Powdered activated carbon prepared from Leucaena leucocephala biomass for cadmium removal in water purification process

Abstract

Activated carbons (ACs) were prepared from Leucaena leucocephala biomass. This is an agricultural solid waste by-product, as well as easily grown species available abundantly in Southeast Asia. In this work, activated carbon derived from Leucaena leucocephala biomass was prepared for sequestration of cadmium from aqueous solutions. The activated carbon was produced by a NaOH chemical activation process using NaOH:char ratios (w/w) of 1:1, 2:1 and 3:1 at 800 °C. The activated carbon’s BET surface areas were determined as 185, 595, and 776 m² g⁻¹ for the NaOH:char ratios of 1:1, 2:1, and 3:1, respectively. At initial concentration of 30 mg/l, maximum cadmium adsorption was achieved within 40 min. The adsorbent also showed good sorption of cadmium at pH 7.0 with solution temperature of 30 °C. Isothermic studies showed the adsorption process best fitted to Langmuir isotherm which indicates monolayer adsorption had happened while kinetic studies showed physisorption process was favorable, determined by pseudo-first order kinetic model. Maximum adsorption capacity was found to be 70.423 mg/g for NaOH:char ratios of 3:1.

Keywords:

• Activated carbon
• Leucaena leucocephala
• cadmium
• adsorption
• isothermic
• kinetic

1. Introduction

Heavy metals receive great concern due to their potential risk as common environmental pollutants. Heavy metal contamination of water is not only harmful to aquatic life but also adversely affects human health. Heavy metal contamination comes from electronic, metal smelting and automotive industries (Ahmad Khan, Ibrahim, & Subramaniam, 2004; Bailey, Olin, Bricka, & Adrian, 1999). One of the heavy metals involved is cadmium. Cadmium (Cd) is a metal identified for its high degree of toxicity. The presence of Cd as an impurity in zinc of galvanized pipes or Cd-containing solders in fittings, water coolers, water heaters and taps leads to contamination of drinking water. Long-term consumption leads to Cd accumulation in the human body especially in the kidneys where dysfunctioning of the organ results in a worst case scenario (Bernard, 2008).

The various methods that are used for water treatment have been developed to be applied for heavy metal removal (Ali et al., 2018). These methods include filtration, screening, oxidation, sedimentation, distillation, evaporation, reverse osmosis, electro-chemical, ion exchange and adsorption (Basheer, 2018). Comparatively, adsorption is one of the applicable methods because of convenience, ease of operation or production and simplicity of design (Yaacoubi, Zidani, Mouflih, Gourai, & Sebti, 2014).

Adsorption using activated carbon is one of the ways to eliminate this problem. However, the high cost of producing activated carbon is a limiting factor. The properties of normally activated carbon are still not sufficient to ensure efficient heavy metal uptake from waste water. Therefore, chemical activation of the activated carbon needs to be employed to further increase the effectiveness of water treatment. Phosphoric acid, sulfuric acid, zinc chloride, sodium hydroxide and potassium hydroxide are among the dehydrating agents usually used in chemical activation (Regti, Laamari, Stiriba, & El Haddad, 2017). Recent research has been conducted by Devi et al. (2017) using nano particles or other products resulting from the development of nanotechnology as an effective adsorbent for removal of cadmium. Other adsorbents used for sequestration of the cadmium ion from water are given in Table 1.

Table 1. Some adsorbents used for removal of cadmium ion from water.

Adsorbent	Reference
Cucumber peel activated carbon	(Basu, Guha, & Ray, 2018)
Humic acid-based carbon materials	(Jin et al., 2018)
nano-montmorillonite	(Liu et al., 2018)
Punica granatum (pomegranate) carpellary membrane	(Saini, Kumar, Chawla, & Kaur, 2017)
Rice husk	(Khan, Khan, Ding, Khan, & Alam, 2018)
Lotus seedpod-derived biochar	(Chen et al., 2018)
Magnetite/carbon nanocomposites	(Andelescu, Nistor, Muntean, & Rădulescu-Grad, 2018)
Aguaje (Mauritia flexuosa) based activated carbon.	(Obregón-Valencia & Sun-Kou, 2014)

Activated carbon is a popular choice of adsorbent for contaminants removal, especially heavy metal and dye from wastewater (Babel & Kurniawan, 2003). Various researches have been conducted, aiming to reduce the cost of activated carbon production without sacrificing the efficiency of the material in the removal of heavy metals from waste water. Low-cost adsorbents are a very popular material and receive much attention for adsorption of pollutants such as heavy metals and dyes (Sadegh, Mazloumbilandi, & Chahardouri, 2017). Therefore, this work on Leucaena leucocephala as a low-cost material for activated carbon production, has been processed by chemical means to obtain highest possible adsorption capacity.

Leucaena leucocephala, which is also known locally as the Petai Belalang tree is native to southern Mexico and northern Central America and is widespread in the Asian tropics and Malaysia. Parts of the Leucaena leucocephala plant are commonly used for animal food and as a vegetable for human consumption. Leucaena leucocephala is widely grown all over Malaysia and can be easily cultivated. The abundance of this plant offers a new opportunity to utilize its biomass in many fields. It is a fast-growing species reaching 10 m in height after 24 months of cultivation. The wood volume produced after 24 months of planting can rise to 91.3 m³ per hectare (MacDicken & Brewbaker, 1988; Rasat et al., 2016). Utilization of Leucaena leucocephala can reduce production cost as it is a wild tree and can be grown without specific silviculture techniques.

Studies on the adsorption behavior of the adsorbent materials towards heavy metals are important to evaluate the optimum condition, thus increasing the efficiency of the water treatment process. Due to lack of information on activated carbon prepared from Leucaena leucocephala biomass, this work explores the potential of this new raw material together with its performance in the water purification process.

2. Experimental

2.1. Material preparation

Samples from wild Leucaena leucocephala were collected around Selangor, Malaysia. The samples were left to air dry until the moisture content became less than 10%. The dried sample was cut into a smaller size before being ground to produce particles between 1 and 2 µm size. The wood particles were kept in a closed container for further use (Rafatullah, Sulaiman, Hashim, & Amini, 2011).

2.2. Activated carbon preparation

Carbonization was carried out using a pyrolyzer to produce a large quantity of charcoal. Carbonized Leucaena leucocephala biomass particles were activated by a chemical process where the carbonized sample was impregnated with NaOH at the NaOH:carbonized sample ratios of 3:1, 2:1 and 1:1. Approximately 10 g of carbonized sample were homogenized with 30 g of NaOH in 100 mL distilled water in a vertical stainless steel reactor under continuous magnetic stirring for 2 h before drying in an oven at 105 °C for 24 h (Cazetta et al., 2011). After heating for 24 h, the sample was placed in the muffle furnace for the activation process. The sample was heated at 800 °C under a nitrogen flow of 150 cm³/min for 90 min during the process.

2.3. Surface area analysis

Surface area analysis was carried out using Micromeritics (ASAP 2010) analyzer. The activated carbon was degassed at 300 °C before nitrogen adsorption was carried out at –196 °C. Surface area was calculated using Brunauer–Emmett–Teller (BET) analysis software provided with the instrument {Sudaryanto, 2006 #4745}.

2.4. Scanning electron microscope (SEM) observation

The raw Leucaena leucocephala and activated carbon samples were sieved to obtain 35–60 µm sized fractions. The particles were sprinkled onto the tub with carbon glue before gold-plating with a vacuum electroplating machine for about 60 s. The samples were then analyzed using an SEM (JSM-IT100 JEOL Co.) microscope at 150x and 550x magnifications.

2.5. Batch adsorption studies

Approximately 0.5 g of the prepared activated carbon was mixed with 100 ml of the aqueous solutions of cadmium inside a conical flask, continuously shaken using a temperature-controlled water bath shaker for a pre-determined period. The mixtures were filtered with filter paper to separate the treated cadmium solution from the adsorbent. The metal ion concentration was determined by inductively coupled plasma optical emission spectrometry, ICP-OES at Forest Research Institute of Malaysia. All the experiments were performed in triplicate to reduce errors (Sulaiman, Amini, Rafatullah, Hashim, & Ahmad, 2010).

2.6. Isothermal studies

2.6.1. Langmuir isotherm

The Langmuir isotherm model suggested an ideal monolayer adsorption onto a homogenous surface. Three temperatures of the reaction were used, predetermined at 30, 40, and 50 °C. The following Equation 1 was used: (1) $$\frac{1}{q_e}=\mathrm{}\frac{1}{q_m}+\mathrm{}\frac{1}{K_a{q}_m{C}_e}\mathrm{}$$(1)

where q_e is the amount of adsorbate adsorbed at equilibrium per gram of sample (mg/g), q_m is the saturated amount of adsorbate adsorbed in mg/g, C_e is the equilibrium concentration of cadmium in mg/l, and Ka is the Langmuir adsorption constant in l/mg. A 1/q_e versus 1/C_e plot was made, showing a straight line with a slope of 1/K_aq_m and an intercept of 1/q_m Ka was then calculated by the formula (Lee, Amini, Sulaiman, Mohamed, & Boon, 2018).

2.6.2. Freundlich isotherm

Freundlich isotherm assumes that heterogenous and multilayer adsorption occurred on the adsorbent surface (Çetinkaya, Targan, & Nüket Tirtom, 2018), calculated using Equation 2(2) $$ln{q}_e=ln{K}_F+\mathrm{}\frac{1}{n}\mathrm{}ln{C}_e\mathrm{}$$(2) : (2) $$ln{q}_e=ln{K}_F+\mathrm{}\frac{1}{n}\mathrm{}ln{C}_e\mathrm{}$$(2)

where K_F is Freundlich equilibrium constant, n is an empirical constant and others as stated in Equation 1(1) $$\frac{1}{q_e}=\mathrm{}\frac{1}{q_m}+\mathrm{}\frac{1}{K_a{q}_m{C}_e}\mathrm{}$$(1) . Thus, a plot of ln qe vs. ln C_e should provide a straight line with a slope of (1/n) and an intercept of lnK_F

2.7. Kinetic studies

Adsorption kinetics which investigate the rate and mechanism of the adsorption process pseudo-first-order kinetic model and pseudo-second order kinetics model.

2.7.1. Pseudo-first-order kinetic model

Pseudo-first-order kinetic model was derived from Equation 3(3) $$\frac{d{q}_t}{q_t}=\mathrm{}{K}_1\mathrm{}\left(q_e-\mathrm{}{q}_t\right)$$(3) : (3) $$\frac{d{q}_t}{q_t}=\mathrm{}{K}_1\mathrm{}\left(q_e-\mathrm{}{q}_t\right)$$(3)

Into linear Equation 4: (4) $$\text{log}\hspace{0.17em}{\mathrm{}(q}_{e\mathrm{}}-\mathrm{}{q}_t)=\hspace{0.17em}\text{log}\hspace{0.17em}\mathrm{}(q_e)-\mathrm{}\frac{K_1}{2.303}\mathrm{}t\mathrm{}$$(4)

where q_e and q_t are the amount of ions adsorbed (mg/g) at the equilibrium and at time t, respectively. K₁ represents the rate constant of pseudo-first order reaction. A plot of log (q_e – q_t) against t was plotted to obtain K₁ from the slope and q_e from the intercept.

2.7.2. Pseudo- second order kinetics model

While the pseudo- second order kinetics model is expressed by Equation 5(5) $$\frac{d{q}_t}{q_t}=\mathrm{}{K}_2\mathrm{}{\left(q_e-\mathrm{}{q}_t\right)}^2$$(5) : (5) $$\frac{d{q}_t}{q_t}=\mathrm{}{K}_2\mathrm{}{\left(q_e-\mathrm{}{q}_t\right)}^2$$(5)

Integration of Equation 5 generates linearized Equation 6(6) $$\frac{t}{q_t}=\mathrm{}\frac{1}{K_2{q}_e^2}+\mathrm{}\frac{1}{q_e}t\mathrm{}$$(6) : (6) $$\frac{t}{q_t}=\mathrm{}\frac{1}{K_2{q}_e^2}+\mathrm{}\frac{1}{q_e}t\mathrm{}$$(6)

where K₂ is the rate constant of pseudo-second order reaction. K₂ and q_e can be determined from the intercept and slope of a linear plot of t/qt versus t, respectively (Borah et al., 2018).

3. Results and discussion

3.1. Surface area of activated carbon

The BET surface areas of Leucaena leucocephala activated carbon were measured to be 185, 595 and 776 m²g⁻¹ for the NaOH:carbonized sample ratios of 1:1, 2:1 and 3:1, respectively. While increasing surface area results in higher adsorption capacity, it also contributes to the reduction in bulk density and physical strength of activated carbons. For harsh cyclic adsorption applications where high volumetric capacity is needed, this characteristic could be potentially a disadvantage (Lee, Byamba-Ochir, Shim, Balathanigaimani, & Moon, 2015). Hence, the activation process should be controlled correctly to obtain an excellent adsorbent with suitable capacity and bulk density for specific applications. The total pore volume and mesopore fraction were known to have positive relationship with the increment of mass ratio of the activating agent: raw material until a certain optimal point.

Among the most important parameters that determine the adsorption capacity of an adsorbent are the pore structure, the specific surface area and the total number of micropores and mesopores (Carrott & Carrott, 2007; Caglar et al., 2013). The International Union of Pure and Applied Chemistry (IUPAC) classifies ultramicropores for pore width less than 0.7 nm, supermicropores for pore width between 0.7 nm and 2 nm, mesopores for pore width between 2 nm and 50 nm, and macropores for pore width bigger than 50 nm. Activation process type and parameters affect the total number of micropores and mesopores, which leads to significant changes in the surface area and porosity, and directly influences the adsorption rate of the adsorbate.

The internal surface of activated carbon was mainly contributed by the micropores which comprise the main portion of the total surface area, while mesopores, macropores and the non-porous surface represent the external surface of the sample. Micropores usually act as adsorption sites, whereas the mesopores and macropores give rise to channels for the adsorbate to reach the micropores. The enlarged radii of the mesopores and macropores, on the other hand, allow the multilayer adsorption to occur.

3.2. Surface morphology analysis

Figure 1 shows 150x (a) and 550x (b) magnified SEM photos of the activated carbon between the raw material of Leucaena leucocephala and activated carbon. It may be seen in Figure 1 that the raw material sample had some tiny holes between activated carbon samples. The SEM images of activated carbon obtained from Leucaena leucocephala (Figure 1(c,d)) demonstrate that activated carbon possessed higher amounts of tiny and large holes than the raw material samples which can be explained by the emergence of the pores in the interlayer spacings of the samples during the activation process through heating (Caglar, Afsin, Tabak, & Eren, 2009).

Figure 1. SEM images of (a) the raw material of Leucaena leucocephala at magnification 150x, (b) the raw material of Leucaena leucocephala at magnification 550x, (c) activated carbon at magnification 150x and (d) activated carbon at magnification 550x.

3.3. Batch adsorption studies

3.3.1. Effect of contact time on the cadmium adsorption

Effects of contact time, initial concentration, pH and temperature on the removal of cadmium by the activated carbon sample prepared from Leucaena leucocephala were studied. Figure 2 shows the removal of cadmium at the activation temperature of 800 °C for NaOH:carbonized sample ratios of 1:1, 2:1 and 3:1 after different contact times between 10 min and160 min with the initial Cd²⁺ concentration of 30 mg/l. Approximately 0.5 g/l of adsorbent dosage was used at pH 7.0 of the solution. Adsorption equilibrium was established within 40 min of treatment. At 160 min of contact time, the maximum amounts of adsorption of the samples were found as 99.86%, 99.82% and 99.97% for NaOH:carbonized sample ratios of 1:1, 2:1 and 3:1, respectively. The higher the ratio of NaOH:carbonized sample used for chemical activation, the higher the adsorption efficiency for cadmium removal as reflected from the larger surface area obtained by the higher NaOH:carbonized sample ratios in BET surface area analysis. No significant increment on the amount of removal of solute from the solutions was recorded beyond the maximum point where the system reaches equilibrium.

Figure 2. Removal of cadmium at a different contact time.

3.3.2. Effect of initial adsorbate concentration on the cadmium adsorption

The effect of initial concentration on the removal of cadmium by Leucaena leucocephala activated carbon was investigated at different sorbate solution concentrations (10, 20, 30, 40 and 50 mg/L) using 0.5 g adsorbent dose at pH 7.0. The percentage of cadmium removal decreased with the increase in the initial concentration of the solution. The surface area and the number of available active sites were relatively high compared to the adsorbate ions to be retained at low initial concentration. Thus, the cadmium ions were easily adsorbed and removed. On the other hand, the total number of available adsorption sites is smaller than the amount of adsorbate ions when the initial solution concentration is higher, thus decreasing the percentage of cadmium removal. The adsorption percentage for all samples was comparably high at relatively low concentrations of 10 mg/L and 20 mg/L as shown in Figure 3. At the concentrations of 30 mg/L, 40 mg/L and 50 mg/L, NaOH:carbonized sample for the ratio 3:1 showed better performance than for the ratios of 2:1 and 1:1. These results clearly indicate that the maximum adsorption percentage of metal ions by activated carbon was affected by the initial metal ion concentration. Higher initial concentration gives rise to lower adsorption rate due to the higher adsorbate: adsorption site ratio.

Figure 3. Initial concentration versus removal of cadmium.

Figure 4. Solution pH versus removal of cadmium.

3.3.3. Effect of pH on the cadmium adsorption

Rao, Rao, Seshaiah, Choudary, and Wang (2008) stated that the most crucial parameter controlling the adsorption process which affects the binding of cadmium ions by surface functional groups was the pH value. Figure 4 previously only indicated the cadmium removal at the same pH and initial concentration. Experimental studies were conducted for 40 min of contact time with 40 mg/l initial cadmium ion concentration and 0.5 g/l of the adsorbent dose at a different pH range. The high pH value of the solution leads to increase in the negative charge on the adsorbent surface (Gupta & Sharma, 2002; Krishnan & Anirudhan, 2003). Therefore, the electrostatic interactions between positive charged Cd²⁺ ions and the layer of negatively charged adsorbent material, cause a more powerful affinity, thus increasing the amount of Cd²⁺ ions adsorbed onto the adsorbent (Banerjee & Chattopadhyaya, 2017). In contrast, where the pH was lowered to pH 5 and pH 3, the percentage of Cd²⁺adsorption was decreasing, which may be ascribed to the competition between H₃O⁺ and Cd²⁺ ions in acidic media (Zheng et al., 2017).

3.3.4. Effect of temperature on the cadmium adsorption

The effect of temperature on the removal of cadmium by the prepared activated carbon is shown in Figure 5. The experiment was carried out for the contact time of 40 min, the initial cadmium ion concentration of 40 mg/l using 0.5 g/l of the adsorbent dose at different temperatures. Figure 5 shows the highest adsorption percentage for all samples was at 30 °C. Adsorption percentages dropped for all samples as the temperature was increased from 40 °C to 50 °C, 60 °C, and 70 °C. Therefore, it can be concluded that the adsorption percentage of cadmium decreases in contrast with the temperature rise and 30 °C may be considered as the equilibrium temperature of the system. This result seems to be in conformity with the previous study by Kumar, Ramakrishnan, Kirupha, and Sivanesan (2010), reporting the decrease of adsorption rate from 86.87 to 76.25% for 50 mg/L of the cadmium ion concentration within the temperature range from 25 °C to 55 °C.

Figure 5. Effect of temperature on removal of cadmium.

3.4. Isothermal studies

3.4.1. Langmuir isotherm

Figure 6 shows 1/q_e vs 1/C_e plot of Langmuir isotherm for Cd(II) ion adsorption for the sample NaOH:carbonized sample ratios of 3:1 (a), 2:1 (b) and 1:1 (c). The value of the correlation coefficient for the NaOH:carbonized sample ratios of 1:1 are 0.9671, 0.9542 and 0.9655 at 30 °C, 40 °C and 50 °C, respectively. NaOH:carbonized sample ratios of 2:1 and 3:1 showed the same high values of correlation coefficient with the lowest value of 0.9542 recorded. The high R² values showed the adsorption process follows Langmuir isotherm which suggested a monolayer type of adsorption.

Figure 6. 1/q_e vs 1/C_e plot of Langmuir isotherm of Cd(II) ion adsorption for NaOH:carbonized sample ratios of 3:1 (a), 2:1 (b) and 1:1 (c).

Table 2 shows the calculated values and constant of the Langmuir equation. The q_m, which is the measure of the adsorption capacity to form a monolayer, is recorded to be as high as 70.423 mg/g at 50 °C. Constant K_L, which denotes adsorption energy, for the corresponding adsorption capacity, ranged between 0.589 and 3.627 l/mg. The maximum monolayer adsorption capacity, q_m (mg/g) was found to increase with the increment of temperature and increment of NaOH:carbonized sample ratio as obtained by Karthikeyan, Rajgopal, and Miranda (2005). Comparison of the adsorption capacity of the Leucaena leucocephala activated carbon compared to other adsorbents for cadmium removal from water in Table 3 showed that this adsorbent performs above average with the maximum adsorption reaching 70.423 mg/g.

Table 2. Isothermic and kinetics models for the adsorption of Cd²⁺ by Leucaena leucocephala based activated carbon.

Sample	Temperature, °C	Langmuir Isotherm			Freundlich Isotherm
		qm (mg/g)	KL (l/mg)	R^2	KF	l/n	R^2
1:1	30	31.153	8.231	0.9671	3.8763	0.9878	0.8265
	40	31.447	5.483	0.9655	3.8045	1.0455	0.7990
	50	31.67	0.589	0.9542	5.1123	2.3296	0.9003
2:1	30	40.984	8.133	0.9855	5.6249	2.1227	0.9703
	40	50.505	4.500	0.9783	4.7040	1.5924	0.9000
	50	53.191	5.371	0.9707	4.8970	1.6174	0.8874
3:1	30	54.054	3.627	0.9627	4.8448	1.7987	0.9401
	40	64.013	2.600	0.9609	4.2177	1.2863	0.7513
	50	70.423	3.302	0.9873	5.7397	2.3551	0.9701

Table 3. Comparison of different adsorption capacity for different cadmium adsorbent.

Adsorbent	Maximum adsorption (mg/g)	Reference
Leucaena leucocephala activated carbon	70.42	This work
Humic acid-based carbon materials	26.3	(Jin et al., 2018)
Nano-montmorillonite	17.61	(Liu et al., 2018)
Punica granatum (pomegranate) carpellary membrane	111.11	(Saini et al., 2017)
Lotus seedpod-derived biochar	51.18	(Chen et al., 2018)
Magnetite/carbon nanocomposites	76.67	(Andelescu et al., 2018)
Aguaje (Mauritia flexuosa) based activated carbon.	26.33	(Obregón-Valencia & Sun-Kou, 2014)

3.4.2. Freundlich isotherm

Figure 7 shows the plots of linearized equations by Freundlich for the adsorption of cadmium at 800 °C activation temperature. The Freundlich model is applicable for non-ideal sorption on heterogeneous surfaces and multilayer sorption processes. Table 1 also shows the difference of R² value for both Langmuir and Freundlich isotherm. The R² value for this activation temperature shows that the Langmuir model exhibits a higher R² value than the Freundlich model which suggests that the adsorption was a better fit to the Langmuir isotherm. It was stated by Annadurai, Ling, and Lee (2008) that the value of the exponent 1/n indicates the favorability and capacity of the adsorbent/adsorbate system. Most of the samples showed n > 1 which indicates favorable adsorption conditions where in most cases the exponent between 1 < n < 10 shows beneficial adsorption.

Figure 7. ln qe vs ln Ce linear plot of Freundlich isotherm of Cd(II) ion adsorption for NaOH:carbonized sample ratios of 3:1 (a), 2:1 (b) and 1:1 (c).

3.5. Kinetic studies

3.5.1. Pseudo-first-order kinetic model and pseudo-second order kinetics model

Figure 8 shows log (qe-qt) vs. t linear plot of pseudo-first-order (a) and t/qt vs. t linear plot of pseudo-second-order (b) kinetic model of Cd(II) ion adsorption using Leucaena leucephala activated carbon. The R² values showed the adsorption process followed the pseudo-firstorder kinetic model, as shown in Table 4. The adsorption process was severely fitted to pseudo-second order kinetics model where the R² value goes as low as 0.0004. The pseudo-first-order kinetic model assumed that the adsorption process depends only on the two factors which are the number of metal ions present in the aqueous solution and the available binding sites on the adsorbent at any particular period, which explain the physisorption nature of the adsorption process. Meanwhile, the pseudo-second-order kinetic model assumed that the rate controlling step of an adsorption process is the chemical adsorption (Manirethan, Raval, Rajan, Thaira, & Balakrishnan, 2018).

Figure 8. log (qe-qt) vs t linear plot of pseudo first order (a) and t/qt vs t linear plot of pseudo second order (b) kinetic model of Cd(II) ion adsorption using Leucaena leucephala activated carbon.

Table 4. Kinetic models for Cd(II) ion adsorption using Leucaena leucephala activated carbon.

	Pseudo first order			Pseudo second order
Sample	qe (mg/g)	K1	R^2	qe (mg/g)	K2	R^2
1:1	33.58	0.0438	0.9650	2.0 x 10^-8	1.24 x 10^15	0.3376
2:1	33.6	0.0433	0.4851	2.0 x 10^-4	12.42 x 10^-6	0.1391
3:1	33.4	0.0451	0.8521	1111.1	4.06 x 10^-7	0.1092

4. Conclusions

Three activated carbon (AC) samples with different characteristics were prepared using chemical activation using the NaOH:carbonized sample ratios of 1:1, 2:1 and 3:1 in the present study. Each sample exhibited different adsorption percentage during batch adsorption studies. Considering the effect of contact time on Cd²⁺ removal, the highest adsorption percentage was observed for the ratio of 3:1. The adsorption equilibrium was reached within 40 min at the initial Cd²⁺ concentration of 30 mg/l. The concentration, pH, and temperature also gave rise to the highest adsorption rate for the NaOH:carbonized sample ratio of 3:1. The higher the initial concentration, the lower the level of adsorption performance. The higher adsorption equilibrium was established at pH 7.0 and reaction temperature of 30 °C is the optimum. Isothermic studies showed the adsorption process best fitted to Langmuir isotherm which indicates monolayer adsorption had happened while kinetic studies showed a physisorption process was favorable. It can be concluded based on the present results that the AC sample obtained from Leucaena leucocephala biomass at the NaOH:carbonized sample ratio of 3:1 could be the best to be used efficiently for removal of cadmium from contaminated water.

Disclosure statement

No potential conflict of interest was reported by the authors.

Additional information

Funding

The authors acknowledged the Ministry of Education of Malaysia for MyMaster scholarship to Wan Muhammad Hilmi bin Wan Ibrahim and Universiti Malaysia Kelantan for Short Term Grant (R/SGJP/A08.00/01046A/001/2015/000242) awarded to Mohd Hazim Mohamad Amini.