1. Acids and Bases

2. Arrhenius Acid
Compound that increases the concentration of hydrogen ions (H+1) in an aqueous solution.
Example of ionization:
HCl → H+1 + Cl-1

3. Arrhenius Base
Compound that increases the concentration of hydroxide ions (OH-1) in an aqueous solution.
Example of ionization:
NaOH → Na+1 + OH-1

4. Bronsted-Lowry Definition
Involves the movement of a proton (hydrogen ion)

5. Bronsted-Lowry Acid Molecule that is a proton donor.
Conjugate base: species that is left over after a Bronsted-Lowry acid has given up a proton.

6. Bronsted-Lowry Base Molecule that is a proton acceptor.
Conjugate acid: species that is formed when a Bronsted-Lowry base has gained a proton.

7. Things Acids and Bases Have In Common
Change colors of indicators
React together to form water and salt
Conduct electricity (electrolytes)

8. The most common types of indicators are:
Indicators – solutions that change color based on the amount of hydrogen ions found (pH).
The most common types of indicators are:
Phenolphthalein
Bromothymol blue
Litmus paper
Universal indicator

9. Properties of Acids Sour taste
React with metals to produce hydrogen (H2) gas
All contain hydrogen (H+1) ions
pH < 7

10. Properties of Bases Bitter taste Feels slippery
 All contain hydroxide (OH-1) ions
pH > 7

11. pH Scale Measures the amount of hydrogen ions in solution. Strong Weak
Neutral
Weak
Strong
Acid
Base
Battery Acid
Gastric Acid
Hydrochloric Acid
Soda
Acid Rain
Black Coffee
Urine, Saliva
Pure Water
Blood
Sea Water
Baking Soda
Milk of Magnesia
Ammonia
Soap
Bleach
Drain Cleaner

12. Strength of Acids and Bases
Based on the amount of ions in solution
Strong acids/bases - completely ionize in aqueous solutions - great conductors of electricity (electrolytes)
Weak acids/bases - do NOT completely ionize (some molecules of that compound do not ionize)

13. Acid Nomenclature (Naming)
Binary acids:  contain only 2 different elements and hydrogen must be the first element
Use “hydro” as prefix and “ic” as suffix + the word “acid” at the end
Example: HBr = 
Oxyacids: contain a polyatomic ion
If ion ends in –ate, acid name ends in –ic
If ion ends in –ite, acid name ends in –ous
Examples: H3PO4 (contains ) =
H2SO3 (contains ) =
hydrobromic acid
“I ate something icky, all nite I was nauseous”
phosphate
phosphoric acid
sulfite
sulfurous acid
NO “hydro” in the name!!

14. Base Nomenclature (Naming)
element + hydroxide
Example: Ca(OH)2 =
calcium hydroxide

15. Neutralization Reactions
acid + base → water + salt
Acid and Base completely ionize.
Ex: HCl + NaOH → H+1 + Cl-1 + Na+1 + OH-1
Hydrogen and hydroxide ions combine to form water (H+1 + OH-1 → H2O)
The remaining ions and will always be the salt. (Na+1 + Cl-1 → NaCl)
HCl + NaOH → H2O + NaCl

16. Depending on the strengths of the acids and bases in the reaction, different types of salts can be made:
Strong acid and weak base → water + acidic salt
Weak acid and strong base → water + basic salt
Strong acid and strong base → water + neutral salt
Weak acid and weak base → water + neutral salt