Not dumb at all! In order to not write an even bigger wall of text, I assumed some things, like everyone already knowing that in water, a pH of 7 is considered neutral. This is because that solution would have an equal amount of acidic ions and basic ions, each with a concentration of approximately 10^(-7) moles per liter. But with a different solvent like ammonia, the change in auto dissociation constant means that to get an equal number of acidic and basic ions, you would only need a concentration of 10^(-15) moles per liter.
So, it would change a lot of the standard practices in a lab, like making buffers, neutralizing solutions, etc. Since it’s Saturday and I’m doing this all off the top of my head, I don’t know what other implications there might be, but basically a lot of things that chemists and biochemists take for granted would need to recalculated. Acids would be more acidic, bases more basic, etc. In ammonia, even water would be a fairly strong acid!
The chemistry doesn’t really change, but a lot of the standard practices would need to be done differently (including the way we make buffers, measure pH, and the range of pH that a solution could be).