Über Dichte und Ausdehnung der Schwefelsäure in wässeriger Lösung, ein Beitrag zu ihrem physikalisch‐chemischen Verhalten

Domke, J.; Bein, Willy

doi:10.1002/zaac.19050430114

Cited by 12 publications

(3 citation statements)

References 89 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…Timmermans, writing in 1960, tabulates data from 19 studies. Of these the work of Domke and Beinwhich covers the ranges 0−100 wt % acid and 0−60 °Cis recommended as the standard work. Timmermans cites a further 34 studies covering the period 1826 to 1953 and dismisses them as insufficiently accurate.…”

Section: Resultsmentioning

confidence: 99%

Densities and Apparent Molar Volumes of Atmospherically Important Electrolyte Solutions. 1. The Solutes H₂SO₄, HNO₃, HCl, Na₂SO₄, NaNO₃, NaCl, (NH₄)₂SO₄, NH₄NO₃, and NH₄Cl from 0 to 50 °C, Including Extrapolations to Very Low Temperature and to the Pure Liquid State, and NaHSO₄, NaOH, and NH₃ at 25 °C

Clegg

Wexler

2011

J. Phys. Chem. A

View full text Add to dashboard Cite

Calculations of the size and density of atmospheric aerosols are complicated by the fact that they can exist at concentrations highly supersaturated with respect to dissolved salts and supercooled with respect to ice. Densities and apparent molar volumes of solutes in aqueous solutions containing the solutes H(2)SO(4), HNO(3), HCl, Na(2)SO(4), NaNO(3), NaCl, (NH(4))(2)SO(4), NH(4)NO(3), and NH(4)Cl have been critically evaluated and represented using fitted equations from 0 to 50 °C or greater and from infinite dilution to concentrations saturated or supersaturated with respect to the dissolved salts. Using extrapolated densities of high-temperature solutions and melts, the relationship between density and concentration is extended to the hypothetical pure liquid solutes. Above a given reference concentration of a few mol kg(-1), it is observed that density increases almost linearly with decreasing temperature, and comparisons with available data below 0 °C suggest that the fitted equations for density can be extrapolated to very low temperatures. As concentration is decreased below the reference concentration, the variation of density with temperature tends to that of water (which decreases as temperature is reduced below 3.98 °C). In this region below the reference concentration, and below 0 °C, densities are calculated using extrapolated apparent molar volumes which are constrained to agree at the reference concentrations with an equation for the directly fitted density. Calculated volume properties agree well with available data at low temperatures, for both concentrated and dilute solutions. Comparisons are made with literature data for temperatures of maximum density. Apparent molar volumes at infinite dilution are consistent, on a single ion basis, to better than ±0.1 cm(3) mol(-1) from 0 to 50 °C. Volume properties of aqueous NaHSO(4), NaOH, and NH(3) have also been evaluated, at 25 °C only. In part 2 of this work (ref 1 ) an ion interaction (Pitzer) model has been used to calculate apparent molar volumes of H(2)SO(4) in 0-3 mol kg(-1) aqueous solutions of the pure acid and to represent directly the effect of the HSO(4)(-) ↔ H(+) + SO(4)(2-) reaction. The results are incorporated into the treatment of aqueous H(2)SO(4) density described here. Densities and apparent molar volumes from -20 to 50 °C, and from 0 to 100 wt % of solute, are tabulated for the electrolytes listed in the title and have also been incorporated into the extended aerosol inorganics model (E-AIM, http://www.aim.env.uea.ac.uk/aim/aim.php) together with densities of the solid salts and hydrates.

show abstract

Section: Resultsmentioning

confidence: 99%

Densities and Apparent Molar Volumes of Atmospherically Important Electrolyte Solutions. 1. The Solutes H₂SO₄, HNO₃, HCl, Na₂SO₄, NaNO₃, NaCl, (NH₄)₂SO₄, NH₄NO₃, and NH₄Cl from 0 to 50 °C, Including Extrapolations to Very Low Temperature and to the Pure Liquid State, and NaHSO₄, NaOH, and NH₃ at 25 °C

Clegg

Wexler

2011

J. Phys. Chem. A

View full text Add to dashboard Cite

show abstract

“…− is fitted to densities of different H 2 SO 4 dilutions. 40 It should be noted that the parameter is fitted simultaneously with binary interaction parameters for 2-MTHF/HSO 4 − and 2-MTHF/H 3 O + . Thus, the applicability of the pure component parameter for different systems might be limited.…”

Section: ■ Materials and Methodsmentioning

confidence: 99%

The Effect of Sulfate Electrolytes on the Liquid–Liquid Equilibrium of 2-MTHF/Water/5-HMF: Experimental Study and Thermodynamic Modeling

et al. 2023

View full text Add to dashboard Cite

We investigate the influence of sulfate salts and sulfuric acid on the equilibrium behavior of 2-methyltetrahydrofuran (2-MTHF)/H 2 O/5hydroxymethylfurfural (5-HMF). Liquid−liquid equilibrium measurements are performed at atmospheric pressure and in a temperature range of T = (293−333) K. The compositions of the aqueous and organic phases, together with the dissociation state of the sulfate species, are determined with infrared spectroscopy and Indirect Hard Modeling. We show that the addition of the salts Na 2 SO 4 and Li 2 SO 4 results in salting out of 2-MTHF and 5-HMF from the aqueous phase. With increasing temperature, this effect gets less pronounced. In contrast, the addition of H 2 SO 4 does not result in any salting-out behavior. The investigation of the dissociation states shows that H 2 SO 4 dissociates to HSO 4 − while Na 2 SO 4 and Li 2 SO 4 dissociate completely to SO 4 2−. Parameter regression is performed to model the liquid−liquid equilibrium with the electrolyte perturbed-chain statistical associating fluid theory (ePC-SAFT) equation of state. For the analyzed salts, Na 2 SO 4 and Li 2 SO 4 , the performed parameter regression accurately predicts the measurement results. Still, we observe slight deviations between measured values and modeling when predicting the liquid−liquid equilibrium and the liquid density in the presence of sulfuric acid.

show abstract

“…It is beyond the scope of this paper to discuss the technical means of producing sulfuric acid of very high concentration or free of water; it may be remarked, however, that the combination of H20 and S03 to yield H2SO4 can obviously be achieved only under conditions in which the impressed S03 pressure exceeds the "latent" partial pressure "p,of the sulfuric acid to be dehydrated. 25 1.8 X IO'7 4 X 10-« 1.3 X IO"4 6 X 10-« io-4 4 x io-7 1.6 X IO-4 7 X IO-6 io-4 2 X IO"9 2 X IO'4 0.02 10'2 50 4.1 X IO'6 5 X 10-8 1.3 X 10"3 1 x io-< 10-8 6 x io-« 1.7 X IO"3 1.2 X IO"3 10-8 4 X IO'8 2 X IO-3 0.2 10'1 100 5.6 X 10-' 3 X IO"2 0.05 0.01 6 X 10-2 4 X io-4 0.065 0.09 The coefficients of the vapor-pressure formula for pr have been obtained from table 5 by linear extrapolation. The coefficients of the formula for the water vapor pressure "pr ("p" in mm.…”

Section: «(G)mentioning

confidence: 99%

The Vapor Phase above the System Sulfuric Acid–Water.

Abel¹

1946

J. Phys. Chem.

View full text Add to dashboard Cite

Über Dichte und Ausdehnung der Schwefelsäure in wässeriger Lösung, ein Beitrag zu ihrem physikalisch‐chemischen Verhalten

Cited by 12 publications

References 89 publications

The Effect of Sulfate Electrolytes on the Liquid–Liquid Equilibrium of 2-MTHF/Water/5-HMF: Experimental Study and Thermodynamic Modeling

The Vapor Phase above the System Sulfuric Acid–Water.

Contact Info

Product

Resources

About