Thread: Acid Base

Am I right, In a solvent like NH3, an electrolyte dissociating to give [NH4]+ ion is a stronger acid than ,say, sulfuric acid in NH3.

Please, I need a reply urgently.

You say "In a solvent like "...but we don't consider acidity or alkalinity in any solvents except water. It is kind of interesting considering ammonia is amphoteric, but yeah...the question isn't really relevant.

Am I right, In a solvent like NH3, an electrolyte dissociating to give [NH4]+ ion is a stronger acid than ,say, sulfuric acid in NH3.

What do you mean by

'' is a stronger acid than ,say, sulfuric acid in NH3''?
Sulfuric acid will react with NH3 anyway.....

Well, considering liquid NH3 to replace water. Now, since we want to make this amphoteric mixture, say, more acidic. So, we need a substance which dissociates to give NH4+ in the solution.


The point is, the solution of such an electrolyte will be more acidic than a solution of sulphuric acid in ammonia (since H2SO4 simply reacts with ammonia and most of it will get neutralised and so, only less H+ ions will remain in the solution to give any acidic character)