Question

There is a dual equilibrium between the indicator methyl orange (Hln/In-) and acetic acid HC2H3O2(aq) and acetate NaC2H3O2. The acetic acid/sodium acetate equilibrium is:

HC2H3O2(aq)+ H2O(l) ⇌ C2H3O- (aq) + H3O+(aq)

a. How will the addition of acid (H3O+) affect this equilibrium? Explain in words how this changes the concentration of any reactants or products and then draw an arrow to show if the equilibrium shifts to the right or left.
b. How will the addition of sodium acetate NaC,H,O2 (aq) affect this equilibrium? Explain in words how this changes the concentration of any reactants or products and then draw an arrow to show if the equilibrium shifts to the right or left.

Answer 1

a. Equilibrium shifts to the left.

b. Equilibrium shifts to the left.

Step-by-step explanation:

Hello.

a. In this case, considering the Le Chatelier's principle which states that the addition of any product shifts the reaction towards the reactants in order to reestablish equilibrium, by the addition of H₃O⁺ we are adding a product, it means that the equilibriums shifts to the left.

b. In this case, since the addition of sodium acetate releases sodium ions and acetate ions, because it is totally ionized, such released acetate ions have the capacity to shift the equilibrium to left as it is a product as well as the H₃O⁺, therefore, adding sodium acetate shifts the equilibrium to the left, by also considering the Le Chatelier's principle.

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