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Acetic Acid Dissociation Contant calculation question

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sarahjane:
a 0.01M solution of acetic acid is 4.17% ionised.calculate the dissociation constant of acetic acid?????how do you do this??????






Edit: Editied subject title to help with indexing. Mitch

Donaldson Tan:
The degree of dissociation is 4.17%.

So Ka
= [H+][Acetate]/[Undissociated Acetic Acid]
= (0.0417x0.01)(0.0417x0.01)/[(1 - 0.0417)x0.01]
= (0.0417)(0.0417)(0.01)/0.9583
= 1.81 X 10^(-5)

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