The XRD patterns (Fig. 1) revealed that the as-prepared samples contain alumina (JCPDS card No. [04-0875]) at 600 and 800°C and some minor amorphous or less crystallized phases appearing as a bump at the 2θ angles of 20°–30°. When the temperature was increased to 1000°C, the Al2O3 peaks became sharper and narrower, whereas the amorphous phase disappeared probably because it reacted with or doped into Al2O3 upon the heat treatment. When the temperature was further increased to 1200°C, mullite (JCPDS card No. [02-0431]) was detected. Therefore, the unidentified phase may be SiO2 because a similar bump at the identical 2θ angles (20°–30°) in the corresponding XRD profiles was previously proven to be SiO2 [22,38]. The existence of Si–O–Si or Si–OH in the network below 1000°C was then confirmed.
FTIR spectroscopy was performed on various samples, including the as-dried, 800°C-heated and 1000°C-heated samples, to verify the formation of Si–O–Si, Al–O–Si, or Si–OH bond in the as-prepared aerogels (Fig. 2). The as-dried one showed Si–OH stretching vibration at 956 cm−1, confirming its existence in the gel network and verifying the reaction between TEOS and H2O has taken place. When the temperature was increased to 800 and 1000°C, the Si–OH peaks (956 cm−1) shifted towards 800 cm−1, suggesting that the H atoms were gradually replaced by Si atoms in the network, forming the symmetric Si–O–Si bond . This result proves that the Si–OH bond initially formed as early as in the drying stage and then transformed into Si–O–Si bond at later processing stages [38–39].
Figure 2. FTIR of the as-prepared aerogels after drying and after firing at 800 and 1000°C (v is for stretching vibration).
On the other hand, Al–OH (474 cm−1), Al–O (632 cm−1), and Al−O−Al (1050 cm−1, stretching vibration) were also detected, indicating the hydrolysis reaction between AlCl3·6H2O and PO has taken place [38–39]. Furthermore, some Al–O–Si (1069 cm−1, stretching vibration ) bonds have also been detected when increasing temperature gradually. This result may be attributed to the condensation reactions between Al−OH and Si−OH/Si−OC2H5.
The presence of Al2O3 rather than SiO2 in the XRD (Fig. 1) and FTIR (Fig. 2) results can be ascribed to the much faster gelation speed and larger composition quantity of the former than the latter . In other words, as the Al−O−Al bond formed, the chance for Al–OH to react with Si–OH/Si–OC2H5 and form Al−O−Si bonds decreased. Hence, a mixture of mainly Al–O–Al and a possibly small amount of Si–O–Al was produced. Subsequently, Si–OH started to react with itself or Si−OC2H5, forming Si–O–Si. Consequently, SiO2 and Si–O–Si were detected in the XRD and FTIR profiles (Figs. 1 and 2), respectively.
Other peaks, such as C–H (2990 cm−1) and H–O–H (1610 cm−1), were also observed in the as-dried and 800°C-heated samples, indicating that some organic solvents remained after the gelation/cross-linking process. When the temperature was increased to 1000°C, the –OH and C–H completely disappeared due possibly to the pyrolysis of these organics.
Fig. 3 shows that the as-prepared aerogels heated at 800°C are porous with pore diameters ranging from 10 to 20 nm and locating between the loosely packed nanoparticles (average diameters of 50–100 nm). The pores are quite homogeneous. Figs. 4(a) and 4(b) from two different locations both show that the as-prepared Al2O3–SiO2 composite aerogels are needle-like and/or plate-like under a transmission electronic microscope, which is consistent with reference [40–41]. The Energy-dispersion X-ray spectroscopy (EDX) shows that the gels are composed of Al, Si, and O. This, together with the XRD and FTIR results, verifies the formation of Al2O3–SiO2 composite aerogels. Element mapping (Figs. 3(d)–3(f)) shows that Al, Si, and O are presented homogeneously at identical positions in the aerogel. Overall, the PO-assisted sol–gel technique enabled the gelation better than traditional sol–gel techniques by avoiding the long pH adjustment procedures and controlling the hydrolysis rate [38–39].
Figure 3. SEM (a, b) of the Al2O3–SiO2 composite aerogel, EDX (c) of point 1 in (b), and element mapping (d–f) corresponding to (b).
As seen from the adsorption–desorption loops (Fig. 5(a)), some clues can be drawn about the pore shapes from its H2 typed loops. These pore shapes might be stacking between the uniform nanoparticles, which is consistent with the SEM observations (Fig. 3). Furthermore, narrow distributions of pore sizes (Fig. 5(b)) were observed with the meso-pore sizes. The average diameters were 9.7, 13.4, 14.8, and 15.8 nm for the as-dried, 600°C-heated, 800°C-heated, and 1000°C-heated samples, respectively (Table 1).
Sample Average pore diameters / nm Total pore volume / (mL·g−1) Porosity BJH specific surface area / (m2·g−1) BET specific surface area / (m2·g−1) As-dried 9.7 1.46 86.0% 827.544 602.462 600°C 13.4 1.28 83.6% 657.778 381.520 800°C 14.8 1.08 81.2% 455.839 292.720 1000°C 15.8 0.59 70.0% 225.984 148.990
Table 1. Average pore diameters, total pore volume, porosity, and specific surface areas of the as-dried, 600°C-heated, 800°C-heated, and 1000°C-heated samples
Figure 5. Adsorption–desorption loop (a) and pore size distribution (b) of the aerogel after drying and firing at 600, 800, and 1000°C. P and P0 stand for pressure at measurement and at standard temperature, respectively; V stands for the volume of absorbed N2; d stands for pore diameter.
Besides, Table 1 shows that the Barrett–Joyner–Halenda (BJH) specific surface area of the as-dried aerogel was 827.544 m2/g, which was higher than those at 657.778, 455.839, and 225.984 m2/g after heat treatment at 600, 800, and 1000°C, respectively. The Brunauer–Emmett–Teller (BET) specific surface area and the pore volume data are also shown in Table 1, suggesting that the aerogel sample has the highest total pore volume of ~1.46 mL/g after OSSD drying, dropping to 1.28, 1.08, and 0.59 mL/g after heat treatment at 600, 800, and 1000°C, respectively. The corresponding porosity was calculated as 86.0% for the as-dried sample, 83.6% for the 600°C-heated sample, 81.2% for the 800°C-heated sample, and 70.0% for the 1000°C-heated sample. These data indicate that the main component is Al2O3 (Fig. 1) and its density is ~3.9 g/cm3. The porosity of this aerogel is up to 86.0%.
Such high surface areas and porosities can be possibly attributed to the OSSD drying method . OSSD reduces the surface tensions and capillary forces between the aerogel channels and walls better than other drying methods . It can also help the aerogel achieve relatively higher specific surface area and pore volume compared with previously reported aerogels (Table 2).
Preliminary tests were conducted on the absorption effect of aerogels on Cu2+. In these spectra, the remaining concentration of Cu2+ dropped sharply within 40 min and reached ~0 afterward (Fig. 6(a)), and the removal efficiency can reach 99% in 40 min (Fig. 6(b)). In addition, the qe (the absorption uptake at equilibrium) profile shows that the equilibrium Cu2+ uptake can reach ~69 mg/g (Fig. 6(c)). These results are better than those obtained in . This high absorption efficiency can be possibly ascribed to the high surface area as shown in the BET and BJH specific surface area measurements (Fig. 5 and Table 1). Furthermore, it has easy accessible pores (Fig. 3) and high porosity (Table 1), which has greatly facilitated the diffusion of Cu2+ into bulk aerogel materials . Finally, the multiple oxygen-containing functional groups (Al–OH, Si–OH, Al–O–Si, etc.) found in the composite aerogels (FTIR in Fig. 2) and the homogeneous distribution of Al, Si, and O (Fig. 3) might have afforded the aerogel excellent absorption properties . The high surface area, easily accessible pores with high porosity, and oxygen-containing functional groups have synergistically promoted the absorption of Cu2+.
Figure 6. Dependence of (a) Cu2+ concentration, (b) removal rate (%), and (c) uptake qe on contact time.
Absorption kinetics was examined by performing the following calculations as previously described . The absorption data of Cu2+ by the Al2O3−SiO2 composite aerogels are consistent with the calculations from the pseudo second-order kinetics model (R2 = 0.9944), which is much better than the pseudo first-order kinetics model (R2 = 0.8829), as shown in Fig. 7. Therefore, the absorption process may follow the pseudo second-order kinetics and be controlled by the chemical absorption where valence forces and electron exchanges take charge .
Figure 7. Fit between the experimental Cu2+ absorption data and (a) pseudo second-order kinetics or (b) pseudo first-order kinetics. t is for absorption time; qt and qe stand for the uptake amount of Cu2+ per gram of the absorbent at time t and at equilibrium, respectively.
The matches between the experimental and calculated data were evaluated using a normalized standard deviation ∆q (%) , to validate the pseudo second-order model. The ∆q (%) for the pseudo second-order model (82.55) fits more closely than the pseudo first-order one (148.83). Therefore, we speculated that the absorption of Cu2+ on the Al2O3–SiO2 composite aerogel follows the pseudo second-order kinetics.
Preparation of Al2O3–SiO2 composite aerogels and their Cu2+ absorption properties
11 November 2019
Revised: 30 May 2020
Accepted: 1 June 2020
Available online: 3 June 2020
Abstract: In order to remediate heavy metal ions from waste water, Al2O3–SiO2 composite aerogels are prepared via a sol–gel and an organic solvent sublimation drying method. Various characterisation techniques have been employed including X-ray diffraction (XRD), Fourier transform infrared spectrometry (FTIR), scanning electron microscope (SEM), Energy-dispersion X-ray spectroscopy (EDX), Brunauer–Emmett–Teller (BET) N2 adsoprtion isotherm, and atomic absorption spectrometer (AAS). XRD and FTIR suggest that the aerogels are composed of mainly Al2O3 and minor SiO2. They have a high specific surface area (827.544 m2/g) and high porosity (86.0%) with a pore diameter of ~20 nm. Their microstructures show that the distribution of Al, Si, and O is homogeneous. The aerogels can remove ~99% Cu2+ within ~40 min and then reach the equilibrium uptake (~69 mg/g). Preliminary calculations show that the Cu2+ uptake by the aerogels follows pseudo second-order kinetics where chemical sorption may take effect owing largely to the high surface area, high porosity, and abundant functional groups, such as Al–OH and Si–OH, in the aerogel network. The prepared aerogels may serve as efficient absorbents for Cu2+ removal.