Predict the direction of the following reaction: HC 2 H 3 O 2 (aq) + H 2 O (liq) ______________ H 3 O + (aq) + C 2 H 3 O 2 – (aq)

Here it says, predict the direction of the following reaction. So here we have acetic acid reacting with water to reduce h three o plus, which is your hydronium ion, plus the acetate ion. Acetic acid is a weak acid. And remember, if you're a weak acid or a weak base, reactants are highly favored. So that means we'd have the larger arrow pointing towards the reactants and a smaller arrow pointing towards the products. The smaller arrow indicates that not much of that product is formed. Here out of the options, the one that looks most like that is option d. So remember, this indicates that we're dealing with the weak species. Whether it's a weak acid or weak base, the reactant side is more favored, and therefore has a larger arrow pointing towards it.

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10. Acids and Bases

Acid and Base Strength

GOB Chemistry

10. Acids and Bases

Acid and Base Strength

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Multiple Choice

Predict the direction of the following reaction:
HC₂H₃O₂ (aq) + H₂O (liq) ______________ H₃O⁺ (aq) + C₂H₃O₂^– (aq)

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Verified step by step guidance

Identify the acid and base on both sides of the reaction. In this case, HC2H3O2 (acetic acid) is the acid, and H2O is the base on the reactant side. On the product side, H3O+ is the conjugate acid, and C2H3O2– is the conjugate base.

Determine the strength of the acids and bases involved. Acetic acid (HC2H3O2) is a weak acid, and its conjugate base (C2H3O2–) is relatively stronger. Water (H2O) is a very weak base, and its conjugate acid (H3O+) is a stronger acid.

Use the concept of equilibrium to predict the direction of the reaction. In an acid-base reaction, the equilibrium will favor the formation of the weaker acid and base. Since H3O+ is a stronger acid than HC2H3O2, the equilibrium will favor the reactants.

Consider the equilibrium constant (Ka) for acetic acid. A small Ka value indicates that the reaction favors the reactants, meaning the reverse reaction is more likely.

Conclude that the reaction will favor the formation of the reactants, meaning the equilibrium lies to the left. This is consistent with the fact that acetic acid is a weak acid and does not dissociate completely in water.