# Problem: How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?A) 0.521B) 0.0120C) 83.7D) 0.0335E) 29.9

###### FREE Expert Solution

We’re being asked to calculate the volume (in mL) of 0.132 M HClO4 (strong acid) required to reach the equivalence point in a titration of 50.00 mL of 0.0789 M NaOH (strong base)

Recall that at the equivalence point of a titration:

Also, recall that moles = molarity × volume

This means:

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

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###### Problem Details

How many milliliters of 0.132 M HClO4 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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Based on our data, we think this problem is relevant for Professor Boyd's class at UT.