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The pH of a 0.150 M solution of a weak base is 10.98. Calculate the pH of a 0.04 M solution of the base.?

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  • Bobby
    Lv 7
    1 month ago

    [OH-] = SQRT(Kb*c) / pOH = 14 - 10.98 = 3.02

    10^-3.02 = SQRT (Kb *0.150)

    9.55E-04 = Kb /0.150

    Kb= 1.43 * 10 ^-4

    in the second solution

     [OH-] = SQRT( 1.43 * 10 ^-4 * 0.04)

     = 2.39E-03

    pOH = 2.62

    pH = 11.4  .... your answer  

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