Payal phd slides final1 [autosaved]

SYNTHESIS AND CHARACTERIZATION OF ZEOLITE
FROM COAL FLY ASH AND ITS APPLICATION IN
REMOVAL OF INORGANIC AND ORGANIC
POLLUTANTS FROM WASTEWATER
SUPERVISOR PRESENTED BY
Dr. M. K. DWIVEDI PAYAL JAIN
GOVT. HOLKAR SCIENCE COLLEGE INDORE

INTRODUCTION
 Coal fly ash (CFA) is a micro spherical particulate by- product of combustion of coal. It is primarily composed of
amorphous aluminosilicate and other crystalline minerals like mullite, quartz, haematite and magnetite [1].
Combustion of coal in thermal power stations produces over 1200 million tonnes of fly ash worldwide annually [2].
The disposal of such huge quantities of ash has become a problem [3].
 Several approaches have been done for proper utilization of fly ash, for reduction of cost of disposal or for
minimizing environmental impact. The production of zeolites is one of the potential applications of CFA. The
aluminosilicate glass in CFA is a readily available source of Si and Al for zeolite synthesis so as to obtain high value
industrial products with environmental technological utilization [4].
 Zeolites are three-dimensional, microporous, crystalline solids with well-defined structures that contain aluminium,
silicon, and oxygen in their regular framework; cations and water are located in the pores. Compositionally, zeolites
are similar to clay minerals. More specifically, both are alumino-silicates. They differ, however, in their crystalline
structure[5].
 Due to rapid growth of industrialization and urbanization with technological advancement, the existing water
resources are becoming increasingly contaminated by discharge of effluent containing organics, colour, heavy
metals and other contaminants. It is discharged into water bodies from mining operation, metal plating and
tanneries

 Heavy metal pollutant with density five times of water[6] has emerged due to anthropogenic activity which is the
prime cause of pollution, primarily due to mining the metal, smelting, foundries, and other industries that are metal-
based, leaching of metals from different sources such as landfills, waste dumps, excretion, livestock and chicken
manure, runoffs, automobiles and roadworks.
 Heavy metals are potentially hazardous in combined or elemental forms. These are highly soluble in the aquatic
environments and therefore they can be absorbed easily by living organisms.
 Chronic toxicity of Cadmium (Cd) in children includes damages of respiratory, renal, skeletal and cardiovascular systems
as well as development of cancers of the lungs, kidneys, prostate and stomach. The US EPA’s regulatory limit of Cd in
drinking water is 5 ppb or 0.005 parts per million (ppm). The WHO recommended safe limits of Cd in both wastewater
and soils for agriculture is 0.003 ppm[7].
 Exposure to Lead (Pb) can occur through inhalation of contaminated dust particles and aerosols or by ingesting
contaminated food and water. Lead poisoning in humans damages the kidneys, liver, heart, brain, skeleton and the
nervous system The regulatory limit of Pb in drinking water according to US EPA is 15 ppb. The WHO recommended safe
limits of Pb in wastewater and soils used for agriculture are 0.01 and 0.1 ppm respectively[8].

 A wide range of copper toxicities have been observed subsequent to accidental or iatrogenic poisonings or suicide
attempts: hepatic and renal failure, cirrhosis, haemolysis, vomiting, melena, hypotension, cardiovascular collapse,
stupor, and coma. The EPA’s established a limit of copper in drinking water as 1.3 ppm. The WHO recommended safe
limits of Cu in wastewater and soils used for agriculture are 0.025 and 0.1 ppm respectively[8].
 Dyes or colouring substances are considered as one of the significant pollutants and they are stated as ‘visible
pollutant[9]. Textile effluents are major industrial polluters because of high color content, about 15% unfixed dyes
and salts[10].
 Safranin is a popular and most ancient dye used in textile and silk industries , this dye is used to dye food and dessert
coloring, despite the benefits of this dye , but when discharge to the water it causes water pollution and respiratory
diseases skin and digestive tract infections on ingestion[11].
 Hazardous pollutant are difficult to remove by conventional wastewater treatment, Possible methods of their
removal include chemical oxidation, froth flotation, adsorption, and coagulation etc. Among these, adsorption
currently appears to offer the best potential for overall treatment.
 Zeolite being effective and reliable source of adsorption was synthesized from coal fly ash and applied to remove
heavy metals and dye in the thesis work.

The work reported in this thesis deals with the the removal of some heavy metals like Copper, Cadmium, Lead
and a dye Safranin by adsorption on zeolites material prepared from coal fly ash, with the following aims and
objectives:
1. To synthesize and employ zeolite from Coal fly ash by Alkali fusion followed by hydrothermal treatment.
2. To characterize the physio-chemical and textural properties of fly ash and Zeolite such as surface area, XRD,
XRF, FTIR and SEM .
3. To investigate the role of zeolite material in adsorption of dye and heavy metal containing wastewater.
4. To optimize the parameters of contact time, adsorbent dose, pH and initial adsorbate concentration and to
determine the applicability of Freundlich, Langmuir, Temkin, and Dubinin-Radushkevitch approach to
estimate design parameters characterizing the performance of the batch tests.
5. To determine the thermodynamic parameters to know the feasibility of the adsorption process.
6. To investigate the kinetic studies to have an understanding of the mechanistic process of the system.

MATERIALS AND METHODS
Coal fly ash that was collected from H.E.G. Thermal Power Station, Mandideep (Bhopal).
Chemicals used were supplied by Merck, India. The stock solutions were prepared in
deionized water supplied by Rankem. The standard calibration curves of known
concentrations of Safranin was plotted by finding out the absorbance at the characteristic
wavelength of λmax 518 nm and metals concentration was measured by Atomic absorption
Spectrophotometer (Perkin elmer-3100 series).
Safranin

PREPARATION OF ZEOLITE FROM FLY ASH
The direct hydrothermal method was used for the synthesis of zeolites since it is fast,
economic and less involving than the other fusion and microwave methods.
NaOH is added with coal fly ash in different ratios of 1:2, 1:1.5 and 1:1.2 and kept for
fusion at varying temperatures of 350°C,450° C and 550° C for 12 hours.
After this fusion mixtures were washed with double distilled water and agitated for 24
hours on magnetic stirrer to wash off excess of alkali, filtered on Whatmann filter
paper and dried in oven for 12 hours at 110°C and stored in desiccator before use.

PREPARATION OF ZEOLITE FROM FLY ASH

ADSORPTION STUDIES
The adsorption was performed using the batch method. The equilibrium adsorption
uptake and percentage removal of adsorbates from the aqueous solution qe (mg/g)
were calculated using the following relationship:
Amount adsorbed qe =
Co−Ce V
W
………(1)
% Removal qe =
100 Co−Ce
Co
……… (2)
Where, Co is initial adsorbate concentration (mgL-1), Ce is equilibrium adsorbate
concentration (mgL-1), V is the volume of solution (L), W is the mass of adsorbent (g).

Adsorption Isotherms
The equilibrium data obtained in the present study were analyzed using Langmuir[12],
Freundlich[13], Dubinin-Radushkevich[14] and Temkin[15] isotherm models.
The rearranged Langmuir and Freundlich isotherm equations can be described as:
1
qe
=
1
qm
+ (
1
bqm
)(
1
Ce
) .............. (3)
log qe= log Kf +
1
n
log Ce. .............(4)
Where qm and b are the Langmuir constants related to maximum adsorption capacity and
energy of adsorption, respectively. Kf is a Freundlich constant related to the adsorption
capacity (mg/g) and n is an empirical constant.

Adsorption Isotherms….
The Dubinin-Radushkevich and Temkin isotherm models are as follows:
ln qe = ln qm – βE2 …………….(5)
qe =
RT
𝑏𝑇
ln 𝐴T𝐶e ……………(6)
Where β is Dubinin-Radushkevich constant, R is gas constant (8.31 Jmol−1 k−1), T is absolute
temperature, and E is mean adsorption energy (KJ mol-1). bT is Temkin constant which is
related to the heat of sorption (Jmol-1) and AT is Temkin isotherm constant (l g-1)

Thermodynamic Studies
Thermodynamic studies play an important role in understanding the process of
adsorption. This work computes the thermodynamic parameters of Gibbs Free
energy (ΔG0), enthalpy (ΔH0) and entropy (ΔS0) of adsorption by carrying out the dye
adsorption process at 303 K. Thermodynamic parameters can also be evaluated by
using the data obtained from the adsorption isotherms.
log
b2
b1
=
ΔH0
R
[
T2−T1
T1T2
] ……… (7)
ΔG°= - 2.303 RT log b ……… (8)
ΔG° = ΔH° - TΔS° ………(9)
Where, b1 and b2 are Langmuir constants at different temperatures, R ideal gas
constant (8.314 J/mol/K), T1 and T2 are temperatures (K).

SPECIFIC RATE CONSTANT OF ADSORPTION:
The rate constant of adsorption for various adsorbates is determined from the following
first order rate expression given by Lagergren.
log (qe-q)= log qe -
Kad
2.303
t …………. (10)
Where q and qe are amounts of adsorbate adsorbed (mg/g) at time‘t’ and at equilibrium
respectively and Kad is the rate constant for adsorption (min-1). A straight line plot of log (qe-
q) versus t suggested the applicability of Lagergren equation. The rate constant of
adsorption (Kad) was calculated from the slope of the plot.

The pseudo second order (PSO) [16] kinetics model was used to investigate whether chemical reaction at the
adsorption site of zeolite was rate determining. The PSO model is given by:
t
q𝑡
=
1
K2
𝑞2
𝑒
+
t
q𝑒
…………. (11)
Where q𝑡 and q𝑒 are the amount of adsorbate per unit of adsorbent(mgg-1) at time t, and at equilibrium
respectively. K2 (g/mg.min) is the adsorption rate constant. From the slope and intercept of the (t/q𝑡) as a
function of t, K2 and q𝑒 can be obtained.
The Elovich[17] equation is mainly applicable for chemosorption kinetics the equation is often valid for
systems in which the adsorbing surface is heterogenous the model is expressed as
q𝑡=
1
β
ln(αβ)+
1
β
lnt ……………..(12)
Where α is initial adsorbate rate(mg g-1 min) and β is related to the extent of surface coverage and the
activation energy for chemosorption (g mg-1). A plot of q𝑡 vs ln t gives a linear trace with slope of (1/β )
and an intercept of 1/β ln (αβ).

Intra particle diffusion model
The intra particle diffusion model (Weber and Morris. 1962) was applied to describe the competitive
adsorption. In a liquid-solid system, the fractional uptake of the solute on particle varies according to a
fraction of D the diffusivity within the particle and r is the particle radius. The initial rate of intra
particle diffusion are obtained by linearization of the curve q𝑡 = f (𝑡0.5)[18]. The plot of qt against 𝑡0.5
may present multi-linearity. This indicates that two or more steps occur in the adsorption processes.
The first sharper portion is external surface adsorption or instantaneous adsorption stage. The second
portion is the gradual adsorption stage where the intra particle diffusion is rate-controlled. The third
portion is the final equilibrium stage, where the intra particle diffusion starts to slow down due to the
extremely low solute concentration in solution
The diffusion model is expressed as :
q𝑡= K𝑖𝑑 𝑡0.5+ C ……………(13)
Where K𝑖𝑑 (mg/g 𝑚𝑖𝑛0.5) is the intraparticle diffusion rate constant q𝑡 , the amount of adsorbate
absorbed at time t and C(mg/g), a constant proportional to thickness of boundary layer.

0
r
Rate Expression:
According to the Fick's first law, the flux J(in moles per unit time and if, cross section, normal
to the path of flow) of the diffusing ion[19] can be expressed by equation (14)
…………..(14)
Where C is the concentration (in moles per unit volume), Di the effective diffusion coefficient
and r gives the direction along which transport is taking place.
Using the Fick’s second law, the governing differential equation for a spherical exchange bed
of radius ro in a solution can be expressed
……………….(15)
Using the proper boundary conditions, the solution of this equation has been obtained as an
infinite series i.e.
…………….(16)
r
C
D
J i










r
r
C
r
C
D
t
C
i





 2
2
2
0
1
Q
Q
F t










 

2
0
2
2
2
1
2
exp
1
6
1
r
n
t
D
n
i
n



 
Bt
n
n
n
2
2
1
2
exp
1
6
1 

 



Where F = fractional attainment of equilibrium at time ‘t’
D = effective diffusion coefficient of ion in the adsorbent phase
r0 = radius of the adsorbent particle
2
0
2
r
D
B i


= time constant …….....……… (18)
and n = l,2,3..... are the integers defining the infinite series solution obtained for a Fourier
type of analysis.
………………….(17)

Thus knowing the value of B and mean particle radius r0 ,the effective diffusion coefficient Di can
be calculated for an adsorption system.
From equation (17), the plot of Bt versus t must be straight line (of slope B) passing through the
origin provided the exchange rate is governed by particle-diffusion mechanism [20].
It is to be noted that the treatment is same with particle diffusion as controlling process as that
for isotopic exchange for which equation (17) is developed except that the self-diffusion
coefficient is replaced by effective diffusion coefficient of exchange ions [21].
The fractional attainment of equilibrium is determined by
…………….(19)
Where Qt= amount adsorbed after time‘t’
Q = amount adsorbed after infinite time or at equilibrium.
Reichenberg’s table[22] is used to obtain the corresponding Bt values for every observed value of
F.


Q
Q
F t

To distinguish between the film and particle diffusion controlled rates of adsorption, the
linearity test of Bt versus t plot have been used and in these studies the experimental
conditions were set up for particle-diffusion mechanism as the rate determining step.
The linear behaviour of log Di versus l/T plot permits the use of Arrhenius equation.
……………..(20)
From the slope and intercept of the linear plot of energy of activation Ea and D0 values of
the process have been calculated. The values obtained for D0 have been used to calculate
the entropy of activation S# using the following equation.
……………(21)
Where k, h and R are the usual constants and d is the distance between the adsorbing sites
of the adsorbent. Conventionally, it is taken as equal to 5 x10-8 cm.







RT
E
D
D a
i exp
0







R
S
h
kT
d
D
#
2
0 exp
72
.
2

The mass transfer study: The mass transfer coefficient values (βL) for the adsorption of
Copper, Cadmium, Lead and Safranin on Zeolite at 250 C were calculated graphically (fig.
38, 39 and 40) by using equation (mass transfer coefficient equation) .
ln [Ct/Co – 1/ 1+mk] = ln mk/1+mk – 1+mk/mk βLSst ……………….(22)
Ss = C0m / (1-€p) dpϼp ………………..(23)
Where, Ct = concentration of adsorbate after time t
C0 = Initial adsorbate concentration
M = mass of adsorbent per unit volume of particle free adsorbent solution
k = Langmuir constant obtained by multiplying adsorption capacity Qm and adsorption
energy b
βL = Mass transfer coefficient
Ss = Outer surface of the adsorbent per unit volume
€p = Porosity of adsorbent
dp = Particle diameter (cm)
ϼp = Density of adsorbent

RESULTS AND DISCUSSION
CHARACTERIZATION OF THE ADSORBENT
XRF Analysis:
The chemical composition of fly ash determined by WDXRF are shown in Table 1 which
depicts that the major constituents of the fly ash .The fly ash mainly contains silica and
alumina with SiO2 to Al2O3 ratio of 2.43 which is consistent with other fly ash (class F)
samples used in literature to synthesize zeolites. Therefore coal fly ash is suitable as raw
material for zeolite synthesis. There was increase in the percentage of Na2O (from 1.23 to
6.19%) in synthesized zeolite compared to coal fly ash. This is due to involvement of Na+
ions required to neutralize the negative charge on aluminate in zeolite.

Chemical composition Percentage by weight Percentage by weight Chemical composition Percentage by weight Percentage by weight
CFA Zeolite CFA Zeolite
Silica: 55.26 49.13 Vanadium oxide: 0.11 0.08
Alumina: 22.75 17.43 Barium oxide: 0.08 0.07
Iron oxide: 7.12 7.06 Manganese oxide: 0.08 0.06
Calcium oxide: 4.1 3.8 Scandium oxide: 0.05 0.04
Titanium oxide: 2.95 2.89 Strontium oxide: 0.04 0.02
Potassium oxide: 2.14 2.04 Zinc oxide: 0.04 0.03
Phosphorus penta-oxide: 1.65 1.57 Nickel oxide 0.03 0.03
Sulphur trioxide: 1.58 1.53 Rubidium oxide: 0.02 0.02
Sodium oxide: 1.23 6.19 Copper oxide: 0.02 0.01
Magnesium oxide: 0.63 0.61 Niobium oxide: 0.01 0.008
Zirconium oxide: 0.11 0.09
Table 1: XRF analysis of Coal Fly ash and zeolite (CFA: NaOH 1:1.5)

EDX Analysis:
Energy-dispersive X-ray spectroscopy (EDX) is an analytical technique used for the
elemental analysis of a sample.
(a) Untreated fly ash (b) Zeolite
Fig 1 : Representing EDX analysis

XRD Analysis:
The X-ray diffraction (XRD) patterns of fly ash and synthesized zeolite material were
obtained using a Philips X-ray diffractometer (Philips BW1710). Operating conditions
involved the use of Cu K α radiation at 4 kV and 30 mA. The samples were scanned from
10–90° (2θ, where θ is the angle of diffraction). Various crystalline phases present in the
samples were identified with the help of JCPDS files number(39-0219) for inorganic
compounds. Quantitative measure of the crystallinity of the synthesized zeolite was
made by using the summed heights of major peaks in the X-ray diffraction pattern
(Szostak 1976). The major peaks were selected specifically because they are least
affected by the degree of hydration of samples and also by others.

XRD of Coal fly ash XRD of zeolite at 550oC
As shown in fig. 2 the XRD pattern of CFA mainly consist of crystalline quartz and mullite phases, CFA is
primarily consist of amorphous material. The lower diffraction angles in CFA is due to the amorphous phases.
After the synthesis of zeolite from CFA, many sharp diffraction peaks of high intensity emerges which confirm
the formation of zeolite. The phases were identified by comparing with other diffractograms from literature
obtained by using inorganic index to the powder diffraction of JCPDS.
The XRD pattern of zeolite indicates that the NaP type of zeolite was synthesised (Na3Al6Si10O32. 12H2O)
Fig 2 : Analysis of XRD

SEM Analysis:
The morphological structure of the untreated fly ash, and synthesized zeolite material
were obtained by using scanning electron micrograph (Jeol, JSM 5800). The bulk
composition was also estimated from SEM by indirect method. The results were further
verified by X-ray fluorescence (XRF) data.
(a) Untreated CFA (b) Zeolite
Fig 3 : SEM Analysis

FTIR Analysis:
Based on the spectrum obtained from Fourier transform infra-red (FTIR) analysis of fly ash
and AAF as shown in fig. 4, it is observed that there are significant changes in the
intensities and the width of various bands due to interaction of fly ash with alkali. It can
be noticed that there is an increase in intensity and broadness of the stretching
frequency OH band at 3452 cm-1 after the treatment. This can be attributed to an
increase in hydrated products due to the reaction between amorphous silicate and the
alkali. Further the shift in the frequency to lower values indicates change in acidic
character of the terminal Si-OH group.
Coal fly ash zeolite material
Fig 4: FTIR Analysis of CFA and zeolite
3452
1000-1076
400-434
603

Moreover, asymmetrical stretching of TO4 (SiO4 and AlO4) band corresponding to the
variation in frequency from 1076 to 1000 cm-1 and the increase in its sharpness
confirms synthesis of silicates and change in its acidic characteristics. This can be
attributed to substitution of Si+4 by Al+3 in some of the tetrahedral framework of the
primary building units of the aluminosilicates and their external linkage with the Na+
ions due to their interaction with the alkali .The band at 434 cm-1 indicates the
increased crystallization of product.
Based on FTIR spectrum in fig. 4, it can be observed that there is presence of pore
opening corresponding to frequency range from 420-400 cm-1in the zeolite which can
be attributed to the dissolution of minerals present in the fly ash and precipitation of
zeolite.

BATCH STUDIES
Safranin
Influence of contact time:
The effect of contact time was studied at Safranin dye concentrations of 5 and 10, 20mg/l with
a fixed adsorbent dose of 5 g/l at 298 K and natural pH of 6.8. The contact time was varied from
15 min to 300 min for both the concentrations studied and the percentage efficiency was
calculated. The results of contact time on adsorption efficiency plotted in figure 5 .
A perusal of figure 5 indicates that the efficiency of dye adsorbed was rapid in initial stage up
to 180 min and after that remains almost constant due to saturation of the active sites which do
not allow further adsorption to take place. It is also observed that at higher concentration of
Safranin (10 mg/l), the adsorption efficiency is high (82.4 %) as compared to the maximum
efficiency of 79.7 % for 5 mg/l after 180 min of contact time. The observed increase in the
adsorption of dyestuffs with increasing concentration may be due to availability of sufficient
adsorption sites at adsorbent. The optimal contact time to attain equilibrium was
experimentally found to be about 180 min.

The effect of contact time was studied for metal ions including Copper, Cadmium and
lead at concentrations of 100 and 500 mg/l with a fixed adsorbent dose of 5 g/l at 298 K
for Copper and 10g/l For Cadmium and Lead at natural pH. The contact time was varied
from 15 min to 300 min for both the concentrations studied and the percentage
efficiency was calculated. The results of contact time on adsorption efficiency plotted in
figure 5. A perusal of fig. 5 (a-d) indicates that the efficiency of adsorption was rapid in
initial stage up to 240, 90, 120 min for Cu, Cd, Pb respectively and after that remains
almost constant due to saturation of the active sites which do not allow further
adsorption to take place.

(a) (b)
(c ) (d)
Fig 5 : Contact time for (a) Safranin (b) Copper (c) Cadmium and (d) Lead

Influence of pH
To determine the optimum pH conditions for the adsorption of safranin on zeolite
material, the effect of pH was observed over the pH range (4.0–10.0). The studies were
conducted at a fixed concentration of adsorbate (5 mg/l), contact time (180 min) and
adsorbent dose 5 g/l at 323 K. The results obtained are presented in fig. 6 which show
that adsorption of safranin increases with increase in pH from 4.0 to 9.0 and after that no
appreciable change has been observed on further increase in pH to 10.0. Maximum
adsorption of Safranin is 90.3 % at an optimum pH of 9.0.
Similarly optimum pH for metal ions was studied over a range (4.0-10.0) for copper and
lead and (2.0-10.0) for cadmium. Studies conducted on fixed adsorbate dose of (10g/l) for
cadmium and lead, (5g/l) for copper, contact time (240, 90, 120 min) for Cu, Cd, Pb
respectively were studied on adsorbent dose of 100 and 500 ppm at 298 K.
The result obtained in fig. (7-9) show that adsorption of metal ions increase with increase
in pH and after no appreciable change is observed on further increase of pH to 6,5 and 5
for Cu, Cd, Pb respectively.
Maximum adsorption of metal ions (Cu, Cd, Pb) was of 95.7%, 85.1%, 89.7% respectively
at pH of 6,5,5 respectively.

Fig:6 Influence of pH on uptake of Safranin Fig 7:Influence of pH on uptake of in Copper
Fig 8:Influence of pH on uptake of in Cadmium Fig 9: Influence of pH on uptake of in Lead

Influence of adsorbent dosage:
In order to investigate the effect of mass of adsorbent on the adsorption of safranin, a
series of adsorption experiments was carried out with different adsorbent dosage at an
initial dye concentration of 10 mg/l. Fig. 10 shows the effect of adsorbent dosage on
the removal of safranin. The percentage removal of safranin increased with the
increase in adsorbent initially from 5 g/l to 10g/l. This can be attributed to increased
adsorbent surface area and availability of more adsorption sites resulting from the
increase adsorbent dosage. But on increasing it further the adsorption efficiency is
reduced. It may be due to the overcrowding of adsorbate molecules which prevent the
diffusion through the actual adsorption sites.
Similarly fig. 11 and 12 (a-b) represents the effect of adsorbent dosage on the removal
of Copper, Cadmium and Lead respectively.

Fig:10 Influence of adsorbent dose on uptake of Safranin Fig 11:Influence of adsorbent dose on uptake of Copper
Fig 12(a): Influence of adsorbent dose on uptake of Cadmium Fig 12 (b): Influence of adsorbent dose on uptake of Lead

 Influence of initial adsorbate concentration and temperature:
The effect of initial concentration of safranin between the ranges of 5 to 60 mg/l was
carried out to observe the absorption efficiency at a fixed adsorbent dosage (5 g/l) and
temperature (298 and 323 K). The pH was maintained at 9.0 and contact time was kept
180 min. The results of the studies are shown in fig. 13 (a) which depict that dye uptake
increases with increase in initial Safranin concentration from 5 to 60 mg/l and thereafter
equilibrium is achieved in dye uptake efficiency at a concentration of 50 mg/l at 298 and
323K. The increment in sorption capacity may be due to the increase of dye
concentration which resulted in higher concentration gradient of the dye, thus leading to
higher sorption capacity. The rate of uptake of dye was found to decrease with increase
in temperature, thereby indicating the process to be exothermic in nature. This decrease
in adsorption efficiency on increase in temperature may be due to the weakening of
adsorptive forces between the active sites of the adsorbent and adsorbate.
Similarly fig. 13(b) and 14(c-d) represents Metal uptake with increase in concentration
from 100-500 ppm.

(c ) (d)
Fig 13 (a),(b) Influence of initial adsorbate concentration and temperature on uptake of Safranin and Copper
Fig 14 (c),(d) Influence of initial adsorbate concentration and temperature on uptake of Cadmium and Lead
(a) (b)

Adsorption Isotherms:
Langmuir, Freundlich, Temkin and D-R isotherm models have been used to evaluate
the adsorption data for all adsorbates.
The values of the regression coefficients in fig (15-18) for safranin indicate that the
experimental data satisfactorily follows order: Freundlich>Langmuir>D-R> Temkin at
298K. The values of Langmuir, Freundlich, Temkin and D-R constant are given in the
Table 2.
The values of the regression coefficients in fig (19-22) for copper indicate that the
experimental data satisfactorily follows order: Langmuir>D-R> Freundlich> Temkin at
Table 3.

Adsorption Isotherms:
The values of the regression coefficients in fig (23-26) for cadmium indicate that the
experimental data satisfactorily follows order: Langmuir>D-R> Freundlich> Temkin at
Table 4.
The values of the regression coefficients in fig (27-30) for Lead indicate that the
experimental data satisfactorily follows order: Freundlich>D-R> Langmuir> Temkin at
Table 5.

(a) (b)
Fig : 15 Langmuir isotherm plot of Safranin at (a) 298 and (b) 323 K
Fig : 16 Freundlich Isotherm plot of Safranin at (c) 298 and (d) 323 K
(c) (d)

(a) (b)
(c) (d)
Fig : 17 Temkin isotherm plot of safranin (a) at 298K and (b) at 323K
Fig : 18 Dubinin-Radushkevitch (D-R) of safranin (c) at 298 K and (d) at 323K

(a) (b)
Fig : 19 Langmuir isotherm plot of Copper at (a) 298 and (b) 323 K
Fig :20 Freundlich Isotherm plot of Copper at (c) 298 and (d) 323 K
(c) (d)

(a) (b)
(c) (d)
Fig : 21 Temkin isotherm plot of Copper (a) at 298K and (b) at 323K
Fig : 22 Dubinin-Radushkevitch (D-R) of Copper (c) at 298 K and (d) at 323K

(a) (b)
Fig :23 Langmuir isotherm plot of Cadmium at (a) 298 and (b) 323 K
Fig :24 Freundlich Isotherm plot of Cadmium at (c) 298 and (d) 323 K
(c) (d)

Fig: 25 Temkin isotherm plot of Cadmium (a) at 298K and (b) at 323K
Fig: 26 Dubinin-Radushkevitch (D-R) of Cadmium (c) at 298 K and (d) at 323K
(a) (b)
(c) (d)

(a) (b)
Fig : 27 Langmuir isotherm plot of Lead at (a) 298 and (b) 323 K
Fig : 28 Freundlich Isotherm plot of Lead at (c) 298 and (d) 323 K
(c) (d)

Fig : 29 Temkin isotherm plot of Lead (a) at 298K and (b) at 323K
Fig : 30 Dubinin-Radushkevitch (D-R) of Lead (c) at 298 K and (d) at 323K
(a) (b)
(c) (d)

At 298 K At 323 K
Langmuir qm mg-g
-1
7.14 Langmuir qm mg-g
-1
5.52
b 1.0687 b 1.1242
R
2
0.979 R
2
0.918
RL 0.1576 RL 0.151
Frendlich KF mg-g
-1
3.79 Frendlich KF mg-g
-1
2.432
1/n 0.758 1/n 0.631
R
2
0.982 R
2
0.976
Temkin At L-mg
-1
6.4867 Temkin At L-mg
-1
4.41217
bt J-mol
-1
1140.16 bt J-mol
-1
1291.68
9
Bt 2.173 Bt 2.079
R
2
0.9 R
2
0.814
Dubinin-
Radushkevich qDR mol-g
-1
8.7146
Dubinin-
-1
4.77789
β
(mol-g
-
1
)
2
9×10
-8
β (mol-g
-1
)
2
8×10
-8
E KJ-mol
-1
2.357 E KJ-mol
-1
2.5
R
2
0.959 R
2
0.666
Table 2 : Langmuir, Frendlich, Temkin, Dubinin-Radushkevich isotherm parameters of Safranin adsorption system

At 298 K At 323 K
Langmuir qm mg-g
-1
-1
166.66
b 11 b 2
R
2
961 R
2
0.959
RL 0.01785 RL 0.0909
Frendlich KF mg-g
-1
113 Frendlich KF mg-g
-1
135.2
1/n 0.552 1/n 0.704
R
2
0.909 R
2
0.975
Temkin At L-mg
-1
-1
0.233
bt J-mol
-1
102.379 Bt J-mol
-1
84.3411
Bt 24.2 Bt 31.84
R
2
0.798 R
2
0.955
Dubinin-
-1
248.88
Dubinin-
-1
400.2142
β (mol-g
-1
)
2
7×10
-9
β (mol-g
-1
)
2
8×10
-7
E KJ-mol
-1
8.451 E KJ-mol
-1
7.905
R
2
0.909 R
2
0.977
Table 3 : Langmuir, Frendlich, Temkin, Dubinin-Radushkevich isotherm parameters of Copper adsorption system

At 298 K At 323 K
Langmuir qm mg-g
-1
-1
41.66
b 1.133 b 1.2
R
2
0.995 R
2
0.989
RL 0.0811 RL 0.0769
Frendlich KF mg-g
-1
-1
22.33
1/n 0.6561 1/n 0.615
R
2
0.984 R
2
0.997
Temkin At L-mg
-1
-1
0.08702
bt J-mol
-1
192.2 bt J-mol
-1
251.208
Bt 12.89 Bt 10.69
R
2
0.979 R
2
0.964
Dubinin-
-1
116.745
Dubinin-
-1
81.695
β (mol-g
-1
)
2
1×10
-8
β (mol-g
-1
)
2
8×10
-9
E KJ-mol
-1
7.071 E KJ-mol
-1
7.905
R
2
0.957 R
2
0.994
Table 4: Langmuir, Frendlich, Temkin, Dubinin-Radushkevich isotherm parameters of Cadmium adsorption system

At 298 K At 323 k
Langmuir qm mg-g
-1
50 Langmuir qm mg-g
-1
66.66
b 2.22 b 15
R
2
0.99 R
2
0.996
RL 0.0431 RL 0.0066
Frendlich KF mg-g
-1
-1
174.2
1/n 0.588 1/n 0.6188
R
2
0.996 R
2
0.991
Temkin At L-mg
-1
-1
0.08702
bt J-mol
-1
194.776 bt J-mol
-1
251.208
Bt 12.72 Bt 15.33
R
2
0.96 R
2
0.982
Dubinin-
-1
115.3533
Dubinin-
-1
275.063
β (mol-g
-1
)
2
9×10
-9
β (mol-g
-1
)
2
5×10
-9
E KJ-mol
-1
7.453 E KJ-mol
-1
10
R
2
0.995 R
2
0.995
Table 5: Langmuir, Frendlich, Temkin, Dubinin-Radushkevich isotherm parameters of Lead adsorption system

Thermodynamic Parameters:
SAFRANIN
Thermodynamic parameters can also be evaluated by using the data obtained from
the adsorption isotherms. The change in standard free energy (ΔG0), Enthalpy (ΔH0)
and entropy (ΔS0) of adsorption for Safranin was calculated by known methods and
the values are given in Table 6. The negative free energy value indicates the feasibility
of the process and spontaneous nature of adsorption. Positive enthalpy value
indicates the process to be endothermic. Positive entropy value supports the affinity
of the adsorbent material with the adsorbate.
ΔG0 (KJmole-1) ΔH0 (KJmole-1) ΔS0 (KJmole-1K-1)
-0.14439 1.762 6.39
Table 6: Thermodynamic Parameters for Safranin

COPPER
and entropy (ΔS0) of adsorption for copper was calculated by known methods and the
values are given in Table 7. The negative free energy value indicates the feasibility of
the process and spontaneous nature of adsorption. Negative enthalpy value indicates
the process to be exothermic. Negative entropy value supports the affinity of the
adsorbent material with the adsorbate.
-5.94 -54.6 -163.2
Table 7: Thermodynamic Parameters for Copper

CADMIUM
and entropy (ΔS0) of adsorption for Cadmium was calculated by known methods and
-0.309 1.839 7.213
Table 8: Thermodynamic Parameters for Cadmium

LEAD
and entropy (ΔS0) of adsorption for Safranin was calculated by known methods and
-19.76 61.167 271.56
Table 9: Thermodynamic Parameters for Lead

Kinetic studies:
Rate Constant of Adsorption:
The linear nature of the plots of log(qe-q) versus time for safranin, Copper,
cadmium and lead at 298K fig. 31 show the applicability of the first order rate
expression equation of Lagergren. The values of rate constant of adsorption (Kad)
were also calculated and are presented in Table 10 .
Adsorbate Kad (min-1)
COPPER
CADMIUM
LEAD
SAFRANIN
0.0115
0.039
0.0207
0.016
Table 10: Legergren constant for Safranin, Copper, cadmium and Lead

(a) (b)
(c) (d)
Figure 31 : Legergren plots for (a)safranin, (b)copper, (c)cadmium and (d) lead

Pseudo Second Order Model
The pseudo second order equation was based on adsorption capacity at equilibrium.
From the slope and intercept of the (t/qt) as a function of t, the plot provided excellent
linearity R2 > 0.99. K and qe values for Safranin, Copper, Cadmium and Lead at 250C was
mentioned in Table 11. Fig. 32 showed the applicability of the pseudo second order rate
expression equation.
Adsorbate K (mg g-1min-1) R2
Safranin 1.726 0.999
Copper 5.35 X 10-3 0.999
Cadmium 2.11 X 10-2 0.999
Lead 1.95 X 10-2 0.998
Table 11: Rate Constants of Adsorption (K) of PSO at 298 K

(a) (b)
( c) (d)
Figure 32 : Pseudo second order plots for (a) Safranin, (b) copper, (c ) Cadmium, (d) lead

Elovich Model
Elovich equation was mainly applicable for chemo adsorption kinetics. The equation was
often valid for systems in which the adsorbing surface was heterogenous. Fig 33 showed
plot of (qt) vs. (ln t) with a linear slope of 1/β and intercept of 1/β ln (α β). The results of
Elovich plot at various concentrations of Safranin, Copper, Cadmium and lead were cited
in Table 12.
Adsorbate α (mg g-1 min-1) β (mg g-1) R2
Safranin 9.45 X 1030 83.33 0.9876
Copper 2185.62 0.667 0.9962
Cadmium 138.03 1.126 0.9815
Lead 3757.16 1.522 0.9291
Table 12: Parameters of Elovich model

Figure 33: plots of Elovich for (a) Safranin ,(b) Copper, ( c) Cadmium and (d) Lead
(a) (b)
(c ) (d)

Intraparticle Diffusion Model
This model was applied to describe the competitive adsorption. The initial rate of diffusion
was obtained by linearization of the curve (qt) Vs (t0.5). The plot of (qt) against (t0.5) for
Safranin, Copper, Cadmium and Lead showed competitive adsorption occurring in solution
Fig. 34. The linear portion of plot for wide range of contact time between adsorbent and
adsorbate did not pass through the origin. The variation from the origin or near saturation
might be due to the variation of mass transfer in the initial and final stage of adsorption.
The values are given in Table 13.
Adsorbate Kdiff (mg g-1 min) Xi R2
Safranin 0.003 0.93 0.9635
Copper 0.302 14.63 0.9684
Cadmium 0.302 5.73 0.9877
Lead 0.198 6.78 0.9805
Table 13: Parameters of Intraparticle Diffusion Model

(a) (b)
(c ) (d)
Figure 34: Intraparticle plots for (a) Safranin, (b) Copper, (c ) Cadmium and (d) Lead

Rate expression and treatment of data:
 The dispersion coefficient of specific species depends upon its size, valance and compound nature. It likewise
depends on the charge density, mesh width, level of swelling and chemical nature of the framework of
adsorbent. Moreover, the composition of the pour fluid and temperature influences the diffusion coefficient.
 Different components are additionally responsible for reducing the mobility of certain species in the pores. It
was observed that the retardation was more prominent on polyvalent than monovalent particles. This
distinction was noticed in all identical environments.
 A favourable explanation was the electrostatic attraction on the ingoing particle by the fixed ionic group of
the adsorbent which normally is stronger on polyvalent particle. The retarding interaction within the
framework might also be other than electrostatic forces. Now and again some particular compound
collaborations might bring about a lower mobility of the species in question. A comparative impact can be
seen, because of London dispersion forces acting between the species and the matrix.

• It was found that Bt versus time plots for Cd2+, Cu2+, Pb2+ ions at different adsorbate concentrations were linear
and did not pass through the origin indicating the process to be film diffusing in nature. To confirm this
assumption, Mckay plots at different adsorbate concentrations had been drawn utilizing the least square
principle. Mckay plots were linear for these ions showing a film diffusion process.
• For Safranin, Bt versus time plots (Fig. 35) were linear at lower concentrations (5 ppm) but did not pass through
the origin indicating the process to be film-diffusion in nature. But at higher concentrations (≥10 ppm) the plots
obtained were curved and passed through the origin. The same could however be resolved into two linear plots
with different slops, thereby indicating the change in mechanism.
• The initial portion passes through the origin and has a smaller slope thus reflecting that the effective diffusion
coefficient was smaller, and the particle-diffusion mechanism was the rate limiting step. However, at a later
stage, the slop and consequently the effective diffusion coefficient increases and the line does not pass
through the origin. At this stage the process might not be purely particle-diffusion controlled, other factors like
micelle formation might also become effective.

• The increase in effective diffusion coefficient was due to an increase in the number of occupied
sites. To confirm this assumption, Mckay plots ( Fig. 36) at different adsorbate concentrations, have
been drawn utilizing the least square principle. Mckay plot was linear at lower concentration (5
ppm) which indicated the film-diffusion process. Mckay plots at higher concentrations (≥10 ppm)
were curved which justified the assumption that particle-diffusion process was the rate limiting
step.

Fig. 35: Plot of Bt versus Time for (a) Safranin, (b) Copper (c ) Cadmium and (d) Lead
(a) (b)
(c) (d)

Figure 36: Mckay plots of (a) Safranin, (b) Copper, (c) Cadmium (d) lead at various adsorbate concentration
(a) (b)
(c ) (d)

Diffusion coefficient
The effective diffusion coefficient values at 250C, 400C and 500C were calculated for
copper, cadmium, lead and safranin (Table 14) . It has been found that the Di
decreases with increase in temperature. It is due to increase in mobility of ions and
increase in the retarding force acting on the diffusing ions results in an de-
enhancement of Di with temperature fig.37 represent trend for Safranin, Copper,
Cadmium and Lead respectively.
The effective diffusion coefficient values observed in the present investigations, are
greater than those reported in case of hydrous ferric oxide (10-17 m2 sec-1) and clay
Montmorillonite (10-18 m2 sec-1). This leads to the inference that the channels in
the developed zeolite material are wider than those of hydrous oxides mentioned
above.

(a) (b)
( c) (d)
Figure 37: Plot of Di versus 1/T for (a)Safranin (b) Copper ( c) Cadmium and (d) Lead

Table: 14 Values of the effective diffusion coefficient (Di) at different temperatures
Adsorbate
Di(m2s-1)
298K (250C) 313K (400C) 323K (500C)
Safranin 2.11×10-10 2.20×10-10 2.29×10-10
Copper 1.89×10-10 1.93×10-10 2.04×10-10
Cadmium 9.26×10-12 1.02×10-11 1.16×10-11
Lead 2.61×10-12 2.85×10-12 3.09×10-12

The pre-exponential constant (Do), energy of activation (Ea) and entropy of
activation (∆S#) for the diffusion of Copper, Cadmium, Lead and Safranin were
calculated and are given in Table 15. The Values of entropy of activation (∆S#)
obtained for the exchange of Cadmium and Lead are positive. The values thus
indicate that the no significant change in the internal structure of the adsorbent
material was found during the exchange of ions .
Table 15 : Do, Ea and ∆S# values for the diffusion of adsorbates
Adsorbate Do (m2s-1) Ea (KJmole-1) ∆S# (KJ-1mole-1)
Safranin 5.9×10-10 2.5 x 10-3 -0.073
Copper 4.6×10-10 2.2 x 10-3 -0.075
Cadmium 1.6×10-10 7.1 x 10-2 0.085
Lead 2.2×10-11 5.3 x 10-3 0.101

The Mass transfer studies
The mass transfer coefficient values (βL) for the adsorption of Safranin, Copper, Cadmium and Lead on
Zeolite at 250C were calculated graphically by using mass transfer coefficient equation and reported in the
Table 16.
The linear nature of the plots (fig.38(a-d)) for all the adsorbates studied suggested the validity of the
diffusion model. The values of mass transfer coefficient suggest that the velocity of the adsorbate transport
from bulk to solid phase is quite rapid.
Table 16: βL and Ss values for different adsorbates
Adsorbate βL (cm sec-1) Ss (cm-1)
Safranin 1.05 X 10-9 2.53 X 106
Copper 6.21 X 10-8 2.51X 106
Cadmium 7.22 X 10-8 5.02X 106
Lead 4.04 X 10-8 5.12X 106

Figure 38 : ln[Ct / C0 - 1/1+mk] vs. time plot for the mass transfer for (a) Safranin (b) Copper ( c) Cadmium
and (d) Lead at 298 K
(a) (b)
( c) (d)

CONCLUSIONS
The following conclusions can be drawn from this research work:
1. Characterization of fly ash and Zeolite material confirmed the rich mineral content and mesoporous texture.
2. Approximately 97.14% of Safranin, 95.7% of Copper, 89.7% of Lead, and 85.1% of Cadmium, were adsorbed
within the 3 hour, 4 hour, 2 hour and 1.5 hour of contact respectively after which there were a slow process.
3. The pH was found to be significant factor which affects the adsorption capacity of Safranin, Copper, Cadmium
and lead. The higher percentage adsorbate removal was found at pH of 9.0, 6.0, 5.0 and 5.0 respectively.
4. The higher percentage removal was found with optimum adsorbent dose of 0.1g (5 gL-1) in case of Safranin
and Copper while it was 0.2g (10gL-1) for Cadmium and Lead.
5. Adsorption capacity of zeolite for Copper was found to be decreasing with increase in temperature suggesting
that the adsorption process was exothermic in nature while in case of safranin, Cadmium and Lead the
adsorption increases with increase in temperature showing the process to be endothermic.

6. The equilibrium adsorption data is better fitted by the Freundlich adsorption model than the Langmuir model
followed by DR and Temkin for Safranin and Lead while in case of Copper and Cadmium, Langmuir model is better
fitted than the Freundlich adsorption model followed by DR and Temkin and DR respectively.
7. Studies on the rate of uptake on zeolite under consideration indicate that the process is quite rapid and typically
24 to 38% of the ultimate adsorption occurs within the first hour of contact. This initial rapid adsorption
subsequently gives way to a very slow approach to equilibrium and the saturation is reached in 5 hours.
8. It is found that the rate of removal decreases with increasing amount of zeolite. For Safranin and Copper, the
optimum amount of fly ash is 5.0 gL-1, whereas the optimum amount of zeolite for Cadmium and Lead is 10.0 gL-1.
9. The linear nature of Kinetic Plots for Safranin, Copper, Cadmium and Lead at 250C show the applicability of the
Pseudo second order rate expression and indicates adsorption to be predominately chemo adsorption.

10. The Bt versus Time plots of Safranin at concentration (≥5 ppm) shows the process is film-diffusion in nature. The
Bt versus time plot for Cu(II), Cd(II) and Pb(II) at higher concentrations (≥300 ppm) indicating the process to be
particle-diffusion but at lower concentrations (≥100 ppm) indicating a film-diffusion process.
11. The effective diffusion coefficient values lead to the inference that the channels in the Zeolite are wider than
those of hydrous oxides and clays.
The cost of synthesized zeolite was very low as compared to commercial zeolite available in the market as it was
prepared from coal fly ash-f waste material from thermal power station. Utilization of fly ash as zeolite for
adsorption will solve not only its disposal problems and environmental hazards, but also helps as potential
adsorbent for removal of pollutant from wastewaters. Results indicate that the developed low cost adsorbent
Zeolite material could be a promising solution to the removal of metals ions and dye from synthetic wastewater.

References
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Azo Dye Using Natural Polymers, Response Surface Methodological Approach, Nigerian Journal of Technology
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adsorption of direct dye onto a novel green adsorbent developed from Uncaria gambir extract. Journal of Physical
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List of Publications
1. Cadmium removal from aqueous solution by Na-P Zeolite Synthesised by caol fly ash Payal jain,
Suresh jain and M.K. Dwivedi. Juni Khyat, Volume no.10, Issue No. 06 , June 2020.
2. Modelling of Copper adsorption onto Na-P Zeolite synthesized from Coal Fly Ash Payal jain, Priyanka
Shrivastava , Richa Pathak and M.K. Dwivedi Research Journal of Chemistry and Environment volume
no.24, Issue No.8 August 2020.
3. Synthesis and characterization of Na-P zeolite from coal fly ash M.K. Dwivedi, Payal Jain, Chanchala
Alawa International Journal of Science Technology and Management Volume No.05, Issue No. 03,
March 2016 .
4. Adsorptive removal of phenol by coal fly ash equilibrium and thermodynamic studies M.K. Dwivedi,
Rashmi Agarwal, Pragati Sharma, Payal Jain . International Journal of Advanced Technology in
Engineering and Science Volume No.02, Issue No. 10, October 2014.

5. Adsorptive Removal of Pb(II) from Aqueous Solution Using NaP Zeolite Synthesized From Coal Fly Ash.
Payal Jain, Priyanka Shrivastava, Vibha Malviya, Suresh Jain and M.K. Dwivedi .AIP Proceedings (Accepted)
2020 E-ISSN 1551-7616.
6. Thermodynamic and Kinetic Studies for the Removal of Safranin Dye from Aqueous Solution Using NaP
Zeolite Synthesized from Coal Fly Ash. Payal Jain, Priyanka Shrivastava, Vibha Malviya, Bijendra Rai and
M.K. Dwivedi. AIP Proceedings (Accepted).2020 E-ISSN 1551-7616.
7. Physicochemical analysis of water and soil samples collected from different sites of Pithampur Industrial
area Indore M.P. Richa Pathak ,Payal Jain, S.L. Garg and M.K. Dwivedi 2019 IJRAR Volume No.06 Issue No.
2 , October 2014.
8. FT-IR and ATR-FTIR studies of sludge (CETP) before and after adsorption of dyes from aqueous solution.
Vibha Malviya, M.K. Dwivedi, H. Bhatt, Arkadev Roy, Priyanka Shrivastava, Payal Jain. AIP Proceedings
(Accepted).2020 E-ISSN 1551-7616.

9. Process Development for the Removal of Malachite Green Dye from wastewater using Sewage
Sludge (STP) as an Adsorbent. Priyanka Shrivastava M. K. Dwivedi, Vibha Malviya and Payal Jain. AIP
Proceedings (Accepted).2020 E-ISSN 1551-7616.
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