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Chem 2

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What is the approximate value of the K for the neutralization of nitrous acid with ammonia? Ka for the acid is 0.00045 and Kb for the base is 0.000018.

Do I multiply Ka*Kb?

  • Chem 2 - ,

    I think that is the hydrolysis constant which is Kw/(KaKb).

  • Chem 2 - ,

    Frist write out what is given:
    HNO2 ⇌ H+ + NO2-
    Ka = 0.00045 = [H+]*[NO2-]/[HNO2]
    and:
    NH3 + H2O ⇌ NH4+ + OH-
    Kb = 0.000018 = [NH4+]*[OH-]/[NH3]

    What is asked for is the K value for:
    HNO2 + NH3 ⇌ NH4+ + NO2-

    K = [NH4+]*[NO2-]/{ [HNO2]*[NH3] }
    = { [NH4+]*[OH-]/[NH3] }*{ [H+]*[NO2-]/[HNO2] }/{ [H+]*[OH-] }
    = Kb*Ka/Kw
    where Kw = [H+]*[OH-] = 10^-14.
    Is that very easy? Please finally do the very simple math.

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