# Equilibrium Isotherm Studies of Adsorption of Pigments Extracted from Kuduk-kuduk (Melastoma malabathricum L.) Pulp onto TiO2 Nanoparticles

Authors: N. T. R. N. Kumara; Nurulhayah Hamdan; Mohammad Iskandar Petra; Kushan U. Tennakoon; Piyasiri Ekanayake
Journal: Journal of Chemistry
 (2014)

---

## Abstract

The adsorption of natural pigments onto TiO2 nanoparticles was investigated. The pigments were extracted from the dark purple colored pulp of the berry-like capsule of Kuduk-kuduk (Melastoma malabathricum L.).  The Langmuir, Freundlich, Redlich-Peterson, and Sips isotherm models were used to analyze the equilibrium experimental data. Data correlated well with the Sips isotherm model, where the heterogeneity factor (n
=
0.24) indicated  heterogeneous adsorption characteristics, with a maximum adsorption capacity of 0.0130 mg/g. The heterogeneous adsorption character was further supported by results obtained from zeta-potential measurements. When a dye-sensitized solar cell (DSSC) was sensitized with the extracted pigment, the photo-energy conversion efficiency was measured to be 0.83%, thus proving the suitability of Kuduk-kuduk fruit pulp as a sensitizer in DSSCs.


---

## Body

## 1. Introduction

Commercially, the quality of a product depends on the product value and acceptability. However, consumers are also attracted to the physical appearances of the product, especially to its colors. In food, beverages, and textile industries, the pigments are employed as coloring agents and for dyeing purposes. Natural colorants extracted from plants have been used for centuries before the first synthetic colorant was introduced. Low cost and ease of application have driven the drift from natural colorants to synthetic. However, due to environmental and health concerns associated with the applications of synthetic colorants the interest of using natural and organic sources as colorants has increased lately.Anthocyanins are natural, water-soluble, and nontoxic pigments which are responsible for the red, orange, pink, blue, or purple color of plants. The resultant color variation depends on the relative pH of the respective plant [1]. The anthocyanin pigments are expressed as red or pink under acidic media, purple in neutral media, and blue, green, or yellow in alkaline media. It turns colorless under extreme alkaline conditions [2]. Thus, anthocyanins also can be used as a pH indicator. Anthocyanins have been employed as additives or colorants in the food industry with limited usage due to its instability with varying pH levels [1]. In the alternative energy sector, natural dye extracts containing anthocyanins are integrated as sensitizers in dye-sensitized solar cells (DSSCs) because of their ability to absorb light [3, 4] and low cost associated with extraction procedures.Many researches had been conducted on analyzing the potential anthocyanins sensitizers extracted from natural resources [5, 6], and currently an efficiency of natural sensitized DSSC of about 2% [4, 7] has been achieved. The performance and the efficiency of the DSSCs can be enhanced by increasing the adsorption capacity of the anthocyanins sensitizer onto the TiO2 nanoparticles surface and selecting pigments with broader absorption capacity. Adsorption is defined as the binding of molecules or particles (adsorbates) onto a surface (adsorbent). In this study adsorbate and adsorbent are anthocyanin pigments and TiO2 nanoparticles, respectively.Kuduk-kuduk (KK) also known as Malabar Melastome (Melastoma malabathricumL.), is a shrub belonging to the family Melastomataceae. This is naturally grown in the disturbed tropical and subtropical habitats under full sunlight [8]. The flower is purple (sometimes pink), while the fruit a berry-like capsule filled with purple color pulp with numerous seeds. The purple-pink color of the flower petals as well as the fruit pulp is due to anthocyanin pigments [9]. These features make it a valuable ornamental plant and a potential source for natural colorants.Currently, many researchers are focusing to achieve highly efficient DSSCs with natural sensitizers [4]. In order to achieve high efficiency in natural sensitized DSSCs, in addition to absorption capacities, the adsorption properties of the pigments onto TiO2 nanoparticles have to be investigated and improved [10]. The aim of this work is to investigate the adsorption properties of anthocyanin pigments extracted from KKP (KK fruit pulp) onto the surface of TiO2 nanoparticles using the Langmuir, Freundlich, Redlich-Peterson, and Sips isotherm models and to evaluate its potential as a natural sensitizer in DSSCs.


## 2. Experimental

### 2.1. Preparation and Characterization of Adsorbate

The natural anthocyanin-containing dye, used in this study, was extracted from KKP. 20 g (fresh weight) of the clean pulp was ground with a small amount of 70% ethanol (diluted from Scharlau 99.9% with distilled water). The crushed sample was mixed with 150 mL of 70% ethanol solution using a vortex mixture and kept at room temperature (25°C) overnight covered with an aluminum foil to ensure no exposure to outside light. The residues of the filtrate were removed by filtering through a filter paper (Whatman, Grade 1). The absorption spectra of the KKP extract were investigated in the range 400 to 700 nm using UV-vis spectrophotometer (1601 PC Shimadzu). According to absorption data in [11] the predominant anthocyanin present in KKP extract is cyanidin-3-glucoside. The total monomeric concentration of anthocyanin pigments in the dye extract was determined by using the pH-differential method [11] which is based on the difference in the pigments absorbance measurement at wavelengths of 520 nm and 700 nm:
(1)
Anthocyanin
pigment
content
(
mg
/
L
)
=
A
×
MW
×
DF
×
10
3
ε
×
l
,
where A
=
(
A
520
nm
-
A
700
nm
) pH 1.0 − (A
520
nm
-
A
700
nm) pH 4.5, MW (molecular weight) = 449.2 g/mol for cyanidin-3-glucoside (cyd-3-glu), DF = dilution factor, ε (molar extinction coefficient) = 26900 L mol−1 cm−1, 103 is the factor for converting g to mg, and l is the path length in cm.


### 2.2. Adsorption Studies

Adsorption isotherms of this study were carried out at different concentrations of KKP extract; a dilution series of six samples was prepared by mixing 0.25 to 0.5 mL of KKP extracts with absolute ethanol up to a volume of 10 mL. 20 mg of commercially available Degussa P-25 (mean particle diameter of 30 nm, 70% anatase, 30% rutile, and specific surface area of 50 g m−2) TiO2 powder was mixed into each sample and kept overnight at room temperature (25°C) without exposing to external light to ensure a good adsorption. The liquid phase of each mixture was separated after centrifuging for 10 min at 3000 rpm in a centrifuge (SiGma 3–18 k). The absorbance of KKP extract pigments in the solution, before and after adsorption, was measured at 520 nm. The adsorbed amount of KKP extract pigments at equilibrium, q
e (mg/g), was calculated using the mass balance equation [12]:
(2)
q
e
=
v
(
C
i
-
C
e
)
m
,
where C
i and C
e (mg/L) are the initial and equilibrium concentrations of KKP extract pigments solution, respectively, V is the volume of the solution used (L), and m is the mass of the dry adsorbent (TiO2 nanoparticles) (g). The Langmuir, Freundlich, Redlich-Peterson, and Sips isotherms were used to analyze the equilibrium data.


### 2.3. Zeta-Potential andI
-
V Measurements

The zeta-potential of the KKP extract at original pH was measured using Zetasizer (Nano MAN 0317) at a temperature of 25.0°C in ethanol solution. In order to prepare the TiO2 paste, a mixture of 0.20 g of TiO2 (Degussa P-25), 12 drops (0.15 g) of glacial acetic acid, one drop (0.02 g) of triton X-100, and 2 mL of ethanol were ground in a ball-mill machine (Paul O. Abbe Roller Mill, Model 202421) for 20 h. Subsequently the TiO2 paste was coated on precleaned fluorine-doped conducting tin oxide (FTO) glasses (Nippon sheet glass 10–12 Ω sq
-
1) by Doctor Blade method. The coated film was sintered for 45 min at 450°C. The thickness of sintered TiO2 electrode was ~9 μm (Dektak Profilometer; Veeco, Dektak 3). This electrode was dipped in the KKP extract overnight at room temperature (25°C) and air-dried at the same temperature [13]. The active solar cell area was 0.25 cm2. The cell was assembled using a Test Cell Assembly Machine (Dyesol) with the Surlyn (50 μm, Dyesol) as the spacer. A mixture of tetrabutylammonium iodide (TBAI; 0.5 M)/I2 (0.05 M), acetonitrile, and ethylene carbonate (6 : 4, v
/
v) was used as redox electrolyte [14]. The assembled solar cell was kept under 1 sun (Dyesol Solar Simulator LP-156B) for about 4 h for light soaking. Finally, I
-
V characteristic of the DSSC was measured.


## 2.1. Preparation and Characterization of Adsorbate

The natural anthocyanin-containing dye, used in this study, was extracted from KKP. 20 g (fresh weight) of the clean pulp was ground with a small amount of 70% ethanol (diluted from Scharlau 99.9% with distilled water). The crushed sample was mixed with 150 mL of 70% ethanol solution using a vortex mixture and kept at room temperature (25°C) overnight covered with an aluminum foil to ensure no exposure to outside light. The residues of the filtrate were removed by filtering through a filter paper (Whatman, Grade 1). The absorption spectra of the KKP extract were investigated in the range 400 to 700 nm using UV-vis spectrophotometer (1601 PC Shimadzu). According to absorption data in [11] the predominant anthocyanin present in KKP extract is cyanidin-3-glucoside. The total monomeric concentration of anthocyanin pigments in the dye extract was determined by using the pH-differential method [11] which is based on the difference in the pigments absorbance measurement at wavelengths of 520 nm and 700 nm:
(1)
Anthocyanin
pigment
content
(
mg
/
L
)
=
A
×
MW
×
DF
×
10
3
ε
×
l
,
where A
=
(
A
520
nm
-
A
700
nm
) pH 1.0 − (A
520
nm
-
A
700
nm) pH 4.5, MW (molecular weight) = 449.2 g/mol for cyanidin-3-glucoside (cyd-3-glu), DF = dilution factor, ε (molar extinction coefficient) = 26900 L mol−1 cm−1, 103 is the factor for converting g to mg, and l is the path length in cm.


## 2.2. Adsorption Studies

Adsorption isotherms of this study were carried out at different concentrations of KKP extract; a dilution series of six samples was prepared by mixing 0.25 to 0.5 mL of KKP extracts with absolute ethanol up to a volume of 10 mL. 20 mg of commercially available Degussa P-25 (mean particle diameter of 30 nm, 70% anatase, 30% rutile, and specific surface area of 50 g m−2) TiO2 powder was mixed into each sample and kept overnight at room temperature (25°C) without exposing to external light to ensure a good adsorption. The liquid phase of each mixture was separated after centrifuging for 10 min at 3000 rpm in a centrifuge (SiGma 3–18 k). The absorbance of KKP extract pigments in the solution, before and after adsorption, was measured at 520 nm. The adsorbed amount of KKP extract pigments at equilibrium, q
e (mg/g), was calculated using the mass balance equation [12]:
(2)
q
e
=
v
(
C
i
-
C
e
)
m
,
where C
i and C
e (mg/L) are the initial and equilibrium concentrations of KKP extract pigments solution, respectively, V is the volume of the solution used (L), and m is the mass of the dry adsorbent (TiO2 nanoparticles) (g). The Langmuir, Freundlich, Redlich-Peterson, and Sips isotherms were used to analyze the equilibrium data.


## 2.3. Zeta-Potential andI
-
V Measurements

The zeta-potential of the KKP extract at original pH was measured using Zetasizer (Nano MAN 0317) at a temperature of 25.0°C in ethanol solution. In order to prepare the TiO2 paste, a mixture of 0.20 g of TiO2 (Degussa P-25), 12 drops (0.15 g) of glacial acetic acid, one drop (0.02 g) of triton X-100, and 2 mL of ethanol were ground in a ball-mill machine (Paul O. Abbe Roller Mill, Model 202421) for 20 h. Subsequently the TiO2 paste was coated on precleaned fluorine-doped conducting tin oxide (FTO) glasses (Nippon sheet glass 10–12 Ω sq
-
1) by Doctor Blade method. The coated film was sintered for 45 min at 450°C. The thickness of sintered TiO2 electrode was ~9 μm (Dektak Profilometer; Veeco, Dektak 3). This electrode was dipped in the KKP extract overnight at room temperature (25°C) and air-dried at the same temperature [13]. The active solar cell area was 0.25 cm2. The cell was assembled using a Test Cell Assembly Machine (Dyesol) with the Surlyn (50 μm, Dyesol) as the spacer. A mixture of tetrabutylammonium iodide (TBAI; 0.5 M)/I2 (0.05 M), acetonitrile, and ethylene carbonate (6 : 4, v
/
v) was used as redox electrolyte [14]. The assembled solar cell was kept under 1 sun (Dyesol Solar Simulator LP-156B) for about 4 h for light soaking. Finally, I
-
V characteristic of the DSSC was measured.


## 3. Results and Discussion

### 3.1. The Optical Properties

The UV-vis absorption spectra of KKP extract confirmed the presence of anthocyanin pigments. It produced a prominent peak at the wavelength of 520 nm when a drop of HCl was added into the original KKP extract [11].


### 3.2. Kinetic Adsorption Studies

The parameters required for kinetic adsorption isotherm study are summarized in Table1. The occurrence of the adsorption process was signified from the differences shown among the values of C
i and C
e, where a decrease in the concentration of anthocyanin pigments was observed. The amount of anthocyanin pigments adsorbed per unit mass of TiO2 is shown in Table 1.Table 1
The parameters required for kinetic adsorption isotherm study.
Vol. of dye extract (mL)
C
i (mg/L)
C
e (mg/L)
q
e (mg/g)
0.25
0.02145
0.00765
0.00686
0.30
0.02574
0.00914
0.00826
0.35
0.03003
0.00963
0.00995
0.40
0.03433
0.01112
0.01178
0.45
0.03860
0.01459
0.01166
0.50
0.04290
0.01756
0.01280Adsorption isotherms models describe the distribution of the adsorbate species between liquid and adsorbent through linearly plotted graphs based on a set of assumptions y related to the heterogeneity or homogeneity of adsorbents, the type of coverage, and the possibility of interaction between the adsorbates [15].


#### 3.2.1. Langmuir Isotherm

The Langmuir adsorption isotherm model explains the variation of adsorption of molecules (adsorbates) with pressure. The isotherm is based on the assumption that maximum adsorption occurs when a saturated monolayer of adsorbate molecules is present on the adsorbent surface, the energy of adsorption is constant, and there is no migration or interaction between the adsorbate molecules in the surface plane [16, 17]. The linear expression of the Langmuir isotherm model is defined by
(3)
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
.By plotting the linear graph of 1/q
e against 1/C
e, the values of K
L and q
m can be determined from the intercept and slope of the plot (Figure 1), where the parameter q
m (mg/g) is the maximum adsorption capacity of dye per unit mass of sorbent to form a complete monolayer on the surface bound at high C
e and K
L (L/mg) is the Langmuir energy constant which is related to the heat of adsorption. Table 2 presents the values of Langmuir constants (q
m
=
0
.
0468 mg/g, K
L
=
28.489 L/mg). The essential characteristics of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor R
L that is given by
(4)
R
L
=
1
(
1
+
K
L
C
i
)
,
where C
i (mg/L) is the highest initial concentration of adsorbate and R
L values between 0 and 1 imply favorable adsorption. The value of R
L in the present investigation was calculated to be 0.45 which indicates favorable adsorption of KKP extract pigments onto TiO2 nanoparticles surface.Table 2
Parameters and correlation coefficient (R
2) of equilibrium isotherm models for the adsorption of KKP extract pigments onto TiO2 nanoparticles.
Isotherm
Equation
Parameters
R
2
Langmuir
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
K
L = 28.489 L/mg
0.915
q
m = 0.047 mg/g
Freundlich
log
q
e
=
1
n
log
C
e
+
log
K
F
K
F = 0.225 (1/g)
0.893
1
n = 0.69
Redlich-Peterson
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
K
R = 10 mg/g
0.657
a
R = 45.814 mg/L
b
R = 0.335
Sips
1
q
e
=
1
Q
max
K
s
(
1
C
e
)
1
/
n
+
1
Q
max
K
S
=
6.97
×
10
8 L/mg
0.971
Q
max = 0.0130 mg/g
n
=
0.24Figure 1
Langmuir adsorption isotherm and experimental data of KKP extract.


#### 3.2.2. Freundlich Isotherm

The Freundlich isotherm explains that the extent of adsorption varies directly with pressure. This empirical relationship describes the multilayer adsorption of heterogeneous systems and assumes that different sites have several adsorption energies involved [18]. The linear model of the isotherm can be expressed logarithmically as in
(5)
log
q
e
=
1
n
log
C
e
+
log
K
F
.The values of parametersK
F and n (listed in Table 2) can be determined from the intercept and slope of the plot log
C
e against log
q
e (Figure 2), where K
F (1/g) is the Freundlich adsorption capacity constant and 1/n is related to the adsorption intensity constant that varies with the heterogeneity of the adsorbate.Figure 2
Freundlich adsorption isotherm and experimental data of KKP extract.


#### 3.2.3. Redlich-Peterson Isotherm

The Redlich-Peterson (R-P) isotherm is a three-parameter empirical adsorption model that incorporates elements from both the Langmuir and Freundlich isotherms [15] and amends the inaccuracies. The adsorption mechanism is unique and does not follow ideal monolayer adsorption characteristics. The linear expression of the R-P isotherm model is defined as [15]
(6)
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
,
where K
R is the Redlich-Peterson adsorption capacity constant determined via trials and errors to obtain the maximum linear regression value of the isotherm graph (Figure 3). The parameter a
R is the R-P isotherm constant and b
R is the exponent between 0 and 1. Numerous studies [19–24] have shown that the R-P isotherm was more accurate than the Langmuir and Freundlich isotherms as it contains three unknown parameters. The reason for this is that the Langmuir and Freundlich isotherms can be derived from the R-P isotherm. When b
R = 1, the R-P equation becomes the Langmuir isotherm equation and when b
R
=
0, it is closer to the Freundlich equation. However, the accuracy of these interpretations strongly depends on the fitting method [25–28].Figure 3
Redlich-Peterson adsorption isotherm and experimental data of KKP extract.


#### 3.2.4. Sips Isotherm

The Sips isotherm is derived from the limiting behavior of the Langmuir and Freundlich isotherms. The model is valid for localized adsorption without adsorbate-adsorbate interactions [15]. When C
e approaches a low value, the Sips isotherm effectively reduces to Freundlich, while at high C
e, it predicts the Langmuir monolayer sorption characteristic. The Sips linear equation model is expressed as [15]
(7)
1
q
e
=
1
Q
max
K
S
(
1
C
e
)
1
/
n
+
1
Q
max
,
where K
S (1/mg) and Q
max (mg/g) are the Sips equilibrium constant and maximum adsorption capacity values obtained from the slope and the intercept of the plot (Figure 4). The Sips isotherm equation is characterized by the dimensionless heterogeneity factor, n, which can also be employed to describe the system’s heterogeneity when n is between 0 and 1. When n
=
1, the Sips equation reduces to the Langmuir equation and it implies a homogeneous adsorption process [21].Figure 4
The Sips adsorption isotherm and experimental data of KKP extract.The parameters and correlation coefficient (R
2) for each of the equilibrium isotherm models of the adsorption process are shown in Table 2. The Redlich-Peterson model clearly shows poor correlation (R
2
=
0.657) to the experimental data. Similarly, the Freundlich isotherm model that assumes an exponential increase in the adsorption amount does not fit well with data (R
2
=
0.893). Both the Langmuir (R
2
=
0.915) and Sips isotherm (R
2
=
0.971) models show good fit to experimental data. However, heterogeneous adsorption process is evidently indicated from the heterogeneity factor value (n
=
0.24). Thus, the isotherm that best describes the adsorption behavior of KKP extract pigments onto the TiO2 nanoparticles is the Sips isotherm.


### 3.3. Zeta-Potential and Photovoltaic Performance in DSSC

For KKP extract, zeta-potential of −9.48 mV was obtained. This indicates the tendency of anthocyanin pigment molecules coagulating at its original pH (~5), which correlates well with the pigment’s adsorption characteristics as explained by the Sips isotherm.The DSSC performance was examined using the current-voltage characteristics, as shown in Figure5. The values obtained for open circuit voltage (V
OC), short circuit current density (J
SC), and fill factor (
f
f
) were 0.448 V, 3.177 mA/cm2, and 0.52, respectively. Although monolayer adsorption condition is favorable for the photoconversion of DSSC anode [29], the KKP extract that showed multilayer adsorption characteristics has demonstrated its capability of sensitizing DSSCs while giving a photoenergy conversion efficiency of 0.83%.Figure 5
I
-
V characteristics of DSSC sensitized with KKP extract.


## 3.1. The Optical Properties

The UV-vis absorption spectra of KKP extract confirmed the presence of anthocyanin pigments. It produced a prominent peak at the wavelength of 520 nm when a drop of HCl was added into the original KKP extract [11].


## 3.2. Kinetic Adsorption Studies

The parameters required for kinetic adsorption isotherm study are summarized in Table1. The occurrence of the adsorption process was signified from the differences shown among the values of C
i and C
e, where a decrease in the concentration of anthocyanin pigments was observed. The amount of anthocyanin pigments adsorbed per unit mass of TiO2 is shown in Table 1.Table 1
The parameters required for kinetic adsorption isotherm study.
Vol. of dye extract (mL)
C
i (mg/L)
C
e (mg/L)
q
e (mg/g)
0.25
0.02145
0.00765
0.00686
0.30
0.02574
0.00914
0.00826
0.35
0.03003
0.00963
0.00995
0.40
0.03433
0.01112
0.01178
0.45
0.03860
0.01459
0.01166
0.50
0.04290
0.01756
0.01280Adsorption isotherms models describe the distribution of the adsorbate species between liquid and adsorbent through linearly plotted graphs based on a set of assumptions y related to the heterogeneity or homogeneity of adsorbents, the type of coverage, and the possibility of interaction between the adsorbates [15].


### 3.2.1. Langmuir Isotherm

The Langmuir adsorption isotherm model explains the variation of adsorption of molecules (adsorbates) with pressure. The isotherm is based on the assumption that maximum adsorption occurs when a saturated monolayer of adsorbate molecules is present on the adsorbent surface, the energy of adsorption is constant, and there is no migration or interaction between the adsorbate molecules in the surface plane [16, 17]. The linear expression of the Langmuir isotherm model is defined by
(3)
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
.By plotting the linear graph of 1/q
e against 1/C
e, the values of K
L and q
m can be determined from the intercept and slope of the plot (Figure 1), where the parameter q
m (mg/g) is the maximum adsorption capacity of dye per unit mass of sorbent to form a complete monolayer on the surface bound at high C
e and K
L (L/mg) is the Langmuir energy constant which is related to the heat of adsorption. Table 2 presents the values of Langmuir constants (q
m
=
0
.
0468 mg/g, K
L
=
28.489 L/mg). The essential characteristics of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor R
L that is given by
(4)
R
L
=
1
(
1
+
K
L
C
i
)
,
where C
i (mg/L) is the highest initial concentration of adsorbate and R
L values between 0 and 1 imply favorable adsorption. The value of R
L in the present investigation was calculated to be 0.45 which indicates favorable adsorption of KKP extract pigments onto TiO2 nanoparticles surface.Table 2
Parameters and correlation coefficient (R
2) of equilibrium isotherm models for the adsorption of KKP extract pigments onto TiO2 nanoparticles.
Isotherm
Equation
Parameters
R
2
Langmuir
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
K
L = 28.489 L/mg
0.915
q
m = 0.047 mg/g
Freundlich
log
q
e
=
1
n
log
C
e
+
log
K
F
K
F = 0.225 (1/g)
0.893
1
n = 0.69
Redlich-Peterson
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
K
R = 10 mg/g
0.657
a
R = 45.814 mg/L
b
R = 0.335
Sips
1
q
e
=
1
Q
max
K
s
(
1
C
e
)
1
/
n
+
1
Q
max
K
S
=
6.97
×
10
8 L/mg
0.971
Q
max = 0.0130 mg/g
n
=
0.24Figure 1
Langmuir adsorption isotherm and experimental data of KKP extract.


### 3.2.2. Freundlich Isotherm

The Freundlich isotherm explains that the extent of adsorption varies directly with pressure. This empirical relationship describes the multilayer adsorption of heterogeneous systems and assumes that different sites have several adsorption energies involved [18]. The linear model of the isotherm can be expressed logarithmically as in
(5)
log
q
e
=
1
n
log
C
e
+
log
K
F
.The values of parametersK
F and n (listed in Table 2) can be determined from the intercept and slope of the plot log
C
e against log
q
e (Figure 2), where K
F (1/g) is the Freundlich adsorption capacity constant and 1/n is related to the adsorption intensity constant that varies with the heterogeneity of the adsorbate.Figure 2
Freundlich adsorption isotherm and experimental data of KKP extract.


### 3.2.3. Redlich-Peterson Isotherm

The Redlich-Peterson (R-P) isotherm is a three-parameter empirical adsorption model that incorporates elements from both the Langmuir and Freundlich isotherms [15] and amends the inaccuracies. The adsorption mechanism is unique and does not follow ideal monolayer adsorption characteristics. The linear expression of the R-P isotherm model is defined as [15]
(6)
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
,
where K
R is the Redlich-Peterson adsorption capacity constant determined via trials and errors to obtain the maximum linear regression value of the isotherm graph (Figure 3). The parameter a
R is the R-P isotherm constant and b
R is the exponent between 0 and 1. Numerous studies [19–24] have shown that the R-P isotherm was more accurate than the Langmuir and Freundlich isotherms as it contains three unknown parameters. The reason for this is that the Langmuir and Freundlich isotherms can be derived from the R-P isotherm. When b
R = 1, the R-P equation becomes the Langmuir isotherm equation and when b
R
=
0, it is closer to the Freundlich equation. However, the accuracy of these interpretations strongly depends on the fitting method [25–28].Figure 3
Redlich-Peterson adsorption isotherm and experimental data of KKP extract.


### 3.2.4. Sips Isotherm

The Sips isotherm is derived from the limiting behavior of the Langmuir and Freundlich isotherms. The model is valid for localized adsorption without adsorbate-adsorbate interactions [15]. When C
e approaches a low value, the Sips isotherm effectively reduces to Freundlich, while at high C
e, it predicts the Langmuir monolayer sorption characteristic. The Sips linear equation model is expressed as [15]
(7)
1
q
e
=
1
Q
max
K
S
(
1
C
e
)
1
/
n
+
1
Q
max
,
where K
S (1/mg) and Q
max (mg/g) are the Sips equilibrium constant and maximum adsorption capacity values obtained from the slope and the intercept of the plot (Figure 4). The Sips isotherm equation is characterized by the dimensionless heterogeneity factor, n, which can also be employed to describe the system’s heterogeneity when n is between 0 and 1. When n
=
1, the Sips equation reduces to the Langmuir equation and it implies a homogeneous adsorption process [21].Figure 4
The Sips adsorption isotherm and experimental data of KKP extract.The parameters and correlation coefficient (R
2) for each of the equilibrium isotherm models of the adsorption process are shown in Table 2. The Redlich-Peterson model clearly shows poor correlation (R
2
=
0.657) to the experimental data. Similarly, the Freundlich isotherm model that assumes an exponential increase in the adsorption amount does not fit well with data (R
2
=
0.893). Both the Langmuir (R
2
=
0.915) and Sips isotherm (R
2
=
0.971) models show good fit to experimental data. However, heterogeneous adsorption process is evidently indicated from the heterogeneity factor value (n
=
0.24). Thus, the isotherm that best describes the adsorption behavior of KKP extract pigments onto the TiO2 nanoparticles is the Sips isotherm.


## 3.2.1. Langmuir Isotherm

The Langmuir adsorption isotherm model explains the variation of adsorption of molecules (adsorbates) with pressure. The isotherm is based on the assumption that maximum adsorption occurs when a saturated monolayer of adsorbate molecules is present on the adsorbent surface, the energy of adsorption is constant, and there is no migration or interaction between the adsorbate molecules in the surface plane [16, 17]. The linear expression of the Langmuir isotherm model is defined by
(3)
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
.By plotting the linear graph of 1/q
e against 1/C
e, the values of K
L and q
m can be determined from the intercept and slope of the plot (Figure 1), where the parameter q
m (mg/g) is the maximum adsorption capacity of dye per unit mass of sorbent to form a complete monolayer on the surface bound at high C
e and K
L (L/mg) is the Langmuir energy constant which is related to the heat of adsorption. Table 2 presents the values of Langmuir constants (q
m
=
0
.
0468 mg/g, K
L
=
28.489 L/mg). The essential characteristics of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor R
L that is given by
(4)
R
L
=
1
(
1
+
K
L
C
i
)
,
where C
i (mg/L) is the highest initial concentration of adsorbate and R
L values between 0 and 1 imply favorable adsorption. The value of R
L in the present investigation was calculated to be 0.45 which indicates favorable adsorption of KKP extract pigments onto TiO2 nanoparticles surface.Table 2
Parameters and correlation coefficient (R
2) of equilibrium isotherm models for the adsorption of KKP extract pigments onto TiO2 nanoparticles.
Isotherm
Equation
Parameters
R
2
Langmuir
1
q
e
=
1
q
m
K
L
·
1
C
e
+
1
q
m
K
L = 28.489 L/mg
0.915
q
m = 0.047 mg/g
Freundlich
log
q
e
=
1
n
log
C
e
+
log
K
F
K
F = 0.225 (1/g)
0.893
1
n = 0.69
Redlich-Peterson
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
K
R = 10 mg/g
0.657
a
R = 45.814 mg/L
b
R = 0.335
Sips
1
q
e
=
1
Q
max
K
s
(
1
C
e
)
1
/
n
+
1
Q
max
K
S
=
6.97
×
10
8 L/mg
0.971
Q
max = 0.0130 mg/g
n
=
0.24Figure 1
Langmuir adsorption isotherm and experimental data of KKP extract.


## 3.2.2. Freundlich Isotherm

The Freundlich isotherm explains that the extent of adsorption varies directly with pressure. This empirical relationship describes the multilayer adsorption of heterogeneous systems and assumes that different sites have several adsorption energies involved [18]. The linear model of the isotherm can be expressed logarithmically as in
(5)
log
q
e
=
1
n
log
C
e
+
log
K
F
.The values of parametersK
F and n (listed in Table 2) can be determined from the intercept and slope of the plot log
C
e against log
q
e (Figure 2), where K
F (1/g) is the Freundlich adsorption capacity constant and 1/n is related to the adsorption intensity constant that varies with the heterogeneity of the adsorbate.Figure 2
Freundlich adsorption isotherm and experimental data of KKP extract.


## 3.2.3. Redlich-Peterson Isotherm

The Redlich-Peterson (R-P) isotherm is a three-parameter empirical adsorption model that incorporates elements from both the Langmuir and Freundlich isotherms [15] and amends the inaccuracies. The adsorption mechanism is unique and does not follow ideal monolayer adsorption characteristics. The linear expression of the R-P isotherm model is defined as [15]
(6)
ln
(
K
R
C
e
q
e
-
1
)
=
b
R
ln
C
e
+
ln
a
R
,
where K
R is the Redlich-Peterson adsorption capacity constant determined via trials and errors to obtain the maximum linear regression value of the isotherm graph (Figure 3). The parameter a
R is the R-P isotherm constant and b
R is the exponent between 0 and 1. Numerous studies [19–24] have shown that the R-P isotherm was more accurate than the Langmuir and Freundlich isotherms as it contains three unknown parameters. The reason for this is that the Langmuir and Freundlich isotherms can be derived from the R-P isotherm. When b
R = 1, the R-P equation becomes the Langmuir isotherm equation and when b
R
=
0, it is closer to the Freundlich equation. However, the accuracy of these interpretations strongly depends on the fitting method [25–28].Figure 3
Redlich-Peterson adsorption isotherm and experimental data of KKP extract.


## 3.2.4. Sips Isotherm

The Sips isotherm is derived from the limiting behavior of the Langmuir and Freundlich isotherms. The model is valid for localized adsorption without adsorbate-adsorbate interactions [15]. When C
e approaches a low value, the Sips isotherm effectively reduces to Freundlich, while at high C
e, it predicts the Langmuir monolayer sorption characteristic. The Sips linear equation model is expressed as [15]
(7)
1
q
e
=
1
Q
max
K
S
(
1
C
e
)
1
/
n
+
1
Q
max
,
where K
S (1/mg) and Q
max (mg/g) are the Sips equilibrium constant and maximum adsorption capacity values obtained from the slope and the intercept of the plot (Figure 4). The Sips isotherm equation is characterized by the dimensionless heterogeneity factor, n, which can also be employed to describe the system’s heterogeneity when n is between 0 and 1. When n
=
1, the Sips equation reduces to the Langmuir equation and it implies a homogeneous adsorption process [21].Figure 4
The Sips adsorption isotherm and experimental data of KKP extract.The parameters and correlation coefficient (R
2) for each of the equilibrium isotherm models of the adsorption process are shown in Table 2. The Redlich-Peterson model clearly shows poor correlation (R
2
=
0.657) to the experimental data. Similarly, the Freundlich isotherm model that assumes an exponential increase in the adsorption amount does not fit well with data (R
2
=
0.893). Both the Langmuir (R
2
=
0.915) and Sips isotherm (R
2
=
0.971) models show good fit to experimental data. However, heterogeneous adsorption process is evidently indicated from the heterogeneity factor value (n
=
0.24). Thus, the isotherm that best describes the adsorption behavior of KKP extract pigments onto the TiO2 nanoparticles is the Sips isotherm.


## 3.3. Zeta-Potential and Photovoltaic Performance in DSSC

For KKP extract, zeta-potential of −9.48 mV was obtained. This indicates the tendency of anthocyanin pigment molecules coagulating at its original pH (~5), which correlates well with the pigment’s adsorption characteristics as explained by the Sips isotherm.The DSSC performance was examined using the current-voltage characteristics, as shown in Figure5. The values obtained for open circuit voltage (V
OC), short circuit current density (J
SC), and fill factor (
f
f
) were 0.448 V, 3.177 mA/cm2, and 0.52, respectively. Although monolayer adsorption condition is favorable for the photoconversion of DSSC anode [29], the KKP extract that showed multilayer adsorption characteristics has demonstrated its capability of sensitizing DSSCs while giving a photoenergy conversion efficiency of 0.83%.Figure 5
I
-
V characteristics of DSSC sensitized with KKP extract.


## 4. Conclusions

The adsorption behavior of KKP extract containing anthocyanin onto TiO2 nanoparticles surface was investigated. Experimental data were modeled using the Langmuir, Freundlich, Redlich-Peterson, and Sips isotherms. Equilibrium adsorption of KKP extract pigments onto TiO2 was well described by the Sips model with a heterogeneous adsorption capacity of 0.0130 mg/g. Zeta-potential data revealed the tendency of pigment molecule coagulation in the solvent. This phenomenon correlated well with its adsorption behavior. From I
-
V analysis, a photo-energy conversion efficiency of 0.83% was obtained indicating that the Kuduk-kuduk fruit-pulp extraction has the potential to be integrated into the dye-sensitized solar cell system as a viable sensitizer.



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*Source: 468975-2014-01-12.xml*