As far as reducing agent strength goes, the pattern is linear: K>Na>Li
But hydroxide base strength shows the following pattern: NaOH>LiOH>KOH
Their relative pkb are as follows:
higher the pKb, weaker the base. I can't figure out a qualitative explanation as to why these base strengths vary in this way. And I can't relate it to a quantitative reason either.
Another issue correlates to this. KOH is way more soluble in EtOH than NaOH. But is NaOH still a stronger base? Does solvent matter that much?
If anyone really thinks they're sure of a reason it would be a great help.