Thermodynamic properties of 0–6 mol kg<sup>–1</sup>aqueous sulfuric acid from 273.15 to 328.15 K

Clegg, Simon L.; Rard, Joseph A.; Pitzer, Kenneth S.

doi:10.1039/ft9949001875

Cited by 210 publications

(357 citation statements)

References 102 publications

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“…Acid errors were not an obvious problem as indicated by reproducible readings in the negative pH range although there was an initial adjustment necessary when changing to solutions of higher acid concentration. After completion of the field work, the response of the pH electrode assembly was assessed by The Pitzer model (20,(23)(24)(25) was used to calculate the theoretical pH of the prepared standard solutions. If the unscaled Pitzer approach is used, pH values for sulfuric acid solutions begin to diverge from MacInnes scaled values at pH values below -0.5.…”

Section: Methodsmentioning

confidence: 99%

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Nordstrom

Alpers

Ptacek

et al. 1999

Environ. Sci. Technol.

468

237

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Extremely acidic mine waters with pH values as low as -3.6, total dissolved metal concentrations as high as 200 g/L, and sulfate concentrations as high as 760 g/L, have been encountered underground in the Richmond Mine at Iron Mountain, CA. These are the most acidic waters known. The pH measurements were obtained by using the Pitzer method to define pH for calibration of glass membrane electrodes. The calibration of pH below 0.5 with glass membrane electrodes becomes strongly nonlinear but is reproducible to a pH as low as -4. Numerous efflorescent minerals were found forming from these acid waters. These extreme acid waters were formed primarily by pyrite oxidation and concentration by evaporation with minor effects from aqueous ferrous iron oxidation and efflorescent mineral formation.

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Section: Methodsmentioning

confidence: 99%

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Nordstrom

Alpers

Ptacek

et al. 1999

Environ. Sci. Technol.

468

237

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“…The thermochemical data for H 2 SO 4 /H 2 O uptake and loss by large aerosol particles derive from the liquid drop model and H 2 SO 4 and H 2 O vapour pressures over bulk solutions, calculated with a computer code (S. L. Clegg, personal communication, 2007) that is based on Giauque et al (1960);Clegg et al (1994). The thermochemical data for uptake/loss of gas phase H 2 SO 4 and H 2 O by intermediate sized particles are a smooth interpolation of the data for the small and large particles (see Lovejoy et al, 2004;.…”

Section: Maiamentioning

confidence: 99%

Aerosol microphysics modules in the framework of the ECHAM5 climate model – intercomparison under stratospheric conditions

et al. 2009

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Abstract. In this manuscript, we present an intercomparison of three different aerosol microphysics modules that are implemented in the climate model ECHAM5. The comparison was done between the modal aerosol microphysics module M7, which is currently the default aerosol microphysical core in ECHAM5, and two sectional aerosol microphysics modules SALSA, and SAM2. The detailed aerosol microphysical model MAIA was used as a reference to evaluate the results of the aerosol microphysics modules with respect to sulphate aerosol.The ability of the modules to describe the development of the aerosol size distribution was tested in a zero dimensional framework. We evaluated the strengths and weaknesses of different approaches under different types of stratospheric conditions. Also, we present an improved method for the time integration in M7 and study how the setup of the modal aerosol modules affects the evolution of the aerosol size distribution.Intercomparison simulations were carried out with varying SO 2 concentrations from background conditions to extreme values arising from stratospheric injections by large volcanic eruptions. Under background conditions, all microphysics modules were in good agreement describing the shape of the aerosol size distribution, but the scatter between the model results increased with increasing SO 2 concentrations. In particular in the volcanic case the setups of the aerosol modules have to be adapted in order to dependably capture the evoluCorrespondence to: H. Kokkola (harri.kokkola@fmi.fi) tion of the aerosol size distribution, and to perform in global model simulations.In summary, this intercomparison serves as a review of the different aerosol microphysics modules which are currently available for the climate model ECHAM5.

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“…The parameters at 298.15 K given in their errata are listed in our Table 3, and were used to calculate values of φ at the 6 experimental concentrations reported in Table 1. were recalculated for consistency using up-to-date ion-interaction models for these reference standards [8][9][10]34], where the CaCl 2 (aq) model of Pitzer et al [10] is based on refitting of results from the critical assessment of Rard and Clegg [41]. Rard and Miller [30,39] generally used two or three isopiestic standards in their isopiestic measurements and the average value of the osmotic coefficient for MgCl 2 (aq) was accepted for each equilibration.…”

Section: Extended Ion-interaction Model Equations For Solutions Of Simentioning

confidence: 99%

“…The general equations for the extended ion-interaction for mixed electrolytes are given in Appendix I of reference [9]. …”

Section: Extended Ion-interaction Model Equations and Calculations Fomentioning

confidence: 99%

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Isopiestic Investigation of the Osmotic and Activity Coefficients of {yMgCl2+(1−y)MgSO4}(aq) and the Osmotic Coefficients of Na2SO4⋅MgSO4(aq) at 298.15 K

et al. 2008

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Isopiestic vapor pressure measurements were made for {yMgCl 2 + (1 -y)MgSO 4 }(aq) solutions with MgCl 2 ionic strength fractions of y = (0, 0.1997, 0.3989, 0.5992, 0.8008, and 1) at the temperature 298.15 K, using KCl(aq) as the reference standard.These measurements for the mixtures cover the ionic strength range I = 0.9794 to 9.4318 mol·kg -1 . In addition, isopiestic measurements were made with NaCl(aq) as reference

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Thermodynamic properties of 0–6 mol kg^–1aqueous sulfuric acid from 273.15 to 328.15 K

Cited by 210 publications

References 102 publications

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Aerosol microphysics modules in the framework of the ECHAM5 climate model – intercomparison under stratospheric conditions

Isopiestic Investigation of the Osmotic and Activity Coefficients of {yMgCl2+(1−y)MgSO4}(aq) and the Osmotic Coefficients of Na2SO4⋅MgSO4(aq) at 298.15 K

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Thermodynamic properties of 0–6 mol kg–1aqueous sulfuric acid from 273.15 to 328.15 K

Cited by 210 publications

References 102 publications

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Negative pH and Extremely Acidic Mine Waters from Iron Mountain, California

Aerosol microphysics modules in the framework of the ECHAM5 climate model – intercomparison under stratospheric conditions

Isopiestic Investigation of the Osmotic and Activity Coefficients of {yMgCl2+(1−y)MgSO4}(aq) and the Osmotic Coefficients of Na2SO4⋅MgSO4(aq) at 298.15 K

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Thermodynamic properties of 0–6 mol kg^–1aqueous sulfuric acid from 273.15 to 328.15 K