In a polymer solution, a theta solvent (or θ solvent) is a solvent in which polymer coils act like ideal chains, assuming exactly their random walk coil dimensions. Therefore, the Mark–Houwink equation exponent is ${\displaystyle 1/2}$ in a theta solvent. Thermodynamically, the excess chemical potential of mixing between a polymer and a theta solvent is zero.^[1][2][3][4]

Physical interpretation

The conformation assumed by a polymer chain in dilute solution can be modeled as a random walk of monomer subunits using a freely jointed chain model. However, this model does not account for steric effects. Real polymer coils are more closely represented by a self-avoiding walk because conformations in which different chain segments occupy the same space are not physically possible. This excluded volume effect causes the polymer to expand.

Chain conformation is also affected by solvent quality. The intermolecular interactions between polymer chain segments and coordinated solvent molecules have an associated energy of interaction which can be positive or negative. For a good solvent, interactions between polymer segments and solvent molecules are energetically favorable, and will cause polymer coils to expand. For a poor solvent, polymer-polymer self-interactions are preferred, and the polymer coils will contract. The quality of the solvent depends on both the chemical compositions of the polymer and solvent molecules and the solution temperature.

Thermodynamic definition

Thermodynamically, the excess chemical potential of mixing between a theta solvent and a polymer is zero. Equivalently, the enthalpy of mixing is zero, making the solution ideal.

One cannot measure the chemical potential by any direct means, but one can correlate it to the solution's osmotic pressure (${\displaystyle \Pi }$) and the solvent's partial specific volume (${\displaystyle v_{s}}$):

${\displaystyle \Delta \mu _{1}=-v_{s}\Pi }$

One can use a virial expansion to express how osmotic pressure depends on concentration:

${\displaystyle {\frac {\Pi }{RT}}={\frac {c}{M}}+Bc^{2}+B_{3}c^{3}...}$

M is the molecular weight of the polymer

R is the gas constant

T is the absolute temperature

B is the second virial coefficient

This relationship with osmotic pressure is one way to determine the theta condition or theta temperature for a solvent.

The change in the chemical potential when the two are mixed has two terms: ideal and excess:

${\displaystyle \Delta \mu _{1}=\Delta \mu _{1}^{ideal}+\Delta \mu _{1}^{excess}}$

The second virial coefficient, B, is proportional to the excess chemical potential of mixing:

${\displaystyle B={\frac {-\Delta \mu _{1}^{excess}}{{v_{s}}{c^{2}}}}}$

B reflects the energy of binary interactions between solvent molecules and segments of polymer chain. When B > 0, the solvent is "good," and when B < 0, the solvent is "poor". For a theta solvent, the second virial coefficient is zero because the excess chemical potential is zero; otherwise it would fall outside the definition of a theta solvent. A solvent at its theta temperature is, in this way, analogous to a real gas at its Boyle temperature.

Similar relationships exist for other experimental techniques, including light scattering, intrinsic viscosity measurement, sedimentation equilibrium, and cloud point titration.

See also

• Flory–Huggins solution theory

References