Question

Titration is a type of experiment that can be performed to investigate a neutralization reaction. The equivalence point is when all of the acid and base is fully neutralized. A sample of 0.884 M aqueous potassium hydroxide was titrated against a standard solution of hydrochloric acid. What was the volume of the potassium hydroxide solution if 43.6 mL of 1.50 M hydrochloric acid was needed to reach the equivalence point? Enter a numerical answer only, in terms of mL.

Answer 1

Answer:

74.0 mL

Explanation:

In the equivalence point we have:

$n_{a} = n_{b}$

Where:

$n_{a}$ is the number of moles of the acid

$n_{b}$ is the number of moles of the base

$M_{a}V_{a} = M_{b}V_{b}$

Where M is the concentration and V is the volume

Hence the volume of the base is:

$V_{b} = \frac{M_{a}V_{a}}{M_{b}} = \frac{1.50 M*43.6 mL}{0.884 M} = 74.0 mL$              

Therefore, is needed 74.0 mL of the potassium hydroxide solution to reach the equivalence point.

I hope it helps you!