1.
List the properties of acids and bases:
ACIDS
2.
BASES
Acids and bases are both electrolytes, as they can conduct electricity when
dissolved in water. Some are good conductors while others are not so good.
 What is the difference?
 This is the same thing that differentiates STRONG versus WEAK acids and bases:
STRONG Acids and Bases
WEAK Acids and Bases
3.
Ha! Get it? Basics? I know…I’m funny!!!
So, let’s get some basics down:
a)
acid:
b)
base:
c)
hydronium ion:
d)
hydroxide ion:
e)
self-ionization of water:
f)
neutral solution:
g)
ion-product constant for water (Kw):
h)
acidic solution:
i)
basic solution:
j)
pH:
k)
pOH:
pH + pOH = _______!
4.
Remember this??? Name these compounds:
a)
HCl ________________________________
g)
NaOH _______________________________
b)
H2SO4 _____________________________
h)
Ca(OH)2 ____________________________
c)
HNO3 ______________________________
i)
KOH _________________________________
d)
H3PO4 _____________________________
j)
Al(OH)3 _____________________________
e)
H2CO3 _____________________________
k)
Mg(OH)2 ____________________________
f)
CH3COOH _________________________
l)
NH3 __________________________________
5.
Remember, acids and bases are opposites: when the concentration of H3O+1 goes
up, the concentration of OH-1 goes down, and vice versa!
 Our pH scale reflects this concept, as 7 is neutral, below 7 is acidic and above 7 is basic:
 We can check the pH of solutions by using an indicator:
 Of course, in more sophisticated labs, there are pH meters available that can
measure with a precision of 0.01 pH units – just like Don’s!
“It’s a pH meter!”
6.
The Brönsted-Lowry classification of acids and bases is a more encompassing
classification system than what we have seen so far (known as Arrhenius). While
the Arrhenius system was revolutionary (from 1890), it is limited to aqueous
systems and does not account for substances that act as both acids and bases.
 Brönsted-Lowry Acid:
 Brönsted-Lowry Base:
Brönsted-Lowry in Action!
NH3
+
H2O
↔
NH4+1
+
OH-1
HCl
+
H2O
↔
H3O+1
+
Cl-1
*Do you notice something weird about
water in the above equations???
“Am I an
amphoteric?”
7.
What is a BUFFER?
A buffer solution is an _______________________ _______________________ consisting of a
mixture of a __________________ acid and its conjugate ____________________ or a
_________________ base and its conjugate ____________________. It has the property that the
pH of the solution changes __________________________________ when a small amount of
____________________ acid or base is added to it. Buffer solutions are used as a means of
keeping pH at a nearly ________________________ value in a wide variety of chemical
applications. Many _________________________________ thrive only in a relatively small pH
range; an example of a buffer solution is _______________________.
Buffer solutions are necessary to keep the correct pH for _______________________ in
many organisms to work. Many enzymes work only under very precise conditions; if
the _____________ strays too far out of the margin, the enzymes slow or stop working and
can _____________________________, thus permanently disabling its catalytic activity. A
buffer of ____________________________ _______________ (H2CO3) and
_____________________________ (HCO3−1) is present in blood plasma, to maintain a
blood pH between _________________ and _________________.
Industrially, buffer solutions are used in ____________________________ processes
and in setting the correct conditions for ________________ used in coloring fabrics. They
are also used in chemical analysis and calibration of _______________________________!
 Who is “buffer”??? 
8.
Neutralization
Because of the fact that [H3O+1] x [OH-1] = 10-14 M2, high concentrations of H3O+1
and OH-1 cannot coexist! When an acid and a base are mixed, the hydronium ions
and hydroxide ions react to form….WATER! The left-over spectator ions will then
combine to form a salt. This is known as a…
 Neutralization Reaction:
9.
Titration
A useful tool in analytical chemistry is the titration, which is a method used to
determine the concentration of an unknown solution by using another solution
with a known concentration. Titrations work GREAT with acids and bases,
because we can track the neutralization reactions through pH, and we can “see”
when the solution becomes neutral through indicators or a pH meter!
 Equivalence point:
 End point:
 Standard solution:
The calculations for acid/base titrations can become rather complex. However,
the ones we will do in lab involve a 1:1 ratio of H3O+1 and OH-1 so we can use an old
friend (with a small twist) for our calculations: M1V1 = M2V2 will become…
MaVa = MbVb
…where “a” stands for acid and “b” stands for base!