AP Chemistry
Kinetics, Equilibrium, Acids and Bases
AP Chemistry/1516
Hart
You should be able to…
Chapter 14 (Kinetics)
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identify and explain the factors that affect reaction rates
calculate average reaction rates with respect to either reactants or products
calculate instantaneous reaction rates from graph or table data
relate the reaction rate of one reactant or product knowing the reaction rate of another reactant or
product (stoichiometry)
use initial reaction rates to determine the rate law for a reaction
calculate the rate constant
predict the units of rate constants based on the rate law
use integrated rate law equations to determine 1) the concentration of a reactant or product
remaining at any time after the reaction has started, 2) the time for a given fraction of a sample to
react, or 3) the time required for a reactant concentration to fall to a certain level
use graphs of ln[reactant] or 1/[reactant] to determine whether a reaction is first or second order
calculate half-life, especially of first-order reactions
explain the changes in reaction rate with temperature in terms of the collision model
interpret energy profile graphs with regard to activation energy, the activated complex,
endothermic vs. exothermic reactions
determine the molecularity of elementary steps
assess multistep mechanisms that incorporate elementary steps for reactions
determine rate laws for multistep mechanisms, when the initial step is or is not rate-limiting
describe/explain the role of catalysts in changing reaction rate
distinguish between homogeneous and heterogeneous catalysts and how they work to change
reaction rates
Chapter 15 (Equilibrium)
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write Keq expression, in units of pressure or concentration
assess the Keq with regard to relative concentrations of reactants and products
manipulate chemical equations and Keq – reciprocal, multiplication, application of Hess’s Law
heterogeneous equilibria – what is included in Keq?
calculate Keq, including use of RICE tables
calculate Q and predict the direction of a reaction by relating Q to Keq
calculate equilibrium concentrations of reactants and/or products when given Keq
apply Le Chatelier’s Principle to predict responses of the equilibrium system to changes in reactant
or product concentrations, changes in pressure or volume, changes in temperature
describe and explain the effects of catalysts on equilibrium
Chapter 16 (Acid-Base Equilibria)
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describe the properties of acids and bases
describe acids and bases using Arrhenius and Brønsted-Lowry definitions
identify conjugate acid-base pairs
write equations demonstrating conjugate acid-base pairs, including amphoteric (amphiprotic)
species
distinguish between strong and weak acids/bases versus concentrated acids/bases
categorize the strengths of acids and bases relative to each other
relate the position of equilibrium to the relative strengths of acids and bases
predict products of acid-base reactions, especially of weak acids and bases
use the relationship Kw = [H+][OH-] = 1.0 x 10-14 and/or pH + pOH = 14.00 to determine [H+],
[OH-], pH, or pOH
write net ionic equations for reactions between weak acids and bases and strong acids and bases and
any combination of weak and strong acids/bases.
name the seven strong acids
describe polyprotic acids
calculate Ka, Kb from pH data and pH from Ka or Kb data
calculate the percent ionization of a weak acid
identify acidic and basic salts
explain the relative strengths of acids based on their chemical structure, especially oxyacids
(oxoacids) and carboxylic acids
Laboratory
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define spectrophotometry
write the equation for the Beer-Lambert Law and define the three variables
design and/or interpret the results of an experiment regarding the absorption of light to determine
the concentration of an absorbing species in a solution (application of the Beer-Lambert Law)