The hydrolytic degradation of squaramides and squaramic acids, the product of partial hydrolysis of squaramides, has been evaluated by UV spectroscopy at 37 °C in the pH range 3-10. Under these conditions, the compounds are kinetically stable over long time periods (>100 days). At pH >10, the hydrolysis of the squaramate anions shows first-order dependence on both squaramate and OH. At the same temperature and [OH], the hydrolysis of squaramides usually displays biphasic spectral changes (A → B → C kinetic model) with formation of squaramates as detectable reaction intermediates. The measured rates for the first step (k ≈ 10 M s) are 2-3 orders of magnitude faster than those for the second step (k ≈ 10 M s). Experiments at different temperatures provide activation parameters with values of ΔH ≈ 9-18 kcal mol and ΔS ≈ -5 to -30 cal K mol. DFT calculations show that the mechanism for the alkaline hydrolysis of squaramic acids is quite similar to that of amides.