Density (p), kinematic viscosity (p), and absolute viscosity ( ) are presented for mixtures of ethane-1,2-dlol and A/,A/-dimethylformamide from -10 to +80 °C. The above properties were fitted by empirical equations stating their dependence on temperature and mole fraction of the mixture. Furthermore, some considerations regarding the meaning of the obtained adjustment parameters are made. The excess functions, such as molar volumes VE, have been derived. The trends of V* data vs mole fraction of the mixtures have exhibited markedly negative deviations from Ideality, indicating extensive molecular Interactions between the components of the binary solvent system.

The extrathermodynamic parameters, relative permittivity (E,) and refractive index ( n ) , have been measured for ethane-l,2-diol-2-methoxyethanol binary mixtures over the entire composition range, at various temperatures ranging between -10 and 80 "C. For this system, as far as for many solvent-cosolvent systems which are useful for analytical and electrochemical applications, the properties cited above are continuous but not linear functions of the binary composition.Various equations have been applied in order to establish the best regression models for the relationship

In CHC, SF is a useful marker for assessing disease duration and progression before starting treatment and for predicting therapeutic response while on therapy. SF rise during antiviral therapy is largely independent of hemolysis and likely indicates activation of macrophages in response to antivirals.

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Densities (ρ) at various temperatures ranging from −10 up to +80 °C have been measured for N,N-dimethylformamide + 2-methoxyethanol + 1,2-dimethoxyethane ternary solvent system, employing 66 mixtures covering the whole miscibility field. Polynomial equations describing the dependence on temperature, ρ = ρ(t/°C), and molar composition, ρ = ρ(X1,X2), have been checked. Furthermore, the excess molar volumes (VE), derived from ρ values, can provide useful suggestions about the formation of solvent–cosolvent complexes. Excess molar volumes have been interpreted on the basis of specific interactions between unlike molecules, taking into account geometric effects and steric hindrances. The VE quantities have been isothermally fitted by an empirical relation of the type VE = VE(X1,X2,X3) formally derived from the well known Redlich–Kister equation. As a rule, for all the here tested relationships, the calculated values agree very well with the experimental ones, indicating that all the equations can be safely employed for predictive calculations in correspondence of the experimental data gaps.