7.7: Solubility
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The maximum solubility of a solute can be determined using the same methods we have used to describe colligative properties. The chemical potential of the solute in a liquid solution can be expressed
μB(solution)=μoB(liquid)+RTlnχB
If this chemical potential is lower than that of a pure solid solute, the solute will dissolve into the liquid solvent (in order to achieve a lower chemical potential!) So the point of saturation is reached when the chemical potential of the solute in the solution is equal to that of the pure solid solute.
μoB(solid)=μoB(liquid)+RTlnχB
Since the mole fraction at saturation is of interest, we can solve for ln(χB).
lnχB=μoB(solid)=μoB(liquid)RT
The difference in the chemical potentials is the molar Gibbs function for the phase change of fusion. So this can be rewritten
lnχB=−ΔGofusRT
It would be convenient if the solubility could be expressed in terms of the enthalpy of fusion for the solute rather than the Gibbs function change. Fortunately, the Gibbs-Helmholtz equation gives us a means of making this change. Noting that
(∂(ΔGT)∂T)p=ΔHT2
Differentiation of the above expression for ln(χB) with respect to T at constant p yields
(∂lnχB∂T)p=1RΔHfusT2
Separating the variables puts this into an integrable form that can be used to see how solubility will vary with temperature:
∫lnχB0dlnχB=1R∫TTfΔHfusdTT2
So if the enthalpy of fusion is constant over the temperature range of Tf to the temperature of interest,
lnχB=ΔHfusR(1Tf−1T)
And χB will give the mole fraction of the solute in a saturated solution at the temperature T. The value depends on both the enthalpy of fusion, and the normal melting point of the solute.