Chemistry(Please help)

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What is the pH of 0.144M aqueous solution of ammonium nitrate?

I am not sure what to do. Would I do 10^-0.144^ = 0.71?

  • Chemistry(Please help) -

    No. You go through the hydrolysis equation.
    .........NH4^+ + H2O ==> H3O^+ + NH3

    Ka for NH4^+ = (Kw/Kb for NH3) = (NH3)(H3O^+)/(NH4^+)
    Substitute for NH3 and H3O^+ in the above. Substitute 0.144-x for NH4 and solve for x = (H3O^+), then convert to pH.

  • Chemistry(Please help) -

    so the values for both NH3 and H3O are 0?

  • Chemistry(Please help) -

    No. They are x. And you're solving for x. And you convert x to pH.

  • Chemistry(Please help) -

    For the Ka of NH4^+^ I did 1.0e-14/1.83-5 = 5.55e-10. What do I do with this value?

    So for (NH3)(H3O) / NH4 it would be


  • Chemistry(Please help) -

    Kb = 5.55E-10 so
    5.55E-10 = x^2/0.144-x

  • Chemistry(Please help) -

    oh ok I get it, thank you!!

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