The Ternary System: Isopropyl Ether—HCl—H<sub>2</sub>O<sup>1</sup>

Cambpell, D. E.; Laurene, A. H.; Clark, Herbert M.

doi:10.1021/ja01144a010

Cited by 12 publications

(6 citation statements)

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“…For the ternary system DiPE + water + HCl reported by Cambell et al [39], the same method using equation (1) and the density was used to convert the initial compositions into mass fractions. Five DiPE + water + HCl systems were prepared by mixing DiPE in 1/1 volume ratio with aqueous HCl solutions of varying HCl mass fractions (x w = 0.0360, 0.1400, 0.2760, 0.3290, and 0.3560) that were prepared by mixing concentrated HCl (x w = 0.37) with milli Q water.…”

Section: Methodsmentioning

confidence: 99%

“…where k presents the number of data points and x exp i experimental data of component i and x cal i calculated data of component i by NRTL model and x exp i;avg average value of all experimental data of component i. [39] was validated experimentally. The analysis of each point was done in triplicate for water and for HCl.…”

Section: Data Treatment and Modeling Proceduresmentioning

confidence: 99%

“…First, the (water + DiPE) parameters were regressed and compared with the binary parameters reported by Aspen using experimental data reported by Hwang et al [41]. Subsequently the experimental data for the ternary system (H 2 O + DiPE + HCl) at 293 K reported by Campbell et al [39] were used to regress the binary H 2 O-HCl and DiPE-HCl interaction parameters. Hereafter, the experimental data of the ternary system of (FeCl 3 + H 2 O + DiPE) at 293 K reported by Maljkovic ´et al [38] were used to regress the binary H 2 O-FeCl 3 and DiPE-FeCl 3 interaction parameters in the NRTL model.…”

Section: Nrtl Modelingmentioning

confidence: 99%

“…The liquid-liquid biphasic region starts from the immiscibility of DiPE with water and disappears at high HCl and FeCl 3 concentra-tions where a three phase systems occurs [23,26]. Experimental data is available from the literature on the quaternary system [37], on the ternary systems DiPE + water + FeCl 3 [38] and DiPE +water + HCl [39], and NRTL binary interaction parameters are available for the binary system DiPE + water from the ASPEN plus database. Because consistency of the data is very important for a proper thermodynamic description, the data from the different sources was experimentally validated and the accuracy of the Di-PE + water binary LLE prediction with the parameters from the AS-PEN plus database was also verified.…”

Section: Introductionmentioning

confidence: 99%

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Thermodynamic modeling of ternary and quaternary (liquid+liquid) systems containing water, FeCl3, HCl and diisopropyl ether

Milošević

Hendriks

Smits³

et al. 2013

The Journal of Chemical Thermodynamics

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Section: Methodsmentioning

confidence: 99%

Section: Data Treatment and Modeling Proceduresmentioning

confidence: 99%

Section: Nrtl Modelingmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 2 more Smart Citations

Thermodynamic modeling of ternary and quaternary (liquid+liquid) systems containing water, FeCl3, HCl and diisopropyl ether

Milošević

Hendriks

Smits³

et al. 2013

The Journal of Chemical Thermodynamics

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“…Only one aqueous system is illustrated (graph 9). 1 Present address: Mobil Chemical Co., Metuchen, N. J.…”

Section: Antimony Chloridementioning

confidence: 99%

Ternary systems of chlorine compounds

Francis¹

1967

J. Chem. Eng. Data

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Graphs of 109 systems involving a compound of chlorine are presented. Most of these are ternary and show two liquid phases. Several involve chlorides of aluminum, antimony, cuprous copper, hydrogen, or mercury. Others include organic chlorine compounds. A table lists the locations of 121 published graphs of similar chlorine compounds. Mercuric chloride is much more soluble (up to 60% instead of 7%) in several organic compounds than in water. In some the maximum is in anhydrous solvents; in others, at about 90% solvent. These systems were studied extensively in the vain hope of finding some mercury salt or combination which absorbs olefins reversibly. Anhydrous cuprous chloride forms several systems with unusual types of phase diagram, some involving a complex with hydrogen chloride, postulated as CuHCk. Hydrogen chloride forms some aqueous systems having two separate binodal curves. Anhydrous systems are more likely to have island curves. The high reactivity of aluminum chloride results in graphs which are highly unconventional.The chlorides of aluminum, antimony, cuprous copper, hydrogen, and mercury are extremely soluble in certain mixtures of organic compounds, and show novel and perhaps useful miscibility relations. Graphs presented here include systems of several organic chlorine compounds not previously published. Some of the latter are almost equivalent to hydrocarbons in miscibility relations. Aqueous systems of ordinary salts are not listed here because of relatively little interest in solvent treatment of hydrocarbons. ALUMINUM CHLORIDEThe more refractory Friedel-Crafts reactions-alkylation of isoparaffins with lower olefins (5, 21) and isomerization of normal paraffins (5, 23), especially n-butane-are catalyzed most vigorously by concentrated solutions, up to 75% of aluminum chloride, in certain oxygen-containing solvents (mixed with the hydrocarbons). Ethyl ether is probably the best. Methyl and isopropyl ethers, ethyl acetate and other esters, acetone, sulfur dioxide, Chlorex, and even acetonitrile may be used, although the last contains no oxygen.Four aluminum chloride systems were reported earlier, with sulfur dioxide (8, graphs 20 to 22) and acetonitrile (9, graph 18). The graphs were approximations because

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