Environ Eng Res > Volume 25(5); 2020 > Article
Saad, Abd Ali, Naji, Faisal, and Al-Ansari: Development of Bi-Langmuir model on the sorption of cadmium onto waste foundry sand: Effects of initial pH and temperature

### Abstract

The present study develops the sorption model for simulating the effects of pH and temperature on the uptake of cadmium from contaminated water using waste foundry sand (WFS) by allowing the variation of the maximum adsorption capacity and affinity constant. The presence of two acidic functional groups with the same or different affinity is the basis in the derivation of the two models; Model 1 and Model 2 respectively. The developed Bi-Langmuir model with different affinity (Model 2) has a remarkable ability in the description of process under consideration with coefficient of determination > 0.9838 and sum of squared error < 0.08514. This result is proved by FTIR test where the weak acids responsible of cadmium ions removal using WFS sorbent can be represented by surface silanol (O-H) functional groups.

### 1. Introduction

Metallic elements with a relatively high density that greater than of the water’s density are defined the “heavy metals” [1]. Recently, an increasing ecological concern related with the environment contamination by heavy metals has been recognized. Due to the mobile nature of these metals, they can be reached to the different geological formations and cause a significant contamination for subsurface environment especially the groundwater where the front of the contamination may be propagated with the time to find its pathway for surface water resources [2]. Erosion, weathering or volcanic eruptions are considered the natural sources for pollution of groundwater with heavy metals as reported by previous studies such as [3, 4]. However, the human activities such as geogenic, industrial, agricultural, pharmaceutical, industrial production and use, domestic effluents and solids waste are represented the main processes that resulted the high concentrations of heavy metals [59]. In addition, the leachates resulted from agriculture sites or surface runoff can infiltrate to the groundwater and cause a potential pollution for subsurface media.
The previous studies reveal that the remediation of contaminated groundwater using conventional techniques such as “pump and treat” or “impermeable barriers” is required high cost. Accordingly, permeable reactive barrier (PRB) is an innovative technology that applied within the polluted site to retain the contaminants by the reactive material of the barrier for restricting the migration of dissolved plume [10, 11]. The migration of the metals within the PRB is governed by the “advection-dispersion-reaction equation” where the reaction (i.e. sorption) process plays a great role in the containment of the contaminant within the reactive medium of the barrier. The sorption process can be formulated by different models like Freundlich, Langmuir etc. where these models are very helpful in the simulation of the experimental data measured at certain values of pH and temperature. However, the common status in the subsurface environment that the pH and temperature are varied in response to the external factors and the reflection of this change in the isotherm model can be considered a unique task of this study. The developed model can be incorporated in the future with the advection-dispersion equation as sink term to describe the contaminant transport under the influences of pH and temperature of the flowing water.
Many studies have been achieved to fit the isotherm models to experimental datasets measured at different conditions. In this direction, Langmuir isotherm was used to represent a set of laboratory measurements collected at various values of pH where the regression related between the adsorption capacity and pH was developed [12, 13]. Adsorption of arsenic from aqueous solutions onto iron oxide can be represented by a modified Langmuir isotherm [14]. Also, the pH-dependent bio-sorption using marine macro-algae for removal of heavy metals with aid of the functional groups can be formulated by modified Langmuir model [15]. A set of empirical and semi-empirical expressions based on the Langmuir isotherm were developed to describe the removal of copper onto the calcium alginate and sphaerotilus natans sorbents under the effect of pH [16]. Further, column tests to monitor the reduction of Cr(VI) from contaminated water onto scrap iron were conducted with the values of pH varied from 2.00 to 7.30. The results signified that the maximum reduction capacity has value of 19.2 mg Cr(VI)/g iron at pH equal to 2.50, however, it is decreased due to increase of pH value [17]. Freundlich and Langmuir models were collected in one form named as the modified Langmuir–Freundlich isotherm and the influence of pH on the adsorption process in the batch tests can be describe by this isotherm. The values of affinity constants in this formula were correlated linearly with pH of aqueous solutions. The adsorption measurements resulted from interaction of goethite-coated sand and pure goethite with the arsenic contaminant was used for validation of developed formula [18]. In addition, the Langmuir model was developed for description the interaction of olive pips and aqueous solution contaminated with copper under the variation of initial pH. The influence of pH was represented by linear and nonlinear relationships for the maximum adsorption capacity and affinity constant respectively as a function of the initial pH. This isotherm was incorporated with solute transport equation to find the distribution of contaminant through the column tests under the effect of initial pH [19]. Finally, the Freundlich model was developed for predicting the adsorption capacity of quinolone by powdered activated carbon at different pH values. This model had excellent prediction capabilities under different laboratory scenarios [20].
The Bi-Langmuir isotherm was suggested for first time by Graham in (1953) [21] and the author assumed that the adsorption onto the surface composed by patches of two different homogeneous surfaces has independent behaviour. On each type of site, the same Langmuir principles of local adsorption are applied without adsorbate - adsorbate interactions. Accordingly, the present work is aimed to develop the Bi-Langmuir isotherm model for predicting the pH and temperature-adsorption effects which can be verified using experimental data of cadmium-waste foundry sand (WFS) interaction. This model opens new horizons for simulating the effects of pH and temperature on the values of retardation factor and, consequently, the longevity of the PRB using available codes of contaminant transport such as COMSOL Multiphysics 3.5a.

### 2.1. Preparation of Sorbent and Contaminant

WFS can be used as reactive material in the batch experiments and this material is resulted from steel foundry industry as byproduct. The particle size distribution of WFS ranged from 0.08 to 9 mm with median size of 320 μm, effective size of 180 μm, and uniformity coefficient of 1.94. The choice of WFS is mainly based on the presence of silica in its composition; therefore, the functional groups of silica (S iO H and (O H)) have able to remove of cadmium ions where the pH and temperature play a significant role in the exchange of proton from these groups. Aqueous solutions were contaminated with cadmium to simulate the pollution of the groundwater. Stock solution with concentration of 1,000 mg/L can be prepared using Cd(NO3)2·4H2O (manufactured by India) and this solution was used to obtain the required concentration by dilution.

### 2.2. Sorption Tests

Experimental batch tests were carried out under different values of initial pH of (3, 4, 4.5, 5, 6), temperature of (30, 40, and 50°C), and initial cadmium concentration (Co) of (10, 50, 100, and 200 mg/L). The 50 mL of cadmium solution was distributed onto the series of the flasks and certain quantity of the reactive material (2.5 g) was added for each flask. Subsequently, continuous agitation of these flasks was achieved for duration reached to 3 h using orbital shaker (Edmund Buhler SM25, German) with an agitation speed of 200 rpm. The aqueous solution was filtered at the end of each test and the measurement of its final pH can be achieved. Also, the remaining concentration of the cadmium ions (Ce) can be measured by atomic absorption spectrophotometer (AAS) (AA-7000 Shimadzu, Japan). Additional tests for interaction of uncontaminated aqueous solution with WFS were conducted under the same conditions of initial pH to investigate the variation of final pH in comparison with final pH of the contaminated solution. The quantity of cadmium sorbed on the reactive material, qe, is calculated by:
##### (1)
$qe=(Co-Ce)Vm$
where V is the volume of aqueous solution (L) and m is the WFS added to the flask (g). The measured sorption data have been fitted with Freundlich, Langmuir and Temkin models using non-linear regression method for calculating the parameters of the models by Excel 2016.

### 2.3. Sorption Isotherm Models

Measured equilibrium data were fitted by “two parameter isotherms” including Freundlich, Langmuir, and Temkin. A brief review of the adopted models is inserted below [22, 23]:
• Freundlich model (1906) is applicable for multilayer sorption and heterogeneous surfaces:

##### (2)
$qe=aFCe1n$
where aF is the constant related with the maximum adsorption capacity of the sorbent and 1/n(< 1) is the intensity of sorption.
• Langmuir model (1916) is applicable for uniform energies of sorption onto the sorbent surface:

##### (3)
$qe=qmaxbCe1+bCe$
where qmax is the maximum sorption capacity (mg/g) and b is the affinity of the metal ions towards reactive material.
• Temkin model is assumed that the adsorption is described by a uniform distribution of the binding energies up to maximum binding energy [24] as below:

##### (4)
$=BlnKT+BlnCe$
where KT is the equilibrium binding constant (L/mg) and B is the constant related to the heat of sorption (J/mol).

### 3.1. Equilibrium Study

Fig. 1 reveals that the removal percentage of the cadmium ions from contaminated water increases due to an increase in the initial pH values for same value of concentration and temperature until arrived to maximum value at initial pH of 4.5 and, thereafter, the removal was decreased. Protonation and deprotonation of the acidic and basic groups for WFS are mainly caused of this behavior, so, the interaction between metal ions and sorbent as a function of the initial pH can be influenced significantly [2527]. The small value of the removal percentage in comparison to the best removal efficiency can be attributed to inactivation of binding sites in the basic conditions [28]. The initial pH of the aqueous solution is tended to rise from acidic state (= 3) with progress of the operation process but it becomes almost constant at higher pH. This trend is resulted from the competition between the cations and protons on the surfaces of the active sites up to a particular point where the protons have been removed from the aqueous solution [29]. In contrast, with an initial alkaline solution (pH = 6), the trend progresses downward as the operation proceeds further until the pH becomes practically constant. This behavior may be correlated to the presence of substantial amount of the Cd(OH)+ ions that are retained by the solid, as well as to the precipitation of Cd(OH)2, that occurs at an alkaline pH, removing the hydroxyl groups from the aqueous solution, resulting in the drop of pH values [3032]. Fig. 1 signifies that the removal efficiency of cadmium was decreased with the increase of the initial concentration [33]. Also, it seems from this figure that the best values of the initial pH and temperature to achieve the maximum removal efficiency were 4.5 and 30°C, respectively.
The Freundlich, Langmuir and Temkin isotherm models, described previously, were employed for fitting the sorption measurements using nonlinear fitting of the regression and the constants of these models is inserted in Table 1. Statistical measures such as coefficient of determination (R2) and the sum of squared error (SSE) are determined for evaluating the concurrence between experimental data and isotherm models. It is clear that the Langmuir model has a good ability to describe the experimental data under different operational conditions adopted in the present investigation in comparison with Freundlich and Temkin models. This certified that the fitting of heterogeneous mode of sorption with the Freundlich model cannot be supported. In addition, this table signified that there is a dramatic change in the value of Temkin isotherm-binding constant (i.e. adsorption activity) as a function of initial pH value for the same temperature. Finally, the application of the Langmuir model on the measured data means that the homogeneous monolayer mode of sorption is predominant for situation under consideration with R2 not less than 0.972.

### 3.2. Development of Bi-Langmuir Model

To develop the Bi-Langmuir model that taken the effects of initial pH and temperature into account, a set of relationships simulated initial pH and temperature-dependent sorption effects are derived with the aid of experimental measurements for interactions of WFS and aqueous solution contaminated with cadmium as described below:

#### Affinity constant

The activation energy of metal sorption onto the sorbent can be calculated by the relationships [34, 35]:
##### (5)
$b(pH,T)=k.(pH)e(QRT)$
where k· is the affinity of the sorbate at reference temperature which can be changed with pH (L/mg) and Q is the heat of sorption (the difference between the activation energies necessary for desorption and sorption).
The calculated values of b for different values of initial pH and temperature mentioned in Table 1 can be used for fitting the Eq. (5) using nonlinear regression and finding the values of k· as function of initial pH. Then, the power relationships are more representative regressions to represent the variation of k· with initial pH based on the coefficient of determination as explained below:
##### (6)
$For initial pH<4.5; k.=e(0.281pH-1.7402),R2=0.9996$
##### (7)
$For initial pH>4.5; k.=e(-0.2427pH+0.5471),R2=0.8198$
This means that the general formula for describing the relationships related between of k· and initial pH can be written as follows:
##### (8)
$k.(pH)=eapH+b$
Eq. (8) can be substituted into the Eq. (5) to yield the following expression:
##### (9)
$b(pH,T)=e(QRT)+apH+b$

#### Maximum sorption capacity

This constant (qmax) is varied as a function to the initial pH and temperature by assuming that there are two functional weakly acid groups responsible of sorption process [15]. The qmax can be written using “subsequent additions method” and the present study derived two forms for qmax as below:
A) The two functional groups have the same affinity and, accordingly, qmax take the following form:
##### (10)
$qmax=Qa1+(Qa2*10pH-Pka1)1+10pH-Pka1+Qb1+(Qb2*10pH-Pka2)1+10pH-Pka2$
where Qa1, Qa2, Qb1 and Qb2 are the maximum adsorption capacities for protonated (AH and BH ) and deprotonated (A and B) forms of the two functional groups. The equilibrium of protonated and deprotonated forms of the functional groups can be described as follows:
##### (11)
$AH↔A-+H+ BH↔B-+H+$
##### (12)
$ka1=[A-][H+][AH] ka2=[B-][H+][BH]$
##### (13)
$Pka1=-log10(ka1) Pka2=-log10(ka2)$
where ka1 and ka2 are the apparent equilibrium constants.
The equilibrium constants are expressed as the difference between entropy change (ΔS°), as a function of temperature, and enthalpy change (ΔH°) for the described reaction [34, 36]. The relationship between ka and temperature was described using the van’t Hoff equation:
##### (14)
$ka=eΔS°R-ΔH°RT$
Combination of Eq. (14) and Eq. (13), the following equation can be written:
##### (15)
$Pka1=(ΔS1°ln (10)R-ΔH1°ln (10)RT) and Pka2=(ΔS2°ln (10)R-ΔH2°ln (10)RT)$
Combination of Eq. (10) with Eq. (15) will produce the following equation:
##### (16)
$qmax(pH,T)=Qa1+(Qa2*10pH+ΔS1°ln (10)R-ΔH1°ln (10)RT)1+10pH+ΔS°ln (10)R-ΔH°ln (10)RT+Qb1+(Qb2*10pH+ΔS2°ln (10)R-ΔH2°ln (10)RT)1+10pH+ΔS2°ln (10)R-ΔH2°ln (10)RT$
where ΔH1° and ΔH2° are the enthalpy change, while ΔS1° and ΔS2° are the entropy change of the first and second reactions, respectively.
Hence, the first form (Model 1) of Bi-Langmuir model for two weakly acid functional groups with same affinity can be written as follows:
##### (17)
$Model 1:qe=Qa1+(Qa2*10pH+β1+β2T)1+10pH+β1+β2T+Qb1+(Qb2*10pH+γ1+γ2T)1+10pH+γ1+γ2Te(α1T)+apH+bCe1+e(α1T)+apH+bCe$
where $β1=ΔS1°ln(10)R,β2=-ΔH1°ln(10)R,γ1=ΔS2°ln(10)R,γ2=ΔH2°ln(10)R,α1=QR$
B) The two functional groups have the different affinity and, accordingly, qmax take the following form:
##### (18)
$q1e=q1maxb1Ce1+b1Ce$
##### (19)
$q2e=q2maxb2Ce1+b2Ce$
where q1max and q2max are the maximum sorption capacities (mg/g) for first and second functional groups, respectively. Similarly, the affinity of the first and second functional groups towards sorbent is denoted as b1 and b2, respectively. The sum of q1e and q2e is equal to qe as follows:
##### (20)
$qe=q1e+q2e$
##### (21)
$qe=q1maxb1Ce1+b1C2+q2maxb2Ce1+b2Ce$
##### (22)
$qe=Qa1+(Qa2*10pH-Pka1)1+10pH-Pka1b1Ce1+b1Ce+Qb1+(Qb2*10pH-Pka2)1+10pH-Pka2b2Ce1+b2Ce$
Assuming qmax(b)is a function to the affinity of the sorbate (b), then:
##### (23)
$qmax(b)=Q1\+(Q2\*b)1+b$
where $Q1\$ and $Q2\$, are constant. Consequently, Eq. (23) can be written as follows and this is the second form (Model 2) of Bi-Langmuir model for two weakly acid functional groups with different affinity:
##### (24)
$Model 2:qe=Qa1\+(Qa2\*b1)1+b1b1Ce1+b1Ce+Qb1\+(Qb2\*b2)1+b2b2Ce1+b2Ce$
where b1 and b2 are the affinities of the first and second functional groups, respectively.
##### (25)
$b1(pH,T)=e(α1T)+a1pH+b1,b2(pH,T)=e(α2T)+a2pH+b2$
where β1, β2, γ1, γ2, α1, α2, a1, a2, b1 and b2 are constants.
The experimental data (qe as a function of Ce) are obtained at different values of pH and temperature. These data were fitted by a non-linear regression method [37] to evaluate the adjustable constants (β1, β2, γ1, γ2, α1, α2, a1, a2, b1 and b2), by minimizing the sum of the squared deviations between experimental and predicted values. Fig. 2 is explained the scatter diagram obtained by plotting values of qe predicted by the Bi-Langmuir model (Models 1 and 2) in comparison with experimental data where the 45 degree line is usually drawn to facilitate interpretation of the scatter plot. Table 2 presents the fitted constants of the developed models together with the statistical measures. This table in combination with Fig. 2 certified that the Model 2 is more representative in the description of measured sorption data and can be incorporated in the future with solute transport equation to describe the migration of contaminant in continuous mode.

### 3.3. Fourier Transform Infrared (FTIR) Analysis

This analysis is considered an important test that can be used to identify the effective functional groups [38] responsible of the binding between the cadmium ions and sites on the WFS in the sorption process. Shimadzu FTIR (8000 series spectrophotometers) with the infrared spectra ranged from 400 to 4000 cm−1 was used to address the change in the transmittance for WFS sample after sorption of cadmium ions as plotted in Fig. 3 for initial pH equal to 4 and 5. The shifts in the infrared frequencies of bonds (O-H band, H-O-H, O-Si-O, and Si-O band) are the main groups for enhancement the binding of cadmium onto WFS with the wavenumbers values at 3,619, 1,668, 662, and 522 cm−1, respectively [39, 40]. These numbers signified that the surface silanol groups (O-H band) are weak acids [41]. The change in the hydroxide group is due to formation of cadmium hydroxide (pH > 4.5) and the change in Si-O due to adsorption cadmium as following:
##### (26)
$For initial pH<4.5; Si-OH+Cd+2→Si-OCd+H+$
##### (27)
$SiO(OH)+Cd+2→SiO(OCd)+H+$
##### (28)
$For initial pH<4.5; Si-OH+Cd(OH)+→Si-OCd(OH)+H+$
##### (29)
$SiO(OH)+Cd(OH)+→O-SiO(OCd(OH))+H+$
The sorption mechanism causes an increase in the absolute difference between values of final pH for contaminated and uncontaminated (control) aqueous solutions due to interaction with WFS as shown in Fig. 4. Hence, the results of this test are consistent with the assumptions of the developed models described in the earlier section. In addition, Table 3 explains the variation of final pH for contaminated and control aqueous solutions as a function of the initial pH. It is clear that the final pH of control (uncontaminated) solution is greater than that of contaminated solution because of the dissolution of CaO; however, the low values of the final pH for contaminated solution may be due to release of H+ ions according to Eq. (26)(29).

### 4. Conclusions

An isotherm expression was developed for simulating initial pH and temperature-dependent sorption effects. Langmuir model was the base expression used for achieving the development process, thereby allowing the variation of the maximum adsorption capacity and affinity constant in response to changes in the initial pH and temperature values. The two forms of developed Langmuir model were derived depending on the number of acidic functional groups and the affinity of metal ions regarding the reactive material. Further, the validity of these models was tested based on the experimental results of cadmium sorption onto WFS for different values of initial pH and temperature. The results proved that the Model 2 for two weakly acidic functional groups with different affinity has a great ability in the description of sorption data as a function of initial pH and temperature with the coefficient of determination (R2) not less than 0.9838 and SSE not greater than 0.08514. This result was satisfied with output of FTIR test which reveals the sorption process can be achieved due to the presence of more than one acidic functional group.

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##### Fig. 1
Removal efficiency of cadmium by WFS as a function of initial concentration, initial pH and temperature (pH = 3–6; Co = 10–200 mg/L; WFS dosage = 2.5 g/50 mL; agitation speed = 250 rpm; T = 30–50°C). (a) T = 50°C, (b) T = 40°C, (c) T = 30°C.
##### Fig. 2
Scatter diagram (qe exp. vs. qe pred.) for cadmium sorption at different values of pH and temperature using developed models 1 and 2. (a) Model 1, (b) Model 2.
##### Fig. 3
FTIR test for WFS before and after sorption of cadmium for two values of initial pH.
##### Fig. 4
The absolute difference between values of final pH for contaminated and uncontaminated (control) aqueous solutions due to interaction with WFS.
##### Table 1
Constants of Freundlich, Langmuir, and Temkin Isotherm Models Using Non-linear Fitting for Sorption of Cadmium onto WFS
pH Freundlich isotherm Langmuir isotherm Temkin isotherm

Parameter Temperature (°C) Parameter Temperature (°C) Parameter Temperature (°C)

50 40 30 50 40 30 50 40 30
3 aF 0.4508 0.3869 0.2793 qmax 1.4397 1.0722 0.9377 B 0.2381 0.1737 0.1678
n 4.0205 4.6981 4.0911 b 0.2095 0.2468 0.1403 KT 3.9548 4.4316 1.9608
R2 0.8886 0.7731 0.799 R2 0.9996 0.9882 0.9875 R2 0.9766 0.8853 0.9083
SSE* 0.1041 0.1088 0.0684 SSE* 0.0004 0.0068 0.0051 SSE 0.0208 0.0534 0.0302

4 aF 0.4969 0.446 0.3228 qmax 1.5153 1.0433 0.9756 B 0.2478 0.1529 0.1666
n 4.1078 5.721 4.4081 b 0.2627 0.3486 0.1866 KT 4.7881 8.7343 2.8806
R2 0.8873 0.6089 0.7799 R2 0.9967 0.9253 0.9855 R2 0.9747 0.7267 0.8897
SEE 0.1203 0.1852 0.0832 SSE 0.0035 0.0383 0.0068 SSE 0.0258 0.1269 0.0405

4.5 aF 0.5606 0.4228 0.3736 qmax 1.5962 1.1756 1.0048 B 0.2553 0.1896 0.1613
n 4.2835 4.5255 4.8716 b 0.3577 0.2959 0.2575 KT 6.3386 5.217 4.6303
R2 0.875 0.8339 0.7323 R2 0.9926 0.9686 0.9728 R2 0.9638 0.9181 0.8428
SSE 0.1529 0.0935 0.1099 SSE 0.0098 0.0185 0.0135 SSE 0.0426 0.0451 0.0631

5 aF 0.4919 0.417 0.3158 qmax 1.5498 1.1588 0.9788 B 0.2639 0.1877 0.171
n 4.0136 4.6403 4.3505 b 0.247 0.2664 0.1697 KT 3.7325 4.653 2.4264
R2 0.8651 0.7858 0.7533 R2 0.9924 0.9894 0.9731 R2 0.9585 0.8944 0.8663
SSE 0.1487 0.1223 0.0935 SSE 0.01 0.0079 0.0124 SSE 0.044 0.0586 0.0493

6 aF 0.4513 0.3485 0.2342 qmax 1.4699 0.9674 0.8744 B 0.2578 0.1564 0.1628
n 3.9486 4.6561 3.8133 b 0.2232 0.2685 0.1106 KT 2.987 4.5644 1.4152
R2 0.8451 0.7607 0.8227 R2 0.9794 0.9422 0.9903 R2 0.9379 0.8505 0.9273
SSE 0.1493 0.0923 0.0505 SSE 0.0234 0.0243 0.0034 SSE 0.0581 0.0567 0.02

* sum of squared error (SSE = ∑(qexperiment – qpredicted)2)

##### Table 2
Constants of the Models Developed in the Present Study for Cadmium Sorption onto Waste Foundry Sand Using Non-linear Regression Analysis
Initial pH ≤ 4.5 > 4.5
Model 1 Qa1 0.33678 0.30854
Qa2 1.46724 0.85749
β1 4.84694 0.37261
β2 −496.566 0.00121
Qb1 0.53699 0.00165
Qb2 0.97140 37.81123
γ1 6.78845 2.17693
γ2 −446.43681 44.29724
α1 −2.10759 −44.3262
a 0.28100 −0.2427
b −1.74020 0.5471
R2 0.9768 0.9668
SSE 0.27969 0.14819

Model 2 $Qa1\$ 17.6611 0.07986
$Qa2\$ 0.09999 0.11920
$Qb1\$ 0.00199 0.00192
$Qb2\$ 2.95984 2.79537
α1 −0.00411 −0.00290
a1 7.80 × 10−6 −3.10 × 10−3
b1 4.999× 10−5 −0.38191
α2 0.30885 0.48269
a2 0.74212 0.88575
b2 −0.13349 −0.26469
R2 0.9868 0.9838
SSE 0.08514 0.06639
##### Table 3
Variation of Final pH for Contaminated and Uncontaminated (control) Aqueous Solutions Due to Interaction with WFS as Function to Initial pH
Initial pH Final pH
Uncontaminated solution Contaminated solution
3 7.15 5.44
4 8.24 5.85
5 9.32 5.82
6 9.4 5.83
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