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

Answer:

The volume of the potassium hydroxide solution was 164.1 mL

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:

$0.723M* V_{KOH}= 79.1mL*1.50 M\\V_{KOH}=\frac{79.1mL*1.50 M}{0.723 M} \\V_{KOH}=164.1mL$