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Since Flourine is such a small molecule, the bond between fluorine and the hydrogen is the shortest when comparing the other halogen-based acids. This would mean that it is much more difficult to break this bond and thus less H+ exist in an aqueous solution of HF.
Another way to look at this is the trend for binary acids within the same group is bond strength. A weaker(longer) bond between the anion and H allows for easier removal of H+ which means that it is a stronger acid because it can dissociate more in water. HF is a weak acid because H-F is a short, strong bond which causes it to be unable to completely dissociate in water. Following this same logic, you would find that for the halogen group, the order of acid strength is HF < HCl < HBr < HI.
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