An aqueous solution contains a [H₃O⁺] that is 1.0 × 10^-3 M. What is the [OH^-] of this solution? A)1.0 × 10^-14 M B)1.0 × 10^-11 M C)1.0 × 10^-3 M D)1.0 × 10¹¹ M

Question

Quizplus · Accepted Answer

The balanced equation for the dissociation of H₃O⁺ is: HSO4- ⇌ H+ + SO4^2- From the given concentration of [HSO4-], we can assume that it completely dissociates in water to form H+ and SO4^2-. Therefore, at equilibrium, the [H+] will be equal to the initial concentration of [HSO4-]. pH is defined as the negative logarithm of the hydrogen ion concentration. So, pH = -log[H+] = -log[HSO4-] = -log(1.0 × 10^-3) = 3 pOH + pH = 14 pOH = 14 - pH = 14 - 3 = 11 Now, pOH = -log[OH-] -log[OH-] = 11 [OH-] = 1.0 × 10^-11 Therefore, [OH-] in the solution is 1.0 × 10^-11 M, and the [OH-] is Answer: B.

An Aqueous Solution Contains a [H3O+] That Is 1

An Aqueous Solution Contains a [H₃O⁺] That Is 1