1. Starter Describe some properties of acids and bases
How would you go about determining if something was an acid or base?

3. Naming of Acids Types of Acids Strengths of Acids/Bases
Ch. 15/16: Acids and Bases
Naming of Acids
Types of Acids
Strengths of Acids/Bases

4. Acids and Bases
Groups of chemical compounds that share certain characteristics
common substances you use everyday
Examples:
soap juice
drain cleaners soda
vinegar antacids

5. Acid Properties sour taste when dissolved in water turns pH paper red
do not taste to test chemicals
many are corrosive and poisonous
turns pH paper red
react with metals to make H2(g)
metals above H2 in activity series
single replacement reaction
Ba(s) + H2SO4(aq)  BaSO4(aq) + H2(g)

6. Acid Properties react with bases to make salt and water
acid is neutralized when added to an equal number of moles of base
produces an ionic compound (also called “salt”) and water
HBr(aq) + KOH(aq)  H2O(l) + KBr(aq)
conduct electricity
strong acids conduct very well
weak acids conduct a small amount

7. Common Acids Sulfuric acid: H2SO4 Nitric acid: HNO3
used in car batteries
Nitric acid: HNO3
used in explosives
Phosphoric acid: H3PO4
used as flavoring in soft drinks
Hydrochloric acid: HCl
stomach produces it
Acetic acid: HCH3COO or HC2H3O2
vinegar contains it

8. Base Properties taste bitter turn pH paper blue
most are caustic (cause burns) so don’t taste to test
turn pH paper blue
feel slippery when dissolved in water
react with acids to make salt and water
conduct electricity

9. Naming of Acids Binary acids
Contains 2 different elements: H and another
Always has “hydro-” prefix
Root of other element’s name
Ending “-ic”
Examples: HI, H2S, HBr

10. Naming Acids Ternary Acids - Oxyacids
Contains 3 different elements: H, O, and another
No prefix
Name of polyatomic ion
Ending “–ic” for “-ate” and “–ous” for “-ite”
Examples: HClO4, H3PO4, HNO2

11. Practice H2SO3 Sulfurous acid HIO3 Iodic acid HF Hydrofluoric acid
H2Se
Hydroselenic acid
Hypoiodous acid
HIO
Perchloric acid
HClO4
Carbonic acid
H2CO3
Hydrocyanic acid
HCN
Pseudobinary acid

12. Types of Acids Monoprotic acids Polyprotic acids- diprotic, triprotic
Only have one acidic proton
HNO2, HBr, HCH3COO
Polyprotic acids- diprotic, triprotic
Contains more than one acidic proton
H3PO4, H2SO4, H2Te
Organic acids
Contain COOH (carboxyl) group
Weak acids

13. Strengths of acids
Depends on polarity and strength of the bond holding the H to the rest of the molecule
Strong acids
Ionize completely
Strong electrolyte
Would these have a strong or weak bond?
Would these have a polar or nonpolar bond?

14. Strengths of Acids Strong Acids Weak Acids
HCl, HBr, HI, HClO4, H2SO4, HNO3
Memorize that list!
Weak Acids
Only ionize partially
Weak electrolytes
Can assume any acid not on that list is weak

15. Strengths of Bases Depends on the amount of dissociation and structure
Strong Bases
Strong electrolytes
All are metal hydroxides
Dissociate completely in water
Examples: KOH, Ba(OH)2
Weak Bases
Weak electrolytes
Examples: NH3, C6H5NH2