Question

An aqueous solution of potassium hydroxide is standardized by titration with a 0.194 M solution of hydrobromic acid. If 25.2 mL of base are required to neutralize 24.2 mL of the acid, what is the molarity of the potassium hydroxide solution? M potassium hydroxide

Answer 1

Answer: The molarity of potassium hydroxide is 0.186 M

Explanation:

To calculate the molarity of base, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is HBr

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is KOH.

We are given:

$n_1=1\\M_1=0.194M\\V_1=24.2mL\\n_2=1\\M_2=?M\\V_2=25.2mL$

Putting values in above equation, we get:

$1\times 0.194\times 24.2=1\times M_2\times 25.2\\\\M_2=0.186M$

Hence, the concentration of potassium hydroxide is 0.186 M.