Refractive Index and Density Measurements for Selected Binary Protic‐Protic, Aprotic‐Aprotic, and Aprotic‐Protic Systems at Temperatures from 298.15 K to 308.15 K

Abstract

The refractive indices (n) and the densities (ρ) of: (1) protic‐protic solvent mixtures (methanol‐ethanol, methanol‐porpanol, methanol‐butanol and ethanol‐water), (2) aprotic‐aprotic solvent mixtures (acetonitrile‐dimethylformamide, acetonitrile‐dimethylsulphoxide, and acetonitrile‐1,4‐dioxane) and (3) aprotic‐protic solvent mixtures (dimethylformamide, acetonitrile with water and some aliphatic alcohols) were measured experimentally at different temperatures (25, 30 and 35 °C). From the values of the measured refractive indices and densities, the excess refractive indices (nE), molar refractions (R), atomic polarization (PA), molar volumes (V), solvated radii (r) and polarizabilities (α) of the mixed solvents were calculated. The results show that the solvent‐solvent interaction reaches maximum value at a definite mole fraction (x) of each solvent depending on its nature. Also, the excess refractive indices, densities and atomic polarizations are found to decrease as the temperature increases. On the other hand, the molar volumes, solvated radii, molar refractions and polarizabilities are found to increase as the temperature increases.

Viscosity Arrhenius Activation Energy and Derived Partial Molar Properties in 1,4-Dioxane + Water Binary Mixtures from 293.15 to 323.15 K

“…Thermodynamic and physico-chemical properties of binary liquid mixtures of 1,4-dioxane with water have been reported [2,3,11,37]. Therefore, the observed negative excess volumes [1-3, 9, 10, 38] are an indication of strong heteromolecular interactions in the liquid mixtures and, according to Fort et al [39], this can be attributed to specific interactions between dioxane and water molecules as investigated in some recent structural studies [14], 0.7870 [36] [1, 2, 7, 8], and non-specific interactions (dipole-dipole, dipole-induced-dipole, dispersion interactions) that depend on temperature [39].…”

Solvation thermodynamic parameters for sodium dodecyl sulfate (SDS) and sodium lauryl ether sulfate (SLES) surfactants in aqueous and alcoholic-aqueous solvents

“…The density measurements had been used to calculate the molar volume of some surfactants [20] and other substances in different solutions [21][22][23][24]. The refractive index measurements had been used to study the solvation of some substances in different solutions [25][26][27]. The effect of the solvent, temperature degree and the chemical nature of the surfactants on the different solvation thermodynamic properties of both SDS and SLES were of little interest in the literatures in the point of view of the CMC, molal volume, association constant and polarizability measurements.…”

Chemical‐assisted femtosecond laser writing of optical resonator arrays

“…The measured logarithmic slopes for all recorded spectra are plotted in Fig. b against the change in refractive index () . A standard deviation of ±0.15 dB in the ORA spectral strength, determined over 5 repeated recordings, led to the ±0.027 dB nm −1 (yellow) and 0.034 dB nm −1 (purple) error bars in the data points.…”

“…Following the sequence of colors in Fig. , reflection spectra have slowly shifted as the water‐methanol ratio filling both ORA resonators was adjusted from 100% water (blue) to an 80%‐20% (by volume) solution of water and methanol (red) that corresponded to a small refractive index increase above water's refractive index (1.3180 RIU) within the stacked resonators. This small index change induced a modest shift of 1577.4 ± 0.25 nm (blue) to 1575.2 ± 0.25 nm (red) in the peak resonant position with a 515 nm RIU −1 sensitivity rate and a large ∼10 −3 RIU minimum sensing resolution as would be expected for a single FPI .…”