Question

A solution of KOH is prepared with a [OH-] concentration of 3.3 × 10-2 M. Calculate [H+], pH, and identify whether the solution is acidic, basic, or neutral.

Answer 1

• [H⁺] = 3.03x10⁻¹³ M

• pH = 12.52

• The solution is basic

Step-by-step explanation:

We can first calculate [H⁺] by using the formula:

• [H⁺] * [OH⁻] = 1x10⁻¹⁴

• [H⁺] * 3.3x10⁻² = 1x10⁻¹⁴

• [H⁺] = 3.03x10⁻¹³ M

Now we proceed to calculate pH:

• pH = -log [H⁺]

• pH = -log (3.03x10⁻¹³)

• pH = 12.52

As the pH is higher than 7, the solution is basic.