1. Acids and Bases
“Tragedy is like strong acid -- it dissolves away all but the very gold of truth.” - D.H. Lawrence

2. Characteristics of Acids
Taste _______________.
Conduct __________________________
Cause _______________________
React with ________ to form ________
React with _____________ to form _____ and a ________.
Produce ___ ions in water.

3. Characteristics of Bases
Taste _____________
Slippery.
Can be _______________
Produce ___________ in water.
React with acids to produce _______ and a __________.

4. Naming Acids and Bases
Acids – Compounds that dissociate in water to give H+ ions
Generic acid formula: _________
H – __________
n – number
If n = 1, acid is monoprotic
If n = 2, acid is diprotic
If n = 3, acid is triprotic
X – monatomic or polyatomic ______

5. Naming Acids Rules for naming acids: IF:
X ends in ______, name is ___________ acid.
X ends in ______, name is _________ acid.

6. Naming Acids
Try these: HF
HNO3 HI
H2CO3
HClO4
H2SO3

7. Naming Bases
Bases – Compound that produces OH- ions when dissolved in water
Names the same as any other ionic compound.
Examples:
Note: Ammonia (NH3) is a base, even though it is not a hydroxide

8. Hydrogen Ions and Acidity
Self ionization of water:
H2O ↔ H+ + OH-
In a neutral solution:
[H+] = [OH-] = ____________
So:
[H+] [OH-] = ______________

9. Hydrogen Ions and Acidity
In acidic solutions:
[H+] > [OH-]
[H+] >__________
In basic (alkaline) solutions:
[H+] < [OH-]
[H+] <__________

10. Hydrogen Ions and Acidity
It’s so hard saying “a concentration of one times ten to the negative seventh molar” all the time…Is there a better way?
YES! All we need is the exponent…
So if the concentration of hydrogen ions is _________, the pH = __

11. pH What is the pH if [H+] = What is the [H+] if the pH = 1 x 10-6 M4 9
5.5
13.5

12. pH pH has a range of 0 to 14 pH < 7, solution is _________
pH is measured with an indicator or pH meter.

13. pH of Some Common Substances

14. Is there a pOH? Sure! It’s pretty much the same thing. pOH = _________
Since [H+] [OH-] = 1 x M2
pH + pOH = ____

15. Strong vs. Weak Acids Strong DOES NOT mean concentrated!
Some acids only partially dissociate in water. E.g. Acetic acid. These are ______ acids.
HC2H3O2 ‹-› H+ + C2H3O2-
Acids that completely dissociate in water are _______ acids. E.g. Hydrochloric acid
HCl → H+ + Cl-

16. Strong vs. Weak Acids Acids can be STRONG and Concentrated 12M HCl
Acids can be STRONG and Dilute
0.01M HNO3
Acids can be WEAK and Concentrated
12M H2CO3
Acids can be WEAK and Dilute
0.01M HC2H3O2

17. How can you tell if an acid is strong?
Look for the Acid Dissociation constant, __
So large Ka = _______ acid.
Small Ka = _______ acid

19. Neutralization Reactions
Acids and Bases react to form water and a salt.
The products are neutral if the number of moles of H+ = moles of OH-
This is referred to as the _________________.
If we add a volume of a known concentration of an acid/base to a volume of an unknown concentration of base/acid, we can determine the unknown’s concentration.
This process is known as _____________.

20. Titrations
Titrations use indicator dyes to determine if the solutions have been neutralized.
___________ – Point at which the indicator changes color and the titration is stopped.
____________ and ______________ are not the same thing. However, the goal of a titration is to have the end point as close to the equivalence point as possible.

21. So how do we use titrations?
We can find the concentration of a solution is we have a solution of known concentration.
Let’s say we have neutralize 25 mL of H2SO4 solution with 18 mL of 1.0 M NaOH solution. What is the concentration of the H2SO4?

22. Titrations
First, we need to write a balanced equation.
Acid
Base

23. Titrations Given: VA= 25 mL, MB= 1.0M, VB=18 mL
Next, you can use the following relationship:
Where __ is the coefficient from the reaction, __ is molarity, __ is volume, __ is the acid, and __ is the base.

24. Titrations