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A bottle labeled 0.01 M HCl is found in the laboratory. Assuming that the HCl is completely ionized calculate the [H+], [OH-] and the pH of the solution. ​

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Answer:

  • [H⁺] = 0.01 M
  • [OH⁻] = 1x10⁻¹² M
  • pH = 2

Explanation:

The assumption that the HCl is completely ionized means that the original concentration of the acid is equal to [H⁺].

  • [H⁺] = 0.01 M

With [H⁺], we can calculate [OH⁻], by using the following formula:

  • [H⁺] * [OH⁻] = 10⁻¹⁴
  • 0.01 M * [OH⁻] = 10⁻¹⁴
  • [OH⁻] = 1x10⁻¹² M

Finally we calculate the pH of the solution:

  • pH = -log[H⁺]
  • pH = 2

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