Question:

Dissociation and pH ?

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For Propanoic acid (HC3H5O2, Ka = 1.3 x 10^-5)

1) Determine concentration of species present

2) Determine pH

3) Determine percent dissociation of a 0.100 M solution

Just the general concept of the steps with terms that I can recognize would be great.

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  1. HC3H5O2 <------> C3H5O2- + H+

    initial conc.

    0.100

    at equilibrium

    0.100-x ,, , , , , , , , , x . . . . . . x

    1.3 x 10^-5 = x^2 / 0.100-x

    x = [C3H5O2-] = [H+] = 0.0011 M

    [HC3H5O2 ] = 0.100 - 0.0011 =0.0989 M

    pH = - log 0.0011 =3.0

    0.0011 x 100 / 0.100 =1.1 %  

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