Disulfide polymer grafted porous carbon composites for heavy metal removal from stormwater runoff

Abstract

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Polymeric Composites with Embedded Nanocrystalline Cellulose for the Removal of Iron(II) from Contaminated Water

“…The adsorption isotherms were then evaluated from the relationship between the amount of metal ions adsorbed on the surface of materials and that of the solution at equilibrium. These isotherms play a fundamental role in describing the nature of interactions between the sorbent and metal ions [7,14,20,21]. The adsorption isotherms of the composite for the removal of iron at acidic and basic pH were evaluated at a wide range of initial metal ion concentrations (Figure 3B).…”

“…The iron-binding capacities of magnetic graphene oxide showed similar adsorption behavior, and complete saturation of metal-binding sites was observed at the saturation capacity of 43 mg/g of nanocomposite [7]. The iron(II)-binding efficacies of the embedded-NCC polymeric composite at basic pH yielded a similar trend; however, an increase in iron-binding capacity (Qe of 52.5 mg/g and 90% removal efficiency) was observed due to the stronger electrostatic interactions between the iron ions and deprotonated functional groups of the polymeric composites [21]. The iron-binding capacity of the composite at equilibrium was found to be 32.3 mg/g and 52.5 mg/g at pH = 3.8 and pH = 10, respectively (Figure 3B).…”

“…This may present a heterogenous surface of the composite that follows the Freundlich isotherm [7]. Moreover, the stronger interactions between the polymeric composite and metal ions calculated from the Freundlich isotherm (n = 1.1; n >1 indicates stronger affinity) suggests that the sorption of iron(II) is facilitated on the surface of the composite [21] (Table 2). PEG-blended chitosan surfaces prepared for the chelation of iron(II) from contaminated water resources also showed strong correlation with the Freundlich isotherm and revealed that the adsorption of iron on the chitosan membranes was a heterogeneous process [28,29,31,32].…”

“…The pH of the filtrate was adjusted to 3.8 and the amount of iron in the supernatant was evaluated as described above. The equilibrium adsorption of the composites (Qe, mg/g) was calculated by taking into consideration the initial amount of iron in the solution and the amount of iron present in supernatant after the adsorption, according to Equation (1); the metal removal efficiency % (R%) was calculated by Equation (2); and the adsorption capacity (Q t ) at time ‘t’ was calculated by Equation (3):Q e = [(C 0 − C e ) × V]/m R (%) = [C 0 − C/m] × 100 Q t = [(C 0 − C t ) × V]/m where C 0 is the initial concentration, C t is the concentration at given time t, and C e is the equilibrium concentration of metal ions (mg/L) in solution; V is the total volume of solution (L); and m is the mass of composites [14,20,21].…”

“…The data were also fitted by the linear form of the Freundlich model:ln q e = ln K F + 1/ n ln C e where K F is the Freundlich constant of the relative adsorption capacity of the adsorbent and 1/ n indicates the heterogeneity factor or adsorption intensity [20,21].…”