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

74.0 mL

Step-by-step 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) = (M_(a)V_(a))/(M_(b)) = (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!