Here is what should be an easy problem that I am somehow messing up 1. The problem statement, all variables and given/known data Calculate the percent dissociation of 0.063 M Hydrobromous acid, HBrO. Do not solve the quadratic equation even if the percent dissociation is high. 2. Relevant equations 3. The attempt at a solution I looked up K_a and found it to be 2.3*10^-9. After doing an equilibrium chart I got that x^2 = (2.3*10^9)(0.63). Therefore, x = 1.20 * 10^-5. I then divided this by 0.063 and multiplied by 100. I got 0.02% as a final answer. This does not sound right due to the hint and I was told it was wrong (online homework. For the equilibrium table I just assumed that HBrO + H2O <--> H3O + BrO. Thanks for any help. I don't know why I am having so much trouble with this one.