1. Day 1
Acid-Base

2. Review of naming acids

3. Determine Name:
H2SO3
H2SO4
H2S
HClO3
HCl
HClO2

4. Determine Name:
H2SO3
H2SO4
H2S
HClO3
HCl
HClO2

5. Determine Formula
Hydrofluoric acid
Carbonic acid
Nitrous acid
Hydroselenic acid

6. Determine Formula
Hydrofluoric acid
Carbonic acid
Nitrous acid
Hydroselenic acid

7. Characteristics of Acids & Bases

8. Acids are Characterized by:
Sour taste
 color of indicator
Release of H2 gas
Reacts with bases  salt ( ionic compound) & H2O

9. Bases are Characterized by:
Bitter taste
Feels slippery
 color of indicator
Reacts with acid  salt( ionic compound) & H2O
Conducts electric current ( its an ionic compound)

10. Adding or removing electrons (e-) Making a cation or anion
Ionization
Adding or removing electrons (e-)
Making a cation or anion

11. Ionizes completely = breaks up completely Conducts electric current
Strong Acids
Ionizes completely = breaks up completely
Conducts electric current
(remember electrolyte demo aka light bulb)

12. Hydrochloric Acid (HCl)
Strong Acids
Examples:
Hydrochloric Acid (HCl)
Sulfuric Acid (H2SO4)
Nitric Acid (HNO3)

13. Strong Base
Ionizes completely = breaks up completely Examples: group 1 hydroxides – sodium hydroxide, potassium hydroxide, etc.

14. Neutralization Reaction
HCl NaOH  NaCl HOH
Strong Strong  Salt Water
Acid Base
HNO KOH  KNO HOH

15. Neutralization Reaction
Is a double replacement rxn b/w … Strong + Strong  Salt (ionic compound) + H2O Acid Base

16. Homework