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Big Idea #6 “Any bond or intermolecular attraction that can be formed can be broken. These two processes are in dynamic competition, sensitive to initial concentration and external perturbations.” Concepts: • • • • • • • • • Equilibrium expression, magnitude of K Le Chatelier’s Principle Reaction Quotient Multistep process ( relationship of equilibrium constant) Ksp Common Ion Effect Acid/Base Equilbria Buffers Titration Equilibrium Review Key topics: •Equilibrium expression •Equilibrium Constant (Kc) •Gas Equilibrium (Kp) •Relationship Kc- Kp •ICE charts (molar relationships) •Reaction Quotient (Q) •Le Chatelier’s Principle •Solubility Constant (Ksp) Equilibrium expression and Kc • • • • Coefficients are used as exponents. Describe concentrations of (aq) and (g) only. Kc = [products]/[reactants] Kc > 1 means equilibrium favors forward direction (formation of product) • Kc < 1 describes an equilibrium that favors reverse reaction (formation of reactants) • Kc =1 system is at equilbrium Relationship: Kc & Kp • Kc = equilibrium concentrations • Kp = equilibrium pressure (gas systems only) • Kp = Kc(RT) Δn (difference in coefficient gaseous products and reactants) ICE charts • Stoichiometric relationship of reactants: products • Assume reaction occurs in the forward direction. • Some strategies: – Perfect square – Quadratic equation – 5% rule (used when K is very small-compared to initial concentration) Reaction Quotient (Q) • Used to determine the direction required for a system to achieve equilibrium. • Q<K - reaction must move forward • Q> K – reaction must move in reverse • Q = K – reaction at equilibrium Le Chatelier’s Principle Factors that disrupt an equilibrium system: 1. Change in concentration (adding/removing reactants or products) 2. Change in volume/pressure (for gas equilibrium) 3. Change in temperature (endo/exo reactions) Catalyst: allows a system to reach equilibrium more quickly but does not alter the equilibrium. Basic concepts: Acid-Base chemistry & pH 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. Recognizing acid/base and conjugate base/acid Calculation of pH, pOH, [H3O+], [OH-] Calculating pH for solutions of strong acids/base Ionization constant: Ka, Kb Polyprotic acid (and associated Ka values) pKa, pKb Acid-Base properties of salts Predicting direction of acid-base reaction Types of acid-base reactions Calculations with equilibrium constants Titration of acid/base and characteristic titration curves Titration Curves Solubility constant (Ksp) • Remember, expression does not include (s) salt(s) cation (aq) + anion(aq) • Common ion effect: presence of an ion at the start of the “reaction”. Alters the solubility (think Le Chatelier) • pH and solubility: role of pH may impact the solubility of an insoluble salt based on the common ion effect (ex. Mg(OH)2 enhances by the presence of H+ ions/acidic) • Formation of a precipitate- again use Q when Q> Ksp a precipitate will form