$NaOH$is a strong electrolyte, and $C{H}_{3}OH$is a nonelectrolyte. How is the solution of $NaOH$different from that of $C{H}_{3}OH$ ?

Nonelectrolytes are substances which do not generate ions once dissolved. A material is considered as a great electrolyte if indeed the physical or chemical process that creates the ions is largely completely efficient (all of the dissolved chemical yields ions).

$NaOH$is a strong electrolyte and $C{H}_{3}OH$is a non-electrolyte.

To find out the difference between both of these electrolytes.

$NaOH$is an example of a great electrolyte that totally segregates into its ions because once dissolved in water, whereas $C{H}_{3}OH$is an illustration of a weak electrolyte that partially ionized particles in water. Thereby, in $NaOH$solutions, only the ions $N{a}^{+}$and $O{H}^{-}$are present, although in $C{H}_{3}OH$solutions, this same ions $C{H}_3{O}^{-}$and $H^{+}$, and also dissolved $C{H}_{3}OH$molecules, are present.

$\mathrm{NaOH}\left(s\right)\underset{\text{Dissociation}}{\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}}{\mathrm{Na}}^{+}\left(aq\right)+{\mathrm{OH}}^{-}\left(aq\right)$