How would applying an external pressure on the following equilibrium affects the distribution of iodide between the polar (aqueous) and non polar (varsol)
Applying an external pressure on an equilibrium system can affect the distribution of iodide between the polar (aqueous) and non-polar (varsol) phases. To understand how, let's first discuss the concept of Le Chatelier's principle.
Le Chatelier's principle states that when a system at equilibrium is subjected to an external stress (such as pressure, temperature, or concentration changes), the system will try to counteract the stress and establish a new equilibrium position.
In the case of the distribution of iodide between the polar and non-polar phases, where it is likely present as ions (I-), we can consider the following equilibrium reaction:
I- (aqueous) ⇌ I- (Varsol)
Now, if we apply an external pressure to the system, we need to consider how pressure affects the equilibrium.
Pressure primarily affects the equilibrium involving gases (in this case, the I- ions are likely present in an aqueous solution, which is not significantly affected by pressure).
However, there may be an indirect effect of pressure if the polar and non-polar phases are not in equilibrium and are separated by a semi-permeable membrane that allows diffusion and equilibration. In this case, applying external pressure could potentially affect the equilibration rate and, consequently, the distribution of iodide between the phases.
If you want a more precise answer, it would be helpful to provide further details regarding the specific experimental setup and the properties of the system in question.