Chapter 7 – Acids & Bases Name
Number Item
On Top This page with your name on it
1 Notes 7.1 Common Acids & Bases Notes
2
7.2 pH: A Powerful Scale Notes
3
7.3 The Prop. of Acids & Bases Notes
4
7.4 Neutralization Reactions Notes
5
CYU P 218 1-4
6
CYU P 225 1-5
7
CYU P 230 1-5
8
CYU P 236 1-5
9
BLM 7-5
10 BLM 7-6
11 BLM 7-10
12 BLM 7-8
13 BLM 7-12
14 BLM 7-13
15 BLM 7-14
16 BLM 7-15
17 BLM 7-16
18 BLM 7-17
19 BLM 7-19
20
21
Ch Review
Lab
1
16
15
21
12
10
9
43
15
18
27
12
Value Your
Mark
5
5
5
5
20
21
18
13
40
30

1.
a.
often occur b.
eg) in sore muscles (not enough oxygen present during work) c.
eg) many fruits including
2.
Properties: a.
Taste
and b.
Feel c.
d.
(corrosive)
Arrhenius found that acids are compounds and when dissolved (aq) they
into their ions. He defined acids as substances that produce

ions in solution.
HCl ions separate in water to make

The more H + ions present in solution the and
the acid
3.
a.
often found naturally in or . b.
Materials which are bases are referred to as being or .
 Eg) is a base found in cinchona bark and used to make tonic water and medicine for malaria.
 Eg) bases are used to make .
4.
Properties: a.
Taste b.
Feel c.
(corrosive) d.
Arrhenius found that bases are ionic compounds and when dissolved (aq) they separate into their ions. He defined bases as substances that produce hydroxide ions in solution. i.
NaOH separates in solution to make and ii.
The more OH present in solution the the base
Na(OH) Na + + OH -
5.
NOTE: Ammonia NH
3
is a base when dissolved in water. Why? a.
The ammonia atom steals one from water to form b.
ammonia vs ammonium ion .
P 218 1-4 (20), BLM 7-5 & 7-6
2
.

 Indicators
 molecules which aq) ions present. with changes in the amount of
Eg) phenolphthalein – turns in base, stays
Eg) Litmus paper: Blue  Red in Acid
Red  Blue in Base aq) ions or
in acidic and neutral conditions.
DO NOT TELL THE STRENGTH OF THE ACID OR BASE
Indicator
Red litmus
Blue litmus
Phenolphthalein
Bromothymol blue
Colour in acid Colour in neutral water Colour in base
Methyl orange
Red cabbage juice
Note: VERY little indicator is needed in the tests. Too much indicator can change the pH of the acid or base. Example: Phenolphthalein is a weak acid.
pH – stands for “ ”
– a scale used to measure the
pH meter OR by looking at the
of an acid or base. Is measured with an
on Universal indicator paper.
Note: neutral solutions have numbers of H + and OH ions.
H
2
O  H + + OH so pure water is neutral.
Fill in the scale below with 10 examples from p 219
Strongest
Acid
Neutral
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14

Each change in 1 pH changes the strength by a factor of 10.
 Eg) pH 1 is 10 3 or 1000 times as strong an acid as pH 4.
Strongest
Base
P 225 1-5 (21), BLM 7-8
3

The strength of an acid is determined by 2 factors:
1) – how much
2)
is dissolved in water.
– the number of molecules that will
Concentration Percent Ionization
H
2
SO
4
 2H + + SO
4
2-
100 all ionize (100%) Strong
Strong
99mL HCl
1mL H
2
O
Weak
1mL HCL
99mL H
2
O
H
2
CO
200
3
 2H + + CO
3
2-
only 1 ionizes (.5%) Weak
Note: - For Percent Ionization the # of H+ ions in the acid DOES NOT DETERMINE THE STRENGTH OF
THE ACID
The strength is only determined by the amount of H+ ions that go into
to release H+ ions for every 100 molecules dissolved.
Not all acids release H+ ions equally easily. (Generally the more bond the the acid.)
the
-
Eg) CH
3
COOH has 4 H atoms but only 1 ionizes:
CH
3
COOH  CH
3
COO + H + Acetic acid
Copy the charts for common acids and bases on p 227.
Some Important Acids
Name Formula Notes
4

Some Important Bases
Name Formula Notes
Why is ammonia considered a base when dissolved in water? HINT: Guess the products of NH
3
+ H
2
O
P 230 1-5, BLM 7-12, 7-13(class activity), 7-14
5

Acids and Bases react with each other to form a salt and water.
Eg) HCl + NaOH  NaCl + H
2
O dbl displacement
Complete and balance the reactions, name the salts.
H
2
SO
4
+ KOH  Salt:______________
H
2
SO
4
+ NaOH 
HNO
3
+ Ca(OH)
2

H2CO3 + Mg(OH)
2

Salt:______________
Salt:______________
Salt:______________
Making Acids
Oxides – compounds containing one element with oxygen.
Eg) CO, CO
2
, Al
2
O
3
, SO
3
, NO
2
Non-metal oxides – compounds containing a single non-metal combined with only oxygen.
ALL non-metal oxides react with water to form acids.
Eg) CO
2
+ H
2
O  H
2
CO
3
Eg) SO
3
+ H
2
O  carbonic acid (makes rain slightly acidic) sulphuric acid
P 236 1-5 & BLM 7-16, 7-17, 7-19 and Text Review P 238-239 1-17, 20, & 21
6