Remember that HClO4 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 acids donate H+ to the base (water in this case). The dissociation of HClO4 is as follows:
HClO4(aq) + H2O(l) → H3O+(aq) + ClO4–(aq)
We can do a mole-to-mole comparison to find [H3O+] and [ClO4–]. Recall that M = mol/L and [H+] is just the same as [H3O+].
Calculate [H+], [ClO4-], 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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