Advertisement

SN Applied Sciences

, 1:239 | Cite as

Adsorption of acid orange 10 on cross-linked porous polyimide

  • Zengxin Pan
  • Xin Zhang
  • Xinbo WangEmail author
Research Article
  • 185 Downloads
Part of the following topical collections:
  1. 1. Chemistry (general)

Abstract

In this work, a cross-linked porous polyimide (PI) network, fabricated from an “elongated” dianhydride and melamine, was synthesized by polycondensation and thermal dehydration. The as-prepared PI revealed an excellent adsorption performance and removal for acid orange 10 (AO-10) from aqueous solution. The adsorption quantity can reach 599 mg/g when the initial concentration is 500 mg/L with the temperature 298 K and pH value of 3. The maximum desorption ratio can be 38.9%. It is expected that the adsorption quantity and desorption ratio can be optimally improved by changing the length of PI monomer, indicating the cross-linked porous PI network is not only served effectively in sewage treatment but also recycled. Pseudo-2nd-order kinetic model and Langmuir isotherm are better fitted with the kinetic data and the adsorption equilibrium data respectively.

Keywords

Porous polyimide Adsorption Desorption Acid orange 

1 Introduction

Dyes are widely used in fibers, plastics, rubbers, inks, leathers, foods, paper-making, etc. The extensive application of dyes greatly satisfies people’s daily life. But it also brings environmental pollution especially industrial wastewaters containing dyes. These industrial wastewaters that contaminated with trace amount of dyes can even cause significant damage to people’s health [1]. Therefore, many methods [2, 3, 4, 5, 6] have been developed to dispose wastewaters containing dyes. Among these approaches, adsorption is usually adopted as a very simple and effective method.

In the past few decades, porous polymers are often used as adsorbing materials in sewage treatment [7, 8, 9]. Among numerous porous polymers, porous polyimide (PI) network has attract much attention because of their excellent mechanical strength, thermal stability and chemical resistance compared with other porous polymers. PI simultaneously contains abundant aromatic components, nitrogen and oxygen atoms in the backbone. In addition, it can be easily functionalized with polar functional groups such as –NH2, –COOH, –CF3, –SO3H and –OH [10, 11, 12, 13, 14], which can generate high affinity towards some gas, guest molecules or ions. Therefore, porous PI network is well-suited for adsorbent. Jens Weber et al. [10] fabricated a new microporous polyimide with strong fluorescence based on perylene type dianhydride, which has a high selectivity adsorption for CO2. Zhonggang Wang et al. [15] synthesized a microporous polyimide network using multi-amino monomer tetraphenyladamantane as crosslinking monomer which exhibited 14.6 wt% uptake of CO2 at 273 K and 1 bar as well as 1.27 wt% uptake of H2 at 77 K and 1 bar.

Here, we reported a cross-linked porous PI network using melamine and an “elongated” dianhydride (Scheme 1). In consideration of abundant N atoms in the PI structure, the adsorption/desorption behavior and the adsorption kinetics were discussed in detail to evaluate the adsorption/desorption of the prepared porous PI network for azo dye acid orange 10 (AO-10, Fig. 1).
Scheme. 1

Synthesis route of cross-linked porous PI network

Fig. 1

Chemical structure of AO-10

2 Experimental

2.1 Materials

All reagents were obtained from Sinopharm Cheical Reagent Co., Ltd (Shanghai, China). Melamine (MA) was dried at 120 °C for 4 h under vacuum before use. Pyromellitic dianhydride (PMDA) and 4,4′-oxydianiline (ODA) were purified by sublimation in vacuo before use. Dimethylsulfoxide (DMSO, ≥ 99.5%) was dried using molecular sieve. Acetone was used directly.

2.2 Fabrication of cross-linked porous PI network

2.00 g (10 mmol) ODA was dissolved in 42.40 g DMSO at room temperature under stirring; 4.36 g (20 mmol) PMDA was added in small quantities after which the system was stirred continuously for 12 h in ice-water bath with N2 atmosphere; then 1.26 g MA was added and stirred at room temperature until it was dissolved completely; the reaction system was heated to 180 °C for 24 h with stirring and cooled to room temperature naturally. The yellow solid was collected through filtering and Acetone-washing. Finally, cross-linked porous PI network was obtained after the yellow solid was dried at 120 °C for 4 h under vacuum.

2.3 Characterization

Fourier transform infrared spectroscopy (FTIR) spectra were recorded at a resolution of 1 cm−1 with a Nicolet 380 spectrometer. The surface morphologies were recorded by field-emission scanning electron microscopy (FESEM) on a JEOL JSM-6700F using accelerating voltages of 1.5 to 3 keV. The thermogravimetric analysis (TGA) was performed using a TG209F3 instrument thermal analyzer system (Netzsch) at the heating rate of 10 °C/min under N2 condition with a flow rate of 50 mL/min. Nitrogen sorption isotherms were conducted on a BET-201A sorptometer from Porous Materials at − 196 °C.

2.4 Adsorption and desorption tests

The synthesized porous PI network was dried in vacuum at 120 °C for 8 h in advance before adsorption test. A series of AO-10 aqueous solutions with different concentration (50 mg/L, 100 mg/L, 200 mg/L, 300 mg/L, 400 mg/L, 500 mg/L) were prepared and the pH values were adjusted to 3 and 7 respectively with hydrochloric acid solution. 2 mg adsorbent (porous PI network) was put in the 10 ml adsorbate solution (AO-10 aqueous solutions) of known concentration at 25 °C and standed for adsorption. The adsorbate solution was separated from adsorbent using 0.22 μL syringe after adsorption with different time. The concentration of separated adsorbate solution was recorded by an UV–Vis detector (wavelength 190–950 nm, Perkin–Elmer). The maximum absorption wavelength of adsorbate was 475 nm. Adsorption equilibrium quantity qa,e was determined by Eq. (1):
$$q_{a,e} = V_{a} \frac{{C_{a,0} - C_{a,e} }}{{m_{a} }}$$
(1)
where Va (L) is adsorbate solution volume and ma (mg) is the weight of the adsorbent; Ca,0 (mg/L) and Ca,e (mg/L) were the initial and equilibrium concentration of the adsorbate in solution, respectively.
The desorption test was conducted as following: the adsorbent was collected from adsorbate solution (Ca,0 = 500 mg/L, pH = 3) when standing for 58 h at 25 °C and dried at 70 °C for 24 h; then 0.7 mg dried adsorbent was added in 5 ml NaOH aqueous solution with the pH value 13 at the temperature 25 °C and standed for desorption. Desorption equilibrium amounts qd,e was determined by Eq. (2):
$$q_{d,e} = V_{d} \frac{{C_{d,e} }}{{m_{d} }}$$
(2)
where Vd (L) is the volume of NaOH aqueous solution with the pH value 13; md (mg) is the weight of the dried adsorbent after 58 h adsorption at 25 °C; Cd,e (mg/L) were the concentration of released adsorbate from adsorbent in NaOH aqueous solution after completion of desorption.

The depth profiling of adsorbate was determined by confocal Raman microscopy. The chemical composition depth profile of the PI/AO-10 bulk was characterized using a Raman microspectrometer, which combines a Renishaw Raman spectroscope and an inverted Leica DMIRBE microscopy. The laser was used as an excitation source and was focused through a 50× objective to ~ 1 μm light spot on the sample surface. Scattered light from the sample surface was collected through the same objective. Raleigh scattering light was cut off by a holographic notch filter. Raman light was passed through an entrance slit with a 65 μm opening and a 1200 L/mm diffraction grating and then measured by a CCD camera. For the distribution depth profile of the AO-10 within the PI/AO-10 bulk, Raman spectra were acquired from the surface of the focal planes at different depths.

3 Results and discussion

3.1 Characterization of PI

As shown in Fig. 2, the FTIR spectra of PI, AO-10 and PI/AO-10 indicated that the wavenumbers at 1775 cm−1, 1716 cm−1, 1373 cm−1 and 721 cm−1 were assigned as characteristic peaks of PI. 1175 cm−1 and 1034 cm−1 were the characteristic peaks of AO-10. After PI had been thoroughly standed in AO-10 solution and dried, the characteristic peaks of both PI and AO-10 appeared (blue curve in Fig. 2), which revealed a successful adsorption of PI to AO-10.
Fig. 2

FTIR spectra of PI, AO-10 and PI/AO-10

The thermal stability of the prepared PI was investigated with TGA in Fig. 3.
Fig. 3

TGA curve of PI under N2 atmosphere

The prepared PI networks exhibited excellent thermal stability with the onset of decomposition at ca. 400 °C (Td,10 = 435 °C) under N2 atmosphere in Fig. 3 as determined by TGA. Small weight losses were observed at the initial stages due to traces of solvent and other volatile substance trapped in the polymer networks. The high thermal stability of prepared PI is ascribed to the plenty of heteroaromatic rings and cross-linking structures in the network in addition to the intrinsic thermal stability of triazine ring from melamine [16].

From the FESEM image in Fig. 4, there exists highly aggregated clusters with the size 1–2 μm. Obvious petal-shaped patterns can be observed on the surface of every cluster indicating this morphology is beneficial for adsorption.
Fig. 4

FESEM image of PI network

Figure 5a shows a typical type IV isotherm (BDDT classification, IUPAC) [17]. The initial up-convex part of the Type IV isotherm is attributed to monolayer adsorption during which adsorbent surface has stronger adsorption ability for adsorbate and adsorption quantity increases rapidly. When relative pressure continues to increase, an inflection point appears indicating multilayer adsorption begins. The isotherm shows another convex shape is associated with capillary condensation taking place in mesopores, and the limiting uptake over a range of high P/P0. The hysteresis loop of Type IV isotherm can be referred to Type H2 loop, suggesting the existence of randomly distributed nanopores. The isotherm keeps going up at the range of high relative pressure (> 0.9) which implies strong interaction of adsorbent-adsorbate (PI and liquid N2 in BET test) and continuous multilayer adsorption. The specific surface area by BET is 110.38 m2/g. The average pore size is 6.7 nm using BJH method from Fig. 5b which is consistent with petal-shaped pattern appeared in the FESEM image of Fig. 4.
Fig. 5

a N2 adsorption-desorption isotherm obtained at 77 K of prepared porous PI; b pore size distribution calculated using the BJH method. The specific surface area around 113.38 m2/g can be estimated from the BET results. The average pore size distribution can be calculated according to the BJH method with the value 6.7 nm

3.2 Adsorption kinetics

As shown in Fig. 6, there is an evident pH-dependence adsorption quantity versus time curve. According to the distribution, adsorption quantity of AO-10 decreased sharply when the initial pH value increased from 3 to 7. There are plenty of long pair electrons in PI molecular structure owing to the electron donors (especially O and N atoms). Accordingly, PI surface will be positively charged from the adsorption of electron donors to H+. Meanwhile, AO-10 will form AO-SO 3 - and Na+ in water; AO-SO 3 - will approach H+ captured by electron donors which results in better adsorption of PI to AO-10 under acidic condition [18]. By contrast, adsorption quantity of PI to AO-10 under neutral condition decreased because lower H+ concentration weakened the interaction between PI surface and AO-10. Therefore, desorption testing can be designed on alkaline condition to evaluate the desorption capability based on the fact. The adsorption quantity increased steadily in both adsorption curves for pH = 3 and pH = 7 until adsorption equilibrium at the time nearly 1500 min. While qa,e value are 377 mg/g and 26 mg/g, respectively.
Fig. 6

The relationship between adsorption quantity and time

The pseudo-1st-order and pseudo-2nd-order kinetic models are introduced in order to evaluate adsorption behavior for Ca,0 = 200 mg/L and the kinetic parameters are listed in Table 1. The following equations were adopted to express the linear forms of pseudo-1st-order and pseudo-2nd-order kinetic models:
$$\ln \left( {q_{a,e} - q_{a,t} } \right) = \ln q_{a,e} - k_{1} t$$
(3)
$$\frac{t}{{q_{a,t} }} = \frac{1}{{k_{2} q_{a,e}^{2} }} + \frac{t}{{q_{a,e} }}$$
(4)
where qa,t is adsorption quantity at time t (min).
Table 1

The fitting parameters of pseudo-1st-order model and pseudo-2nd-order model

PH value

Pseudo-1st order

Pseudo-2nd order

K1 (/min)

q a,e cal (mg/g)

R2

k2 (g/mg min)

q a,e cal (mg/g)

R2

3

0.00228

190.8714

0.8618

0.00003

386.1004

0.9993

7

0.00258

27.9336

0.9050

0.00005

33.1236

0.9546

q a,e cal , calculated value of qa,e; k1, k2, rate constants of the pseudo-1st-order and pseudo-2nd-order models, respectively; R2, correlation coefficient

As shown in Fig. 7, correlation coefficient (R2) of pseudo-1st-order kinetic curve is lower than that of pseudo-2nd-order kinetic curve (0.8618 vs 0.9993, 0.9050 vs 0.9546) which means pseudo-2nd-order kinetic model has better correlation than pseudo-1st-order kinetic model. It also shows both calculated and experimental values of qa,e are well matched at the condition of pH = 3 (386.1004 mg/g vs 377 mg/g) combined with Table 1. This indicates that both chemical adsorption and physical adsorption exist during adsorption process under the above condition, in the meantime chemical adsorption is possibly the rate-limiting step and adsorption process is determined by electron sharing or electron exchange [19].
Fig. 7

Kinetic curves of a: pseudo-1st-order model and b: pseudo-2nd-order kinetic model with Ca,0 = 200 mg/g

If the movement of dye ions through the bulk liquid to the adsorbent solids is ignored, there are three steps in the adsorption process [20]: firstly, dye ions reach the adsorbent surface through boundary film of liquid–solid (film diffusion); secondly, dye ions arrive specific adsorption activity points via either surface diffusion and/or pore diffusion (intraparticular diffusion); thirdly, the dye ions are adsorbed on the surface of the adsorbent through the active sites. The first or the second step is the rate-determing step while the last step is rapid and assumed to be negligible. To describe the adsorption process of pH = 3, an intraparticular diffusion model developed by Weber and Morriss [21] expressed in Eq. (5):
$$q_{a,t} = k_{i} t^{0.5}$$
(5)
where ki is rate constant of intraparticular diffusion.
According to this model, plot of qa,t~t0.5 will be linear from Eq. (5) if the adsorption process is affected by the intraparticular diffusion. It is considered that the intraparticle diffusion is the only rate-controlling step when the line of qa,t~t0.5 passes through the origin. There are three stages of line segments appeared in Fig. 8 and it indicates that the process of intraparticular diffusion is involved. However, the three lines do not pass through the origin, indicating that some degree of film diffusion control and the intraparticular diffusion is not the only rate-controlling step 20. That the slope of the first line segment is bigger than that of the second means the first stage is faster than the second stage owing to the film diffusion to some extent. When the concentration of dye ions decreases with the extension of time, the diffusion rate of the film decreases at the same time leading to a decrease in the overall adsorption rate. More importantly, the intraparticle diffusion can be carried out in two stages. The adsorbate molecules rapidly fill the macropores and wider mesopores, and then penetrates the smaller mesopores more slowly [22]. The third line segment refers to the final equilibrium stage in which the intraparticular diffusion slows down and gradually disappears because the dye concentration is very low or has reached the maximum adsorption.
Fig. 8

The internal particle diffusion curve based on Eq. (5)

3.3 Concentration effect

It can be seen from Fig. 9 that qa,e increased with the increasing of Ca,0 under the condition of 298 K and pH = 3. qa,e value reached 599 mg/g when Ca,0 was 500 mg/L. This means our synthesized porous PI has adsorption or scavenging capability to AO-10. Meanwhile, as the increase of Ca,0, note that though acid orange dyes have some degree of solubility in water, they will change into aggregations followed by precipitation because of self-association and aggregation among dye molecules when the concentration is too high. However, when the dye concentration is below 0.01 M, the average aggregation is equal to 1 and the risk of aggregation of dye molecules goes away [23]. In our experiments the maximum initial concentration of AO-10 is 500 mg/L (that is 0.001 M) which implies no aggregation occurs in the concentration range during testing process.
Fig. 9

The effect of initial concentration on the adsorption of AO-10

3.4 Adsorption isotherm

Adsorption isotherms of AO-10 on PI with pH = 3 and pH = 7 are plotted in Fig. 10. Langmuir and Freundlich equations [24, 25] are employed to fit the adsorption isotherms shown in Eqs. (6) and (7):
$$q_{a,e} = \frac{{Q_{\hbox{max} } K_{L} C_{a,e} }}{{1 + K_{L} C_{a,e} }}$$
(6)
$$q_{a,e} = K_{F} C_{a,e}^{1/n}$$
(7)
$$\frac{{C_{a,e} }}{{q_{a,e} }} = \frac{{C_{a,e} }}{{Q_{\hbox{max} } }} + \frac{1}{{Q_{\hbox{max} } K_{L} }}$$
(8)
$$\ln q_{a,e} = \frac{1}{n}\ln C_{a,e} + \ln K_{F}$$
(9)
where Qmax (mg/g) is maximum adsorption quantity; KL (L/mg) is Langmuir constant; KF (mg/g (L/mg)1/n) and n are constants in Freundlich model. Equations (8) and (9) are linear form of Eqs. (6) and (7), respectively. The related parameters are summarized in Table 2. It is can be found that the correlation coefficient R2 of Langmuir model is higher than that of Freundlich model (0.9875 vs 0.9655, 0.9826 vs 0.8455), which demonstrates that the former is more suitable for the adsorption of AO-10 in our experiments and further implies adsorption activity points distribute evenly on porous PI surface. As a result, Qmax can be 833.33 mg/g (pH = 3) from Langmuir model. This is more favorable for our prepared porous PI to adsorb AO-10 and the prepared porous PI can eliminate AO-10 in aqueous solution effectively.
Fig. 10

a Langmuir model curve and b Freundlich model curve

Table 2

Parameters of AO-10 on porous PI fitted by Langmuir model and Freundlich model

Temperature (K)/pH value

Langmuir model

Freundlich model

KL(L/mg)

Qmax (mg/g)

R2

n

KF (mg/g (L/mg)1/n)

R2

298/3

0.0061

833.3333

0.9875

1.6453

17.3072

0.9655

298/7

0.0318

29.4724

0.9826

6.5466

10.9673

0.8455

Similar adsorption studies have been carried out with azo dyes as adsorbates [26, 27, 28]. Table 3 illustrates the capacity of azo dye adsorption using different adsorbents. Obviously organic adsorbents have higher adsorption capacity to azo dyes than inorganic adsorbents. Cross-linked chitosan has higher Qmax, but it takes longer time to reach Qmax value compared to cross-linked porous PI in this work. During the adsorption test, there is no shaking and only standed in this work while the adsorption process of cross-linked chitosan is shaking all the time; the initial concentration of adsorbate solution in this work is only half of that in the adsorption process of cross-linked chitosan. So to some extent, the cross-linked porous PI exhibits a high-efficiency adsorption capability to azo dyes among organic adsorbents.
Table 3

Comparison of maximum adsorption capacity (Qmax) of this work and other studies

References

Adsorbent

Adsorbate

pH and temperature (K)

Qmax (mg/g)

Time to reach Qmax (min)

Initial concentration of adsorbate (mg/L)

Shaking rate (rpm)

Model

This work

Cross-linked porous polyimide (powder)

Acid orange 10

3/298

599

1500

500

0

Langmuir

[26]

Cross-linked quaternary chitosan (powder)

Reactive orange 16

4/298

1060

2000

1000

250

Langmuir

[27]

Modified magnetic silica (powder)

Acid orange 10

3/298

61.33

200

48

400

Langmuir

[28]

Calcined Mg/Al layered double hydroxides

Acid orange 10

4/303

303.1

120

1000

Shaking (the accurate value is not mentioned)

Langmuir

3.5 Desorption

When pH value reaches to 13, lots of hydroxide anions gather around PI surface and consequently generates electrostatic repulsion with sulfonate anions. In such situation, the adsorption capability of porous PI to AO-10 decreases inevitably. As is shown in Fig. 11, desorption equilibrium is achieved at the time 120 h. Desorption rate was faster during the first 14 h and 51.5% of AO-10 was desorbed at the time of 14 h. Since qa,e value was 599 mg/g (Fig. 9) in the adsorption testing of Ca,0 = 500 mg/L and qd,e value was 233 mg/g in the desorption testing, it is can be calculated that 38.9% of adsorbed AO-10 was released and 61.1% of adsorbed AO-10 there is still kept in porous PI, which means once AO-10 is adsorbed into porous PI it is difficult to release. We speculate that maybe this is attributed to nano-size effect. Similar phenomenon was found in other research where liquid small molecule compound cannot be released even under reduced pressure after it was adsorbed into the nanochannels of porous matrix [29]. Thus, we believed 38.9% of the released AO-10 is more probably to lie in the very shallow surface area.
Fig. 11

Concentration–time curve of AO-10 desorption at pH = 13

We used Raman spectra to examine the dependence of bulk samples at different depths from the surface. In Fig. 12, the wavenumbers at solid lines and dash lines can be marked as the characteristic peaks of PI and AO-10 respectively. We can conclude that no AO-10 is adsorbed at the depth of adsorbent lower than 20 μm from Fig. 12a; while in the desorption testing no signals of AO-10 were found at the surface and the depth of adsorbent lower than 20 μm (Fig. 12b). This strongly confirms that AO-10 is adsorbed by PI in the depth range of 0–20 μm from PI surface and only a small amount of AO-10 in depth range of 0–5 μm from PI surface is released during the desorption process, indicating most AO-10 is kept in the depth range of 5–20 μm. There must exist competition repulsion and attraction between AO-10 and PI during desorption process.
Fig. 12

Raman spectra taken with a focal plane of bulk samples at different depths from the surface of a: adsorption testing and b desorption testing

As is mentioned above, all concentrations of AO-10 are lower than the aggregation concentration and thus AO-10 appears as a single stretchable molecule in aqueous solution used in this article. Since AO-10 is still a small molecule, the size of a single AO-10 molecule is not greater than 1 nm. AO-10 can easily enter the channel of the synthesized porous PI (average pore diameter is 6.7 nm from Fig. 5b). So electrostatic interaction became the only factor to determine the adsorption/desorption of AO-10 when porous PI is used. During the adsorption process of pH = 3, electrostatic interaction is favorable to adsorption. As more AO-10 molecules are adsorbed in the channels of porous PI, a certain degree of pore-blocking appears unavoidably. It is this reason that no AO-10 molecules were adsorbed at the depth lower than 20 μm. The smaller of the pores, the easier to block the pore channels for adsorbate. Hence, it is believed that the adsorbed layer will become thinner if the pore size decreases. Note that for our porous PI, the pore size can be fine-tuned by regulating the length of dianhydride as demonstrated in Scheme 1. Correspondingly, during the desorption process, different pore size will also affect thickness of the desorbed layer (0–5 μm for the desorption testing in our work) and further desorption efficiency. The relationship between the length of dianhydride and adsorption/desorption is very critical, and the related work is underway.

4 Conclusions

A cross-linked porous PI network was fabricated by an “elongated” dianhydride and used as an efficient adsorbent for the adsorption of AO-10. The prepared PI displayed good thermal stability, abundant micro/mesopores with average pore size 6.7 nm. The adsorption equilibrium quantity can reach 377 mg/g under the condition of 298 K, pH = 3 and Ca,0 = 200 mg/L within 1500 min. The maximum desorption ratio can be 38.9% under the condition of 298 K, pH = 13 after adsorption equilibrium of Ca,0 = 500 mg/L. Pseudo-2nd-order kinetic model is better fitted with the kinetic data. The Langmuir isotherm correlated better with the adsorption equilibrium data and the maximum adsorption capacity to AO-10 is 833.33 mg/g at 298 K. Meanwhile, changing the length of PI monomer can fine-tune the pore size of synthesized porous PI, suggesting a potential approach to better improve the adsorption of AO-10 by porous PI.

Notes

Acknowledgements

The authors are very grateful for the assistance in all characterization and testing from the Analysis and Testing Center of School of Materials Science and Engineering, Harbin Institute of Technology (Weihai).

Compliance with ethical standards

Conflict of interest

The authors declare that they have no conflict of interest.

References

  1. 1.
    Ahmad T (2009) Oil palm biomass-based adsorbents for the removal of water pollutants-a review. J Hazard Mater 167:1–9CrossRefGoogle Scholar
  2. 2.
    Shi BY et al (2007) Removal of direct dyes by coagulation: the performance of preformed polymeric aluminum species. J Hazard Mater 143:567–574CrossRefGoogle Scholar
  3. 3.
    Chen W, Lu W, Yao Y, Xu MH (2007) Highly efficient decomposition of organic dyes by aqueous-fiber phase transfer and in situ catalytic oxidation using fiber-supported cobalt phthalocyanine. Environ Sci Technol 41:6240–6245CrossRefGoogle Scholar
  4. 4.
    Mahanta D, Madras G, Radhakrishnan S, Patil S (2009) Adsorption and desorption kinetics of anionic dyes on doped polyaniline. J Phys Chem B 113:2293–2299CrossRefGoogle Scholar
  5. 5.
    Mahanta D, Madras G, Radhakrishnan S, Patil S (2008) Adsorption of sulfonated dyes by polyaniline emeraldine salt and its kinetics. J Phys Chem B 112:10153–10157CrossRefGoogle Scholar
  6. 6.
    Alqadami A et al (2016) Adsorptive removal of toxic dye using Fe3O4–TSC nanocomposite: equilibrium, kinetic, and thermodynamic studies. J Chem Eng Data 61:3806–3813CrossRefGoogle Scholar
  7. 7.
    Zhang YL et al (2009) Superhydrophobic nanoporous polymers as efficient adsorbents for organic compounds. Nano Today 4:135–142CrossRefGoogle Scholar
  8. 8.
    Zou ZM, Jiang CH (2017) Solvothermal polycondensation of novolacs phenolic-resin to nanopowders and their derived activated nanocarbons as efficient adsorbents for water cleaning. J Porous Mater 24:1555–1564CrossRefGoogle Scholar
  9. 9.
    Hori K, Sano M, Suzuki M, Hanabusa K (2018) Preparation of porous polymer materials using water-in-oil gel emulsions as templates. Polym Int 67:909–916CrossRefGoogle Scholar
  10. 10.
    Liao YZ, Weber J, Faul CFJ (2015) Fluorescent microporous polyimides based on perylene and triazine for highly CO2-selective carbon materials. Macromolecules 48:2064–2073CrossRefGoogle Scholar
  11. 11.
    Kim J et al (2016) One-step synthesis of nano-porous monolithic polyimide aerogel. Microporous Mesoporous Mat 234:35–42CrossRefGoogle Scholar
  12. 12.
    Wang Y et al (2016) Porous polyimide framework: a novel versatile adsorbent for highly efficient removals of azo dye and antibiotic. React Funct Polym 103:9–16CrossRefGoogle Scholar
  13. 13.
    Einsla BR et al (2004) Sulfonated naphthalene dianhydride based polyimide copolymers for proton-exchange-membrane fuel cells. I. Monomer and copolymer synthesis. J Polym Sci Polym Chem 42:862–874CrossRefGoogle Scholar
  14. 14.
    Jin XZ, Ishii H (2005) Novel positive-type photosensitive polyimide with low dielectric constant. J Appl Polym Sci 98:15–21CrossRefGoogle Scholar
  15. 15.
    Shen C, Bao Y, Wang Z (2013) Tetraphenyladamantane-based microporous polyimide for adsorption of carbon dioxide, hydrogen, organic and water vapors. Chem Commun 49:3321–3323CrossRefGoogle Scholar
  16. 16.
    Wu F et al (2018) Controlled synthesis and evaluation of cyanate ester/epoxy copolymer system for high temperature molding compounds. J Polym Sci Polym Chem 56:1337–1345CrossRefGoogle Scholar
  17. 17.
    Sing KSW et al (1985) Reporting physisorption data for gas solid systems with special reference to the determination of surface-area and porosity (recommendations 1984). Pure Appl Chem 57:603–619CrossRefGoogle Scholar
  18. 18.
    Yang S, Wu Y, Wu Y, Zhu L (2015) Optimizing decolorization of acid fuchsin and Acid Orange II solution by MnO2 loaded MCM-41. J Taiwan Inst Chem Eng 50:205–214CrossRefGoogle Scholar
  19. 19.
    Ho YS, Mckay G (1999) Pseudo-second order model for sorption processes. Process Biochem 34:451–465CrossRefGoogle Scholar
  20. 20.
    Aksu Z, Tatli AI, Tunç O (2008) A comparative adsorption/biosorption study of Acid Blue 161: effect of temperature on equilibrium and kinetic parameters. Chem Eng J 142:23–39CrossRefGoogle Scholar
  21. 21.
    Weber WJ, Morris JC (1963) Kinetics of adsorption on carbon from solution. J Sanit Eng Div 89:31–60Google Scholar
  22. 22.
    Lorenc-Grabowska E, Gryglewicz G (2007) Adsorption characteristics of Congo Red on coal-based mesoporous activated carbon. Dyes Pigments 74:34–40CrossRefGoogle Scholar
  23. 23.
    Bracko S, Span J (1997) Osmotic coefficients of CI Acid Orange 7 in aqueous solution and in the presence of simple electrolyte. Dyes Pigment 35:165–169CrossRefGoogle Scholar
  24. 24.
    Haghseresht F, Lu GQ (1998) Adsorption characteristics of phenolic compounds onto coal-reject-derived adsorbents. Energy Fuel 12:1100–1107CrossRefGoogle Scholar
  25. 25.
    Tan IAW, Hameed BH, Ahmad AL (2007) Equilibrium and kinetic studies on basic dye adsorption by oil palm fibre activated carbon. Chem Eng J 127:111–119CrossRefGoogle Scholar
  26. 26.
    Rosa S et al (2008) Cross-linked quaternary chitosan as an adsorbent for the removal of the reactive dye from aqueous solutions. J Hazard Mater 155:253–260CrossRefGoogle Scholar
  27. 27.
    Atia AA, Donia AM, Al-Amrani WA (2009) Adsorption/desorption behavior of acid orange 10 on magnetic silica modified with amine groups. Chem Eng J 150:55–62CrossRefGoogle Scholar
  28. 28.
    Extremera R et al (2012) Removal of acid orange 10 by calcined Mg/Al layered double hydroxides from water and recovery of the adsorbed dye. Chem Eng J 213:392–400MathSciNetCrossRefGoogle Scholar
  29. 29.
    Uemura T et al (2008) Sol−gel synthesis of low-dimensional silica within coordination nanochannels. J Am Chem Soc 130:9216–9217CrossRefGoogle Scholar

Copyright information

© Springer Nature Switzerland AG 2019

Authors and Affiliations

  1. 1.School of Materials Science and EngineeringHarbin Institute of Technology (Weihai)WeihaiPeople’s Republic of China

Personalised recommendations