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What is the pH of a .10M (CH3)3N solution? Kb=6.40e-5

  • chemistry - ,

    (CH3)3N + HOH ==> (CH3)3NH^+ + OH

    Kb = [(CH3)3NH^+](OH^-)[CH3)3N]
    Set up ICE chart, substitute into Kb expression above and solve for OH, convert to pH. Post your work if you get stuck.

  • chemistry - ,

    I did my ice chart and found x=.00253
    then i did the -log(.00253) to find the pH to be 2.597, but that's the wrong answer

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