3.1. Scale Inhibitor Structure Analysis
The degradable scale inhibitor MA-AA-AMPS was structurally characterized by infrared spectroscopy. The analysis, combined with the infrared features of monomers MA and AMPS, is as follows (
Figure 2). In the characteristic region of C=C double bond (around 1640 cm
−1 (grey area)), no obvious absorption peak appeared in the spectrum of MA-AA-AMPS, indicating that the reactive monomers had been effectively removed through purification, and the C=C double bonds of the monomers were opened to participate in the polymerization reaction, confirming that the product was a polymer of monomers, such as MA and AMPS. A stretching vibration peak of -OH was observed around 3417 cm
−1, a characteristic absorption peak of C=O double bond existed at 1729 cm
−1 (grey area), and a stretching vibration peak of C-O bond appeared at 1412 cm
−1 [
27]. The broad peaks in the range of 2596–3220 cm
−1 (orange area) jointly confirmed the presence of carboxylic acid groups (-COOH) in the product, which was consistent with the reaction path of MA ring, opening hydrolysis to generate carboxylic acid groups. The absorption peak at 1565 cm
−1 (grey area) was attributed to the bending vibration of -NH bond in the amide group (-CONH-), proving that the amide functional group of the AMPS monomer was introduced into the product. The stretching vibration peak of the S=O bond at 1047 cm
−1 (pink area) and the stretching vibration peak of the S-O bond at 642 cm
−1 were typical infrared characteristics of sulfonic acid groups (-SO
3H), indicating that the sulfonic acid structure of the AMPS monomer was retained in the product [
23]. In conclusion, infrared spectroscopy effectively characterized the functional group composition of MA-AA-AMPS. The polymerization reaction made the C=C double bonds of the monomers disappear, and the product retained carboxylic acid groups derived from MA and amide and sulfonic acid groups derived from AMPS, which was consistent with the structural design of the target copolymer and the requirements for scale inhibition function, providing a structural basis for the study of its scale inhibition performance.
To further verify the successful synthesis of MA-AA-AMPS, a
1H NMR analysis was performed (
Figure 3). In the low-field region (δ 7.42–11.67), the singlet at δ 10.13–11.67 can be assigned to the active hydrogen signals of carboxyl groups (-COOH) and those adjacent to nitrogen-containing carbonyl groups [
27]. These hydrogens exhibit significantly reduced electron density due to the strong electron-withdrawing effect of O and N atoms, resulting in low-field chemical shifts. Moreover, the rapid exchange of active hydrogens weakens the coupling effect, thus showing a singlet feature, which matches the -COOH and nitrogen-containing functional groups (e.g., amide structures) in the molecular structure. The singlet at δ 7.42 can be further assigned to hydrogens on nitrogen-containing heterocycles or amide groups, localized in this region due to the synergistic effect of N electronegativity and carbonyl groups. In the mid-field region (δ 2.00–4.00), the multiplets (e.g., d peaks, m peaks) near δ 2.51–3.14 correspond to hydrogens of methylene (-CH
2-) and methine (-CH-) groups connected to heteroatoms (N, S, etc.) or electron-withdrawing groups (-SO
3H, -COOH, etc.) [
23]. In the molecule, -SO
3H and nitrogen-containing side chains reduce the electron density of hydrogens on the connected carbons, shifting the chemical shifts to the mid-field. The spin-spin coupling of adjacent hydrogens (e.g., J coupling for d peaks, multiple couplings for m peaks) complicates the peak shapes, which is consistent with the carbon-hydrogen environments of side chains and functional group connections. In the high-field region (δ 1.00–2.00), the peak cluster at δ 1.07–1.54 is assigned to saturated C-H hydrogens on alkyl chains (e.g., -CH
2-, -CH
3 in the molecular backbone). Alkyl hydrogens have high electron density, leading to high-field chemical shifts. Methyl groups (-CH
3) often show singlets (e.g., the singlet at δ 1.49) due to a relatively uniform surrounding environment. Methylene groups (-CH
2-) in long-chain alkyls exhibit multiplets due to coupling with adjacent hydrogens, consistent with the carbon-hydrogen distribution in the molecular backbone. In summary, the chemical shifts and peak shapes in the
1H NMR spectrum match the electron densities and coupling characteristics of hydrogens in different environments (active hydrogens, hydrogens connected to heteroatoms, alkyl hydrogens) in the MA-AA-AMPS molecular structure. This effectively confirms the presence of functional groups, such as carboxyl, nitrogen-containing carbonyl, and sulfonic acid groups, as well as the connection mode of alkyl chains, verifying the successful synthesis of the MA-AA-AMPS scale inhibitor.
Thermogravimetric analysis was performed to obtain the mass loss of the MA-AA-AMPS scale inhibitor at different temperature ranges, enabling quantitative evaluation of its thermal stability (
Figure 4). The results show that the thermal decomposition of MA-AA-AMPS mainly occurs in three stages: the first stage (20~220 °C), with a mass loss rate of approximately 10%, which is mainly due to the evaporation of water molecules adsorbed on the polymer; the second stage (220~335 °C), with a mass loss of about 23%, resulting from the decomposition of polymer side chains (e.g., sulfonic acid groups, carboxylic acid groups); and the third stage (335~436 °C), with a mass loss rate of around 37%, primarily caused by the thermal decomposition of the molecular main chain and cleavage of C-C bonds. When the temperature exceeds 436 °C, the scale inhibitor is completely carbonized, leading to minimal mass change. The mass loss at this stage is mainly attributed to the sublimation of carbon residues.
3.2. Evaluation of Scale Inhibition Efficiency
The terpolymer MA-AA-AMPS was successfully synthesized in this study. To investigate the effects of various factors on its efficacy in inhibiting calcium carbonate scaling, static experiments were conducted to evaluate its scale inhibition performance. The terpolymer synthesized under optimal conditions was selected for subsequent assessments, with parameters such as copolymer dosage, water bath temperature, pH value, and calcium ion concentration adjusted individually. As shown in
Figure 5a, MA-AA-AMPS exhibits a “low dosage-high efficiency” characteristic: the scale inhibition rate exceeds 80% at a dosage of 2%, which is approximately 2% lower than that of commonly used phosphoric acid scale inhibitors (requiring 4% dosage to achieve similar efficacy). This is attributed to the synergistic effect of carboxylic acid, amide, and sulfonic acid groups in its molecular structure: carboxylic acid groups reduce supersaturation by chelating Ca
2+, amide groups adsorb onto crystal surfaces via hydrogen bonds, and sulfonic acid groups induce lattice distortion [
29]. The combination of these multiple mechanisms enables the scale inhibitor to efficiently occupy crystal growth sites. In contrast, phosphoric acid scale inhibitors rely on single P-O bond chelation, and their scale inhibition rate only tends to stabilize when the dosage is increased to 3%, indicating that a small amount of MA-AA-AMPS can achieve high-efficiency scale inhibition.
With the scale inhibitor concentration set at 3%, the effect of different pH values on the scale inhibition rate of MA-AA-AMPS was tested and compared with that of phosphoric acid scale inhibitors (
Figure 5b). The results show that the scale inhibition rate of MA-AA-AMPS is consistently higher than that of phosphoric acid scale inhibitors under all pH conditions, maintaining over 80% in the pH range of 3–8, indicating a wide application range. At low pH (2–5), the molecular chains of MA-AA-AMPS are curled up due to hydrogen bonding. As the pH increases, carboxyl and sulfonic acid groups undergo deprotonation, and enhanced electrostatic repulsion stretches the molecular chains, exposing more active sites (e.g., -COO
−, -SO
3−) to inhibit calcium carbonate crystal growth through the “adsorption-encapsulation” dual effect. At high pH (>5), the ionization equilibrium of HCO
3− shifts rightward, leading to a surge in CO
32− concentration, which accelerates calcium carbonate nucleation. However, MA-AA-AMPS can still delay crystal aggregation and crystallization through hydrogen bonding between amide groups and crystal surfaces, with a scale inhibition rate (64%) significantly higher than that of phosphoric acid scale inhibitors (43%), breaking the limitation of traditional scale inhibitors with sharply reduced performance under extreme pH conditions. As shown in
Figure 5c, temperature significantly affects the scale inhibition effect. In the high-temperature range of 80–150 °C, the scale inhibition rate of MA-AA-AMPS is consistently superior to that of phosphoric acid scale inhibitors, with a fluctuation of <5% before 110 °C. This is because a moderate temperature increase promotes the ionization of side chain groups (e.g., -COOH→-COO
−), enhancing chelation efficiency with Ca
2+. When the temperature exceeds 110 °C, although the scale inhibition rate decreases rapidly (still >50% at 150 °C), the thermal stability of C-C bonds and amide bonds in its molecular main chain is better; only partial side chains break, and the remaining carboxylic acid and sulfonic acid groups can still interfere with crystal growth through “point adsorption”, while the scale inhibition rate of phosphoric acid scale inhibitors is <26% at 150 °C. Regarding calcium ion concentration, as the Ca
2+ concentration increases from 240 mg/L to 1200 mg/L, the scale inhibition rate of MA-AA-AMPS shows a “slow decline-rapid decline” trend (
Figure 5d). At a Ca
2+ concentration of 840 mg/L, the scale inhibition rate remains at 54% because multiple chelating functional groups in the molecule can form stable five-membered/six-membered ring complexes with Ca
2+, delaying precipitation formation. When the concentration exceeds 840 mg/L, chelating sites become saturated, and excess Ca
2+ rapidly combines with CO
32− to form scale, leading to a sharp drop in the scale inhibition rate (down to 33% at 1200 mg/L). Compared with phosphoric acid scale inhibitors (with a scale inhibition rate of <50% at a Ca
2+ concentration of 600 mg/L), the chelating capacity of MA-AA-AMPS is increased by approximately 15%. The spatial distribution of its multiple functional groups optimizes the synergistic chelation efficiency for Ca
2+, expanding the application boundary in high-calcium hard water.
To investigate the effects of various factors on the efficacy of terpolymer MA-AA-AMPS in inhibiting calcium sulfate scaling, static experiments were conducted to evaluate its scale inhibition performance. The terpolymer synthesized under optimal conditions was selected for subsequent assessments, with parameters such as copolymer dosage, water bath temperature, pH value, and calcium ion concentration adjusted individually. As shown in
Figure 6a, the scale inhibition rate of MA-AA-AMPS exceeds 80% at a dosage of 2%, while commonly used phosphoric acid scale inhibitors require a 4% dosage to achieve the same effect. This is attributed to the synergistic effect of carboxylic acid, amide, and sulfonic acid groups in its molecular structure: carboxylic acid groups reduce the supersaturation of calcium sulfate by chelating Ca
2+, inhibiting crystal nucleation. Amide groups adsorb onto the surface of calcium sulfate crystals via hydrogen bonds, blocking growth sites. Sulfonic acid groups induce lattice distortion, disrupting the crystal structure [
29]. The combination of these multiple mechanisms enables MA-AA-AMPS to efficiently occupy key growth sites. In contrast, phosphoric acid scale inhibitors rely on single P-O bond chelation, and their scale inhibition rate only tends to stabilize when the dosage is increased to approximately 3%, highlighting the advantage of MA-AA-AMPS in achieving high-efficiency scale inhibition with low dosage.
With the scale inhibitor concentration set at 3%, the effect of different pH values on the scale inhibition rate of MA-AA-AMPS against calcium sulfate was tested and compared with that of phosphoric acid scale inhibitors (
Figure 6b). The results show that the scale inhibition rate of MA-AA-AMPS is consistently higher than that of phosphoric acid scale inhibitors under all pH conditions, maintaining over 80% in the pH range of 3–8, indicating a wide application range. At low pH (2–5), the molecular chains of MA-AA-AMPS are curled up due to hydrogen bonding. As pH increases, carboxyl and sulfonic acid groups undergo deprotonation, and enhanced electrostatic repulsion stretches the molecular chains, exposing more active sites, such as -COO
− and -SO
3−, to inhibit the crystallization and growth of calcium sulfate crystals through the “adsorption-encapsulation” dual effect. At pH > 5, although changes in the chemical environment of the solution do not significantly alter the scaling driving force of calcium sulfate (unlike calcium carbonate, which is affected by carbonate ionization), MA-AA-AMPS can still delay crystal aggregation and crystallization through hydrogen bonding between amide groups and crystal surfaces, with a scale inhibition rate (92%) significantly higher than that of phosphoric acid scale inhibitors (64%), breaking the limitation of traditional scale inhibitors with sharply reduced performance in acidic/alkaline water. In the high-temperature range of 80–150 °C, the scale inhibition rate of MA-AA-AMPS against calcium sulfate is consistently superior to that of phosphoric acid scale inhibitors (
Figure 6c). The scale inhibition rate of MA-AA-AMPS fluctuates by <5% before 110 °C because the moderate temperature increase promotes the ionization of side chain groups (e.g., -COOH→-COO
−), enhancing chelation efficiency with Ca
2+ and more effectively inhibiting the nucleation and growth of calcium sulfate crystals. When the temperature exceeds 110 °C, although the scale inhibition rate decreases rapidly, it remains >50% at 150 °C. Compared with phosphoric acid scale inhibitors (with a scale inhibition rate <26% at 150 °C), the thermal stability of C-C bonds and amide bonds in the molecular main chain of MA-AA-AMPS is better; only partial side chains break, and the remaining carboxylic acid and sulfonic acid groups can interfere with the growth of calcium sulfate crystals through “point adsorption”, exhibiting good temperature resistance and solving the problem of high-temperature failure of traditional scale inhibitors.
As shown in
Figure 6d, as the Ca
2+ concentration increases from 1500 mg/L to 7500 mg/L, the scale inhibition rate of MA-AA-AMPS against calcium sulfate shows a “rapid decline-slow decline” trend. At a Ca
2+ concentration of 4000 mg/L, the scale inhibition rate remains at 50% because multiple chelating functional groups in the molecule can form stable five-membered/six-membered ring complexes with Ca
2+, binding Ca
2+ and delaying the formation of calcium sulfate precipitation. When the concentration exceeds 2000 mg/L, chelating sites become saturated, and excess Ca
2+ rapidly combines with SO
42− to form scale, leading to a sharp drop in the scale inhibition rate (down to 29% at 7500 mg/L). Compared with phosphoric acid scale inhibitors (with a scale inhibition rate <14% at 7500 mg/L), the chelating capacity of MA-AA-AMPS is increased by approximately 15%. The spatial distribution of its multiple functional groups optimizes the synergistic chelation efficiency for Ca
2+, expanding the application boundary in high-calcium hard water.
Calcium carbonate crystalline phases are classified into anhydrous and hydrated phases, with the anhydrous phase further subdivided into three crystal forms: calcite, aragonite, and vaterite. In natural environments, calcite is the most dominant and common form of calcium carbonate due to its excellent thermodynamic stability. Without the addition of scale inhibitors, calcite-phase calcium carbonate crystals exhibit a regular cubic morphology with smooth and flat surfaces, free of obvious pores, flaws, or other defects (
Figure 7a). However, after introducing the MA-AA-AMPS scale inhibitor, the surface structure of calcium carbonate crystals undergoes significant changes: the crystals become loose and porous overall, most exhibit irregular scaling characteristics, some even form irregular flocculent spherical morphologies, and the crystal edges show softening (
Figure 7b).
Based on the changes in crystal morphology (
Figure 7), the inhibition mechanism of MA-AA-AMPS on calcium carbonate scaling is mainly attributed to the synergistic effect of lattice distortion and chelation. Carboxyl and sulfonic acid groups in the copolymer molecules selectively adsorb onto the active surfaces of calcium carbonate crystals, disrupting their original regular structure. This structural damage not only hinders the normal growth of crystals but also makes them more susceptible to being scoured and stripped under water flow. Meanwhile, the chelation of calcium ions by carboxyl groups and the synergistic destruction of calcium carbonate lattices by other groups further enhance the scale inhibition effect, collectively achieving effective inhibition of calcium carbonate scaling.
3.3. Scale Inhibition Mechanism
Based on the molecular structure characterization and scale inhibition performance test results of the terpolymer MA-AA-AMPS, its scale inhibition mechanism can be analyzed as shown in
Figure 8. As illustrated in
Figure 8, the side chains of MA-AA-AMPS molecules contain functional groups, such as carboxylic acid, sulfonic acid, and amide groups. Among them, carboxylic acid groups adsorb onto the surfaces of calcium carbonate and calcium sulfate nuclei, increasing the repulsion between different nuclei, which causes distortion during crystal growth and forms layered or porous structures. Secondly, sulfonic acid groups in the molecular chain can enhance the dispersibility and solubility of calcium carbonate and calcium sulfate precipitates. Amide groups interfere with the growth of calcium carbonate and calcium sulfate crystals through adsorption and chelation, leading to the formation of irregular structures. Under the synergistic effect of multiple functional groups, MA-AA-AMPS hinders the normal growth of calcium carbonate crystals and promotes the formation of defective porous structures, thereby effectively inhibiting the generation of calcium carbonate precipitates.
According to the existing literature, calcite is the most stable polymorph among the three crystal forms of CaCO
3, with the (1 1 0) and (1 0 4) crystal planes serving as its primary growth faces. The molecular models of the calcite surface and maleic anhydride-acrylic acid-2-acrylamido-2-methylpropanesulfonic acid (MA-AA-AMPS) copolymer were constructed using the Materials Studio 2023 (MS) software package. Subsequent structural optimization via energy minimization and molecular dynamics (MD) simulations were performed [
30]. The unit cell of calcite was retrieved from the American Mineralogist Crystal Structure Database (AMCSD), followed by optimization using the COMPASS force field. The optimized calcite crystal was cleaved along the (1 1 0) and (1 0 4) planes, respectively, and then subjected to supercell expansion. This process yielded supercells with dimensions of 24.287427 Å × 19.125326 Å × 32.603196 Å (for the (1 1 0) plane) and 24.287427 Å × 14.970004 Å × 33.738492 Å (for the (1 0 4) plane). To ensure consistency between the simulation results and experimental data, the MA-AA-AMPS copolymer was designed with a degree of polymerization of 17, and the molar ratio of MA:AA:AMPS was set to 1:3.6:12. For investigating the interaction between the MA-AA-AMPS copolymer and the calcite surface in an aqueous environment, a “liquid layer” composed of 200 water molecules and 1 MA-AA-AMPS molecule was prepared. This liquid layer was added to the simulation box and positioned adjacent to the (1 1 0) and (1 0 4) surfaces as the initial state. A vacuum slab with a thickness of 15 Å was introduced along the Z-axis (c-axis) to eliminate the influence of free boundaries on the structure. The interface model is illustrated in
Figure 9. On this basis, the Berebdsen temperature control method was adopted, and micro-canonical ensemble -canonical ensemble - micro-canonical ensemble (NVT-NPT-NVT) ensemble simulations were used to simulate the model at 353.15 K for 50 ps-1000 ps-200 ps.
Binding energy indicates the adsorption probability and strength between scale inhibitors and the surface of CaCO
3 crystals. The formula for calculating the binding energy between MA-AA-AMPS and the (1 1 0) and (1 0 4) planes of CaCO
3 crystals is as follows:
Here,
EA-B-C represents the total binding energy between the MA-AA-AMPS aqueous solution and the CaCO
3 crystal;
EA is the total binding energy between MA-AA-AMPS molecules and water;
EB; denotes the total binding energy between the CaCO
3 crystal and water;
EC stands for the total binding energy between water molecules; and
Eint is the interaction energy between MA-AA-AMPS molecules and the CaCO
3 crystal. As observed in
Table 2, the
Eint; between the MA-AA-AMPS molecules and CaCO
3 crystals is negative, indicating that the binding of MA-AA-AMPS to CaCO
3 crystals is exothermic. This confirms that MA-AA-AMPS molecules can stably bind to CaCO
3, thereby inhibiting the growth of CaCO
3. Meanwhile, the binding energy
EA-B-C between the MA-AA-AMPS aqueous solution and CaCO
3 crystals is much lower than the interaction energy
Eint; between the MA-AA-AMPS molecules and CaCO
3 crystals, suggesting that water molecules can enhance the binding energy between MA-AA-AMPS molecules and CaCO
3. This further reflects the scale inhibition performance of the MA-AA-AMPS inhibitor, and the conclusion is consistent with the experimental results.
To further explore the inhibition mechanism of the maleic anhydride-acrylic acid-2-acrylamido-2-methylpropanesulfonic acid (MA-AA-AMPS) copolymer, the radial distribution function (RDF) and coordination number (CN) of MA-AA-AMPS on different calcite crystal planes were analyzed based on molecular dynamics (MD) simulation results (
Figure 10) [
24]. In general, in the g(r)-r plot, peaks within 3.5 Å are mainly composed of chemical bonds and hydrogen bonds, while peaks beyond 3.5 Å are primarily formed by Coulomb forces and van der Waals forces [
31,
32]. As shown in
Figure 9, the first sharp peak in the g(r) curves of both the (1 0 4) and (1 1 0) planes appears at approximately 1.09 Å. This value is slightly greater than the sum of the covalent radii of oxygen and hydrogen atoms (0.96 Å), indicating the presence of strong hydrogen bonds between the MA-AA-AMPS copolymer and the calcite surface, with the length of these hydrogen bonds being shorter than that of normal hydrogen bonds. A sharp peak is observed at r = 2.53 Å, which matches the Ca-O bond length of 2.39 Å. This phenomenon arises because the carboxyl oxygen atoms of MA-AA-AMPS carry a negative charge, while calcium ions (Ca
2+) carry a positive charge, leading to the formation of strong ionic bonds between them. Additionally, MA-AA-AMPS exhibits a higher binding affinity for Ca
2+ on the (1 1 0) plane compared to the (1 0 4) plane. The intensity of the first peak in the g(r) curve of the (1 1 0) surface is greater than that of the (1 0 4) surface, which is consistent with the findings from binding energy studies. Meanwhile, the variation in the CN curve further confirms that the oxygen-containing functional groups (e.g., sulfonic acid groups, carboxyl groups) in MA-AA-AMPS form a coordination complex structure with the Ca
2+ on the crystal surface.