Chromium(VI) is one of the major heavy metals of great concern in wastewater management. Most of the chromium contamination in Uganda arises from industrial activities which include leather tanning, cement mining, electroplating, photography, dye manufacturing, and fertilizer industries. Majority of these industries are small scale and cannot afford the conventional methods of treating wastewater containing chromium. These industries therefore, channel untreated or partially treated effluents into the neighbouring water bodies, especially Lake Victoriaor deposit precipitated chromium into landfills from where it leaches into the underground water  . The level of chromium contamination in Jinja wetlands close to the tannery industry in Uganda has reached as high as 271 ppm compared to the recommended limits in soils of 40 - 50 ppm   . Therefore, there is a need to search for cheaper and environmentally friendly alternative methods to alleviate the chromium pollution challenge.
Some studies show that heavy metals can be removed from aqueous solution using plant materials such as papaya seeds  , Molinga oliefera  , wheat bran  . Such plant materials extract metals by adsorption process which is regarded as the most efficient method due to its low costs, availability, design simplicity, easy operation, biodegradability and ability to treat solutes in a more concentrated form.
In this study, the effectiveness of Artocarpus heterophyllus (jackfruit) seed powder in removing the chromium(VI) from aqueous solution by adsorption was investigated. The Artocarpus heterophyllus believed to originate from the rain forests of the Western Ghats of India is the largest tree-born fruit in the world. It is widely distributed in Uganda, both cultivated and wild, and a popular food item. The juicy pulp is commonly eaten as dissert but the seeds are often regarded as a waste and therefore, discarded. Since the seeds can be readily obtained from the consumers in large quantities, it might provide material for the remediation of chromium contamination from the contaminated water system as well.
2. Materials and Methods
Fresh jackfruit seeds were collected from Bugema village, Luwero district, Ugandain February, 2013 and the seed coat removed. The seeds were dried completely under the sun for 30 days, pulverised and sieved using a sieve of particle size 710 µm.
A stock solution containing 100 mg・l−1 of Cr(VI) was prepared by dissolving 0.2828 g of AR grade potassium dichromate, K2Cr2O7 (Merck) in distilled water to make 1000 mL of solution. The stock solution was appropriately diluted to give Cr(IV) standard solutions of the required concentrations. The pH of the standard solutions was adjusted with either 0.1 M sulphuric acid or 0.1 M sodium hydroxide solution.
2.3. Batch Adsorption Procedure
Batch adsorption studies were conducted at different conditions to assess the potential of jackfruit seed powder in the adsorption of Cr(VI) from aqueous solution. Experimental procedures followed were as outlined in  in triplicates and the average of the results reported. Cr(VI) concentration in the solutions was determined by the standard colorimetric method using 1,5-diphenylcarba- zide in an acid medium, which gave a violet complex with acidified Cr(VI)  . Metal concentration in the solution was analysed with a digital colorimeter at wavelength (λ) of 545 nm which gave the absorbance of Cr(VI) ions  . Percentage adsorption (Aeq) and adsorption capacity (Qe) at equilibrium were determined using the equations below;
where; V is the initial solution volume (L), Co and Ce are theinitial and equilibrium Cr(VI) concentration of the solution (mg・l−1), and W is the amount of JSP (g).
The effect of initial pH, contact time, temperature, adsorbent dosage level and initial chromium(VI) ion concentration were determined as per the procedures described by  as below.
2.4. Effect of Initial pH
While maintaining all other factors constant, the initial pH of the standard Cr(VI) solution was varied from 1, 2, 3, 4, 5, 6, 7, 8, 9 and 10 using 0.1 M H2SO4 or 0.1 M NaOH solution. Jackfruit seed powder (2.0 g) was added to 250 ml Pyrex glass beaker containing 5 mg・l−1 Cr(VI) solution (100 ml). The mixture was agitated using a glass rod every after 10 minutes. After 1 hour, 10 ml of the solution was obtained, to which was added 0.2 ml of 0.1 M H2SO4 followed by 1 ml of 1,5-diphenyl carbazide. The solution was left to stand for 5 to 10 minutes and residual concentration of Chromium(VI) determined.
2.5. Effect of Contact Time
Jackfruit seed powder (2.0 g) was added to 100 ml of 5 mg・l−1 chromium(VI) solution at pH 2 for 1, 3, 5, 10, 20, 30, 40, 50, 60, 90 and 120 minutes at 25˚C. The mixture was filtered and the amount of residual chromium(VI) in solution determined.
2.6. Effect of Temperature
Jackfruit seed powder (2.0 g) was added to 100 ml of 5 mg・l−1 chromium(VI) solution at pH 2 while maintaining the temperature at 25, 30, 40, 50, 60 and 70˚C using a water bath for 1 hour.
2.7. Effect of Adsorbent Dosage Level
Different masses of jackfruit seed powder (0.2, 0.5, 0.8, 1.0, 1.5, 2.0 and 3.0 g) were added to 100 ml of 5 mg・l−1 chromium(VI) at pH 2, and temperature of 25˚C and the mixture stirred after every 10 minutes for 1 hour.
2.8. Effect of Initial Chromium(VI) Ion Concentration
Jackfruit seed powder (2.0 g) was added to 100 ml of 5.0, 7.5, 10.0, 12.5, 15.0, 17.5 and 20.0 mg・l−1 of chromium(VI) at the pH 2 for 1hour while maintaining the temperature at 25˚C.
2.9. Effect of Interfering Ions
Effect of interfering ions was determined as per the procedure listed in  &  .
A solution of chromium(VI) (100 ml, 5.0 mg・l−1) was added different sodium chloride, potassium nitrate or sodium sulphate of concentration of 0, 5, 10 and 20 g/l at pH 2. To the resulting solutions, 2.0 g of jackfruit seed powder was added. While maintaining the temperature at 25˚C, the mixture was stirred after every 10 minutes for 1 hour. The procedure was repeated for 7.5 mg・l−1 chromium(VI).
3. Results and Discussion
3.1. Effect of Initial pH
Cr(VI) removal by JSP was found to be highly dependent on the initial pH of the solution as illustrated by Figure 1. The optimal pH for the removal of 5 mg・l−1 Cr(VI) by the jackfruit seeds was 2.0 (96.05% removal). At low pH, the surface of the JSP (active sites) became positively charged owing to the protonation of its functional groups (amines, carbxyl, and hydroxyl) and hence increasing the attraction for the, predominant at pH 2 and below  . As the pH increases, sites become less protonated and the electrostatic force of attraction between JSP and chromium(VI) anionic species decreases leading to reduction in
Figure 1. Effect of initial pH on Cr(VI) adsorption percentage and percentage.
perecentage adsorption. The pH best suitable for the adsorption of Cr(VI) species by plant seeds is 2    .
There was a slight change in the pH of the solution after the whole adsorption process as illustrated by Figure 2. This may be attributed to ion exchange between jackfruit seed powder surface and matrix interface. It may also be due to the adsorption of chromate ion by ion exchange mechanism as depicted in the equations below  .
3.2. Effect of Contact Time
The general increase in adsorption as per Figure 3 was due to the time allowed
Figure 2. Final pH and adsorption capacity varying with initial pH.
Figure 3. Effect of contact time on adsorption capacity and percentage of Cr(VI) by JSP.
for the chromium(VI) ions to interact with the JSP active sites. The initial rapid rate of adsorption leading up to 85.91% adsorption after 10 minutes may be due to the availability of the free active sites on JSP for the Cr(VI) ions. The next gradual adsorption rate to 98.73% at 90 minutes was either due to the electrostatic hindrance caused by the already adsorbed chromium(VI) anionic species and the incoming ions, or reduced probability of the chromium(VI) in finding a free adsorption site, since most active sites are already occupied  . Similar trend of results were obtained as in  .
3.3. Effects of Temperature
The general increase in adsorption in Figure 4 with temperature is attributed to the provision of the thermal energy, required to overcome the energy barrier for active sites and chromium(VI) bond formation  . The effect of temperature on the adsorption process is twofold; increasing the temperature increases the diffusion rate of the chromium(VI) ions in solution; and secondary, changing the temperature will modify the equilibrium capacity of the adsorbent for a particular adsorbate  . However, adsorption beyond 60˚C decreased to 98.76%, owing to desorption of adsorbed species at high temperatures. As the temperature is increased, the thermal energy is also increased and hence increasing mobility of the chromium(VI) ion in solution. Thus desorption rate outweighed the rate of adsorption at high thermal energy (beyond 60˚C)  .
3.4. Effect of Adsorbent Dosage
Figure 5 shows a general increase of adsorption percentage with adsorbent dose, which was due to the increased contact surface. It was more probable for and ions to adsorbed onto the jackfruit seed powder active sites leading to increased adsorption percentage  .
On the contrary adsorption capacity diminished with increasing adsorbent dose because adsorption capacity is inversely proportional to the adsorbent
Figure 4. Effect of temperature on adsorption percentage and capacity of Cr(VI).
Figure 5. Effect of adsorbent dosage level on adsorption percentage and capacity of Cr(VI).
3.5. Effect of Initial Cr(VI) Ion Concentration
Percentage adsorption decreased with initial ion concentration as illustrated by Figure 6. At low Cr(VI) concentrations, there are many jackfruit seed powder active sites for the few ions and subsequently fractional adsorption is independent of the initial concentration. However, at higher concentrations, the available sites for adsorption become fewer and hence the percentage removal of Cr(VI) ion which depends upon the initial concentration decreases  . On increasing the initial concentration, the adsorption capacity increased towards the saturation point owing to the increasing availability of Cr(VI) at the interface, thus enhancing the degree of adsorption  . Increasing the concentration of chromium(VI) ions in solution increased the availability of chromium(VI) ions at the interface, thus enhancing adsorption.
3.6. Evaluation of the Thermodynamic Parameters
The adsorption thermodynamic parameters were determined from the relations as described in    .
The standard change in the Gibbs free energy was calculated from
where R is gas constant (8.314 kJ・mol−1) and T is temperature in kelvin (K), Kc is the equilibrium constant obtained by the equation below
Cad is the concentration of Cr(VI) adsorbed onto the JSP at a given temperature, Co is initial Cr(VI) concentration.
Finally, the standard enthalpy change ∆Ho of +61789.648 J・mol−1 and entropy changes ∆So of +232.38 JK−1・mol−1 were obtained using the slope and intercept of Figure 7 from the linear Vant Hoff plot as illustrated by Equation (5) below.
The positive value of ∆Ho indicated that the adsorption process between jackfruit seed powder and chromium(VI) was endothermic  , implying mono- layer accompanying chemisorption. Therefore, it requires heat to overcome the energy barrier for adsorption to take place  . The positive value of ∆So reflected an increase in affinity of chromium(VI) towards jackfruit seed powder as well as an increase in the degree of disorder and randomness of the reaction mixture with temperature.
The negative values of ∆Go indicated the feasibility and spontaneity of the adsorption process. Furthermore, the amount of ∆Go (>41.858 kJ or 10 kcal) suggests
Figure 6. Adsorption percentage and capacity varying with initial ion concentration.
Figure 7. A graph of lnKc against 1/T for the evaluation of ∆Ho and ∆So.
that adsorption is chemical. The increasing magnitude of ∆Go with temperature as shown in Table 1 shows that adsorption is more favourable with temperature increase  .
3.7. Effects of Interfering Ions
Presence of a salt in the solution introduced interfering anionic species that competed with chromium(VI) for the same jackfruit seed powder adsorption sites. Interference significantly occurred in presence of the nitrate and chloride ions as per Figure 8 and Figure 9. Reduced adsorption was greatly manifested at higher salt concentrations. This is because increasing the salt concentration increased the number of interfering nitrate or chloride ions in the solution, enhancing competition for the jackfruit seed powder adsorption sites.
Table 1. Thermodynamic parameters for chromium(VI) adsorption by the JSP.
Figure 8. The effect of ion on Cr(VI) adsorption by JSP.
Figure 9. The effect of Cl− ion on Cr(VI) adsorption by JSP.
Interference by the chloride or nitrate ions was because of their relative small size as compared to in addition to possession of the same charge (single negative), and hence targeting the same positively charged JSP active sites. Similar trend of results were obtained as per  .
On the contrary, increasing sodium sulphate concentration and hence sulphate () ions in solution favoured adsorption of more chromium(VI) as shown by Figure 10. It could be attributed to the combined effect of from sulphuric acid and sodium sulphate.
In this case, the jackfruit seed powder may have acted as a reducing agent owing to the presence of electron-donor groups under acidic conditions. In turn, Cr(VI) probably received electron which then reduced it to Cr(III)  . The Cr(III) could have then reacted with the sulphate ions forming a complex  .
From Table 2, Cr(VI) adsorption in presence of nitrate ions (p < 0.05) indicated Cr(VI) adsorption interference by nitrate ions. Similar results in presence of chloride ion were also observed. The p values further indicated that increasing interfering ions or Cr(VI) ions in solution, further hindered adsorption. Most of the results obtained in presence of sulphate ions had p > 0.05, meaning that presence of sulphate ions in solution instead favours Cr(VI) adsorption process. Therefore presence of some ionic species in waste water may interfere with the Cr(VI) adsorption process by either enhancing or retarding it.
3.8. Adsorption Isotherms
Two adsorption isotherm models were selected to fit the data, namely the Langmuir and Freundlich models  . The Langmuir assuming a monolayer adsorption is,
where Qm is the maximum adsorption capacity, while Ka is a coefficient related to the affinity between the adsorbent and metal ions also related to the energy of adsorption, used to determine a dimensionless constant separation factor or
Figure 10. The effect of ion on Cr(VI) adsorption by JSP.
Table 2. The effect of other ions on the adsorption by JSP at 5.0 and 7.5 mg・l−1 Cr(VI).
*(p ≤ 0.05), **(p ≤ 0.005), ***(p ≤ 0.0005) and ****(p ≤ 0.00005).
equilibrium parameter RL, which is defined by the following relationship:
The parameter RL indicates the shape of the isotherm accordingly; if RL > 1, adsorption is unfavourable; RL = 1, Linear adsorption; RL = 0, irreversible adsorption; therefore, RL has a shape of 0 < RL < 1 for the sorption process to be favourable  .
Rearranging the equation, a linear equation is obtained
A linear plot of Ce/Qe vs. Ce, in Figure 11 was obtained and used to determine Qm, and Ka.
Additionally, the empirical data was fitted to the Freundlich adsorption isotherm, which can be expressed as below:
Figure 11. Langmuir isotherm for Cr(VI) adsorption by jackfruit seed powder.
The Freundlich isotherm being empirical, it is used for non-ideal adsorption and when the surface is heterogeneous. This isotherm describes nonlinear adsorption where Kf is the Freundlich constant, indicating the relative adsorption capacity related to the binding energy. The factor n, known as heterogeneity factor, represents the deviation from linearity of the adsorption. The linearised form of the Freundlich model is as shown below:
A linear plot of logQe vs. logCe yielded Freundlich isotherm at 25˚C.
The experimental results were fitted into the Langmuir as per Figure 11 and Freundlich isothermsas per Figure 12 as shown above and the constants obtined from the obtained plots are presented in Table 3. According to the values of RL obtained from the Langmuir isotherm, which were found to be between 0.0336 and 0.1220 for the used initial concentration range, indicated that the adsorption of Cr(VI) by JSP was judged to be favourable.
3.9. Comparison with Other Adsorbents
Maximum adsorption capacity (Qm) of Cr(VI) using JSP was 0.57 mg/g, which compared well with those reported in literature for other bioadsorbents (Table 4).
Activated rice husk carbon, activated alumina and modified oak sawdust exhibited higher Qm owing to the high initial carbon content, activation process as well as the pore development due to the basic morphology of the raw material  .
JSP successfully demonstrated the ability to remove Cr(VI) from aqueous acidic solution and its Qm compared well with those of other bio adsorbents reported in literature. Cr(VI) removal percentage by JSP was dependent on pH, temperature, contact time, adsorbent doses, and initial Cr(VI) concentration. Furthermore, it
Figure 12. Freundlich isotherm for Cr(VI) adsorption by JSP.
Table 3. Estimated isotherm parameters for Cr(VI) adsorption JSP.
Table 4. Comparison of adsorption capacities of Cr(VI) with other adsorbents.
was found out that Cr(VI) adsorption strongly depended on initial pH of the solution. Thus, the removal of Cr(VI) is highly applicable at very low pH values owing to the need for protonation of the surface active sites of JSP. Thermodynamic investigation showed that the process is spontaneous even at room temperature. The affinity of JSP for the Cr(VI) increases with temperature as well as the process being majorly chemisorption, as portrayed by positive standard entropy changes. The positive value of enthalpy change indicates that the reaction is endothermic.
Both Freundlich and Langmuir adsorption models well described the equilibrium data of Cr(VI) adsorption by JSP as the data best fitted both with high regression coefficients. According to Langmuir model, the monolayer adsorption capacity (Qm) was found to be 0.57 mg of Cr(VI) per gram of JSP. The obtained Qm implies that JSP is a better adsorbent as compared to saw dust, pine leaves, raw rice bran among others. Therefore, JSP is a potential adsorbent for chromium(VI) contaminated water. Finally, it was observed that the adsorption efficiency of Cr(VI) by JSP was highly influenced by interfering ionic species present in the matrix. Therefore, it is important to have an idea of the ionic species present in the effluent before the use of JSP to remediate it or the effectiveness of JSP to remove Cr(VI) from aqueous environments will greatly depend on the chemical components present. Similarly, because percentage adsorption decreases with increasing Cr(VI) concentration, it would be better to increase the amount of the JSP used as well as contact time in the case of highly polluted water systems.
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