So I'm taking a compressible flow class soon, and I've been thinking beforehand about the topic. A substance like water can easily be pressurized, but its density doesn't change easily, meaning there has to be some microscopic force between molecules in equilibrium with the pressure force. What force would this be though? Would it be Van der Waals force perhaps?

  • $\begingroup$ Hydrogen bonding is more likely, Van der Waals forces are comparatively weak $\endgroup$
    – Nic
    Jun 30 '16 at 22:32
  • $\begingroup$ @Nic the correct answer is that given by starrise. Hydrogen bonding and van der Waals forces have little to do with fluid incompressibility. $\endgroup$ Jul 6 '16 at 0:56

Two factors contribute to the incompressibility of liquids. The first is the electrostatic repulsion between the electron fields of neighboring molecules keeping the molecules from getting closer to each other without increasing force. The second is that intermolecular spacing is similar to that of solids made from the same material, due to intermolecular attraction and in turn due to some form of secondary bonding.

Note that no conventional material is totally incompressible, and greater hydrostatic force results in higher density. This is reflected in a material's bulk modulus, and the relationship between hydrostatic stress, bulk modulus, and volumetric strain. For example, water has a bulk modulus of approximately 3.12 GPa, meaning that an application of 3.12 MPa hydrostatic stress would result in a volume decrease of about 0.1%, and thus a density increase of close to the same amount. Other liquids have similar bulk moduli. For many applications this is a negligible change and can be safely ignored, and hence liquids are generally treated as incompressible.


For comparison, I found a table of some compressible liquids. I don't know the original source. Just look at Hg!
BTW, I've seen notes indicating that liquid H and He are pretty compressible, but a quick search didn't turn up easily translatable data.

enter image description here

  • $\begingroup$ The Table is from engineeringtoolbox.com. I don't know where they source their information from. $\endgroup$ Jul 6 '16 at 0:57

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.