Chemical composition and hydrolysis of organic nitrate aerosol formed from hydroxyl and nitrate radical oxidation of α-pinene and β-pinene

Atmospheric organic nitrate (ON) is thought to play a crucial role in the formation potential of ozone and aerosol, which are the leading air pollutants of concern across the world. Limited fundamental knowledge and understanding of the life cycles of ON currently hinder the ability to quantitatively assess its impacts on the formation of these pollutants. Although hydrolysis is currently considered an important loss mechanism of ON based on prior field measurement studies, this process for atmospherically relevant ON has not been well constrained by fundamental laboratory studies. In this comprehensive study, we investigated the chemical composition and hydrolysis process of particulate ON (pON) formed from the oxidation of α-pinene and βpinene by hydroxyl (OH q) and nitrate radicals (NO3 q). For pON that undergoes hydrolysis, the hydrolysis lifetime is determined to be no more than 30 min for all systems explored. This is significantly shorter than those reported in previous chamber studies (i.e., 3–6 h) but is consistent with the reported lifetime from bulk solution measurement studies (i.e., 0.02–8.8 h). The discrepancy appears to stem from the choice of proxy used to estimate the hydrolysis lifetime. The measured hydrolyzable fractions of pON (FH) in the α-pinene+OH q, β-pinene+OH q, α-pinene+NO3 q, and β-pinene+NO3 q systems are 23 %–32 %, 27 %–34 %, 9 %– 17 %, and 9 %–15 %, respectively. While a very low FH for the NO3 q oxidation system is expected based on prior studies, FH for the OH q oxidation system is surprisingly lower than predicted in past studies. Overall, the hydrolysis lifetime as well as FH obtained in this study serve as experimentally constrained parameters that are required in regional and global chemical transport models to accurately evaluate the impacts of ON on nitrogen budget and formation of ozone and aerosol.


Introduction
The oxidation of biogenic volatile organic compounds (BVOCs) by ozone (O 3 ), hydroxyl radicals (OH q ), and nitrate radicals (NO 3 q ) is a major source of secondary organic aerosol (SOA) globally (Kanakidou et al., 2005;Goldstein and Galbally, 2007;Spracklen et al., 2011).Many studies have pointed to the synergistic effects of anthropogenic emissions on biogenic SOA formation in the atmosphere (Weber et al., 2007;Carlton et al., 2010;Hoyle et al., 2011;Shilling et al., 2013;Xu et al., 2015a;Shrivastava et al., 2019).The oxidation of BVOC in environments with anthropogenic NO x emissions is an important mechanism for coupled biogenic-anthropogenic interactions.In the presence of NO x , the oxidation of BVOC can lead to the formation of organic nitrate (ON), a large component of reactive oxidized nitrogen.Results from ambient field measurements have revealed the ubiquitous presence of particulate ON ( p ON), where it contributes to a large fraction of submicron organic aerosol at different sites worldwide (Fry et al., 2013;Xu et al., 2015b;Liu et al., 2012;Rollins et al., 2012Rollins et al., , 2013;;Lee et al., 2016;Kiendler-Scharr et al., 2016;Ng et al., 2017).These findings highlight the importance to understand the formation and fates of ON to accurately evaluate its roles in NO x recycling, O 3 formation, and SOA formation.
Published by Copernicus Publications on behalf of the European Geosciences Union.
Monoterpenes (C 10 H 16 ) are a major class of BVOC with annual emissions of 157-177 Tg C yr −1 (Guenther et al., 2012).Laboratory studies have demonstrated that the NO 3 q oxidation of monoterpenes leads to a substantial formation of ON and SOA with ON yields up to ∼ 70 % (Wangberg et al., 1997;Berndt and Boge, 1997;Griffin et al., 1999;Hallquist et al., 1999;Spittler et al., 2006;Fry et al., 2009Fry et al., , 2014;;Boyd et al., 2015Boyd et al., , 2017;;Nah et al., 2016;Slade et al., 2017;Claflin and Ziemann, 2018).For photooxidation of monoterpenes in the presence of NO x , ON yields as high as 26 % have been reported for α-pinene (Noziere et al., 1999;Aschmann et al., 2002;Rindelaub et al., 2015).Monoterpene emissions do not depend strongly on light and typically continue at night, making them important ON and SOA precursors at any time of day (daytime and nighttime) and throughout the year (different seasons).It has been shown that monoterpene-derived ON is prevalent in areas where there are substantial biogenic-anthropogenic interactions and oxidation of monoterpenes contributes to a large fraction of SOA observed in the Southeastern US (L.Xu et al., 2015aXu et al., , b, 2018;;Lee et al., 2016;Zhang et al., 2018).
One of the largest uncertainties in our understanding of monoterpene ON chemistry is the extent to which ON acts as a permanent sink versus temporary reservoir of NO x (Takeuchi and Ng, 2018).This would depend on the fates of ON as they can either retain or release NO x upon further reactions.Once formed, gas-phase ON can undergo photolysis or OH q oxidation to release NO x or partition into the particle phase.p ON in turn can undergo further chemistry to release NO x or hydrolyze in the particle phase to form nitric acid (HNO 3 ).Further, ON and HNO 3 can be removed via dry and wet deposition.One important reaction of ON in the particle phase is hydrolysis in the presence of aerosol water, which is a mechanism for NO x loss (Day et al., 2010;Russell et al., 2011).Studies with bulk solutions showed that particlephase hydrolysis of tertiary nitrate is fast with a lifetime of minutes, while primary and secondary nitrate is stable (Darer et al., 2011;Hu et al., 2011).However, the hydrolysis of p ON in aerosol water is largely unconstrained.Results from field and modeling studies suggested a p ON lifetime of a few hours (Pye et al., 2015;Lee et al., 2016;Fisher et al., 2016;Zare et al., 2018).A few recent laboratory chamber studies elicited a complex picture where p ON formed from photochemical oxidation and NO 3 q oxidation of monoterpenes appears to experience different magnitudes of hydrolysis (Boyd et al., 2015(Boyd et al., , 2017;;Rindelaub et al., 2015;Bean and Hildebrandt Ruiz, 2016), likely due to the difference in the relative amount of primary, secondary, and tertiary nitrate in these oxidation systems.Overall, there are very limited studies on the further evolutions of ON produced from the oxidation of monoterpenes.
Here, we present results from a laboratory chamber study on the chemical composition and hydrolysis process of p ON formed from oxidation of α-pinene and β-pinene by OH q and NO 3 q .Specifically, we report the hydrolysis lifetimes and the fraction of hydrolyzable p ON formed in the systems examined in this study.This comprehensive chamber study on the hydrolysis of p ON produced from various oxidation pathways of monoterpenes and peroxy radical (RO 2 q ) fates provides the fundamental data to better constrain the role of hydrolysis in modulating p ON concentrations and lifetimes in the atmosphere; their potential as a NO x loss pathway; and their impacts on overall nitrogen budget, O 3 formation, and SOA formation.

Chamber experiment design and procedure
A series of chamber experiments were performed in the Georgia Tech Environmental Chamber facility (Boyd et al., 2015) housing two 12 m 3 Teflon reactors.Precursor volatile organic compounds (VOCs) were α-pinene (99 %, Sigma-Aldrich) and β-pinene (99 %, Sigma-Aldrich) and the oxidation conditions of interest were OH q and NO 3 q oxidation, which were represented as "daytime" and "nighttime" experiments, respectively.Specifically, four different systems of VOC and oxidation conditions were studied: αpinene + OH q , β-pinene + OH q , α-pinene + NO 3 q , and βpinene + NO 3 q .In order to infer the hydrolysis process, experiments were performed under low-RH (relative humidity; i.e., ∼ 5 %) or high-RH (i.e., ∼ 50 %-70 %) conditions and with effloresced or deliquesced seed particles for the same initial concentrations of precursor VOC and oxidant precursors.Temperature in the reactors was kept at room temperature (22-25 • C).Experimental conditions are summarized in Table 1.
Prior to every experiment, the reactor was flushed with zero air (Aadco, for at least a day.A typical experiment began with the injection of seed aerosol into the reactor by atomizing dilute ammonium sulfate (AS; 0.015 M) or sulfuric acid + magnesium sulfate (SA + MS; 0.01 + 0.005 M) aqueous solution.The seed aerosol was either directly atomized into the reactor or passed through a dryer before entering the reactor.The difference between efflorescence RH (∼ 35 %) and deliquescence RH (∼ 80 %) for AS aerosol is fairly large (Seinfeld and Pandis, 2016).Taking advantage of this property, it is possible to vary the amount of water in aerosol under the same RH in the reactor.Initial seed number and volume concentrations upon atomization for 20 min were approximately 2 × 10 4 cm −3 and 2 × 10 10 nm 3 cm −3 , respectively.A known amount of precursor VOC in the liquid form was transferred into a glass bulb, which was then evaporated and carried into the reactor by flowing zero air at 5 L min −1 through the bulb.Although the measurement of the precursor VOC concentration was not available for all experiments, the target and measured concentrations in the experiments when the measurements were available were consistent.For daytime experiments, an oxidant precursor (i.e., H 2 O 2 ) was introduced to the reactor in the same manner as VOC except that the glass bulb was gently heated by a heat gun to help evaporate faster.During the injection of H 2 O 2 , a desired amount of NO was introduced into the reactor from a cylinder containing 500 ppm of NO (Matheson).For Exps. 3-5, 5 ppm of NO at 5 L min −1 was continuously injected to the reactor until the SOA growth ceased.For Exps. 1, 2, 6, and 7, 15 ppm of NO at 5 L min −1 was injected for 5-20 min several times until the SOA growth ceased.The NO concentration was usually on the order of tens of ppb and always remained above a few ppb, making the bimolecular reaction with NO a favorable RO 2 q reaction pathway.The experiment was initiated by turning on the irradiation of UV light approximately 20 min after the end of the last injection to ensure that particles and vapors were mixed well inside the reactor.
The procedure for nighttime experiments was the same until the end of the precursor VOC injection.An oxidant precursor (i.e., N 2 O 5 ) was pre-made in a flow tube by simultaneously injecting 500 ppm of NO 2 (Matheson) at 0.4 L min −1 and ∼ 250 ppm of O 3 (Jelight 610) at 0.5 L min −1 .A simple kinetic box model was used to adjust the concentration of O 3 and flow rates of both NO 2 and O 3 to maximize the production of N 2 O 5 and minimize the concentration of O 3 , such that the VOC was dominantly oxidized by NO 3 q .Once N 2 O 5 entered the reactor, it thermally decomposed to generate NO 2 and NO 3 q .VOC was usually depleted within the first 15 min of the experiment.For Exps. 8 and 14, the injection order of precursor VOC and oxidant precursor was switched such that the injection of VOC marked the beginning of the experiment.For Exps. 12 and 13, 25 ppm of formaldehyde was added to the reactor to enhance the branching ratio of RO 2 q + HO 2 q (Schwantes et al., 2015;Boyd et al., 2015) by injecting an appropriate amount of formalin solution (37 % HCHO, Sigma-Aldrich) in the same manner as the injection of H 2 O 2 .We do not discuss the details of the effect of the injection order nor the effects of the RO 2 q fate here as they had negligible impact on the results concerning hydrolysis.

Instrumentation and data analysis
A high-resolution time-of-flight aerosol mass spectrometer (HR-ToF-AMS; Aerodyne Research Inc.) measured the concentrations of non-refractory organics (Org), sulfate (SO 4 ), nitrate (NO 3 ), ammonium (NH 4 ), and chloride (Chl) (DeCarlo et al., 2006).The data were analyzed using PIKA v1.16I and the unity collection efficiency was applied to all datasets.For the majority of nitrate-containing aerosol regardless of the class (i.e., inorganic or organic), the nitrate moiety (i.e., -NO 2 , -ONO 2 , and -O 2 NO 2 ) was known to be thermally fragmented into NO + and NO + 2 and was measured as NO 3 (Farmer et al., 2010).As many past studies have demonstrated the feasibility to separate the contribution of inorganic (NO 3,Inorg ) and organic nitrate (NO 3,Org ) to the measured NO 3 based on the ratio of NO + and NO + 2 (Fry et al., 2009(Fry et al., , 2018;;Farmer et al., 2010;Xu et al., 2015b;Kiendler-Scharr et al., 2016), we used Eq.(1) presented in Farmer et al. (2010) to obtain NO 3,Org .R AN (i.e., NO + /NO + 2 from ammonium nitrate) was obtained from the routine ionization efficiency calibration of HR-ToF-AMS using 300 nm ammonium nitrate particles.The drawback of this method is that R ON (i.e., NO + /NO + 2 from organic nitrate aerosol) could vary depending on the chemical composition (Xu et al., 2015b).In addition, a non-negligible contribution of ammonium nitrate could be expected in experiments with deliquesced seed aerosol owing to high solubility of HNO 3 .Thus, we obtained the R ON measured in low-RH experiments for each system of VOC and oxidation condition.In order to account for changes in R AN over time, R ON was scaled accordingly assuming that the ratio of R ON to R AN in the same system was constant (Fry et al., 2013).R AN , R ON , and R ON /R AN values obtained in this study were consistent with previously reported values (Fry et al., 2009;Bruns et al., 2010;Boyd et al., 2015;Nah et al., 2016) and are summarized in Table S1 in the Supplement.
A Filter Inlet for Gases and AEROsols (FIGAERO) (Lopez-Hilfiker et al., 2014) coupled to a high-resolution time-of-flight iodide chemical ionization mass spectrometer (HR-ToF-I-CIMS; Aerodyne Research Inc.) detected a suite of gaseous and particulate oxidized organic species as well as selected inorganic species (Bertram et al., 2011;Lee et al., 2014).The operation of FIGAERO-HR-ToF-I-CIMS was detailed in the previous studies (Nah et al., 2016;Sanchez et al., 2016).Reagent ions were generated by flowing a mixture of CH 3 I and dry N 2 (Airgas) through a polonium-210 source (NRD; model P-2021).The instrument measured gaseous compounds by sampling air from the reactor at ∼ 1.7 L min −1 while collecting particles onto a Teflon filter.Upon completion of the collection period, collected particles were desorbed by temperature-programmed dry N 2 flow and subsequently analyzed by HR-ToF-I-CIMS.Sensitivity could decrease if the amount of reagent ions was significantly depleted and/or if the secondary chemistry in the ion-molecule reaction (IMR) chamber occurred at a significant degree (Lee et al., 2014).To avoid changes in sensitivity among experiments, gas-phase sampling flow was diluted with zero air immediately before the inlet such that the evaporation of aerosol was minimal.The amount of aerosol collected on the filter was also adjusted by varying the sampling rate from 1 to 6 L min −1 depending on the aerosol mass concentrations inside the reactor.Overall, the fraction of reagent ions to the total ions was kept above 80 %.In addition, iodide ion chemistry has been known to be affected by the water vapor pressure inside the IMR owing to the difference in thermodynamics between I − and IH 2 O − to analyte compounds (Lee et al., 2014).In order to minimize changes in the water vapor pressure inside the IMR, a small continuous flow of humidified N 2 (30-50 cm 3 ) through a bubbler at a reduced pressure was continuously added to the IMR directly.Therefore, while the instrument was not calibrated to report the concentration of detected species, it was possible to quantitatively compare the measured signal of each ion among experiments because the instrument was operated under configurations that prevented undesired changes in sensitivity.The data were analyzed using Tofware v2.5.11 and all the masses presented in this study were I − adducts.
A scanning mobility particle sizer (SMPS) that consisted of a differential mobility analyzer (TSI 3040) and a con-densation particle counter (TSI 3775) was operated under the low-flow mode with the sheath flow of 2 L min −1 to detect particles up to 1 µm in electrical mobility size.A cavity attenuated phase shift monitor (CAPS; Aerodyne Research Inc.) (Kebabian et al., 2005), an ultra-sensitive NO x analyzer (Teledyne M200EU), and an UV absorption O 3 analyzer (Teledyne T400) measured NO 2 , NO x , and O 3 , respectively.In selected experiments, a gas chromatograph coupled to a flame ionization detector (GC-FID; Agilent) was used to make sure that a desired amount of a precursor VOC was injected.Except the CAPS, NO x analyzer, and O 3 analyzer, all instruments had their own dedicated sampling line.

Chemical composition of secondary organic aerosol
Shown in Fig. 1 are the mass spectra of particle-phase species obtained from FIGAERO-HR-ToF-I-CIMS at peak SOA growth.Many of the major species detected in this study are previously reported using the same or different technique (Eddingsaas et al., 2012;Claflin and Ziemann, 2018;Boyd et al., 2015;Nah et al., 2016;Lee et al., 2016;Romonosky et al., 2017).Concerning the chemical composition of SOA from each system, a more distinct difference is observed between different oxidation conditions (i.e., OH q vs. NO 3 q oxidation) than between different precursor VOC (i.e., α-pinene vs. β-pinene).This is expected as α-pinene and β-pinene have the same chemical formula and very similar structures, while the oxidation conditions are distinctively different (Kroll and Seinfeld, 2008;Ziemann and Atkinson, 2012).
For daytime experiments where OH q are the dominant oxidants, the contribution of ON (i.e., C x H y N 1,2 O z ) and non-nitrated organics (i.e., C x H y O z ) are comparable and their contributions are well spread out over a wide range of masses.A large contribution of C x H y O z is expected because the formation of ON is a minor pathway in RO 2 q + NO (Perring et al., 2013).In Eddingsaas et al. (2012), the major compounds reported in the α-pinene + OH q system include C 8 H 12 O 4−6 and C 10 H 16 O 4,6 , which are also detected in our study.A suite of C 10 ON from the chamber experiment of the α-pinene + OH q system are reported in Lee et al. (2016) with the chemical formula of C 10 H 15,17,19 NO 4−9 .All of these masses are detected in this study, though we observe a considerable contribution of C <10 ON (i.e., C 7 H 9,11 NO 6 and C 9 H 13,15,17 NO 6 ) as well as a small fraction of C 10 dinitrate (i.e., C 10 H 14,16 N 2 O 9,10 ) that has been rarely reported (Fig. 1a).This significant contribution from species containing C <10 indicates the large contribution of fragmentation process that is a preferred pathway in high NO conditions (Kroll and Seinfeld, 2008;Ziemann and Atkinson, 2012;Perring et al., 2013).It is possible that these species with C <10 are thermally decomposed products during the ther- mal desorption process (Stark et al., 2017).However, it is unlikely that thermal decomposition plays a significant role for the SOA generated via OH q oxidation of monoterpenes because the desorption temperature for these compounds (i.e., peaking at ∼ 50-70 • C) is much lower than the temperature at which decarboxylization or dehydration reactions (> 120 • C) are expected to occur (Stark et al., 2017).SOA chemical composition of the β-pinene + OH q system is similar to that of the α-pinene + OH q system but with a larger contribution of C x H y O z .
Another interesting observation in the α-/β-pinene + OH q systems is that a selected class of compounds (i.e., C 10 H 13,15,17 NO 5−8 ) with the same H/C ratio exhibits the same time evolutions regardless of the number of oxygen (Fig. S1 in the Supplement).This observation is consistent with the autoxidation mechanism, in which highly oxidized molecules are formed in a short timescale (Ehn et al., 2014;Crounse et al., 2013;Jokinen et al., 2015).Based on FIGAERO-HR-ToF-I-CIMS data (Fig. S1), C 10 H 17 NO ≥6 peak at 75 min.This is comparable to the lifetime of α-pinene at 53 min in the same experiment, which is related to the characteristic time of OH oxidation.This suggests that the aforementioned ON species are likely formed via one OH oxidation reaction, which is consistent with the autoxidation scheme to generate C 10 H 17 NO ≥6 proposed in prior studies (Berndt et al., 2016;Xu et al., 2019;Pye et al., 2019).It is important to note that the concentration of NO in our experi-ments has been mostly kept on the order of tens of ppb over the course of the experiments by a continuous injection of dilute NO and, therefore, this result suggests that autoxidation is not a negligible pathway of RO 2 q fate even at a moderately high NO level in laboratory experiments and in polluted ambient environments.Indeed, recent studies (Berndt et al., 2016;Xu et al., 2019;Pye et al., 2019) suggest that the autoxidation rate constant for the α-pinene + OH q system could be up to a few per second, which is comparable to the NO level of ∼ 10 ppb, assuming a typical RO 2 q + NO reaction rate constant of 1 × 10 −11 cm 3 molecule −1 s −1 (Orlando and Tyndall, 2012).The autoxidation rate constant as well as the role of NO in autoxidation based on this observation will be discussed in detail in a forthcoming publication.
In contrast, the signals of C x H y N 1−2 O z are dominant in the NO 3 q oxidation condition, indicating that the production of ON is greatly favored over non-nitrated organics.This observation is consistent with a direct addition of a nitrate functional group to a double bond (Wayne et al., 1991;Ng et al., 2017), whereas the formation of ON in OH q oxidation condition is a minor channel of RO 2 q + NO reaction (Perring et al., 2013).Although this is generally true for many monoterpenes, the organic nitrate yield in α-pinene + NO 3 q has been known to be low (Fry et al., 2014) due to loss of a nitrate functional group followed by alkoxy radical bond scission (Kurten et al., 2017).Fry et al. (2014) observe no SOA formation in the same system, though another study has reported the formation of non-negligible SOA mass even at a relatively low initial concentration of α-pinene (Nah et al., 2016).Since the particle-phase compounds represent < 10 % of overall α-pinene + NO 3 q products by mass, it is not necessarily inconsistent to observe a higher abundance of ON than non-nitrated organics in the particle phase if low-volatility compounds mainly consist of ON.
Moreover, the contribution from species containing C <10 is minimal in the NO 3 q oxidation condition.Once NO 3 q attacks a double bond in the initial oxidation reaction, the majority of the reaction products no longer contain any double bond.Unlike OH q , a hydrogen abstraction reaction by NO 3 q is slower by orders of magnitude (Atkinson and Arey, 2003).Therefore, multigeneration oxidation is unlikely to occur within the timescale of experiments (Wayne et al., 1991;Ng et al., 2017).This means that once the precursor VOC undergoes functionalization upon the initial NO 3 q oxidation, it is not likely to experience fragmentation during the experiment.Unlike daytime SOA, the distribution of masses is dominated by a few signature ions, such as C 10 H 15 NO 5,6 and C 20 H 32 N 2 O 8−10 (Fig. 1c and 1d).In Boyd et al. (2015), Nah et al. (2016), and Lee et al. (2016), the major species reported in the α-/β-pinene + NO 3 q systems are monomeric nitrate aerosol (i.e., C 10 H 13,15,17,19 NO 4−10 ), while in this study a substantial contribution of dimeric species (i.e., C 20 H 32 N 2 O 8−11 ) is observed.The abundant presence of dimeric compounds has been previously observed in some studies on NO 3 q oxidation of α-/β-pinene (Romonosky et al., 2017;Claflin and Ziemann, 2018) and particle-phase reactions to produce such dimers have been proposed by Claflin and Ziemann (2018).Many of the reported species in Claflin and Ziemann (2018) except the trimeric species (mass scan range not extended to trimeric species in our study) are observed in our study.One major difference between Claflin and Ziemann (2018) and this study is the substantial presence of monomeric nitrate aerosol (i.e., 30 %-60 % by signal) in this study.This difference may be attributed to the difference in the amount of available monomeric blocks to form dimer species.Assuming a reversible dimerization process, the concentration of dimer species shall be proportional to the square of monomer concentration, such that the monomer-to-dimer ratio increases in a quadratic manner as the available monomer concentration decreases.Since the amount of SOA formed in Claflin and Ziemann (2018) is approximately 2 orders of magnitude higher than that in this study, the concentration of monomers in the particle phase is higher, favoring a more efficient formation of dimeric species.Together, these results suggest that the contribution of dimeric nitrate aerosol could vary greatly depending on the concentrations of monomeric blocks at the specific time and location.
Previous field studies have reported the mass spectra of ambient C 10 p ON obtained by FIGAERO-HR-ToF-I-CIMS in a rural Alabama site during the Southern Oxidant and Aerosol Study (SOAS) (Lee et al., 2016) and in a rural forest in Germany (Zhang et al., 2018).A comparison of the ambient mass spectra with those obtained in this study reveals that average ambient p ON resembles daytime p ON more than nighttime p ON (Fig. S2).p ON from daytime experiments has a distribution of masses centered around C 10 H 13,15,17 NO 7 , which is consistent with the ambient measurement data.On the other hand, NO 3 q oxidation does not seem to oxidize organic species enough such that the distribution of masses would be skewed towards a less-oxidized region (i.e., C 10 H 13,15,17 NO 5−6 ).However, it is difficult to draw a quantitative conclusion simply based on this comparison because O 3 , another important oxidant at night, is not studied.Moreover, an average lifetime of aerosol could extend up to a week and thus ambient aerosol is continuously exposed to further oxidation while the experiments here are more applicable to freshly formed aerosol.In addition, the use of C 10 p ON alone may not be a good representative of monoterpenederived p ON as 42 %-74 % of p ON in this study contains fewer or more than 10 carbon atoms (Table S2).Nonetheless, the chemical composition of aerosol generated in this study is comparable to those in the atmosphere and thus the results shall be directly applicable to relevant ambient conditions.

Proxy used to evaluate hydrolysis process
Various proxies using HR-ToF-AMS data have been used to infer ON hydrolysis in previous studies.In Bean and Hildebrandt Ruiz (2016), NO 3 measured by an aerosol chemical speciation monitor (ACSM, practically similar to how AMS operates and measures aerosol species) (Ng et al., 2011) is normalized to SO 4 as a means to account for particle wall loss and is fitted by an exponential function to estimate the ON hydrolysis rate.On the other hand, Boyd et al. (2015) normalize NO 3 measured by HR-ToF-AMS to Org and attribute the relative decay of NO 3 /Org between humid (RH ∼ 50 %) to dry (RH < 5 %) conditions to hydrolysis.Other approaches include the SMPS-derived particle wall-loss correction of NO 3 measured by HR-ToF-AMS followed by fitting its decay trend (Liu et al., 2012) and the determination of the fraction of total (i.e., gas and particle) ON to the precursor VOC consumed as a function of RH using Fourier-transform infrared spectroscopy (FTIR).Below, we systematically examine the use of different proxies using HR-ToF-AMS data to infer hydrolysis and discuss how the corresponding results are interpreted.
Figure 2 shows the time series of Org, NO 3 , SO 4 , and NH 4 measured by HR-ToF-AMS for the α-pinene + NO 3 q system.There is a substantial difference in NO 3 for the same VOC system but under different reactor RH and phase state of seed particles (Exps.10 and 11), while Org and SO 4 concentrations are similar.The spike in NO 3 in the high-RH wetseed experiment (Fig. 2b) is attributed to the uptake of N 2 O 5 and/or dissolution of HNO 3 into aqueous aerosol followed by neutralization with ammonia to produce ammonium nitrate.This is consistent with the sharp increase in molar ratio of NH 4 /SO 4 to higher than 2, which is the theoretical value for AS particles.It is also possible that inorganic nitrate is generated via hydrolysis of gaseous ON that is too volatile to condense but is soluble enough to dissolve in aqueous aerosol and thus only appears in high-RH experiments.Since we do not have a way to quantitatively differentiate the contribution of the aforementioned sources, the focus of this study is on hydrolysis of p ON that partitions to the aerosol due to condensation rather than dissolution.However, further study is required to investigate the hydrolysis of volatile yet soluble gaseous ON, and the approach must be different from the comparison between low-and high-RH experiments to obtain meaningful results.
To evaluate the extent of p ON hydrolysis, the contributions of inorganic nitrate (NO 3,Inorg ) and organic nitrate (NO 3,Org ) to the measured NO 3 need to be calculated.Firstly, NO 3,Org is estimated by subtracting NO 3 associated with excess NH 4 .Secondly, NO 3,Org is derived from NO + /NO + Exp. 5 (high RH, wet AS).These mass concentrations of aerosol water translate to 0, 6, and 36 mol L −1 , respectively, under the assumption that SOA is miscible with liquid water.It is speculated that SOA formed in Exps.3-5 are miscible with water because (1) the measured O/C ratio in HR-ToF-AMS (Canagaratna et al., 2015) is close to 0.7, which is near the lower end but above the liquid-liquid phase separation condition (Song et al., 2012) and ( 2) there is evidence of aqueous-phase reactions which highly depend on the availability of aerosol water, as discussed in Sect.3.3.Thus, the decay rate of NO 3,Org normalized to SO 4 and/or Org between Exp. 4 and Exp. 5 shall differ by a factor of 6 based on the molar concentrations of aerosol water.
Figure 3a shows the mass ratio of NO 3,Org /SO 4 and the decay rate as a characteristic time in Exps.3-5.The characteristic times of Exps. 4 and 5 (4.4 vs. 4.0 h) do not differ regardless of the molar concentrations of aerosol water, suggesting that the decreasing trend in NO 3,Org /SO 4 may not be due to changes in aerosol water content and p ON hydrolysis, but arise from the difference in the reactor humidity alone.A comparison of NO 3,Org /SO 4 and NO 3,Org /Org also reveals that these two proxies capture a different range of decay mechanisms.Figure 3b shows the relative decay trend of NO 3,Org /SO 4 and NO 3,Org /Org between Exp. 4 (high RH) and Exp. 3 (low RH).If hydrolysis is a dominant decay mechanism of p ON, the trend of NO 3,Org /Org would be identical to that of NO 3,Org /SO 4 .This is because the organic moiety of hydrolysis product is generally considered to have a substituted alcohol group (Boschan et al., 1955) and to have a relatively similar vapor pressure and shall remain in the particle phase (Pankow and Asher, 2008).Similar to this is the formation of organic sulfate from hydrolysis of p ON (Liggio andLi, 2006, 2008;Surratt et al., 2008), which has sufficiently low volatility to remain in the particle phase as with alcohol-substituted products.However, the measured decay trend of the two proxies is greatly different.It is possible that some organic moiety of hydrolysis product could be significantly more volatile and repartition back to the gas phase (Rindelaub et al., 2016;Bean and Hildebrandt Ruiz, 2016) and thus both organics and HNO 3 formed from hydrolysis evaporate.In this case, not only NO 3,Org but also some fraction of Org would decrease because Org measured by HR-ToF-AMS includes the contribution from the organic part of p ON.This will lead to the relatively smaller decrease in NO 3,Org /Org compared to NO 3,Org /SO 4 .We can reconstruct the decay rate of NO 3,Org /Org assuming (1) the decay rate of NO 3,Org /SO 4 is solely due to hydrolysis of p ON and (2) the maximum contribution of p ON to organic aerosol (OA) is 35 % (see Fig. 4 and discussions below).The reconstructed decay rate of NO 3,Org /Org is shown in Fig. 3b.As observed in the figure, the decay rate of the reconstructed NO 3,Org /Org is much larger than the measured NO 3,Org /Org.This suggests that hydrolysis is not the only loss process reflected in the decreasing trend of NO 3,Org /SO 4 , while NO 3,Org /Org is likely a better proxy that isolates hydrolysis from other loss processes.The likely important loss process manifested in NO 3,Org /SO 4 is the loss of organic vapors to the walls of the reactor (Matsunaga and Ziemann, 2010;Krechmer et al., 2016;Huang et al., 2018;Loza et al., 2010;Mcvay et al., 2014;Zhang et al., 2015Zhang et al., , 2014;;La et al., 2016).For example, Huang et al. (2018) observe that the decay of isoprene hydroxy nitrate depends on the reactor humidity.While SO 4 is practically nonvolatile in the experimental condition of this study, both ON and non-nitrated organics could have some fractions of semi-volatile species whose vapors are subject to wall loss.Assuming a uniform loss rate of ON and non-nitrated organic vapors to the reactor walls, the effect of vapor wall loss could be effectively canceled out in NO 3,Org /Org, but not in NO 3,Org /SO 4 .This assumption is likely reasonable because the vapor wall-loss rate is a func-tion of saturation mass concentration (Zhang et al., 2015) and the average saturation mass concentrations of bulk ON and non-nitrated organic aerosol are similar based on the thermal desorption profiles in FIGAERO-HR-ToF-I-CIMS (Fig. S5).Therefore, NO 3,Org /Org is a better proxy to infer hydrolysis of p ON than others.

Hydrolysis lifetime of particulate organic nitrate
In order for the data to be easily comparable with those reported in models or using other techniques, the use of general terms instead of the AMS-specific terms (i.e., NO 3,Org and Org) can be convenient.We define p ON as the total mass concentration of particulate organic nitrate (includes the organics part and nitrate part of the ON compounds) and OA as the total mass concentration of organic aerosol (includes nitrate and non-nitrated organics).The inclusion of nitrate mass concentration in OA is important as the contribution of nitrate functional groups to the total organic aerosol mass concentration is large.The conversion method from NO 3,Org /Org into p ON/OA is illustrated in Eq. ( 1).
MW p ON represents the average molecular weight of p ON per nitrate functional group estimated from FIGAERO-HR-ToF-I-CIMS data assuming a uniform sensitivity among detected species, and MW NO 3 indicates the molecular weight of nitrate (i.e., 62 g mol −1 ).Since MW p ON does not significantly vary during the course of experiments (i.e., relative standard deviation of < 1.2 %), the average value is applied to each experiment.The variability in MW p ON among different systems is also found to be small, ranging from 229 to 238 g mol −1 and thus an average MW p ON is used for experiments where FIGAERO-HR-ToF-I-CIMS data are not available.Figure 4 shows the time series data of p ON/OA for all the systems investigated in this study.
For nighttime experiments, the relative ratio of C x H y N 1−2 O z and C x H y O z obtained from FIGAERO-HR-ToF-I-CIMS data in Fig. 1 does not appear to match well with p ON/OA from HR-ToF-AMS data.For example, the signals are dominated by C x H y N 1−2 O z in the βpinene + NO 3 q system, as shown in Fig. 1d, while p ON/OA is at most 0.5, as shown in Fig. 4d.The discrepancy would be attributed to the overestimation of Org (in particular, C x H y family) in HR-ToF-AMS and/or underestimation of C x H y O z in FIGAERO-HR-ToF-I-CIMS.The relative ionization efficiency (RIE) of less-oxidized organic species in HR-ToF-AMS is experimentally measured to be higher at least by a factor of 2 (W.Xu et al., 2018).As previously reported (Boyd et al., 2015), the HR-ToF-AMS mass spectrum of SOA formed from β-pinene + NO 3 q contains significant amounts of C x H y fragments, indicating the less-oxidized nature of SOA from β-pinene + NO 3 q .For example, if the true RIE of Org by β-pinene + NO 3 q SOA were to be a factor of 2 higher than the default RIE of Org (i.e., 1.4), the reported concentration of Org would have been overestimated by a factor of 2, such that the actual p ON/OA would have been higher than reported in Fig. 4d.On the other hand, an iodide reagent ion is not quite selective enough to detect less-oxidized species, which could overestimate the contribution of p ON to OA (Aljawhary et al., 2013).Nonetheless, this discrepancy between HR-ToF-AMS and FIGAERO-HR-ToF-I-CIMS data, however, should not affect the results regarding the hydrolysis lifetime and hydrolyzable fraction of p ON presented later.
As illustrated in Fig. 4, the time series of p ON/OA stabilizes fairly quickly in most of the experiments, regardless of RH and/or the phase state of seed aerosol, supporting the appropriateness of the reconstructive approach shown in Fig. 3b.This suggests that the timescale of p ON hydrolysis in the systems studied is significantly shorter or longer than the timescale of our experiments.It is also evident from Fig. 4 that p ON/OA in high-RH experiments are always lower than that in low-RH experiments.These two observations imply that the rate of p ON hydrolysis may be fast enough such that the decay trend of p ON compared to OA is not visibly manifested, though a clear difference of p ON/OA between lowand high-RH experiments is exhibited as a result of fast hydrolysis.Since no sudden, drastic change in p ON/OA is observed except for a few initial data points, we conclude that the hydrolysis lifetime of hydrolyzable p ON for α-/β-pinenederived ON shall be no more than 30 min (i.e., third data point in Fig. 4).Particle acidity is found to enhance hydrolysis rate of α-pinene hydroxy nitrate (Rindelaub et al., 2016), though no clear difference is observed here between experiments with AS and SA + MS seed particles (i.e., Exps. 5 and 2).It is worth noting that aqueous AS particles are not neutral but slightly acidic due to partitioning of ammonium to the gas phase once the particles enter the chamber (Gao et al., 2004).In Gao et al. (2004), the reported pH of aqueous AS particles is 4.6 and we expect a similar pH in our study.In Rindelaub et al. (2016), the reported hydrolysis lifetime is short at 1.3 h at a pH of 4.0.On the other hand, previous studies have shown that isoprene-derived hydroxy nitrates do not require low pH to undergo fast hydrolysis (Darer et al., 2011;Hu et al., 2011).Thus, p ON formed from OH q and NO 3 q oxidation of α-pinene and β-pinene may not require a low pH to undergo hydrolysis at a rate comparable to the timescale of chamber experiments.
Comparing with the results from past chamber studies reporting a p ON hydrolysis lifetime of 3 to 6 h (Liu et al., 2012;Bean and Hildebrandt Ruiz, 2016;Boyd et al., 2015), our estimated hydrolysis lifetime is substantially shorter, but is consistent with the range (i.e., 1 min to 8.8 h) reported in studies using the bulk solution method (Darer et al., 2011;Figure 4. Time series data of p ON/OA in (a) α-pinene + OH q from Exps.1-5, (b) β-pinene + OH q from Exps.6-7, (c) α-pinene + NO 3 q from Exps.8-13, and (d) β-pinene + NO 3 q from Exps.14-15.Data points are colored by conditions concerning reactor RH and phase state of seed aerosol.For α-pinene + NO 3 q , data points are also shaped differently depending on the expected dominant RO 2 q fate.Hu et al., 2011;Jacobs et al., 2014;Rindelaub et al., 2016) (Fig. 5).In Liu et al. (2012) and Bean and Hildebrandt Ruiz (2016), the hydrolysis lifetime is derived from the decay rate of NO 3 corrected for the particle wall loss or normalized to SO 4 .As demonstrated in Sect.3.2.1, this NO 3 /SO 4 decay rate is likely affected by other loss processes, such as vapor wall loss, and thus is not a good proxy to estimate the hydrolysis lifetime.The apparent discrepancy does not stem from the contradiction in the obtained data itself but rather in the data interpretation.Indeed, the lifetime estimated based on the decay of NO 3,Org /SO 4 in our study is 4 h (Fig. 3a), which is consistent with 6 and 3 h reported in Liu et al. (2012) and Bean and Hildebrandt Ruiz (2016).On the other hand, in Boyd et al. (2015) the hydrolysis lifetime is estimated based on the decay rate of NO 3 /Org.The discrepancy in the reported hydrolysis lifetime here could be attributed to the fact that NO 3 is not separated into NO 3,Org and NO 3,Inorg .Figure S6 shows our data analyzed in the same manner as Boyd et al. (2015).The lifetime calculated based on the decay is 2.2 h, which is close to the reported 3-4.5 h (Boyd et al., 2015).The reduction of NO 3 /Org in Fig. S6 (∼ 30 %) is greater than in Boyd et al. (2015) (10 %), which could be be-cause (1) the amount of N 2 O 5 , a source of inorganic nitrate, used in our study is slightly larger and (2) RH in our study is higher by 10 %-20 %, which may have allowed for greater uptake of N 2 O 5 to produce inorganic nitrate due to changes in aerosol viscosity (Gržinić et al., 2015).
In previous bulk solution studies where the concentration of interested organic nitrate (in particular hydroxy nitrate) in aqueous solution rather than in aerosol water is monitored over time, it is unlikely that the data interpretation is affected by other loss processes present in chamber experiments, such as vapor wall loss.It is also common to monitor the organic moiety of hydrolysis product (Darer et al., 2011), while it is extremely difficult in chamber experiments where hundreds of organic species are present at the same time, leading to the difficulty in accurately measuring the hydrolysis lifetime in chamber experiments.Based on the comprehensive analysis we demonstrate above on evaluating p ON hydrolysis in chamber experiments, we recommend the use of the hydrolysis lifetime reported in this study, which is no more than 30 min, for p ON formed from α-pinene and β-pinene.Comparison of hydrolysis lifetime of organic nitrate and hydrolyzable fraction of p ON in literature."Chamber" refers to laboratory studies of organic nitrate aerosol via chamber experiments, "Bulk" refers to laboratory studies of organic nitrate compounds using bulk solution measurements, and "model" refers to modeling studies using ambient measurement data as constraints.Data points are colored by the system of VOC and oxidant condition and are alphabetized based on the reference.The relevant systems explored in this study are emphasized by enlarging the corresponding font size.Pink shaded regions are ranges reported in literature, while blue shaded regions are ranges reported in this study.

Hydrolyzable fraction of particulate organic nitrate
The fraction of hydrolyzable p ON (F H ) can be directly estimated from the difference in p ON/OA between low-and high-RH experiments shown in Fig. 4.Although we show that hydrolysis is substantially faster than the timescale of chamber experiments in our study, there still appears to be a clear difference in p ON/OA between high-RH experiments but with a different phase state of seed aerosol (i.e., Exps. 4 and 5).The difference in mass spectra among Exps.3-5 obtained from FIGAERO-HR-ToF-I-CIMS reveal that the difference in p ON/OA between Exps. 4 and 5 does not arise from the reduction in p ON but from the increase in nonnitrated organics (Fig. 6).The reason for this OA increase with the abundant presence of aerosol water is speculated to be uptake and other aqueous-phase reactions than hydrolysis and is briefly discussed in Sect.3.3.Thus, the absolute difference in p ON/OA between low RH with dry seed and high RH with dry seed experiments best indicates F H . Depending on the fate of the organic moiety of the hydrolysis product (i.e., stay in the particle phase or repartition back to the gas phase), F H varies. Since we are unable to determine the fate of hydrolysis product, an upper and lower limit of F H are reported as a range of F H .For the α-pinene+OH q system, 23 %-32 % of p ON formed undergoes hydrolysis within the timescale of the experiments.For the other systems with no experiment under high RH with dry seed aerosol, the same level of additional contribution from non-nitrated organics encoun- < 30 min 27 %-34 % α-pinene + NO 3 q < 30 min 9 %-17 % β-pinene + NO 3 q < 30 min 9 %-15 % a Lower or higher limit of hydrolyzable p ON fraction is based on the assumptions that organic moiety of hydrolysis products remains in aerosol or partitions back to the gas phase.
tered in α-pinene + OH q system is assumed and F H is scaled accordingly.For the β-pinene + OH q , α-pinene + NO 3 q , and β-pinene + NO 3 q systems, 27 %-34 %, 9 %-17 %, and 9 %-15 %, respectively, of p ON are found hydrolyzable within the timescale of the experiments.Table 2 summarizes the hydrolysis lifetime and F H in the systems explored in this study.F H has been only reported in a few studies (Liu et al., 2012;Boyd et al., 2015;Zare et al., 2018).The determination of F H is essential because the assumption that all p ON hydrolyzes biases the relative importance of hydrolysis among the loss mechanisms of p ON and NO x .Boyd et al. (2015) report that F H of p ON formed via β-pinene + NO 3 q is ∼ 10 %, which is in a good agreement with our range of 9 %-15 %.Based on the proposed molecular structures of p ON from Claflin and Ziemann (2018), < 5 % of p ON from β-pinene + NO 3 q is tertiary and thus hydrolyzable.In our study, a considerable contribution of monomeric (C 10 ) p ON is observed (Fig. 1d), while dimeric (C 20 ) p ON is dominant in Claflin and Ziemann (2018).This may indicate that monomeric p ON is more susceptible to hydrolysis such that F H in this study is slightly higher than expected based on the proposed molecular structures of p ON in Claflin and Ziemann (2018).
F H for α-/β-pinene + OH q systems are higher than those from α-/β-pinene + NO 3 q systems.This trend is consistent with the understanding that p ON via OH q oxidation have a larger fraction of tertiary nitrate groups, which are significantly more susceptible to hydrolysis (Darer et al., 2011;Hu et al., 2011) than those formed via NO 3 q oxidation (Ng et al., 2017).Although the relative trend of F H between α-/β-pinene + OH q and α-/β-pinene + NO 3 q systems is consistent, the magnitude of F H in the α-/β-pinene + OH q system appears to be smaller than expected based on the tertiary nitrate fraction estimated via the explicit gas-phase chemical mechanism (Browne et al., 2013;Zare et al., 2018).In previous studies, F H is estimated to be 62 % and 92 % for α-/β-pinene + OH q systems, respectively.However, our results indicate F H is 23 %-32 % and 27 %-34 % for the same systems (Fig. 5).The chemical mechanism used in Browne et al. (2013) and Zare et al. ( 2018) is based on the Master Chemical Mechanism (MCM) that is well known in the degradation chemistry of VOC in the gas phase (Jenkin et al., 1997;Saunders et al., 2003).However, the same mechanism performs poorly in regards to the chemical composition of SOA (Faxon et al., 2018) as well as the prediction of SOA formation (Ruggeri et al., 2016;Boyd et al., 2017) when equipped with gas-particle partitioning modules based on the absorptive gas-particle partitioning theory (Pankow, 1994).It is, therefore, reasonable to argue that the chemical composition of p ON could greatly differ from that of total ON predicted by the MCM.Thus, F H reported in this study provides the fundamental experimental constraints on p ON hydrolysis that can be used in regional and global models for elucidating potential impacts of ON on nitrogen budget and formation of ozone and aerosol.

Signature of other aqueous-phase reactions besides hydrolysis
As briefly discussed in the above section, the presence of elevated levels of aerosol water seems to have enhanced the contribution of small (i.e., C <9 ) but more-oxidized organic species to SOA.As shown in Fig. 5c Aljawhary et al. (2016).The reason for this less-oxidized nature of SOA in this study may be attributed to our experiments being performed in moderately high NO conditions that promote a higher contribution of a carbonyl group than a hydroperoxyl group, which is preferred in low-NO conditions.In Aljawhary et al. (2016), the starting compound is a product in low-NO conditions (pinonic acid, C 10 H 16 O 3 ).Thus, it is reasonable that products of the aqueous processing in this study are slightly less oxidized than observed in Aljawhary et al. (2016).
The enhancement of non-nitrated organic aerosol in FIGAERO-HR-ToF-I-CIMS may be due to aqueous processing of species in the particles in the presence of aerosol water.This can come from further reactions of semi-volatile and/or low-volatility species in the particle phase, or reactive uptake of volatile (but highly water soluble) species into the aerosol followed by subsequent aqueous-phase reactions to form low-volatility products (Ervens et al., 2011).A comparison of the average thermogram at peak SOA growth among Exps.3-5 indicates a higher contribution of low-volatility compounds in Exp. 5 than in Exps. 3 and 4, as illustrated by the bimodal peaks (Fig. S7).Given the same degree of gas-phase oxidation expected among Exps.3-5, these results show that aqueous chemistry in wet aerosol contributes to Atmos.Chem. Phys., 19, 12749-12766, 2019 www.atmos-chem-phys.net/19/12749/2019/ the further formation of low-volatility compounds.Overall, the highest average degree of oxidation (O/C = 0.77) is observed in the high-RH wet-aerosol experiment (Exp.5).The effect of particle water on monoterpene SOA formation warrants further studies.

Atmospheric implications
There is emerging evidence that monoterpene SOA greatly contributes to atmospheric aerosol in the Southeastern US (Zhang et al., 2018;L. Xu et al., 2018).ON is no exception; a substantial fraction of p ON is considered to be from monoterpenes (Lee et al., 2016;Huang et al., 2019;Xu et al., 2015a).While C 10 p ON measured in FIGAERO-HR-ToF-I-CIMS is a good tracer of monoterpene-derived p ON, we show that a fair amount of α-/β-pinene p ON is found as C <10 or C 20 depending on the oxidation condition.This implies that the contribution of monoterpene-derived p ON could be substantially underestimated when only considering C 10 p ON.The fraction of p ON with different number of carbon atoms reported in this study (Table S2) is a useful parameter to quantitatively determine the contribution of monoterpene-derived p ON to total p ON.Many previous modeling studies using ambient measurement data as constraints report that the lifetime of p ON is likely several hours (Pye et al., 2015;Fisher et al., 2016;Lee et al., 2016;Zare et al., 2018).Hydrolysis of p ON is used as a dominant loss process with the lifetime of several hours to improve the concentration of modeled OA (Pye et al., 2015) and to improve the concentrations of gaseous and particulate ON (Fisher et al., 2016).If the ambient p ON concentration is indeed governed by a loss process with a few hours of lifetime, our results imply that the particle-phase hydrolysis may not be the only dominant loss process because the hydrolysis lifetime reported in this study is significantly shorter.Other potential but less-studied loss mechanisms of ON and p ON include deposition (Nguyen et al., 2015), photolysis (Müller et al., 2014), and aqueous photooxidation (Romonosky et al., 2017;Nah et al., 2016).For instance, an enhanced photolysis rate is observed for carbonyl nitrate derived from isoprene (Müller et al., 2014), while no similar study is available for monoterpene-derived ON in literature.Also, it has been demonstrated that different monoterpene p ON can have drastically different photochemical fates (Nah et al., 2016).Taken together, results from this study highlight the importance to investigate other potential loss processes of monoterpenederived p ON.
Aside from the hydrolysis lifetime, many modeling studies assume F H as unity (Pye et al., 2015;Fisher et al., 2016;Lee et al., 2016).Even when F H is considered, the value of F H used in other studies is still substantially higher than estimated in this study (Browne et al., 2013;Zare et al., 2018).The use of higher F H would result in overestimating the contribution of hydrolysis as a loss process of p ON and NO x .While hydrolysis is considered a permanent sink of NO x , many other loss processes, such as further OH q oxidation and photolysis, are considered a temporary reservoir of NO x .If the relative importance of p ON fates in models was not accurate, the role of ON in NO x cycling and the formation potential of ozone could have been inaccurately interpreted.Therefore, results from this study regarding the hydrolysis lifetime and F H serve as experimentally constrained parameters for chemical transport models to accurately evaluate the role of ON in regards to nitrogen budget and the formation of ozone and fine aerosol.

Figure 1 .
Figure 1.FIGAERO-HR-ToF-I-CIMS mass spectra of SOA in (a) α-pinene + OH q from Exp. 3, (b) β-pinene + OH q from Exp. 6, (c) α- pinene + NO 3 q from Exp. 10, and (d) β-pinene + NO 3 q from Exp. 14. Top portion of each panel represents C x H y N 1−2 O z , whereas bottom represents C x H y O z .Bars are colored by the number of carbon atoms as noted in the legend.Prominent masses are labeled with the corresponding chemical formulae without an iodide ion.

Figure 2 .
Figure 2. (a, b) NO 3 concentration and the molar ratio of NH 4 to SO 4 and (c, d) concentrations of Org, SO 4 , and NH 4 measured by HR-ToF-AMS.Data presented in panels (a) and (c) are from Exp. 10 (low RH, dry AS), while those in panels (b) and (d) are from Exp. 11 (high RH, wet AS).These two experiments are essentially the same except for RH and phase state of seed aerosol.

Figure 3 .
Figure 3. (a) Time series data of NO 3,Org /SO 4 from Exps.3-5 (α-pinene + OH q ) and the exponential fits with corresponding characteristic times.(b) NO 3,Org /Org, NO 3,Org /SO 4 , and reconstructed NO 3,Org /Org based on the decay rate of NO 3,Org /SO 4 .Each proxy in Exp. 4 is divided by that in Exp. 3 to determine the relative decay between high-and low-RH experiments.

Figure
Figure5.Comparison of hydrolysis lifetime of organic nitrate and hydrolyzable fraction of p ON in literature."Chamber" refers to laboratory studies of organic nitrate aerosol via chamber experiments, "Bulk" refers to laboratory studies of organic nitrate compounds using bulk solution measurements, and "model" refers to modeling studies using ambient measurement data as constraints.Data points are colored by the system of VOC and oxidant condition and are alphabetized based on the reference.The relevant systems explored in this study are emphasized by enlarging the corresponding font size.Pink shaded regions are ranges reported in literature, while blue shaded regions are ranges reported in this study.

Figure 6 .
Figure 6.FIGAERO-HR-ToF-I-CIMS difference mass spectra of SOA in α-pinene + OH q .(a) Exp. 4 (high RH, dry AS) minus Exp. 3 (low RH, dry AS).(b) Exp. 5 (high RH, wet AS) minus Exp. 3 (low RH, dry AS).(c) Exp. 5 (high RH, wet AS) minus Exp. 4 (high RH, dry AS).Bars are colored by the difference in chemical composition (i.e., red for C x H y O z and blue for C x H y N 1−2 O z ).Prominent masses are labeled with the corresponding chemical formulae without an iodide ion.

Table 1 .
Summary of experimental conditions considered in this study.
a The target for the initial reactor RH is ∼ 70 %.However, the irradiation of UV light increases the reactor temperature by several degrees Celsius and hence decreases RH. b Ammonium sulfate c Sulfuric acid and magnesium sulfate

Table 2 .
Hydrolysis lifetime and corresponding fraction of hydrolyzable p ON.
, the enhancement is observed for a variety of non-nitrated organic aerosol including C 4 H 6,8 O 3 , C 4 H 4 O 4 , C 5 H 6 O 5 , C 7 H 8,10 O 4 , and C 8 H 8,10 O 4,5 , while p ON overall neither increase nor decrease.C 5 H 6 O 5 has been reported as a product of the aqueous-phase reaction of α-pinene-derived compounds (Aljawhary et al., 2016).Other compounds, such as C 4 H 4 O 4 , C 7 H 8,10 O 4 , and C 8 H 10 O 5 ,