hydrogen halides are acidic in nature why what is the order of acidic strength in different hydrogen halide and why
Answers
Answer:
HCl is a very strong acid, and HBr even more so. HF is the only weak acid. This is because it binds hydrogen much more strongly then the other halides.
The effect decreases with larger halide ions. Very strong hydrogen bonding exists between the hydrogen fluoride molecules and water molecules. This costs a large amount of energy to break.
Acid strength can be determined by the stability of the conjugate base (for most acids, the conjugate base is what you get when you remove H+ from the acid). In this case the conjugate bases are the halides.
As the size of the halide ion increases, the charge is dispersed over a larger volume, and thus the ion is more stable. In this manner, one can say that the order of acid strengths is HF<HCl<HBr<HI (I’m not considering the radioactive ones here; they fit in the same trend though).
HCl,HBr,HI are all strong acids. HCl has a pKa of −7 (the smaller the pKa is, the more acidic it is), HBr is approximately −9, and HI is also approx −9.
On the other hand, HF is 3.2. The H−F bond is pretty strong, so it has a smaller tendency to dissociate—making it a weak acid (not to say that it isn’t dangerous
Answer:
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Explanation:
No, it can’t be generalised. Amongst the haloacids, only HF is weak.
Acid strength can be determined by the stability of the conjugate base (for most acids, the conjugate base is what you get when you remove H+ from the acid). In this case the conjugate bases are the halides.
As the size of the halide ion increases, the charge is dispersed over a larger volume, and thus the ion is more stable. In this manner, one can say that the order of acid strengths is HF<HCl<HBr<HI (I’m not considering the radioactive ones here; they fit in the same trend though).
HCl,HBr,HI are all strong acids. HCl has a pKa of −7 (the smaller the pKa is, the more acidic it is), HBr is approximately −9, and HI is also approx −9.
On the other hand, HF is 3.2. The H−F bond is pretty strong, so it has a smaller tendency to dissociate—making it a weak acid (not to say that it isn’t dangerous).
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