Question

In the reaction between `NO_2^(-)` and water, which species is the acid?

Answer 1

The `"Bronsted acid"` is the proton donor....

Explanation:

And as written....

`NO_2^(-) + H_2O(l) rightleftharpoons HNO_2(aq) + HO^-`

....the `"water molecule"` is the `"Bronsted acid"`, `"the proton donor...."`

Do you agree?

Which is the `"Bronsted base"`?

Answer 2

In the reaction between `NO_2^(-)` and water, which species is the acid?

Explanation:

The Bronted acid always donates a proton.

`underbrace(NO_2^(-))_"conjugate base" +H_2O -> underbrace(HNO_2)_"parent acid" + OH^-`

In this case, water donates a hydrogen to `NO_2` to make `HNO_2`. Water then becomes `OH^-` since it lost one hydrogen.