Question

A volume of 60.0 mL of a 0.120 M HNO3 solution is titrated with 0.840 M KOH. Calculate the volume of KOH required to reach the equivalence point.

Answer 1

Answer: 8.57 ml of KOH is required to reach the equivalence point.

Explanation:

To calculate the volume of acid, 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 $HNO_3$

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

We are given:

$n_1=1\\M_1=0.120M\\V_1=60.0mL\\n_2=1\\M_2=0.840M\\V_2=?$

Putting values in above equation, we get:

$1\times 0.120\times 60.0=1\times 0.840\times V_2\\\\V_2=8.57mL$

Thus 8.57 ml of KOH is required to reach the equivalence point.