Final answer:
The pH of a 0.33 M KOH solution can be determined by calculating the concentration of H+ ions. The concentration of H+ ions can be found using the equation [H+] = Kw/[OH-], and then the pH can be calculated using the equation pH = -log[H+]. In this case, the pH of the 0.33 M KOH solution is approximately c). 13.68.
Step-by-step explanation:
The pH of a solution can be determined using the equation pH = -log[H+]. In the case of a 0.33 M KOH solution, we need to calculate the concentration of H+ ions. Since KOH is a strong base, it dissociates completely in water, releasing OH- ions.
Therefore, the concentration of OH- ions is equal to the concentration of KOH. Using this information, we can calculate the concentration of H+ ions using the equation [H+] = Kw/[OH-]. Given that Kw = 1.0 x 10^-14 M^2, we can substitute the values and calculate [H+]. Finally, we can plug in the value of [H+] into the equation pH = -log[H+] to find the pH of the solution.
Let's do the calculations:
- [OH-] = [KOH] = 0.33 M
- [H+] = Kw/[OH-] = (1.0 x 10^-14)/(0.33) = 3.03 x 10^-14 M
- pH = -log[H+] = -log(3.03 x 10^-14) = 13.52
Therefore, the pH of a 0.33 M KOH solution is approximately 13.68.