• Definition: ICE Tables (Initial, Change, Equilibrium) are a systematic method to track the concentrations of reactants and products in a chemical reaction at different stages - initial, change, and equilibrium.

• Purpose: ICE Tables simplify the process of solving for unknowns in equilibrium problems, especially in acid-base reactions, solubility equilibria, and other reversible reactions.

Key Concepts of ICE Tables

• Initial Concentrations: The concentrations of reactants and products at the start, before the reaction reaches equilibrium.

• Change in Concentrations: The increase or decrease in concentrations of reactants and products as the reaction proceeds towards equilibrium.

• Equilibrium Concentrations: The final concentrations of reactants and products when the reaction is at equilibrium.

Steps for Using ICE Tables

• Write the Balanced Equation: Ensure the chemical equation for the reaction is balanced.

• Determine Initial Concentrations: List the initial molar concentrations or partial pressures of reactants and products.

• Identify Changes: Represent the changes in concentration as variables (e.g., -x for reactants, +x for products).

• Apply the Equilibrium Constant: Use the expression for K (equilibrium constant) to relate the changes in concentration.

• Solve for the Unknowns: Calculate the unknown variable (often x) and find the equilibrium concentrations.