A volume of 50.0 mL of a 0.510 M HNO3 solution is titrated with 0.810 M KOH. Calculate the volume of KOH required to reach the equivalence point.
Solution:
Balanced chemical equation,
HNO3 (aq) + KOH (aq) -----> KNO3 (aq) + H2O (l)
M1 = 0.510 M M2 = 0.810 M
V1 = 50.0 mL V2 = ?
n1 = 1 n2 = 1
At equivalence point, the number of moles of an acid is exactly equal to number of moles of a base,
(M1V1 / n1) = (M2V2 / n2)
V2 = (M1V1 / n1) * (n2 / M2)
= (( 0.510 * 50.0) / (1)) * (1 / 0.810)
V2 = 31.5 mL
A:- The volume of 0.810 M KOH required to reach the equivalence point is 31.5 mL
A volume of 50.0 mL of a 0.510 M HNO3 solution is titrated with 0.810 M...