[zeroblade]

Hi all, I have a question from my textbook that I don't quite understand so any help is much appreciated!

Q: The sodium cation Na⁺, is more soluble in water than the silver cation Ag²⁺. Why is this so?

A: Because silver is more electronegative than sodium, we expect sodium to maintain itself as a "naked" cation, which leads to large ion-dipole interactions with the water.

To me this doesn't make much sense. If silver is more electronegative doesn't that mean it will interact much more strongly with the slightly positive hydrogen end of water?