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I am very confused about how to start this problem:

A 29.8 mL sample of 0.354 M methylamine, CH3NH2, is titrated with 0.231 M hydrochloric acid.

The pH before the addition of any hydrochloric acid is ?.
The Kb of methylamine is 4.2x10^-4

  • Chemistry -

    ........MeNH2 + HOH ==> MeNH3^+ + OH^-

    Kb = (MeNH3)(OH^-)/(MeNH2)
    Substitute and solve for OH^- and convert to pH.

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