1. Important Definitions and Ideas
Acid Base Theories
Important Definitions and Ideas

2. Arrhenius Acids and Bases
States that ALL Acids release a Hydrogen ion (H+) in water
Also states that acids react with metals
States that ALL BASES MUST have and release OH- ions in water (THIS IS A PROBLEM)
Limits his definition of what bases are
States that if a substance does NOT have OH- to give then its not a base

4. What does AMPHOTERIC Mean?
Amphoteric Substances can be both an acid and a base
Depends on what the reactants are in the reaction
Water is an example of an amphoteric substance but many more exist

5. Acid Types 1. Monoprotic----Acids with only one Hydrogen ion to give
Ex: HCl
2. Diprotic—Acids that have two Hydrogen ions to lose
Must go through 2 rounds of reactions to get rid of both since acids can only lose one Hydrogen per reaction
Ex: H2SO4
3. Triprotic—Acids that have 3 Hydrogen ions to lose.
Must go through 3 rounds of reactions to lose all 3
Ex: H3PO4

6. Acid Types Continued
The number of Hydrogen ions that can be lost has NOTHING TO DO with Strength
The strongest acids are the ones that the Hydrogen ions the fastest in water
We call this a Ka measurement
Strong Acids have high values and weak acids have low values

9. Bronsted-Lowry Acids and Bases
Theory that states that acids are any substance that loses at least 1 Hydrogen ion when placed in a reaction
This is the “normal” definition
States that BASES are ANY SUBSTANCE THAT TAKES or GAINS at least ONE HYDROGEN ION.
This is different and is more inclusive and a better definition of what a base is
Substances like Ammonia, and Baking Soda are bases that fit this definition

12. Bronsted-Lowry Vocabulary
1. Conjugate Acid-----Substance that the base becomes on the product side of the reaction after it has gained one hydrogen ion
2. Conjugate Base----Substance that the ACID becomes after it has lost one Hydrogen ion on the product side
If you reverse the reaction you can get back your starting acid/base combination
All Bronsted-Lowry reactions are equilibrium reactions
Shows that acid/base reactions will reach a point of constant concentration

15. Acid and Base Strength 1. Strong Acids---
Ionize completely or nearly to completion
Ionize fast when placed in water or combined with a substance
Create a solution with a high concentration of H+ ions
pH range is typically 1-3
For every 100 Acid Molecules have lost a hydrogen

17. Weak Acids Acids that do not ionize completely
This means that some/most of the acid molecules hold onto the Hydrogen that they should be losing
1 or 2 of every 100 molecules lose a hydrogen when placed into solution
These will be weak and will have a pH of 4---6
Typically these are organic acids

19. Strong Bases
Bases that release OH- ions quickly and completely when placed into solution
Or these are bases that aggressively take a hydrogen ion from an acid or from water
pH will be 10-14

20. Weak Bases
Bases that do not ionize completely (hold onto the hydroxide ions)
OR these bases do not aggressively take hydrogen ions from water or other substances
Most of these bases are molecular substances like Ammonia
pH is from