Question

Write a net ionic equation to show that nitrous acid behaves as a brønsted-lowry acid in water.

Answer 1

Step-by-step explanation:

According to Bronsted-Lowry an acid is defined as the specie which is able to donate hydrogen ions when dissolved in water.

For example,
`HNO_(2) + H_(2)O \rightarrow H_(3)O^(+) + NO^(-)_(2)`

Chemical formula of nitrous acid is
`HNO_(2)` . Since, it donates a hydrogen ion in water hence, it acts as a Bronsted-Lowry acid.

On the other hand, bases are the species which are able to accept hydrogen ions when dissolved in water.

For example,
`NH_(3) + H_(2)O \rightarrow NH^(+)_(4) + OH^(-)`

Answer 2

Balanced chemical reaction: HNO₂(aq) + H₂O(l) ⇄ NO₂⁻(aq) + H₃O⁺(aq).
According to Bronsted-Lowry theory acid are donor of protons and bases are acceptors of protons (the hydrogen cation or H⁺).
Nitrous acid is weak Bronsted acid and it can lose proton and become conjugate base NO₂⁻ and water is Bronsted base.