Removal of Basic Blue 41 dyes using Persea americana-activated carbon prepared by phosphoric acid action

  • Abdelmajid Regti
  • My Rachid Laamari
  • Salah-Eddine Stiriba
  • Mohammadine El Haddad
Open Access

DOI: 10.1007/s40090-016-0090-z

Cite this article as:
Regti, A., Laamari, M.R., Stiriba, SE. et al. Int J Ind Chem (2017) 8: 187. doi:10.1007/s40090-016-0090-z


Adsorption study of Basic Blue 41 dye onto activated carbon from Persea americana nuts with phosphoric acid activation was achieved. The effect of operating parameters, the effect of pH (2–12), adsorbent amount (5–30 mg/50 mL), dye concentration (25–125 mg/L), contact time (0–200 min) and temperature (298–323 K), on the adsorption capacity was examined. The experimental isotherm data were analyzed using Langmuir and Freundlich models, which showed that the best fit was achieved by the Langmuir model with the maximum monolayer adsorption capacity at 625 mg/g. The adsorption kinetic process followed pseudo-second-order kinetics. Thermodynamic evaluation showed that the process was endothermic (ΔH0 = 144.60 kJ/mol) and spontaneous (ΔG0 varied from to −11.64 to −19.50 kJ/mol), while the positive value of entropy (ΔS0 = 524.3 J/mol K) revealed increased randomness at the adsorbent–adsorbate interface. It was found to be a very efficient adsorbent and a promising alternative for dye removal from aqueous solutions.


Removal of dye Persea americana-activated carbon Surface area Adsorption Kinetics and thermodynamic studies 


The textile industry plays a part in the economy of several countries around the world. However, effluents from textile and dyeing have a low biological oxygen demand and strong chemical oxygen demand. Disposal of this colored water into receiving water can be toxic to aquatic life and cause food chain contamination, resulting in deleterious health effect even in very low concentrations. Moreover, most of these dyes can cause allergy, dermatitis, skin irritation and also provoke cancer and mutation in humans [1, 2]. Dyes are usually highly visible, very difficult to biodegrade, and extremely difficult to eliminate in natural aquatic environments [3, 4].

To improve the effluent quality, the addition of physical and/or chemical treatments comprising adsorption [5, 6, 7, 8, 9], photocatalytic [10, 11] or electrochemical methods [5] and reverse osmosis [12] are necessary. Adsorption is the most simple and known for the treatment of effluents containing dyes using the new low-cost and environmentally friendly adsorbents in the carbon-based or not activated means [13, 14, 15, 16, 17, 18].

The potential properties of activated carbon as adsorbents are due to their highly developed porosity, favorable pore size distribution, large surface area, and high degree of surface reactivity [19]. Chemical activation and physical activation are two methods for the preparation of activated carbon. Chemical activation uses chemical agents for the preparation of activated carbon in a single step method, while physical activation involves carbonization of carbonaceous materials followed by activation of the resulting substrate in the presence of dioxide carbon or steam as activating agents [20]. It is recognized that the carbon yields of chemical activation are higher than the physical one. The most common precursors used for the production of activated carbon are organic materials that are rich in carbon.

Several studies to find low-cost carbonaceous materials have been reported. These materials include Jerusalem artichoke [21], waste rice hulls [22], homemade cocoa shell [23], waste tea [24], coir pith [25], orange peels [26], jute sticks [27], walnut [28], palm oil shell [29], Acacia mangium wood [30] and waste tires [31].

In the present study, we examine the feasibility of using activated carbon prepared using Persea americana as adsorbent for the removal of Basic Blue 41 dyes from aqueous solutions. The effect of different parameters including solution pH, adsorbent dosage, dye concentration, temperature and contact time were studied to optimize the adsorption process. The isotherm and kinetic and thermodynamic parameters were examined to analyze the experimental data.

Materials and methods

The Persea americana nuts were collected, washed with distilled water and dried at ambient temperature for several days. The unmodified Persea americana nuts were abbreviated as PAN. The carbonization of PAN was carried out using an appropriate weight of PAN and 25 mL concentrated phosphoric acid with a mass ratio (1:4). A glass beaker of 100 mL was heated to 500 °C for 1 h producing a black carbonaceous residue. The solid material was neutralized with KOH solution until a neutral pH was obtained. The resulting carbonized Persea americana nut (C-PAN) was filtered and washed intensively with water. The C-PAN was then dried at 100 °C for 2 h and kept in desiccators for further use.

The characterization of C-PAN was achieved by FT-IR spectroscopy and X-ray powder diffraction measurements. FT-IR spectra (4000–450 cm−1 range) were recorded with a Nicolet 5700 FT-IR spectrometer on samples prepared as KBr pellets. The polycrystalline sample of each adsorbent was lightly ground in an agate mortar and pestle and filled into 0.5 mm borosilicate capillary prior to being mounted and aligned on an Empyrean PANalytical powder diffractometer using Cu Kα radiation (λ = 1.54056 Å). Three repeated measurements were obtained at room temperature in the 10° < 2θ < 60° range with a step size of 0.01°. Scanning electronic microscopy (SEM) images were obtained with HITACHI-S4100 equipment operated at 20 kV.

Adsorption–desorption isotherms of nitrogen at −196 °C were measure with an automatic adsorption instrument (NOVA-1000 Gas Sorption analyzer) to determine the surface areas and total pore volumes. The BET surface area and the total pore volumes of the obtained Persea americana-activated carbon were found to be 1593 and 1.053 cm3/g, respectively.

Deionized water was used throughout the experiments for solution preparation. The adsorption studies for evaluation of the C-PAN adsorbent for the removal of the Blue Basic 41 dye from aqueous solutions were carried out in triplicate using the batch contact adsorption method. Basic Blue 41 dye used in this study, abbreviated as BB41, was purchased from Sigma-Aldrich. The chemical structure of BB41 is shown in Fig. 1.
Fig. 1

The chemical structure of Basic Blue 41

For the adsorption experiments, fixed amounts of adsorbents (5–30 mg) were placed in a 100 mL glass Erlenmeyer flask containing 50 mL of dye solution at various concentrations (25–125 mg/L), which were stirred for a suitable time (5–200 min) from 293 to 313 K. The pH of the dye solutions ranging from 2 to 10 was adjusted by 0.1 M HCl or 0.1 M NaOH to investigate the effect of pH on the adsorption processes. Subsequently, to separate the adsorbents from the aqueous solutions, the samples were centrifuged at 3600 rpm for 10 min, and aliquots of 1–10 mL of the supernatant were taken. At a predetermined time, the residual dye concentration in the reaction mixture was analyzed by centrifuging the reaction mixture and then measuring the absorbance by UV–visible spectroscopy of the supernatant at the maximum absorbance wavelength of the sample at 606 nm.

The amount of equilibrium adsorption qe (mg/g) was calculated using the formula:
$$q_{\text{e}} = \frac{{C_{0} - C_{\text{e}} }}{W}V,$$
where Ce (mg/L) is the liquid concentration of the dye at equilibrium, C0 (mg/L) the initial concentration of the dye in solution, V the volume of the solution (L) and W the mass of the dye biosorbent (g). The BB41 removal percentage (%) can be calculated as follows:
$$\% \text{Re} {\text{moval}} = \frac{{C_{0} - C_{\text{e}} }}{{C_{0} }}\; \times \;100,$$
where C0(mg/L) is the initial dye concentration and Ce (mg/L) is the concentration of the dye at equilibrium.

Results and discussion

Characterization of C-PAN adsorbent

To investigate the surface characteristics of the C-PAN adsorbent, FT-IR and XRD spectra were recorded. As shown in the FT-IR spectrum in Fig. 2, the frequencies of the absorption bands of C-PAN are 876, 1074, 1149, 1563, 2916 and 3415 cm−1. The absorption band at 3415 cm−1 is attributed to the hydroxyl group (O–H) vibration [32]. The bands at 2916, 1563 and 1381 cm−1 correspond, respectively, to unsymmetrical aliphatic C–H stretching, C=C stretching of aromatic rings and aromatic C=C stretching vibration. The band at 1149 cm−1 is ascribed to C–O stretching in alcohol or ether or the hydroxyl group [33, 34]. The bands at 1074 and 876 cm−1 could result from ionized linkage of P+ O− in acid phosphate esters, to symmetrical vibration in a chain of P–O–P and to P–C phosphorus-containing compound [35, 36]. These functional groups are due to the presence of H3PO4 acid as an activation agent in the preparation of C-PAN.
Fig. 2

FT-IR spectrum of C-PAN adsorbent

Figure 3 shows an X-ray powder diffraction pattern of C-PAN. An amorphous peak with the equivalent Bragg angle at 2θ = 24.6 was recorded, together with other peaks recorded at 2θ = 17.5°, 31.2° and 47.5°. The surface morphology of the C-PAN adsorbent was examined. Figure 4 shows the SEM image indicating that the surface is relatively smooth and contains many pores. The SEM of C-PAN show very distinguished dark spots, which can be taken as a sign for effective adsorption of dye molecules in the cavities and pores of this adsorbent.
Fig. 3

XRD spectrum of C-PAN adsorbent

Fig. 4

SEM image of C-PAN adsorbent

Effect of pH

To examine the pH effect of the initial aqueous dye solution, a concentration of BB41 dye at 100 mg/L and 20 mg of C-PAN adsorbent was used, keeping the temperature at 20 °C at different pH values in the range 2–12. Figure 5 shows the variation of dye removal vs. pH. In fact, the amount of dye adsorbed onto C-PAN was found to be constant for all pH values being studied. The experiments carried out at different pH values showed that there was no significant change in the percent removal of dye over the entire pH range. This indicates the strong affinity of the dye to C-PAN and that either H+ or OH ions could influence the dye adsorption capacity. The dye removal  % uptake comprised between 92 and 97 %. If the adsorption would have occurred through an ion exchange mechanism, there should have been an influence on the dye adsorption while varying the pH. This observation and the high positive ∆H0 value obtained indicate irreversible adsorption, probably due to nonpolar interactions [37]. Other studies for different dyes were also found to be independent of pH [37, 38, 39].
Fig. 5

Effect of pH on the removal of BB41 from aqueous solution onto C-PAN. Initial dye concentration 100 mg/L; adsorbent amount 200 mg; agitation time 80 min; temperature 20 °C

The effect of C-PAN adsorbent dosage

The effect of C-PAN dosage on adsorption was studied at 20 °C with 100 mg/L dye solution. The adsorbent dosage ranged from 5 to 30 mg. The plots of dye removal (%) versus time at different adsorbent dosages are shown in Fig. 6. The results follow the expected pattern, in which the removal (%) of BB41 increased with increase in C-PAN adsorbent dosage. This might be due to an increase in the surface active sites in C-PAN samples. The adsorption equilibrium was achieved after 120 min of stirring the dye solution with the appropriate amount of C-PAN adsorbent. At this time, the removal of BB41 (%) increased from 45.7 to 99 % for C-PAN adsorbent dosage of 5 mg to 30 mg. However, the amount of BB41 adsorbed onto C-PAN, q (mg/g) was found to decrease from 457.46 to 165.83 mg/g upon increasing the adsorbent dosage. This behavior could be due to the high number of unsaturated sorption sites during the adsorption process.
Fig. 6

Effect of C-PAN adsorbent dosage and contact time on the removal of BB41 from aqueous solution. Initial dye concentration 100 mg/L; temperature 20 °C

Effect of BB41 concentration

The initial adsorbate concentration provides an important driving force to overcome all mass transfer resistances of dye between the aqueous and solid phases. The effect of initial concentration of dye on the adsorption was studied at 20 °C with 30 mg of C-PAN adsorbent. The adsorbate concentration ranged from 25 to 125 mg/L. The plots of dye removal (%) vs. time at different initial BB41 concentrations are shown in Fig. 7. The removal dye (%) shows a decreasing trend as the initial dye concentration of the dye is increased. At lower concentrations, all adsorbate ions present in the medium could interact with the binding sites, resulting in higher dye removal (%). At higher concentrations, the dye removal (%) shows a decreasing behavior because of the saturation of the adsorption sites. Similarly, the adsorption equilibrium was achieved after 120 min of stirring the appropriate dye solution with the C-PAN adsorbent. At this time, the removal of BB41 (%) decreased from 99 to 77.5 % for the initial BB41 concentration of 25 to 125 mg/L. However, the amount of BB41 adsorbed onto C-PAN, qe(mg/g) was found to increase from 124.41 to 484.35 mg/g upon increasing the initial dye concentration
Fig. 7

Effect of initial dye concentration and contact time on the removal of BB41 from aqueous solution. C-PAN 30 mg/L; temperature 20 °C

Adsorption kinetics

To study the sorption process of BB41 onto C-PAN adsorbent, the data obtained from kinetic adsorption experiments were simulated with pseudo-first-order and pseudo-second-order models.

The pseudo-first-order equation is generally represented as follows [40]:
$$\log \left( {q_{\text{e}} - q_{t} } \right) = \log \left( {q_{\text{e}} } \right) - \frac{{k_{1} }}{2.303}t,$$
where qe is the amount of dye adsorbed at equilibrium (mg/g), qt the amount of dye adsorbed at time t (mg/g), k1 the pseudo-first-order rate constant (min−1) and t the time (min).
The values of k1, qe calculated from the equation and the correlation coefficient (R2) values of fitting the first-order rate model at different concentrations are presented in Table 1. The linearity plots of log (qeqt) versus time at different initial dye concentrations (Fig. 8) suggested that the process of dye adsorption did not follow the pseudo-first-order rate kinetics. Also from Table 1, it is indicated that the values of the correlation coefficients are not high for the different dye concentrations. Furthermore, the estimated values of qe calculated from the equation qe differ substantially from those measured experimentally. This gives confirmation that the adsorption process of BB41 onto C-PAN did not obey the pseudo-first-order model.
Table 1

The pseudo-first-order and pseudo-second-order kinetic parameters for BB41 removal using C-PAN

Concentration of BB41 (mg/L)

Pseudo-first order

Pseudo-second order

qe,exp (mg/g)

k1 (min−1)

qe,cal (mg/g)


k2 × 10−4 (g/mg min)

qe,cal (mg/g)










































Fig. 8

Pseudo-first-order plots for different initial dye concentrations removal using C-PAN adsorbent. C-PAN adsorbent 30 mg; temperature 20 °C

The pseudo-second-order equation is generally represented as follows [41]:
$$\frac{t}{{q_{\text{t}} }} = \frac{1}{{k_{2} q_{\text{e}}^{2} }} + \frac{1}{{q_{\text{e}} }}t,$$
where k2 is the pseudo-second-order rate constant (g/mg min).
A plot of t/qt and t should give a linear relationship if the adsorption follows pseudo-second-order model. To understand the applicability of the model, a linear plot of t/qt vs. t under different dye concentrations was plotted as in Fig. 9. The constants k2, qe and correlation coefficients (R2) were calculated from the plot and are given in Table 1. The qe determined from the model along with correlation coefficients indicated that qe was very close to qexp and the correlation coefficient was also greater than 0.99. As a matter of consequence, the system BB41–C-PAN could be well described by the pseudo-second-order model. This adequate model shows that the adsorption of BB41 onto C-PAN is controlled by chemisorption mechanism.
Fig. 9

Pseudo-second-order plots for different initial dye concentration removal using C-PAN adsorbent. C-PAN adsorbent 30 mg; temperature 20 °C

Adsorption isotherms

Adsorption isotherms are basic requirements for the design of adsorption systems. It can express the relationship between the amounts of adsorbate by unit mass of adsorbent at a constant temperature. Herein, we analyzed our experimental data by Langmuir and Freundlich isotherms models. The best-fitting model was evaluated using the correlation coefficient.

The Langmuir model [42] permits the evaluation of maximum dye adsorption capacity when all sites have equal affinities and active sites of adsorbent are independent of each other. The linear form of the Langmuir isotherm is expressed as follows:
$$\frac{{C_{\text{e}} }}{{q_{\text{e}} }} = \frac{1}{{q_{\text{m}} K_{\text{L}} }} + \frac{1}{{q_{\text{m}} }}C_{\text{e}} ,$$
where Ce (mg/L) is the equilibrium concentration of the BB41 dye and qe (mg/g) is the amount of BB41 adsorbed per unit mass of adsorbent. qm (mg/g) and KL (L/mg) are the constants related to the maximum adsorption capacity and is the Langmuir constant, respectively.
A straight line with a slope of 1/qm and intercept of 1/qmKL is obtained when Ce/qe is plotted against Ce. Table 2 shows the values of these parameters.
Table 2

Adsorption isotherm constants for removal of BB41 onto the C-PAN adsorbent



298 K

303 K

313 K

Langmuir isotherm

 qm (mg/g)




 KL (L/mg)








Freundlich isotherm

 KF (mg/g) (L/g)












The essential characteristics of the Langmuir equation can be expressed in terms of the dimensionless separation factor, RL, defined as:
$$R_{\text{L}} = \frac{1}{{1 + K_{\text{L}} C_{0} }},$$
where C0 is the initial concentration of the BB41 dye; the RL value implies whether the adsorption is unfavorable: RL > 1, linear: RL = 1, favorable: 0 < RL < 1, or irreversible: RL = 0.
Figure 10 depicts the plot of the calculated RL values versus the initial dye concentration at 298, 303 and 313 K. It was observed that all the RL values obtained were between 0 and 1, showing that the adsorption of BB41 onto C-PAN was favorable. The RL values decrease upon increasing the initial dye concentration, which indicates that the adsorption is more favorable at higher BB41 concentrations. The adsorption capacity increases on increasing the temperature, attaining a higher value of adsorption capacity of 625 mg/g at 313 K. The values of KL increased on an increase in temperature. Therefore, by increasing the temperature, higher adsorption capacities were achieved.
Fig. 10

Dimensionless separation factor, RL, versus concentration dye

Freundlich isotherm [43] is observed if the sites with stronger binding affinities are occupied by the dye molecules first and the binding strength decreases with increase in the degree of site occupation. The linear form of the Freundlich isotherm is expressed as follows:
$$\log \left( {q_{\text{e}} } \right) = \log \left( {K_{\text{f}} } \right) + \frac{1}{n}\log \left( {C_{\text{e}} } \right),$$
where Kf (mg/g) (L/g) and n are Freundlich constants related to the adsorption capacity and adsorption intensity, respectively.

The Freundlich constants n and Kf were obtained from the plot of log (qe) versus log (Ce) that should give a straight line with a slope of (1/n) and intercept of log (Kf) (as shown in Table 2). In this study, the values found for n were superior to 1, which indicates that the adsorption of BB41 onto C-PAN is favorable.

Thermodynamic study

The thermodynamic data reflect the feasibility and favorability of the adsorption. The parameters such as free energy change (ΔG0), enthalpy change (ΔH0) and entropy change (ΔS0) can be estimated by the change of equilibrium constants with temperature. The free energy change of the sorption reaction is given by:
$$\Delta G^{0} = - RT\ln K_{C} ,$$
where ΔG0 is the free energy change (kJ/mol), R the universal gas constant (8.314 J/mol K), T the absolute temperature (K) and KC the equilibrium constants (qe/Ce). The values of ΔH0 and ΔS0 can be calculated from the Van’t Hoff equation:
$$\ln K_{C} = - \frac{{\Delta H^{0} }}{RT} + \frac{{\Delta S^{0} }}{R},$$
where LnKC is plotted against 1/T, and a straight line with the slope (−ΔH0/R) and intercept (ΔS0/R) are found. The calculated thermodynamic parameters are depicted in Table 3.
Table 3

Thermodynamic data for the adsorption of BB41 onto C-PAN

T (K)


ΔG0 (kJ/mol)

ΔH0 (kJ/mol)

ΔS0 (J/mol K)















In the study, ΔG0 values were determined at different temperatures and decrease from −11.64 to −19.50 kJ/mol when the temperature increases from 298 to 323 K. The negative values of ΔG0 suggest that the adsorption of BB41 onto C-PAN is a highly favorable process. The values of ΔH0 and ΔS0 were obtained as 144.6 and 524.3 J/mol K, respectively. The positive value of ΔH0 shows that the adsorption is an endothermic process, while a positive value of ΔS0 reflects the increase of randomness state at the solid/solution interface during the adsorption.

Comparison of adsorption capacities of C-PAN with those of various AC adsorbents

Table 4 depicts the values of maximum monolayer adsorption capacities of many AC adsorbents. It appeared that C-PAN can be classed belong the best ACs adsorbents with an adsorption capacity of 625 mg/g.
Table 4

Comparison of the maximum monolayer adsorption capacities of C-PAN with those of various AC adsorbents

AC adsorbent



qm (mg/g)


Pomegranate peel

Remazol brilliant




Homemade cocoa shell

Reactive violet 5




Rambutan peel

Acid yellow 17




Rice husks

Methylene blue




Pomelo skin

Methylene blue




Stricta algae based

Safranin O




Persea americana

Basic Blue 41



This study


Based on the results obtained in this study, it appears that the activated carbon prepared from Persea American nut constitutes a good adsorbent for removing a dye from aqueous solutions:
  • The percent (%) removal of BB41 was observed to increase with increasing initial dye concentration and increasing adsorbent dose.

  • The Langmuir isotherm best described the equilibrium data with acceptable R2, which signifies that a homogeneous adsorption takes place between the BB41 dye and C-PAN.

  • The pseudo-second-order equation best describes the kinetics of the C-PAN adsorption system due to its high R2. In addition, the theoretical qe generated by the pseudo-second-order equation is in good agreement with the experimental qe value. This implies that the rate-limiting step is a chemisorption process.

  • Thermodynamic studies indicated that the adsorption process is endothermic and spontaneous.

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© The Author(s) 2016

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors and Affiliations

  • Abdelmajid Regti
    • 1
  • My Rachid Laamari
    • 1
  • Salah-Eddine Stiriba
    • 2
    • 3
  • Mohammadine El Haddad
    • 1
  1. 1.Equipe de Chimie Analytique and Environnement, Faculté Poly-disciplinaireUniversité Cadi AyyadSafiMorocco
  2. 2.Equipe de Chimie Moléculaire, Matériaux et Modélisation, Faculté Poly-disciplinaireUniversité Cadi AyyadSafiMorocco
  3. 3.Instituto de Ciencia Molecular/ICMolUniversidad de ValenciaValenciaSpain

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