Giving stable examples explain the terms conjugated acids and conjugated base
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A conjugate acid, within the Brønsted–Lowry acid–base theory, is a chemical compound formed by the reception of a proton (H+) by a base—in other words, it is a base with a hydrogen ion added to it. On the other hand, a conjugate base is what is left over after an acid has donated a proton during a chemical reaction. Hence, a conjugate base is a species formed by the removal of a proton from an acid. Because some acids are capable of releasing multiple protons, the conjugate base of an acid may itself be acidic.
In summary, this can be represented as the following chemical reaction:
Acid + Base ⇌ Conjugate Base + Conjugate Acid
HNO3 + H2O → H3O+ + NO−3
Nitric acid (HNO3) is an acid because it donates a proton to the water molecule and its conjugate base is nitrate (NO−3). The water molecule acts as a base because it receives the Hydrogen Proton and its conjugate acid is the hydronium ion (H3O+).
