Solubility of gases in water in comparison to their liquefiability

My textbook of physical chemistry says



> 
> ...The following factors affect the solubilities of gases in liquids:
> 
> 
> **(i) Nature of the gas and solvent:** Generally, the gases which
> can be easily liquefied are more soluble in common solvents. For example, $CO\_2$ is more soluble in water than oxygen or hydrogen. The gases which react with the solvent posses higher solubility. For example, $HCl$ and $NH\_3$ are highly soluble in water.
> 
> 
> Oxygen, nitrogen and carbon dioxide are much more soluble
> in ethyl alcohol than in water at the same temperature and
> pressure.
> 
> 
> **(ii) Temperature:** The solubility of most of the gases in
> liquids decreases with increase...
> 
> 
> 


*Why is it so that the gases which can be easily liquefied are more soluble?*


I mean, more liquefiable gases would have a stronger attractive forces amongst the molecule. This would mean that it would become increasingly tougher to dissolve them as their ability to be liquified increase. Then why the opposite is true?




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Edit


I found a similar question on Chemistry.SE here asking [Why does physisorption (physical adsorption) increase with ease of liquefaction?](https://chemistry.stackexchange.com/questions/68366/why-does-physisorption-physical-adsorption-increase-with-ease-of-liquefaction#:%7E:text=You%20are%20correct%20to%20say,(van%20der%20Waals%20forces).&text=So%20if%20the%20gas%20molecules,der%20Waals%20forces%20of%20attraction.). I know the above question (and answers) are aimed at adsorption and mine is about solubility, but I think there must be an explanation like that for the aforementioned one.


