Final answer:
In a 0.155 M HCIO4 solution, the concentration of [H+] and [ClO4-] is 0.155 M, and the [OH-], calculated using the ion-product constant of water, is approximately 6.45 x 10^-13 M.
Step-by-step explanation:
To calculate the concentration of hydronium ions [H+] and perchlorate ions [ClO4-] in a 0.155 M HCIO4 solution, we need to acknowledge that HCIO4 is a strong acid and fully dissociates in water. Consequently, the concentration of [H+] would also be 0.155 M, and the same applies for the concentration of [ClO4-].
Next, to find the hydroxide ion concentration ([OH-]), we can use the ion-product constant for water (Kw) which at 25 °C is 1.0 × 10-14. The relationship between hydronium and hydroxide concentrations in water is given by the formula Kw = [H3O+][OH-]. Solving for [OH-] gives us [OH-] = Kw / [H+] which equals 1.0 × 10-14 / 0.155 M, resulting in approximately 6.45 × 10-13 M.