Because NaOH is a strong base that fully dissociates, the hydroxide ion concentration equals 0.01 M, leading to a pOH of 2 and thus a pH of 12, since $$pH + pOH = 14$$.

A pH of 12 indicates that NaOH does not significantly contribute hydroxide ions in the solution, implying weak basic character.

Although one might expect that all bases behave similarly upon dissociation, the complete ionization of NaOH ensures that its hydroxide ion concentration directly determines the pOH, and by extension the pH, accurately calculated via the relation $$pH = 14 - pOH$$, thereby confirming the pH of 12 for a 0.01 M solution.

NaOH partially dissociates, resulting in a pH lower than 12 despite a 0.01 M concentration.