Question

Calculate the percent ionization of nitrous acid in a solution that is 0.311 M in nitrous acid (HNO2) and 0.189 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is
4.5 × 10^-4 Calculate the percent ionization of nitrous acid in a solution that is 0.311 M in nitrous acid (HNO2) and 0.189 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is
4.5 × 10^-4 @Chemistry

Answer 1

You know this is a weak acid.
Use the ICE table.
Reaction HNO2 <-> H+ + NO2-
I: Initial concentration .31 0 0
Change -x +x +x
Equilibrium .31-x x x
4.5 x 10-4 = [x][x]/.31-x
Assume .31-x is almost .31
Solve for x
4.5x 10-4 = x2

Answer 2

x will give you the fraction of ionization.