# Testing the Performance of Various Polymeric Antiscalants for Mitigation of Sb-Rich Precipitates Mimicking Stibnite-Based Geothermal Deposits

Authors: Celal Çiftçi; Emre Karaburun; Serhat Tonkul; Alper Baba; Mustafa M. Demir; Mehmet İrfan Yeşilnacar
Journal: Geofluids
 (2020)

---

## Abstract

Scaling is frequently observed in geothermal fields and reduces the energy harvesting of power plants. Recently, Sb-rich deposits have developed in many fields around the world. Various polymeric macromolecules have been used as antiscalants to mitigate the formation of scale. Testing potential commercial antiscalants in field conditions is a tedious and costly process. The artificial synthesis of geothermal deposits in the lab is a more practical and economical way to test the performance of antiscalants. This study obtained a Sb-rich deposit by refluxing SbCl3 and Na2S·3H2O in 18 h. The product was found to be a mixture of Sb2O3 and Sb2S3. We examined the performance of antiscalants such as poly(ethylene glycol), poly(vinyl pyrrolidone), Gelatin, and poly(vinyl alcohol) of various molecular weights at 5 to 100 ppm. The formation of Sb2S3 is suppressed in the presence of the polymeric antiscalants. The dosage was found to be critical for the solubilization of Sb-rich deposits. Gelatin of 5 ppm showed the highest performance under the conditions employed in this study. While low dosages improve the concentration of [Sb3+], high dosages are required to increase the solubility of [S2-]. Moreover, the amount of deposit is reduced by 12.4% compared to the reference (in the absence of any polymeric molecules). Thus, comparatively, Gelatin shows the most promising performance among the molecules employed.


---

## Body

## 1. Introduction

Scaling is one of the main handicaps for geothermal power plants, as it remarkably reduces energy harvesting. Polymeric antiscalants have been employed to mitigate deposits [1]. Antiscalants prevent the formation of the deposit, reducing power plants’ performance and minimizing the occurrence of potential corrosion [2].The solubility of most species in aqueous solution strongly depends on the thermodynamic properties of the geothermal system. If disperse ions or inactive species are present near their saturation concentration, a slight perturbation in temperature or pressure can result in precipitation for a portion of these ions or species, which often combine and precipitate as a scale on a solid surface with which they come in contact. The equipment and piping in which the solution is confined may be restricted or plugged as a result of scale deposition [3]. Carbonates and silicates are the main scaling chemistry, which is a big problem for both energy harvesting and drinking water supply since the chemistry of scale acts as an insulator [4–10]. In addition, sulfide and sulfur scaling also create similar problems, especially in binary cycle geothermal power plants [10–13]. It is not only a problem of geothermal power plants but also one of the main obstacles frequently encountered in oil fields [14]. Sulfur scaling in geothermal systems can occur in medium, low, and high enthalpy fluids. Criaud and Fouillac (1989) stated that corrosion in low enthalpy areas containing dissolved matter is at high concentrations. Corrosive geothermal fluid corrodes casing wells and exposes metals such as Fe, Pb, and Zn for aqueous systems [15]. These metals precipitate in metal sulfide form. They are often accompanied by silica precipitation on high-temperature sites. The formation of sulfide deposits has been reported by various plants on the west coast of Turkey [16]. Recently, more emphasis is being placed on antimony (Sb)-rich deposits. While carbonates and silicates have been studied for a long time, little is known about stibnite (Sb2S3) deposits. Antimony forms stable interaction with sulfur. Antimony is found in sulfide deposits such as stibnite, sulfosalts, and, in some cases, natural Sb [17]. In natural geothermal systems, antimony usually occurs in two oxidation states: trisulfide, Sb3+ and pentasulfide, Sb5+ [18, 19]. Sb-rich scaling has been observed in various plants worldwide, including in Turkey, Italy, New Zealand, and El Salvador [20, 21]. Stibnite (Sb2S3), known as antimony trisulfide, is a sulfur mineral and is the main component of hydrothermal systems. In recent years, with the prevalence of binary cycle power plants in Turkey, stibnite scaling has also increased [22]. In hydrothermal systems, stibnite precipitation is controlled by pH and temperature and thus is commonly observed in condensers and heat exchangers where the temperature and pH may also play an essential role in the thermodynamics of deposition of sulfur-based scales. Although the concentration of antimony in the brine is low, antimony sulfide scaling is a major problem at low temperature and pH in binary cycle power plants. Typical antimony concentrations are less than one ppm in brine [23]. However, studies have shown that antimony can still be stored as stibnite in natural geothermal systems.In geothermal systems, stibnite dissolves in water in the form of hydroxide. As the storage of stibnite increases, the concentration of hydrogen sulfide increases. This situation can be expressed simply by the following equation:(1)Sb2S3+6H2O⟶2SbOH3+3H2SMoreover, stibnite scaling may cause corrosion in natural geothermal systems [12]. Mitigation of the deposit is vital for geothermal power plants.This work tested various polymeric antiscalants, namely poly(vinyl alcohol) (PVA), polyethylene glycol (PEG), poly(vinyl pyrrolidone) (PVP), and Gelatin, to reduce deposits in geothermal power plants. All these molecules were chosen because they contain functional groups that may interact with the deposit’s precursor ions. PVA has hydroxyl groups that can act in functional groups interacting with the main cations [24, 25]. PEG has oxygen with two lone pairs of electrons on its backbone [9]. PVP contains a cyclic pendant group consisting of amide as an electron-rich species to interact with ions. Gelatin, a biopolymer, possesses both amine and hydroxyl groups in its structure. According to our best knowledge, there is limited literature on the minimization of Sb-rich precipitates mimicking geothermal deposits [26, 27]. The results of this study showed that Gelatin displayed the most remarkable performance among the antiscalants employed. The product of the reflux was used as an artificial deposit/precipitate in this study. The scale obtained in the real geothermal plant is called a deposit. Both words are used interchangeably in the text.


## 2. Experimental

### 2.1. Materials

For the synthesis of artificial deposits, a Radleys Carousel 6 Plus Reaction Station (Saffron Walden, UK) was used as the reflux system (Scheme1). All chemicals were supplied by Sigma-Aldrich (St. Louis, MO, USA) and were used as received without any further purification. Antimony (III) chloride (SbCl3) and sodium sulfide trihydrate (Na2S·3H2O) were purchased from Sigma-Aldrich (New York, USA). The various molecular weights of polymeric antiscalants were supplied by Sigma-Aldrich: Polyvinyl alcohol (PVA) (Mw: 31-70, and 146-186 kg/mol), Poly(vinyl pyrrolidone) (PVP) (Mw: 8, and 40 kg/mol), and Poly (ethylene glycol) (PEG) (0.2 kg/mol). The chemical structure of the polymeric antiscalants is given in Scheme 2. A Milli-Q Advantage water treatment system produced the deionized water (18.2 MΩ cm−1 at 25°C) used in all experiments.Scheme 1
Experimental setup for the synthesis of Sb-rich deposit.Scheme 2
Chemical structure of the polymeric antiscalants employed in this study for the mitigation of the antimony-rich deposit.
(a)
PEG(b)
PVP(c)
PVA(d)
Gelatin


### 2.2. Methods

The method consists of two stages: the synthesis of artificial deposit and antiscaling performance of the polymeric antiscalants. In the first stage, artificial deposits were synthesized from synthetic brine, which was prepared by mixing an equivolume solution (50 mL) of antimony (III) chloride (SbCl3) and Na2S·3H2O. Synthetic brine was prepared by dissolving Na2S·3H2O (0.43 g 3.2 mmol) and SbCl3 (0.5 g, 2.2 mmol) in 100 mL distilled water. The entire synthetic brine was placed in the reflux system at 100°C for 18 h. Afterward, nitrogen gas was passed through for 10 min and mixed at 400 rpm. During the 18 h period, the solution changed from light orange to dark gray. Subsequently, the reaction mixture was left to cool in the ice bath. After 30 min, the reaction mixture consisted of solid particles in aqueous solutions, which were isolated via centrifugation, and then the leftover decantation solution was collected. In the second stage, the antiscaling performance of the polymers was examined. The chemical structure of the polymers is given in Scheme 2. Polymer solutions (10 mL) were added to the mixture in various dosages (5, 25, 50, and 100 ppm) to the artificial brine solution (90 mL). Then, the resulting solution was bubbled through with N2 for 10 min and placed in the reflux system at 100°C for 18 h. The decantate was analyzed by inductively coupled plasma mass spectroscopy (ICP−MS). Centrifugation was performed to separate the deposit from the decantate. The precipitate was dried at 80°C for 12 h after being centrifuged. Powder X-ray diffraction (XRD) measurements were performed on a PANalytical Powder Diffractometer with a copper Kα (λ=1.5416Å) tube. The 2θ was scanned from 10 to 80° at a scan rate of 0.08° s−1. The morphology of the precipitates was determined by using a scanning electron microscope (SEM; 300VP, Carl Zeiss, Oberkochen, Germany).


## 2.1. Materials

For the synthesis of artificial deposits, a Radleys Carousel 6 Plus Reaction Station (Saffron Walden, UK) was used as the reflux system (Scheme1). All chemicals were supplied by Sigma-Aldrich (St. Louis, MO, USA) and were used as received without any further purification. Antimony (III) chloride (SbCl3) and sodium sulfide trihydrate (Na2S·3H2O) were purchased from Sigma-Aldrich (New York, USA). The various molecular weights of polymeric antiscalants were supplied by Sigma-Aldrich: Polyvinyl alcohol (PVA) (Mw: 31-70, and 146-186 kg/mol), Poly(vinyl pyrrolidone) (PVP) (Mw: 8, and 40 kg/mol), and Poly (ethylene glycol) (PEG) (0.2 kg/mol). The chemical structure of the polymeric antiscalants is given in Scheme 2. A Milli-Q Advantage water treatment system produced the deionized water (18.2 MΩ cm−1 at 25°C) used in all experiments.Scheme 1
Experimental setup for the synthesis of Sb-rich deposit.Scheme 2
Chemical structure of the polymeric antiscalants employed in this study for the mitigation of the antimony-rich deposit.
(a)
PEG(b)
PVP(c)
PVA(d)
Gelatin


## 2.2. Methods

The method consists of two stages: the synthesis of artificial deposit and antiscaling performance of the polymeric antiscalants. In the first stage, artificial deposits were synthesized from synthetic brine, which was prepared by mixing an equivolume solution (50 mL) of antimony (III) chloride (SbCl3) and Na2S·3H2O. Synthetic brine was prepared by dissolving Na2S·3H2O (0.43 g 3.2 mmol) and SbCl3 (0.5 g, 2.2 mmol) in 100 mL distilled water. The entire synthetic brine was placed in the reflux system at 100°C for 18 h. Afterward, nitrogen gas was passed through for 10 min and mixed at 400 rpm. During the 18 h period, the solution changed from light orange to dark gray. Subsequently, the reaction mixture was left to cool in the ice bath. After 30 min, the reaction mixture consisted of solid particles in aqueous solutions, which were isolated via centrifugation, and then the leftover decantation solution was collected. In the second stage, the antiscaling performance of the polymers was examined. The chemical structure of the polymers is given in Scheme 2. Polymer solutions (10 mL) were added to the mixture in various dosages (5, 25, 50, and 100 ppm) to the artificial brine solution (90 mL). Then, the resulting solution was bubbled through with N2 for 10 min and placed in the reflux system at 100°C for 18 h. The decantate was analyzed by inductively coupled plasma mass spectroscopy (ICP−MS). Centrifugation was performed to separate the deposit from the decantate. The precipitate was dried at 80°C for 12 h after being centrifuged. Powder X-ray diffraction (XRD) measurements were performed on a PANalytical Powder Diffractometer with a copper Kα (λ=1.5416Å) tube. The 2θ was scanned from 10 to 80° at a scan rate of 0.08° s−1. The morphology of the precipitates was determined by using a scanning electron microscope (SEM; 300VP, Carl Zeiss, Oberkochen, Germany).


## 3. Results and Discussion

### 3.1. Structural Characterization of the Sb-Rich Precipitates

For the fabrication of artificial Sb-rich deposits, namely precipitate, it is wise to use water-soluble salts of Sb and S. Refluxing is carried out through the aqueous reaction of SbCl3 and Na2S·3H2O under ambient conditions. Figure 1 presents the X-ray diffraction patterns of the Sb-rich precipitate obtained at various reaction times. In the beginning, the deposit does not show evident reflections and most probably contains crystalline regions in a large amorphous matrix. As the reaction time is extended to 14 h, an oxide phase that is indexed to valentinite (00-011-0691) forms. The resulting powder is orange. The valentinite is colorless in nature. This orange color may originate from a minute amount of amorphous stibnite, the reflections of which are present in the diffractogram with very weak intensity. Increasing the reaction time to 16 h, the reflections of Sb2S3 appear, indicating the formation of the grey-colored sulfide phase (stibnite: 00-001-0538) along with the presence of the oxide phase. At 18 h, the products show a similar stable combination of oxide and sulfide. Thus, the reaction time is fixed to 18 h for the testing of the performance of the antiscalants. Reaction times longer than 18 h cause the formation of crystals other than oxides and sulfides such as Sb2OS2 and Sb4O5Cl2 (not shown in this text).Figure 1
XRD patterns of the precipitates prepared at various reaction times.Since the product was a mixture of Sb2O3 and Sb2S3, we characterized the mixture with Rietveld refinement analysis of the XRD patterns with X’Pert HighScore Plus. The results are presented in Table 1. The reference deposit (prepared in the absence of antiscalants) has the following combination (Sb2S3 : Sb2O3, 86 : 14 in terms of the mole). However, the composition of the product mixture changed in the presence of polymeric antiscalants. The sulfides disappeared, while oxides became a dominant component in the product mixture.Table 1
The composition of deposit based on Rietveld method. The reference deposit has the following combination (Sb2S3 : Sb2O3) (86 : 14 in terms of mole). The data are obtained from Rietveld method run by using X’Pert HighScore Plus software program.
2550100PVA 310 : 1000 : 1000 : 100PVA 14.670 : 300 : 1000 : 100PEG—77 : 2377 : 23Gelatin52 : 480 : 10075 : 25PVP 5868 : 3267 : 330 : 100PVP 80 : 1000 : 1000 : 100Figure2 shows an X-ray diffraction patterns of the precipitates prepared in the presence of Gelatin at various dosages. In all diffractograms, the precipitates are the mixture of Sb2S3 and Sb2O3 with varying compositions. However, Gelatin does not influence the crystal structure.Figure 2
XRD patterns of the precipitates prepared in the presence of Gelatin at 25, 50, and 100 ppm.The existence of polymeric antiscalants has a clear influence on the morphology of precipitates. Scanning electron microscopy (SEM) images of the precipitates display the morphology of the deposits (Figure3). The morphology of the precipitates is heterogeneous in nature. There are needles, aggregates of microspheres, dumbbell-shaped crystals, and plates. While the needles, aggregates of microspheres (average diameter: 1.0±0.8μm), and dumbbell shape morphologies seem crystal and most probably Sb2S3, the plates may refer to Sb2O3. The morphology of the stibnite-based geothermal deposits has previously been shown [28]. The size and shapes of the precipitates were consistent with the literature [29]. For instance, the needles had 4.8±3.7μm length and 1.0±0.8μm width. Plate and dumbbell-shaped morphologies were also observed for some particular crystals. Figure 4(a) shows the crystals prepared in the presence of 50 ppm Gelatin. The needles are split into more substantial and more complex geometrical structures by the assembly of the process of needles. The dumbbell-shaped crystals probably formed from the merging and splinting of the long needles [30]. Figure 4(b) displays the morphology of the precipitates in the presence of 50 ppm PVP. Aggregates of spheres (sulfide phase) and a plate of the needles (oxide phase) coexist.Figure 3
SEM image of the reference prepared by refluxing of SbCl3 and Na2S·3H2O in 18 h. The magnification is 5000x.Figure 4
SEM image of the representative samples prepared in the presence of 50 ppm (a) Gelatin and (b) PVP. The magnification is 25000x.
(a)(b)It is crucial to dispose of geothermal fluid by reinjection, either into shallow or deep geothermal wells. The temperature changes may bring about the oversaturation of some minerals such as stibnite, thus creating a tendency to precipitate. It is important to assess the state of mineral saturation in the waste geothermal fluid that will be disposed of by reinjection to find the optimum temperature for reinjection. Figure5 indicates the activity product for the stibnite and stibnite solubility curve. For example, stibnite is equal to zero at around 100°C. The degree of supersaturated decreases as the temperature increases, particularly above 100°C in geothermal fluid in western Turkey.Figure 5
Changes in the state of stibnite in geothermal fluid.The seeping of the polymeric antiscalants into the deposit structure, if it takes place, is a significant question. It becomes an even more critical question since the amount of deposit is used for the determination of antiscalant performance. At low dosages, the amount of deposit after subtracting the polymeric antiscalant portion is almost unchanged. We could not detect the amount of polymeric antiscalant in the precipitated deposit by thermogravimetry; however, we observed the presence of the antiscalant molecule by vibrational spectroscopy. Figure6 displays the vibration spectra of the deposits presented in the absence and presence of the polymeric antiscalants. While the reference does not show vibrational signals in the infrared region, the precipitates prepared in the presence of PVA and Gelatin show characteristic signals of specific bonds that belong to the polymer of interest. For instance, the one prepared in the presence of Gelatin showed characteristic bending at 1649 cm-1 of N-H bond. Another characteristic signal of Gelatin could be seen at 1144 cm-1 of C-N stretching. Thus, the combination of both thermogravimetry and spectroscopy results suggest that a small amount of polymeric antiscalant remains in the deposit.Figure 6
Fourier transform infrared spectra of the reference, the precipitate prepared in the presence of 100 ppm PVA and Gelatin.


### 3.2. Performance of the Antiscalants

Using antiscalant in the model reaction, there are two success criteria: (i) the decrease of the amount of precipitate; (ii) the concentration of the ions in the decantate such as Sb3+ and S2- after the isolation of precipitate. Table 2 presents the concentrations of Na+, Sb3+, and S2- left in the decantate solution in terms of ppm. Independent of the chemistry of the antiscalants, the concentration of the Sb3+ increases in the presence of antiscalants. An electrostatic interaction may take place between Sb cations and electron-rich groups on the backbone of polymeric antiscalants such as hydroxyl for PVA, oxygen of PEG, the nitrogen of pyrrolidone and hydroxyl and amine groups of Gelatin. Thus, both Na+ and Sb3+ are held in the solution and do not contribute to the formation of solid precipitated by the aforementioned groups. However, the antiscalants were not as effective as in the dissolution of the sulfur ions. Most probably, they do not have positively charged (or at least partially positively charged) functional groups on their backbone; therefore, negatively charged sulfur anions are not able to find available sites on polymeric molecules to interact with. Reduction of the amount of precipitate is another criterion for the performance of antiscalants; in fact, it is the main motivation for using antiscalants in the geothermal fields. In the model reaction, the amount of precipitate is also studied. The reference sample provides 290 mg of the precipitate. The ones prepared in the presence of the antiscalants are lower than this value, except PVA 31-70 kg/mol by which the amount of precipitate is above the reference point most, probably due to the existence of polymeric molecules in the precipitate. The maximum reduction of the solid deposit that refers to scaling in real fields is obtained by the application of Gelatin (nearly %12.4). Considering that a certain amount of polymeric antiscalant is kept inside the precipitate as the vibrational spectroscopy suggests, the reduction of the amount of deposit may be even higher in terms of percentage.Table 2
Concentration of several of ions (mg·L-1) in the decantate solution after isolation of solid content so-called deposit. Dosage of the antiscalants is 5 ppm. The reference points out the reaction carried out in absence of antiscalants.
Antiscalants[Na+][S=][Sbn+]The amount of depositThe amount of deposit after subtraction of the polymer/mgThe amount of deposit after subtraction of the polymerReference98056222902900PVA 31116020643133130PVA 14.6119021512832830Gelatin117015622542540PVP117018792602600The dosage of the antiscalant was also examined, taking Gelatin as a representative example. Dosages higher than 5 ppm were studied: 25, 50, and 100 ppm. The concentration of the ions and the amount of deposit after the reaction are given in Table3. The application of 5 mg of Gelatin increases the concentration of Sb from 22 to 62 ppm. As the dosage of antiscalant increases, the concentration of Sb remains almost unchanged compared to the reference sample. It seems that Gelatin only works for low dosage. In contrast, the concentration of sulfur increases as the dosage increases. At 5 ppm, 5 ppm sulfur concentration is lower than that of the reference and gradually increases as the dosage increases to 96 ppm. Thus, the polymeric antiscalant was found to play the opposite effect on the concentration of the Sb3+ and S2- ions. While the Sb ion was suspended in the decantate solution at low dosages, [S2-] was found to be higher compared to that of the reference. A similar trend is seen in other antiscalants (Figure 7).Table 3
The effect of Gelatin at various dosages. The concentration of the ions is given in terms of ppm. The amount of polymeric antiscalant remains in the deposit is determined by gravimetry.
Dosage/ppm[Na+][S=][Sbn+]The amount of deposit/mgThe amount of deposit after subtracting of the polymer/mgThe amount of polymer remaining in the deposit/mgReference9805622290511701662254254025166060102372352501260891428327851001370961234733710Figure 7
The concentration of Sb3+ and S2- in the presence of the antiscalants at all dosages. The dashed line represents the concentration of the ion of interest for reference (without antiscalants).At low dosages, the amount of deposit decreased from 290 mg to 254 mg. The lowest was recorded when 25 ppm was applied (18%). At the highest dosage of 100 ppm antiscalant, the amount of deposit was even higher (337 mg). The remarkable increase in the amount of precipitate at high dosages may have originated from flocculation (Scheme3).Scheme 3
Schematic representation of flocculation.Briefly, flocculation is a process that promotes agglomeration of the particles by the help of a high dosage of the long polymeric chain. As a result, sedimentation of the particles takes place. Meanwhile, the settling of the particles is assisted by the presence of flocculants, which are organic molecules. A long polymer chain interacts with more than one particle such that agglomeration occurs and the agglomerated structure has a larger massive structure. At high dosages, flocculation may be the main mechanism taking place.


## 3.1. Structural Characterization of the Sb-Rich Precipitates

For the fabrication of artificial Sb-rich deposits, namely precipitate, it is wise to use water-soluble salts of Sb and S. Refluxing is carried out through the aqueous reaction of SbCl3 and Na2S·3H2O under ambient conditions. Figure 1 presents the X-ray diffraction patterns of the Sb-rich precipitate obtained at various reaction times. In the beginning, the deposit does not show evident reflections and most probably contains crystalline regions in a large amorphous matrix. As the reaction time is extended to 14 h, an oxide phase that is indexed to valentinite (00-011-0691) forms. The resulting powder is orange. The valentinite is colorless in nature. This orange color may originate from a minute amount of amorphous stibnite, the reflections of which are present in the diffractogram with very weak intensity. Increasing the reaction time to 16 h, the reflections of Sb2S3 appear, indicating the formation of the grey-colored sulfide phase (stibnite: 00-001-0538) along with the presence of the oxide phase. At 18 h, the products show a similar stable combination of oxide and sulfide. Thus, the reaction time is fixed to 18 h for the testing of the performance of the antiscalants. Reaction times longer than 18 h cause the formation of crystals other than oxides and sulfides such as Sb2OS2 and Sb4O5Cl2 (not shown in this text).Figure 1
XRD patterns of the precipitates prepared at various reaction times.Since the product was a mixture of Sb2O3 and Sb2S3, we characterized the mixture with Rietveld refinement analysis of the XRD patterns with X’Pert HighScore Plus. The results are presented in Table 1. The reference deposit (prepared in the absence of antiscalants) has the following combination (Sb2S3 : Sb2O3, 86 : 14 in terms of the mole). However, the composition of the product mixture changed in the presence of polymeric antiscalants. The sulfides disappeared, while oxides became a dominant component in the product mixture.Table 1
The composition of deposit based on Rietveld method. The reference deposit has the following combination (Sb2S3 : Sb2O3) (86 : 14 in terms of mole). The data are obtained from Rietveld method run by using X’Pert HighScore Plus software program.
2550100PVA 310 : 1000 : 1000 : 100PVA 14.670 : 300 : 1000 : 100PEG—77 : 2377 : 23Gelatin52 : 480 : 10075 : 25PVP 5868 : 3267 : 330 : 100PVP 80 : 1000 : 1000 : 100Figure2 shows an X-ray diffraction patterns of the precipitates prepared in the presence of Gelatin at various dosages. In all diffractograms, the precipitates are the mixture of Sb2S3 and Sb2O3 with varying compositions. However, Gelatin does not influence the crystal structure.Figure 2
XRD patterns of the precipitates prepared in the presence of Gelatin at 25, 50, and 100 ppm.The existence of polymeric antiscalants has a clear influence on the morphology of precipitates. Scanning electron microscopy (SEM) images of the precipitates display the morphology of the deposits (Figure3). The morphology of the precipitates is heterogeneous in nature. There are needles, aggregates of microspheres, dumbbell-shaped crystals, and plates. While the needles, aggregates of microspheres (average diameter: 1.0±0.8μm), and dumbbell shape morphologies seem crystal and most probably Sb2S3, the plates may refer to Sb2O3. The morphology of the stibnite-based geothermal deposits has previously been shown [28]. The size and shapes of the precipitates were consistent with the literature [29]. For instance, the needles had 4.8±3.7μm length and 1.0±0.8μm width. Plate and dumbbell-shaped morphologies were also observed for some particular crystals. Figure 4(a) shows the crystals prepared in the presence of 50 ppm Gelatin. The needles are split into more substantial and more complex geometrical structures by the assembly of the process of needles. The dumbbell-shaped crystals probably formed from the merging and splinting of the long needles [30]. Figure 4(b) displays the morphology of the precipitates in the presence of 50 ppm PVP. Aggregates of spheres (sulfide phase) and a plate of the needles (oxide phase) coexist.Figure 3
SEM image of the reference prepared by refluxing of SbCl3 and Na2S·3H2O in 18 h. The magnification is 5000x.Figure 4
SEM image of the representative samples prepared in the presence of 50 ppm (a) Gelatin and (b) PVP. The magnification is 25000x.
(a)(b)It is crucial to dispose of geothermal fluid by reinjection, either into shallow or deep geothermal wells. The temperature changes may bring about the oversaturation of some minerals such as stibnite, thus creating a tendency to precipitate. It is important to assess the state of mineral saturation in the waste geothermal fluid that will be disposed of by reinjection to find the optimum temperature for reinjection. Figure5 indicates the activity product for the stibnite and stibnite solubility curve. For example, stibnite is equal to zero at around 100°C. The degree of supersaturated decreases as the temperature increases, particularly above 100°C in geothermal fluid in western Turkey.Figure 5
Changes in the state of stibnite in geothermal fluid.The seeping of the polymeric antiscalants into the deposit structure, if it takes place, is a significant question. It becomes an even more critical question since the amount of deposit is used for the determination of antiscalant performance. At low dosages, the amount of deposit after subtracting the polymeric antiscalant portion is almost unchanged. We could not detect the amount of polymeric antiscalant in the precipitated deposit by thermogravimetry; however, we observed the presence of the antiscalant molecule by vibrational spectroscopy. Figure6 displays the vibration spectra of the deposits presented in the absence and presence of the polymeric antiscalants. While the reference does not show vibrational signals in the infrared region, the precipitates prepared in the presence of PVA and Gelatin show characteristic signals of specific bonds that belong to the polymer of interest. For instance, the one prepared in the presence of Gelatin showed characteristic bending at 1649 cm-1 of N-H bond. Another characteristic signal of Gelatin could be seen at 1144 cm-1 of C-N stretching. Thus, the combination of both thermogravimetry and spectroscopy results suggest that a small amount of polymeric antiscalant remains in the deposit.Figure 6
Fourier transform infrared spectra of the reference, the precipitate prepared in the presence of 100 ppm PVA and Gelatin.


## 3.2. Performance of the Antiscalants

Using antiscalant in the model reaction, there are two success criteria: (i) the decrease of the amount of precipitate; (ii) the concentration of the ions in the decantate such as Sb3+ and S2- after the isolation of precipitate. Table 2 presents the concentrations of Na+, Sb3+, and S2- left in the decantate solution in terms of ppm. Independent of the chemistry of the antiscalants, the concentration of the Sb3+ increases in the presence of antiscalants. An electrostatic interaction may take place between Sb cations and electron-rich groups on the backbone of polymeric antiscalants such as hydroxyl for PVA, oxygen of PEG, the nitrogen of pyrrolidone and hydroxyl and amine groups of Gelatin. Thus, both Na+ and Sb3+ are held in the solution and do not contribute to the formation of solid precipitated by the aforementioned groups. However, the antiscalants were not as effective as in the dissolution of the sulfur ions. Most probably, they do not have positively charged (or at least partially positively charged) functional groups on their backbone; therefore, negatively charged sulfur anions are not able to find available sites on polymeric molecules to interact with. Reduction of the amount of precipitate is another criterion for the performance of antiscalants; in fact, it is the main motivation for using antiscalants in the geothermal fields. In the model reaction, the amount of precipitate is also studied. The reference sample provides 290 mg of the precipitate. The ones prepared in the presence of the antiscalants are lower than this value, except PVA 31-70 kg/mol by which the amount of precipitate is above the reference point most, probably due to the existence of polymeric molecules in the precipitate. The maximum reduction of the solid deposit that refers to scaling in real fields is obtained by the application of Gelatin (nearly %12.4). Considering that a certain amount of polymeric antiscalant is kept inside the precipitate as the vibrational spectroscopy suggests, the reduction of the amount of deposit may be even higher in terms of percentage.Table 2
Concentration of several of ions (mg·L-1) in the decantate solution after isolation of solid content so-called deposit. Dosage of the antiscalants is 5 ppm. The reference points out the reaction carried out in absence of antiscalants.
Antiscalants[Na+][S=][Sbn+]The amount of depositThe amount of deposit after subtraction of the polymer/mgThe amount of deposit after subtraction of the polymerReference98056222902900PVA 31116020643133130PVA 14.6119021512832830Gelatin117015622542540PVP117018792602600The dosage of the antiscalant was also examined, taking Gelatin as a representative example. Dosages higher than 5 ppm were studied: 25, 50, and 100 ppm. The concentration of the ions and the amount of deposit after the reaction are given in Table3. The application of 5 mg of Gelatin increases the concentration of Sb from 22 to 62 ppm. As the dosage of antiscalant increases, the concentration of Sb remains almost unchanged compared to the reference sample. It seems that Gelatin only works for low dosage. In contrast, the concentration of sulfur increases as the dosage increases. At 5 ppm, 5 ppm sulfur concentration is lower than that of the reference and gradually increases as the dosage increases to 96 ppm. Thus, the polymeric antiscalant was found to play the opposite effect on the concentration of the Sb3+ and S2- ions. While the Sb ion was suspended in the decantate solution at low dosages, [S2-] was found to be higher compared to that of the reference. A similar trend is seen in other antiscalants (Figure 7).Table 3
The effect of Gelatin at various dosages. The concentration of the ions is given in terms of ppm. The amount of polymeric antiscalant remains in the deposit is determined by gravimetry.
Dosage/ppm[Na+][S=][Sbn+]The amount of deposit/mgThe amount of deposit after subtracting of the polymer/mgThe amount of polymer remaining in the deposit/mgReference9805622290511701662254254025166060102372352501260891428327851001370961234733710Figure 7
The concentration of Sb3+ and S2- in the presence of the antiscalants at all dosages. The dashed line represents the concentration of the ion of interest for reference (without antiscalants).At low dosages, the amount of deposit decreased from 290 mg to 254 mg. The lowest was recorded when 25 ppm was applied (18%). At the highest dosage of 100 ppm antiscalant, the amount of deposit was even higher (337 mg). The remarkable increase in the amount of precipitate at high dosages may have originated from flocculation (Scheme3).Scheme 3
Schematic representation of flocculation.Briefly, flocculation is a process that promotes agglomeration of the particles by the help of a high dosage of the long polymeric chain. As a result, sedimentation of the particles takes place. Meanwhile, the settling of the particles is assisted by the presence of flocculants, which are organic molecules. A long polymer chain interacts with more than one particle such that agglomeration occurs and the agglomerated structure has a larger massive structure. At high dosages, flocculation may be the main mechanism taking place.


## 4. Conclusions

This paper presented a model lab reaction to test potential polymeric antiscalants against Sb-rich scaling. We examined a simple reaction between Sb and S salts under ambient conditions. In short reaction times (12 h), the product was Sb2O3. The formation of Sb2S3 occurred gradually when the reaction time was extended to 18 h. Saturation index based on thermodynamic consideration suggests the formation of stibnite. The performance of the antiscalants was found to be strongly dependent on the dosage. A low dosage of polymeric antiscalants helped to increase the concentration of antimony ions in the decantate; on the other hand, high dosages improved the solubilization of sulfur ions. The antiscalants remarkably reduced the amount of precipitate. Gelatin was found to be the most promising antiscalant among those employed in this study. The amount of precipitate increased at high dosages, most probably due to the occurrence of flocculation. To investigate ways to improve the performance of antiscalants, a computational study focusing on the calculation of binding energy between Sb3+/S2- ions and functional groups in aqueous systems should be performed. The functional groups should have high binding energy to the constituent atoms of the deposit.



---

*Source: 8867084-2020-08-01.xml*