An aqueous solution with = 1.0 × has a pH of 12.0.

Question

An aqueous solution with  = 1.0 ×  has a pH of 12.0.

Quizplus · Accepted Answer

The given solution is basic with a pH of 12.0, which means the concentration of H+ ions is very low and the concentration of OH- ions is high. Thus, the value of [OH-] in this solution is greater than 1.0 x 10^-2 M.

According to the definition of the dissociation constant of water, Kw = [H+][OH-] = 1.0 x 10^-14 at 25°C.

Therefore, [H+] = Kw/[OH-] = 1.0 x 10^-14/[OH-] > 1.0 x 10^-14/1.0 x 10^-2 = 1.0 x 10^-12 M.

Since the concentration of [H+] is less than 1.0 x 10^-12 M and the pH is greater than 7, we can conclude that the given solution has a concentration of hydroxide ions greater than 1.0 x 10^-2 M, and TB6909_11 does not have a concentration of 1.0 x 10^-11 M. Thus, the statement is false.

An Aqueous Solution with = 1