Acetic acid is the active ingredient in vinegar. in a solution of acetic acid the following equilibrium is established. hc2h3o2(aq) < --> h+(aq) + c2h3o2-(aq) the equilibrium constant for this reaction is 1.8 x 10–5. what is the equilibrium constant for the following reaction ? h+(aq) + c2h3o2-(aq) < --> hc2h3o2(aq)

the equilibrium constant is 1.8 x 10⁻5 and strongly favor the reactants.

Explanation:

the chemical reaction provided for the two equation are the same but different direction i.e a reversible reaction. Assuming, the mass of reactants and product and temperature remain constant.

therefore, the equilibrium constant K, is 1.8 x 10⁻5. this is a very small value of K, thereby strongly favor the backward direction to form reactant.

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