1.
Be
familiar with the general characteristics of acids and bases. Know the
definitions of Arrhenius acids and bases and Bronsted-Lowry
acids and bases. Be able to use these definitions to identify acids and bases
in a chemical equation.
2.
Understand
that protons liberated from acids in aqueous solution exist as hydrated
ions. Know the name and formula for this
type of ion.
3.
Know
the meanings of the terms conjugate acid and conjugate base and be able to identify
conjugate acids and bases in a chemical equation. Be able to write formulas for conjugate
acid-base pairs.
4.
Understand
how acid-base reactions can be represented as equilibrium processes and how the
acid dissociation constant, Ka, can be used to express the relative
strength of the acids and bases involved.
Be able to write equilibrium expressions and Ka expressions
for the dissociation of any acid in water.
5.
Understand
the difference between strong acids and weak acids. Know the seven common strong acids (list
provided in class).
6.
Understand
the meaning of the terms: diprotic acid, oxyacid, monoprotic acid, and amphoteric substance.
7.
Understand
that water is amphoteric and that it is slightly
ionized in the pure state.
8.
Be
able to write the equilibrium equation which shows the auto-ionization of
water. Understand what is meant by the
ion product constant of water (Kw). Know
how it is calculated and its value in pure water and dilute aqueous solutions
at 25°C.
9.
Be
able to use Kw to calculate ion concentrations. Be able to describe relative concentrations
of H3O+ and
10.
Understand
how pH and pOH are calculated. Be able to perform calculations of pH and pOH. Be able to use
pH or pOH to find [H3O]+
and [OH]-. Be familiar with
the relationships between pH and pOH and be able to
use these relationships to calculate pOH from pH and
pH from pOH.
11.
Be
able to identify the major species present in and calculate the pH of strong
acid solutions.
12.
Be
able to write equilibrium equations and equilibrium constant expressions for
weak acid dissociation processes. Understand
the meanings of the generic formulas HA and A- as they relate to
weak acids.
13.
Be
able to calculate equilibrium concentrations from Ka. Understand when you can make the assumption
that x is sufficiently small so that “initial conc. – x” @ “initial conc.”
14.
Be
able to identify the dominant producer of H+ in a mixture of weak
acids and calculate the pH of a solution containing a mixture of weak acids.
15.
Be
able to perform calculations of percent dissociation. Recognize the trend that exists between
degree of dilution and percent dissociation.
16.
Be
able to calculate acid dissociation constants (Ka) for weak acids
using equilibrium concentrations, percent ionization data, and/or pH data.
17.
Know
the identity of the strong, soluble bases.
Be able to calculate the pH of a solution of a strong base.
18.
Understand
how amines and ammonia form basic solutions in water. Be able to calculate Kb, pH, pOH, and percent ionization for equilibria involving weak
bases. Be able to use pH or Kb
to calculate equilibrium concentrations of weak bases.
19.
Understand
that ionization of polyprotic acids occurs stepwise
and that separate Ka values are needed to describe the equilibrium
at each step. Be able to use these
dissociation constants to calculate the concentrations of all species present
in an aqueous solution of a polyprotic acid (weak or
strong).
20.
Be
able to relate strength of conjugate acids and bases to the strength of the
acid or base from which it is derived.
For example, understand the difference between a conjugate base derived
from a strong acid and a conjugate base derived from a weak acid.
21.
Be
able to qualitatively predict and quantitatively calculate the pH of the
following solutions: salt of a strong base and a weak acid, salt of a weak base
and a strong acid, salt of a strong base and a strong acid.
22.
Be
able to qualitatively compare the relative base strength of anions (conjugate
bases) of various acids and the relative acid strength of cations
(conjugate acids) of various bases.
(Note: knowing identities of strong acids and bases will be very helpful
here!)
23.
Understand
how solutions of salts containing small, highly charged cations
can have an acidic pH. Be able to
calculate the pH of these solutions.
Know the trend for relative acidity of these salts based on size and
charge of the cation.
24.
Be
able to qualitatively predict the pH of a solution of the salt of a weak base
and a weak acid.
25.
Be
familiar with and understand the factors governing relative strengths of binary
and ternary acids. Be able to use these
factors to compare strengths of acids.
26.
Be
able to write chemical equations to show how non-metal oxides form acidic
solutions and how metal oxides form basic solutions.
27.
Be
familiar with the definitions of Lewis acids and bases.
28.
Know
what is meant by the term coordinate covalent bond and understand how a
coordinate covalent bond forms in a Lewis acid-base reaction.