vii
TABLE OF CONTENTS
CHAPTER
TITLE
PAGE
THESIS STATUS DECLARATION
SUPERVISOR’S DECLARATION
1
TITLE PAGE
i
DECLARATION
ii
DEDICATION
iii
ACKNOWLEDGEMENT
iv
ABSTRACT
v
ABSTRAK
vi
TABLE OF CONTENTS
vii
LIST OF TABLES
xii
LIST OF FIGURES
xvi
LIST OF SYMBOLS
xxii
LIST OF ABBREVIATIONS
xxiii
LIST OF APPENDICIES
xxv
INTRODUCTION
1
1.1
Research Background
1
1.1.1
2
1.2
1.3
Water Purification
Heavy Metals
5
1.2.1
5
Pollution and Remediation Approaches
Activated Carbon
13
1.3.1
Historical Aspect of Carbon
14
1.3.2
Structure of Activated Carbon
15
viii
1.3.2.1
1.3.3
Surface Functional Groups
16
Preparation
20
1.3.3.1
23
Processing of Lignocellulosic
Materials
1.3.3.2
Utilization of Oil Palm and
27
Coconut Shells as Carbon
Precursor
1.4
Adsorption of Metal Ions onto Activated Carbon
30
1.5
Adsorption Equilibrium Models
41
1.5.1
Langmuir Adsorption Model
42
1.5.2
Freundlich Adsorption Model
43
1.6
1.7
2
Aims and Objectives
45
1.6.1
46
Objectives
Scope and Limitations
46
MATERIALS AND METHODS
47
2.1
Chemicals and Reagents
47
2.2
Instruments
48
2.3
Preparation of Activated Carbon
48
2.3.1
Raw Material Preparation
49
2.3.2
Activation and Washing
50
2.4
Modification of Activated Carbon
51
2.5
Characterization of Activated and Composite
53
Carbon
2.5.1
Yield Determination
54
2.5.2
Surface Porosity Characterization (N2
54
Adsorption-Desorption)
2.5.3
Surface Morphology (SEM and EDX)
55
2.5.4
Fourier Transform Infrared Spectroscopy
55
(FTIR)
2.5.5
Boehm’s Titration
55
2.5.6
Determination of pH at Point of Zero
56
Charge (pHZPC)
ix
2.6
2.5.7
Thermogravimetric Analysis (TGA)
57
2.5.8
Leaching Test of Fe
57
Adsorption Studies
58
2.6.1
Test and Standard Metal Ion Solutions
58
2.6.2
Adsorption Equilibrium Studies: Metal
60
Cations
2.6.2.1
Selection of Prepared Activated
60
Carbons for Metal Cations
2.6.2.2
Single Solute Adsorption
61
2.6.2.3
Binary Solute Adsorption
62
2.6.2.4
Ternary Solute Adsorption
62
2.6.2.5
Reuse of Cation-Exhausted
62
Activated Carbon
2.6.3
Adsorption Equilibrium Studies: Cr(VI)
63
2.6.4
Adsorption Equilibrium Studies: As(III) and
64
As(V)
2.6.5
Adsorption Dynamics: Cu(II), Ni(II), Pb(II)
64
and Cr(VI)
2.6.6
Determination and Uptake of Species of
65
Metal/Metalloid
3
RESULTS AND DISCUSSION: ADSORBENT
67
DEVELOPMENT
3.1
Preparation
67
3.1.1
Activated Carbon
67
3.1.2
Carbon-Hydrated Iron Oxide (C-HFO)
68
Composite
3.2 Characterization of Prepared Activated Carbon
3.2.1
69
Surface Porosity and Morphology
70
3.2.1.1
Effect of Precursor Type
72
3.2.1.2
Effect of Pretreatment
72
3.2.1.3
Effect of Impregnation Condition
76
3.2.1.4
Effect of Precursor Size
78
x
3.2.1.5
3.2.2
Effect of Activation Temperature
80
Surface Functional Groups
82
3.2.2.1
83
Fourier Transform Infrared (FTIR)
Spectroscopy
3.2.2.2
Boehm’s Titration
84
3.2.2.3
Determination of pHZPC of
86
activated carbon (pH Drift
Method)
3.2.3
Thermogravimetric Analysis (TGA) of
87
activated carbon
4
3.3
Characterization of C-HFO Composites
87
3.4
Leaching Test of Fe from C-HFO Composites
92
RESULTS AND DISCUSSION: APPLICATION OF
94
ADSORBENTS
4.1
4.2
Application of Prepared Adsorbents
94
4.1.1
95
Selection of Prepared Activated Carbon
Adsorption Equilibria
97
4.2.1
98
Single Solute Adsorption Equilibria: Metal
Cations
4.2.1.1
Single Solute Adsorption
98
Equilibria: Cu(II)
4.2.1.2
Single Solute Adsorption
103
Equilibria: Ni(II)
4.2.1.3
Single Solute Adsorption
107
Equilibria: Zn(II)
4.2.1.4
Single Solute Adsorption
110
Equilibria: Pb(II)
4.2.2
Binary Solute Adsorption Equilibria:
115
Competitive Adsorption of Cu(II) and
Ca(II) (Cu-Ca) and Evaluation of
Mechanism
4.2.3
Ternary Solute Adsorption Equilibria:
122
xi
Competitive Adsorption of Cu(II), Ni(II)
and Pb(II) (Cu-Ni-Pb)
4.2.4
Reuse of Cation-Exhausted Activated
128
Carbon
4.2.5
Adsorption Studies: Cr(VI)
130
4.2.5.1
Selection of Prepared Adsorbents
130
4.2.5.2
The Effect of pH
132
4.2.5.3
Effect of Initial Concentration and
134
Data Fitting to Models
4.2.6
4.3
Adsorption Studies: Arsenic
137
Adsorption Dynamics
142
4.3.1
144
Adsorption Dynamics of Cu(II) on PSW-Pad-500
4.3.2
Adsorption Dynamics of Ni(II), Pb(II) and
146
Cr(VI) on PSW-P-ad-500
4.4
5
Summary of Thesis
150
CONCLUSIONS AND SUGGESTIONS FOR
152
FUTURE STUDY
5.1
Conclusions
152
5.2
Problems Encountered in Present Study
155
5.3
Recommendations for Further Studies
156
REFERENCES
157
APPENDICES A - L
166
xii
LIST OF TABLES
TABLE NO.
1.1
TITLE
A survey of recent literatures on the production of
PAGE
23
activated carbons from various lignocellulosic precursors
1.2
Proximate analysis of solid oil palm residues (Husain,
29
Zainac and Abdullah, 2002)
1.3
Ultimate analysis of solid oil palm residues (Mahila et al.,
30
2001)
1.4
Proximate and ultimate analyses of coconut shell
30
(Banerjee, et al.,1976)
2.1
Preparation variables of various activated carbons activated
51
either in a muffle (M) or in a tube furnace (T)
2.2
The operating parameters of FAAS in the determination of
66
metal cations
3.1
The contents of Fe, oxygen, Na/Ca and C in the prepared
69
composites and in their parent activated carbons
3.2
Yield, BET surface area, average pore width, total pore
71
volume and pore-types of various activated carbons
3.3
Contents of phosphorous (P) in some of the selected
71
activated carbons as determined by EDX
3.4
Base neutralization capacity and quantification of acidic
85
groups on surfaces of some of the prepared activated
carbons by Boehm’s titration method
3.5
The pHZPC of some activated carbons obtained from pH
86
drift method
3.6
The proximate analysis of activated carbons using TGA
87
xiii
technique
3.7
The BET surface area, average pore width, total pore
88
volume and pore-types of C-HFO composites and their
parent activated carbons
3.8
Properties of Virgin GAC and Fe-GAC obtained from
92
Norit Americas Inc. (Reed, Vaughan and Jiang, 2000)
4.1
Cu(II) uptake capacity of various activated carbons in a
96
single solute solution while initial solution (adsorbate)
concentration and pH were kept constant at 292 ± 6 mg.L-1
and 6 respectively with a constant adsorbent concentration
of 2 g.L-1
4.2
Langmuir and Freundlich model parameters for the
101
adsorption of Cu(II) in single-solute solution while initial
concentrations were varied, < 5 - < 120 mg.L-1
4.3
Langmuir and Freundlich model parameters for the
105
adsorption of Ni(II) by various activated carbons at initial
pH 5 while initial concentrations were varied from 6 to 227
mg.L-1 and adsorbent concentration was kept constant at 2
g.L-1
4.4
The initial and equilibrium concentrations, and fractions
107
removal of Ni(II) by various activated carbons in the low
concentration solution at a constant initial pH 5
4.5
Langmuir model parameters for the adsorption of Zn(II) by
110
various activated carbons at initial pH 5 while initial
concentrations were varied from 19 to 310 mg.L-1 and
adsorbent concentration was kept constant at 2 g.L-1
4.6
Langmuir and Freundlich model parameters for the
112
adsorption of Pb(II) at initial pH 5 and at varying
concentrations, < 50 - < 600 mg.L-1
4.7
The initial and equilibrium concentrations, and fractions
removal of Pb(II) by various activated carbons in the low
concentration range at pH 5
113
xiv
4.8
Langmuir and Freundlich parameters for the adsorption of
115
Pb(II) on PSW-P-ad-500 for initial pH 3 at varying
concentrations, 50.6 ± 0.6-583 ± 2 mg.L-1
4.9
The Langmuir model parameters of Cu(II) and Ca(II) for
117
the adsorption in binary solution at an initial pH 5, while
initial concentrations of Cu(II) and Ca(II) were varied as
23.6 ± 0.1 to 117.5 ± 0.7 and 23.8 ± 0.2 to 120 ± 1 mg.L-1
respectively
4.10
Langmuir and Freundlich parameters for the adsorption of
120
Cu(II) on PSW-P-ad-500 at a constant initial pH 4.5 while
initial solution concentrations were varied from < 25
to < 700 mg.L-1 keeping adsorbent concentration 2 g.L-1
4.11
The Langmuir model parameters of Cu(II) and Ca(II) for
122
the adsorption in binary solution at initial pH 3 while
initial concentrations of Cu(II) and Ca(II) were varied as
26-151 and 20-109 mg.L-1 mg.L-1 respectively
4.12
Langmuir and Freundlich model parameters for the
124
isotherms of Ni(II), Pb(II) in ternary and Cu(II) in single
and ternary solutes solutions at initial pH 5
4.13
The initial and equilibrium concentrations, adsorption
125
capacities and fractions removal of Cu(II), Ni(II), Pb(II) in
the single and ternary solutes solutions by the best-selected
carbon, PSW-P-ad-500 at initial pH 5 and at adsorbent
concentration of 2 g.L-1
4.14
Langmuir model parameters for the adsorption-desorption
130
of Cu(II)
4.15
The adsorption capacities of various adsorbents in the
132
removal of Cr(VI) while initial pH was obtained without
adjustment as 4.79 and adsorbent concentration was
maintained as 2 g.L-1
4.16
Langmuir and Freundlich model parameters for the
adsorption of Cr(VI) on PSW-P-ad-500 while initial
concentrations were varied from 40 - < 200 mg.L-1 at an
136
xv
optimum pH 3, keeping adsorbent concentration constant
at 2 g.L-1
4.17
The initial and equilibrium concentrations, and fractions
136
removal of Cr(VI) by various activated carbons in the low
concentration at an optimum pH 3
4.18
Aqueous and solid phase equilibrium concentration of
139
adsorbents (adsorption capacity) while adsorbate
concentration was 1 mg.L-1, pH 7 and adsorbent
concentration 0.2 g.L-1 (Reed, Vaughan and Jiang, 2000)
4.19
Experimental adsorption equilibrium capacity, qe and
146
kinetic model parameters for the adsorption of Cu(II) at
constant initial concentration, < 50 mg.L-1 and at pH 5,
while contact time was varied from 0.5 to 72 h
4.20
Experimental adsorption equilibrium capacity, qe and
kinetic model parameters for the adsorption of Ni(II),
Pb(II) and Cr(VI)
147
xvi
LIST OF FIGURES
FIGURE NO.
1.1
TITLE
The periodic table showing classification of metals based
PAGE
11
on Lewis acidity as: Class A-hard metals (black), Class
B-soft metals (light grey), Class AB-borderline (dark
grey) (IUPAC, 2002)
1.2
Structures of carboxyl, phenolic hydroxyl and quinone
18
type carbonyl groups
1.3
Structures of lactones, acid anhydrides and cyclic
18
peroxide
1.4
A cross section of masocarp of oil palm fruit bunch
28
showing fibre, shell, kernel and pericarp
1.5
Process flow diagram of palm oil extraction showing the
29
production of crude oil and wastages such as shells,
kernel and fibres
2.1
A flow diagram of activated carbon preparation
49
2.2
A flow diagram of modification of activated carbons
52
3.1
N2 adsorption-desorption isotherms of various activated
70
carbons prepared from oil palm and coconut shell
precursors under various process conditions
3.2
N2 adsorption-desorption isotherms of activated carbons
73
derived from oil palm (A) and coconut shell (B)
precursors
3.3
Yield of various activated carbons as a function of
precursor pretreatment such as non-pretreated (NP),
74
xvii
H2SO4 pretreated (SAP) and H3PO4 pretreated (PAP)
conditions
3.4
BET surface area of various activated carbons as a
75
function of precursor pretreatment such as non-pretreated
(NP), H2SO4 pretreated (SAP) and H3PO4 pretreated
(PAP) conditions
3.5
BET surface areas of various activated carbons derived
77
from different charge states such as wet (PSW-P-500),
apparently/semi-dried (PSW-P-ad-500) and completely
dried (PSW-P-ed-450)
3.6
Total pore volumes of activated carbons derived from
77
different charge states, as wet (PSW-P-500), semi-dried
(PSW-P-ad-500) and dried (PSW-P-ed-450)
3.7
SEM micrograph of an activated carbon obtained from
78
semi-dried feedstock of oil palm shell precursor, namely
PSW-P-ad-500
3.8
N2 adsorption-desorption isotherms of two activated
79
carbons, derived from smaller (1.18-0.6 mm) and larger
(2.36-1.18 mm) particle sizes, namely PSWfg-P-450 and
PSW-P-ed-450
3.9
The development of surface areas of various activated
80
carbons prepared under different activation temperatures
3.10
FTIR spectrums of some of the prepared activated
83
carbons, namely, PSW-P-500, CPW-P-500 and PSW-Pad-500
3.11
Graphs of equilibrated pH (pHf) vs. initial pH (pHi) by
86
some of the prepared activated carbons for determining
the pHZPC from the crossover point
3.12
SEM micrographs of composites of C-HFO-1 (A) and C-
89
HFOCa-1 (B) obtained from parent activated carbon
PSW-P-500 using different bases, such as NaOH and
Ca(OH)2
3.13
SEM micrographs of a composite, C-HFO-2 obtained
90
xviii
from parent activated carbon CPW-P-500 while
magnification factor is different as 200X (A) and 800X
(B)
3.14
SEM micrographs of C-HFO-3 obtained from parent
91
activated carbon PSW-P-ad-500 while magnification
factor is different as 250X (A) and 1200X (B)
4.1
Langmuir adsorption isotherms of Cu(II) at initial pH 3
99
(A) and pH 5 (B) by various activated carbons while
initial solution concentrations were varied from < 5 to
<120 mg.L-1
4.2
Langmuir adsorption isotherms of Cu(II) by prepared
100
activated carbons for initial pH 3 (A) and pH 5 (B) and
by a commercial activated carbon for initial pH 3 and pH
5 (C) while initial concentrations were varied, < 5 - < 120
mg.L-1
4.3
Freundlich adsorption isotherms of Cu(II) at pH 3 (A)
101
and at pH 5 (B) while initial solution concentrations of
Cu(II) were varied, < 5 - < 120 mg.L-1
4.4
Langmuir (A, B, C) and Freundlich (D) adsorption
104
isotherms of Ni(II) at initial pH 5 by various activated
carbons while initial solution concentrations were varied
as 6 - 227 mg.L-1
4.5
Langmuir non-linear (A) and linear (B) isotherms of
108
Zn(II) by CAC at initial pH 5 while solution
concentrations were varied, 19 - 250 mg.L-1
4.6
Langmuir non-linear isotherms of Zn(II) at initial pH 5 by
109
prepared activated carbons, PSW-P-500 (A), CPW-P-500
(B) and PSW-P-ad-500 (C) while initial solution
concentrations were varied, 19 – 310 mg.L-1
4.7
Langmuir linear isotherms of Zn(II) at initial pH 5 by
various prepared activated carbons while initial solution
concentrations were varied from 19 to 310 mg.L-1
110
xix
4.8
Langmuir non-linear (A) and linear (B and C) adsorption
111
isotherms of Pb(II) at initial pH 5 by various activated
carbons while initial concentrations were varied as < 50 < 600 mg.L-1
4.9
Freundlich adsorption isotherms of Pb(II) at initial pH 5
112
by various activated carbons while initial concentrations
were varied as < 50 - < 600 mg.L-1
4.10
Langmuir non-linear (A) and linear (B) adsorption
114
isotherms of Pb(II) at initial pH 3 by the best-selected
activated carbon, PSW-P-ad-500 while initial solution
concentrations were varied from 50.6 ± 0.6 to 583 ± 2
mg.L-1
4.11
Freundlich adsorption isotherms of Pb(II) at initial pH 3
115
by activated carbon, PSW-P-ad-500 while initial solution
concentrations were varied from 50.6 ± 0.6 to 583 ± 2
mg.L-1
4.12
Langmuir non-linear and linear isotherms of Cu(II) (A
116
and B) and Ca(II) (A and C) while Cu(II) ions were
adsorbed from single (Cu), binary (Ca-Cu) and ternary
(Cu-Ni-Pb) solutions and Ca(II) from binary solution
(Ca-Cu) by PSW-P-ad-500 at initial pH 5 and at varying
initial concentrations, < 25 - ≤ 120.mg.L-1
4.13
The proposed interactions of Cu(II) and Ca(II) cations
118
(Lewis acids) onto the surfaces of activated carbon where
SO− and SOH (Lewis bases) represent the deprotonated
surface functional groups on activated carbon. The
vertical bars are depicted as solution-solid interface
4.14
Langmuir non-linear (A), linear (B) and Freundlich (C)
119
isotherms of Cu(II) by the carbon PSW-P-ad-500 at
constant initial pH 4.5 while initial solution
concentrations were varied from < 25 to < 700 mg.L-1
keeping adsorbent concentration constant at 2 g.L-1
4.15
Langmuir non-linear (A) and linear (B and C) isotherms
121
xx
of Cu(II) and Ca(II) for the adsorption in binary solute
solution while concentration of Cu(II) and Ca(II) were
varied as 26-151 and 20-109 mg.L-1 respectively keeping
initial pH and adsorbent concentration constant, at pH 3
and 2 g.L-1 respectively
4.16
Langmuir non-linear (A), linear (B) and Freundlich (C)
123
isotherms of ternary solute, Cu(II), Ni(II) and Pb(II), by
the best selected carbon, PSW-P-ad-500 at initial pH 5,
while their initial concentrations were varied as < 25 ≤ 600 mg.L-1. (Ni samples were analysed for initial
concentration range, < 25 to 305 ± 2 mg.L-1)
4.17
Langmuir non-linear and linear adsorption-desorption
129
isotherms of Cu(II), while adsorbed at varying
concentration, < 25 to < 700 mg.L-1
4.18
Adsorption capacity of Cr(VI) by various selected
133
adsorbents while pH were varied from 3 to 8 keeping
initial concentration constant at about 40 mg.L-1
4.19
Langmuir non-linear (A), Linear (B) and Freundlich (C)
135
adsorption isotherms of Cr(VI) by activated carbons,
CAC and PSW-P-ad-500, at initial pH 3 while initial
concentrations were varied from 40 - < 200 mg.L-1
4.20
Adsorption equilibrium capacities of a HFO composite
138
and its counter activated carbon for the species of As(V)
and As(III), while adsorptions were carried out in the
solutions of As(V) and As(III) with constant initial
concentrations, 1.641 and 2.170 mg.L-1 and with constant
initial pH, at 5.5 and 7.6 respectively
4.21
An illustration of selective bond formation of dispersed
141
hydrated iron oxide with As(V) and As(III) species in
aqueous phase predominantly through Lewis acid-base
interaction
4.22
Graph to check kinetics data of Cu(II) with first order
kinetic model
144
xxi
4.23
Graph of pseudo-second order kinetic model for the
145
adsorption of Cu(II) at constant initial concentration, < 50
mg.L-1 and at pH 5
4.24
A graph of adsorption capacity vs. contact time for the
145
adsorption of Cu(II) at constant initial concentration, < 50
mg.L-1 and at pH 5
4.25
Graphs of pseudo-second order kinetic model for the
147
adsorptions of Ni(II), Pb(II) and Cr(VI) at constant initial
concentrations, < 45, 95 ± 1 and 77 ± 1 mg.L-1
respectively, while the initial pH of solutions of Ni(II)
and Pb(II) were adjusted to 5 and that of Cr(VI) to 3
4.26
Graphs of adsorption capacities vs. contact time for the
148
adsorption of Ni(II) (A), Pb(II) (B) and Cr(VI) (C)
4.27
A comparison in the rate constants of various metal ions
149
for the adsorption onto acid activated carbon, PSW-P-ad500
4.28
A comparison in adsorption capacities (qe) of various
metal ions while qe obtained from adsorption equilibrium
data for kinetics studies for the adsorption onto acid
activated carbon, PSW-P-ad-500
150
xxii
LIST OF SYMBOLS
°C
-
Degree Celsius
C0
-
Initial concentration
Ce
-
Equilibrium concentration
cm
-
Centi meter
dm
-
Deci meter
g
-
Gram
L
-
Liter
m
-
Meter
M
-
Molar
mA
-
Mili ampere
meq
-
Mili equivalent
mg
-
Mili gram
min
-
Minute
mL
-
Mili Liter
mm
-
Mili meter
mM
-
Mili Molar
nm
-
Nano meter
q or qt
-
Metal uptake at any time, t
qe
-
Metal uptake at equilibrium
t
-
Tonne
y
-
year
Å
-
Angstrom
µg
-
Micro gram
µm
-
Micro meter
µmol
-
Micro mole
xxiii
LIST OF ABBREVIATIONS
AAS
-
Atomic absorption spectrophotometer
Av
-
Average
B.C.
-
Before Christ
BET
-
Brunauer, Emmett and Teller
CAC
-
Commercial activated carbon
DDW
-
Distilled deionized water
Dia
-
Diameter
DPC
-
1,5-Diphenylcarbazide
EDL
-
Electric double layer
EDX
-
Energy dispersive X-ray analysis
EFB
-
Empty fruit bunches
EPA
-
Environment Protection Agency
Et
-
Ethyl
FAAS
-
Flame atomic absorption spectroscopy
FTIR
-
Fourier transform infrared spectrophotometer
GAC
-
Granular activated carbon
h
-
hour
HFO
-
Hydrated iron oxide
HSAB
-
Hard and Soft Acids and Bases
ICP-MS
-
Inducedly coupled plasma mass spectrophotometer
IUPAC
-
International Union of Pure and Applied Chemistry
Max
-
Maximum
MOX
-
Malaysian Oxygen
NOM
-
Naturally occurring organic matter
PAC
-
Powered activated carbon
xxiv
QC
-
Quality control
rpm
-
Revolution per minute
RSD
-
Relative standard deviation
SCF
-
Surface complex formation
SD
-
Standard deviation
SEM
-
Scanning electron microscope
SOC
-
Synthetic organic chemicals
SOCs
-
Synthetic organic compounds
TGA
-
Thermogravimetric analysis
USA
-
United States of America
USEPA
-
United States Environment Protection Agency
UV
-
Ultra violet
VOCs
-
Volatile organic compounds
WHO
-
World Health Organization
xxv
LIST OF APPENDICES
APPENDIX
A
TITLE
National Drinking Water Quality
PAGE
166
Standards, 2000 of Malaysia for some
species of metals and metalloids
B
EDX Spectrums of Some Selected
167
Activated and Modified Carbons
C
Summary Report of N2 Adsorption-
170
Desorption Data and BJH Pore size
distribution Graph
D
FTIR Spectrums of Some of the Selected
174
Activated Carbons
E
Quantification of Acidic Groups on the
175
Surface of Some Selected Activated
Carbons as meq Base per Gram Carbon
F
TGA Thermograms of Some of the
176
Selected Activated Carbons
G
FAAS Determined Fe Content in Samples
186
of Leached Water Contacted with C-HFO-1
Composite Adsorbent at pH 4.5
H
FAAS Determined Adsorption Equilibrium
Data of Various Metal Cations in Single,
Binary and Ternary Solutes Solutions by
Various Activated Carbons at Varying
Initial Concentration and pH
187
xxvi
I
UV-Vis Spectrophotometer Determined
203
Adsorption Equilibrium Data of Cr(VI) in
Single Solute Solution By Various
Activated Carbons and C-HFO Composite
Adsorbents
J
ICP-MS Determined Adsorption
208
Equilibrium Data of As(III) and As(V) for
the Adsorption in a Single Point Initial
Concentration By a Typical Prepared
Activated Carbon and its modified ones,
namely, PSW-P-500 and C-HFO-1
respectively
K
Adsorption Kinetics Data of Cu(II), Ni(II),
209
Pb(II) and Cr(VI)
L
Presented Papers and Expected
Publications from This Study
212