Of the following acids, the one that is strongest is:a)HBrO4b)HOC1c)HNO2d)H3PO3Correct answer is option 'A'. Can you explain this answer?

Question

Answer

Higher the oxidation no. of the central atom, stronger is the acid..
Here, Br=+7
Cl=+1
N=+3
P=+3
Thus HBrO4 is the strongest acid amongst the given alternatives..

Answer

BrO4(-) is very much resonance stable that is why HBrO4 is strongest acid among those

Answer

Explanation:

Definition of Acid Strength:
Acid strength refers to the tendency of an acid to donate a proton (H+) to a base. Strong acids are those that completely dissociate in water, while weak acids only partially dissociate.

Factors Affecting Acid Strength:
1. Bond Strength: The strength of the bond between hydrogen and the rest of the molecule affects acid strength. Weaker bonds are more likely to dissociate and release H+ ions, making the acid stronger.
2. Electronegativity: The electronegativity of the atom to which hydrogen is bonded also affects acid strength. More electronegative atoms are better at stabilizing the negative charge that results from the dissociation of the acid.
3. Resonance: Acids with resonance structures are more stable, making them weaker acids.
4. Inductive Effect: The presence of electron-withdrawing groups near the acidic hydrogen atom makes the acid stronger.

Comparison of Acids:
Now let's compare the given acids to determine the strongest one:

a) HBrO4 (Perbromic Acid):
- Bromine (Br) is highly electronegative, so it can stabilize the negative charge after dissociation.
- Perbromic acid has a weak O-H bond, which is likely to dissociate easily.
- It does not have any resonance structures and there are no electron-withdrawing groups near the acidic hydrogen atom.

b) HOCl (Hypochlorous Acid):
- Chlorine (Cl) is moderately electronegative, so it can stabilize the negative charge after dissociation.
- Hypochlorous acid has a weak O-H bond, which is likely to dissociate easily.
- It does not have any resonance structures and there are no electron-withdrawing groups near the acidic hydrogen atom.

c) HNO2 (Nitrous Acid):
- Nitrogen (N) is moderately electronegative, so it can stabilize the negative charge after dissociation.
- Nitrous acid has a weak O-H bond, which is likely to dissociate easily.
- It does not have any resonance structures and there are no electron-withdrawing groups near the acidic hydrogen atom.

d) H3PO3 (Phosphorous Acid):
- Phosphorous (P) is less electronegative compared to bromine, chlorine, and nitrogen, so it is less capable of stabilizing the negative charge.
- Phosphorous acid has relatively stronger P-H bonds, which are less likely to dissociate easily.
- It does not have any resonance structures and there are no electron-withdrawing groups near the acidic hydrogen atom.

Conclusion:
Among the given acids, HBrO4 (Perbromic Acid) is the strongest acid. It has the weakest O-H bond and the most electronegative atom (bromine) to stabilize the negative charge after dissociation.

Answer

According to bronsted acid concepts,  br can easily donate proton.  so opt a is more acidic

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