The nearest to an ideal fluid is a hard sphere fluid, but this is removed from the ideal gas or even solution concept of ideality in a critical way.
Ideal (also called perfect) gases are ideal because they lack intermolecular interactions. A statistical description that ignores the intermolecular potential suffices to describe an ideal gas. A first extension toward nonideality, following the vdW equation, describes particles in a gas as hard spheres (having an excluded volume).
The property of reduced compressibility encoded by a hard sphere potential also provides the simplest model for a liquid. The hard sphere potential suffices to describe a simple liquid, and it is about as ideal an abstraction of a liquid as you can get. However, while it shows a liquid-solid phase transition, it does not display a liquid-gas transition. In that sense it is not a universal model, it does not capture some key properties of liquids, in the same sense that the ideal gas law is not universal because it too does not address some simpler key properties of real gases (such as excluded volume). However, introduction of an additional attractive term as in the full vdW model, bringing us further away from ideality, allows us to observe a critical point below which a phase transition clearly occurs between liquid and gas. I should add that the hard sphere potential can be expressed in reduced units, making it universal within the scope of that limited model. It is a suitable first approximation for understanding some properties of nonpolar liquids, for instance condensed noble gases.
I would add that Raoult's law is another ideal model for a liquid, and consistent with the ideal gas concept (or rather Dalton's law). It is also a limiting law (or model), like the ideal gas, and applies to dilute solutions.