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March 30, 2017

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A chemist is given an unknown base. She finds that a 1.0461 M aqueous solution of this base has a pH of 13.065 at 25oC. What is the value of Kb for this unknown base ?.

  • Chemistry - ,

    pH = 13.065 = pOH = 0.935
    pOH = -log(OH^-) and (OH^-) = 0.116

    ........BOH ==> B^+ + OH^-
    initial.1.0461...0.......0
    change...-x.....x.......x
    equil.1.0461-x...x.....x

    Kb = (B^+)(OH^-)/(BOH)
    Substitute the ICE chart data into Kb expression and solve for Kb.
    (B) = 0.1161 = (OH^-) and (BOH) = 1.0461-0.1161

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