Final answer:
The pH and pOH of a 0.2 M NaOH solution are calculated using the hydroxide ion concentration, resulting in a pH of 13.301 and a pOH of 0.6990.
Step-by-step explanation:
To calculate the pH and pOH of a 0.2 M solution of NaOH, we first need to understand that NaOH is a strong base that completely dissociates in water. Hence, the concentration of hydroxide ions, [OH-], is equal to the concentration of NaOH, which is 0.2 M. The pOH can be calculated using the formula pOH = -log[OH-].
pOH = -log(0.2) = -(-0.6990) = 0.6990
The pH can then be found using the relationship pH + pOH = 14.
pH = 14 - pOH = 14 - 0.6990 = 13.301
Therefore, the solution has a pH of 13.301 and a pOH of 0.6990.