Water ionization becomes much less evident if the hydrogen bonds are just a few percent stronger but pure water contains considerably more $\ce{H+}$ ions if they are few percent weaker.
I found this line in some article. You can even copy/paste this line on search bar of Google. I didn't understood the latter part of this statement which is "but pure water contains considerably more $\ce{H+}$ ions if they are few percent weaker". The author is indicating to which of the following three situations?
- only $\ce{H+}$ ion concentration will increase
- both $\ce{H+}$ and $\ce{OH-}$ will increase
- $\ce{H+}$ will increase and $\ce{OH-}$ will decrease that is the equilibrium constant remains same.