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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14. Acids and Bases

Acid and Base Strength

Introduction to Chemistry

14. 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 components of the reaction: HC2H3O2 (acetic acid) and H2O (water) are the reactants, while H3O+ (hydronium ion) and C2H3O2– (acetate ion) are the products.

Understand that this is an acid-base reaction where acetic acid donates a proton to water, forming hydronium and acetate ions.

Consider the strength of acetic acid as a weak acid, which means it does not completely dissociate in water.

Recognize that the equilibrium position of the reaction depends on the relative concentrations of the reactants and products, as well as the acid dissociation constant (Ka) of acetic acid.

Use the concept of equilibrium to predict the direction: if the reaction mixture initially contains more reactants than products, the reaction will proceed forward to form more products until equilibrium is reached.