Measurement and prediction of densities, viscosities, and surface tensions for aqueous solutions of potassium citrate

Lu, Jian-Gang; Hua, Ai-Chun; Xu, Zhaoyi; Fan, Fan; Lü, Cheng; Lin, Fengying

doi:10.1016/j.fluid.2012.05.007

Cited by 14 publications

(7 citation statements)

References 15 publications

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“…Validation details can be also found in our previous work [30,31]. Results of validation in this work using glycol and glycerol at 295.15 K are shown in Table 2.…”

Section: Validation For the Methods And Procedures Of Measurementsmentioning

confidence: 91%

“…Reported results are the average values of five samples. Experiments were carried out by the following procedures [30,31]. (1) Determining the volume of the pycnometer: first, determine the mass of the empty dry pycnometer.…”

Section: Density Measurementsmentioning

confidence: 99%

“…The temperature control system was the same as that for the density measurements. The flow times of samples were recorded using a stopwatch with accuracy ±0.01 s. Experiments were carried out as follows [30,31]. The viscometer was cleaned with 15 % H 2 O 2 and 15 % HCl before use.…”

Section: Viscosity Measurementsmentioning

confidence: 99%

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Density, Viscosity and Excess Molar Volume of the Aqueous Ionic Liquid Tris(monoethanolamine) Citrate at 293.15–323.15 K

Zhang

et al. 2014

J Solution Chem

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A new ionic liquid, tris(monoethanolamine) citrate (TMEAC), was synthesized and characterized by FT-IR spectrometry and 1 H NMR. Densities and viscosities of aqueous TMEAC mixtures were determined at 293.15-323.15 K and atmospheric pressure. The thermal expansion coefficient a, excess molar volume V E m , and excess logarithm of viscosity (ln g) E were calculated to evaluate the properties of the aqueous TMEAC ionic liquid. Correlation equations were fitted using these data for the calculation of density and viscosity. The results show that the density increases almost linearly as the mass fraction of TMEAC increases. The mass fraction of TMEAC has little influence on the density at low mass fraction. The viscosity changes significantly and sharply increases at mass fractions larger than 60 %. Both density and viscosity decrease as the temperature increases. The thermal expansion coefficient initially decreases and then increases with increase of the mass fraction of TMEAC. The change of the excess molar volume presents a W-shape. The excess logarithm of viscosity shows a variation where the value initially rises but subsequently drops. Values calculated from the correlation equations are in good agreement with the experimental values. The correlation equations can offer additional results for the aqueous TMEAC ionic liquid.Electronic supplementary material The online version of this article (

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“…Validation details can be also found in our previous work [30,31]. Results of validation in this work using glycol and glycerol at 295.15 K are shown in Table 2.…”

Section: Validation For the Methods And Procedures Of Measurementsmentioning

confidence: 91%

Section: Density Measurementsmentioning

confidence: 99%

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Density, Viscosity and Excess Molar Volume of the Aqueous Ionic Liquid Tris(monoethanolamine) Citrate at 293.15–323.15 K

Zhang

et al. 2014

J Solution Chem

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“…Surface tension was measured with a ±1.7% uncertainty. The measurement procedures in detail for the density, viscosity and surface tension can be also found in our previous work [26,27]. Conductivity was measured by a DDS-307 conductivity meter (Precision & Scientific Instrument Co., Ltd., Shanghai, China).…”

Section: Physical Propertiesmentioning

confidence: 99%

Property of diethanolamine glycinate ionic liquid and its performance for CO2 capture

Liu

et al. 2015

Journal of Molecular Liquids

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“…These values at higher concentration show a nonlinear trend in comparison to others. One more point about comparison shows that values given in the research paper by Lu et al 46 for aqueous tripotassium citrate solutions deviate very much from all other data represented in Figure 1. Further in Figure 2, the comparison of experimental and literature speed of sound values show that experimental speeds of sound at 0.6 mol·kg −1 deviate from other reported values.…”

Section: Resultsmentioning

confidence: 68%

Densities and Speeds of Sound of d(+)-Glucose, d(−)-Fructose, d(+)-Xylose and d(−)-Ribose in Aqueous Tripotassium Citrate Solutions at Different Temperatures

Kumar

Sheetal

2016

J. Chem. Eng. Data

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Apparent molar volumes (V ϕ ) and apparent molar isentropic compressions (K ϕ,S ) for some monosaccharides {D(+)-glucose, D(−)-fructose, D(+)-xylose and D(−)-ribose} in (0.0, 0.2, 0.4, 0.6) mol·kg −1 aqueous solutions of tripotassium citrate (TPC) have been determined from density and speeds of sound measurements along four isotherms at temperatures between (288.15 and 318.15) K at experimental pressure p = 0.1 MPa using an automated vibrating tube densimeter (Anton Paar DSA 5000 M). The experimental values are used to determine partial molar volume (V ϕ 0 ), partial molar isentropic compression (K ϕ,S 0 ) at infinite dilution and their corresponding partial molar volumes of transfer (ΔV ϕ 0 ), and partial molar isentropic compression of transfer (ΔK ϕ,S 0 ). The expansibility parameter (∂V ϕ 0 /∂T) P and its derivative (∂ 2 V ϕ 0 /∂T 2 ) P along with pair (V AB , K AB ) and triplet (V ABB , K ABB ) interaction coefficient for density and speed of sound data have been determined. The interpretation of the data has been made in terms of solute−solvent interactions.

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Measurement and prediction of densities, viscosities, and surface tensions for aqueous solutions of potassium citrate

Cited by 14 publications

References 15 publications

Density, Viscosity and Excess Molar Volume of the Aqueous Ionic Liquid Tris(monoethanolamine) Citrate at 293.15–323.15 K

Density, Viscosity and Excess Molar Volume of the Aqueous Ionic Liquid Tris(monoethanolamine) Citrate at 293.15–323.15 K

Property of diethanolamine glycinate ionic liquid and its performance for CO2 capture

Densities and Speeds of Sound of d(+)-Glucose, d(−)-Fructose, d(+)-Xylose and d(−)-Ribose in Aqueous Tripotassium Citrate Solutions at Different Temperatures

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