Post a New Question

Chemistry

posted by .

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

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

More Related Questions

Post a New Question