Question

In a titration, what volume of 0.50 M HNO3 is required to completely react with 16.0 mL of 1.250 M KOH according to the equation HNO3(aq) KOH(aq) -> KNO3(aq) H2O(l)

Answer 1

Given :

A reaction , HNO3(aq) + KOH(aq) -> KNO3(aq) +  H2O(l)

To Find :

Volume of 0.50 M HNO3 is required to completely react with 16.0 mL of 1.250 M KOH .

Solution :

From the equation we can see that 1 mol of HNO3 react with 1 mol of KOH.

So,

$\text{Moles of HNO3 = Moles of KOH}\\\\M_1V_1=M_2V_2\\\\0.5 \times V_1 = 1.25\times 16\\\\V_1=\dfrac{1.25\times 16}{0.5}\\\\V_1=40\ ml$

Therefore, volume of HNO3 required is 40 ml.

Hence, this is the required solution.