
•Arsenic is deposited in association with iron (hydr)oxides and sulfides.•Arsenic sulfides survive burial and are a primary form of solid-phase •Arsenic lower in the aquifer reductive dissolution of iron (hydr)oxide minerals in the surface and near-surface releases arsenic to solution. •Arsenic is transported in the aquifer and drawn to the wells with the groundwater
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This is how arsenic is deposited and gets into a aquifer.
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Molecular Structure
H
H
H
O
O
O OAs
Arsenite Arsenate
H
H
HO
O
O As
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For the scientifically and chemically oriented audience members!
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Where Does Arsenic Come From?
• Natural sources of arsenic (contained in 250 naturally-occurring minerals)– Minerals (particularly sulfides)– Oxides (particularly metals)– Volcanic-derived sediment– Can affect large areas, such as extensive aquifers
• Significant human activity sources– mineral extraction and processing– glass manufacturing– wood preserving– pesticide production and application– waste pile leaching– and coal/oil production and processing – Extent/occurrence is usually over a limited area 7
The picture is a sample of arsenic sulfide.
Important points to emphasize are that:
•Aquifers are “vessels” that can, potentially, extend a contamination problem over a wide area.
•Human activity sources of arsenic, though potentially and actually life-threatening, usually create contamination zones that are limited, relative to natural sources.
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Arsenic Redox Reaction
• H3AsO4 + 2H+ + 2e- H3AsO3 + H2O
• The key is that arsenic is “locked away” in iron oxyhydroxides when there is plenty of oxygen present. The oxidized form, arsenate, dominates. When the oxygen level is low, “reducing environment”, arsenate converts to arsenite.
• When arsenite is exposed to oxygen, it oxidizes, but the rate in air is only a few percent in one week. (Clifford, D., Ceber, L., Chow, S. (1983)
Arsenite – As(III)Arsenate – As(V)
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A reducing environment can create and preserve arsenite. When we withdraw it from that environment, as in withdrawing water from a well, it can take a long time for a significant portion of the arsenite to oxidize and become “safer”!
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Perspective on Long Term Exposure Drinking Water - Health Impact
• Cancer of the skin, lungs, urinary bladder, kidney • Skin changes: pigmentation changes & thickening • Increased risks of lung/bladder cancer and of
arsenic-associated skin lesions have been observed at arsenic concentrations less than 0.05 mg/L (50 ppb)
• No universal definition of the disease (combination of harmful symptoms/maladies) caused by arsenic. This complicates assessment of the breadth of arsenic’s effect on the health in any population.
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This is the result of arsenic ingestion – including inhalation impact on the lungs. (I don’t have a specific reference for the 50 ppb statement, but it is stated in at least one place in USGS or WHO publications. JWC)
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Arsenic’s Effects
Source: Wilson, R., (2006) Chronic Arsenic Poisoning: History, Study and Remediation. Maintained website.
(Photo by Steven Lamm MD)
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Plenty more on the referenced website!
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Scope of the Problem!
• “The life-time risk of dying from cancer by drinking one liter of water per day containing an arsenic concentration of 50 μg/L could be as high as 1 in 100.“ (NRDC, 2001)
• “The theoretical lifetime excess risk for bladder and lung cancer combined is estimated to be approximately 1 in 1000 at 3 micrograms per liter.”
• “According to some estimates, arsenic in drinking-water will cause 200,000 -- 270,000 deaths from cancer in Bangladesh alone (NRC, 1998; Smith, et al, 2000).
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This is how the
Contamination
Location and Level of contamination
Population
Health
and Life and Death
come together!
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>50 ppb >50 ppb
>50 ppb
>10 ppm
>50 ppb
>50 ppb
>500 ppb
Areas of High Arsenic Concentration in Drinking Water
>200 ppb
>100 ppb
>200 ppb
>1000 ppb>1000 ppb
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The values shown are far from the highest recordings in these areas, but they are presented to provide a “sampled picture” of how arsenic contamination is spread throughout the world. (The next slide – if used – is a table showing the ranges of concentrations encountered in some of these areas.)
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International Arsenic Contamination Sites
Location Conc. As (ppb).Taiwan: Southwest Coast 100–1810
Taiwan: Putai 470–897
Chinese Inner Mongolia (Hetao Plain) 50–1080
Bangladesh: Ganges Delta 10–2040
Bangladesh: Pabna (North District) 50–14,000
India: West Bengal 50–3400
Vietnam: Hanoi and Red River Valley 1–3050
Note: Table adapted from Joanna Shaofen Wang and Chien M. Wai, U.Of Idaho. J. Chem. Ed.,vol. 8, n.2, p.209 Feb., 2004 13
Clearly, the values on the previous slide (which showed 100 ppb in Taiwan, > 200 ppb in Bangladesh and >1,000 in China) were not maximum values! In fact the next slide shows haw bad the problem is in one area in Bangladesh.)
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Arsenic Concentrations in US Drinking Water
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Here is map of the sampled concentrations of arsenic in the water in the United States. Recently (January 2006), the USA has imposed a standard of <10 ppb (<10 mg/L) concentration in drinking water in the Country. This change from the previous 50 ppb has intensified the search for improved processes for reducing the amount of arsenic in drinking water – on top of the demands caused by much more hazardous concentrations in other areas of the world.
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Houston Tap Water
NRDC Report 2002 15
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Perspective: Contamination Levels• According to some estimates, arsenic in drinking-water will cause 200,000
-- 270,000 deaths from cancer in Bangladesh alone (NRC, 1998; Smith, et al, 2000).
• Seven of 16 districts of West Bengal (India) have been reported to have ground water arsenic concentrations above 0.05 mg/L; total population is over 34 million ( 1996); estimated that the population using arsenic-rich water is more than 1 million (above 0.05 mg/L) and 1.3 million (above 0.01 mg/L) (Chowdhury et al,1997).
• According to a British Geological Survey study in 1998 on shallow tube-wells in 61 of the 64 districts in Bangladesh, 46% of the samples were above 0.010 mg/L and 27% were above 0.050 mg/L. It was estimated that the number of people exposed to arsenic concentrations above 0.05 mg/l was 28-35 million and the number exposed to more than 0.01 mg/l (10μg/L) is 46-57 million (BGS 2000).
• EPA estimated that some 13 million of the population of USA, mostly in the western states, are exposed to arsenic in drinking- water at 0.01 mg/L, although concentrations appear to be typically much lower than those encountered in areas such as Bangladesh and West Bengal. (USEPA 2001)
Source” World Health Organization (United Nations) Fact Sheet No. 210 (rev. May, 2001)16
This is an “encapsulation of information” that briefly gives glimpse of the extent of the contamination and potential health impact of arsenic contamination.
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Drinking Water “Recommendations” & “Standards”
• World Health Organization RecommendationsYear Concentration1958 0.20 mg/L (200 ppb)1963 0.05 mg/L (50 ppb)1993 0.01 mg/L (10 ppb)
• United States– 50 ppb was set by Public Health Dept. in 1942 – EPA adopted this standard in 1975 as “interim” regulation– IN 1986 Congress converted this “interim” to a National
Regulation and requested EPA review and set new standards.
– 50 ppb (0.050 mg/L) prior to January, 2006– 10 ppb, currently
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ES&T March 15, 2004 18
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Effects of New Standard
• Max. Levels reduced from 50 μg/L to 10 μg/L
• 13 million people in areas of higher standard (West, Midwest, N. England)
• Annual Estimated Reductions:Cases Deaths
Bladder Cancer 19-31 5-8Lung Cancer 19-25 16-22Diabetes ? ?Heart Disease ? ?
Source: Environmental Protection Agency (US) (Jan. 2001) Technical Fact Sheet EPA 815-F-00-016
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Here is the Environmental Protection Agency’s assessment of the annual impact of reducing the levels of arsenic in drinking water in the United States
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Annual Estimated Cost of Raising Arsenic Standard: <50ppb to <10ppb
$ 181Total
1.0State Costs
2.7Monitoring
$ 177*Treatment
EPA estimates the total national annualized costs of treatment, monitoring, reporting, recordkeeping, and administration for this rule to be approximately $181 million (using 1999 dollars at a three percent discount rate.
**(3% Discount Rate, $millions)(3% Discount Rate, $millions)
Source: Environmental Protection Agency (US) (Jan. 2001) Technical Fact Sheet EPA 815-F-00-016
In millions of dollars
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Note that this is the annual cost.
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Motivation for Our Work with Nanotechnology
• A need for a cost-effective and high-performance technology to remove arsenic from drinking water – Reduce arsenic to less than 10μg/L in less than
a minute
• The mechanism of arsenic removal by iron oxides
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Current Technologies
• US EPA As standard level: 10μg/L
Solid-liquid separationCoagulations with iron salts
ExpensiveMembrane methods
No As(III) removal
Interference from SO42-& TDS
Ion exchange
DisadvantagesTechnology
http://www.unu.edu/env/Arsenic/Han.pdf (accessed October 16, 2006)
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Nano-MagnetiteControl Synthesis of Engineered Nano-Magnetite
Collaboration with Vicki Colvin: Science 314, 964 2006
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Magnetic Properties of Nano-magnetite
Magnetite nanocrystals < 40 nm: Single domain magnetSize dependent magnetic properties: ferromagnetic (>20 nm)
paramagnetic (6-20 nm)(Science 2006)
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Magnetic Separator
Solution before column
Solution after
column
Magnetic Separator
Nano-magnetite can be separated by hand held magnetic device (Science 2006) 25
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Magnetite Nanoparticles
• Mean particle diameter: 20nm
• Surface area: 60m2/g100 nm
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Experimental Set-up: Vessel Apparatus
• Temperature controlled
• Overhead agitator/stirrer
• 3 connectors by 3-way valves– Sampling
– Ar gas
– Solution injection/gas purging
• Anoxic/ Oxic conditions27
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Effect of solid concentration on As removal
0
20
40
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0 0.5 1 1.5 2time(hrs)
% A
sV in
so
luti
on
0
20
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0 0.5 1 1.5 2
time(hrs)
% A
sIII
in s
olu
tio
n
0.05g/L0.05g/L
0.1g/L0.1g/L
0.2g/L0.2g/L
0.5g/L0.5g/L
AsV AsIII
Initial Conc. ~100μg/L28
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Modified Rate Equation
t*rSSAk
swmax
00
swmax
0t
swme*)r)b*q(1
]As[]As([
r)b*q(1
]As[]As[ ∗∗
∗+−+
∗+=
[As]t: As concentration at time, t (s)[As]0: As concentration at time = 0, (μg/L)qmax *b: Langmuir isotherm (L/g)rsw: solid to solution ratio (g/L or g/m3)SSA: specific surface area (m2/g)t: time (s)
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Model Prediction
AsV AsIII
qmax*b = 15.04 L/gkm = 1.057e-7 m/s
r = 0.992
qmax*b = 19.17 L/gkm = 9.360e-8 m/s
r = 0.992
0
10
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0 20 40 60 80 100
As measured ug/L
As
calc
. ug
/L
0.05g/L
0.1g/L
0.2g/L
0.5g/L
0
10
20
30
40
50
60
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80
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100
0 20 40 60 80 100
AsIII measured ug/L
AsI
II c
alc.
ug
/L
0.05g/L
0.1g/L
0.2g/L
0.5g/L
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Competitive Adsorption: Bicarbonate
0
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% A
sIII
in s
olu
tio
n
0mg/L HCO3 10mg/L HCO350mg/L HCO3 100mg/L HCO3250mg/L HCO3 500mg/L HCO3fitted values
0
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0 0.5 1 1.5 2
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% A
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in s
olu
tio
n
0mg/L HCO3 10mg/L HCO350mg/L HCO3 100mg/L HCO3250mg/L HCO3 500mg/L HCO3fitted values
AsIII AsV
Initial Conc. ~100μg/L31
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Competitive Adsorption: Sulfate
AsIII AsV
0
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0 0.5 1
time(hrs)
%A
s in
so
luti
on
0mg/L SO450mg/L 100mg/L250mg/L
0
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0 0.5 1
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%A
s in
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on
0mg/L SO450mg/L100mg/L250mg/L
Initial Conc. ~100μg/L 32
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Competitive Adsorption: Organic Matter
AsIII AsV
0
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0 0.2 0.4 0.6 0.8 1
time(hrs)
%A
sV
in s
olu
tio
n
0mg/L OM
5mg/L OM
10mg/L OM
25mg/L OM0
20
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0 0.2 0.4 0.6 0.8 1
time(hrs)
%A
s II
I in
so
luti
on
0mg/L OM
5mg/L OM
10mg/L OM
25mg/L OM
Initial Conc. ~100μg/L 33
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Competitive Adsorption: Silica
AsIII AsV
Initial Conc. ~100μg/L
0
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0 0.2 0.4 0.6 0.8 1
Time (hrs)
% A
sV
in s
olu
tio
n
0 mg/L SiO2 10mg/L
25mg/L 50mg/L
100mg/L
0
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0 0.2 0.4 0.6 0.8 1
Time (hrs)
% A
sIII
in s
olu
tio
n
0 mg/L SiO2 10mg/L
25mg/L 50mg/L
100mg/L
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As/Nano-Fe3O4 Adsorption/Desorption Hysteresis
0
100
200
300
400
500
600
0 10 20 30 40 50
As in soluition (ug/L)
As
ad
sorb
ed
(m
g/K
g)
35
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Field Test – Brownsville, TX
• Arsenic-contaminated water from Southmost Regional Authority Desalination Plant Brownsville,TX in August, 2006: Wells #8 and 12 (Brackish water: ~ 5mS/cm)
36
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Characterization of Brownsville Wells
36.441.4Silica
(mg/L as SiO2)
0.160.23PO43- (mg/L)
1192.51165SO42- (mg/L)
464.6335Alkalinity
(mg/L as HCO3-)
7.397.32pH
39.027.2Initial As (μg/L)
Well #12Well #8
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Results: 0.5g/L Fe3O4 for Brownsville Water
0
5
10
15
20
25
30
35
40
0 0.2 0.4 0.6 0.8 1
time (hrs)
As
in s
olu
tio
n u
g/L
38
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Results – Field Tests: Well #120.1g/L Fe3O4 and varying conc. of Fe3+
0
10
20
30
40
0.0 0.2 0.4 0.6 0.8 1.0
Time (h)
As
co
nc
in S
olu
tio
n (
ug
/L) 5mg/L Fe3+
7.5mg/L Fe3+
10mg/L Fe3+
39
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Results – Field Tests: Well #8 0.1g/L Fe3O4 and 5mg/L Fe3+
0
5
10
15
20
25
30
0 0.2 0.4 0.6 0.8 1
Time (h)
As
co
nc
in s
olu
tio
n (
ug
/L)
40
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Nano- Magnetite Column Study
100ppb As(V) at3ft/day
No As(V) after 122 days
Column:15%
Fe3O4, Lula soil
As(V) Transport in Soil Column
Feed solution: 100 ug/L As(V), pH 8, 0.02 M IS
00.10.20.30.40.50.60.70.8
0 50 100 150 200Time (days)
As
Co
nc
. (C
/Co
)
PredictedObserved
41
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Nano-magnetite Column
42
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Arsenic Removal with Magnetite NPs
0
~ 3
Periodic
14
Backwash Frequency
(day)
(7.5 to 75 )2
est.
0.014
(0.003) est.
0.003
Efficiency1
1.1
4328.13
2.883
Waste to dispose of
kg (1 yr)3
100.09Nano-
magnetite
No Removal of Toxic As(III)3Ion Exchange
0.002360.7Activated Neutralized
Red Mud [As(III)]
3.80.24Alumina + Metal
Oxide
1 gram treats ____
L water
Sorbent (kg)/ month
Material
Enormous sorption capacity Amenable for magnetic separation Cost-effective ($3 to $6 per year per family). InterferencesImplementationApplication to other contaminants
2g 11.7 nm Magnetite
1 gal
Magnet
43
Lets start with some applications.
As you know, Mason and Vicki are working to develop a novel approach to remove arsenic from drinking water using magnetite nanoparticles that are not only superior sorbents with minimal bleed-off potential, but are also amenable for magnetic separation.
This could therefore result in a cost-effective treatment system that could be used at the household-level to alleviate arsenic poisoning in many areas of the world that. Clorox who makes Britta filters has shown a lot of interest.
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Conclusions• Sulfate, organic matter, silica, bicarbonate
have intermediate to large effect on adsorption
• Ca, Mg, K, Trace Metals have little to insignificant effect on adsorption
• Arsenic concentration < 10μg/L in a minute by adding iron salts and magnetite nanoparticles
• Successful field test• Inhibition of arsenic removal and iron oxide
formation in the presence of citrate 44
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Acknowledgement
• Funding of this project is from the Center for Biological and Environmental Nanotechnology (CBEN) at Rice University, NSF, and EPA STAR nanotechnology grant
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Shas MattigodShas Mattigod
Pacific Northwest National LaboratoryPacific Northwest National LaboratoryRichland, WashingtonRichland, Washington
NIEHS/EPA Nanotechnology & Superfund NIEHS/EPA Nanotechnology & Superfund February 13, 2007February 13, 200746
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Functionalized Ceramic Functionalized Ceramic NanoporousNanoporous SorbentsSorbents
1. Introduction
2. Nanoporous SorbentsSubstrate SynthesisMonolayer Functionalization process (SAMMS)Host design for molecular recognition
3. Performance – SAMMS (Self Assembled Monolayerson Mesoporous Supports)thiol SAMMSCu-EDA SAMMSHOPO SAMMS
4. Treatment costs & waste form stability
5. Potential Applications & Commercialization
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NanoscienceNanoscience & Technology& TechnologyNanoparticles Nanoporous
MaterialsSurface Area (m2/g) 10 - 100 600 - 1000Pore Size (nm) -- 2 - 40Particle Size (nm) <100 5 x 103 – 2 x 105
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Why Why NanoporousNanoporous Sorbents?Sorbents?
Technology Needppb – ppt treatment levels
Large surface area - controlled pore sizeDense packed functionalityHigh contaminant loadingEnhanced adsorption kinetics
Particle size: 5 – 120 μmSilt and sand size material (non toxic)Easier to fabricate engineered forms(vs nanoparticles)
Silica based substrateInexpensive to produceEnvironmentally compatible & stable 49
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Inverse
Cubic Inverse
Hexagonal
Inverse Cylindrical Micelles
Microemulsion Domain
Cylindrical
Spherical
Hexagonal
Surfactant
Water Oil
Inverse Spherical
Cubic Lamellar
SurfactantSurfactant--OilOil--Water Phase Diagram:Water Phase Diagram:Template for Template for NanoporousNanoporous Silica Substrate SynthesisSilica Substrate Synthesis
50
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Surfactants
R-N+-(CH3)3X-
MicellesSol-Gel
TemplateRemoval
Nanoporous Ceramic Substrate SynthesisNanoporousNanoporous Ceramic Substrate SynthesisCeramic Substrate Synthesis
51
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Large surface area ~600 - 1000 m2/g
Controlled pore channels 1.5 - 40 nm
~5 – 9 grams
NanoporusNanoporus Ceramic SubstrateCeramic Substrate
52
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US Patents # 6326326, 65312246733835, 6753038
The novel hybrid material (SAMMS) - formed by attaching highly organized functional molecules to ordered nanoporous supports
SAMMS SAMMS ––Self Assembled Self Assembled MonolayersMonolayerson on MesoporousMesoporous SilicaSilica
53
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SAMMS SAMMS --Tailored Surface ChemistryTailored Surface ChemistryHost Design for Molecular RecognitionHost Design for Molecular Recognition
H He
Li Be B C N O F NeNa Mg Al Si P S Cl ArK Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt Uun Uuu Uub 113 Uuq 115 117
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Chemistry of Materials 1999, 11, 2148-2154J. Physical. Chem. B. 2001, 105, 6337-6346.J. Synchrotron Radiation, 2001, 8, 922-924
Cu-EDA
OOSi
SH
OOSi
SH
HO OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OHOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
HO OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OOSi
SH
OHOSi
SH
OOSi
SH
OHOSi
SH
Science, 1997, 276, 923-926.J. Synchrotron Radiation, 1999, 6, 633-635Sep. Sci. & Technol. 1999, 3411, 2329-2345Mat. Tech. Adv. Perf. Mat. 1999, 14, 183-193Surf. Sci. & Catalysis, 2000, 105, 729-738.Radiochimica Acta 2003
thiol
SiO2
Si
O
O O
NH
O
N
HO
O
3,2 HOPO
CH3
HOPO
Env. Sci & Tech. 2005, 39, 1324-1331
Cu-FC-EDACs
Env. Sci & Tech. 2001, 35(19), 3962-3966
54
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0
100
200
300
400
500
600
700
0 100 200 300
Hg Equil. Conc (ppm)
Hg Loading (mg/g)
ThiolThiol--SAMMSSAMMSTMTM Adsorption of Hg SpeciesAdsorption of Hg Species
HgOH+
Hg(OH)20
Hg(Cl)20
CH3Hg+
(CH3Hg)2OH+
55
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SAMMSSAMMSTM TM –– Hg AdsorptionHg AdsorptionIonic Strength & pH EffectsIonic Strength & pH Effects
4
5
6
7
8
9
10
1.0E+06 1.0E+07 1.0E+08
Kd (ml/g)
pH (SU)
0.0
1.0
2.0
3.0
4.0
Ion. Str (M)
56
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Thiol SAMMSThiol SAMMSTM TM Hg Adsorption: Cation EffectsHg Adsorption: Cation Effects
1.0E+04
1.0E+05
1.0E+06
1.0E+07
1.0E+08
4 7
Kd (ml/g)
Na (100 mM)
Na (100 mM), Ca Cu(II), Fe(II), Pb (0.1mM each)
Na (100 mM), Ca, Cd, Cu(II), Fe(II), Ni, Pb, Zn (0.1 mM each)
pH (SU)
57
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1.E+05
1.E+06
1.E+07
Cl CO3 SO4 PO4
Ligands (0.5 mM)
Kd (ml/g)
pH 4.0
pH 7.0
Thiol SAMMSThiol SAMMSTM TM Hg Adsorption: Ligand EffectHg Adsorption: Ligand Effect
Hg: 0.1mMHgCl2
0
Hg(OH)20
HgHCO3+ HgOH+Hg2+HgCO3
0
Hg(OH)20
HgOH+Hg2+
Hg(OH)20HgOHCl0
HgCl20
Hg(OH)20
Hg(OH)20
pH 4 pH 7
Cl
CO3
SO4PO4
58
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0
2
4
6
8
10
0 100 200 300 400 500
Time (min)
Hg Conc. (ppm)
Thiol SAMMSThiol SAMMSTM TM -- Hg Adsorption KineticsHg Adsorption Kinetics
GT-73
thiol SAMMS
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Bonding Mechanism: thiol – Hg2+ IonBonding Mechanism: thiol Bonding Mechanism: thiol –– HgHg2+2+ IonIon
A graphic of self-assembled monolayer within the nanopores of the silica substrate The monolayer consists of tris-methoxy mercaptopropylsilanemolecules crosslinked and anchored into the pore surface. The yellow spheres represent the thiol functionality
Bidentate bonding of Hg to thiolfunctionalitiesBond Length: 2.39 – 2.41 ÅJ. Sync. Radiation 1999, 6, 633 - 635
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y = 2.1644x2 - 12.405x + 18.296
R2 = 0.9685
0.0
2.0
4.0
6.0
8.0
2.5 3.0 3.5 4.0 4.5
Misono Softness Parameter
Ads.(meq/g)
Adsorption Adsorption vsvs MSP MSP -- thiolthiol SAMMSSAMMS
Cu(II)Cd Pb
Ag
Hg
INORG. CHEM. COMM (1): 96-98 2006 61
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0.1
1
10
100
1000
580 590 600 610 620
Hg Loading (mg/kg)
Hg conc (ppb)
EPA Limit 200 ppb
ThiolThiol--SAMMS SAMMS –– Waste Form StabilityWaste Form StabilityTCLP TestTCLP Test
62
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Mercury RemovalPreliminary Cost Comparison
Mercury RemovalMercury RemovalPreliminary Cost ComparisonPreliminary Cost Comparison
$10,000
$100,000
$1,000,000
$10,000,000
SAMMS Resin GAC
63
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CuEDA - SAMMSCuEDACuEDA -- SAMMSSAMMS
64
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Adsorption Adsorption -- CrOCrO44 & AsO& AsO44 CuEDACuEDA--SAMMSSAMMS
y = 0.0066x + 0.3108
R2 = 0.9478
y = 0.0083x + 0.0325
R2 = 0.9985
0.0
1.0
2.0
3.0
4.0
5.0
6.0
0 200 400 600 800
Equil. Conc (mg/L)
C/(x/m) g/L
AsO4
CrO4
65
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Arsenic (V) Adsorption KineticsArsenic (V) Adsorption KineticsCu EDA SAMMSCu EDA SAMMS
0
50
100
150
200
0 100 200 300 400 500
Time (min)
As (V)Conc. (ppb)
66
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Cu Coordination:Cu Coordination:OctahedralOctahedral
Cu(EDA) ComplexCu(EDA) ComplexLog KLog K1,2,31,2,3 10.7510.75
9.289.28--1.001.00
Bonding Mechanism: CuEDA - MO4- IonBonding Mechanism: Bonding Mechanism: CuEDACuEDA -- MOMO44-- IonIon
Cu coordination: Cu coordination: trigonaltrigonal bipyramidbipyramid
AsAs--O bond 1.71 O bond 1.71 ÅÅ
Kelly et al. 2001. Kelly et al. 2001. PhyPhy. . ChemChem B,B, 27: 633727: 6337--6363
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Actinide Binding SAMMSActinide Binding SAMMSActinide Binding SAMMS
HydroxypyridonatesHydroxypyridonates (HOPO) (HOPO) -- selectively bind actinidesselectively bind actinides
Need for actinide separation Need for actinide separation from nuclear wastesfrom nuclear wastes
HOPO SAMMS HOPO SAMMS –– superior class superior class of actinide of actinide sorbentssorbents
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Actinide Adsorption : 3,2-HOPO SAMMSActinide AdsorptionActinide Adsorption : : 3,23,2--HOPO SAMMSHOPO SAMMS
1.0E+04 1.0E+05 1.0E+06 1.0E+07
Distribution Coefficient (Kd: ml/g)
Np(V)
Pu(IV)
U(VI)
Lin et. Al. ES&T 2005, 39:1332Lin et. Al. ES&T 2005, 39:1332--13371337
69
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237237Np Adsorption Np Adsorption –– HOPO SAMMSHOPO SAMMS
0.0E+00
1.0E+06
2.0E+06
3.0E+06
4.0E+06
5.0E+06
0 25 50 75 100
Equilibrium Activity (pCi/mL)
237Np Adsorbed
(pCi/g)
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Molecular Model - HOPO SAMMS binding NpO2+Molecular Model Molecular Model -- HOPO SAMMS binding NpOHOPO SAMMS binding NpO22++
VorpagelVorpagel 20042004LANL2ZP ECP Basis Set ModelingLANL2ZP ECP Basis Set Modeling
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SAMMSSAMMSTMTM Performance SummaryPerformance Summary
Adsorption not affectedMacro/trace cations, anions, Organics
pH Range ~3 – 13 SU
Highly Stable Waste FormLow disposal cost
Loading ~ 40 – 600 mg/gFast Kinetics ~99.9% - 5 min
Very High Specificity Kd ~ 103 – 108 ml/g
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SAMMS – ApplicationsSAMMS SAMMS –– ApplicationsApplications
Crude OilCrude Oil
Produced WaterProduced WaterWaste WaterWaste Water
SensorsSensors
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SAMMSSAMMSTMTM CommercializationCommercialization
50 L Batch Production 50 L Batch Production ––Green ChemistryGreen ChemistryThiolThiol functionalizationfunctionalization using using supercritical COsupercritical CO22
SAMMS patents SAMMS patents LicenceeLicenceeChattanooga, TNChattanooga, TN
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SAMMSSAMMSTMTM CommercializationCommercialization
Engineered FormsEngineered FormsPerry Equipment CorporationPerry Equipment CorporationMineral Wells, TXMineral Wells, TX
Produced waterProduced waterNatural GasNatural GasGas CondensatesGas CondensatesCrude OilCrude Oil
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Next Generation Next Generation NanoporousNanoporous MaterialsMaterials
Nanoporous Metal Phosphates
Hierarchial Pore structured Materials
Targeted Applications
Flue gas Hg removal
Precious metal recovery
Sensors
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Research SupportResearch Support
BattelleBattelle
Pacific Northwest National LaboratoryPacific Northwest National Laboratory
United States Department of EnergyUnited States Department of Energy
Perry Equipment CorporationPerry Equipment Corporation
Steward Environmental SolutionsSteward Environmental Solutions
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