Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow: (c) HCO3-1aq2 + F-1aq2 Δ

Verified step by step guidance

1. Identify the acid and base on the reactant side. In this case, \( \text{HCO}_3^- \) can act as an acid, and \( \text{F}^- \) can act as a base.
2. Determine the conjugate base of the acid and the conjugate acid of the base. \( \text{HCO}_3^- \) will donate a proton to become \( \text{CO}_3^{2-} \), and \( \text{F}^- \) will accept a proton to become \( \text{HF} \).
3. Write the balanced chemical equation for the reaction: \( \text{HCO}_3^- + \text{F}^- \rightleftharpoons \text{CO}_3^{2-} + \text{HF} \).
4. Consider the relative strengths of the acids and bases involved. \( \text{HF} \) is a weak acid, and \( \text{HCO}_3^- \) is a weaker acid compared to \( \text{HF} \).
5. Predict the direction of the equilibrium. Since \( \text{HF} \) is a stronger acid than \( \text{HCO}_3^- \), the equilibrium will lie to the left, favoring the formation of reactants.

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, an acid donates a proton while a base accepts it. Understanding the roles of acids and bases is crucial for predicting the products of the reaction and determining the direction of equilibrium.

Equilibrium Position

The position of equilibrium in a chemical reaction indicates the relative concentrations of reactants and products at equilibrium. If the equilibrium lies to the right, products are favored, while a leftward shift indicates that reactants are favored. Factors such as concentration, temperature, and the nature of the reactants influence this position.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of an acid and its corresponding base that differ by a single proton. In the given reaction, HCO3- acts as a weak acid and F- as a base. Recognizing these pairs helps in predicting the products and understanding the strength of the acids and bases involved, which is essential for determining the direction of equilibrium.