# 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

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+].

###### 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?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.

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Our tutors rated the difficulty ofCalculate [H+], [ClO4-], and [OH-] in an aqueous solution th...as medium difficulty.

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Based on our data, we think this problem is relevant for Professor Stec's class at UIC.