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Equilibrium

This resource covers the principles of equilibrium in chemical reactions, including the rates of forward and reverse reactions and the significance of the equilibrium constant (K). It distinguishes between Kc for concentrations and Kp for partial pressures, along with special constants for acids (Ka), bases (Kb), and solubility (Ksp). The guide explains the reaction quotient (Q) and its use in predicting the shift in reaction direction. Additionally, it introduces RICE tables for solving equilibrium problems and discusses strong and weak acids and bases, including buffer systems and titration concepts.

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Equilibrium

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  1. Equilibrium

  2. Kinetics and Equilibrium rate forward = kfor[reactants]x and rate reverse = krev [products]z Since rates are equal at equilibrium, kfor [reactants]x = krev [products]z Keq= [products]z [reactants]x

  3. K’s • Kc- used when dealing with concentrations • Kp – used when dealing with partial pressures • Ka- used for acids • Kb – used for bases • Ksp – used for how soluble an ‘insoluble’ salt is

  4. THE SIGNIFICANCE OF K K > 1means that the reaction favors the products at equilibrium Keq = [products]z [reactants]x K < 1 means that the reaction favors the reactants at equilibrium Keq= [products]z [reactants]x K = 1Keq = [products]z [reactants]x

  5. Reaction Quotient-Q • Used if you have concentrations that may or not be equilibrium concentrations. • Can be used predict the direction the reaction will proceed to establish equilibrium. Q > K Q < K Q = K system at equilibrium Q K Shift left (toward reactants) Q K Shift right (toward products) No shift

  6. General steps for solving equilibrium problems A. Write a balanced equation. (* do stoichiometry first in moles if needed). B. Set up equilibrium expression. C. Set up RICE diagram.

  7. “RICE” TABLES --reaction, initial concentration, change in concentration, equilibrium concentration! Never Fails!! R = write a balanced reaction for the predominant reacting species I = fill in the initial concentrations C = what change is taking place E = equilibrium concentrations

  8. Acids and bases • Strong – completely ionizes • Memorize (7 strong acids and the ‘b’ of strong bases • Weak –partially dissociates • If not strong, they are weak.

  9. Buffers Solutions that resist changes in pH when either OH- or H+ ions are added. Example: NH3/NH4+ buffer system HC2H3O2 / C2H3O2- buffer system

  10. Systems that work • weak acid + salt of weak acid • weak base + salt of weak base • weak acid + ½ # of moles of strong base • weak base + ½ # of moles of strong acid • weak acid + weak base

  11. Conjugates • Difference of one H+ (ONLY!!)

  12. Titration Coeff of base x M a x V a = M b X V b x coeff of acid -vol needed for equivalence point

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