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 0.723 M aqueous potassium hydroxide was titrated against a standard solution of hydrochloric acid. What was the volume of the potassium hydroxide solution if 79.1 mL of 1.50 M hydrochloric acid was needed to reach the equivalence point?

Answer 1

The volume of the potassium hydroxide solution was 164.1 mL

Step-by-step explanation:

In the equivalence point of a titration between an acid an a base, the moles of H⁺ are equal to the moles of OH⁻.

In the case of potassium hydroxide (KOH) and hydrochloric acid (HCl), an equation that represents the equivalence point would be:

`V_(KOH)*M_(KOH)=  V_(HCl)*M_(HCl)`

Using that equation and the data given in the problem, we can calculate the volume of potassium hydroxide:

`0.723M* V_(KOH)= 79.1mL*1.50 M\\V_(KOH)=(79.1mL*1.50 M)/(0.723 M) \\V_(KOH)=164.1mL`