Chemical Forums
Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: _Cassie_ on June 01, 2005, 11:30:53 PM
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Hey all,
I am trying to work out the following question:
What is the percent ionization of the acid in a 0.0005M solution of acetylsalicyclic acid (aspirin) with a Ka of 3.0 by 10 to the negative 4.
Not sure if this is the way you work it out, but I worked out the [H3O+] and got an answer of 0.019535. I then substituted divided that by the original concentration of the aspirin and multiplied by 100%.
The answer I got was huge, and abviously not right... Can anybody help me?
Cassie.
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Use unabbreviated Ostwald dilution law and solve quadratic equation
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Not sure if this is the way you work it out, but I worked out the [H3O+] and got an answer of 0.019535.
This is obviously wrong - concentration of H+ is larger than the concentration of acid (and we are far from the area where such effect is justified by the water autoionization).