Write a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each. (a) AgI in aqueous NaCN to form [Ag(CN)2]-

Verified step by step guidance

1. Identify the dissolution reaction: AgI(s) dissolves in NaCN to form [Ag(CN)_2]^-.
2. Write the balanced chemical equation for the dissolution: AgI(s) + 2CN^-(aq) -> [Ag(CN)_2]^-(aq) + I^-(aq).
3. Write the net ionic equation by removing spectator ions: AgI(s) + 2CN^-(aq) -> [Ag(CN)_2]^-(aq) + I^-(aq).
4. Use the solubility product constant (K_{sp}) for AgI and the formation constant (K_{f}) for [Ag(CN)_2]^- to find the equilibrium constant (K_{eq}).
5. Calculate K_{eq} using the formula: K_{eq} = K_{sp} * K_{f}.

Key Concepts

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions. It focuses on the ions and molecules that undergo a change during the reaction, providing a clearer picture of the chemical processes. For dissolution reactions, this involves identifying the ions that form in solution and their interactions.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that quantifies the solubility of a sparingly soluble ionic compound. It is derived from the concentrations of the ions in a saturated solution at equilibrium. Understanding Ksp is crucial for predicting whether a precipitate will form when solutions are mixed and for calculating the concentrations of ions in solution.

Formation Constant (Kf)

The formation constant (Kf) is a measure of the stability of a complex ion in solution, representing the equilibrium between the complex and its constituent ions. A higher Kf value indicates a more stable complex. In the context of the given question, Kf is used to calculate the equilibrium constant for the formation of the complex ion [Ag(CN)2]-, which is essential for understanding the reaction's dynamics.