Acid Folk
'I have been told HBr acid is stronger than HCl acid' is this assumption right?
my reasoning is that:
HBr has a larger atomic radius,
and increased nuclear charge (compared to HCl)
however, has increased electron shielding,
therefore, less electrostatic attraction between its nucleus and surrounding electrons,
therefore, bond between H and Br is weaker (than H and Cl in HCl) (also as Br is less electronegative than Cl)
therefore, it is more likely to break,
therefore, it is a stronger acid
just confirm is this is right, or if i have missed anything out. Bearing in mind this is A-level chemistry... cheers folks
but hold on.... surely the more electronegative the halide ion, the better the acid would be, like HF would be a stronger acid than HCl would it not?
Strength of these halogen acids in aqueous solutions increases in the order: HF < HCl < HBr < HI. In this order the H-X bond strength decreases, perceivably due to increase in the size of X (indeed your good reasoning). by the same logic, HBr bond is less stronger than HCl.
Hydrofluoric acid is much weaker than the others -- H-F bond is much stronger than the O-H bond of water; also, HF molecule is stabilized more by its hydrogen bonding in aqueous solutions (most electronegative elements form stronger hydrogen bonds) and this further reduces its acid strength.
This is for your additional reading
Further, acid strength = dehydration energy + dissociation energy + ionization energy of H+ plus electron affinity of X- plus energy of Hydration of H+ and X-
The molecules should be supplied with energy for ionisation and dissociation processes.
By this we understand that hydration
HX ---> H+ (hydrated) + X- (hydrated)
and electron affinity release energy and this energy should be sufficient to offset other terms given above ( ionisation and dissociation processes).Hydration energy and electron affinity of Br- (-347 and -324) is lesser than those of Cl- (-381 and -348 kJ/mol).
This gives a negative total enthalpy value and negative free energy values. HBr has total enthalpy of -64 and HCl has -60 kJ/mol.
More negative enthalpy and hence more negative free energy make the acid HBr dissociation more favorable.
Thermodynamically, these terms determine the acid strengths of HBr and HCl.
Therefore, it is not the electronegativity of X that determines the acid strength in aqueous solution, as is often misunderstood.
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