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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.

Sagot :

Maacastrobridn

Answer:

  • [H⁺] = 3.03x10⁻¹³ M
  • pH = 12.52
  • The solution is basic

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.

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