Determine the pH of a 0.116 M Ba(OH)₂ solution at 25°C. A)8.62 B)13.06 C)13.37 D)0.63 E)12.56

Question

Quizplus · Accepted Answer

Ba(OH)2 is a strong base, and it fully dissociates in water:

Ba(OH)2 (s) -> Ba2+ (aq) + 2OH- (aq)

Therefore, the concentration of hydroxide ions in the solution is:

[OH-] = 2 x 0.116 M = 0.232 M

Using the equation for the ionization of water:

Kw = [H+][OH-] = 1.0 x 10^-14

At 25°C, Kw = 1.0 x 10^-14, therefore:

[H+] = Kw/[OH-] = 1.0 x 10^-14 / 0.232 = 4.31 x 10^-14

pH = -log[H+] = -log(4.31 x 10^-14) = 13.37

Therefore, the pH of the solution is 13.37, and the correct answer is (C).

Determine the PH of a 0