This subject is known as chemistry which is a sub branch of science. The ppt is about acids and bases and there types, definitions and etc

1. Acid and Bases

2. Acid and Bases

3. Acid and Bases

4. Acids
Have a sour taste. Vinegar is a solution of acetic acid. Citrus
fruits contain citric acid.
React with certain metals to produce hydrogen gas.
React with carbonates and bicarbonates to produce carbon
dioxide gas
Have a bitter taste.
Feel slippery. Many soaps contain bases.
Bases

5. Some Properties of Acids
 Produce H+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion
attached to a water molecule)
 Taste sour
 Corrode metals
 Electrolytes
 React with bases to form a salt and water
 pH is less than 7
 Turns blue litmus paper to red “Blue to Red ACID”

6. Anion
Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Acid Nomenclature Review
No Oxygen
w/Oxygen
An easy way to remember which goes with which…
“In the cafeteria, you ATE something Icky”

7. Acid Nomenclature
Flowchart
hydro- prefix
-ic ending
2 elements
-ate ending
becomes
-ic ending
-ite ending
becomes
-ous ending
no hydro- prefix
3 elements
ACIDS
start with 'H'

8. • HBr (aq)
• H2CO3
• H2SO3
 hydrobromic acid
 carbonic acid
 sulfurous acid
Acid Nomenclature Review

9. Some Properties of Bases
 Produce OH- ions in water
 Taste bitter, chalky
 Are electrolytes
 Feel soapy, slippery
 React with acids to form salts and water
 pH greater than 7
 Turns red litmus paper to blue “Basic Blue”

10. Some Common Bases
NaOH sodium hydroxide lye
KOH potassium hydroxide liquid soap
Ba(OH)2 barium hydroxide stabilizer for plastics
Mg(OH)2 magnesium hydroxide “MOM” Milk of magnesia
Al(OH)3 aluminum hydroxide Maalox (antacid)

11. Acid/Base definitions
• Definition 1: Arrhenius (traditional)
Acids – produce H+ ions (or hydronium ions H3O+) in water
Bases – produce OH- ions in water
(problem: some bases don’t have hydroxide ions!)

12. Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water

13. Acid/Base Definitions
• Definition 2: Brønsted Lowry
Acids : proton donor
Bases : proton acceptor
A “proton” is really just a hydrogen atom
that has lost it’s electron!

14. A Brønsted-Lowry acid is a proton donor
A Brønsted-Lowry base is a proton acceptor
acid
conjugate
base
base
conjugate
acid

15. ACID-BASE THEORIES
The Brønsted definition means
NH3 is a BASE in water and
water is itself an ACID
Base
Acid
Acid
Base
NH4
+
+ OH-
NH3 + H2O

16. Amphoteric Substances
• A substance that is Amphoteric can act as
either an acid or a base.
• In the previous slide, water acted as an acid.
• In the following example, water acts as a base.
HCl (g) + H2O (l)  H3O+ (aq) + Cl- (aq)
acid base conj. acid conj. base

17. Conjugate Pairs

18. Acid-Base Behavior
• Consider a compound having the formula HOX.
• If X is highly electronegative, it will have a strong attraction
for the electrons shared with O.
o The O, will in turn, pull strongly on the electrons held shared
with H.
o This H will then be easily lost = acid
• If X has a low electro negativity, the oxygen will pull the
electrons away from X.
o The hydrogen will remain joined to the oxygen.
o Since the O and H can easily remain together, it is likely that OH-
will be formed = base
• Nonmetals tend to have high EN = acids
• Metals tend to have low EN = bases

19. Acids & Base Definitions
Lewis acid: A substance
that accepts an electron
pair
Lewis base: A substance
that donates an electron
pair
Definition 3: Lewis

20. Formation of hydronium ion is also an excellent
example.
Lewis Acids & Bases
•Electron pair of the new O-H bond
originates on the Lewis base.
H
H
H
BASE
••
•
•••
O—H
O—H
H+
ACID

21. Lewis Acid/Base Reaction