Question

CH3CO2H(aq) + H2O(l) ⇄ CH3CO2-(aq) + H3O+(l)

As acetic acid dissolves in water, the acetate ion and hydroniium ion are produced. Predict the direction that the equilibrium position will shift to reattain equilibrium as the acetic acid concentration is increased.

A) The equilibrium position will remain unchanged and not shift.
B) The equilibrium position will shift to the left toward the reactants.
C) The equilibrium position will shift to the right toward the products.
D) The equilibrium position will shift in small increments to both sides

Answer 1

b

Step-by-step explanation:

b

Answer 2

Correct Answer: Option C: The equilibrium position will shift to the right toward the products.

Reason:
1) This problem is based on Le Chatelier's principle. It is stated as 'any changes in the temperature, volume, or concentration of a system will result in predictable and opposing changes in the system in order minimize this change and achieve a new equilibrium state.'

2) In present case, the reaction involved is:
CH3CO2H(aq) + H2O(l) ⇄ CH3CO2-(aq) + H3O+(l)
Hence, when the concentration of acetic acid (reactant) is increased, the equilibrium will shift to right to minimize the effect of change in concentration of reactant.