For the following acid–base reaction, (b) calculate the equilibrium constant.

Verified step by step guidance

1. Identify the acid and base on both sides of the reaction. Determine the conjugate acid and conjugate base formed after the reaction.
2. Look up the pKa values of the acid on the reactant side and the conjugate acid on the product side. These values are essential for calculating the equilibrium constant.
3. Use the relationship between the equilibrium constant (K_eq) and the pKa values: \( K_{eq} = 10^{\text{pKa (acid on product side)} - \text{pKa (acid on reactant side)}} \).
4. Substitute the pKa values into the equation. Ensure that the pKa values are correctly assigned to the respective acids.
5. Simplify the expression to calculate \( K_{eq} \). This will give you the equilibrium constant for the acid-base reaction.

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In these reactions, acids donate protons while bases accept them. Understanding the nature of the acids and bases involved is crucial for predicting the direction of the reaction and calculating equilibrium constants.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is calculated using the formula K = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. A larger K value indicates a reaction that favors products, while a smaller K suggests a preference for reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is essential for understanding how changes in concentration, pressure, or temperature affect the position of equilibrium and, consequently, the value of the equilibrium constant.