Question

68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The end point is reached after 25 m/L of KOH solution is added. what is the molarity of the HNO3 solution ?

1 р . HNO3 + KOH --> KNO3 + H20 68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The endpoint is reached after 25.0 mL of KOH solution is added. What is the molarity of the HNO3 solution?

Answer 1

HNO3 + KOH - KNO3 + H2O

Molarity = Number of gram moles of solute/Number of litres (dm3) of solution

Stoichiometric ratio = Number of moles of acid/Number of moles of base

= 1

Here, Molarity = V1M1 = V2M2

V1 = Volume of HNO3 =68.5 mL

V2 = Volume of KOH = 25 mL

M1 = concentration of HNO3 =?

M2 = concentration of KOH = 0.150 M

68.5 * M1 = 25 * 0.150

=3.75

M1 = 3.75/ 68.5

= 0.054 M