Chem 1B
Dr. White
1
Study Guide For Exam 1
The exam will cover Chapters 13 and 14 in the textbook. I have summarized the material
below. A BAD way to study for the exam is just to look at this study guide, check things off
and think you are ready for the exam. A GOOD way to study for the exam is to look at this
study guide and find the appropriate sections in your notes and/or the textbook to go over the
material in detail. Also, you MUST work problems for each section in order to succeed on the
exam! Be able to do the problems without looking at the solutions. It’s a good idea to rework
the class examples without looking at the solutions. Don’t forget to try the recommended
book problems given on the website (especially for those topics you are having trouble with)
Note: You must bring your own non-programmable, scientific calculator.
Sharing of calculators during the exam will not be allowed. You will also
need a pen/pencil, but will not need any other materials.
Keys to studying chemistry
 Be sure to review notes and your text.
 Be able to work all pertinent problems from homework assignments, book
problems, lecture problems, lab calculations, and example problems in the
textbook
 Use frequent but short study periods, rather than long hours just before an
exam
 Practice! Chemistry uses lots of terms and can seem like a foreign
language. Practice problems in writing, do old homework or other
exercises in the text to check your answers.
 Read each problem carefully to determine what is being asked, make a
plan for solving the problem, check the answer to see if it is reasonable!
Below are some guidelines of what will be emphasized but you should be
prepared for anything from the chapters or lectures unless otherwise
specified.
Chapter 13 Equilibrium –
 Definition of equilibrium – when RATES of fwd and rev reactions are equal, when
product and reactant concentrations no longer change, when ratio of product to
reactant concentrations has reached a constant value that’s characteristic of that
reaction at given T
 Reaction Quotient Q & Equilibrium Constant K
 MUST know how to write these for any reaction
o In terms of concentrations
o In terms of pressures
o Do you include solids or liquids?
 What does magnitude of K tell us?
 What does magnitude of Q compared to K tell us?
 How to find Q (or K) for some reaction given another reaction you know Q (or K)
for
o Reaction is reverse of known one
Chem 1B
Dr. White
2
o Reaction is known one x some factor
o
Reaction is sum of known ones
 How to convert between K and Kp
 How to solve equilibrium problems (ICE tables)
o Given equilibrium concentrations, solve for K
o Given initial concentration of reactants, solve for equilibrium concentrations
o When can you simplify??
o Given initial concentration of reactants and products, solve for equilibrium
concentrations
 Le Chatelier’s Principle
 What it is says, how to use it, and how to explain the shift
 Effect of Concentration changes
 Effect of Volume/Pressure changes
 Effect of Temperature change
 When K actually changes (only with Temperature!!)
Chapter 14 – Acids and Bases
 Know how to write reactions of acids or bases with water and the corresponding Ka and Kb
expressions
 Given the formula for acids or bases, be able to write out reaction with water
 You should be able to recognize a strong acid and strong base based on the rules
given in class
 Weak acids and bases
 Know what it means to be a weak acid or base (compared to strong acid or base)
 Know what does the size of Ka and Kb tell you about the acid/base strength
 Know about the relative strength of conjugate acid base pairs
o example: conjugate acid of a strong base is a weak acid
 Acid Strength and periodic trends
 Be able to predict acid strength for binary acids
 Be able to predict acid strength for oxyacids
 Understand Kw, what chemical equation it corresponds to, its expression, and its
connection to Ka & Kb for conjugate acid-base pairs (KNOW Kw = Ka x Kb)
 know what constitutes an acidic solution, a basic solution, and a neutral solution in
terms of [OH-] and [H3O+]
 Understand the pH concept, the pH scale and pH calculations
 pH = - log[H3O+] (KNOW THIS EQUATION)
 know what is considered acidic pH and basic pH
 pOH = - log[OH-] (KNOW THIS EQUATION)
 Be able to solve pH and pOH for strong acids/bases, weak acids/bases, and salts
(how are they different?)
 Equilibrium constants for acids and bases
 Know what chemical equation does Ka or Kb corresponds to
 Know what info does the Ka or Kb value give us
o Be able to compare strength of species based on K values
o Of course be able to write expression for Ka or Kb
o Be able to calculate Ka value from pKa value or vice versa (pKa = -log Ka)
o Be able to use Ka or Kb , % dissociation, and concentration info, either initial or
equilibrium, to do problems
Chem 1B
Dr. White
3
 Solve for equilibrium concentrations
 Solve for pH or pOH
 Solve for % dissociation
 “ICE” tables, just like we used them in Ch 13!
 Since most of the acids or bases are weak, remember how & when to use
the simplifying assumption! (don’t forget to check that assumptions are
valid!)
 Understand polyprotic acids – what are they? Know how do you solve for the pH of
weak polyprotic acids
 Know that salts can be acidic or basic – how do you tell? Write equations! Be able to solve
for the pH of a salt
 Lewis Acids and Bases (what’s the definition?)
 Be able to recognize Lewis acids and bases in a reaction
GIVEN EQUATIONS AND CONSTANTS: Any K, Ksp, of Kf values you will need
R=0.08206 L·atm/mol·K