Chemical Forums
Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: Mr. Phlogiston on July 20, 2005, 10:06:53 PM
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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:
NaOH, pKb=0.2
LiOH, pKb=0.36
KOH, pKb=0.5
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.
Thanks!