Solubility of oxalic, malonic, succinic, adipic, maleic, malic, citric, and tartaric acids in water from 278.15 to 338.15 K

Apelblat, Alexander; Manzurola, Emanuel

doi:10.1016/0021-9614(87)90139-x

Cited by 236 publications

(235 citation statements)

References 11 publications

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“…Their vapor pressures as shown in Fig. 12 are however very close to those of the solution saturated with respect to the dihydrate, calculated from the supercooled melt vapor pressures and the solubility of the oxalic acid dihydrate (Apelblat and Manzurola, 1987). Bradley and Cotson (1953) (solid) 311-325 Kruif et al (1975) (solid) 303-328 1.10×10 −2 (α-form) de Wit et al (1983) (Marcolli et al, 2004) were used for interpolating/extrapolating the vapor pressure of the measured aqueous solutions to those of the saturated solution, using the measured activities.…”

Section: Oxalic Acidsupporting

confidence: 57%

“…This is an indication that both may have measured the supercooled melt instead of the crystalline solid, as was first speculated by Zardini et al (2006) and later supported by Koponen et al (2007) and Riipinen et al (2007). If we calculate the vapor pressure of the saturated solution from the vapor pressures of the aqueous solutions, using solubility, x sat (298.15 K)=0.215 (Marcolli et al, 2004) and its temperature dependence (Apelblat and Manzurola, 1987) as well as the activity coefficients of UNIFAC-Peng, the resulting vapor pressures agree within error with the measured pressure of the solid (see Fig. 7), proving the consistency of our measurements of aqueous solutions and the solids.…”

Section: Malonic Acidmentioning

confidence: 73%

“…9). Comparing these vapor pressures with the one of the saturated solution, p sat,L (298.5 K)=(1.3±0.6)×10 −5 Pa, calculated from solubility, x sat (298.15 K)=0.014 (Apelblat and Manzurola, 1987), the corresponding UNIFAC-Peng activity, a (x),sat =0.01, and the pressure of the supercooled melt, p •,L (298.5 K)=(1.3±0.4)×10 −3 Pa, shows that the lower vapor pressure agrees within error with those of the saturated solution, which proves that it takes a significant time to evaporate material (solvent inclusions and defective crystal structures) that has not crystallized to the thermodynamically stable crystalline solid. It is interesting to note that in contrast to solid glutaric acid particles, evaporating solid succinic acid particles showed sudden changes in the optical resonances spectra (Zardini et al, 2009(Zardini et al, , 2010, which we interpreted as rearrangements within the particle upon evaporation, but could also be connected to the sudden exposure of solvent inclusions to the gas phase upon evaporation.…”

Section: Succinic Acidmentioning

confidence: 99%

“…Bradley and Cotson (1953) (solid) 311-325 Kruif et al (1975) (solid) 303-328 1.10×10 −2 (α-form) de Wit et al (1983) (Marcolli et al, 2004) were used for interpolating/extrapolating the vapor pressure of the measured aqueous solutions to those of the saturated solution, using the measured activities. Temperature dependence of water-solubilities were taken from Apelblat and Manzurola (1987) and Apelblat and Manzurola (1989).…”

Section: Oxalic Acidmentioning

confidence: 99%

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The vapor pressures and activities of dicarboxylic acids reconsidered: the impact of the physical state of the aerosol

et al. 2010

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Abstract. We present vapor pressure data of the C 2 to C 5 dicarboxylic acids deduced from measured evaporation rates of single levitated particles as both, aqueous droplets and solid crystals. The data of aqueous solution particles over a wide concentration range allow us to directly calculate activities of the dicarboxylic acids and comparison of these activities with parameterizations reported in the literature. The data of the pure liquid state acids, i.e. the dicarboxylic acids in their supercooled melt state, exhibit no even-odd alternation in vapor pressure, while the acids in the solid form do. This observation is consistent with the known solubilities of the acids and our measured vapor pressures of the supercooled melt. Thus, the gas/particle partitioning of the different dicarboxylic acids in the atmosphere depends strongly on the physical state of the aerosol phase, the difference being largest for the even acids.Our results show also that, in general, measurements of vapor pressures of solid dicarboxylic acids may be compromised by the presence of polymorphic forms, crystalline structures with a high defect number, and/or solvent inclusions in the solid material, yielding a higher vapor pressure than the one of the thermodynamically stable crystalline form at the same temperature.

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Section: Oxalic Acidsupporting

confidence: 57%

Section: Malonic Acidmentioning

confidence: 73%

Section: Succinic Acidmentioning

confidence: 99%

Section: Oxalic Acidmentioning

confidence: 99%

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The vapor pressures and activities of dicarboxylic acids reconsidered: the impact of the physical state of the aerosol

et al. 2010

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“…As can be seen from the phase diagram, the aerosol consists of highly concentrated solution droplets with about 62 wt% oxalic acid. As a comparison, the saturation concentration of oxalic acid at 244 K is about 0.7 wt%, based on a thermodynamic extrapolation of bulk solubilities measured at higher temperatures (Apelblat and Manzurola, 1987;Omar and Ulrich, 2006).…”

Section: Introductionmentioning

confidence: 99%

High variability of the heterogeneous ice nucleation potential of oxalic acid dihydrate and sodium oxalate

et al. 2010

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Abstract. The heterogeneous ice nucleation potential of airborne oxalic acid dihydrate and sodium oxalate particles in the deposition and condensation mode has been investigated by controlled expansion cooling cycles in the AIDA aerosol and cloud chamber of the Karlsruhe Institute of Technology at temperatures between 244 and 228 K. Previous laboratory studies have highlighted the particular role of oxalic acid dihydrate as the only species amongst a variety of other investigated dicarboxylic acids to be capable of acting as a heterogeneous ice nucleus in both the deposition and immersion mode. We could confirm a high deposition mode ice activity for 0.03 to 0.8 µm sized oxalic acid dihydrate particles that were either formed by nucleation from a gaseous oxalic acid/air mixture or by rapid crystallisation of highly supersaturated aqueous oxalic acid solution droplets. The critical saturation ratio with respect to ice required for deposition nucleation was found to be less than 1.1 and the size-dependent ice-active fraction of the aerosol population was in the range from 0.1 to 22%. In contrast, oxalic acid dihydrate particles that had crystallised from less supersaturated solution droplets and had been allowed to slowly grow in a supersaturated environment from still unfrozen oxalic acid solution droplets over a time period of several hours were found to be much poorer heterogeneous ice nuclei. We speculate that under these conditions a crystal surface structure with less-active sites for the initiation of ice nucleation was generated. Such particles partially proved to be almost ice-inactive in both the deposition and condensation mode. At times, the heterogeneous ice nucleation ability of oxalic acid dihydrate significantly changed when the particles had been processed in preceding cloud droplet activation steps. Such behaviour was also observed for the second investiCorrespondence to: R. Wagner (robert.wagner2@kit.edu) gated species, namely sodium oxalate. Our experiments address the atmospheric scenario that coating layers of oxalic acid or its salts may be formed by physical and chemical processing on pre-existing particulates such as mineral dust and soot. Given the broad diversity of the observed heterogeneous ice nucleability of the oxalate species, it is not straightforward to predict whether an oxalate coating layer will improve or reduce the ice nucleation ability of the seed aerosol particles.

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Adipic Acid

Davis

Kemp

2000

Kirk-Othmer Encyclopedia of Chemical Technology

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Adipic acid, hexanedioic acid, 1,4‐butanedicarboxylic acid, mol wt 146.14, HOOCCH 2 CH 2 CH 2 CH 2 COOH, is a white crystalline solid with a melting point of about 152°C. Little of this dicarboxylic acid occurs naturally, but it is produced on a very large scale at several locations around the world. The majority of this material is used in the manufacture of nylon‐6,6 polyamide, which is prepared by reaction with 1,6‐hexanediamine. Adipic acid is a colorless, odorless, sour‐tasting crystalline solid that undergoes reactions including esterification, amidation, reduction, halogenation, salt formation, and dehydration. It also undergoes several industrially significant polymerization reactions. Adipic acid historically has been manufactured predominantly from cyclohexane. During the 1970s and 1980s, however, much research has been directed to alternative feedstocks, especially butadiene and cyclohexene, as dictated by shifts in hydrocarbon markets. Growing concern with air quality may exert further pressure for alternative routes as manufacturers seek to avoid NO x abatement costs. When dispersed as a dust, adipic acid is subject to normal dust explosion hazards. The material is an irritant, especially upon contact with the mucous membranes. Protective goggles or face shields should be worn when handling the material. The material should be stored in corrosion‐resistant containers, away from alkaline or strong oxidizing materials. Adipic acid is a very large‐volume organic chemical and is one of the top 50 chemicals produced in the United States in terms of volume, although demand is highly cyclic. Adipic acid for nylon takes about 60% of U.S. cyclohexane production. Adipic acid is relatively nontoxic.

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Solubility of oxalic, malonic, succinic, adipic, maleic, malic, citric, and tartaric acids in water from 278.15 to 338.15 K

Cited by 236 publications

References 11 publications

The vapor pressures and activities of dicarboxylic acids reconsidered: the impact of the physical state of the aerosol

The vapor pressures and activities of dicarboxylic acids reconsidered: the impact of the physical state of the aerosol

High variability of the heterogeneous ice nucleation potential of oxalic acid dihydrate and sodium oxalate

Adipic Acid

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