The densities of the phases were measured precisely by a densitometer (Anton Paar®, DMA 5000) at 25 °C. The densitometer accuracy is 10−6 g cm−3. The viscosities of the phases were measured precisely by a microviscometer (Anton Paar®, Lovis 2000M) at 25 °C. The microviscometer accuracy is 10−3 mPa s. The dynamic interfacial tensions (IFT) were measured by an interfacial tensiometer (Krüss, DSA25) via the pendant drop method.32,33 (link)
Dma 5000
Manufactured by Anton Paar
Sourced in Austria
The DMA 5000 is a density and sound speed meter from Anton Paar. It measures the density and sound speed of liquids, gases, and supercritical fluids.
Automatically generated - may contain errors
Lab products found in correlation
Optima xl a, by Beckman Coulter (2 mentions)
Lovis 2000m, by Anton Paar (1 mentions)
Dsa25, by Krüss (1 mentions)
Lovis 2000 me, by Anton Paar (1 mentions)
Amvn rolling ball viscometer, by Anton Paar (1 mentions)
Dpx 400 mhz spectrometer, by Bruker (1 mentions)
50 ti rotor, by Beckman Coulter (1 mentions)
D8 advance diffractometer, by Bruker (1 mentions)
6890 series gas chromatograph, by Agilent Technologies (1 mentions)
Sigma 70 tensiometer, by Biolin Scientific (1 mentions)
Ar g2 rheometer, by TA Instruments (1 mentions)
Fe20 basic, by Mettler Toledo (1 mentions)
26 protocols using dma 5000
1
Measuring Interfacial Properties of Phases
2
Partial Molar Volumes and Thermal Expansivity
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Partial molar
volumes were estimated with a density meter Anton Paar DMA 5000 M
at 20, 25, and 30 °C from the concentration–density dependency
for compounds dissolved in 50 mM phosphate buffer (pH 11). The experimental
procedure and the data analysis method were described previously.36 (link),57 (link),58 (link) The partial molar volume at 25
°C (V20) and thermal volumetric
expansivity of the solute (α20 = ∂V20/∂T) were
estimated globally from two independent dilution series. The density
of pure solvent (d0) was extrapolated
individually for each experimental condition (i.e., temperature and
buffer preparation). The change of d0 with
temperature was further used to determine thermal volumetric expansivity
coefficient of the bulk buffer according to the formula α0 = −(∂d0/∂T)/d0.
volumes were estimated with a density meter Anton Paar DMA 5000 M
at 20, 25, and 30 °C from the concentration–density dependency
for compounds dissolved in 50 mM phosphate buffer (pH 11). The experimental
procedure and the data analysis method were described previously.36 (link),57 (link),58 (link) The partial molar volume at 25
°C (V20) and thermal volumetric
expansivity of the solute (α20 = ∂V20/∂T) were
estimated globally from two independent dilution series. The density
of pure solvent (d0) was extrapolated
individually for each experimental condition (i.e., temperature and
buffer preparation). The change of d0 with
temperature was further used to determine thermal volumetric expansivity
coefficient of the bulk buffer according to the formula α0 = −(∂d0/∂T)/d0.
3
Density Measurement of Micellar Solutions
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To enable the
conversion between
concentration scales and to calculate the apparent molar volumes of
the micellar solutions in the concentration range of the experiments,
the densities of all prepared solutions were measured at the 0.1 MPa
pressure in the temperature range from 278.15 to 328.15 K using a
vibrating tube densimeter, Anton Paar DMA5000, with a stated reproducibility
of ±1·10–3 kg·m–3.
conversion between
concentration scales and to calculate the apparent molar volumes of
the micellar solutions in the concentration range of the experiments,
the densities of all prepared solutions were measured at the 0.1 MPa
pressure in the temperature range from 278.15 to 328.15 K using a
vibrating tube densimeter, Anton Paar DMA5000, with a stated reproducibility
of ±1·10–3 kg·m–3.
4
Density and Viscosity Measurements
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The densities and viscosities of the samples were measured at 37 °C using a density meter DMA5000 (Anton Paar, Ashland, VA, USA) and a viscometer Lovis 2000ME (Anton Paar), respectively.
5
Measuring Kinematic Viscosity and Density
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Kinematic viscosity (η) was measured with a micro Ubbelohde viscometer (type and capillary no. 537 10/I, apparatus no. 1070016; SI Analytics GmbH, Mainz, Germany) and an automatic flow time measuring system ViscoSystem® AVS 370 (SI Analytics GmbH, Mainz, Germany). The density (d), which is needed for calculating dynamic viscosity, η, was measured with a vibrating tube densitometer (DMA5000, Anton Paar GmbH, Germany). All details regarding η and d measurements were reported previously [38 (link)]. The cumulative error in η determination was estimated to be ±1%.
6
Density and Viscosity Measurement Protocol
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Solution density was measured using an Anton Paar DMA5000 oscillating capillary density meter (Anton Paar GmbH, Graz, Austria). Solution viscosity was measured using an Anton Paar AMVn rolling ball viscometer (6 d.mm silanised capillary, 5 d.mm steel ball). All measurements were performed at 20.00°C, controlled to within ±0.005°C, and are shown in S1 Table .
7
Characterization of Ionic Liquids by NMR and Thermal Analyses
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Nuclear magnetic
resonance (NMR) was performed to confirm the chemical structures of
these four ILs. The NMR spectrum was obtained on a Bruker DPX 400
MHz spectrometer with CDCl3 as the standard solvent. Thermal
stability was determined using TGA under an N2 atmosphere
at a scanning rate of 10 K·min–1 to explore
the decomposition temperature of ILs. DSC was carried out using a
Mettler Toledo DSC1 with liquid nitrogen cooling. Samples were heated
under a nitrogen atmosphere from 193.2 to 303.2 K at a rate of 10
K·min–1 to explore the melting point (Tm) of ILs. Densities and viscosities were measured
on an Anton Paar DMA 5000 type automatic densitometer with a precision
of 0.0001 g/cm3 and a Brookfield LVDV-II + Pro viscometer
with an uncertainty of ±1%, respectively. Linear sweep voltammetry
(LSV) was performed on a CHI760E electrochemical workstation. Glassy
carbon (GC), a platinum wire, and the Ag/AgCl electrode were used
as the working electrode, the counter electrode, and the reference
electrode, respectively. The ILs were dried on a Schlenk line at 0.15
mbar and 60 °C for 6 h until no further bubbles’ evolution
was observed. Coulometric Karl Fisher titration was used to measure
the water concentration of these IL samples. The water contents of
[P4442][PTSNTF], [Py14][PTSNTF], [P4442][PTS2N], and [Py14][PTS2N] were
67, 79, 73, and 71 ppm, respectively.
resonance (NMR) was performed to confirm the chemical structures of
these four ILs. The NMR spectrum was obtained on a Bruker DPX 400
MHz spectrometer with CDCl3 as the standard solvent. Thermal
stability was determined using TGA under an N2 atmosphere
at a scanning rate of 10 K·min–1 to explore
the decomposition temperature of ILs. DSC was carried out using a
Mettler Toledo DSC1 with liquid nitrogen cooling. Samples were heated
under a nitrogen atmosphere from 193.2 to 303.2 K at a rate of 10
K·min–1 to explore the melting point (Tm) of ILs. Densities and viscosities were measured
on an Anton Paar DMA 5000 type automatic densitometer with a precision
of 0.0001 g/cm3 and a Brookfield LVDV-II + Pro viscometer
with an uncertainty of ±1%, respectively. Linear sweep voltammetry
(LSV) was performed on a CHI760E electrochemical workstation. Glassy
carbon (GC), a platinum wire, and the Ag/AgCl electrode were used
as the working electrode, the counter electrode, and the reference
electrode, respectively. The ILs were dried on a Schlenk line at 0.15
mbar and 60 °C for 6 h until no further bubbles’ evolution
was observed. Coulometric Karl Fisher titration was used to measure
the water concentration of these IL samples. The water contents of
[P4442][PTSNTF], [Py14][PTSNTF], [P4442][PTS2N], and [Py14][PTS2N] were
67, 79, 73, and 71 ppm, respectively.
8
Sedimentation Velocity Analysis of Protein Samples
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Sedimentation velocity experiments were carried out on a Beckman XL-I analytical ultracentrifuge (Beckman-Coulter). Sedimentation velocity was performed at 20°C using 2 channel centre pieces, with protein loading concentrations of 2 mg/ mL, 1.0 mg/ mL and 0.5 mg/ mL in 20 mM TrisHCl, pH 7.5 containing 200 mM NaCl. Data were obtained at 40,000 rpm, using a Beckman 50Ti rotor, with the cells scanned radially with interference optics and with absorbance optics at a wavelength of 280 nm. Scans were obtained every 10 minutes and data were analyzed using the program SEDFIT v11.3 (www.analyticalultracentrifugation.com ). Sedimentation coefficient distributions were obtained using the c(S) methodology114, and figures were created in GUSSI 1.0.3. Solution densities and viscosities were measured directly using an Anton Paar DMA5000 densitometer/viscometer.
9
Glycine Solubility Measurement in Inorganic Salts
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In this study, glycine solubilities in solutions with inorganic salts at 25 °C and 28 °C were measured using a similar method [15 (link)]. The rationale for choosing this pair of temperatures will be discussed in Section 3.1 and Section 3.4 .
The isothermal method for glycine solubility [15 (link)] is briefly described here. A suspension of a given solid form (either α- or γ-form) of glycine fine crystals was agitated in a jacketed beaker to establish the isothermal liquid-solid equilibrium at a temperature controlled by a Julabo FP50-HL circulator (Seelbach, Germanywith a temperature resolution of 0.01 °C). A precision densitometer (Anton Paar DMA5000, Graz, Austria) was used to regularly measure glycine solution density so as to determine solution concentration over a period of time (typically 30 min), until the solution was saturated, which was indicated by the unchanged glycine concentration (i.e., solubility) within a concentration uncertainty of 0.2%. The polymorphic form of the glycine crystals was examined before and after a solubility determination using powder X-ray diffraction (PXRD; refer toFigure S1 in the Supplementary Materials ) (Bruker D8 Advance Diffractometer, Billerica, MA, USA).
The isothermal method for glycine solubility [15 (link)] is briefly described here. A suspension of a given solid form (either α- or γ-form) of glycine fine crystals was agitated in a jacketed beaker to establish the isothermal liquid-solid equilibrium at a temperature controlled by a Julabo FP50-HL circulator (Seelbach, Germanywith a temperature resolution of 0.01 °C). A precision densitometer (Anton Paar DMA5000, Graz, Austria) was used to regularly measure glycine solution density so as to determine solution concentration over a period of time (typically 30 min), until the solution was saturated, which was indicated by the unchanged glycine concentration (i.e., solubility) within a concentration uncertainty of 0.2%. The polymorphic form of the glycine crystals was examined before and after a solubility determination using powder X-ray diffraction (PXRD; refer to
10
Physicochemical Properties of Coconut Oil
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The physicochemical properties of the CCO were determined and shown in Table 1 . The CCO density was measured with an Anton Paar DMA5000 instrument, while the kinematic viscosity was determined using an Ubbelohde glass viscometer. The fatty acid composition, shown in Table 2 , was determined using the official and practice method AOCS (Ce 1–62) using Agilent Hewlett-Packard 6890 series gas chromatograph equipped with flame ionization detector, SP-2340 capillary column (60 m in length, 25 mm of internal diameter, and 0.2 mL film thickness), and a split ratio of 100 : 1. CCO was found to be holding primarily eleven fatty acids. Of these, linoleic (9,12-octadecadienoic) acid, palmitic (hexadecanoic) acid, stearic (octadecanoic) acid, oleic (octadec-9-enoic) acid are frequently presented in most of oils. The other fatty acids, including myristic, palmitoleic, margaric, linolenic, arachidic, gadoleic, and behenic were present in minor amounts.
The oil had a significantly high content of FFA (3.18%) evaluated by AOCS standard titration method, which is higher than the content (>1.0%) permitted in oil to be catalyzed by alkali catalysts.
The oil had a significantly high content of FFA (3.18%) evaluated by AOCS standard titration method, which is higher than the content (>1.0%) permitted in oil to be catalyzed by alkali catalysts.
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