3 posts • Page 1 of 1
So, HF < HCl < HBr < HI, in order of increasing acidity. So then why is IOH < BrOH < ClOH in order of increasing acidity? I know HF is weaker than the other binary acids going down a column because of weaker bond strength, but then why is IOH less acidic than ClOH? Is it because of electronegativity?
OH is hydroxide. Hydroxide will generally indicate basic solutions, therefore, to address your question, ClOH has the highest acidity relative to the rest because it has the weakest bond strength to the OH molecule, it is the most acidic relative to the rest.
When considering oxoacids particularly, the one with the more electronegative halogen is more acidic. If you consider the end result of an acid dissociation, a complete dissociation of a strong acid comes to be partially because the conjugate base is stable. Therefore, we can look at the relative stabilities of IO-, BrO-, and ClO-. We would expect ClO- to be the most stable of the three because the high electronegativity of the chlorine atoms allows for the electron density to be more spread out. Since ClO- is a more stable product, we would expect the greatest acid dissociation from ClOH, making it the strongest acid.
Who is online
Users browsing this forum: No registered users and 1 guest