PROPERTIES OF ACIDS
• A tart or sour taste
• Can be strong or weak electrolytes (conduct electricity)
• React with metals to produce hydrogen gas!
• Examples: Lemons contain citric acid

IS IT AN ACID?
1. Gastric Juice
2. Pure Water
3. Lemon Juice
4. Coffee
5. Sea water
6. Milk
1. Yes
2. No
3. Yes
4. Yes
5. No
6. Yes, barely

ARRHENIUS ACIDS AND BASES
• Swedish chemist in 1887
• Defined acids and base according to their ions!

ARRHENIUS ACIDS
Hydrogen containing compounds to produce H +
HCl, HI, HBr, HClO
3
, HClO
4
, HNO
3
,
H
2
SO
4

DID YOU KNOW?!
• A strong acid completely dissociates!
• Meaning it completely breaks down in H + ions!
• Way to go Arrhenius!
Hypothesize: would a weak acid completely dissociate?

DOES THE NUMBER OF H’S MATTER?
H
3
H
2
4
H
3
4
H
2
YES!

MONOPROTIC, DIPROTIC, TRIPROTIC
M O N O P R O T I C
1 hydrogen able to ionize
D I P R O T I C
2 hydrogens able to ionize
T R I P R O T I C
3 hydrogens able to ionize
(1 reactions) (2 reactions) (3 reactions)

WHY PROTIC?
NOT HYDROGEN?
How many protons, neutrons, electrons?
Think about H + …
What’s left over?
Only a proton, so H + is commonly referred to as a proton

1. HClO
3
1. Monoprotic
2. Diprotic 2. H
2
SO
3
3. H
3
PO
3
4. HF
3. Triprotic
4. Monoprotic
5. HCl
6. H
2
S
7. H
3
PO
4
5. Monoprotic
6. Diprotic
7. Triprotic

BINARY ACID NOMENCLATURE
• Made of 2 different elements
• One will be hydrogen and the other will be a highly electronegative element
• Inorganic acids
 Not containing carbon

BINARY ACID NOMENCLATURE
• MUST have a hydro prefix then stem of the other element and –ic
• Hydro- stem- ic and Acid
• HCl  ?
• Hydro-chlor-ic Acid

BINARY ACID NOMENCLATURE
Name these:
1.
HF
2.
HCl
3.
HBr
4.
HI

OXYACIDS
• Acids with oxygen
– Typically containing H, O, and another nonmetal
– Ternary- meaning 3 elements
• Like our polyatomics
C
Hg
NH
2
H
2
+2
4
+1
3
O
2
-
CH
3
COO -
CN -
HCO
C
CO
2
O
ClO -
-2
3
3
-
4
-2
ClO
ClO
ClO
PO
PO
HPO
4
4
-
-3
2
-
3
-
-3
3
4
-2 dimercury (I) ammonium acetate acetate cyanide carbonate hydrogen carbonate oxalate hypochlorite chlorite chlorate perchlorate phosphate phosphite hydrogen phosphate
CrO
Cr
2
O
MnO
MnO
NO
NO
2
4
-
3
-
-2
4
7
-2
OH -
4
-
-2
SiO
3
-2
SCN -
S
SO
SO
2
O
3
-2
4
-2
HSO
HSO
3
4
-
3
-
-2 chromate dichromate permanganate manganate nitrite nitrate hydroxide silicate thiocyanate sulfite
Sulfate hydrogen sulfate hydrogen sulfite thiosulfate

NAMING OXYACIDS
• Whatever the charge of the polyatomic is tells you how many hydrogen’s you need
• For example: CO
3
-2 would be  H
2
CO
3
• NO HYDRO PREFIX!!!!
• Change –ate to –ic and add acid
• Carbonate  carbonic acid

NAMING OXYACIDS
• PO
4
-3 
Phosphate
• NO
3
-1  Nitrate

NAMING OXYACIDS
• If the ending is –ite, change the ending to – ous and add acid
• For example: NO
2
is nitrite
 HNO
2 or nitrous acid

NAMING OXYACIDS
To remember think of 300, leonidas (leon-ite-ous)
PO
3
-3 
Phosphite
SO
2
-2  Sulfite

ACID NOMENCLATURE REVIEW
Hydro- stem- ic acid
-ate  ic acid
-ite  ous acid

Name or write the formula for the following acids:
1. HClO
3
2. H
2
SO
3
3. H
3
PO
4
4. Hydrofluoric Acid
5. Hydrochloric Acid
6. Phosphorous
7. Hydrosulfuric acid
1. Chloric Acid
2. Sulfurous Acid
3. Phosphoric Acid
4. HF
5. HCl
6. H
3
PO
3
7. H
2
S

PROPERTIES OF BASES
• A bitter taste
• Slippery feel like soap
• Also, form strong or weak electrolytes
• Examples: Soaps, household cleaning products

IS IT A BASE?
1. Lemon juice
2. Sea water
3. Pure water
4. Blood
5. Ammonia
1. No
2. Yes
3. No
4. Yes, barely
5. Yes

ARRHENIUS BASES
Hydroxide containing compounds to produce OH -

DECIDE WHETHER IT IS AN ARRHENIUS ACID OR
BASE?
1. Acid
1. HNO
3
2. KOH
2. Base
3. Acid
3. H
2
SO
4
4. Sr(OH)
2
5. H
3
PO
4
6. H
2
S
4. Base
5. Acid
6. Acid

• What is the name for OH ?
• Group 1 and 2 make strong bases (Except the 1 st two of each group and last ones)
• Metal + Hydroxide NaOH is Sodium Hydroxide

NAME THE FOLLOWING BASES:
1. KOH
2. Sr(OH)
3. Ba(OH)
4. CsOH
2
2
1. Potassium hydroxide
2. Strontium hydroxide
3. Barium hydroxide
4. Cesium hydroxide

WHAT IF A COMPOUND DOES NOT HAVE AN H + OR
OH ?
WE NEEDED TO HAVE OTHER RULES FOR FIGURING
THIS OUT

BRONSTED-LOWRY
A C I D S
A hydrogen (H + ) donor
B A S E
A hydrogen (H + ) acceptor
NH
3
+ H
2
O  NH
4
+ +OH -
BASE ACID

CLASSIFY THE ACID/BASE IN THE FOLLOWING
ACCORDING TO BRONTED-LOWRY
•
2

-
3
+
ACID BASE
•
2
2
4
BASE ACID

4
-
3
+

•
Theorist Acid
Arrhenius
Bronsted-
Lowry
Base

WHAT ABOUT THE PRODUCTS?
• They are called conjugates, in Latin, means to join together
• With the reactants, they are known as conjugate acid-base pairs
• A pair meaning out two will be together: no more, no less

CONJUGATES
• The conjugate will be the opposite strength and type on the product side
• An acid will have a conjugate base
• A base will have a conjugate acid
• HCl + H
ACID
2
BASE
O  Cl + H
3
O +
• H
2
O + H
2
SO
4
BASE ACID
 HSO
4
+ H
3
O +

TRY THESE:
• HNO
3
+ H
2
O  H
3
O + + NO
3
-
Acid Base Conj. Acid Conj. Base
• H
2
O + HF  F + H
3
O +
Base Acid Conj. Base Conj. Acid

BUT WHAT IF THEY DON’T HAVE A PROTON (H + ) TO
DONATE!?!!?

LEWIS (LAST, BUT NOT LEAST THEORIST)
A C I D
Accepts a pair of electrons to form a covalent bond
B A S E
Donates an electron pair to form a covalent bond
H + + OH  H
2
O
Acid base

LEWIS ACID OR BASE?
DRAW THE LEWIS STRUCTURE TO HELP
1. H
2
S 1. Lewis Base
2. Lewis Acid 2. BCl
3
3. PF
3
3. Lewis Base

REVIEW TOPICS FOR QUIZ

Decide the B.L Acid/base and conjugates:
1. NH
3
+ H
2
O  NH
4
+ + OH -
2. HBr + H
2
O  H
3
O + + Br -
3. Notice anything special about water?

AMPHOTERIC
•
•
3
2

SELF IONIZATION OF WATER
•
•
2
2

-
+
•

SELF IONIZATION OF WATER (KW)
• Kw is the self ionization constant of water
• Kw = [H + ] x [OH ]
• The bracket [ ] mean concentration
• Kw is equal 1.00x10
-14 M 2
• For a neutral solution [H + ] = [OH ] = 1.00x10
-7 M

KW PROBLEMS
• If the [H + ] is 1.00x10
-5 M, what is the [OH ] ? Is this solution neutral, acidic, or basic?
• Step one: Figure out what you have
 Kw = [H + ] x [OH ]= 1.00x10
-14 M 2
• Step two: plug in your values and solve for [OH ]
 1.00x10
-14 M 2 = [1.00x10
-5 M] x [OH ]
 1.00x10
-9 M
 Step three: decide what range it is in
Acidic because the H + is greater than the OH -

TRY THESE ON YOUR OWN
•
+
-
-2

+
-13
•
-
+
-10

ION PRODUCT CONSTANT (KW)
•
+
-
•
+
-
•
+
-

DECIDE WHETHER ACID, BASE, OR NEUTRAL:
1. [H+]=6.0x10
-10 M
2. [OH-]=3.0x10
-2 M
3. [H+]=2.0x10
-7 M
4. [OH-] =1.0 x10 -7 M
1. Basic
2. Basic
3. Acidic
4. Neutral

• The power of hydrogen!
• Also, known as pH!
• Jot down anything you already know about pH!

P
H CONCEPT
• Proposed in 1909 by Soren
Sorenson as a more practical way to express the [H+]

P
H CONCEPT
• pH = -log [H+]
• If the pH is from <7 it is an acid
• If the pH is 7 it is a neutral
• If the pH is >7 it is a base

pH Common Items

pH Scale

PUTTING LOG IN OUR CALCULATOR!

LET’S TRY ONE!
• What is the pH of a solution with a [H+] of 4.2x10
-10 M?
Is it an acid or base
• > than 7, so it’s a BASE!

PST..
• pH will not have a unit 

TRY THESE ON YOUR OWN
• Calculate the pH of the following and decide if an acid or base:
1.
[H + ]= 0.045 M
2.
[H + ] = 8.7x10
-6 M
3.
[H + ] = 0.0015 M
4.
[H + ]= 1.0x10
-12 M
1. 1.35; acid
2. 5.06; acid
3. 2.82; acid
4. 12; base

HELPFUL HINT HERE!
• If the coefficient (number in front) is 1, then the exponent is the pH!!
• Example: 1.00 x 10-7 M is… pH= 7.00
• What about 1.00 x 10 -9 is… pH = 9.00
 Hold your applause 

BUT WHAT IF YOUR GIVEN [OH-]?!?!
• Use your Kw equation!
• What is the pH of a solution with [OH-] of 3.00x10
-2 M?
•
+
-13
• Then plug it into pH = - log (3.33x10-13 )= 12.5

• Calculate the pH for the following and decide acid or base
1. [H+]=1.00x10-6 M
2. [H+] =0.000200 M
3. [OH ] = 5.60x10
-2 M
• pH=-log[H+]
1. 6.00; acid
2. 3.7; acid
3. 12.7; base

DID YOU KNOW?!?
• Log is a base ten function!
• This comes in handy if we are given pH and have to find
[H+]!
• pH = -log[H + ] when you divide by log to solve for [H + ] it becomes the antilog or 10!
• [H + ] = 10 -pH

LET’S TRY ONE TOGETHER
• Calculate the [H+] for a solution with a pH of 5.00
• [H + ] = 10 -pH
• [H + ] = 10 -5.00 = 1.00x10
-5 M

TRY THESE ON YOUR OWN
• Calculate the [H+]
1. pH= 8.56
2. pH=3.45
3. pH= 10.57
• [H + ] = 10 -pH
1. 2.57x10
-9 M
2. 3.55x10
-4 M
3. 2.692x10
-11 M

MEASURING
P
H
• We can calculate pH, but how do you think we can measure it?
• Have you measured pH before? Maybe with a pool?

MEASURING P
• Using acid/base indicators
• Typically a weak acid or base and turns color at different pH’s
• Some indicators work better for certain solutions and only at 25 o C
• Examples: Brothymol blue, phenolphthalein, universal, pH paper, etc