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Appendix A. Supplementary data for
Effective Capture of Aqueous Uranium from Saline Lake with Magnesium-based
Binary and Ternary Layered Double Hydroxides
Jingwei Tu a,b, Xiaoqian Peng a,b, Shuting Wang a,b , Chen Tian a,b,*, Hong Deng a,b, Zhi
Dang a, Guining Lu a, Zhenqing Shi a, Zhang Lin a,b
a School of Environment and Energy, The Key Laboratory of Pollution Control and
Ecosystem Restoration in Industry Clusters (Ministry of Education), South China
University of Technology, Guangzhou, Guangdong 510006, China
b Guangdong Engineering and Technology Research Center for Environmental
Nanomaterials, South China University of Technology, Guangzhou, Guangdong
510006, China
Submitted to Science of the Total Environment
*Corresponding author
E-mail: [email protected] (Dr. Chen Tian)
Content
Supplemental Materials and Experiments
12 pages, 7 figures, 5 tables
Table S1
Isotherm parameters of U(VI) adsorption by MgAl-LDH and MgAlFe-LDH for
Freundlich simulation.
MgAl-LDH MgAlFe-LDH
U(VI)Kf
(mg g-1)
n R2Kf
(mg g-1)
n R2
Whole 126.43 2.81 0.945 186.94 2.09 0.932
part A 580.22 1.95 0.9569 976.42 1.33 0.992
part B 151.52 4.06 0.9348 169.03 3.50 0.931
Table S2
Comparison of the distribution coefficient value (Kd) of MgAl-LDH and MgAlFe-
LDH with other adsorbents.
MaterialExperimental
conditionsKd (L g-1) References
MgFeAl LDH T = 298 K, pH = 5.0 96.63 (Song et al.,
2018)
NiFeAl LDH T = 298 K, pH = 5.0 3.00 (Song et al.,
2018)
rGO/LDH T = 298 K, pH = 5.0 234.67 (Tan et al.,
2015)
HTlca T = 298 K, pH = 4.0 53.23 (Zhang et al.,
2014)
Fe3O4@C@Ni-Al LDH T = 298 K, pH = 6.0 19.55 (Zhang et al.,
2013)
magnetic citrate MgAl LDH T = 298 K, pH = 6.0 4.88 (Zhang et al.,
2012)
clinoptilolite zeolite T = 298 K, pH = 6.0 62.50 (Camacho et
al., 2010)
Saccharomyces cerevisiae T = 298 K, pH = 6.0 13.23 (Bai et al.,
2016)
amidoximated silica T = 298 K, pH = 5.0 5.72 (Yin et al.,
2017)
Oxime-mesoporous carbon T = 298 K, pH = 4.5 1.24 (Tian et al.,
2011)
talc T = 298 K, pH = 4.5 0.28 (Sprynskyy et
al., 2011)
POP-oNH2-AO T = 298 K, pH = 6.0 Around
8.36 × 106
(Sun et al.,
2018)
MgAl-LDH T = 298 K, pH = 6.0 377.31 This work
MgAlFe-LDH T = 298 K, pH = 6.0 434.78 This work
Table S3
Kinetic parameters of U(VI) adsorption by MgAl-LDH and MgAlFe-LDH
sorbent
Pseudo-first-order model Pseudo-second-order model
Qe
(mg g−1 )
k1
(min−1)R2
Qe
(mg g−1)
k2
(g mg−1 min−1)R2
MgAl-LDHs 4.849 0.01168 0.9723 22.13 0.008540 0.9995
MgAlFe-LDHs 3.813 0.008797 0.8330 23.07 0.01032 0.9996
Table S4
Specific surface areas and pore parameters of MgAl-LDH and MgAlFe-LDH
samples
Surface
area(m2/g)a
Pore diameter
(nm)b
Pore volume
(cm3/g)b
MgAl-LDH 90.0114 36.74247 0.826810
MgAlFe-LDH 132.1487 30.25010 0.999378
a Performed by multipoint BET method.
b Cumulative desorption pore volume and average pore diameter performed by BJH method.
Table S5
Desorption yields of some desorptive solutions.
EluantConcentration
(mol L-1)
Desorption efficiency for
MgAl-LDH
(%)
Desorption efficiency for
MgAlFe-LDH
(%)
H2O - 6.35 5.15
NaOH 0.5 23.29 23.19
Na2CO3 0.5 41.59 52.99
HCl 0.5 87.4 93.81
Fig. S1 TGA curves of as-prepared MgAl-LDH and MgAlFe-LDH samples.
100 200 300 400 500 600 700 800 90050
60
70
80
90
100
110M
ass (
%)
Temperature ( )℃
MgAlFe-LDH MgAl-LDH
Fig. S2 The Fredundlich fitting for U(VI) adsorption in part A (C0=0.2 mg L-1 to 5 mg
L-1) , part B (C0=5 mg L-1 to 30 mg L-1).
Fig. S3 U(VI) adsorption and desorption percentages in 5 consecutive cycles for
MgAl-LDH and MgAlFe-LDH.
90
92
94
96
98
100
102
54321
uran
ium
rem
oval
rat
e (%
)
cycles
MgAl-LDH MgAlFe-LDH
Fig. S4 Effect of initial pH on adsorption property of MgAl-LDH and MgAlFe-LDH.
Fig. S5 Species distribution of U(VI) species without precipitation as a function of
pH. C0 = 0.5 mg L-1, T = 25 .℃
Fig. S6 Zeta potentials of LDHs at pH= 6-9.
Fig. S7 FT-IR spectra of MgAl-LDH and MgAlFe-LDH samples after U(VI) sorption.
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