All structure optimizations and energy calculations were performed using the Gaussian 09 program (Frisch et al., 2009). Geometry optimization and frequency calculation for the reactants (R), products (P), transition states (TS), pre-reactive complexes (RC), intermediates (IM), and post-reactive complexes (PC) were conducted at the M06-2X/6-31+G(d,p) level of theory (Zhao and Truhlar, 2008). Single-point energy (SPE) calculations were performed at the M06-2X/6-311++G(3df,2pd) level. The employed quantum chemistry calculation method can be succinctly represented as M06-2X/6-311++G(3df,2pd)//M06-2X/6-31+G(d,p). Previous studies have demonstrated that the M06-2X method is suitable for predicting energies and kinetics for the aqueous-phase reactions of organic compounds with a good balance between accuracy and computational efficiency (Ji et al., 2020; Shi et al., 2024a; Zhang et al., 2022; Piletic et al., 2013). The solvation model based on density (SMD) was applied to account for the effects of solvent water molecules in the aqueous phase (Marenich et al., 2009). Intrinsic reaction coordinate calculations were used to confirm that the well-defined TSs connect with the corresponding reactants and products (Fukui, 1981). For reaction pathways where TSs could not be successfully located, relaxed scan methods were employed to obtain free-energy surfaces (Zhao et al., 2023; Ryu et al., 2018). Gibbs free energy (G) values for each structure at 298.15 K were calculated by combining the SPE with the Gibbs correction energy calculated at the theoretical level of geometry optimization. A correction factor of 1.89 kcal mol⁻¹ was applied to the activation free energy (ΔG‡) and reaction free energy (ΔrG) calculations for reactions where the number of molecules decreases or increases by one from R to TS or from R to P to explain the free energy change from the gas phase standard state of 1 atm to the aqueous phase standard state of 1 mol L⁻¹ (Sadlej-Sosnowska, 2007; Zhang et al., 2015). The combined use of Molclus 1.9.9.9 and Gaussian 09 programs was applied to search for the global minimum of the reactants (Lu, 2022).

A previous study found that the simplest protonated water cluster H⁺(H₂O)₁ model overestimated acid-catalyzed hydrolysis rates of ROOHs by combining with feasible DFT method (Hu et al., 2022). This is probably because H⁺(H₂O)₁ clusters with water molecules in the aqueous solution and the proton activity decreases (Agmon et al., 2016). The protonated water cluster model has been found to predict the acid-catalyzed hydrolysis kinetics of other organic compounds such as epoxydiols with high accuracy (Piletic et al., 2013). Here, we screened an appropriate protonated water cluster model by comparing calculated kA values for reactions between H⁺(H₂O)_n (n=1, 2, 3, 4) and the selected ROOHs with experimental values. Specially, C₁₃ α-AH, C₁₂ α-AH₍₁₎, C₁₂ α-AH₍₂₎, and C₁₀ α-HH were chosen due to the available experimental kinetic data under different pH values (Qiu et al., 2020b; Enami, 2022; Hu et al., 2022). The structures of these four ROOHs and H⁺(H₂O)_n (n=1, 2, 3, 4) are presented in Figs. S1 and S2 in the Supplement.

The second-order reaction rate constants kA of the elementary reactions in acid-catalyzed hydrolysis pathways were calculated using transition state theory (Eq. 1) (Zhao et al., 2023; Xu et al., 2019). The pseudo-first-order rate constants (kA′) were calculated by combining kA with the concentration of protonated water clusters, which are determined by pH. Corresponding acid-catalyzed hydrolysis lifetimes (τ1/e) can be subsequently derived by τ1/e=1/kA′. 1kA=σkBThexp⁡-ΔG‡RT, where σ is the reaction path degeneracy, T is the temperature (298.15 K), kB is the Boltzmann constant (J K⁻¹), h is the Planck constant (J s), R is the gas constant (8.314 J mol⁻¹ K⁻¹), ΔG‡ is the activation free energy.

The QSAR models were developed for kA of α- and β-substituted compounds, respectively, among the selected 45 ROOH model compounds. The Taft (σ*) constants, which are widely used to quantify the inductive effects of substituents in aliphatic systems (Lee and von Gunten, 2012; Kim and Huang, 2021; Ra et al., 2025), were employed to correlate with the logarithms of kA (log⁡kA) values in this study. The σ* values for different substituents, as shown in Table S1 in the Supplement, were obtained from the literature (Perrin et al., 1981). Herein, the total effects were evaluated by summing the σ* values (∑σ*) of each substituent (except the –OOH group) at the reaction center, i.e., the C_α site (Table S2).

We investigated the acid-catalyzed hydrolysis of four ROOHs, i.e., C₁₃ α-AH, C₁₂ α-AH₍₁₎, C₁₂ α-AH₍₂₎, and C₁₀ α-HH, using H⁺(H₂O)_n (n=1, 2, 3, 4) models with the DFT method. The calculated free-energy profiles for these reactions are presented in Figs. S3–S6. Concluded from the reaction profiles, a two-step acid-catalyzed hydrolysis pathway is revealed for these four ROOHs, with the first step being the rate-limiting step. As shown in Fig. S7, the H⁺ of H⁺(H₂O)_n attacks the -OOH group of the selected four compounds, leading to C_α-O bond rupture and simultaneous formation of a carbocation intermediate and H₂O₂ in the first step. Subsequently, the carbocation reacts with water molecules and yields the corresponding protonated alcohols.

Using the activation free energies of the rate-limiting step, the pseudo-first-order rate constants kA′ were calculated over a pH range of 0–14 using the M06-2X/6-311++G(3df,2pd)//M06-2X/6-31+G(d,p) method. The calculated kA′ values for the four selected ROOHs with H⁺(H₂O)_n models are presented in Fig. 1, along with the experimentally determined hydrolysis rates at different pH values (Qiu et al., 2020b; Enami, 2022; Hu et al., 2022; Endo et al., 2022). The H⁺(H₂O)₂ model was found to best reproduce the experimental data among H⁺(H₂O)_n (n=1, 2, 3, 4) models. In most cases, the discrepancies between the calculated and the experimental kA′ values are within a factor of 0.5 to 2.2. Two exceptions are C₁₀ α-HH at pH 3.3 and C₁₂ α-AH₍₂₎ at pH 4.5, but their uncertainties remain within one order of magnitude, an acceptable error range. In contrast, the H⁺(H₂O)₄, H⁺(H₂O)₃, and H⁺(H₂O)₁ models result in much larger discrepancies, with errors reaching 1.0×10-5, 1.1×10-3, and 2.1×108 times, respectively. Therefore, the computational strategy combining the H⁺(H₂O)₂ model with the M06-2X/6-311++G(3df,2pd)//M06-2X/6-31+G(d,p) method is well-suited for predicting kA values of ROOHs.

Employing the H⁺(H₂O)₂ model and the M06-2X/6-311++G(3df,2pd)//M06-2X/6-31+G(d,p) method, we conducted a systematic investigation for structure-activity relationships of kA values across 45 ROOH model compounds (Fig. 2a). We selected the simplest unsubstituted primary, secondary, and tertiary ROOHs, i.e., CH₃CH₂OOH, CH(CH₃)₂OOH, and C(CH₃)3OOH, as the reference compounds to assess the influence of substituents. Specifically, the influence of substituents was examined by comparing the kA values of α-substituted primary, secondary, and tertiary ROOHs, as well as β-substituted tertiary ROOHs, represented as CH2(X)OOH, CH(CH₃)(X)OOH, C(CH₃)2(X)OOH, and C(CH₃)₂(CH₂(X))OOH, with the corresponding unsubstituted ones, respectively. Here, X denotes substituents including –NH₂, –OH, –OCH₃, –CH = CH₂, –SH, –PH₂, –F, –Cl, and –CHO, covering the major functional group types found in atmospheric ROOHs. Therefore, the effects of different carbon skeletons at the C_α site (primary, secondary, and tertiary) and different substituents at the C_α and C_β sites of the –OOH group on the kA values of ROOHs were revealed.

For the selected 45 ROOH model compounds, their reaction free-energy profiles were calculated and shown in Figs. S8–S12. They follow two distinct reaction pathways, which are simplified and illustrated in Fig. 2b. CH₃CH₂OOH, CH2(X)OOH, and CH(CH₃)(X)OOH (X = F, Cl, CHO) undergo a one-step reaction pathway, where H⁺(H₂O)₂ and an H₂O molecule simultaneously attack the –OOH group and the C_α, respectively, leading to the formation of protonated alcohols and H₂O₂. Meanwhile, the other ROOH model compounds follow the two-step reaction pathway via the formation of a carbocation intermediate, similar to that of C₁₃ α-AH, C₁₂ α-AH₍₁₎, C₁₂ α-AH₍₂₎, and C₁₀ α-HH. It is found that these model compounds share nearly identical reaction sites (i.e., the –OOH group and its adjacent C_α atom) and follow analogous reaction pathways to C₁₃ α-AH, C₁₂ α-AH₍₁₎, C₁₂ α-AH₍₂₎, and C₁₀ α-HH. This mechanistic similarity implies that despite variations in their carbon skeletons and substituents, protonation and subsequent reactions are primarily localized at the C_α-OOH site, which is a common structural feature among ROOHs. Therefore, even though experimental data for these model compounds are currently lacking to validate the computational results, we believe the screened protonated water cluster model can be reasonably extended to investigate the acid-catalyzed hydrolysis of diverse ROOHs with acceptable uncertainty.

Based on reaction activation free energies, the kA values for 45 ROOH model compounds were calculated, as well as kA′ values under different pH conditions (Table S3 and Fig. 3). As shown in Fig. 3a, the kA′ of tertiary ROOH is the highest among the three unsubstituted ROOHs at the same pH, followed by secondary and primary ROOHs, aligning with the previous research findings (Hu et al., 2022). Furthermore, to clarify the effects of substituent types, we calculated the enhancement factors (EF) for kA′ of substituted ROOHs relative to their unsubstituted reference compounds. Because the predicted kA′ values for ROOHs exhibit a linear dependence on pH, the resulting EF values remain constant across different pH values. These EF values for α-substituted ROOH model compounds, CH2(X)OOH, CH(CH₃)(X)OOH, and C(CH₃)2(X)OOH are shown in Fig. 3b–d, with CH₃CH₂OOH, CH(CH₃)₂OOH, and C(CH₃)₃OOH as reference compounds, respectively. Substituents such as –NH₂, –OH, –OCH₃, –SH, and –CH = CH₂ increase kA′, with EF values ranging from 5.1×103–6.4×1023 for primary, 1.3×105–5.0×1018 for secondary, and 1.4–5.7×1013 for tertiary ROOHs. The –PH₂ substituent shows a divergent effect, increasing kA′ of primary and secondary ROOHs with the EF values of 1.3×105 and 2.5, respectively, but decreasing that of tertiary ones. While –OH and –OCH₃ are known to facilitate the acid-catalyzed hydrolysis of ROOHs (Hu et al., 2021a, b, 2022; Qiu et al., 2020b; Enami, 2022; Endo et al., 2022), our study is the first to show that –NH₂, –SH, –CH = CH₂, and –PH₂ can also enhance it. Among them, –NH₂ has the highest EF, followed by –OH and –OCH₃, –SH, –CH = CH₂, and –PH₂. In contrast, –F, –Cl, and –CHO significantly decrease the kA′.

To further evaluate the effectiveness of acid-catalyzed hydrolysis for these α-substituted model compounds in the atmosphere, we calculated their τ1/e values at pH 3.8 and 0.9, representing typical aerosol conditions in inland China and the Southeastern United States, respectively (Wang et al., 2022; Jia et al., 2018; Ding et al., 2019; Shi et al., 2019; Xu et al., 2020; Wang et al., 2020; Guo et al., 2015). Compared to the typical atmospheric retention time of ambient aerosols with approximately 1–2 weeks (Hodzic et al., 2016; Kristiansen et al., 2016), Table 1 shows the calculated kA and τ1/e values of the α-substituted ROOH model compounds that undergo effective acid-catalyzed hydrolysis on this time scale at pH 3.8 and 0.9. The τ1/e values for –NH₂-substituted primary ROOH, -NH₂- and -OH-substituted secondary ROOHs, as well as –NH₂–, –OH–, and –OCH₃-substituted tertiary ROOHs range from less than 1 s to 5.5 h at pH 3.8. As pH decreases to 0.9, effective hydrolysis occurs for –OH-substituted primary ROOH, –OCH₃-substituted secondary ROOH, and –SH-substituted tertiary ROOH, with τ1/e ranging from 40.9 min to 6.8 d. The τ1/e values for other compounds exceeding 2 weeks are shown in Table S3, indicating the limited effectiveness of acid-catalyzed hydrolysis under typical atmospheric conditions. In summary, substituents such as –NH₂, –OH, and –OCH₃ can facilitate effective acid-catalyzed hydrolysis of ROOHs under typical ambient conditions, while the –SH substituent is only effective under exceptionally low pH. Although –OH and –OCH₃ substituents are well-documented, we show that the –NH₂ substituent leads to significantly shorter τ1/e for the corresponding ROOHs. Despite the –NH₂ group prefers to exit in its protonated form (–NH3+) in the aqueous phase, the rapid reaction of ROOHs with unprotonated -NH₂ group may shift the equilibrium –NH3+ + H₂O ↔ –NH₂ + H₃O⁺ forward. Recent studies (Ji et al., 2020; Shi et al., 2024a) have reported fast reactions between small α-dicarbonyls and amines or ammonia under acidic aqueous conditions, with corresponding products detected experimentally. This indicates that the ROOHs with unprotonated –NH₂ group can still participate in the reaction. In addition, Enami et al. (2010) found that trimethylamine remains largely unprotonated at the air-water interface even at pH 4.0. These findings inspire us that both aqueous-phase and interfacial transformations of α-NH₂-substituted ROOHs are plausible. Previous studies demonstrate that α-NH₂-substituted ROOHs and their analogues α-N(CH₃)₂-substituted ones are primarily formed via the reactions of CIs with ammonia or the oxidation of tertiary amines (Li et al., 2024; Kjaergaard et al., 2023; Ma et al., 2021). Therefore, investigating the transformation of these nitrogen-containing ROOHs should be important, particularly in regions with high amine and ammonia concentrations.

It is intriguing to discuss why substituents such as –NH₂, –OH, –OCH₃, –CH = CH₂, –SH, and –PH₂ can enhance the acid-catalyzed hydrolysis of ROOHs. As discussed above, a common feature for the acid-catalyzed hydrolysis of these substituted ROOHs is the formation of carbocation intermediates during their two-step reaction pathway. As illustrated in Fig. 4, the greater the enhancing potential of a substituent, the lower the reaction free energy required for carbocation intermediate formation, resulting in higher intermediate stability. This trend remains consistent when using the other computational method, despite differences in the absolute free energies (Fig. S13). Furthermore, carbocation hydration shows minimal impact on reaction energetics, as demonstrated by comparing results from the monohydrated system to those from the implicit solvation model alone, using the reaction of C(CH₃)₂(OCH₃)OOH as a test case (Fig. S14). These findings suggest that the stabilizing effect of these substituents on carbocation intermediates is the driving force behind the enhanced acid-catalyzed hydrolysis. Exceptions for the –OH– and –OCH₃-substituted ROOHs should be caused by the slight difference in their two-step reaction pathways (Fig. S7). According to electronic effect theory (Naredla and Klumpp, 2013; Olah, 2001), substituents –NH₂, –OH, –OCH₃, –SH, –CH = CH₂, and –PH₂ stabilize carbocation intermediates through conjugated electron donation into the unoccupied orbital of the carbocation. This stabilizing effect follows the order: –NH₂ > –OH ≈ –OCH₃ > –SH ≈ –CH=CH₂ ≈ –PH₂. This order aligns with the observed trend in kA values, where α-NH₂-substituted ROOHs exhibit higher kA values than α-OH– and –OCH₃-substituted ones, which in turn are higher than α-SH–, –CH = CH₂–, and –PH₂-substituted ones (Table S3). Similarly, the stabilizing effect of these substituents on carbocation intermediates can also explain the order of kA values for tertiary ROOHs >secondary ROOHs > primary ROOHs. Tertiary ROOHs exhibit higher kA values due to stronger hyperconjugation interactions between the unoccupied p orbital of the carbocation and the additional C–H σ-bonds from the methyl group, which stabilize the carbocation intermediates (Alamiddine and Humbel, 2013).

Based on the above analysis, we deduced that the presence of N and O atoms is the main reason for the strongest facilitating effect of –NH₂, –OH, and –OCH₃ in the acid-catalyzed hydrolysis of ROOHs. This raises an interesting question of how do substituents attached to N or O atoms affects the kA′ values. To explore this, we examined the effect of substituents attached to O atom as a test case and calculated the EF for kA′ of C(CH₃)₂(OY)OOH (Y being substituents) compared to the reference compound C(CH₃)₂OCH₃OOH. As shown in Fig. 3f, substituents –CH₂CH₃ and –CH₂CH₂CH₃ lead to only a minor reduction for kA′. This is validated by the similar experimental kA′ of C₁₂ α-AH₍₁₎ and C₁₃ α-AH, which possess –OCH₂CH₃ and –OCH₂CH₂CH₃, respectively (Hu et al., 2022). Substituents –CH(CH₃)₂ and –C(CH₃)₃ increase the kA′, with EF values of 10.6 and 45.9, respectively. However, –CH=CH₂ and –CHO substituents dramatically decrease kA′ by approximately 5 and 10 orders of magnitude, respectively. As shown in Table 1, the C(CH₃)2(OY)OOH with Y being four alkyl substituents undergo rapid acid-catalyzed hydrolysis with τ1/e values ranging from 3.5 s to 6.0 min even at pH 3.8, while C(CH₃)₂(OCH = CH₂)OOH only undergoes effective reaction at pH 0.9 (τ1/e=1.4 h). In contrast, the acid-catalyzed hydrolysis of C(CH₃)₂(OCHO)OOH is difficult to occur. These findings underscore that not all oxygen-containing substituents at the C_α site are equally effective in promoting acid-catalyzed hydrolysis of ROOHs, highlighting the importance of specific structural features. The substituent effects on the O atom could be reasonably extrapolated to the N atom. It should be noted that although the direct acid-catalyzed hydrolysis of C(CH₃)₂(OCHO)OOH is impossible, the indirect reaction initiated by the hydrolysis of the -OCHO group has been proposed (Chang et al., 2025; Zhao et al., 2018), which is beyond the range of this study.

For the β-substituted ROOHs, tertiary C(CH₃)₂(CH2(X))OOH (X = –NH₂, –OH, –OCH₃, –CH = CH₂, –SH, –PH₂, –F, –Cl and –CHO) were chosen as model compounds, as they potentially exhibit higher kA′ values compared to primary and secondary ones. By calculating the EF for kA′ values of C(CH₃)₂(CH2(X))OOH relative to the reference compound C(CH₃)₃OOH, we found that all nine substituents reduce the kA′ (Fig. 3e). Thus, we conclude that substitutes at C_β site could hinder the acid-catalyzed hydrolysis. The unfeasible acid-catalyzed hydrolysis of them aligns with previous experimental results that non-α-substituted monoterpene-derived organic peroxides exhibit greater persistence in aqueous environments (Zhao et al., 2022).

Based on the calculated log kA values and the ∑σ* constants (Table S2), QSAR models were developed for α- and β-substituted ROOH model compounds. As shown in Fig. S15, a strong linear correlation was established for α-substituted compounds, including CH2(X)OOH, CH(CH₃)(X)OOH, C(CH₃)2(X)OOH, and C(CH₃)₂(OY)OOH, with the equation as log kA=-11.555∑σ*+19.251 (n=21, R2=0.9083) after excluding compounds with unknown ∑σ* and those with substituents –CH = CH₂ and –CHO. The poor performance in describing the effects of substituents –CH = CH₂ and –CHO is likely because ∑σ* primarily characterizes the inductive effects of substituents (Perrin et al., 1981), while its description of conjugation effects is inadequate. A relatively weaker fit to the QSAR plot (log⁡kA=-3.499∑σ*-6.437 (n=9, R2=0.7446)) was found for compounds including C(CH₃)₃OOH and β-substituted compounds C(CH₃)₂(CH2(X))OOH (Fig. S16). Nonetheless, a negative correlation was found in both QSAR models. This indicates that the weaker the inductive effects of substituents (i.e., the smaller the ∑σ*), the higher the kA, which is consistent with the trend explained by the stability order of the formed carbocation intermediates discussed earlier.

To evaluate the applicability of the structure-activity relationship derived from model compounds to more complicated atmospheric ROOHs, we investigated the acid-catalyzed hydrolysis of eight ROOHs derived from isoprene (Wennberg et al., 2018), α-pinene (Zhang et al., 2017; Claflin et al., 2018), trimethylamine (Kjaergaard et al., 2023; Ma et al., 2021), and dimethyl sulphide (Berndt et al., 2019) using the screened H⁺(H₂O)₂ model via the DFT calculations (Figs. S17–S24). These ROOHs feature distinct substituents at the C_α site, including –N(CH₃)₂, –N(CH₃)(CHO), –OH, –CH = CH₂, –SCH₃, –SCHO, and –CHO, and unsubstituted. As shown in Fig. 5, the order of kA′ values for these ROOHs at the same pH (3.8 or 0.9) according to their substituents is as follows: –N(CH₃)₂ > –OH > –N(CH₃)(CHO) > unsubstituted > –CH = CH₂ > –SCH₃ > –CHO > –SCHO, similar to the trends observed in model compounds in three aspects. First, a –N(CH3)2 or –OH substituent at the C_α site of trimethylamine-OOH₍₁₎ or α-pinene-OOH₍₁₎ results in their high kA′ values, with τ1/e values less than 2 d (pH 3.8) and 3.6 min (pH 0.9), respectively. Second, the introduction of a –CHO group to the N atom in the –N(CH₃)(CHO) substituent of trimethylamine-OOH₍₂₎ leads to a remarkable reduction in kA′ values, with τ1/e values exceeding 45 d, even at pH 0.9 (Table S4). The possible reaction of trimethylamine-OOH₍₂₎ initiated by the hydrolysis of –N(CH₃)(CHO) group is not considered in this work (Zhang et al., 2015). Moreover, the attachment of a –CHO group to the S atom in the –SCHO substituent leads the corresponding dimethyl sulfide-OOH₍₂₎ to exhibit the lowest kA′ values, even lower than that of α-pinene-OOH₍₃₎ featuring a –CHO substituent. Finally, the –CH = CH₂ and –SCH₃ substituents contribute to the relatively low kA′ values of isoprene-OOH and dimethyl sulfide-OOH₍₁₎, respectively. Although the existence of enhancing substituents, their kA′ values are lower than the unsubstituted α-pinene-OOH₍₂₎, which is attributed to the reducing effect of an additional –OH substituent at the C_β site for isoprene-OOH, and the primary C_α of dimethyl sulfide-OOH₍₁₎ compared to tertiary C_α of α-pinene-OOH₍₂₎. The reproduction of the substituents effect trend on kA′ values in atmospheric ROOHs demonstrates that the structure-activity relationship derived from model ROOHs can be effectively extended to predict the kA values of structurally diverse ROOHs.

In the aerosol aqueous phase, anions such as nitrate (NO3-) and sulfate ions (SO42-) are important components in addition to H₂O. These anions can either directly nucleophilically attack the C_α of ROOHs or react with the formed carbocation intermediates to produce organic nitrates and organic sulfates (Figs. S3–S6 and S17–S24). Understanding the competition between acid-catalyzed hydrolysis and esterification reactions of atmospheric ROOHs is crucial for elucidating their transformation products in ambient aerosols. Herein, we use C₁₃ α-AH, C₁₂ α-AH₍₁₎, C₁₂ α-AH₍₂₎, and C₁₀ α-HH as examples to elucidate the competition between their acid-catalyzed hydrolysis and esterification reactions. As shown in Figs. S3–S6, reactions of their derived carbocations with H₂O and NO3- are endothermic, while those with SO42- are barrierless and exothermic. Although the formation of hemiacetals/geminal diols through reactions with H₂O is thermodynamically unfavorable, these species can subsequently be transformed into lactols (Qiu et al., 2020b; Enami, 2022; Hu et al., 2022). Therefore, competitive reactions with H₂O and SO42- must be considered. If the concentrations of H₂O and SO42- are equal, carbocations preferentially react with SO42- at near diffusion-controlled rate constants (∼1010 L mol⁻¹ s⁻¹) to form organic sulfates. In fact, the distribution of products, including hemiacetals/geminal diols, transformed lactols, and organic sulfates in aerosols, is determined by the second-order rate constants for carbocation reactions with H₂O and the variable concentrations of H₂O and SO42-. The formation mechanisms of organic sulfates have been a hot research topic in atmospheric chemistry. To date, a variety of formation mechanisms have been proposed; among them, the acid-catalyzed ring-opening of epoxides has been widely adopted to explain organic sulfates formation in acidic sulfate aerosol (Surratt et al., 2010; Lin et al., 2012; Cooke et al., 2024). Nevertheless, existing mechanisms still cannot fully explain the observed ambient abundance of organic sulfates. Here we present a plausible carbocation-mediated organic sulfates formation mechanism that occurs during the aqueous-phase transformation of ROOHs in the presence of H⁺ and SO42-. However, our structure-activity relationship analysis indicates that, among our studied ROOHs, only those with C_α substituents such as –OH, –OCH₃, –NH₂, and –N(CH₃)₂, can effectively generate the corresponding carbocation intermediates on the lifetime scale of aerosols under the considered pH conditions (pH 3.8 and 0.9). In the atmosphere, such ROOHs primarily derive from the reactions of water, alcohols, or ammonia with CIs produced via ozonolysis of unsaturated hydrocarbons or from ⚫OH oxidation of tertiary amines (Wang et al., 2023; Li et al., 2024; Kjaergaard et al., 2023). Therefore, we speculate that the proposed carbocation-mediated mechanism would be helpful to explain organic sulfates formation in SOA derived from the aforementioned reactions, whereas its applicability to other sources such as ⚫OH / NO3⚫ oxidation of volatile organic compounds (Surratt et al., 2008) could be limited unless the precursor compounds contain activating substituents that support the formation of the α-substituted ROOHs mentioned above.