A 100.0 mL sample of 0.18 M HClO4 (Strong acid) is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 75.0 mL of LiOH

pH = 12.11

Explanation:

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In this case, since the chemical reaction between perchloric acid and lithium hydroxide is:

Whereas the mole ratio between the acid and base is 1:1, it means they react in the same proportion. In such a way, given the volume and concentration of acid, we compute the moles:

Now, the moles of base that reacted:

Thus, since there is an excess of lithium hydroxide of:

We compute the new concentration considering the total final volume of 175.0 mL:

Now, since there is a strong base remaining in solution, we compute its pOH first:

Because LiOH is fully ionized to Li⁺ and OH⁻ ions. Therefore the pH is:

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