2.3: 3. AB1- Equilibrium Acids and Bases
- Page ID
- 436098
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Summary of AB1 and AB2:
Acid and base chemistry has so many applications and so many essential properties throughout chemistry that it is broken down into two Core Goals:
AB1: Equilibrium Acids and Bases - focused on the qualitative nature of acid/base chemistry and the equilibrium between them.
AB2: Quantitative understanding of the various properties of complex acid/base systems.
AB1: Equilibrium Acids and Bases
Demonstrate chemical literacy regarding chemical equilibrium with an emphasis on:
- how chemical systems change as they move toward a state of equilibrium;
- how the equilibrium condition itself can be characterized;
- how a system at equilibrium will respond to changes in conditions;
- the relationship chemical equilibrium to chemical kinetics and thermodynamics;
- the relative reactivity of acids and bases;
- quantitative calculations involving chemical equilibria & aqueous solutions of acids, bases, and salts.
- Relate the equilibrium constant to the rate constants for the forward and reverse reactions (moved to SOL)
- Define reaction quotient, Q, relate Q to the equilibrium constant, K, and explain how Q can be used to predict whether a system is at equilibrium, and if not, the direction a chemical system will move to establish equilibrium (moved to SOL)
- Given a chemical equation, write the expression for the reaction quotient and/or equilibrium constant (moved to SOL)
- Apply equilibrium concepts to calculations involving chemical reactions, concentrations, gas pressures, free energy, and other variables. (moved to SOL)
- Interpret the magnitudes of equilibrium constants regarding the extent of reaction that has occurred in the forward direction once equilibrium has been established (moved to SOL)
- Identify factors that can stress a system that is in a state of equilibrium and explain why these factors stress the equilibrium system (moved to SOL)
- Of the above factors, identify those that will alter the magnitude of the equilibrium constant, and how the constant will change as a result of the stress (moved to SOL)
- Apply Le Châtelier’s principle to predict the direction a system, originally in a state of equilibrium, will shift when stressed by adding or removing reactants, adding or removing products, or heating or cooling the system (moved to SOL)
- Identify common strong acids and bases by name and formula
- Characterize acids and bases according to the Arrhenius and Bronsted-Lowry definitions (model)
- Identify Bronsted-Lowry Acid-Base pairs (acid and conjugate base, base and conjugate acid) in a given reaction
- Write chemical reaction equations and equilibrium expressions for the ionization of an acid and for the ionization of a base in water
- Write the equation for the auto-ionization of water and relate to Kw, [H+], [OH-], pH, and pOH
- Describe changes in Kw, [H+], [OH-], pH, and pOH as a solution increases in acidity or in alkalinity
- Characterize acids and bases in terms of their strength using the following properties: Ka, pKa, Kb, pKb, [H+], pH, [OH-], pOH, % ionization in water, and strength relative to water
- Identify structural factors that influence the strength of a substance as an acid or as a base and use that information to predict/rank the relative strengths of another given group of substances
- Use Ka, pKa, Kb, or pKb to predict the extent of an acid-base reaction
- In terms of Le Châtelier’s Principle, explain why the addition of a salt containing the conjugate base of a weak acid, or the conjugate acid of a weak base, suppresses the ionization of the acid or base respectively