We’re being asked to **calculate the volume (in mL) of 0.132 M HClO _{4} (strong acid)** required to reach the equivalence point in a titration of

Recall that at the ** equivalence point** of a titration:

$\overline{){\mathbf{moles}}{\mathbf{}}{\mathbf{acid}}{\mathbf{=}}{\mathbf{moles}}{\mathbf{}}{\mathbf{base}}}$

Also, recall that **moles = molarity × volume**.

This means:

$\overline{){\left(\mathbf{MV}\right)}_{{\mathbf{acid}}}{\mathbf{=}}{\left(\mathbf{MV}\right)}_{{\mathbf{base}}}}$

How many milliliters of 0.132 M HClO_{4} solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

A) 0.521

B) 0.0120

C) 83.7

D) 0.0335

E) 29.9

Frequently Asked Questions

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 Equivalence Point concept. If you need more Equivalence Point practice, you can also practice Equivalence Point practice problems.

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