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.

a. Equilibrium shifts to the left.

b. Equilibrium shifts to the left.

Explanation:

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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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the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.