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? asked in Science & MathematicsChemistry · 1 decade ago

What is the pH of a 0.300 M ammonia solution?

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  • 1 decade ago
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    NH3 in water <=> NH4+ & OH-

    (0.300 Molar -x) <=> [X] & [X]

    because the "X" is small, this simplifies to

    NH3 in water <=> NH4+ & OH-

    (0.300 Molar ) <=> [X] & [X]

    Kbase = 1.78 e-5

    from http://www.chemtutor.com/acid.htm#phst

    Kb = [NH4+] [OH-] / [NH3}

    1.78 e-5 = [X] [X] / [0.300]

    X^2 = 5.34 e-6

    X = [OH-] = 2.31 e-3

    pOH = - log of 2.31 e-3

    pOH = 2.636

    since pH + pOH = 14

    pH = 14 - 2.636

    pH = 11.364

    most people only have the Kb good to 2 sig figs

    at which their answer would round off to

    pH = 11.36

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