Name:
Unit 2 Outline —Chemistry
Chapter 5: Acids & Bases
DAY
2
3
4
5
6
7
-
DATE
OUTLINE
5.lNotes (slides #1-4) (p.130)
Assignment: Read text p.220-227
Do Ch.5 Key Terms (p.129)
Do Acids versus Bases w.s. (p132).
Do Acid/Base Data Booklet w.s. (p.133)
5.1 (slides 5-8) (p.131)
Read Acid/Base Lab in preparation for tomorrow (p.137-138)
Assignment: Read text p.228-233
Do Names of Acids w.s. (p.134)
Do Names & Formulae of Acids & Bases w.s. (p.135)
Acid/Base Lab (p.137-13 8)
5.2 Notes (p.136)
Assignment: Read text p.234-243
Do Recognizing Acids, Bases and Salts w.s. (p.139)
Do Acid-Base Neutralization Rx. w.s. (p.140)
Do Metal oxides and Non-metal oxides w.s. (p.141)
Study_for_Quiz_next_class!
5.1/5.2 Quiz Acid naming, MOB, NOA
5.3 Notes (p.142)
Assignment: Read text p.244-251
Do Recognizing Org & Inorg Compounds w.s. (p.143)
Do Organic Comp vs. Inorganic Comp w.s. (p.144)
Study for Quiz next class!
5.3 Quiz
Assignment: Read Summary Notes (p.325-327)
Do 5.1, 5.2 and 5.3 Assessment w.s. (p.145-146)
Do Ch.5 Text Review p.252-253#l,2,S,6,9,l 1-13,
15-18,1 9(a,c,e),20(a,c,e),2 1-23 (p.
1 47-148)
Study for Test next class!
Ch.5_Pckg_Due_next_class!_(Do_Self evaluation)
Ch.5 Test (25 multiple choice questions on scantron bring a pencil).
—
—
Ch.5 Pkg Due
SUMMARY STUDY NOTES: p.325-327
Chapter 5: Acids & Bases KeV Terms
1.
Acid
2. Base
3. Indicators
4. pH
5. Salts
6. Non-metal Oxides
7. Metal Oxides
8. Organic Compounds
—
9, Inorganic Compounds
Key Term
Definition
Example/Graphic
5.1 Acids and Bases
•
are very common.
and
•
and
Acids and bases can be very
try to identify an acid or base by taste or touch!
pH Scale
of acids and bases is measured on the pH scale
The
0123456
7
891011121314
Neutral
Acids
—
pHabove7=
pH7=
pHbelow7=
Bases
more acidic
Each decrease of 1 on the pH scale indicates
•
Eg. pH 4 is 10 X more acidic than pH 5 & pH 3 is 1000X more acidic than pH6
pH Indicators
•
be determined by sight.
The pH of acids and bases
—
—
Instead, pH is measured by other chemicals called
that measures the electrical conductivity of the
or by a
solution using electrical probes to measure how solutions conduct electricity.
based on the solution they are placed in.
pH indicators change
is the most common indictor.
-
(<7).
(>7) & Red
2 colours of litmus paper: Blue =
Acids
•
—
—
•
may be able to identify it as an acid.
If you know a compound’s
Acids often behave like acids only when dissolved in
Therefore, acids are often written with subscript (aq)
=
=
water
The chemical formula of an acid usually starts with
—
Acids with a carbon usually have the C written first.
•
HCI
=
(aq)
hydrochloric acid, HNO
=
3(aq)
nitric acid, CH COOH
3
=
(aq)
acetic acid
Naming Acids
Hydrogen+...-ide=Hydro...icacid
—
•
HF
hydrogen fluoride = hydrofluoric add
=
(aq)
—
Hydrogen+...-ate=...icacid
•
H CO
—
Hydrogen +
•
= hydrogen carbonate = carbonic acid
3(aq)
2
.-ite =
..
.ous acid
= hydrogen sulphite = sulphurous acid
H SO
2
. .
3(aq)
Bases
•
If you know a compound’s chemical formula, you
—
—
may be
able to identify it
as a
Bases, like acids, often behave like bases only when dissolved in
Therefore, bases are often written with subscript
•
The chemical formula of a base usually ends with
•
Examples of
common bases:
NaOH
,
(aq)
Mg(OH)
(aq)
=
aqueous
Ca(OH)
,
,
NH
2(aq)
2(aq)
=
water
OH
4
(aq)
Production of Ions
•
in
Acids and bases can conduct electricity because they release
solution.
+
—
—
The
—
ions, H
Acids release
OH
Bases release
pH
(aq)
(aq)
of a solution refers to the
+
Square brackets are used to signify concentration,
[H
of ions
(aq)
], [OH
it
has.
(aq)
]
+
•
High [H
(aq)
High [OH
I
very acidic
=
(aq)
]
very basic
=
+
—
have BOTH high [H
A solution
(aq)
I
each other out and form water. This process is called
+
-H
(aq)
+OH
(aq)
->HO
2
()
and [OH
(aq)
j; they cancel
i
Use with textbook pages 220-229.
AcId
1. Compare and contrast acids and bases by completing the lollowing table.
-
Iclle
p14
tt to look br in
denal bguiju
cglciois
e&sct4cal conQMcfly
ego
e)CsspleS
2 Classify each of the following as an add or a base,
(a)
+
4
HPO
OH
4
(b)NH
(c) Mg(Ol(d)hasapHof4.
(e)
(U
has a pH of 9
suiphurous acid
hydrogen bromide
(h) potassium hydroxide
(i) causes methyl orange to turn red
U)
causes phenolphthalein to turn pink
(k) causes indigo carmine to turn yellow
(I) causes bromothym I blue to turn yellow
Block:_______
Name:________________________________
Date:________
5.1 Acid/Base Data Booklet Worksheet
Science 10
Assignment
Use your data book to answer the following questions.
1. For each of the following, write the corresponding pH values:
a) acid:
b) base:
c) neutral:
2. What color is litmus paper in an acidic solution?
3. What color is bromothymol blue at the following pH levels?
a)
pH5:
b) pH7:
c) pH9:
4. Solution A has a pH of 3. Solution B has a pH of 6.
a) Which solution is more acidic?
b) How many times more acidic is it?
5. Complete the following chart:
Indicator
I
Color at p11 1
Color at pH 7
Color at pH 10
Red litmus paper
Blue litmus paper
6. If methyl red is ORANGE what is the pH range of your solution?
7. If bromthymol blue is YELLOW and methyl orange is YELLOW what range is you pH
solution?
8. What color will phenolphthalein be if placed in a bleach solution?
9.
Write the pH value you would expect for each of the following items:
a)
milk
d) grapes
b) lemons
e) water
c) soap
f) baking soda
13’3
Date
Name
Use with textbook pages 225-226.
c cc
1. An acid wfll have the suffix “—ic add” at the end of its name when the negative
ion has a suffix
For example, “hydrogen carbonate (H
CO is called
2
“carbonic ack1.
Z An add will have the suffix “-ous acid” at the end of its name when the negative
ion has a surix
For example, “hydrogen suiphite 3
8”
2
(H
)
0 is cailed
“suiphurous scd”
3. What is the name of each of the following acids?
CO
2
(a) H
(b) CHCOOH
3 P0
(c) H
4
2
(d)KCIO
(e) H
S0
2
(1 HNO
3
g)HF
HC[
4. What is the chemical formula for each of the following acids?
(a) hydriodic acId
sulphuric acId
(c) perchioric add
(ci) nitrous add
—
chioric add
(t) hydrobromic add
phosphorous acid
(h) hypochiorous add
Block:_______
Name:_______
Science 10
Date:
5.1 Names & Formulae of Acids & Bases
1. a) How can you recognize an acid by its chemical formula?
b) Which acid is an exception to this rule?
2. Complete the following table of acids. The first row has been completed as an example.
Name of Substance
a) hydrogen sulphide
Chemical Formula
Name of Acid
S
2
H
hydrosulphuric acid
0
3
C
2
H
b)
phosphoric acid
c)
d) hydrogen chlorate
sulphurous acid
e)
OOH
CH
C
3
f)
g) hydrogen iodide
3. How can you recognize a base by its chemical formula?
4. Complete the following table of acids and bases. Indicate whether each compound is an acid or a base.
Name of Substance
a) hydrochloric acid
b)
Chemical Formula
Acid or Base?
HC1
Acid
NaOH
c) hydrogen nitrate
d) magnesium hydroxide
e) chlorous acid
f)
H
NH
O
4
j-)
5.2 Notes
[3b
Block:
Name:
Date:
5.1 Testin2 for Acids and Bases
Science 10
Lab
Abstract:
By the 1500’s alchemists recognized a certain group of substances that had a sour taste. They called this group of
substances acids, from the Latin word acidus, meaning “sour”. Acids were known to react with some metals. By 1800,
early chemists knew that the reaction of an acid with certain metals would produce hydrogen gas. Today chemists
• turns blue litmus paper red
define an acid as any compound that:
• tastes sour
• reacts with some metals to produce hydrogen
• conducts electricity when dissolved in water
Early scientists also recognized another group of compounds that they called alkalis. They made alkalis by dissolving
such materials as wood ashes or seaweed in water and then evaporating the liquid. These compounds were used both as
cleaning agents and to make other cleaning agents, such as soap. The alkalis are now called bases. A base is a
• turns red litmus paper blue
compound that:
• has a bitter taste
• feels slippery
conducts electricity when dissolved in water
When a base solution reacts with an acid solution, a third type of compound results. This compound often has a saltlike taste. Evaporating the liquid in such a solution yields a solid crystalline substance, which early chemists called “an
earth.” Modern chemists call this compound a salt. Table salt and bath salts are common examples of salts.
In ancient times, the most common salt, sodium chloride (NaC1), or table salt, was used to purchase slaves and to pay
Roman soldiers. When there was no refrigeration, salt was used to preserve foods. Humans have used salt for at least
5000 years as a food preservative.
Not all compounds are acids, bases, or salts. Common table sugar may look like table salt, but it is not a salt and cannot
be made by mixing an acid and a base. Nevertheless, this grouping of compounds (acids, bases, and salts) is still used
today to classify many of the compounds in chemistry.
Acids and bases can be distinguished from one another by the colour they turn certain indicators, such as litmus paper,
bromothymol blue, and phenolphthalein.
Purpose:
Part 1:
Part 2:
To observe the behavior of acids and bases when they are added to various types of indicators.
To identify the six unknown solutions as acids or bases or salts.
Materia’s:
Blotting plate
Hydrochloric Acid solution
Red litmus paper
Blue litmus paper
Bromothymol blue solution
Set of six unknown solutions
Phenolphthalein solution
Sodium hydroxide solution
Procedure:
Part 1: Characterization of Acids and Bases
1. Place a few drops of HC1 in 4 dips in the blotting plate.
2. Place a few drops of NaOH in the next 4 dips in the blotting plate.
3. Add a few drops of phenolphthalein in the top dip in both the HC1 & NaOH columns.
uid
2
dip in both columns.
4. Add a few drops of bromothymol blue indicator in the
rd
3
dip in both columns.
5. Place a small piece of red litmus paper in the
6. Place a small piece of blue litmus paper in the last dip in both columns.
7. Record all observations in your data table.
Part 2: Unknown Solutions of Acids and Bases
1. Place a few drops of unknown solution A in 4 dips in the blotting plate.
2. Add a few drops of phenolphthalein in the top dip with the Unknown A solution.
3. Add a few drops of bromothymol blue indicator in the 21 dip with the unknown A solution.
rd
3
dip with the unknown A solution.
4. Place a small piece of red litmus paper in the
5. Place a small piece of blue litmus paper in the last dip with the unknown A solution.
6. Record all observations in your data table.
7. Repeat steps 1 to 6 using unknown solutions B through F.
8. Rinse off all glassware used, return all materials to their proper locations, and wipe down your lab area. All waste
solutions may go down the sink with plenty of fresh water. Any spent litmus paper must be placed in the garbage.
l3
pH SCALE
oven
baking
soda
arr,rnoriio
soap
bleach
•r4
cleaner
L_—
[OH-]
4
2
S
B
B
Neutral
AotdiC
12
11
10
14
Baste
Methyl Orange
Methyl Red
Bromtliymol Blue
Litmus
Phenolphllielain
Indigo Carmine
Observations:
Part 1: Table 1
-
Behavior ofAcids and Bases in Various Indicators
Colour
In a base
n an acid
Phenolphthallein
Bromothymol
Red
blue
litmus
Blue
Litmus
Part
2: Table 2
—
Behavior of Unknown Solutions in Various Indicators
Chemical Indicators
Unknown
Fhenolphthalein
Solution
Bromothymoll
Blue
Red
Blue Litmus
Litmus
A
B
C
D
E
F
Questions
1. What
does an acid do to phenolphthalein, bromothymol blue, blue litmus, and red litmus?
2. What
does a base do to phenolphthalein, bromothymol blue, blue litmus, and red litmus?
3. If there
is no change in
how
both
litmus indicators, what conclusion
and
4.
Explain
5.
Other than using indicators to differentiate between acids
you decided which solutions were acids
can
you draw?
which were bases.
and bases,
what other ways can you
find out which solutions are acids and which are bases?
Conclusion
Which of the unknown solutions you tested were acids and which were bases?
j
Name
Use with textbook pages 234-239.
ecogrzing ocid, bas, crnd oIt
t State whether each of the following is an acid, a base, or a salt.
(a) HI
(I) 4
(S0
2
A1
3
)
(b) HBr
(rn) GHCOOH
*
(c) KQH
2
Mg(
C
(n) 3
OO
CH
)
(d) HNO
3
(a) calcium nitrate
(e) NaOH
(p) sodium chloride
(f) H
4
S
2
0
(q) hydrocyanic acid
3
C
2
(g) H
0
(r) hydrogen fluoride
(h) H
4
P
3
0
(s) barium hydroxide
i) NaPO
4
hypochlorous acid
(j) Sr(OH
2)
(k) 05(01-1)2
——____________
_
(u) aluminum hydroxide
__,
(v) magnesium carbonate
2. What acid is present in vinegar?.
See Text
p.225-2
29
3. What is the chemical name for table salt?
—__________________
____
4. What acid is used in automobile batteries?
5. What base is found in drain and oven cleaners?
6. What base is the active ingredient in some antacids?
7. What add Is produced in the stomach to help digest food?
I
i
intsb
Name
Use dth textbook pages 2W23
octor
AcId-base nutroWzofion
acid
base
+
—‘
water
+ salt
I. Complete and balance the following neutralization reactions.
(a)
S0 +
2
H
4
NaOH
(b)HNOa+KOH
HCI
+
(o)
2
Ca(OH)
-*
2 +
(d) 4
P0 ÷ Ba(OH)
3
H
+
NaOH
00H
0
(O>CHa
(f)
(g)
(h)
HNO + Sr(QH)
2 -*
HF
÷
HSr ÷
3
Fe(OH)
+
4
Sn(OH)
2. Complete and balance the following acid-base neutralization reactions. Include both the word
equation and the formula. See (a) for an example.
(a) sulphuric acid + potassium hydroxide
S0
2
H
4
+
->
2 KOH
(b) acetic acid + barium hydroxide
-*
nitric acid + lithium hydroxide
-—
-
(e) sulphuric acid + calcium hydroxide
(f)
S0
2
K
4
-
(c) phosphoric acid + aluminum hydroxide
(d)
potassium sulphate + water
-
hydrochloric acid + magnesium hydroxide -
+
2 H
0
2
Aayzh
Name
[
Us with textbook pages 237.
Metal oxe and nonm4oI oxides
1. What element reacts with a metal or a non-metal to form an oxide?
2. What Is a chemical compound that contains a metal chemically combined with
oxygen?
3 What Is a chemical compound that contains a non-metal chemically combined with
oxygen?
4. What happens to a solution when a metal oxide dissolves In water?
5. What happens to a solution when a non-metal oxide dissolves In water?
6. What is formed when a metal oxide reacts with water?
7. What is formed when a non-metal oxide reacts with water?
8. Classify each of the following as a metal oxide or a non-metal oxide.
(a Na
0
2
(e) SO
2
-
(b) 8203
(f BeO
2
(c)N0
(g)C10
(d) GaO
(h) U
0
2
9. Indicate whether an acid or a base will be produced.
(a)MgO+H
0
2
(b)
503
(c)CaO
+
+
H
0
2
-÷
2 ÷ H
(d)C0
0
2
0
CD
z
U,
Name
Oats
Ccn
use with textboi.k pages 244-248
ecognizin orgonic on inorcniic comzound
Classify each of the following compounds as organic or inorganic by examining their
formulas.
i6.CHOK
1.CO.....
3
17. NaHCO
2. Cl-I
4
3. HCI
-._________________________
18. CH
6
O
12
3
4 NH
CO
2
i9.Na
5. CO
2
20. 2
0).
K
0
r
6. CrS
21. Ca(OH)
2
7, C
4
H
2
22. Co(N0
2
)
3
10
H
4
8.C
2
HO
19
23.C
9.C
1
H
5
4
OH
4
24.NH
10. C
1
H
8
26. 3
OCH
CH
11. Cu
0
2
26. 3
18
C
N
2
H
O
3
0
2
12. Cr
27. CH
COOH
3
13. CHCI
3
NHCH
CH
28. 3
14. CaCO
3
29. 2
CH
3
CH
O
15. C
0
8
H
2
30. 2
CHOCH
3
CH
C
H
Det&
oro
(
Use with textbook pages 244-248.
Oc
comou
cjnii cour
Classify each of the following compounds as organic or inorganic by examining the
structural formula, ball-and-stick model, or space-filling model.
Structural fomiul, ball-aud-stick TI,pe o conioid
model, or space4flhin model
Wraelc er
(
jOi
5;.i
g. What happens to the number of W after
S0 is added to water?
2
H
4
Use with textbook pages 220-229.
A. it increases
B. it decreases
tch the Term on the left wIth the best
be
Descflptor On t)e tI(ht E ChDeSCdpt04
used only once.
C. it stays the same
iO Which of the following is a base?
4cid
base
1.
2.
4.
pH scale
5, __corrosWe
pHindicator
6
of
7.
hydrogen
A.asolutionwithapH
of 7
B. can burn skin or eyes
on contact
C, number of hydrogen
ions in a specific
volume of solution
D. a chemical compound
that produces a solu
Hon with a pH less
than 7
E. a number scale for
measuring how acidic
or basic a solution is
. a chemical compound
that produces a
soluhon with a pH
greater than 7
0. a chemical that
changes colour
depending on the pH
of the solution it is
placed in
*
a
hasapHoflessthan7
II,
can conduct electndty
HI.
produce hydroxide ions when
dissolved In solution
C. LiON
8. HBr
D. HNO
3
Ii. What is the name for HC10
?
3
A. chtoric acid
*
a
a
*
*
B. chiorous acid
C perchloric acid
0. hypochlorous acid
12. What is the chemical formula for
suipharous acid?
C. 3
S0
2
H
0. 4
S0
2
H
A. HS
B. HSO
4
a
a
4
13. What is the pH of a substance that causes
methyl orange to turn yellow and methyl
red to turn red?
A.3
C.6.5
8.4.5
0.8
14. Which of the following would occur if eggs
were tested with vazious pH indicators?
8. Which of the following desczibes acids?
I.
A. lcd
a
*
I.
indigo carmine turns blue
IL
phenoiphthaiein turns pink
I_____
bromothyrnol blue turns blue
A.Iandionly
A. I and 11 only
B.Iandfflonly
B. I and Ill only
C. 11 and [II only
C.llandfflorily
0. L Ii. and III
D.I,ll,andffl
D.NaO
LHtO
3
F. NH,O+f
B, I, II. and Ill
A.? and II only
10an
C. HCO
B. HCO
LI
6.2
4
S
2
11
0
+
eqaasion?
0.4
C.3
NaOH
Na
S
2
O
+
I3O
5
BaCO
+
2 1IO
-
1
fri-z1
lsrJ
.
l.
A. CO
B. Co,
10. Vlsa5 coefficient is needed for sodium
hydawido in ordet to balance the following
-*
13. Which of the following statements is true?
3 ÷ Ba(OI1)
HCO
2
Use the following acid4sase
neutralizatIon reaction to answer
question U.
0. HPO, and Fe(OH),
B. 5
11 and Fe(Oii)
P
C. l4O and Fe(OH),
A. PO and 5
Fe
0
,
12. Which reactants form the salt PePO, in a
neutrali ration reaction?
B. land 111 only
C. TI and ill only
9. Carbon diratide forms which of the
following in water?
B. acidic
C. neutral
A. basic
the solution becomes
8. ‘A’hen non-metal osides dissolve in water,
C. francium
B. magnesium
A. copper
B. sodium
reactive?
7. Which of the following metals in most
4._anacid
5._ar
odde
6._a rrOetal
2
LNO
C.Mgfl
A.Hp
1._..walr
2._amS
3. ..__alase
.
C. KCIO,
B. KCIO,
A. llO
B, Kf1
he used only once.
for the salt produced by this ueusnslizatlon’l
Match the Term on the left with tile best Chemlal
Formula on the right Each Chemical Formula may
11. Hydrochloric acid can be used to neutralise
potassium hydroxide. Whst is the formula
Salts
Use with testboa* pages 234-239.
(
on tile left with the best Formula! Model that
H
a
H
a
6. Which formula represents a hydrocarbon?
A. HClO
B. CH
COOH
5
C. CH
CH.CHCOOH
5
0. cHcapidll
cn
2
A. crhon
B. oxygen
C. chlorine
0. hydrogen
organic compound?
-_-_:9,_j
,
8.
5. What element mutt always be present in an
1.__slwcturat
fonoda
2._molecular
iotmth
3.__space-tth
rsodet
4.
bat-and-airs
represents athena on the tiGhi tacit Formula I
?odeI may be used oSty Once,
Using tile compound athena. match the Descriptor
Orçjonlc compounds
Use with teObaok pages 244-248.
Nat-n
—
a
H
H
Br
H
Llsadliossly
B. land Ill only
C. 11 and Ill only
0.1,11, and III
_
L_j-
:*
H—t—o—H
8. Which of the following represents methane,
Cli,?
SHaH
H—C—C—C—C—OH
W
H—c—c—C—H
H
act
H—C—C—H
H,
r
D
C.
B.
A.
7. Which of the following represents an
alcohol?
jAeso
Ch.5 Review Checking Concepts. P.252-253#1,2,5,6,9,11-13,15-18,19(a,c,e),21,22,23 (Comp. Sent)
Ch.5 Review Checking Concepts. P.252-253#1,2,5,6,9,11-13,15-18,19(a,c,e),21,22,23 (Cont)