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. 2022 Apr 30;15(9):3253.
doi: 10.3390/ma15093253.

Snail Based Carbonated-Hydroxyapatite Material as Adsorbents for Water Iron (II)

Bernard Owusu Asimeng  1 , Edward Kwame Amenyaglo  1 , David Dodoo-Arhin  2 , Johnson Kwame Efavi  2 , Bright Kwakye-Awuah  3 , Elvis Kwason Tiburu  1 , E Johan Foster  4 , Jan Czernuska  5
Affiliations

Snail Based Carbonated-Hydroxyapatite Material as Adsorbents for Water Iron (II)

Bernard Owusu Asimeng et al. Materials (Basel). .

Abstract

Carbonated hydroxyapatite (CHAp) adsorbent material was prepared from Achatina achatina snail shells and phosphate-containing solution using a wet chemical deposition method. The CHAp adsorbent material was investigated to adsorb aqua Fe(II) complex; [Fe(H2O)6]2+ from simulated iron contaminated water for potential iron remediation application. The CHAp was characterized before and after adsorption using infrared (IR) and Raman spectroscopy. The IR and the Raman data revealed that the carbonate functional groups of the CHAp adsorbent material through asymmetric orientation in water bonded strongly to the aqua Fe(II) complex adsorbate. The adsorption behaviour of the adsorbate onto the CHAp adsorbent correlated well to pseudo-second-order kinetics model, non-linear Langmuir and Freundlich model at room temperature of a concentration (20-100 mg L-1) and contact time of 180 min. The Langmuir model estimated the maximum adsorption capacity to be 45.87 mg g-1 whereas Freundlich model indicated an S-type isotherm curvature which supported the spectroscopy revelation.

Keywords: adsorption kinetics; carbonated-hydroxyapatite; iron(II) adsorption; water remediation.

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Conflict of interest statement

The authors declare no conflict of interest.

Figures

Figure 1
Figure 1
SEM image of CHAp.
Figure 2
Figure 2
IR spectra of CHAp adsorbent material (a) pristine CHAp (b) residue CHAp after Fe(II) adsorption.
Figure 3
Figure 3
Raman spectra of CHAp adsorbent material (a) pristine CHAp (b) residue CHAp after Fe(II) adsorption (c,d) are Raman spectroscopic imaging of pristine CHAp and residue CHAp, respectively.
Figure 4
Figure 4
Show adsorption capacity at time, qt for various concentrations (a) 20 (b) 40 (c) 60 (d) 80 and (e) 100 mg L−1 of aqua Fe(II) complex adsorbates. The pictures shown in (f) from deep orange-red to light orange after the equilibrium adsorption time indicates the removal of the adsorbates from the Fe(II) solution. The pH of the before and after ChAp treatment is ~3.68 and 7.69, respectively.
Figure 5
Figure 5
(a) pseudo-first-order (b) pseudo-second-order kinetic plots at room temperature for the CHAp adsorption of aqua Fe(II) complex adsorbates.
Figure 6
Figure 6
Nonlinear Langmuir and Freundlich isotherms at room temperature for the CHAp adsorption of aqua Fe(II) complex adsorbates.
See this image and copyright information in PMC

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