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Posted by on Monday, March 5, 2012 at 3:47pm.

A 0.035 M solution of a weak base has a pH of 10.88. What is the Kb for the acid?

Where Di I even begun**???

  • Chemistry - , Monday, March 5, 2012 at 4:00pm

    You ALWAYS start with one or all of the following:
    1. balanced equation
    2. ICE chart
    3. think in terms of mols.

    pH = 10.88 so pOH = 3.12 and OH^- = 7.58E-4
    M..........BOH ==> B^+ + OH^-
    initial.0.035M.....0......0
    change..7.58E-4..7.58E-4..7.58E-4
    equil..0.035-7.58E-4....etc

    Kb = (B^+)(OH^-)/(BOH)
    Substitute from the ICE chart and solve for Kb. Note that 0.035-7.58E-4 is not = 0.035

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