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chemistry

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You have 20.00 mL of a 0.1M aqueous solution of the weak base (CH3)3N (Kb = 7.4x10^-5). This solution will be titrated with 0.100 M HCl.

How do you find the pH of this solution before any acid has been added.

  • chemistry -

    To save typing I will call (CH3)3N--triethyl amine--RN
    ...........RN + HOH ==> RNH^+ +OH^-
    initial....0.1............0....0
    change.....-x............x......x
    equil......0.1-x.........x......x

    Kb = (RNH^+)(OH^-)/(RN)
    Substitute from the ICE chart above into Ka expression and solve for x = (OH^-) and convert to pH.

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