Write the equilibrium constant expression for this reaction:2H+(aq)+CO2−3(aq) → H2CO3(aq

Break Down the Problem

1. Identify the reactants and products in the given chemical reaction.
2. Understand what the equilibrium constant expression represents.

Relevant Concepts

1. The equilibrium constant expression (K) for a reaction is given by the ratio of the concentrations of the products raised to the power of their coefficients to the concentrations of the reactants raised to the power of their coefficients.
2. The reaction provided is: $2 \text{H}^+(aq) + \text{CO}_3^{2-}(aq) \rightleftharpoons \text{H}_2\text{CO}_3(aq)$

Analysis and Detail

1. In this reaction:
   • Reactants: $2 \text{H}^+(aq)$ and $\text{CO}_3^{2-}(aq)$
   • Product: $\text{H}_2\text{CO}_3(aq)$
2. The equilibrium constant $K_c$ for the reaction can be expressed as: $K_c = \frac{[\text{H}_2\text{CO}_3]}{[\text{H}^+]^2 [\text{CO}_3^{2-}]}$ where:
   • $[\text{H}_2\text{CO}_3]$ is the concentration of carbonic acid.
   • $[\text{H}^+]$ is the concentration of hydrogen ions, raised to the power of 2 due to its coefficient.
   • $[\text{CO}_3^{2-}]$ is the concentration of carbonate ions.

Verify and Summarize

1. Check that the coefficients of each species in the balanced equation are correctly represented in the equilibrium constant expression.
2. Summarize that the expression correctly reflects the relationship between the reactants and products in the reaction.

Final Answer

The equilibrium constant expression for the reaction: $2 \text{H}^+(aq) + \text{CO}_3^{2-}(aq) \rightleftharpoons \text{H}_2\text{CO}_3(aq)$ is given by: $K_c = \frac{[\text{H}_2\text{CO}_3]}{[\text{H}^+]^2 [\text{CO}_3^{2-}]}$