What is the pH of a 0.0035 M KOH solution?

Question

Quizplus · Accepted Answer

KOH is a strong base, which completely dissociates in water to form K+ and OH- ions. The OH- ions then react with water to form H2O and OH- ions, which increases the concentration of OH- ion in solution. To find the pH of the solution, we need to find the concentration of H+ ion, which can be calculated using the equation:

Kw = [H+][OH-]

Where Kw is the ion product constant of water (1.0 x 10^-14 at 25°C).

At equilibrium, the concentration of [H+] and [OH-] are equal. Thus:

Kw = [H+]^2

[H+] = sqrt(Kw) = 1.0 x 10^-7 M

Using the equation for a strong base:

KOH + H2O → K+ + OH-

We know the concentration of KOH, so we can calculate the concentration of OH-:

[OH-] = 0.0035 M

To find the pOH:

pOH = -log[OH-] = -log(0.0035) = 2.46

Since pH + pOH = 14, the pH can be calculated as:

pH = 14 - pOH = 14 - 2.46 = 11.54

Therefore, the answer is D) 11.54.

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