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)

Question

Javion Strong

Chemistry

28 August, 11:54

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)

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Answers (1)

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Ellie Jensen · Answer 1

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.