A) Strong vs Weak
A strong acid or base is 100 % ionized in solution. For example:
A weak acid or base is <100% ionized or dissociated in solution. For example:
Do Not Confuse STRONG with CONCENTRATED!!!
0.001 M HCl is a ______________________, _____________________ acid.
10.0 M HF is a ________________________, _____________________ acid.
B) Distinguishing Between Strong and Weak Acids at the Macroscopic Level
Experimentally you can tell the difference between a strong and a weak acid by placing a light bulb in the solution. As long as the two acids are the same concentration, the strong acid will be a better conductor of electricity. Which of the two acid solutions below is stronger?
TITRATION CANNOT BE USED TO DISTINGUISH BETWEEN A STRONG AND A WEAK
ACID OF THE SAME CONCENTRATION. BOTH WILL REQUIRE THE SAME AMOUNT OF
BASE TO REACH THE END POINT.

C) Table of Relative Bronsted-Lowry Acid-Base Strengths
Use the table below to answer the following questions.
1.
Where are the strongest acids located? ____________________________________
2.
What type of arrow is used in the ionization equation for the top six acids? _________
3.
What is the Ka value given for the top six acids? _____________________________
4.
The top six acids must be ___________________ acids.
5.
What is the concentration of the actual HCl molecule in a bottle labeled 1.0 M HCl? ____
6.
Where are the strongest bases located? ___________________________________
7.
What type of arrow is used in the reaction of the bottom two bases? ______________
8.
The bottom two bases must be __________________ bases. Other strong bases include the alkali and alkaline earth hydroxides like: NaOH, LiOH, Sr(OH)
2
etc. Notice that some of the alkaline earth hydroxides are not very __________________ in water.
However, 100% of the dissolved base is ______________________.
9.
Is NH
3
a strong base, weak base, strong acid or weak acid? ______________________
10.
What type of arrow is used in the ionization equations for all the acids below H
2
SO
4
?___
11.
These acids must be ___________________.
12.
What happens to the Ka values as you go down the table? _______________________
13.
As you go down the table do the acids become weaker or stronger? ________________
14.
As you go down the table do the conjugate bases become weaker or stronger? ________
15.
The stronger an acid, the _____________________ its conjugate base.
16.
Identify a substance that appears both on the acid side and on the base side of the table.__________________. This substance must act like an acid or a base and therefore is ______________________________.
17.
Identify three complex ions that behave like acids.____________________________

D) The Levelling Effect
Notice that the top six strong acids all ionize ____________ in water to give __________ and their ____________________________________. Because this is a one way reaction, the strong acid molecule no longer exists. Instead _________ becomes the strongest acid present in all six solutions. Since all six strong acids are equivalent to solutions of H
3
O + , they all exhibit the same ______________________. This phenomenon is called the __________________________________________. In a similar fashion, the strongest base in water is __________ as shown.
NH
2
+ H
2
O ---->
What is the strongest acid and base that can exist in ammonia?
E) Conductivity and Total Ion Concentration
Acid, base and salt solutions are all able to conduct electricity. The extent to which they conduct is directly related to the ___________________________________________.
When estimating the total ion concentration you must consider the ___________________ of the acid or base or the _______________________ of the salt. For example rank the following solutions with respect to increasing conductivity. a) 1.0 M HCl b) 1.0 M Na
2
SO
4 c) 2.0 M NaOH d) 1.0 M HCN

F) Writing Bronsted-Lowry Equilibria
The table of relative acid-base strength can be used to write equations representing the
Bronsted-Lowry equilibria that occur when two acids are mixed. For example:
Write the Bronsted-Lowry equilibria that occur when the following are mixed and indicate whether reactants or products are favoured. a) HC
6
H
5
O
7
2 + HC
2
O
4
b) Fe(H
2
O)
6
3+ + HSO
3
-
Hebden: p122 #20 p125 #21-27 p133 #38 odds, 39 odds, 40 odds, 41, 42, 45, 46
Silberberg: p823 #4,13,15,17,53,55,57,59,60,129