Waiting for answer This question has not been answered yet. You can hire a professional tutor to get the answer.

QUESTION

# Which is the strongest acid among these: HBr, HF, HI, and HCl?

Acidity increases in the order: HF, HCl, HBr, HI. Note that in water dissociation is fairly complete.

Acidity may be related to the reaction:

HA rightleftharpoonsH^+ + A^-

The stronger the acid; the further to the right lies this equilibrium. Of course, the acidity is modified by the identity of the . In water, the acid base reaction is often represented as:

HX(g) + H_2O(l)rightleftharpoonsH_3O^+ + X^(-)

In water, for all the hydrogen halides, EXCEPT for HF, the equilibrium would lie almost quantitatively to the right. We could measure [H^+] or its equivalent in another solvent, say acetic acid, and we would find the order of acidity as HI>HBr>HCl>HF.

This clearly relates to the of the H-X bond, and also to an effect. The larger halides, X^-, are entropically favoured in that they are less charge dense, and cause less solvent order upon solvolysis.