1. ACIDS and BASES Operational ACIDS BASES Sour Electrolyte – makes ions
in solutions
Perform single replacement
Rxns:
Table J
Any metal above H2 will react with an acid to produce H2(g)
Where found –Table K
Bitter
Electrolyte – makes ions
in solutions
Referred to as
caustic
alkaline
“Feel slippery”
Where found –Table L
Operational
(properties)
List:
HI, HBr, HCl, H2SO4, HNO3
Any group 1 metal bound to OH-
NaOH, KOH, LiOH
Strong

2. “D” INDICATORS: ACIDS BASES Acids turn litmus RED ACID “B”
Bases turn litmus BLUE
BASE
BLUE
Litmus
Colorless
Phenolphthalein
PINK
pH < 7 (below 7)
[H3O+] > [OH-] pH
Note: H+ = H3O+
pH > 7 (above 7)
[H3O+] < [OH-]
Neutral pH=7 is when
[H3O+] = [OH-]
H3O+ is called Hydronium ion
Comes from
H+ + H2O H3O+
OH- is called hydroxide ion

3. ACIDS BASES Types of Acids/Bases Produces OH- PRODUCE H+
H+: is the only positive ion in
solution
Ex. HCl H+ + Cl-
Produces OH-
OH- : is the only negative ion in
solution
Ex. NaOH Na+ + OH-
Arrhenius
Neutralization
It’s when pH =7
Pure water
Net ionic result :
It’s also double replacement reaction
Acid + Base Salt + water
Hx__ + MetalOH Metal with nonmetal + water
H+ + OH H2O
HI + KOH KI + H2O
Ionic

4. ACIDS BASES PROTON DONOR (gives an H ) PROTON ACCEPTOR
H+: is “given” to an acceptor
moves from acid to base
Ex. CH3COOH can give up that
Might see it written HC2H3O2
PROTON ACCEPTOR
H+ : is accepted by the base and
makes a coordinate
covalent bond
Ex. NH3 + H NH4+
The NH3 is the acceptor
Bronsted- Lowry
Conjugate Acid/Base Pairs
Appear on opposite sides of the equation (opposite sides of arrow)
Differ only in an H
If it’s an acid on the left side becomes the base on the right side of arrow
If it’s a base on the left side becomes the acid on the right
Acid/base pairs
NH HSO NH SO42- B A

5. NAMING ACIDS Type of Acid How you name it Binary
2 elements
In compound
Hx___y
Ex. H2S, HCl
Always start with “hydro”
Hydro____________ic acid
Route name of second element
Ex. HCl - hydrochloric acid
H2S – hydrosulfuric acid
Going backwards – hydrobromic acid - HBr
Tertiary
3 or more elements
In compound
Hx___y___z
TABLE E
**NO HYDRO
Look at anion ending in table E
Ends in –ate, change ending to -ic acid
Ex. HClO3—chlorate---becomes chloric acid
Ends in –ite, change ending to –ous acid
Ex. HNO2 – nitrite----becomes nitrous acid
Writing formula-phosphoric acid –PO43-: H3PO4

6. NAMING BASES Type of Base How you name it Any Metal + OH- contains the
OH- ion
**Name metal then add hydroxide
Ex. NaOH—sodium hydroxide
Ex. Ca(OH)2—calcium hydroxide
Writing formula --
Magnesium Hydroxide (criss-cross)
Mg2+ OH- :: Mg(OH)2
organic
Not CH3OH
Make sure
There is a metal

7. Equilibrium constants and pH
Kw – Is the equilibrium constant for water
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
Kw = [H3O+][OH-] = 1.0 x @ 25ºC
pH + pOH = 14
What is the hydroxide ion concentration if th hydronium ion concentration is 1.0 x 10-5M?
1.0 x 10-5M[OH-] = 1.0 x 10-14
[OH-] =
1.0 x 10-14
1.0 x 10-5
= 1.0 x 10-9
Determining pH – always use concentration of H+ ion
pH= -log[H+]
Another way to look at it
[H+] = 1.0 x 10 -pH
The numerical value of exponent = value of pH
pH is a log scale. Each number change is a 10 fold change (factor of 10) 1 14
Acid
Base 7
Neutral H+
OH-
As you go H+ decrease, OH- increase, pH increase
As you go H+ increase, OH- decrease, pH decreases
If the pH changes from 4 to 8, what is the change in H+ concentration
4 to 5 to 6 to 7 to 8 10
10x10x10x10=10,000 fold change DECREASE in H+

8. Practice problems What is the pH of 1.0 x 10-3 M solution of NaOH?
What is the pH of 1.0 x 10-3 M solution of HCl?
HCl – is an acid so = [H+]
[H+] = 1.0 x 10-3
pH = 3
What is the pH of 1.0 x 10-3 M solution of NaOH?
NaOH – is a base so = [OH-]
Concentration of [OH-][H+]=1x10-14
[H+] = 1 x 10-11
pH = 11
What is the pH of M solution of HCl?
M = 1 x 10-5 =[H+]
pH = 5
What is the pH of M solution of NaOH?
NaOH – is a base so = [OH-]
Concentration of [OH-][H+]=1x10-14
[H+] = 1 x 10-11
pH = 11
NaOH = 1x10-3

9. TITRATION
Use of a known solution to calculate the concentration of an unknown solution
Buret
USE TITRATION FORMULA
MAVA = MBVB VB
Solution
Of base. We find MB
How much base used will
Equal how many moles
Acid is there.
If 50 mL of 0.5M HCl is used to completely neutralize 25 mL of KOH, what is the molarity of the base?
MAVA = MBVB
(0.5M)(50mL) = MB(25mL)
1.0 M = MB
Solution of known concentration
With a known volume, VA
known MA
Moles H+ = moles OH-
Phenol (indicator)
Place the indicator in the unknown solution
When it changes color you’ve reached the equivalence pnt - you have neutralized it!

10. OTHER Indicators – TABLE M
Below the 1st # - 1st color listed
Above the 2nd # - 2nd color listed
Between the #’s on the chart – will be a blend of the colors
Ex. A solutions pH = 5.8 then
In methyl orange – color would be yellow
In bromthymol blue – color would be yellow
In litmus – color would be a reddish-purple (in middle)