Final answer:
To calculate the pH of a 0.10 M monoprotic acid, you can use the dissociation constant (K) of the acid. Calculate the concentration of H₃O⁺ ions using [H₃O⁺] = √(K[acid]), and then determine the pH using the equation pH = -log[H₃O⁺].
Step-by-step explanation:
The pH of a 0.10 M monoprotic acid can be calculated using the dissociation constant (K) of the acid. In this case, the given K is 9.5x10⁻⁸. First, calculate the concentration of H₃O⁺ ions using the equation [H₃O⁺] = √(K[acid]). Substitute the given values and calculate [H₃O⁺]. Next, calculate the pH using the equation pH = -log[H₃O⁺]. Substitute the calculated value of [H₃O⁺] and calculate the pH.
For example, if the acid is acetic acid (CH₃COOH) with a K value of 1.8x10⁻⁵, the calculation would be:
- Calculate [H₃O⁺] = √(K[acid]) = √(1.8x10⁻⁵ * 0.10) = 3.79x10⁻³ M
- Calculate pH = -log[H₃O⁺] = -log(3.79x10⁻³) = 2.42
Therefore, the pH of a 0.10 M monoprotic acid with a K value of 9.5x10⁻⁸ would be calculated in a similar manner.