An acid is a substance that produces H+ or H3O+ solution.
Properties of acids:
1. Sour taste
2. React with certain metals to produce hydrogen gas
3. React with carbonates and bicarbonates to produce carbon
dioxide gas
4. Corrode metals
5. React with bases to form a salt and water
6. pH is less than 7
7. Turns blue litmus paper to red “Blue to Red A-CID”
8. Electrolytes- conduct electricity because of ions
ACIDS
Hydrogen/nonmetal
Not in water
1. Hydrogen
2. Name of anion
Examples:
Formula
HCl
H 2S
HCN
not in water
hydrogen chloride
hydrogen sulfide
hydrogen cyanide
In water
Use prefix “hydro” –root- ic acid
in water
hydrochloric acid
hydrosulfuric acid
hydrocyanic acid
RULES FOR NAMING ACIDS
#1: ACIDS THAT DO NOT CONTAIN OXYGEN
HA
Hydrogen/polyatomic anion
Not in water
In water
1. Hydrogen
2. Name of anion
Root name then check
ending of anion
-ite
The anion ending changes to –ous acid
RULES FOR NAMING ACIDS
#2: ACIDS THAT CONTAIN OXYGEN
HAOX
-ate
The anion ending changes to –ic acid
EXAMPLES:
Formula
salt/gas
Formula
aqueous
HNO2 hydrogen nitrite
HNO2 (aq)
nitrous acid
HNO3 hydrogen nitrate
HNO3 (aq)
nitric acid
H2SO3 hydrogen sulfite
H2SO3 (aq)
sulfurous acid
H2SO4 hydrogen sulfate
H2SO4 (aq)
sulfuric acid
H2CO3 hydrogen carbonate
H2CO3 (aq)
carbonic acid
RULES FOR NAMING ACIDS
GIVE THE FORMULA FOR THE NAME OR THE NAME FOR THE FORMULA
H2 S
H2SO3 (aq)
HF (aq)
HClO2
HIO
HNO2
H2SO4 (aq)
HI (aq)
H2C2O4 (aq)
Acetic Acid
nitrous acid
iodic acid
PRACTICE PROBLEMS
Acid
Formula
Where found
1. Hydrochloric
HCl
stomach, cleaning supplies
2. Sulfuric
H2SO4
car batteries, fertilizer
3. Nitric
HNO3
explosives, fertilizer
4. Phosphoric
H3PO4
detergents, fertilizers
5. Carbonic
H2CO3
soda (carbonated)
6. Ascorbic
H2C2H6O6
vitamin C (fruits, vegetables)
7. Acetylsalicylic
HOOC-C6H4-OOCCH3
aspirin
8. acetic
CH3COOH
vinegar
COMMON ACIDS AND USES
The most widely used chemical in the world is sulfuric acid.
It can cause severe burns because it is a dehydrating
agent.
This means that takes all the water out of materials,
including skin.
A strong acid completely ionizes (breaks apart) in water and
releases a lot of H+. Example: sulfuric acid (battery acid)
A weak acid only partially breaks down in water, so it
doesn’t release much H+. Example: acetic acid (vinegar)
STRONG AND WEAK ACIDS
A base is a substance that produces OH- solution.
Properties of bases:
1.Tastes bitter, chalky
2.Are electrolytes
3.Feel soapy, slippery
4.React with acids to form salts and water
5.pH greater than 7
6.Turns red litmus paper to blue “Basic Blue”
BASES
Base
Formula
Where found
1. Sodium hydroxide
NaOH
soap, lye, drain cleaner
2. Potassium hydroxide
KOH
liquid soap
3. Barium hydroxide
Ba(OH)2
stabilizer for plastics
4. Magnesium hydroxide
Mg(OH)2
laxative, antacid
5. Calcium hydroxide
Ca(OH)2
mortar, plaster, lime
6. Aluminum hydroxide
Al(OH)3
deodorant, antacid
7. Ammonia
NH3
cleaners, fertilizer, rayon, nylon
COMMON BASES AND USES
A strong base completely dissociates
(breaks apart) in solution and releases
a lot of OH-. Example: sodium hydroxide
A weak base does not completely break
apart in solution and does not release
as much OH-. Example: aluminum
hydroxide
STRONG AND WEAK BASES
There are many ways to consider acids and bases. One of these is
pH.
[H+] is critical in many chemical reactions.
A quick method of denoting [H+] is via pH.
By definition pH = -log [H+], [H+] = 10-pH
The pH scale, similar to the Richter scale, describes a wide range
of values
An earthquake of “6” is 10x as violent as a “5”
Thus, the pH scale condenses possible values of [H+] to a 14 point
scale
Also, it’s easier to say pH = 7 vs. [H+] = 1 x 10-7
P
H
The pH scale is a way
of expressing the
strength of acids
and bases
Instead of using very
small numbers, we
just use the
NEGATIVE power of
10 on the Molarity
of the H+ (or OH-)
ion.
pH < 7 = acid
pH > 7 = base
pH = 7 = neutral
P
H
Indicators: substance that
change color in the
presence of acids and
bases
Example: bromthymol blueyellow acid/ blue base/
green neutral
phenolthalein- clear acid/
pink base/ light pink
neutral
phenol red- yellow acid/
pink base/ peach neutral
methyl orange- red acid/
yellow base/ orange
neutral
P
H
Kw = [H+][OH−] = 1 x 10-14
pH + pOH = 14
pH = - log [H+] and pOH = - log [OH-]
(The [ ] means Molarity of H+)
Example: If [H+] = 1 x 10-10
pH = - log (1 x 10-10)
pH = - (- 10)
pH = 10
P
H CALCULATIONS
1. If [H+] = 1 X 10-5
pH = - log (1 x 10-5)
pH =
2. If the molarity of H+ in a solution is x10 -4, what is
the pH?
P
H CALCULATIONS
Calculating [H+]
1. If the pH is 2 what is the [H+]
10 -pH = [H+]
[H+] =
2. If the pH is 7 what is the [H+]?
P
H CALCULATIONS
Calculating pOH
If [OH-] is 1 x 10 –9
pOH = -log (1 x 10 –9)
pOH=
P
H CALCULATIONS
Calculating [OH-]
1. If the pOH is 3, what is the [OH-]?
[OH-] = 10 –pOH
2. If the pH is 8, what is the [OH-]?
pOH + pH =
or [H+] + [OH-] = 1x10-14
pOH=
[OH-] = 10-pOH
P
H CALCULATIONS
If you want to neutralize an acid or base, you add a buffer.
Buffers are acids, bases, or salts that are mixed with acids or bases
to make their pH closer to 7.
If you want to neutralize an acid, your buffer must be a base.
If you want to neutralize a base, your buffer must be an acid.
Buffers in your body help keep your blood’s pH at 7.4. This is
necessary because most of your food contains acids.
NEUTRALIZATION
Neutralization is a chemical reaction between an acid and a base.
H+ from the acid combine with the OH- from the base to form water.
Metals from the base combine with the nonmetals from the acid to form a
salt.
Example:
HCl + NaOH  NaCl + H2O
Most salts are formed with a metal and a nonmetal other than oxygen.
Some salts are formed with a metal and a polyatomic ion.
NEUTRALIZATION
Salt
formula
uses
1. Sodium chloride
NaCl
food preparation
2. Sodium bicarbonate
NaHCO3
baking soda
3. Calcium carbonate
CaCO3
chalk
4. Ammonium chloride
NH4Cl
batteries
5. Sodium phosphate
Na3PO4
detergents
COMMON SALTS
Unpolluted rain typically has a pH value of 5.6, which is acidic, but not harmful. Any rain that is below 5.6 is
considered acid rain.
Acid rain can:
1. Dissolve marble in buildings and statues
2. Corrode metal (buildings, cars)
3. Kill plankton (then fish die)
Ways acid rain can occur:
1. Burning coal releases sulfur sulfur combines with water in the air  sulfuric acid forms
2. Car exhaust releases nitrogen oxide 
Ways to prevent acid rain:
1. “scrubbers” in smoke stacks
2. Nuclear power
3. Cleaner fuel
ACID RAIN
combines with water  nitric acid forms
Soaps are organic salts. This means they contain carbon.
Soaps are made by reacting fats or oils with sodium
hydroxide or potassium hydroxide.
Soaps made with NaOH are solids. Soaps made with KOH
are liquids. Another product of this reaction is glycerin
which is used in lotion.
The process of making soap is called saponification.
SOAPS, DETERGENTS, AND ESTERS
Detergents are similar to soap, but do not form soap scum which is
a precipitate that forms when soap is used in hard water (lots of
minerals). This is why most laundry products are detergents ,
not soaps.
An ester is an organic compound formed by the reaction of an
organic acid with an alcohol. Esters are responsible for the
odors and flavors of flowers, fruits, and other foods. Esters are
added to jello and candy to give the flavors of strawberry,
banana, or apple.
Organic acids are also used to make polyester fibers.
SOAPS, DETERGENTS, AND ESTERS