1. Acids and Bases

2. H+ water Acetic acid Citric acid Tannic acid Formic acid
Acids H+
Acid – a compound that produces ions when dissolved in
Examples:
Vinegar –
Lemon juice –
Tea –
Ant venom –
water
Acetic acid
Citric acid
Tannic acid
Formic acid

3. Sour Corrosive red Aqueous electrolytes bases H2O salt
Properties of Acids
Sour
taste
Turns litmus paper
Reacts with metals to form gas
solutions of acids are
(must be mixed with water!)
Reacts with to form and
Corrosive
red H2
Aqueous
Litmus paper is an indicator.
Electrolytes can conduct electricity.
“Salt” is not always NaCl! It can be other ionic compounds.
electrolytes
bases
H2O
salt

4. Properties of Acids
Sugar, corn syrup, modified corn starch, citric acid, tartaric acid, natural and artificial flavors, yellow 5, yellow 6, red 40, blue 1
What ingredients make these…
so sour?

5. “hydro-” root “-ic” hydro chlor ic acid
Naming Binary Acids
H + one other element
Begin with
Use the of the element name
Add the suffix
HCl
“hydro-”
root
“-ic”
hydro
chlor ic
acid

6. Hydrobromic acid Hydroiodic acid Hydrofluoric acid
Naming Binary Acids
Hydrobromic acid
HBr 
HI 
HF 
Hydroiodic acid
Hydrofluoric acid

7. polyatomic ending -ate -ic -ous -ite Nitrate Nitric acid
Naming Ternary Acids
H + polyatomic ion
Begin with ion without
the
Add suffix if there was an
Add suffix if there was an
HNO3 
polyatomic
ending
-ate
-ic
-ous
-ite
Nitrate
Nitric acid

8. Chloric acid Phosphoric acid Carbonic acid
Naming Ternary Acids
Chloric acid
HClO3 
H3PO3 
H2CO3 
Phosphoric acid
Carbonic acid

9. 2 Strong ionize H+ HCl HBr HI O H 3 – 1 = 2 4 – 2 = 2
Strength of Acids
Strong
ionize
acids – completely
in water (create a lot of )
3 binary acids
Ternary acids
Strong if # of atoms - # of atoms ≥
H2SO4 HNO3 H+
HCl
HBr HI 2 O H
3 – 1 = 2
4 – 2 = 2

10. 1 2 – 1 = 1 3 – 3 = 0 Weak slightly aqueous O H Strength of Acids
acids – ionize only in
solution
Binary acids – all others not listed above
Ternary acids
Weak if # of atoms - # of atoms ≥
H3PO3 HNO2
aqueous 1 O H
2 – 1 = 1
3 – 3 = 0

11. OH- (hydroxide) water Magnesium hydroxide Sodium hydroxide
Bases
OH-
Base – a compound that produces ions
when dissolved in
Examples:
Milk of Magnesia – neutralizes stomach acid
Drain cleaner–
(hydroxide)
water
Magnesium hydroxide
Sodium hydroxide

12. Bitter Slippery blue Aqueous electrolytes acids H2O salt
Properties of Bases
Bitter
taste
Turns litmus paper
solutions of bases are
(must be mixed with water!)
Reacts with to form and
Slippery
blue
Aqueous
electrolytes
Litmus paper is an indicator.
Electrolytes can conduct electricity.
“Salt” is not always NaCl! It can be other ionic compounds.
acids
H2O
salt

13. polyatomic Sodium hydroxide Calcium hydroxide Potassium hydroxide
Naming Bases
polyatomic
Use the same rules as for ions (name the cation, then name the anion)
NaOH 
Ca(OH)2 
KOH 
Sodium hydroxide
Calcium hydroxide
Potassium hydroxide

14. Strong ionize OH- 1 2 Be Weak ionize slightly
Strength of Bases
Strong
ionize
bases – completely in water (create a lot of ions).
All hydroxides with groups and metals (except ).
bases only
All bases not listed above as strong.
OH- 1 2 Be
Weak
ionize
slightly

15. Types of Acids Type # of H+ donated Example Monoprotic 1 HNO3 Diprotic
Defined by how many H+ they can donate.
Type
# of H+ donated
Example
Monoprotic 1
HNO3
Diprotic 2
H2SO4
Triprotic 3
H3PO3

16. pH = 0 pH = 7 pH = 14 acid base neutral
Acidity/Basicity
pH = 0
pH = 7
pH = 14
[H+]
[OH-]
acid
base
neutral

17. Neutral [H+] = [OH-] Acidic > Basic <
Acidity/Basicity
Neutral
[H+] =
[OH-]
Acidic
>
Basic
<

18. pH is < 7 Solution is acidic pH is = 7 Solution is neutral
Solution is basic

19. Neutralization Reactions
What happens with you mix an acid with a base? A ____________________________________________ reaction
Neutralization Reactions
What happens with you mix an acid with a base? A reaction
HCl NaOH 
Products are always a (
and ) and
This is called a reaction
double replacement
H2O
NaCl
salt
nonmetal
metal
water
neutralization