Question

A 25.00-mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution?

Answer 1

Answer: The concentration of $H_2SO_4$ comes out to be 0.109 M.

Explanation:

To calculate the concentration of acid, we use the equation given y 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 $H_2SO_4$

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

We are given:

$n_1=2\\M_1=?M\\V_1=25.00mL\\n_2=1\\M_2=0.1322M\\V_2=41.22mL$

Putting values in above equation, we get:

$2\times M_1\times 25=1\times 0.1322\times 41.22\\\\M_1=0.109M$

Hence, the concentration of $H_2SO_4$ comes out to be 0.109 M