Final answer:
The concentration of [H⁺] in the 0.100 M HClO₄ solution is also 0.100 M. The concentration of [ClO⁻₄] will be negligible. The concentration of [OH⁻] is 1 × 10⁻¹³ M.
Step-by-step explanation:
To calculate the concentrations of [H⁺], [ClO⁻₄], and [OH⁻] in the aqueous solution of 0.100 M HClO₄ at 25°C, we need to understand the dissociation of HClO₄ in water. HClO₄ is a strong acid, meaning it completely ionizes in water. Thus, the concentration of H⁺ in the solution will be equal to the initial concentration of HClO₄, which is 0.100 M.
Since HClO₄ is a strong acid, it does not significantly contribute to the concentration of ClO⁻₄ ions. Therefore, the concentration of ClO⁻₄ will be negligible in this solution.
The concentration of [OH⁻] can be found using the equation Kw = [H⁺] × [OH⁻], where Kw is the ion product constant for water, which is 1 × 10⁻¹⁴ at 25°C. Rearranging the equation, we find [OH⁻] = Kw / [H⁺]. Plugging in the values, we get [OH⁻] = (1 × 10⁻¹⁴) / (0.100) = 1 × 10⁻¹³ M.