Characteristics of Acids: Table K
 Electrolytes
 pH
scale: less than 7
 Litmus: RED
 Phenolphthelein: colorless
 Contains a high concentration of Hydrogen
ions (H+) or Hydronium Ion (H3O+)
H2O + H+ = H3O+
 React with certain metals to produce
hydrogen gas (H2) – TABLE J
Metal must be higher
than H2 to react
Characteristics of Bases: Table L
 Electrolytes
 pH
scale: greater than 7
 Litmus: BLUE
 Phenolphthelein: pink
 Contains a high concentration of Hydroxide
ions (OH-)
 Tastes bitter; feels slippery/soapy
Characteristics of Salts

An ionic compound that has positive ions other
than hydrogen (H+) and negative ions other than
hydroxide (OH-).

Example: NaCl (Na+ and Cl-).

Salts conduct electricity (salts are electrolytes).

ACIDS, BASES & SALTS ARE ELECTROLYTES
Beware of Tricks . . .

Organic Acids have a functional group –COOH,
so when you see a compound with carbon and
this functional group it is an acid!!
Ex: CH3COOH

Alcohols have a functional group –OH (hyroxyl),
not OH- (hydroxide); alcohols are not bases!!
Ex: CH3OH
Table K
Table L
Strong Acids & Bases
HCl
 HBr
 HI
 HNO3
 H2SO4
 HClO3
 HClO4

NaOH
 KOH
 Ca(OH)2
 LiOH
 RbOH
 CsOH
 Ba(OH)2

NH3 is a weak base!!
ARRHENIUS THEORY OF ACIDS & BASES
An Arrhenius Acid has H and releases H+ in
an aqueous solution.
 The H+ ion is the only positive ion in these
solutions. The H+ ions are always attached to H2O
forming H3O+ (hydronium ions).

An Arrhenius base has OH (hydroxide) and releases
OH- (hydroxide ion) in an aqueous solution.
 The OH- ion is the only negative ion in these
solutions.

Bronsted-Lowry Theory (Alternate
Acid-Base Theory)
Bases
Accept
Acids
Donate
 Bases:
H+ acceptor (proton
acceptor)
 Acids:
H+ donor (proton
donor)
Conjugate Acid Base Pairs
1. NH4+ + OH- → NH3 + H2O
2. H3PO4 + NO2- → HNO2 + H2PO4-
3. HI (aq) + H2O (l) → H3O+ (aq) + I- (aq)
Some substances can sometimes act like an acid and
sometimes act like a base. Examples are H2O &
HSO4-
Neutralization Reactions

ACID + BASE = WATER + SALT (IONIC SOLID)
Titration

Titration is a lab process in
which a volume of a solution
of known concentration is
used to determine the
concentration of another
solution.
MAVA =MBVB
Example 1:

What is the molarity of HCl (aq) if 10. milliliters of 4.0 M
NaOH (aq) neutralizes exactly 20. milliliters of HCl (aq)?
Example 2:

What is the molarity of NaOH (aq) if 10. milliliters of 2
M HBr (aq) neutralizes exactly 5. milliliters of NaOH
(aq)?
pH Scale
 Movement
from one whole number to the
next represents a change by a power of 10.
 Acids:
1-7, [H3O+] > [OH-]
 Neutral: 7, [H3O+] = [OH-]
 Bases: 7-14, [H3O+] < [OH-]
Meaning of pH & pOH
pH = -log[H+]
pH = -log[1.0X10-5] = -(-5) = 5
 The solution is acidic.

pOH = -log[OH-]

pOH is the concentration of OH- instead of the
concentration of H+

pH + pOH = 14