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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: sarahjane on March 18, 2004, 07:12:35 PM

Title: Acetic Acid Dissociation Contant calculation question
Post by: sarahjane on March 18, 2004, 07:12:35 PM

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

Title: Re:hey im confused
Post by: Donaldson Tan on March 19, 2004, 05:44:04 AM

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)