Catalysts: Affect the rate of reaching equilibrium but not the position of equilibrium.
Pressure: For gaseous reactions, increasing pressure shifts equilibrium towards the side with fewer moles of gas.
Temperature: Changing temperature affects the equilibrium position depending on whether the reaction is exothermic or endothermic.
Concentration: Adding/removing reactants or products shifts the equilibrium.
Principle: If a system at equilibrium is disturbed by changing conditions, the system will adjust to counteract the disturbance and restore a new equilibrium.
Equilibrium Calculations
ICE Tables: Initial, Change, Equilibrium approach for solving equilibrium problems.
Using K: Solve for unknown concentrations or equilibrium positions.
Biochemical Systems: Metabolic pathways, drug interactions.
Biological Systems: Enzyme-catalyzed reactions, pH regulation in blood.
Bronsted-Lowry Theory
Dynamic Equilibrium: In weak acids/bases, equilibrium is established between the acid/base and its conjugate base/acid.
Weak Acids/Bases: Partially dissociate (low Kₐ or K_b).
Strong Acids/Bases: Completely dissociate in water (high Kₐ or K_b).
Bases: Proton acceptors (H⁺)
Acids: Proton donors (H⁺)
Dynamic Equillibrium
Ongoing Reactions: Both forward and reverse reactions occur continuously.
Constant Concentrations: Not equal, but steady over time.
Definition: A state in a reversible reaction where the rates of the forward and reverse reactions are equal, so concentrations of reactants and products remain constant.
