IHJPAS. 36(1)2023 

186 
This work is licensed under a Creative Commons Attribution 4.0 International License 

 

   

 

 

Study the Interaction Adsorptive Behavior of Sunset Yellow Dye and 

Loratadine Drug: Kinetics and Thermodynamics Study 

 

 

 
 

 

 

Abstract 

The performance of drug treatment and assessments of different drugs' side effects both can be 

affected by the interaction between food additives and drugs. Organic compounds such as food 

colorants dyes are utilized as additives in a wide range of foods. In this study, the adsorption 

interaction behavior between the colorant food dye sunset yellow (SY) and the drug loratadine was 

examined. The adsorption procedure is conducted at different drug dosages, various SY dye 

concentrations, and different temperature (288-318K). The equilibrium data were explained by 

using Freundlich and Langmuir adsorption isotherms, but Langmuir offering the best fit model. 

Kinetics adsorptive behavior of sunset yellow on loratadine matched pseudo-second order kinetics. 

Thermodynamics study show that the process is exothermic, spontaneous and the disorder at the 

solid-solution interface was proven from the negative entropy (-140.556 J/ K.mol) of adsorption 

process. 

.Thermodynamics, Adsorption, Kinetics, Loratadine: Sunset Yellow, Key words 

1. Introduction  

The performance of pharmacological treatment and evaluation of many drugs' adverse reactions 

can both be influenced by the interaction between food additives and drugs. Some pharmaceuticals 

cannot be taken with particular foods because they include chemical components such as dyes, 

which can induce a reaction that alters the drug's effect. It also can cause or exacerbate negative 

effects [1]. 

Nowadays, the majority of food dyes are synthesized and derived from petroleum and coal tar. In 

reality, consumption of artificial food dyes has risen by 500% in the previous 50 years, with 

children being the main consumers [2]. 

doi.org/10.30526/36.1.2974 

Article history: Received  8 Augest 2022, Accepted  27 September 2022, Published in January 2023. 

 

 

 

Ibn Al-Haitham Journal for Pure and Applied Sciences 

Journal homepage: jih.uobaghdad.edu.iq 

 

Furat A. Hiawi 

Department of Chemstry , College of Science for 

Women, University of Baghdad, 

Baghdad, Iraq. 

Abdulallah1205a@csw.uobaghdad.edu.iq 

 

 

 

Inaam H. Ali 

Department of Chemstry , College of 

Science for Women, University of 

Baghdad,Baghdad, Iraq. 

inaam.mohmmed@gmail.com 

 

 

https://creativecommons.org/licenses/by/4.0/
mailto:Abdulallah1205a@csw.uobaghdad.edu.iq
mailto:Abdulallah1205a@csw.uobaghdad.edu.iq
mailto:inaam.mohmmed@gmail.com


IHJPAS. 36(1)2023 
 

187 

Food coloring dyes may be harmful and have no important nutrients, and can cause a number of 

diseases, such as cancer and allergies [3]. Synthetic dyes are bioaccumulate so they have adverse 

environmental effects, carcinogenic effects, causing metabolic disorders and genetic problems 

especially if they are used in large quantities. [4]. Children who consume too many food dyes may 

suffer a number of negative effects, including allergies, hyperactivity, and attention deficit 

disorders [5]. The health consequences of these dyes are negligible because they are regarded as 

safe when used in accordance with authorized production techniques. 

Since each government regulates all types and levels of food dyes that are authorized, the 

investigations were shown that some dyes are used at quantities over the limit permissible, 

exposing consumers at significant risks [6]. 

Sunset yellow (SY) is a synthesized compound contains azo groups (Figure 1). It is soluble in 

water, slightly soluble in ethanol, have IUPAC name disodium, 6-hydroxy-5-(4-sulfonatophenyl) 

diazenyl) naphthalene-2-sulfonate [7]. Many production processes, like those in the food, 

pharmaceuticals, cosmetic, textile, and leather trades, utilize sunset yellow as a colorants material. 

When these azo dyes are used frequently, it could really lead to many health risks such allergic 

reactions, chromosomal abnormalities, and hyperactivity in children [8]. 

S

HO

O

O

ONa

NN

S

O

O

NaO

 
Figure 1. Structure of sunset yellow 

Contrarily, drugs administered as pharmaceuticals are often aromatic hydrocarbons compounds 

that have an effect on the whole organism. Generally, the therapeutic effects of these drugs seen 

with daily use may be enhanced in an overdose [9]. 

Antihistamine drugs like loratadine (Figure 2) are used to treat the allergy symptoms. It is usually 

used to treat the hives, a rash, itchy eyes, runny nose, nasal congestion, and nasal congestion [10]. 

Due to its poor ability to dissolve, loratadine has a rate-limiting step in the absorption process. 

Loratadine has a low variable oral absorption considering that it is practically insoluble in water 

[11]. 

N

N

C OCH2CH3

O

Cl

 

Figure 2. Loratadine chemical structure 

The hazards of interactions between food dye and insoluble or weakly soluble drugs in water have 

not yet been studied. If the additives in food like colorant dyes adsorb on such drugs, it cause an 

interaction that may decrease the efficiency of the treatments in curing diseases and increasing 

their biocompatibility within the body. 



IHJPAS. 36(1)2023 
 

188 

Taking into account the health risks that food dyes cause to humans, the objective for carrying out 

this investigation is to study that how food dye sunset yellow and the drug loratadine interact 

during the adsorption process. To illustrate the equilibrium in processes, various adsorption 

isotherms will be employed such as the Langmuir and Freundlich models. Kinetics and 

thermodynamics parameters of the process will be used to assess the feasibility of the adsorption 

process 

 

2. Materials and Experiments 

          Loratadine was provided by a state company in Samarra for the production of 

pharmaceuticals and medical equipment. Sunset yellow dye was supplied from locally Market. 1 

g of the dye was accurately dissolved in one liter of distilled water to obtain 1000gL-1 of sunset 

yellow stock solution. Shimadzu double-beam UV-Vis spectrophotometer was used to determine 

the absorbance of different concentrations (10-60 mg/L) of sunset yellow dye which were prepared 

by diluting the appropriate dye stock solution in accordance with the calibration curve and 

adsorption process requirements. At a wavelength of 480 nm, sunset yellow's maximum absorption 

was detected as in Figure (3). 

 

Figure 3. The UV-Visible spectra of sunset yellow dye. 

For building the calibration curve of sunset yellow dye, a range of concentrations of sunset yellow 

dye (10–60 mg/L) were made from stock solution, and the absorbance for each concentration was 

observed as shown in figure (4) at its optimum wavelength (480 nm). 

 

Figure 4. Calibration curve of sunset yellow 

y =0.0337x
R² =0.9993

0

0.5

1

1.5

2

0 10 20 30 40 50 60 70

A
b

so
rb

a
n

ce

Conc.

https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751
https://discovery.nationalarchives.gov.uk/details/c/F162751


IHJPAS. 36(1)2023 
 

189 

To investigate that how process is influenced by different factors, such as SY concentration, 

loratadine amount, contact time, and temperature, batch adsorption studies have been carried out. 

The quantity of SY adsorbed on the loratadine drug's surface was calculated using the formula 

below: 

𝑞𝑒 =  
(𝐶0 −  𝐶𝑒 ) 𝑉

𝑤
                    (1) 

 

Where V represents for the volume of the solution (L), the mass of the drug w is (g), and C0 and 

Ce are the concentrations of SY (mg/L) at initial and equilibrium, respectively. 

For a 30 mg/L of SY dye solution, the effects of many adsorbent dosages (0.05, 0.1, 0.15, 0.2, and 

0.25 g) in 50 mL of dye were investigated. The thermostatic shaker bath's agitation speed was set 

at 200 rpm for all the experimental steps, and the temperature was kept constant at 298 K. 

To evaluate the effect of contact time on the adsorption process of SY, 0.1g of loratadine drug was 

added to 50 mL of SY solution (30 mg/L) in 250 mL flasks. 5mL of the sample was drawn out 

every 10 minutes, and until equilibrium is achieved, the concentration was determined. The 

adsorption process was studied at temperatures in the range 288–318 K to examine the effect of 

temperature on the process. 

 

3. Results and Discussion: 

Effect of Drug Dosage 

Because it directly influences an adsorbent's capacity at a specific initial concentration of 

adsorbate, the dosage of an adsorbent is a significant factor to be studied. A series of adsorption 

experiments were conducted with various adsorbent doses from (0.05g - 0.25g) in 50 ml of initial 

concentration 30 mg/ L SY dye and at constant contact time to examine the effects of drug dosage 

on the adsorption of SY. 

Figure (5) reveals that using 0.1g of loratadine increases the amount of SY adsorbed with drug 

dosage enhancement to its maximum value. 

In fact, the dye adsorption remained approximately constant as the dose of the drug was increased, 

and then it decreased as the dosage was increased. Additional dye was adsorbed when the dosage 

of the drug was increased until equilibrium was reached. This due to the competition between 

adsorbent molecules for adsorption as well as the influence of the variation in SY molecules 

concentration and drug quantity [12]. The use of this adsorbent dose was confirmed in all 

experiments. 

 

 

 

Figure 5. Effect of drug quantity on the amount of sunset yellow absorbed 

4

6

8

10

0 0.05 0.1 0.15 0.2 0.25

q
e

(m
g

/g
)

Drug dosage (g)



IHJPAS. 36(1)2023 
 

190 

Effect of initial concentration and contact time 

The impact of contact time on dye adsorption was assessed throughout a variety of times and initial 

dye concentrations, ranging from 10 to 50 mg L-1, as shown in Figure (6). It was revealed that the 

adsorption process began rapidly and slowed down after the initial contact time. To attain 

equilibrium in the adsorption of SY on the drug, it required 50 min to reach equilibrium then the 

amount of dye adsorption did not significantly alter over time. This is possible because vacant 

surface sites are available during the initial stages of adsorption, but after some time passes, the 

vacant sites become filled by dye molecules [13]. The relating plot Figure (6) illustrates how the 

amount of SY adsorbed depends on changing initial SY concentration and rises with initial SY 

concentration enhancement. 

 

Figure 6. Contact time and initial SY concentration's effect on the adsorption process. 

Adsorption Isotherm  

Understanding the interaction between the amounts adsorbed of the food colorant sunset yellow 

on the surface of the drug at equilibrium is facilitated by adsorption isotherms. The relationship 

between amount adsorbed and dye concentration at equilibrium illustrates in Figure (7). This 

figure shows the curve has an S-shape because of the small initial slope followed by a fast rise. 

Based on this specific isotherm, the affinity of the adsorptive surface is enhance with higher initial 

concentration and decreases with it droplets [14]. 

 
Figure 7.Adsorption isotherm of SY on loratadine at 298K. 

The experimental data were tested to match the Freundlich and Langmuir adsorption models. 

Langmuir model, which affirmatively assume a monolayer, homogeneous and confined adsorption 

site. It is possible that a minimum threshold after which no further adsorption will take place. The 

0

2

4

6

8

10

12

14

0 10 20 30 40 50 60

q
e

(m
g

/g
)

Time (min)

20 mg/L

30 mg/L

40 mg/L

50 mg/L

0

3

6

9

12

15

0 4 8 12 16 20 24

q
e

 (
m

g
/g

)

Ce (mg/L)



IHJPAS. 36(1)2023 
 

191 

Langmuir equation is established and given as follows equation (2) for a surface with a small 

number of similar locations and monolayer saturation [15]: 

𝐶𝑒
𝑞𝑒

=  
1

𝐾𝐿 . 𝑄°
+

𝐶𝑒
𝑄°

                    (2) 

Where the Langmuir constants Q° (mg/g) and KL (L/mg) are represented. KL is roughly the energy 

adsorption constant, and Q° is the maximum adsorption capacity. The Langmuir constants Q° and 

KL were obtained from the slope and interception of a linear plot of Ce/qe against Ce, respectively. 

Figure (8) depicts the application of the Langmuir isotherm equation to the experimental data of 

adsorption SY dye on the drug adsorbent.  

 

Figure 8. The Langmuir isotherm of SY adsorption of  

The Langmuir isotherm is used to construct the Freundlich isotherm [16], which requires a 

heterogeneous surface with an adsorption capacity and is given by: 

ln 𝑞𝑒 = ln 𝐾𝑓 +
1

𝑛
 𝑙𝑛𝐶𝑒                       (3) 

The efficiency of adsorption is proportional to the dimensionless constant n, and the capacity of 

adsorption is related to the Freundlich constant (mg/L), or Kf. The value of n denotes how nonlinear 

the relationship is between the adsorption process and concentration of adsorbate. Figure (9) 

illustrates how the values of Kf and n were calculated from the intercept and slope of the fitted line 

of lnqe against ln Ce, respectively.. 

 

Figure 9. The Freundlich isotherm of SY adsorption 

y =0.0558x +0.4958
R² =0.9589

0

0.2

0.4

0.6

0.8

1

1.2

1.4

1.6

1.8

2

0 5 10 15 20 25

C
e
/q

e

Ce

y =0.5247x +0.985
R² =0.9139

0.5

1

1.5

2

2.5

3

0.5 1 1.5 2 2.5 3 3.5

ln
 q

e

ln Ce



IHJPAS. 36(1)2023 
 

192 

It is clear from the findings in Table 1 and based on the R2 (regression coefficients), the Langmuir 

model was higher from that predicted by Freundlich This demonstrated that the results of the SY 

dye's adsorption onto the drug were well fitted by the Langmuir model. n values greater than unity 

showed a good synergistic association and a heterogeneous binding arrangement [17]. 

Furthermore, the Langmuir equation's estimate of maximal monolayer capacity (Q0) showed a 

reduction in value with rising temperature, indicating an increase in adsorption capacity at low 

temperatures. 

Table 2. Adsorption isotherm parameters of SY dye on drug. 

Isotherm Langmuir model Freundlich model 

Temperature (K) R2 Q⁰ (mg/g) KL(Lmg
-1) R2 Kf (Lmg

-1) n 

288 0. 9874 19.08 0.129 0.9791 3.125 1.946 

298 0.9589 17.92 0.112 0.9139 2.667 1.905 

308 0.9513 19.34 0.063 0.9468 1.679 1.594 

318 0.9764 24.44 0.033 0.988 1.102 1.372 

 

Adsorption Kinetics  

          The rate constant and mechanisms of SY adsorption on drug surface were determined using 

two kinetics models. These models are Lagergren-first-order equation and the pseudo-second-

order equation which have been used to investigate the adsorption kinetic behavior of SY (30 

mg/L) onto drug at temperatures ranged (288-318K). The best-fit was selected based on the results 

of the linear regression correlation coefficient (R2).  

The linear formula pattern of the pseudo-first order kinetic model is as follows (18): 

log(𝑞𝑒 − 𝑞𝑡 ) = 𝑙𝑜𝑔𝑞𝑒 −(𝑘1/2.303) 𝑡                         (4)  

Where k1 is the rate constant of the pseudo-first order kinetics (min
-1), The quantity of SY adsorbed 

on the drug's surface at equilibrium is termed as qe, and the quantity at any given time is termed as 

qt. The qe and k1 are frequently estimated using the intercept and slope of plots of log (qe - qt) vs t, 

respectively. In Figure 10, the result of such a plot is shown. 

 

Figure 10. Adsorption kinetics pseudo-first order of SY on drug dye at 298K 

The pseudo-second order kinetic model in linear form (19) is as follows: 

𝑡

𝑞𝑡
=

1

𝑘2𝑞𝑒
2

+ (
1

𝑞𝑒
) 𝑡                        (5) 

y =-0.0363x +0.98
R² =0.9592

-0.8

-0.6

-0.4

-0.2

0

0.2

0.4

0.6

0.8

0 10 20 30 40 50

lo
g

 q
e
-q

t

Time (min)



IHJPAS. 36(1)2023 
 

193 

Where k2 is the pseudo-second order kinetics rate constant (g.mg
-1.min-1). The intercept and slope 

of plots of t/qt against t were obtained to calculate k2 and qe, as shown in Figure 11. 

 

Figure 11. Adsorption kinetics pseudo-second order of SY on drug dye at 298K 

      As illustrated in Table 2, the value (R2) of the two models are approximately identical, 

although the pseudo-second order equation's R2 value is significantly higher. According to this, the 

pseudo second order kinetic model described the kinetics of the adsorption system more precisely 

than the pseudo-first order model. 

 

 

Table 2. Kinetics data of SY dye adsorption on drug. 

Kinetics models Pseudo First order Pseudo Second order 

Temperature (K) R2 k1 (min
-1) qe (mg/g) R

2 k2(g mg
-1 min-1) qe (mg/g) 

288 0.9428 0.0637 5.193 0.9962 0.0166 10.775 

298 0.9592 0.0835 9. 549 0.9962 0.0092 11.312 

308 0.9576 0.0852 5.591 0.9956 0.0163 9.310 

318 0.9484 0.0817 12.723 0.994 0.0023 13.020 

 

Thermodynamic Study 

          At four different temperatures in the range of (288- 318 K), adsorption studies were carried 

out to estimate the thermodynamic properties (free energy function (∆G°), enthalpy function 

(∆H°), and entropy function (∆S°). 

The thermodynamic properties were determined using these equations [20]: 

∆𝐺° = −𝑅𝑇 ln 𝐾𝐿                       (6) 

ln 𝐾𝑐 =
∆𝑆°

𝑅
−

∆𝐻°

𝑅𝑇
                    (7) 

Where T is the temperature in kelvin, Kc is the equilibrium constant (L/g), and R is the value of 

the gas constant in joules (8.314 J/mol K). The van't Hoff plots of ln(Kc) against 1/T were used to 

y =0.0884x +0.8456
R² =0.9962

0

1

2

3

4

5

6

0 10 20 30 40 50 60

t/
q

t

Time (min)



IHJPAS. 36(1)2023 
 

194 

estimate the values of (∆H°) and (∆S°). Plotting of this relationship is illustrated in e Figure (12) 

represents this plotted relation and Table (3) depicts the thermodynamic parameters derived at 

various temperatures. The negative values of ∆G° provide as evidence for the feasibility and nature 

of spontaneous adsorption. The fact that the negative value of ∆G° diminishes as temperature rises 

suggests adsorption of SY on lotatadine is preferable and more strongly at low temperature. 

As shown, the exothermic aspect of the process was proven by the negative value of (∆H°) (-

40.276 kJ/mol). Likewise, practically, (∆H°) has a value approximately 40 kJ/mol. This indicated 

that adsorption of SY onto loratadine was a physical process [21]. 

 

Figure 12. Van't Hoff plots for SY adsorption on loratadine 

Entropy (∆S°) is an indicator of randomness and show how a system's solid/liquid interface varies 

with temperature. Its negative value (-140.556 J/K mol) indicates the adsorption system tends to 

make the solid/liquid interface less irregular [22]. 

 

 

Table 3: Thermodynamic properties of the adsorption of SY on drug. 

 

 

 

 

4. Conclusions 

    Precautions must be considered prior to clinical instances because of the prevalence of drugs 

and food colorant dye interactions globally. The interaction in this study was clarified by 

adsorption of the food additive sunset yellow dye and the drug loratadine. The most effective 

model for illustrating the adsorption isotherm of SY dye onto the drug loratadine was observed to 

be the Langmuir isotherm model. The pseudo-second order equation can be used to explain the 

kinetics of SY adsorption on the drug loratadine, because it closely matched the results of the 

experiments. Thermodynamic study confirms that the SY adsorption onto loratadine was 

exothermic and spontaneous. The SY adsorption on loratadine is physisorption, as evidenced by 

the negative ∆H° value, which is -40.276 kJ/mol. 

 

y =4844.4x-16.906
R² =0.9208-1.8

-1.6

-1.4

-1.2

-1

-0.8

-0.6

-0.4

-0.2

0

0.0031 0.0032 0.0033 0.0034 0.0035

ln
 K

L

1/T

Temp.(K) ∆G° (kJ/mol) ∆H°(kJ/mol) ∆S° (J/K.mol) 

288 -0.224 -40.276 -140.556 

298 -0.365 

308 -1.319 

318 -1.676 



IHJPAS. 36(1)2023 
 

195 

Conflict of interest 

No actual conflict of interest that could have influenced this study. 

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http://dx.doi.org/10.1007/s13738-022-02500-3
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	Conflict of interest
	7. Kong, Q.;  Liu Qun ;  M. Miao  ;   Liu, Y.  ;   Chen , Q.;  Zhao, C., Kinetic and equilibrium studies of the biosorption of sunset yellow dye by alligator weed activated carbon.,  Treatment. 2017 ,66, 281-290.