Question

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. ​

Answer 1

• [H⁺] = 0.01 M

• [OH⁻] = 1x10⁻¹² M

• pH = 2

Step-by-step 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