Chemistry

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 4.50 × 10-4.

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  1. ........HNO2 ==> H^+ + NO2^-
    I.....0.311......0.......0
    C......-x.........x........x
    E.....0.311-x......x......x

    ......KNO2 ==>K^+ + NO2^-
    I.....0.189...0......0
    C....-0.189..0.189...0.189
    E......0.....0.189..0.189

    Ka = (H^+)(NO2^-)/(HNO2)
    Substitue for Ka,
    For (H^+) = x
    For (NO2^-) = x(from HNO2) + 0.189(from KNO2)
    (HNO2) = 0.311-x
    Solve for x = (H^+), then
    %ion = [(H^+)/(0.311)]*100 = ?

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