Remember that **HClO _{4} is a strong, monoprotic oxyacid**. It’s a strong oxyacid since there are 3 more O than H in the formula.

Recall that ** strong acids** completely dissociate in water and that

**HClO _{4}(aq)** + H

Calculate [H_{3}O^{+}], [ClO_{4}^{-}], and [OH^{-}] in an aqueous solution that is 0.125 M in HClO_{4}(aq) at 25 °C.

Is the solution acidic, basic or neutral?

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