1. SPG
K A P I T M U
STRIKTONG PAKIKINIG SA GURO
Ang Kinakailangan
2. Diversity of Materials in
the Environment
Imagination is more important than knowledge. Knowledge
is limited. Imagination encircles the world.”
-Albert Einstein
19. In Grade 6, you have learned about
different mixtures and their characteristics.
different mixtures and their
characteristics.
mixing a solid and a liquid or combined two
different liquids.
homogeneous or heterogeneous mixtures
23. You observed in Activity 1 that
a solution is not always a liquid;
it can be solid, liquid, or gas. In
addition, solutions may either be
found in nature or are
manufactured.
24. • Solutions are homogeneous
mixtures made up of
molecules or ions.
• Composed of solute and solvent.
• A solution does not always
have to be liquid, it can be
solid or gaseous.
25. What are the Properties of Solutions?
In Activity 2, you found out that a solution is
formed when a solute dissolves in a solvent to
form a single phase that appears uniform
throughout. A solution is clear. In a solution, the
particles are too small that they cannot be seen by
the unaided eye. The particles in solution are
smaller than the pores of the filter paper or the
cheesecloth and so these can pass through the
filter.
28. Type
(Phase)
Solute Solvent Example
Liquid solid liquid seawater,
brine
Solid gas solid charcoal filter
liquid solid dental
amalgam
(Hg and other
metal except Fe)
Types of
Solution
41. NATURALLY OCCURRING
SOLUTIONS
Examples of solutions that occur
naturally are natural bodies of
water like the seas and ocean,
blood plasma, air, and some
mineral ores.
42. MANUFACTURED/PROCESSED
SOLUTIONS
Almost every household uses vinegar
for cooking and cleaning purposes.
Vinegar usually contains about 5% acetic
acid in water. Some vinegar are clear
homogeneous mixtures (solutions). Other
kinds of vinegar are colloidal.
43. ACTIVITY 3
What is the Evidence that a Solution is
Saturated?
In Activity 3, you will find out how much solute
can dissolve in a given amount of solvent and find
out the type of solution based on whether there
is excess solute or not.
At higher grade levels, you will learn more of the
detailed processes that happen when a solute
dissolves in a solvent.
44. In Activity 3, you have observed that there is a maximum
amount of solute that can dissolve in a given amount of
solvent at a certain temperature. This is what is called the
“solubility”
of the solute. From your everyday experience,
you also observe that there is a limit to the
amount of sugar you can dissolve in a given
amount of water.
45. The solubility of some solutes decreases as
temperature increases.
On the other hand, there are solutes that
increase their solubility at higher
temperatures. For some other solutes, their
solubility is not affected by an increase in
temperature. Since the effect of
temperature on different solutes is more
accurately explained using solubility curves,
47. SATURATION
My brain really
hurts! I can’t take
it anymore… Stress
week! huhuhu
Saturated
Unsaturated
Supersaturated
During the addition of solid solute
into a liquid solvent, a condition is
reached where no more solute
dissolves.
The excess solid simply lies
undissolved at the bottom.
55. TYPES OF
SOLUTIONS
At 25oC, a saturated solution of table salt has only 36.0 g
(3 tablespoons) dissolved in 100 mL of water. Any
additional table salt will no longer dissolve.
58. YOU CAN EXPRESS
CONCENTRATION IN OTHER
WAYS SUCH AS:
(1)percent by volume, which is the amount
of solute in a given volume of solution
expressed as grams solute per 100 milliliter
of solution (g/100 mL), and
(2)percent by mass, which is the amount of
solute in a given mass of solvent expressed
as grams solute per 100 grams of solution.
59. OFTEN SHOW THE
CONCENTRATIONS OF SOLUTES
EXPRESSED AS PERCENT (%) BY
VOLUME OR MASS.
The alcohol used as a
disinfectant is a
solution of 70% ethyl
or isopropyl alcohol,
meaning 70 mL
alcohol.
61. THE CONCENTRATION OF SOLID
SOLUTIONS, LIKE GOLD
JEWELRY, IS EXPRESSED AS
KARAT.
PURE GOLD IS REFERRED TO AS
24 KARATS.
62. SAMPLE PROBLEM 1
HOW MANY ML OF ETHYL ALCOHOL ARE
PRESENT IN A 50 ML BOTTLE OF
RUBBING ALCOHOL?
50 mL Rubbing Alcohol 𝑥
70 mL ethyl alcohol
100 mL rubbing alcohol
= 35 mL
ethyl alcohol
63. SAMPLE
PROBLEM 2
100 g coin
75 g copper
𝑥 5.4 g coin = 4.0 g copper
A one peso coin has a mass of 5.5 grams.
How many grams of copper are in a one
peso coin containing 75% copper by
mass?
So, a 5.4 grams one peso coin contains,
65. Factors Affecting How Fast a
Solid Solute Dissolves
Stirring or Agitation
Particle Size
Increase in temperature
Concentration of solution
Pressure on Gas
Like dissolves like
68. Agitation makes the solute
dissolves more rapidly because
it brings fresh solvent into
contact with the surface of the
solute. However, agitation
affects only the rate at which
a solute dissolves.
69. It cannot influence the
amount of solute that
dissolves. An insoluble
substance will remain
undissolved no matter
how much the system
is agitated.
70. Also, particle size does not
affect solubility. It can
affect the RATE at which
something dissolves, but it
will not change the total
amount of material that
can ultimately dissolve
(solubility).
72. Particle Size
The size does not
that matters on the
rate of solubility,
but the area of
contact.
73. We see that the dissolving
of an object happens
because there are
collisions between the
solvent and the solute.
When the solute is BIG, for
example a block, the
solvent can only collide
with the surface of the
block, but not the middle
of the block. that means it
will take a longer time for
the solvent to dissolve the
solute.
74. When the block is
pondered into a
powdery state, it is
easier for the solvent
to dissolve the solute
because of the larger
area of collisions.
76. Temperature
The solubility of
a gas in a liquid
decrease with a
temperature. In
fact, the
solubility of a
gas in water is
usually zero at
its boiling point.
77. The solubility of
solids and liquids is
closely related to
the heat of
solution.
The heat of
solution is the heat
evolved with to
the surroundings,
the process is
exothermal and
exothermic
78. If heat is absorbed
from the
surroundings, the
process is
endothermal or
endothermic and
the heat of solution
is a positive
quantity.
79. CONCENTRATION OF SOLUTION
We have already discussed concentration of
solution.
#1 #2 #3 #4
What do you remember?
80. Pressure
Liquids and solids exhibit
practically no change of
solubility with changes in
pressure. Gases as might
be expected, increase in
solubility with an increase
in pressure.
81. Henry's Law states
that: The solubility of
a gas in a liquid is
directly proportional to
the pressure of that
gas above the surface
of the solution.
82. Gas Molecules
EFFECT OF PRESSURE TO
SOLUBILITY OF GAS
PRESSURE:
Dissolved gas
molecules
Gas at L
Ho
ig
w
hP
Pr
re
es
ss
su
ur
re
e
When the gas is compressed,
G
g
a
a
s
sm
m
o
o
l
l
e
e
c
c
u
u
l
l
e
e
s
secnatnerthe
e
l
i
n
q
t
u
e
i
d
rt
m
h
o
e
r
l
e
iqf
u
rie
dq
uae
nn
dt
l
y
,
so b
m
e
o
c
ro
em
ae
rs
e dissolved.
84. If the pressure is
increased, the gas
molecules are "forced"
into the solution since
this will best relieve
the pressure that has
Carbonated beverages
provide the best example been applied.
of this phenomena.
87. WHAT HAVE YOU
LEARNED?
Now that you have completed the activities in this module, you have
learned the properties of a solution, the ways of reporting its
concentration, as well as the effects of stirring, particle size,
temperature, and type of solute on how fast a solid dissolves in water.
While learning about solutions, you also had the chance to gather
information and gain new knowledge through the process of
conducting science investigations. You also learned the importance of
identifying the variables that had to be controlled in order to make a
good plan for measuring and testing the variables you are concerned
about.
What you have started doing in these investigations is what scientists
usually do when they seek answers to a scientific question or problem.
In the next modules, you will be challenged to ask more questions
about materials around you. You will try to explain answers to your
hypothesis
(your suggested explanation) after you have done your investigation.
88. SUMMAR
Y:
SOLUTION is a system in which one or more substances are
homogenous mixed.
A solution has two (2) components: SOLUTE AND SOLVENT.
SOLUBILITY is the maximum amount of solute that dissolves in a
given amount of solvent at a specified temperature.
The 6 factors that affect solubility are: (a) Stirring or Agitation (b)
Particle Size (c) Increase in temperature, (d) Concentration of
solution (e) Pressure on Gas (f) Like dissolves like.
The concentration of solution expresses the amount of solute
dissolved in a given quantity of solvent: Concentration can be
expressed in different ways:
As dilute or concentrated
As saturated, unsaturated, and supersaturated
Percent by weight, percent by volume, or percent by weight/volume.
128. Direction: Fill in the blanks with letters to
complete the sentence.
1. The S_ _ _T_ is the component of the
mixture that gets dissolved.
2. A solution is a kind of _ _ X _ _ R E.
3. A solution is a H_ _ O _ _ N _ _ _S
mixture.
4. The S _ L _ _ _ T is the component of the
solution that does the dissolving.
5. The universal solvent is _ _ _ _ R.
129. 6. S _ _ _ B _ _ _ _ Y refers to the amount of
solute that can dissolve in a certain volume or
mass of solvent, at a certain temperature.
7. Solubility is a P _ _ _ _ C _ _ property.
8. Sugar candy is an example of a _ U _ _ R _
_ _ _ R _ _ _ D solution.
9. 5 grams of sugar dissolve in 1 L of water is
called a D _ _ _ T _ solution.
10. A substance is I _ S _ _ _ _ L _ if it is
incapable of dissolving.
130. 1. Which of the following refers to the
solution that contains the maximum
amount of solute dissolved by a given
amount of solvent?
A. Solubility
B. Saturated solutions
C. Unsaturated solutions
D. Supersaturated solutions
131. 2. Which of the following refers to the
solution that contains less amount of
solute than can dissolve by a given
amount solvent?
A. Solubility
B. Saturated solutions
C. Unsaturated solutions
D. Supersaturated solutions
132. 3. What is the solution that
contains more solute than a
saturated solution under
the same conditions?
A. Solubility
B. Saturated solutions
C. Unsaturated solutions
D. Supersaturated solutions
133. 4. In a salt water solution, what
substance is considered the
solvent?
A. Salt
B. Both are solvents
C. Water
D. Neither substance is a solvent
134. 5. Why is a solution considered a
homogeneous mixture?
A. It is usually liquid.
B. It can be dilute or concentrated.
C. It contains a solute and solvent.
D. Its component are distributed
evenly.
135. IDENTIFICATION:
1. A substance which gets dissolved.
2. A substance that dissolves solute.
3. It describes whether a certain solute can
be dissolved in a specific solvent.
4. It is composed of two or more substances
physically combined together which are
well-mixed.
5.It is said to be the universal solvent.
140. QUALITATIVEL
Y
•Using words such
as ‘dilute’ or
‘concentrated’
•By simply
observing their
appearance.
QUANTITATIVELY
•Using numbers.
•By comparing
the number of
drops per
volume of
water.
151. YOU CAN EXPRESS CONCENTRATION
IN OTHER WAYS SUCH AS:
1. Percent by Volume- is
defined as the volume of
solute present in 100 mL of
solution (% v/v)
152. 1. Percent by Volume-
which is the amount of
solute in a given volume of
solution expressed as grams
solute per 100 milliliter of
solution (g/100mL)
153.
154. SAMPLE PROBLEM 1:
A CONTAINS 50 ML OF
ETHANOL IN 300 ML
ALCOHOL OF SOLUTION.
WHAT IS THE PERCENT BY
VOLUME CONCENTRATION
OF THE SOLUTION?
157. TAKE NOTE!
The volumes of the solute,
solvent, and solution must
be expressed in the same
units.
158. SAMPLE # 2
•The active ingredient in wines and
other alcoholic beverages is ethanol.
A 300mL sample of wine was found
to contain 37.5mL of ethanol. What
is the percentage by volume
concentration of ethanol in the wine
sample?
161. LET’S TRY THIS
Problem #1: What is the
percent by volume of a
solution formed by mixing
25mL of isopropanol with
45mL water?
162. Problem #2: A photographic
“stop bath” contains 160mL
of pure acetic acid, HC2H3O2(l)
in 650mL solution. What is
the v/v concentration of
acetic acid in the stop bath?
163. PROBLEM # 1
•Given:
Volume of solute (isopropanol)=
25mL
Volume of solvent (water)= 45 mL
Asked: % volume
167. LET’S ANSWER THIS!
•1. If I make a solution by adding
water to 75mL of ethanol until
the total volume of the solution is
375mL, what is the percent by
volume of ethanol in the solution?
168. 2. Rubbing alcohol is sold
as a 70% (v/v) solution of
isopropyl alcohol in water.
What volume of isopropyl
alcohol is used to make
500mL of rubbing alcohol?
169. 3. A bottle of hydrogen
peroxide also known as agua
oxigenada is labeled 3%
(v/v). How many mL of agua
oxigenada are in a 400mL
bottle of this solution?
170. When we express the
concentration of a solution
as the percent one
component in the solution,
we call it the mass
percentage (w/w).
171. 2. Percent by mass – it is
defined as the amount of
solute in each mass of
solvents. It is expressed as
grams of solute per 100
grams of solution (% m/m).
172.
173. Example 2:
What is the percent by
mass concentration of a
solution that contains
5.30 g of salt dissolved in
19.7 g of water?
174.
175.
176. Sample Problem 2:
What is the percent by
mass of a salt solution
by dissolving 11 g of
salt in 80 g of
solutions?
177.
178.
179. Labels of products sold often show
the concentration of solute
expressed as percent (%) by volume
or mass. The alcohol used as a
disinfectant is a solution of 70%
ethyl or isopropyl alcohol, meaning
70mL alcohol. There are also
solutions sold as 40% ethyl or
isopropyl alcohol.
180. Vinegar is often labeled
as “5% acidity”, which
means that it contains 5
grams of acetic acid in
100 g of vinegar.
