5-12-15
• TURN IN ACID/BASE WS
• TURN IN STUNTED SOL REVIEW
• GET YOUR SCANTRON FROM THE FRONT
• GET OUT ACIDS NOTES

NAMING ACIDS
• ACIDS - ALL HAVE H+ , SO THE NAME IS BASED ON THE ANION (- PART)
Anion ending
Rule
-ide Hydro(stem)ic acid
Example
HCl has Chloride =Hydrochloric acid
HBr has bromide = Hydrobromic acid
-ite (stem)ous acid
HNO
2 has nitrite = nitrous acid
HClO
2 has chlorite = chlorous acid
-ate (stem)ic acid H
3
PO
4 has phosphate = phosphoric acid
H
2
SO
4 has sulfate = sulfuric acid
HNO
3 has nitrate = nitric acid
*S compounds use (sulfur) as the root
* P compounds use (phosphor) as the root

FORMULAS OF ACIDS
• USE H+ AS THE CATION.
• DETERMINE THE ANION FROM THE NAME.
• COMBINE ENOUGH OF EACH TO BALANCE OUT THE CHARGE.
Example
Phosphorous acid anion hydronitric acid nitride ions
H + N -3 phosphite H + PO
3
-3 carbonic acid carbonate H + CO
3
-2 formula
H
3
N
H
3
PO
3
H
2
CO
3
• Bases are named like any other ionic compound: Cation Anion
• Formulas are “ “ “ “ “
Fill in

BASES
Naming Bases = like any ionic compound
Cation anion (change ending to –ide if not a polyatomic ion)
NaOH = ____________________
Ca(OH)
2
=______________________
Base formulas – like any ionic compound
EX: Magnesium hydroxide
Mg +2 OH = Mg (OH)
2

NEUTRALIZATION REACTIONS
Reaction in which an acid and a base react in an aqueous solution to produce a salt and H
2
O
(Double Replacement reaction)
Steps:
1.
Write acid and base formulas
2.
Write HOH(water) as product
3.
Combine remaining cation and anion using subunits to make neutral compound (salt)
4.
Balance
Example:
HNO
3
H
2
SO
4
+ KOH

2HCl + Mg(OH)
2
+ 2NH
4

OH 

PROPERTIES OF ACIDS
• TURNS LITMUS RED
• HAVE PH LESS THAN 7
• TASTE SOUR
• REACTS WITH BASES IN A NEUTRALIZATION
REACTION
• REACTS WITH METALS TO PRODUCE H
2
• EX: LEMON JUICE

PROPERTIES OF BASES
• TURNS LITMUS BLUE
• HAVE A PH GREATER THAN 7
• TASTE BITTER
• FEEL SLIPPERY
• NEUTRALIZE ACIDS
• EX: SOAP

Uses of Acids and Bases in our every day Life:
HCl : Pool Acid, cleaning metals, leathering processes
Nitric Acid: Fertilizers, Explosives, extraction of gold
Tartaric Acid: Soft Drink manufacturing, an agent to induce vomiting (emetic)
Benzoic Acid: Salts used to preserve foods
Carbonic Acid: Carbonate drinks
Ethanoic Acid: Vinegar
Ammonia: Fertilizer, petroleum industry, synthesis of latex
Aluminum hydroxide: Making of ant-acids
Calcium Hydroxide: Cement, limewater, sewage treatment
Sodium Hydroxide: Soaps, detergents, cleaners
Magnesium Hydroxide: Antacids, antiperspirant, neutralize waste water

• ACIDS AND BASES ARE BOTH STRONG OR WEAK
ELECTROLYTES (CONDUCT ELECTRICITY)
• ELECTROLYTES = DISSOCIATE (BREAK APART INTO
IONS) WHEN DISSOLVED
• STRONG = COMPLETELY
• WEAK = PARTIALLY
• NON = NOT AT ALL

TYPES OF ACIDS/BASES
Arrhenius Acids/Bases 1884
Acids release H+ into water
Bases release OH- into water
Ex: Acid: HCl (aq)

H+ (aq) + Cl- (aq)
Base: NaOH (aq)

Na+ (aq) + OH- (aq)
Monoprotic = acid that contains 1 proton (H+)
Ex.) HBr, HC
2
H
3
O
2
Diprotic = 2 protons, 2H + Ex.) H
2
SO
4
Triprotic = 3 protons, 3H + Ex.) H
3
PO
4

BRONSTED-LOWRY ACIDS/BASES 1923 - 2 INDEPENDENT SCIENTISTS
• ACID = H + DONOR
• BASE = H + ACCEPTOR
• EX: NH
3
+ HOH ↔ NH
4
+ + OH -
AMPHOTERIC = SUBSTANCE THAT ACTS AS BOTH AN ACID AND A BASE
• NH
3
+ HOH ↔ NH
4
+ + OH -
• HCL + HOH ↔ H
3
O + + CL -
LEWIS ACIDS/BASES
• ACID = ACCEPTS A PAIR OF E-
• BASE = DONATES A PAIR OF E-

Strong Acids (Memorize)
HBr = Hydrobromic acid
HCl = Hydrochloric acid
HI = Hydriodic acid
HNO3 = Nitric acid
HClO4 = perchloric acid
H2SO4 = Sulfuric acid
All other acids are weak (sauce)
Strong acids dissociate completely
HCl

H + + Cl- (break apart 100%)
Weak Acids
Dissociate (ionize) only slightly
HC
2
H
3
O
2
(99%) + H
2
O ↔ H
3
O + C
2
H
3
O
3
(1%)

Strong Bases (memorize)
Ba(OH)
2
Ca(OH)
2
KOH
NaOH
LiOH
• CONJUGATE ACIDS/BASES
• ****PRODUCTS*** (RIGHT SIDE OF ARROW ONLY)
• CONJUGATE ACID = PARTICLE FORMED WHEN BASE GAINS A H +
• CONJUGATE BASE = PARTICLE FORMED WHEN ACID HAS LOST/DONATED H +
EX: NH
3
+ H
2
O  NH
4
+ + OH -
*** BASE BECOMES CONJ. ACID
*** ACID BECOMES CONJ. BASE
EX: HCL + H
2
O  H
3
O + + CL -

H + & ACIDITY
• H + FROM WATER (SELF IONIZATION) : H
2
O( L )  H + ( AQ ) + OH ( AQ )
• H + JOINED TO H
2
O AS HYDRONIUM (H
3
O + )
• [OH ] = 1 X 10 -7 M [ ] = MOLARITY CONCENTRATION
• [H + ] = 1 X 10 -7 M
• [OH ] = [H + ] IN PURE WATER, SO IT IS A NEUTRAL SOLUTION
• K
W
= WATER DISSOCIATION CONSTANT
• K
W
= [H + ] [OH ] = 1 X 10 -14
• Acidic Solution
[H + ] > [OH ]
• Basic Solution (Alkaline)
[H + ] < [OH ]
• Neutral solution
[H + ] = [OH ]

5-13-2015
•
DO NOT TURN IN YOUR HOMEWORK
•
ANY QUESTIONS FROM LAST
NIGHT’S HOMEWORK?
•
LECTURE ON PH
•
PH DEMO
•
SOL REVIEW

• Soren Sorensen (potenz Hydrogen) “power”
• Easier way to express [H + ], from 0-14.
pH = - log [H + ]
Acidic Solution
Neutral Solution
Basic Solution pH <7.0
pH = 7.0
pH >7.0
[H + ] > 1 X 10 -7
[H + ] =1 X 10 -7
[H + ] <1 X 10 -7

POH

•
Find pH if [H + ] = 1 X 10 -9
•
Find [H + ] if pH =6
•
Find pOH if pH = 6.8
•
Find pOH if [H + ] = 1 X 10 -9
•
Find [OH ] if [H + ] = 1 X 10 -9
EXAMPLES

INDICATORS = PH DEMO

1. What are the H+ Concentrations for the following pH values?
6.3, 8, 12.5

WHAT IS THE OH- CONCENTRATION OF A SOLUTION
WITH A H+ CONCENTRATION OF 1 X 10 -4

Bronsted-Lowry Acids/Bases
Acid = H + Donor
Base = H + Acceptor
Lewis Acids/Bases
Acid = accepts a pair of e-
Base = donates a pair of e-
Arrhenius Acids/Bases 1884
Acids release H + into water
Bases release OH into water

5-14-15
• TAKE A QUIZ FROM THE FRONT. COMPLETE
(WITH NOTES) TURN IN UP FRONT
• TAKE A COPY OF THE STUNTED SOL WORKSHEET
(YES YOU’VE SEEN THIS BEFORE)
• TOMORROW THERE IS A LAB. NO OPENED TOED
SHOES = AUTOMATIC 15 POINT DEDUCTION

TITRATIONS:
METHOD OF DETERMINING THE CONCENTRATION
OF AN ACID OR A BASE.
STEPS FOR CALCULATIONS
1. WRITE A BALANCED NEUTRALIZATION EQUATION.
2. CALCULATE THE MOLES OF KNOWN SOLUTION USING : MOL
= M*L
3. USE THE BALANCED EQUATION TO FIND THE MOLES OF
UNKNOWN STARTING W/ MOLES OF KNOWN. SET UP A
PROPORTION, DIVIDING BY THE COEFFICIENTS.
4. CALCULATE THE CONCENTRATION OF UNKNOWN, USING
CALCULATED MOLES AND MEASURED VOLUME. M=MOL/L
EX. WHAT IS THE MOLARITY OF PHOSPHORIC ACID, IF 15.0 ML OF
THE SOLUTION IS TITRATED BY 38.5 ML OF 0.15 M SODIUM
HYDROXIDE?

WHAT IS THE MOLARITY OF PHOSPHORIC
ACID, IF 15.0 ML OF THE SOLUTION IS
TITRATED BY 38.5 ML OF 0.15 M SODIUM
HYDROXIDE?

EX: How many mL of 0.45M HCl must be added to
25.0 mL of 1.00 M KOH to make a neutral solution?

TITRATION GRAPH

K
A
, K
B
, K
EQ
• STRONG ACIDS & BASES = DISSOCIATE 100%
(ALL OF IT IONIZES OR BREAKS APART INTO IONS)
• H
2
SO
4
 2 H + + SO
4
-2
0% 100%
• WEAK ACIDS & BASES = ONLY DISSOCIATE PARTIALLY
• H
3
N  3H + + N -2
95% 5%

EQUILIBRIUM
• EQUILIBRIUM = RATE OF FORWARD AND REVERSE REACTIONS ARE
EQUAL (AMOUNTS OF PRODUCTS AND REACTANTS DO NOT
CHANGE)
• WHEN WE HAVE EQUILIBRIUM, WE CAN WRITE, K
A
, K
B
, K
EQ
• K
EQ
= EQUILBRIUM CONSTANT
K
EQ
= [PRODUCTS] COEFF
[REACTANTS] COEFF

K
A
& K
B
• K
A
= ACID DISSOCIATION CONSTANT. A MEASURE OF HOW MUCH A WEAK
ACID BREAKS INTO IONS. K
EQ
FOR A WEAK ACID:
• H
2
X  2H + + X -2 K
A
=
• EX: H
3
PO
4
 3H + + PO
4
-3 K
A
=
• LARGER K
A
VALUE = STRONGER WEAK ACID
•
• K
B
= BASE DISSOCIATION CONSTANT. A MEASURE OF HOW MUCH A WEAK
BASE BREAKS INTO IONS. K
EQ
FOR A WEAK BASE
EX: BE(OH)
2
 BE +2 + 2OH K
B
=
• LARGER K
B
VALUE = STRONGER WEAK BASE

5-15-2015
• YOU MAY TURN IN LAST NIGHTS
HOMEWORK AT THE END OF CLASS
TODAY WITH NO LATE PENALTY
• DEMO FOR LAB
• LAB
• ADDITIONAL WS IF WE (YOU) ARE
NOT ON TASK
Keep lab safe today