Limitations of Henry's law Consider the diagram


Henry's law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. The proportionality factor is called Henry's law constant.

Suppose the weights on the piston are so increased such that the pressure of the gas becomes numerically equal to Henry's law constant.
Then Henry's law gives that the mole fraction of the gas in solution is equal to 1.
Mole fraction of solute in solvent being equal to 1 implied that there is absolutely no solvent.
But in the situation described by the diagram, the solvent molecules are always present.
How is this so? Perhaps there is a limitation to Henry's law which has not been mentioned?
(Source: chem.libretexts.org)
In the image, we see that for a &quot;real gas&quot; (indicated by non-ideal solution), Henry's law is applicable for $\ce{\chi} &lt;&lt; 1$.
As, $$\ce{p = K_H \cdot \chi}$$ hence the pressure should be low.
Limitations of Henry's law:

The pressure should be low and the temperature should be high i.e the gas should behave like an ideal gas.

The gas should not undergo compound formation with the solvent or association or dissociation in the solvent.