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Posted by on Sunday, March 28, 2010 at 5:25am.

1.) What must be the molarity of an aqueous solution of trimethylamine (CH3)3N
if it has a Ph of 11.04? Kb = 6.3*10^-5

if someone can show the mechanics of doing this, will be appreciated much.

  • chemistry - , Sunday, March 28, 2010 at 12:55pm

    Think ammonia, NH3.
    NH3 + HOH ==> NH4^+ + OH^-
    Kb = (NH4^+)(OH^-)/(NH3). You've probably solved 100 problem where you know pH of a NH3 solution and you calculate (NH3).

    (CH3)3N does EXACTLY the same thing.
    (CH3)3N + HOH ==> (CH3)3NH^+ + OH^-
    Write Kb expression, look up Kb, calculate OH from pH and solve for (CH3)3N.
    Post your work if you get stuck.

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