Using qualitative reasoning for the acid–base reactions shown,
(i) which is stronger, the acid or the conjugate acid?
(ii) Which side of the reaction is favored?
(iii) Would you expect a K_eq greater than, equal to, or less than 1?
(a)

검증된 단계별 안내

Step 1: Identify the acid and the conjugate acid in the reaction. The acid is the species donating a proton (H⁺), and the conjugate acid is the species formed when the base accepts a proton.

Step 2: Compare the relative strengths of the acid and the conjugate acid using pKa values. Recall that a lower pKa value indicates a stronger acid. Use qualitative reasoning to determine which is stronger.

Step 3: Determine which side of the reaction is favored. Acid-base reactions favor the side with the weaker acid and weaker base. Use the relative strengths of the acid and conjugate acid to predict the favored side.

Step 4: Analyze the equilibrium constant (K_eq) qualitatively. If the reaction favors the products, K_eq > 1. If it favors the reactants, K_eq < 1. If both sides are equally favored, K_eq ≈ 1.

Step 5: Conclude whether K_eq is greater than, equal to, or less than 1 based on the favored side of the reaction and the relative acid strengths.

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주요 개념

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Acid-Base Strength

Acid-base strength is determined by the ability of an acid to donate protons (H+) and the ability of a base to accept protons. Strong acids completely dissociate in solution, while weak acids only partially dissociate. The strength of an acid is often compared to its conjugate base, where a stronger acid has a weaker conjugate base, and vice versa.

Equilibrium and Reaction Favorability

In acid-base reactions, the position of equilibrium indicates which side of the reaction is favored. The side with the weaker acid and weaker base is favored, as this corresponds to a lower energy state. The equilibrium constant (K) can be used to quantify this favorability, with values greater than 1 indicating a preference for products.

Quantitative Analysis of K

The equilibrium constant (K) for an acid-base reaction provides insight into the relative strengths of the acids and bases involved. If K is greater than 1, the products are favored, indicating that the reaction proceeds to the right. Conversely, if K is less than 1, the reactants are favored, suggesting that the reaction does not proceed significantly toward products.

Using qualitative reasoning for the acid–base reactions shown,(i) which is stronger, the acid or the conjugate acid?(ii) Which side of the reaction is favored?(iii) Would you expect a Keq greater than, equal to, or less than 1?(a)