Question

Write a net ionic equation to show that acetylsalicylic acid (aspirin), hc9h7o4, behaves as a brønsted-lowry acid in water.

Answer 1

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

1. An acid is defined as a substance which looses donates protons and thus forming conjugate base.
2. A base is defined as a substance which accepts protons and thus forming conjugate acid.

Acetylsalicylic acid when dissolved in water donates its proton to form conjugate base and water gains the proton to form conjugate acid.The net ionic equation is given as:

$HC_9H_7O_4(0+H_2O\rightarrow (C_9H_7O_4)^{-}+H_3O^+$

Answer 2

Balanced chemical reaction of aspirin in water:
HC₉H₇O₄(aq) + H₂O(l) ⇄ C₉H₇O₄⁻(aq) + H₃O⁺(aq).
In this chemical reaction aspirin(HC₉H₇O₄) is an acid because it donates a proton (H⁺) to water and becomes its conjugate base (C₉H₇O₄⁻) and water is a base because it accepts a proton from aspirin and becomes its conjugate acid, the hydronium ion, (H₃O⁺).