Question

acidic strength of nitrous acid ​

Answer 1

Answer:

Ka Acid Base

1.3 * 10-2 Sulfurous acid HSO3 -

1.0 * 10-2 Hydrogen sulfate ion SO4 2-

7.1 * 10-3 Phosphoric acid H2PO4 -

7.2 * 10-4 Nitrous acid NO3 -

Answer 2

Answer:

in NO2−, the resonance effect is pronounced, but in the case of NO3−, we have a case of cross resonance. Put simply, in NO2− the negative charge de-localizes to double bonded oxygen atom. In the case of NO3−, same thing happens, but we have another O−

here due to which there is a cross of 2 resonance effects (If I am using the correct terminology). So, resonance effect of nitrate ion should be weaker than nitrite ion and therefore nitrite ion should be more stable.

If I am true then nitrous acid must be a stronger acid, but all my sources suggest otherwise. They insist that in NO3−

, the negative charge is distributed over 3 oxygen atoms, and hence its resonance is more powerful. My confusion is that there are also 2 negatives that need to be stabilized as opposed to one negative in NO2−.

Explanation:

actually I have compared nitrous acid with nitric acid hope it helps.