chemistry

What is the pH of a 2.23 M HCHO2, formic acid, aqueous solution at 25 °C? ( Ka = 1.8E-4 )

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  1. ............HCOOH ==> H^+ + HCOO^-
    begin....... 2.23M....0.......0
    change.......-x.......x........x
    final......2.23-x.....x........x

    Ka = (H^+)(HCOO^-(/(HCOOH)
    Substitute from the ICE chart into Ka expression and solve for (H^+). Convert to pH.

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