Why do LiOH is weak base as compared to NaOH even though it's hydration enthalpy is greater than Na?


closed as off-topic by Todd Minehardt, M.A.R. ಠ_ಠ, Klaus-Dieter Warzecha, jerepierre, ron Mar 23 '16 at 0:54

This question appears to be off-topic. The users who voted to close gave this specific reason:

If this question can be reworded to fit the rules in the help center, please edit the question.

  • 2
    $\begingroup$ Well, besides hydration energy, there's other factors at play. How do their lattice energies compare? Look them up, maybe that'll help you answer your own question. $\endgroup$ – getafix Mar 22 '16 at 12:37
  • $\begingroup$ link.aip.org/link/?JCPSA6/122/194509/1 $\endgroup$ – Lighthart Mar 22 '16 at 21:40

$\ce{NaOH}$ and $\ce{LiOH}$ are both classified as ionic compounds, but as with most things in chemistry, this is always on a continuum scale, in this case between ionic and covalent bonds. $\ce{NaOH}$ is 'more' ionic in character which means its $\ce{OH^-}$ is more frequently unaccompanied by its counter cation, $\ce{Na+}$ as compared to $\ce{LiOH}$ and its corresponding $\ce{Li+}$.

Without the cation to balance the character, $\ce{OH^-}$ will balance its charge via deprotonation, and hence it is a stronger base.


Not the answer you're looking for? Browse other questions tagged or ask your own question.