1. Introduction

JEP

Journal of Environmental Protection

2152-2197

Scientific Research Publishing

10.4236/jep.2019.109069

JEP-95000

Articles

Earth&Environmental Sciences

Removal of Some Toxic Ions from Seawater and Wastewater by Sorption onto Natural, Synthetic Hydroxyapatite and Alginate-Hydroxyapatite Composite Nanoparticles: A Comparative Study

Mohamed

A. Shreadah

¹^*Osama

E. M. Rizk

¹Mohamed

A. Aly-Eldeen

¹Amal

R. Rashad

²Mohamed

E. Mahmoud

Chemistry Department, Faculty of Science, Alexandria University, Alexandria, Egypt

National Institute of Oceanography and Fisheries, Alexandria Branch, Alexandria, Egypt

04092019

1009115511732, August 20199, September 2019 12, September 2019

2014

This work is licensed under the Creative Commons Attribution International License (CC BY). http://creativecommons.org/licenses/by/4.0/

The main objective of this paper is to study the removal of Cadmium(II), Lead(II), Chromium(VI), and Mercury(II) ions by sorption onto different natural and synthetic nanoparticles. Special attention has been given to the application of fish bone in nanoform as a useful, inexpensive and eco-friendly alternative material. A comparison between natural hydroxyapatite (fish bone), synthetic hydroxyapatite nanoparticles (HAP) and alginate-hydroxyapatite composite (Alg/Hap) to assess their removal efficiencies to remediate the selected heavy metals has been done. Surface characterization by using different techniques has also been performed to understand the influence of surface characteristics of the adsorbent materials in the removal process. Different parameters (pH, contact time, mass dose and metal ion concentration) have been examined to identify the optimum conditions for remediation of different metals from polluted water. The potential applications of the biosorbents for removal and sorption of these metal ions from seawater and wastewater samples were also investigated and evaluated.

Cadmium(II) Lead(II) Chromium(VI) Mercury(II) Ions Removal Nano-Biosorbent Seawater and Wastewater

1. Introduction

Environmental pollution, in general, is a major hazard facing the world today and there is an increasing awareness about protection of the marine environment which became one of the major challenges facing the world [1] - [9] . Pollution due to the discharge of heavy metals in the marine environment of Egypt has received recently considerable concern due to their toxicity, abundance and persistence in the environment [10] - [19] .

Common removal technologies of heavy metals are membrane separation, ion exchange, electrodeposition, and chemical precipitation. These methods proved to be costly and inept, especially in removing trace amounts of heavy metals. Another disadvantage is the production of sludge or mud, which requires proper disposal and confinement. On the other hand, adsorption effectively removes contaminants from wastewater with high solute loadings and even at dilute concentrations (<100 mg/l) [20] [21] [22] [23] .

A wide range of biomaterials available in nature has been employed as biosorbents for the desired pollutant removal. Various forms of fish bones have been utilized including but not limited to a) cobalt removal by animal bones; b) lead removal by fish bone waste hydroxyapatite powder; c) immobilization of lead with nanocrystalline carbonated apatite present in fish bone; d) anchoring hazardous metal ions using modified fishbone; e) lead removal using unmodified fishbone; f) lead removal using waste fish bone via ion exchange; and g) desorption of lead adsorbed by fish bone. Thus, fish bones have become an attractive, cheap and abundant waste for in-situ lead stabilization from contaminated waters [24] [25] [26] [27] [28] .

In this study, special attention has been given to the application of fish bones in a nanoform to remove Cadmium(II), Lead(II), Chromium(VI), and Mercury(II) ions from contaminated waters. A comparison between natural hydroxyapatite (fish bones), synthetic hydroxyapatite nanoparticles (HAP) and alginate-hydroxyapatite composite (Alg/Hap) was carried out to assess their removal efficiencies to remediate the selected heavy metals.

2. Materials and Methods2.1. Equipment

A scanning electron microscope (SEM) was used equipped with FEI Quanta 250 Orbit to monitor and characterize the surface morphology of all nanobiosorbents under study. A JEOL-JEM2100 (Japan) high resolution transmission electron microscope (HR-TEM) was applied to determine the particle size diameters and the inner surface morphology of all nanobiosorbents. A FT-IR spectra was recorded on a Shimazdu Prestige-21 FTIR between 400 and 4000 cm⁻¹. A Powder X-ray diffractometer (XPERT-PRO-Analytical-Netherland) was used to evaluate the surface structure of the prepared nanobiosorbent by using Ni-filtered CuKα radiation at 45 KV in the range of 10 - 80 (2-theta) and by using K = 0.9 as Scherrer constant. The crystalline size is calculated by using Scherrer Equation (1):

D = 0.9 λ β cos θ (1)

where λ is the wavelength of the X-ray radiation and β is the full width at half maximum of the peaks at a diffracting angle θ.

Thermogravimetric analyses (TGA) were carried out in a nitrogen atmosphere using Perkin-Elmer TGA7 Thermo balance. The selected operating conditions are a temperature heating range = 20˚C - 600˚C, a heating rate = 10 ˚C∙min⁻¹, a flow rate = 20 mL∙min⁻¹ pure nitrogen atmosphere and the sample mass was taken in the range of 5.0 - 6.0 mg.

Determination of metals concentrations was carried out by using an Agilent atomic absorption spectrophotometer (240 AA Spectrometer). The flame unit was used together with an auto-sampler (Agilent SPS3 Autosampler) for automated flame operation at the appropriate wavelength for each metal.

2.2. Preparation of Different Biosorbents2.2.1. Preparation of Nanopowders Hydroxyapatitefrom Fish Scales

Bones of Tilapia nilotica fish were collected from a local market, and then washed with hot distilled water for several times to remove any organic compounds. Additional washing with 0.1 M HCl followed by distilled water for several times. The remaining proteins of fish bones were then treated with 5% NaOH, heated and stirred at 70˚C for 5 hr. Next, the washed fish bones were dried in an oven at 80˚C and then ground by ball mill and sieved for the desired size range. The HAP nanopowder was then washed thoroughly with deionized water until the washing solution became neutral and then dried at 80˚C [29] .

2.2.2. Preparation of Nanohydroxyapatite (HAP)

Hydroxyapatite compounds were prepared by the solution-precipitation method using calcium nitrate (Ca(NO₃)₂·4H₂O) and diammonium hydrogen phosphate ((NH₄)₂HPO₄), in addition to ammonia solution for pH adjustment. A suspension of Ca (NO₃)₂·4H₂O ( 23.61 g in 350 ml distilled water) was vigorously stirred at 25˚C. A solution of (NH₄)₂HPO₄ ( 7.92 g in 250 ml distilled water) was slowly added dropwise to the Ca(NO₃)₂·4H₂O solution. In all experiments pHs were kept at 11 by ammonia solution. This can be explained by the following reaction:

1 0 Ca ( NO 3 ) 2 ⋅ 4H 2 O + 6 ( NH 4 ) 2 HPO 4 + 8NH 4 OH → Ca 1 0 ( PO 4 ) 6 ( OH ) 2 + 2 0 NH 4 NO 3 + 2 0 H 2 O

Precipitated HAP was removed from the solution by centrifugation at 3000 rpm. The resulting powder was dried at 80˚C [30] .

2.2.3. Preparation of Alginate/Hydroxyapatite Composite (Alg/Hap)

The alginate/hydroxyapatite composite was prepared by dissolving 1.5 g of sodium alginate (SA) in 36 mL of distilled water at 40˚C and 1000 rpm. After the complete dissolution of SA, 0.6 g of diammonium hydrogen phosphate ((NH₄)₂HPO₄) was dissolved in 12.5 mL of distilled water. Then it was added slowly into the SA aqueous solution with stirring the mixture for 1 hr to ensure the homogeneity of the system. Subsequently, the aqueous solution containing SA and (NH₄)₂HPO₄ was added dropwise into 6% Ca(NO₃)₂∙4H₂O (30 g in 500 mL distilled water) aqueous solution at 30˚C with moderate stirring (50 rpm) through a 1.2 mm inner diameter needle, using a hypodermic syringe. The pH of the system was maintained in the range 10 - 10.5 using ammonia solution. The milky white composite beads were formed immediately (Figure 1) and further cross linked for 16 hr. After that, the Alg/Hap composite beads were filtered and rinsed three times with distilled water to remove the excess Ca(II) and other impurities on the surface of the beads. It then dried at 40˚C overnight [31] .

2.3. Biosorption Studies

All batch sorption experiments were carried out at room temperature (25˚C ± 1˚C). Each experiment was performed by mixing a 1.0 ml of 0.1 mol∙L⁻¹ metal ion solution in 50 mL pyrex bottle with 30 mg of the dry biosorbent and the pH was adjusted by adding 9.0 ml of buffer solution (pH 1-7). Then shaking by using a shaker for 30 min, filtered and washed with 50 ml distilled water. The residual metal ions in the filtrate were determined by EDTA titrations and each experiment was repeated three times.

To estimate the effect of mass of the novel cellulose sorbent, similar batch experiments were carried out by using different biosorbents masses of 5.0, 10.0, 15.0, 20.0, 30.0, 40.0 and 50.0 mg.

The effect of the reaction time was investigated for different shaking time of 5, 10, 15, 20, 30, 40 and 50 min) at the optimum buffering condition of each metal.

Sorption equilibrium and isotherm studies were evaluated by varying the initial metal ion concentration from 0.025 to 1.0 M.

Removal and biosorption capacity of Cd(II) and Pb(II) ions were investigated in presence of other competing ions of molar concentration. The examined solutions were prepared by mixing a 1.0 mL of 0.1 mol∙L⁻¹ solution of the metal under study with a 100 mg of an interfering ion (Na(I), K(I), Ca(II) and Mg(II)) individually. The residual metal content was determined by atomic absorption spectrometer.

Biosorption capacity of metal ions (µmol∙g⁻¹) was calculated from Equation (2).

q = ( C o − C ) V m × 10 3 (2)

where, C_o and C (mol∙L⁻¹) are the initial and residual metal ion concentration respectively, V (L) is the aqueous volume of the sorption reaction, m (g) is the mass of dry biosorbent and q (µmol∙g⁻¹) is the biosorption metal capacity that represents the amount of metal ion (µmol) adsorbed per gram of dry biosorbent.

2.4. Removal of Cd(II), Pb(II), Cr(VI), and Hg(II) Ions from Seawater and Wastewater Samples

Seawater samples were collected from the Eastern harbor and El-Max bay at the Egyptian Mediterranean Coast in addition to a wastewater sample collected from Al-Qala drain at Lake Mariout. Water samples were studied and evaluated to examine the efficiency of various biosorbents for removal and selective extraction of Cd, Pb, Cr(VI), and Hg(II) ions. Each sample was first analyzed to identify the concentrations of each metal ion and then spiked with Cd, Pb, Cr(VI), and Hg(II) ions. One liter of each sample was passed triplicate times throughout a multi-stages micro-column packed with 100 mg of the dry biosorbent under constant flow rate (10 mL∙min⁻¹). The effluent was collected and the concentrations of different metals were analyzed by the atomic absorption spectrometer. The percentage of metal extraction was then calculated using Equation (3).

% = ( C o − C ) C o × 100 (3)

where, C_o and C (mol∙L⁻¹) are the initial and residual metal ion concentration respectively [32] .

3. Results and Discussion3.1. Surface Morphology and Characterization

The SEM micrographs of the different biosorbents before the adsorption process are shown in Figures 2(a)-(c) for natural fish bones (F.B), synthetic hydroxyapatite (HAP)and (C) alginate hydroxyapatite composite (Alg/Hap).to adsorb on its surface. The pores with its clear openings facilitate the accessibility of metal ions adsorption into the internal part of the biosorbent [33] .

HR-TEM micrographs of the different biosorbents are shown in Figures 3(a)-(c) for natural fish bones (F.B), synthetic hydroxyapatite (HAP) and alginate hydroxyapatite composite (Alg/Hap), respectively. Powders were dispersed in ethanol under ultra-sonication. Then a drop of the solution was placed onto a Cu grid coated with a thin holey carbon film. The samples were measured at 200 kV. It is noticed that there are several numbers of heterogeneous porous layer which may provide a good possibility for the adsorption of the examined metals.

Fourier transform infrared (FT-IR) spectroscopy was employed to characterize the different functional groups of (HAP) powder obtained from fish bones, synthetic hydroxyapatite (HAP) and alginate hydroxyapatite composite

(Alg/Hap) (Figures 4(a)-(c)). All Peaks assignments are listed in Table 1. Stretching (3430 cm⁻¹) and vibration (634 cm⁻¹) peaks illustrate the characteristic bands of the HAP structure. The broad band at 3430 cm⁻¹ corresponds to stretching mode of hydroxyl (-OH) groups. A broad band at (2800 - 3400 cm⁻¹) was mainly due to stretching vibrations of -OH groups of adsorbed water. The band at (1658 cm⁻¹) is attributed to the ν₂ bending mode of the H₂O molecule. The group of bands between (1410 - 1550 cm⁻¹) were assigned to carbonate (CO₃)²⁻. The intense bands in the range of (950 - 1100 cm⁻¹) corresponding to P-O stretching vibration mode (asymmetric or ν₃) of the phosphate groups. The sharp peaks at (604 - 560 cm⁻¹) correspond to the (O-P-O) bending mode [29] .

XRD patterns of HAP (Ca₁₀(PO₄)₆(OH)₂) powder obtained from fish bones, synthetic hydroxyapatite (HAP) and alginate hydroxyapatite composite (Alg/Hap) are shown in Figures 5(a)-5(c); respectively. Crystal size was calculated according to Debye-Scherrer equation and listed in Table 2. It should be noted that the particle dimension obtained by HR-TEM is higher than the corresponding calculated crystal size. This difference may be explained by the presence of aggregates in HR-TEM grain consisting of several crystallites [31] .

Table 1 FT-IR peaks positions and their assignments for different biosorbents

Peak assignment	Peak position wave number (cm⁻¹)
Peak assignment	F.B	HAP	Alg/Hap
Stretching O-H	3430	3470	3400
Adsorbed water	3400 - 2800	3250	3100
Bending mode, ν₂ of adsorbed water	1658	1650	----
Stretching mode, ν₃ of CO 3 2 − group	1456	1410	1380
Asymmetric or ν₃of (PO₄)³⁻ group	1030	1050	----
The O-P-O bands of (PO₄)³⁻ group	604 - 560	630 - 560	552
Asymmetric stretching vibration of the carboxylate (-COO^-) groups	----	----	1630
The C-O-C (cyclic ether) stretching vibration	----	----	1040

The strong absorption band at (1630 cm⁻¹) in case of Alg/Hap is attributed to asymmetric stretching vibration of the carboxylate (-COO⁻) groups on the polymeric backbone.

The absorption band at (1040 cm⁻¹) is attributed to the C-O-C (cyclic ether) stretching vibration. An absorption band can be observed at (552 cm⁻¹) which is attributed to the bending of PO 4 3 − of HA. The broad band (3100 cm⁻¹) is assigned to stretching of the -OH groups of absorbed water [30] .

The TGA thermograms of the studied biosorbents are shown in Figure 6. The first endothermic region ranged from 30˚C to 400˚C was corresponding to the dehydration of the precipitating complex and the loss of physically adsorbed water molecules. The weight loss in this region is approximately 16% in case of natural fish bone (Figure 6(a)); while this percentage increase slightly in synthetic hydroxyapatite powder due to the remaining water content from the preparation (Figure 6(b)). With increasing temperature from 400˚C to 600˚C no peak has been observed, except a weight loss of 4% - 6% which is probably due to the gradual hydroxylation in hydroxyapatite powder.

Table 2 Average Crystal size of basic peaks for different biosorbents

Sorbent	Peak Position (2 Theta)	FWHM*	Average Crystal Size (nm)
F.B	30.17	2.30	3.75
HAP	31.85	1.17	7.33
Alg/Hap	31.77	1.67	5.14

FWHM = Full Width at Half Maximum.

The TGA of alginate hydroxyapatite graph (C) shows loss of water below 200˚C at about 15%. The weight loss between 200˚C - 400˚C (around 25%) indicates the rupture of chains, fragments, and monomers in Alg/Hap. This step is mainly related to the possible loss of organic content loaded on the surface of hydroxyapatite [34] .

3.2. Biosorption Studies3.2.1. Effect of the Medium pH on the Metal Biosorption Capacity

The effect of pH value of contact solution on the metal sorption capacity values was studied in various acidic and neutral solutions at different pH 1.0 - 7.0 as plotted in Figure 7(a) & Figure 7(b). The results of this study for Pb(II) are

shown in Figure 7(a). The efficiency of all biosorbents towards lead (II) removal was strongly affected by the solution pH. As a general trend, the maximum sorption capacity values were observed at pH 1. In addition, the lead sorption was found to gradually decrease from pH 1 to pH 3 followed by a significant decrease to a minimum value at pH 7. The high sorption capacity values observed at lower pH values (pH < 7); where the biosorbents are positively charged; are attributed to the predominance of the cation exchange mechanism [35] . On the other hand, the effect of pH on the Cd(II) sorption capacity indicated that the maximum biosorption capacities of various investigated biosorbents were observed at pH 5 (Figure 7(b)). The metal biosorption was found to gradually increase from pH 1 to pH 4, followed by a dramatic rising in the biosorption capacity values by the pH 5 and pH 6. By increasing the pH value to pH 7, maximum biosorption capacity values were obtained by the studied and evaluated biosorbents. In addition, at low pH, the low sorption capacity values are attributed to the interference caused by the high concentration of hydrogen ions which occupy active binding sites leading to inhibition of metal sorption. The significant increase in metal ions uptake in the range of pH 4 - 7, is mainly due to increasing the active binding sites by deprotonation of the surface functional groups occurred at higher pH [32] .

The results indicated also that the maximum biosorption capacities of various investigated biosorbents were observed at pH 5 for Cr(VI) and pH 6 for Hg(II). The metal biosorption was found to gradually increase from pH 1 to pH 4, followed by a dramatic rising in the biosorption capacity valuesin case of Cr(VI) at pH 5 and pH 6 in case of Hg(II). Worth mentioning that the low sorption capacity values at low pH values are attributed to the interference caused by the high concentration of hydrogen ions which occupy active binding sites leading to inhibition of metal sorption [36] . The significant increase in metal ions uptake in the range of pH 4 - 7, is mainly due to increasing the active binding sites by deprotonation of the surface functional groups occurred at higher pH [32] .

The functional groups responsible for binding with heavy metal ions are generally in the form of hydroxyl (-OH), phosphate ( PO 4 3 − ), carbonate ( CO 3 2 − ) in the three phases and carboxylate (-COO⁻) for Alg/Hap only. Two dominant mechanisms for the ability of HAP to take up divalent cations have been proposed [36] . The first mechanism is the adsorption of metal ions on the HAP surfaces following an ion exchange reaction between metal ions adsorbed and Ca(II) ions of HAP. These ion exchange reaction mechanisms are expressed as:

Ca 1 0 ( PO 4 ) 6 ( OH ) 2 + xM 2 + → xCa 2 + + Ca 1 0 − x M x ( PO 4 ) 6 ( OH ) 2 (4)

The second mechanism is the dissolution of HAP in aqueous solution containing metal ions followed by precipitation such as hydroxyl pyromorphite [Pb₁₀(PO₄)₆(OH)₂, HPy] in case of solution containing Pb(II) i.e., the dissolution-precipitation mechanism, which is written as:

Dissolution:

Ca 1 0 ( PO 4 ) 6 ( OH ) 2 + 14H + → 1 0 Ca 2 + + 6H 2 PO 4 − + 2H 2 O (5)

Precipitation:

1 0 Pb 2 + + 6H 2 PO 4 − + 2H 2 O → 14H + + Pb 1 0 ( PO 4 ) 6 ( OH ) 2 (6)

The comparable study of all investigated biosorbents towards Pb(II), and Cd(II) biosorption indicates that:

- The optimum buffering condition of all biosorbents for Pb(II) removal is pH 1; while that for Cd(II) is pH 5 at which each biosorbent exhibit maximum metal sorption capacity.

- The maximum Pb(II) sorption capacity values of all biosorbents are similar in the beginning (at low pH values) but have slightly difference in the ending as the following order: Alg/Hap > F.B > HAP.

While, that for Cd(II) removal are in the order of: HAP > Alg/Hap > F.B.

- The maximum Cr(VI) sorption capacity values of all biosorbents are in the order of: HAP = Alg/Hap > F.B. While, that for Hg(II) removal are in the order of: HAP > F.B > Alg/Hap.

3.2.2. Effect of the Reaction Contact Time on the Metal Biosorption Capacity

To identify the change in biosorption capacity values versus the contact time factor, the metal ion solution was shaken with 30 ± 1 mg of each biosorbents, F.B, HAP, Alg/Hap at different times. The sorption capacity values (µmol∙g⁻¹) of Pb(II), Cd(II), Cr(VI) and Hg(II) as a function of reaction contact time are shown in Figures 8(a)-(d). The metal ions uptake processes by all biosorbents were found to proceed with high rate of metal sorption capacity values after 5 min of the contact time. The interaction between metal ions and the biosorbent was generally found to proceed via two successive stages. The first stage involves a rapid increase in the removal efficiency of the metal ions onto biosorbents due to the abundant availability of active binding sites on biosorbent surface, and with gradual occupancy of these sites, the metal biosorption become less efficient. The second stage, at which the equilibrium is reached, is mainly based on the complete saturation (100%) of the biosorbent surface with the target metal ions. The fast operating time is one of the advantages of using these investigated biosorbentsas the biosorption equilibrium of each metal ion with all biosorbents were established within ~15 - 20 minutes. The maximum biosorption values of Pb(II) obtained at equilibrium are the same for all three biosorbents and equal 2785 µmol∙g⁻¹; while the maximum sorption values of Cd(II) obtained at equilibrium are 675, 1250 and 812 µmol∙g⁻¹ for F.B, HAP and Alg/Hap; respectively. On the meantime, the maximum biosorption values of Cr(VI) obtained at equilibrium are 1013, 1109 and 1221 µmol∙g⁻¹ for F.B, HAP and Alg/Hap; respectively. While the maximum biosorption values of Hg(II) obtained at equilibrium are 866, 1533 and 583 µmol∙g⁻¹ for F.B, HAP and Alg/Hap; respectively. In the light of the above, it can be concluded that one of the vital advantages of these biosorbents as solid phase extractors is saving operation time (about 20 min).

3.2.3. Effect of the Biosorbent Dosage on the Metal Biosorption Capacity

The effect of the biosorbent dosage on the biosorption capacity values were investigated under optimum buffering conditions for each metal ion by different biosorbent doses (5 - 50 mg) with initial concentration (0.1 mol∙L⁻¹) of each metal ion (Figures 9(a)-(d)). The maximum biosorption capacity was achieved when 5 mg biosorbent dose was used.

Based on the previous results, it can be concluded that the biosorption capacity values of the examined metal ions showed a decreasing order with increasing the biosorbent dosage until achieve equilibrium [37] . However, the high determined metal biosorption capacity values in lower biosorbent doses (5 and 10 mg) are mainly due to the high availability of metal ion solution compared to the exposed surface area as well as active centers. In the case of high sorbent dose (50 mg), the opposite trend was observed. This behavior may be attributed to the formation of aggregates during biosorption causing a direct decrease in the effective uptake with respect to the exposed surface area at high biosorbent dosage [29] [38] .

3.2.4. Effect of Interfering Ions on the Metal Biosorption Capacity

The effect of matrix or interfering ions can be presented by a competitive study for the sorption of the metal ion under study in presence of other interfering cations. A number of competing species were used in this study including Na(I), K(I), Ca(II) and Mg(II) by using equimolar concentration of each metal ion. This study was performed at optimum conditions for each metal ion by various

biosorbents, F.B, HAP, and Alg/Hap (Figures 10(a)-(d)). The results of the metal biosorption capacity values in presence of an interfering ion and the value obtained in absence of the interfering ion for Pb(II), Cd(II), Cr(VI) and Hg(II) are listed in Table 3. It was found that Na(I) and K(I) causing limited inference behaviors compared to Ca(II) and Mg(II). The different affinities of interfering ions in competitive biosorption are due to the difference in their ionic charges and ionic radii as well as the nature of functional groups present on the biosorbent [39] .

The results of the present study confirmed that the effect of interfering ions on the metal biosorption by different biosorbents is based on the following order: Ca²⁺ > Mg²⁺ > K⁺ > Na⁺.

3.3. Potential Applications of Biosorbents for Removal of Pb, Cd, Cr(VI), and Hg(II) Ions from Water Samples

The potential applications of the biosorbents for removal and sorption of Pb, Cd, Cr(VI), and Hg(II) from seawater samples were studied. The concentrations of Pb and Cd ions in water samples before removal are illustrated in Table 4.

In general, the slight decrease in the removal values of Pb and Cd ions from the seawater samples compared to those obtained in the case of the synthetic seawater sample may be attributed to the possibility of presence of other interfering ions such as sulfate, phosphate, or other nutrients in the seawater which compete with the metal ions towards the active binding sites on the biosorbent surface.

Table 3 Effect of interfering ions on (a) Pb(II), (b) Cd(II), (c) Cr(VI) and Hg(II) biosorption capacity

Interfering ions	Pb(II)	Biosorption (µmol∙g⁻¹)	Capacity	Cd(II)	Biosorption (µmol∙g⁻¹)	Capacity	Cr(VI)	Biosorption (µmol∙g⁻¹)	Capacity	Hg(II)	Biosorption (µmol∙g⁻¹)	Capacity
	F.B	HAP	Alg/Hap	F.B	HAP	Alg/Hap	F.B	HAP	Alg/Hap	F.B	HAP	Alg/Hap
In absence of ions	2785	2785	2785	675	1250	812	965	1173	1141	866	1533	583
Na(I)	2685	2742	2657	650	1125	750	917	1141	1093	833	1466	533
K(I)	2628	2714	2614	637	1075	712	869	1109	1061	816	1423	483
Ca(II)	2108	2154	2042	577	1017	637	645	981	933	747	1244	304
Mg(II)	2174	2271	2148	587	1039	665	725	1013	949	771	1323	336

The extractions of metal ions were successfully accomplished by triplicate analysis via a multi-stages micro-column system and the percentage extraction values by different biosorbents for each metal ion (Table 4). It is important to report here that the fish bones (F.B) (Natural Hydroxyapatite), synthetic hydroxyapatite (HAP), and modified hydroxyapatite (Alg/Hap) biosorbents exhibited high efficiency for removal of different metal ions (>90%).

4. Conclusion

The current work describes a method to prepare nanopowder of natural hydroxyapatite from fish bone of the tilapia (F.B), to synthesis the same substance (HAP) chemically and prepare the hydroxyapatite composite with alginic acid (Alg/Hap) to use as biosorbent materials. The modified sorbents were used for

Table 4 Comparative study of concentrations of Pb(II) (mg∙L<sup>−1</sup>), Cd(II) (mg∙L<sup>−1</sup>), Cr(VI), and Hg(II) in different water samples before removal and after using F.B (%), HAP (%), and Alg/HAP (%)

Area	Before removal				F.B.				HAP				Alg/HAP
	Pb(II) (mg∙L⁻¹)	Cd(II) (mg∙L⁻¹)	Cr(VI) (mg∙L⁻¹)	Hg(II) (mg∙L⁻¹)	Pb(II) (%)	Cd(II) (%)	Cr(VI) (%)	Hg(II) (%)	Pb(II) (%)	Cd(II) (%)	Cr(VI) (%)	Hg(II) (%)	Pb(II) (%)	Cd(II) (%)	Cr(VI) (%)	Hg(II) (%)
Eastern harbour	1.554	1.087	1.0376	0.174	90.92	93.11	91.39	91.95	93.11	94.28	92.75	93.67	91.82	92.40	93.16	90.80
El-Max bay	1.639	1.018	1.0282	0.363	90.11	90.05	93.66	93.66	91.15	90.88	93.25	94.76	91.94	91.58	94.32	93.11
Al-Qalaa drain	1.553	1.016	1.0439	0.549	91.95	91.22	93.39	91.25	91.75	92.92	91.22	94.71	91.17	92.60	91.60	93.07

sorption and solid phase extraction of Pb(II) and Cd(II) ions. Surface characterization and modification were examined and confirmed by using the SEM, HR-TEM, FT-IR, XRD, and TGA. The biosorption studies were studied and accomplished by using the batch techniques for removal and selective extraction of the metal ions previously mentioned. Various experimental factors affecting biosorption capacity such as solution pH, contact time, biosorbent dosage, initial metal concentration and presence of competitive ions were studied. Removal of Pb(II) ions was observed to selectively carried out at pH 1 - 2. The removal percentage values of different metal ions were >90% even in presence of other interfering ions

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

Cite this paper

Shreadah, M.A., Rizk, O.E.M., Aly-Eldeen, M.A., Rashad, A.R. and Mahmoud, M.E. (2019) Removal of Some Toxic Ions from Seawater and Wastewater by Sorption onto Natural, Synthetic Hydroxyapatite and Alginate-Hydroxyapatite Composite Nanoparticles: A Comparative Study. Journal of Environmental Protection, 10, 1155-1173. https://doi.org/10.4236/jep.2019.109069

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ElDeeb, M.K.Z., Said, T.O., El Naggar, M.H. and Shreadah, M.A. (2007) Distribution and Sources of Apliphatic and Polycyclic Aromatic Hydrocarbons in Surface Sediments, Fish and Bivalves of Abu Qir Bay. Bulletin of Environmental Contamination and Toxicology, 78, 373-379. https://doi.org/10.1007/s00128-007-9173-z

Abdel Ghani, S.A., Shobier, A.H., Said, T.O. and Shreadah, M.A. (2010) Organotin Compounds in Egyptian Mediterranean Sediments. Egyptian Journal of Aquatic Research, 36, 221-229.

AbdelGhani, S.A., Shobier, A.H. and Shreadah, M.A. (2013) Assessment of Arsenic and Vanadium Pollution in Surface Sediments of the Egyptian Mediterranean Coast. Journal of Environmental Technology and Management, 16, 82-101.https://doi.org/10.1504/IJETM.2013.050673

Abdel Salam, S., El Zokm, G., Shobier, A., Othman, T. and Shreadah, M.A. (2013) Metal Pollution in Surface Sediments of Abu Qir Bay and the Eastern Harbour of Alexandria, Egypt. The Egyptian Journal of Aquatic Research, 39, 1-12. https://doi.org/10.1016/j.ejar.2013.03.001

Abd ElMoneam, N.M., Abd ElMaguid, N.E., El-Sikaily, A.M., Zaki, M.G. and Shreadah, M.A. (2016) Biomarkers and Ultra Structural Evaluation of Marine Pollution by Polycyclic Aromatic Hydrocarbons. Journal Environmental Protection, 7, 1283-1304. https://doi.org/10.4236/jep.2016.710113

Shreadah, M.A., El-Sikaily, A.M., Abd El Moneam, N.M., Abd El Maguid, N.E. and Zaki, M.G. (2017) Polycyclic Aromatic and Aliphatic Hydrocarbons in Two Egyptian Coastal Areas along the Mediterranean Sea. Expert Opinion Environmental Biology, 6, 2. https://doi.org/10.4172/2325-9655.1000145

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Shriadah, M.A. and Emara, H.I. (1991) The Distribution of Chromium, Copper, Cadmium, and Lead in Areas of Multi-Polluting Factors of Alexandria. International Proceedings Symposium of Marine Chemistry in the Arab Region, Suez, April 1991, 30-50.

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Emara, H.I., Shriadah, M.A., Moustafa, T.H. and El-Deek, M.S. (1995) Trace Metals-Nutrient Salts Relationship in Coastal Seawater of Alexandria. MEDCOAST, Tarragona, Spain, 24-27 October 1995, 1457-1464.

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Shreadah, M.A., Said, T.O., Abd El Ghani, S.A. and Ahmed, A.M. (2008) Alkyllead and Alkyltin Species in Different Fishes Collected from the Suez Gulf, Egypt. Egyptian Journal Aquatic Research, 34, 64-73.

Masoud, M.S., Said, T.O., El-Zokm, G. and Shreadah, M.A. (2010) Speciation of Fe, Mn and Zn in Surficial Sediments from the Egyptian Red Sea Coasts. Chemical Speciation and Biodiversity, 22, 257-269. https://doi.org/10.3184/095422910X12894975123773

Khalil, M.K., El-Zokm, G.M., Fahmy, M.A., Said, T.O. and Shreadah, M.A. (2013) Geochemistry of Some Major and Trace Elements in Sediments of Edku and Mariut Lakes, North, Egypt. World Applied Sciences Journal, 24, 282-294.

Shreadah, M.A., Fahmy, M.A. and Fattah, L. (2015) Heavy Metals in Some Fish Species and Bivalves from the Mediterranean Coast of Egypt. Journal of Environmental Protection, 6, 1-9. https://doi.org/10.4236/jep.2015.61001

Taha, A.A., Shreadah, M.A., Heiba, H.F. and Ahmed, A.M. (2016) Multi-Component Adsorption of Pb(II), Cd(II), and Ni(II) onto Egyptian Na-Activated Bentonite; Equilibrium, Kinetics, Thermodynamics, and Application for Seawater Desalination. Journal of Environmental Chemical Engineering, 4, 1166-1180.https://doi.org/10.1016/j.jece.2016.01.025

Taha, A.A., Shreadah, M.A., Heiba, H.F. and Ahmed, A.M. (2017) Validity of Egyptian Na-Montmorillonite for Adsorption of Pb2+, Cd2+ and Ni2+ under Acidic Conditions: Characterization, Isotherm, Kinetics, Thermodynamics and Application Study. Asia-Pacific Journal of Chemical Engineering, 12, 292-306.https://doi.org/10.1002/apj.2072

Yakout, A.A., El-Sokkary, R.H., Shreadah, M.A. and Abdel Hamid, O.G. (2016) Removal of Cd(II) and Pb(II) Ions from Wastewater of Different Matrices by Using Triethylenetetramine Functionalized Cellulose Acetate Crafted Copolymer-Manganese Dioxide Composite. Carbohydrate Polymer, 148, 406-414.https://doi.org/10.1016/j.carbpol.2016.04.038

Yakout, A.A., El-Sokkary, R.H., Shreadah, M.A. and Abdel Hamid, O.G. (2017) Cross- Linked Graphene Oxide Sheets via Modified Extracted Cellulose with High Metal Adsorption. Carbohydrate Polymer, 172, 20-27. https://doi.org/10.1016/j.carbpol.2017.05.004

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