Question

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)

Answer 1

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

Step-by-step 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.