If hydrogen bonding in water was weaker, what happens to H+ ion concentration? 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.
The article by Martin Chaplin 'Water's Hydrogen Bond Strength' (arXiv:0706.1355 [cond-mat.soft], no evidence of peer review) is discussing how changes to the properties of water would alter life.  

If the hydrogen bonding in water was stronger, there would be less ionization (less $\ce{H+}$ and less $\ce{OH-}$).

If the hydrogen bonding in water was weaker, there would be more ionization (more $\ce{H+}$ and more $\ce{OH-}$).