Modiﬁcation of Natural Peat for Removal of Copper Ions from Aqueous Solutions

: This study aimed at estimating peat adsorption properties for copper ion removal from aqueous solutions during peat modiﬁcation. Two peat modiﬁcations have been studied using batch tests and quantitatively reproduced with instrumental analysis by using spectrometric, potentiometric, and thermodynamic modeling methods. The ﬁrst variation—mechanical activation—was carried out in a planetary mill; for the second one—mechanochemical activation—dry sodium percarbonate (Na 2 CO 3 · 1.5H 2 O 2 ) was added. The adsorption of copper ions was studied in the concentration range from 10–150 mg/L with an interaction time from 0.25–12 h. Both modiﬁcations led to signiﬁcant changes in the interaction energy in the adsorption layer; thus, the acceptor properties of macromolecules were enhanced from natural peat to mechanically activated peat and mechanochemically activated peat. FTIR spectra, speciﬁc surface area characteristics, and sorption experiments show the predominantly chemical nature of copper sorption. Maximum adsorption capacity was determined to be 24.1, 42.1, and 16.0 mg/g for natural peat, mechanically activated peat, and mechanochemically activated peat, respectively. The example of peat mechanochemically oxidized with Na 2 CO 3 · 1.5H 2 O 2 shows that the improvement in the physicochemical properties (C BET and speciﬁc surface area) plays a smaller role in the sorption capacity in relation to copper ions than the presence of phenolic and carboxyl groups, the content of which decreases during oxidation. writing—original preparation, O.S. and T.S.; writing—review and editing, O.G., O.S., T.S., and E.P.; visualization, T.S.; supervision, O.S.; funding acquisition, O.S., T.S., and E.P.


Introduction
Despite the intention to switch to waste-free and environmentally friendly production, many industries still produce wastes containing toxic and carcinogenic organic and inorganic compounds. Wastewater often contains high concentrations of heavy metals, exceeding permissible standards. In such concentrations, heavy metals exhibit toxic properties and are not biodegradable. On the other hand, environmental regulations now require the treatment of contaminated waters before they can be discharged into receiving waters. The toughening of environmental laws and increased control in the field of nature management has propelled the search for reliable methods of wastewater treatment.
It is suggested that adsorption is one of the best methods, not only because of its simplicity and potential for regeneration but also because it is a cost-effective and environmentally friendly technology for removing heavy metals from wastewater [1][2][3][4][5][6][7][8][9][10]. Various materials have been suggested for use as a sorbent for contaminated water, including clay minerals, zeolites, zero-valent iron, polymers, activated carbon, adsorption resin, and where C 0 is initial concentration of copper ions in solution (mmol/L); C e is the equilibration concentration of copper in solution (mmol/L); q e is the amount of copper sorbed by peat at equilibrium time (mg/g).
The Langmuir equation is theoretically derived from simple mass-action kinetics, assuming chemisorption [46]. The linearized form of the Langmuir equation has been used to analyze the obtained adsorption results [45,47]: where C e and q e have the same definition as mentioned above; Q is the adsorption maximum (mmol/g); K L is a constant related to the intensity of adsorption (L/kg of peat).
The Freundlich isotherm is empirical and has been derived by assuming a heterogeneous surface with a nonuniform distribution of the heat of adsorption over the surface [48]. The linear expression of this isotherm can be written as [45,49]: log q e = log Kf + (1/n) log C e , where q e and C e have the same definition mentioned before; Kf and 1/n are positive valued adjustable parameters.
The parameter 1/n is varied between zero and one and it is a measure of the heterogeneity of adsorption sites on the surface of the adsorbent.

Thermodynamic Calculations
Calculations were performed in the heterophas 5-component system H-O-Cu-N-Ark-COOH at 25 • C and a total pressure of 1 atm by the GIBBS algorithm and UNITHERM database of the "HCh" software [50]. Here, Ark-COOH is a quasi-element with a Gibbs free energy of formation equal to zero. This quasi-element simulated the condensed ring of the corresponding acids (Ark) and peripheral acid groups of different types, mainly carboxyl (-COOH). These elemental structures are assumed to determine total acidity and to provide the formation of complexed compounds of peat HA with the main ions of natural water and heavy metals in particular.
A discrete site-specific nonelectrostatic model of the interactions of a Cu ion with FA and HA, is applied to the experimental data modeling. Copper binding is described with a site density (mmol/g) and two intrinsic equilibrium constants: dissociation of the carboxyl groups (-COOH) and association of the Cu 2+ with -COOH.

Characterization of Sorbents
Peat is a very heterogeneous material composed with a majority of organic compounds and detrital minerals. Metal(oid) concentrations, pH, and electrical conductivity (EC) detected in natural peat prior to the experiments are presented in Table 1. It is considered that the humidity and the saturated soil water content in Sphagnum peat are the highest. The moisture content of the peat moss is 92.7%, the ash content is 2.2%. At the same time, the bog water pH is 4.0 (slightly acidic). Peat properties reflect the peat-forming environment and the types of peat-forming plant. Among the elemental compositions of peat ash, the major elements Si, Ca, Al, S, Mg, Fe, and Na account for approximately 90% of the total elements of the ash. The content of Cu does not exceed 14 ppb. The content of organic substances in dry matter was observed at 97.8%. The results of elemental composition (C, H, N, and S), shown in Table 2, indicate significant similarity between the peat with those presented in the literature. The composition of peat varies depending on botanical composition, age, climate, and other environmental factors. Composition of C, H, and N revealed the H/C ratio of 1.5. The H/C ratio is associated with the degree of aromaticity; the lower the ratio, the greater the presence of aromatic compounds. C/N ratio correlates with the humification degree of peat, where a low C/N ratio usually indicates a high humification degree, and vice versa [51]. In our case, the ratio was 91.1. The surface morphology of the natural peat (NP) and the sorbents obtained after modification (MAP and MCAP) were characterized by scanning electron microscopy ( Figure 1). The morphology of the natural peat is represented by the remnants of plant tissues with a large number of conducting vessels and pores (Figure 1a) [30]. X-ray energy dispersive spectroscopy (EDS) data (TM1000 EDS detector (Hitachi, Tokyo, Japan), data not shown) indicate the following elements inherent in the peat composition: Al up to 1.5%, Si up to 1%, and Ca up to 0.51%. A microphotograph of the MAP sample ( Figure 1b) shows a characteristic pattern of mechanically processed plant materials with signs of plastic grinding, the structure of the material stratifies, and the particles greatly decrease in size. Small amounts of iron chafing (Fe up to 0.36% (EDS, data not shown)) may occur during mechanical activation. For the MCAP sample ( Figure 1c) under mechanochemical activation with Na 2 CO 3 ·1.5H 2 O 2 , the formation of a large number of small particles capable of aggregation on the larger crushed particles of the original peat is observed. The appearance of Na up to 1% in the MCAP sample composition is observed (EDS, data not shown).
grinding, the structure of the material stratifies, and the particles greatly decrease in size. Small amounts of iron chafing (Fe up to 0.36% (EDS, data not shown)) may occur during mechanical activation. For the MCAP sample ( Figure 1c) under mechanochemical activation with Na2CO3•1.5H2O2, the formation of a large number of small particles capable of aggregation on the larger crushed particles of the original peat is observed. The appearance of Na up to 1% in the MCAP sample composition is observed (EDS, data not shown).  Figure 2 shows the X-ray diffraction patterns of NP, MAP, and MCAP. It is shown that peat has an amorphous-crystalline structure characteristic of plant polymers [32]. Mechanical and mechanochemical influence leads to the amorphization of the peat crystal structure. XRD patterns of MAP and MCAP identified the hexagonal quartz phase in the composition, which may be present in peat samples up to 1%.  Figure 2 shows the X-ray diffraction patterns of NP, MAP, and MCAP. It is shown that peat has an amorphous-crystalline structure characteristic of plant polymers [32]. Mechanical and mechanochemical influence leads to the amorphization of the peat crystal structure. XRD patterns of MAP and MCAP identified the hexagonal quartz phase in the composition, which may be present in peat samples up to 1%.
As follows from the data presented in Table 3, both modifications of the peat sample led to significant changes in the interaction energy in the adsorption layer from 6.3 to 27.8. Differences in the values of the monolayer capacity and specific surface area indicate variations in the effects of mechanical and mechanochemical treatment of peat. The lowest specific surface area (BET method and Greg and Sing approximation) is a characteristic for the mechanically activated sample. The mechanochemical activation of peat in the presence of an alkaline oxidizing reagent results in increasing specific surface area and monolayer capacity, which may have an effect on the sorption capacity of the obtained sorbent. As follows from the data presented in Table 3, both modifications of the peat sample led to significant changes in the interaction energy in the adsorption layer from 6.3 to 27.8. Differences in the values of the monolayer capacity and specific surface area indicate variations in the effects of mechanical and mechanochemical treatment of peat. The lowest specific surface area (BET method and Greg and Sing approximation) is a characteristic for the mechanically activated sample. The mechanochemical activation of peat in the presence of an alkaline oxidizing reagent results in increasing specific surface area and monolayer capacity, which may have an effect on the sorption capacity of the obtained sorbent. The curves of inverse potentiometric titration of the studied peat samples by 0.1 M HCl solution, as well as the similar curve for a blank sample presented by 0.1 M NaOH are given in Figure 3. In the regions of рН 10-11, рН 6.9-9.5, and рН 2.5-6.0, three titrated groups-phenolic hydroxyls Ph-OH, carboxyl groups at aromatic rings Ar-СОOН, and carboxyl groups in hydrocarbon chains Alk-COOН-were established. By various amounts of acid groups in the study samples, a curve is shifted in the region of the lower values of titrant addition. By the inflection points of the curves, related to the electrode potential drop, neutral points are found corresponding to all the three aforementioned groups. Calculated contents of functional groups are given in Table 4.  The curves of inverse potentiometric titration of the studied peat samples by 0.1 M HCl solution, as well as the similar curve for a blank sample presented by 0.1 M NaOH are given in Figure 3. In the regions of рН 10-11, рН 6.9-9.5, and рН 2.5-6.0, three titrated groups-phenolic hydroxyls Ph-OH, carboxyl groups at aromatic rings Ar-CОOН, and carboxyl groups in hydrocarbon chains Alk-COOH-were established. By various amounts of acid groups in the study samples, a curve is shifted in the region of the lower values of titrant addition. By the inflection points of the curves, related to the electrode potential drop, neutral points are found corresponding to all the three aforementioned groups. Calculated contents of functional groups are given in Table 4.
According to the potentiometric titration, similar ratios of phenolic and carboxyl groups are determined in all three samples, however, with a decrease in their number from NP to MCAP samples. Therefore, the number of acid groups decreases in the peat composition. Peat becomes more hydrophobic, i.e., acceptor properties of macromolecules are enhanced (reaction capacity with ions), which is consistent with data on the determination of energy characteristics (C BET and a m ) from Table 3. The solution pH and presence of different background electrolytes effectively influence the adsorption efficacy towards ion adsorption and sorbent zeta-potential [52]. Cations of the inorganic salts can bind with the peat surface and the surface becomes positive (Cu 2+ ). The polarizability of the counter anions, such as NO 3 − , play a role in the variation of the surface charge of peat samples. The change in the surface charge of peat depending on the concentration of solution ions will be described in our following works.
FTIR analysis revealed main functional groups in the composition of peat samples and indicated qualitative changes during the modification of natural peat ( Figure 4). A broad absorption band with a maximum area from 3420-3400 cm −1 was assigned to the stretching vibrations of hydroxyl groups involved in intramolecular and intermolecular hydrogen bonds. The bands at 2925 and 2855 cm −1 are ascribed to the asymmetric and symmetric C-H stretching of methylene and methyl (CH 2 and CH 3 ) groups.  The band from 1710-1725 cm −1 , corresponding to the С=О-stretching vibrations of mainly carboxyl groups and other oxygenated functionalities, usually has high intensity in HA spectra. The band from 1610-1625 cm −1 , which refers to the stretching vibrations of the С=С conjugated groups in aromatic structures, including oxygen-containing groups such as quinones, hydroxylquinones, etc., as well as nitrogen-containing heterocycles. This region (1630 cm -1 ) is also responsible for bending vibrations of the O-H group of adsorbed water. The bands at 1515 cm −1 and 1420 cm −1 are attributed to skeletal vibrations of the lignin aromatic ring. Additionally, the bands at 1420 cm −1 and 1380 cm −1 are attributed to the asymmetric and symmetric bending vibrations of the C-H bond in methoxyl and methyl groups [53].
The band at 1270 cm −1 , together with the band at 1235 cm −1 , corresponds to skeletal vibrations of the aromatic ring and asymmetric stretching vibrations of the C-O bond in phenolic groups and aromatic ethers. The adsorption band in the area of 1156 cm −1 refers The band from 1710-1725 cm −1 , corresponding to the C=O-stretching vibrations of mainly carboxyl groups and other oxygenated functionalities, usually has high intensity in HA spectra. The band from 1610-1625 cm −1 , which refers to the stretching vibrations of the C=C conjugated groups in aromatic structures, including oxygen-containing groups such as quinones, hydroxylquinones, etc., as well as nitrogen-containing heterocycles. This region (1630 cm -1 ) is also responsible for bending vibrations of the O-H group of adsorbed water. The bands at 1515 cm −1 and 1420 cm −1 are attributed to skeletal vibrations of the lignin aromatic ring. Additionally, the bands at 1420 cm −1 and 1380 cm −1 are attributed to the asymmetric and symmetric bending vibrations of the C-H bond in methoxyl and methyl groups [53].
The band at 1270 cm −1 , together with the band at 1235 cm −1 , corresponds to skeletal vibrations of the aromatic ring and asymmetric stretching vibrations of the C-O bond in phenolic groups and aromatic ethers. The adsorption band in the area of 1156 cm −1 refers to the hydroxylic groups of alcohols, the bands of 1065 and 1036 cm −1 refer to the stretching vibrations of the C-O bond in the stretching of polysaccharidic structures [54]. For the MAP sample, the absorption bands of the O-H groups are shifted to the area of lower frequencies indicating a distinct intramolecular nature of hydrogen bonds and ordered structure. For the MCAP sample, the band in the area of 1724 cm −1 , corresponding to the carboxyl group vibrations, is not separately detected, merging with the band from 1610-1612 cm −1 and presenting on it in the form of a shoulder, which may be partly due to the oxidation during the mechanochemical treatment [55]. Such samples are usually humate, not humic acid. A decrease in absorption in the regions of 1725 and 1260 cm −1 , with a simultaneous increase in the area of 1613 and 1418 cm −1 , indicates the passage of a chemical reaction of neutralization of acidic groups of HA and their conversion into the form of sodium humate as a result of the mechanochemical treatment of peat with Na 2 CO 3 ·1.5H 2 O 2 .

Adsorption Studies of Cu(II) on Natural and Modified Peat
The degree of Cu 2+ sorption on the sorbents depends on initial solution concentration ( Figure 5). The effect of contact time on the copper ions adsorption on NP is low. The adsorption occurred rapidly within the first 30 min (gray circulars). These results indicated that chemical adsorption rather than intraparticle diffusion was the rate-controlling step [56]. With increasing initial concentration, the removal percent of copper ions decreases from 99% to ~75% due to the reduction in available adsorption sites. To be more precise, a large number of vacant surface sites are available for adsorption at a low concentration, whereas all the active sites are saturated with sorbate ions at a certain point. The increased concentration of metal ions is accompanied by a corresponding decrease in binding such that the total binding is constant when it is at its maximum value [57,58]. This is reflected in the model, which assumes competition of all ions for the same binding sites.
At the initial copper concentration of 150 mg/L (2.36 mmol/L), there is a slight increase in R,% to 84 ± 2%., that can be associated with the formation of a complex with another stoichiometry, for example, according to Equation (5). Precipitation of a solid phase of a CuO type at pH~3.5 according to the thermodynamic calculations should not occur [45,59]: Distribution ratio involves the water-peat ratio in an explicit way according to Equa- With increasing initial concentration, the removal percent of copper ions decreases from 99% to~75% due to the reduction in available adsorption sites. To be more precise, a large number of vacant surface sites are available for adsorption at a low concentration, whereas all the active sites are saturated with sorbate ions at a certain point. The increased concentration of metal ions is accompanied by a corresponding decrease in binding such that the total binding is constant when it is at its maximum value [57,58]. This is reflected in the model, which assumes competition of all ions for the same binding sites.
At the initial copper concentration of 150 mg/L (2.36 mmol/L), there is a slight increase in R,% to 84 ± 2%, that can be associated with the formation of a complex with another stoichiometry, for example, according to Equation (5). Precipitation of a solid phase of a CuO type at pH~3.5 according to the thermodynamic calculations should not occur [45,59]: Distribution ratio involves the water-peat ratio in an explicit way according to Equation (2). Figure 6a shows that sorption is most efficient at the lowest Cu concentration (log K D = 3.9), when the metal concentration increases, the ratio drops to log K D = 2.5. Thus, at the constant temperature and water-peat ratio of 100:1, the experimental distribution ratio does not reach constant values in the region up to C 0 = 2.36 mmol/L. If the distribution ratio at constant temperature varies, the distribution of components between the solution and peat is not subjected to a linear isotherm. At each point of the experiment, we can only talk about reaching the empirical equilibrium described by reaction Equation (5) and the relative equilibrium constant K emp (Equation (6)) [45,59]: Based upon the location of a point set of the same color in Figure 6, this empirical equilibrium is quickly attained, even at the highest concentrations; the time does not exceed 30 min.
Another important parameter affecting the sorption is the solution acidity: the logKD shows an inverse relationship with pH compared with a dependence on increasing concentration (Figure 6b). The equilibrium pH is slightly lower than the initial pH, indicating that H + /Na + release from carboxylic and phenolic groups during the adsorption process, and negatively charged macromolecules repel each other, making a greater number of active sites available for the adsorption of metal ions [60][61][62]. Distribution ratio increases with increasing pH, while the lower Cu-concentration solutions have pH from 3.7 to 4.2 (blue squares), and higher ones have pH from 3.2 to 3.6 (yellow and red squares). It is known, that the biosorption process is strongly pH-dependent and the level of metal binding is influenced by both H + ion competition and speciation effects [63,64]. Regular changes of copper concentrations in solution indicate a predominance of sorption affecting the visible change in the solution pH. A graph view (Figure 6b) allows to assume that the reaction Equation (7) is valid. The pH dependence of the metal ions adsorption can be explained by a competitive adsorption of copper and H + ions [45,59]: Alk-COOH + Cu 2+ = Alk-COOCu + + H + .
The adsorption of Cu 2+ on sorbents is shown in Figure 7. All three peat modifications (NP, MAP, and MCAP) remove copper ions from solutions with approximately the same efficiency. The confidence intervals for the initial and MA peat overlap in most values. Based upon the location of a point set of the same color in Figure 6, this empirical equilibrium is quickly attained, even at the highest concentrations; the time does not exceed 30 min.
Another important parameter affecting the sorption is the solution acidity: the logK D shows an inverse relationship with pH compared with a dependence on increasing concentration (Figure 6b). The equilibrium pH is slightly lower than the initial pH, indicating that H + /Na + release from carboxylic and phenolic groups during the adsorption process, and negatively charged macromolecules repel each other, making a greater number of active sites available for the adsorption of metal ions [60][61][62]. Distribution ratio increases with increasing pH, while the lower Cu-concentration solutions have pH from 3.7 to 4.2 (blue squares), and higher ones have pH from 3.2 to 3.6 (yellow and red squares). It is known, that the biosorption process is strongly pH-dependent and the level of metal binding is influenced by both H + ion competition and speciation effects [63,64]. Regular changes of copper concentrations in solution indicate a predominance of sorption affecting the visible change in the solution pH. A graph view (Figure 6b) allows to assume that the reaction Equation (7) is valid. The pH dependence of the metal ions adsorption can be explained by a competitive adsorption of copper and H + ions [45,59]: Alk-COOH + Cu 2+ = Alk-COOCu + + H + .
The adsorption of Cu 2+ on sorbents is shown in Figure 7. All three peat modifications (NP, MAP, and MCAP) remove copper ions from solutions with approximately the same efficiency. The confidence intervals for the initial and MA peat overlap in most values. Therefore, to analyze the differences in sorption efficiency, we further consider sorption isotherms. The amount of adsorbed Cu ion on MCAP decreased with the increase in Cu 2+ concentration. In sum, as confirmed by the sorption constants below, the MCA peat sample shows a worse ability to remove copper ions from solutions. It was expected that the mechanochemical oxidation of peat using Na2CO3•1.5H2O2 would proceed similarly to the examples described for brown coal. It has long been known that on the surface of brown coal many radicals are formed as a result of mechanical activation [65,66]. In [38] it was shown that the mechanochemical oxidation of brown coal by Na2CO3•1.5H2O2 occurs with the participation of a free radical mechanism and produces new oxygen-containing groups. By potentiometric titration (Table 4), a decrease in the number of Alk-COOH groups from 2.0 to 0.5 mmol/g for mechanochemically oxidized peat was proven. One can conclude that in the case of the mechanochemical treatment of peat with Na2CO3•1.5H2O2, the oxidation of carboxyl groups is more extensive and accompanied by their removal from the structure of organic matter. A similar effect was observed during the mechanochemical oxidation with Na2CO3•1.5H2O2 of chitosan, which is accompanied by deacetylation [67]. In addition, the alkaline component of Na2CO3•1.5H2O2 is also involved in the reaction, so the neutralization of acidic groups of HA occurs, which is reflected in the IR spectra ( Figure 4). In the IR spectra of MCAP, the band from 1710-1725 cm −1 is not separately detected, merging with the band from 1610-1612 cm −1 . Such samples are sodium humates, not HA. In addition to the data, obtained using potentiometric titration, that account for carboxyl groups in both the salt and acid states, we can conclude that the mechanochemical oxidation of peat with Na2CO3•1.5H2O2 is accompanied by decarboxylation. According to Tables 3 and 4, physicochemical properties for the MCAP sample were improved (CBET and Sspec), but they did not improve the sorption capacity of this sample with respect to copper ions.

Adsorption Isotherm
The equilibrium adsorption isotherms of copper ions on peat were built to establish the relationship between the physicochemical parameters of the sorbent and sorption ability. Figure 8 shows the graph obtained for the adsorption of Cu 2+ onto NP. This graph indicates an L-type adsorption isotherm, which is characterized by a decreasing slope as the adsorbate concentration increases due to increased coverage of vacant adsorption sites [18,47,68,69]. These results were then analyzed using Langmuir and Freundlich sorption It was expected that the mechanochemical oxidation of peat using Na 2 CO 3 ·1.5H 2 O 2 would proceed similarly to the examples described for brown coal. It has long been known that on the surface of brown coal many radicals are formed as a result of mechanical activation [65,66]. In [38] it was shown that the mechanochemical oxidation of brown coal by Na 2 CO 3 ·1.5H 2 O 2 occurs with the participation of a free radical mechanism and produces new oxygen-containing groups. By potentiometric titration (Table 4), a decrease in the number of Alk-COOH groups from 2.0 to 0.5 mmol/g for mechanochemically oxidized peat was proven. One can conclude that in the case of the mechanochemical treatment of peat with Na 2 CO 3 ·1.5H 2 O 2 , the oxidation of carboxyl groups is more extensive and accompanied by their removal from the structure of organic matter. A similar effect was observed during the mechanochemical oxidation with Na 2 CO 3 ·1.5H 2 O 2 of chitosan, which is accompanied by deacetylation [67]. In addition, the alkaline component of Na 2 CO 3 ·1.5H 2 O 2 is also involved in the reaction, so the neutralization of acidic groups of HA occurs, which is reflected in the IR spectra (Figure 4). In the IR spectra of MCAP, the band from 1710-1725 cm −1 is not separately detected, merging with the band from 1610-1612 cm −1 . Such samples are sodium humates, not HA. In addition to the data, obtained using potentiometric titration, that account for carboxyl groups in both the salt and acid states, we can conclude that the mechanochemical oxidation of peat with Na 2 CO 3 ·1.5H 2 O 2 is accompanied by decarboxylation. According to Tables 3 and 4, physicochemical properties for the MCAP sample were improved (C BET and S spec ), but they did not improve the sorption capacity of this sample with respect to copper ions.

Adsorption Isotherm
The equilibrium adsorption isotherms of copper ions on peat were built to establish the relationship between the physicochemical parameters of the sorbent and sorption ability. Figure 8 shows the graph obtained for the adsorption of Cu 2+ onto NP. This graph indicates an L-type adsorption isotherm, which is characterized by a decreasing slope as the adsorbate concentration increases due to increased coverage of vacant adsorption sites [18,47,68,69]. These results were then analyzed using Langmuir and Freundlich sorption parameters. From the slope and intercept of the lines in Figure 9a, the values of Q and KL were estimated and are listed in Table 5. The correlation factor (r 2 ) shows that the linear fit of Ce/qe vs. Ce is the highest for the MAP sample (0.997) over the concentration range from 3-50 mg/L. The Langmuir model assumes that the uptake of ions occurs on a homogenous surface by monolayer adsorption without any interaction between adsorbed molecules; hence, the mechanical treatment of peat moss (MAP) led to the formation of the more uniform sorbent. Maximum Cu 2+ adsorption capacity (Q) was determined to be 24.1, 42.1, and 16.0 mg/g for NP, MAP, and MCAP, respectively. The data obtained are well correlated with published data from different previous studies [70][71][72][73][74]. KL is a constant related to the intensity of adsorption and is the highest for the NP (0.3).  From the slope and the intercept of the straight line of logqe vs. logCe (Figure 9b), the values of Kf and n have been determined and are given in Table 4. The correlation coefficient (r 2 ) demonstrates that the Freundlich model is more suitable than the Langmuir model for the natural peat sample (NP). Therefore, it can be assumed that the process has a surface character [34]. This finding may imply that all groups (Table 4) are responsible for Cu 2+ adsorption behavior. The positive contribution of the carboxyl and phenolic groups and the aromatic compounds for adsorbing Cu 2+ has been previously reported [57]. From the slope and intercept of the lines in Figure 9a, the values of Q and K L were estimated and are listed in Table 5. The correlation factor (r 2 ) shows that the linear fit of C e /q e vs. C e is the highest for the MAP sample (0.997) over the concentration range from 3-50 mg/L. The Langmuir model assumes that the uptake of ions occurs on a homogenous surface by monolayer adsorption without any interaction between adsorbed molecules; hence, the mechanical treatment of peat moss (MAP) led to the formation of the more uniform sorbent. Maximum Cu 2+ adsorption capacity (Q) was determined to be 24.1, 42.1, and 16.0 mg/g for NP, MAP, and MCAP, respectively. The data obtained are well correlated with published data from different previous studies [70][71][72][73][74]. K L is a constant related to the intensity of adsorption and is the highest for the NP (0.3). From the slope and intercept of the lines in Figure 9a, the values of Q and KL were estimated and are listed in Table 5. The correlation factor (r 2 ) shows that the linear fit of Ce/qe vs. Ce is the highest for the MAP sample (0.997) over the concentration range from 3-50 mg/L. The Langmuir model assumes that the uptake of ions occurs on a homogenous surface by monolayer adsorption without any interaction between adsorbed molecules; hence, the mechanical treatment of peat moss (MAP) led to the formation of the more uniform sorbent. Maximum Cu 2+ adsorption capacity (Q) was determined to be 24.1, 42.1, and 16.0 mg/g for NP, MAP, and MCAP, respectively. The data obtained are well correlated with published data from different previous studies [70][71][72][73][74]. KL is a constant related to the intensity of adsorption and is the highest for the NP (0.3).  From the slope and the intercept of the straight line of logqe vs. logCe (Figure 9b), the values of Kf and n have been determined and are given in Table 4. The correlation coefficient (r 2 ) demonstrates that the Freundlich model is more suitable than the Langmuir model for the natural peat sample (NP). Therefore, it can be assumed that the process has a surface character [34]. This finding may imply that all groups (Table 4) are responsible for Cu 2+ adsorption behavior. The positive contribution of the carboxyl and phenolic groups and the aromatic compounds for adsorbing Cu 2+ has been previously reported [57].  From the slope and the intercept of the straight line of log q e vs. log C e (Figure 9b), the values of Kf and n have been determined and are given in Table 4. The correlation coefficient (r 2 ) demonstrates that the Freundlich model is more suitable than the Langmuir model for the natural peat sample (NP). Therefore, it can be assumed that the process has a surface character [34]. This finding may imply that all groups (Table 4) are responsible for Cu 2+ adsorption behavior. The positive contribution of the carboxyl and phenolic groups and the aromatic compounds for adsorbing Cu 2+ has been previously reported [57].

FTIR Spectroscopy Data before and after Experiments
FTIR spectra of two modifications of peat (MAP and MCAP) before and after sorption are shown in Figure 10a,b. A number of adsorption bands exhibited relative intensities, typical to peat-like materials, containing HA. For example, stretching vibrations of hydroxyl groups from 3420-3400 cm −1 and stretching vibrations of aliphatic CH 2 and CH 3 groups at the 2925 and 2855 cm −1 regions of HA were typical functional groups of the peat. FTIR spectroscopy data did not show HA structure conversion and the occurrence of solid-phase chemical reactions. After Cu 2+ adsorption, a peak shift from approximately 3374-3418 cm −1 in HA was observed, and the intensity of the peaks decreased (Figure 10b). The narrowing of the peaks from approximately 1374-1386 cm −1 in HA was observed, which may arise from the formation of hydrogen bonds after Cu 2+ adsorption. The peaks from approximately 1599-1633 cm −1 in HA shifted approximately to 7-24 cm −1 ; the peaks from approximately 1252-1268 cm −1 in HA almost disappeared after the adsorption of Cu 2+ . The above findings suggested that carboxyl and hydroxyl groups on humic substance (HS) surfaces were involved in Cu 2+ adsorption. The crucial role of carboxyl and hydroxyl groups in metal ion binding with HS has also been reported previously [75].
However, for the studied samples, no significant changes in the FTIR spectra before and after the sorption of copper ions were observed. A slight decrease in absorption in the 1430-1375 cm −1 area may indicate a decrease in C-H bonds in peat after the copper sorption. For MCAP, there is an increase in adsorption in the area of 1725 cm −1 , which is explained by the transition of a part of sodium humate to the form of HA due the presence of peat in an aqueous solution with pH 3.2-4.6.
which may arise from the formation of hydrogen bonds after Cu 2+ adsorption. The peaks from approximately 1599-1633 cm −1 in HA shifted approximately to 7-24 cm −1 ; the peaks from approximately 1252-1268 cm −1 in HA almost disappeared after the adsorption of Cu 2+ . The above findings suggested that carboxyl and hydroxyl groups on humic substance (HS) surfaces were involved in Cu 2+ adsorption. The crucial role of carboxyl and hydroxyl groups in metal ion binding with HS has also been reported previously [75]. However, for the studied samples, no significant changes in the FTIR spectra before and after the sorption of copper ions were observed. A slight decrease in absorption in the

Thermodynamic Modeling
Based on the above-mentioned data set, a mechanism of chemical adsorption with the formation of surface complexes was selected for thermodynamic modeling. Physicochemical modeling of the biosorption process makes it possible to choose such a working technological scheme, at which the minimum consumption of the adsorbent or modifier can be used and the most satisfactory results obtained. In the context of development, a model applied to environmental conditions (wetlands, tailing impoundments), we have to propose a model able to reproduce the copper sorption on native peat, in a pH range from 3-4, which is typical for the specified environments. Between pH 3.2 and 4.1 (Figure 6), despite a high dispersion of points depending on the initial Cu concentration, the totality of log K D values obtained by sorption were comprised between 2.0 and 4.0 mL/g, attesting to a high sorption capacity of native peat.
It has been shown in Table 4 that the total content of sorption positions in natural peat is 15 mmol/g. However, the number of Alk-COOH carboxyl groups easily eliminating the proton at pH 3.5 (dissociating) is only 2 mmol/g. It is most likely that adsorption occurs particularly with the formation of surface complexes by reactions [45,59]: Alk-COO − + Cu 2+ = Alk-COOCu + .
Thermodynamic data are presented in Table 6. Further details have been provided in our previous studies [76][77][78]. Some of the parameters were determined experimentally, others were adopted from [59,79]. It should be said that the weighed average log K diss (Equation (10)) [45,59] of carboxyl, phenolic, and other groups vary considerably for different samples of HA and FA, while the aqueous samples differ in more positive logarithm values: where γ( Cu 2+ ) is the activity coefficient of the Cu aqueous species calculated with the Davies equation. The activity coefficients of the adsorbed species are unknown, but their ratio is expected to be constant and fixed at 1.
A provident explanation can be made on the reaction dissociation constant (Equation (10)). At pH < 3.5, the presence of HA has a slight impact on copper adsorption, since in this region HA molecules are semi-protonated (Alk-COOH) and cannot bond the metal ion. Figure 11 shows the comparison of copper sorption on peat according to the experimental and calculated data depending on the initial content of Cu 2+ in the solution. In general, the accepted constants adequately describe the sorption process with an increase in its initial concentrations. Certainly, the sorption curve trend is smoother, and no such strong deflection has been detected in the region of 100 mg/L Cu 2+ . It is not necessary to optimize the process in the region of low concentrations (1 g of peat/100 mL of solution) due to the sufficient number of sorption positions (dissociated carboxyl groups). At 50, 100, and 150 mg/L of copper, a calculation was made at 2.5 g peat/50 mL solution. It turned out that the sorption of 96% can be attained even in the region of high concentrations. Thus, a nonlinear increase in the removal percent of Cu ions with an increase in the adsorbent concentration is observed.
Water 2022, 14, x FOR PEER REVIEW 16 of 20 Figure 11 shows the comparison of copper sorption on peat according to the experimental and calculated data depending on the initial content of Cu 2+ in the solution. In general, the accepted constants adequately describe the sorption process with an increase in its initial concentrations. Certainly, the sorption curve trend is smoother, and no such strong deflection has been detected in the region of 100 mg/L Cu 2+ . It is not necessary to optimize the process in the region of low concentrations (1 g of peat/100 mL of solution) due to the sufficient number of sorption positions (dissociated carboxyl groups). At 50, 100, and 150 mg/L of copper, a calculation was made at 2.5 g peat/50 mL solution. It turned out that the sorption of 96% can be attained even in the region of high concentrations. Thus, a nonlinear increase in the removal percent of Cu ions with an increase in the adsorbent concentration is observed.

Conclusions
Kinetic and equilibrium studies on copper ion adsorption on three peat modifications-natural peat (NP), mechanically activated (MAP), and mechanochemical activated (MCAP)-were carried out.
The activation of peat enhanced its physicochemical properties (CBET and specific surface area (Sspec)) but led to a decrease in the content of phenolic and carboxyl groups.
The studies showed that equilibrium of copper adsorption was established after 30 min. The thermodynamic modeling showed that under optimized conditions, the removal performance was found to be efficient enough, reaching 96%. A slight increase in the pH of the solution was observed following cooper adsorption. This could be interpreted by reverse hydrolysis reactions, which consume H + , thus, raising the pH.
Freundlich and Langmuir equations were followed and the corresponding constants were established. From these constants, empirical rate equations were derived for the prediction of the adsorption capacity of copper ions at a given time. Adsorption on NP and MCAP was successfully simulated with the Freundlich isotherm equation. The Langmuir model has been shown to fit well for mechanically activated peat. The adsorption capacity

Conclusions
Kinetic and equilibrium studies on copper ion adsorption on three peat modificationsnatural peat (NP), mechanically activated (MAP), and mechanochemical activated (MCAP)were carried out.
The activation of peat enhanced its physicochemical properties (C BET and specific surface area (S spec )) but led to a decrease in the content of phenolic and carboxyl groups.
The studies showed that equilibrium of copper adsorption was established after 30 min. The thermodynamic modeling showed that under optimized conditions, the removal performance was found to be efficient enough, reaching 96%. A slight increase in the pH of the solution was observed following cooper adsorption. This could be interpreted by reverse hydrolysis reactions, which consume H + , thus, raising the pH.
Freundlich and Langmuir equations were followed and the corresponding constants were established. From these constants, empirical rate equations were derived for the prediction of the adsorption capacity of copper ions at a given time. Adsorption on NP and MCAP was successfully simulated with the Freundlich isotherm equation. The Langmuir model has been shown to fit well for mechanically activated peat. The adsorption capacity increased in the order MCAP-NP-MAP and was found to be 16-24-42 mg/g.
The obtained experimental data provide a prediction of similar sorption capacity of peats in relation to copper ions, but the mechanical modification of peat could be efficiently used for the enhanced removal of cooper from wastewater.
By the example of peat mechanochemically oxidized with Na 2 CO 3 ·1.5H 2 O 2 , it is shown that the improvement of the physicochemical properties (C BET and specific surface area), plays a smaller role in the sorption capacity in relation to copper ions than the presence of phenolic and carboxyl groups, the content of which decreases during oxidation under the studied conditions.
Only one peat type (Sphagnum peat) was tested in the present study. Peat is an extremely heterogeneous material whose structure ranges from fibric to sapric while the relative composition (C, H, N, O) and features depend upon the botanical composition and degree of decomposition [54]; therefore, further studies are needed. In addition, further research will include the development of the present study to address the competition effects of metal co-ions on the biosorption process and extension of the mathematical modeling to polymetallic systems.