Problem: 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? 

FREE Expert Solution
FREE Expert Solution

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+].


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Problem Details

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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