Calculate the pOH, [H+] and pH of the solutions having the following hydroxide
ion concentrations:
a [OH–] = 4.6 × 10–3 mol/L�
First, we can use the KW constant to find the [H+] of the solution:
KW = [H+][OH-] = 1.0 x 10^-14
[H+] = KW/[OH-] = (1.0 x 10^-14)/(4.6 x 10^-3) = 2.17 x 10^-12 mol/L
pH = -log[H+] = -log(2.17 x 10^-12) = 11.66
pOH = 14 - pH = 14 - 11.66 = 2.34
Therefore, the pOH of the solution is 2.34, the [H+] is 2.17 x 10^-12 mol/L, and the pH is 11.66.