[_Cassie_]

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.

[AWK]

Use unabbreviated Ostwald dilution law and solve quadratic equation

[Borek]

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).