Daily
Lesson
Plan
I. OBJECTIVES
A. Content Standards
B. Performance Standards
C. Learning Competencies/
Objectives/MELC/S
II. TOPIC
School
PAOAY NATIONAL HIGH SCHOOL
Grade Level
12
Pre-service Teacher
Teaching Dates & Time
Freesia Mae P. Espiritu
February 28- March 02, 2023
Learning Area General Chemistry 2
Quarter
Second
Semester
First
The learners demonstrate understanding of properties of solutions, solubility, and the stoichiometry of reactions in solution.
The learners should be able to design a simple investigation to determine the effect on boiling point or freezing point when a solid is dissolved in
water.
At the end of the discussion, 90% of the students should be able to use different ways of expressing concentration of solutions: percent by
mass, mole fraction, molarity, molality, percent by volume, percent by mass, and ppm STEM_GC11PPIIId-f-111.
Ways of Expressing Concentration of Solutions
III. LEARNING RESOURCES
A. References
1. Teacher’s Guide Pages
2. Learner’s Material Pages
General Chemistry 2 – Quarter 1 Learning Activity Sheet, p. 46-66
General Chemistry 2 – Quarter 3 – Module 2 Physical Properties of Solution, p. 2-9
3. Textbook Pages
4. Additional Materials
from Learning Resources
B. Other Learning Resources
IV. PROCEDURES
A. Reviewing previous lesson
or presenting the new
lesson
Teacher’s Activity
May I request Ms. April to please come in front and lead our prayer
today.
Learner’s Activity
April: Yes, ma’am.
Go on, dear.
April: Dear Lord and Father of all, Thank you for today. Thank you for
ways in which you provide for us all. For your protection and love, we
thank you. Help us to focus our hearts and minds now on what we are
about to learn. Inspire us by your Holy Spirit as we listen and write. Guide
us by your eternal light as we discover more about the world around us.
We ask all this in the name of Jesus. Amen.
Amen.
All: Amen
Good morning, Grade 12- Copernicus.
All: Good morning, ma’am!
Before we proceed, may I first check your attendance?
All: Yes, ma’am.
As I call on your name, kindly raise your right hand for me to see if
you are present.
All: Yes, ma’am.
(Calls on the name of the students one-by-one.)
(Students raises their hands as they hear on their names.)
Everybody is present.
Anyway, how are you dear students?
All: We are fine, just like you are ma’am.
Is that so? Okay!
So, our new topic for today is about the concentration of solutions
but, before we start our discussion, may we first try the activity in
locating the words that are associated with it.
We are going to do a word search activity. And 10 words are hidden
here. As I call on your names, stand and give one word that you can
see which is connected to our new topic. Is that clear?
All: Yes, ma’am.
(Calls on name one-by-one in giving answers)
Random students: (Responding actively)
Very good!
Answer key:
 Percent by Mass
 Percent by Volume
B. Establishing a purpose for
the lesson
C. Presenting examples/
instances of the new lesson
 Molality
 Molarity
 Mole Fraction
 PPM
 Solute
 Solvent
 Solution
 Concentration
In the previous lessons, you have discovered the phase changes in
terms of the accompanying changes in energy and forces between
particles.
Many chemical reactions take place between ions and molecules
dissolved in water or other solvents, rather than between pure
solids, liquids, or gases. Previously, you have learned the properties
of gases, liquids, and solids. In this lesson, we will examine the
properties of solutions, concentrating mainly on the role of
intermolecular forces in solubility and other physical properties of
solution.
Quantitative study of a solution requires knowing its concentration,
that is, the amount of solute present in a given amount of solution.
Several different concentration units are used by chemists, each of
which has strengths as well as drawbacks. Let us examine the units
of concentration: percent by mass, mole fraction, molarity, molality,
percent by volume, and parts per million (ppm).
Many people have a qualitative idea of what is meant
by concentration. Anyone who has made instant coffee or
lemonade knows that too much powder gives a strongly flavored,
highly concentrated drink, whereas too little results in a dilute
solution that may be hard to distinguish from water. In chemistry,
the concentration of a solution is the quantity of a solute that is
contained in a particular quantity of solvent or solution. Knowing
the concentration of solutes is important in controlling the
stoichiometry of reactants for solution reactions. Chemists use
many different methods to define concentrations such as percent
by mass, mole fraction, molarity, molality, percent by volume, and
parts per million.
All: (Intently listening)
All: (Intently listening)
D. Discussing new concepts
and practicing new skill #1
What is a solution? How can we define solution?
Ms. Nicole can you read the definition of solution, please?
Nicole: Yes, ma’am.
A solution is a mixture of two or more substances that is identical
throughout.
In other words, a solution is a mixture of one or more solutes
dissolved in a solvent.
A solution is a mixture of solute and solvent where in, the solvent is
the large part of it whereas the solute is the small part.
All: (Intently listening)
Next, concentration. A concentration is referred to the amount of
solute dissolved in a solvent at a given temperature.
A solution is said to be dilute if it has a low concentration of solute
dissolved. And a solution is described as concentrated when it has
a high concentration of solute dissolved.
So, a solution can be unsaturated, saturated, and supersaturated.
What do we mean by when we say unsaturated?
Can you read it, Mr. Powelle?
Okay, when a solution has a lesser amount of solute being absorb in
a solvent, its concentration results to being unsaturated.
Whereas, in saturated solution, it has the maximum concentration
of solute dissolved.
And a supersaturated solution contains more dissolved solute than
normally possible. It usually requires an increase in temperature
followed by cooling.
Powelle: Unsaturated solution has a less than the maximum
concentration of solute dissolved.
E. Discussing new concepts
and practicing new skill #2
We already know that there are 6 different ways in expressing
concentration of solutions as I’ve said a while back. These are the,
what?
Now, we are ready to discuss them one by one.
Let’s start first with the Percent by Mass. The percent by mass, also
called percent by weight or weight percent, is the ratio of the mass
of a solute to the mass of the solution, multiplied by 100 percent.
Equation:
% 𝑏𝑦 𝑚𝑎𝑠𝑠 =
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
× 100
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
The percent by mass is a unitless number because it is a ratio of two
similar quantities.
(Insert, example problems to be solved on percent by mass
concentration.)
Next, the Mole Fraction in which, it is a way of describing solution
composition. It is the ratio of the number of moles of one
component of a mixture to the total number of moles of all
components.
The mole fraction is also unitless because it has a ratio of two similar
quantities.
Equation:
Mole Fraction for Component A:
𝑚𝑜𝑙 𝐴
𝑋𝐴 = 𝑚𝑜𝑙 𝐴 +𝑚𝑜𝑙 𝐵
Mole Fraction for Component B:
𝑚𝑜𝑙 𝐵
𝑋𝐵 = 𝑚𝑜𝑙 𝐴 +𝑚𝑜𝑙 𝐵
All: Percent by mass, Mole fraction, Molarity, Molality, Percent by
volume, and Parts per million or ppm.
In general, the mole fraction of component “i” in a mixture is given
by:
𝑛
𝑋𝑖 = 𝑖
𝑛𝑇
(Insert, example problems to be solved regarding mole fraction.)
We also have the Molarity, also known as molar concentration. It is
defined as the number of moles of solute per liter of solution.
The SI unit for molarity is mol/m3, however, you will almost always
encounter molarity with the units of mol/L.
It is important to keep in mind that molarity refers only to the
amount of solute originally dissolved in water and does not take into
account any subsequent processes, such as the dissociation of a salt
or the ionization of an acid.
We can express this as either equation or algebraically:
Equation:
𝑀𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝑀 = 𝐿𝑖𝑡𝑒𝑟 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
Algebraically:
𝑛
𝑀=𝑣
(Insert, example problems to be solved regarding on molarity.)
We also have the Molality, where in, the number of moles of solute
dissolved in 1 kg (1000 g) of solvent. And unlike molarity, which
depends on the volume of the solution, molality depends only on
the mass of the solvent.
The SI unit for molality is mol/kg. A solution with a molality of 3
mol/kg is often described as “3 molal” or “3 m.” However, following
the SI system of units, mol/kg or a related SI unit is now preferred.
Equation:
𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝑚 = 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
(Insert, example problems to be solved with regards to molality.)
Next, we have the Percent by Volume as well. It is related to the
molar concentration but the difference is that the volume percent
is expressed with a denominator of 100.
It is used for reporting concentration of liquids solutes in solution.
It is also called %V/V and it is always expressed as percentage (%)
and the units of the volume should be in mL.
Equation:
𝑃𝑒𝑟𝑐𝑒𝑛𝑡 𝑉𝑜𝑙𝑢𝑚𝑒 =
𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 +𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
× 100%
(Insert, example problems to be solved regarding percent by
volume.)
And last, the Parts per Million. It is a term used in chemistry to
denote a very, very low concentration of a solution. So, when the
amount of solute is very small, as with trace impurities in water,
concentration is often expressed in parts per million.
The SI unit of parts per million is either gram (g), mg/L, or ppm itself.
Equation:
𝑃𝑎𝑟𝑡𝑠 𝑝𝑒𝑟 𝑀𝑖𝑙𝑙𝑖𝑜𝑛 =
𝐺𝑟𝑎𝑚 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 =
𝐺𝑟𝑎𝑚 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝐺𝑟𝑎𝑚 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
× 106
(𝑝𝑝𝑚)(𝑔𝑟𝑎𝑚 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛)
1000000
(Insert, example problems to be solved with regards to parts per million.)
F. Developing Mastery
Complete the table by giving the equation and the units of
concentration mentioned.
All: Yes, ma’am.
Units of
Concentration
1. Percent by Mass
2. Molarity
3. Mole Fraction
4. Molality
5. Percent by
Volume
6. Parts per Million
G. Finding practical
applications of concepts &
skills in daily living
Equation
Unit
For you to relate or connect our topic today in your reality, I’ll pick
four students to give at least two examples of each topic listed
below that we usually use in our everyday lives.
A. Solute
B. Solvent
C. Solution
D. Concentration
H. Making generalizations &
abstractions about the
lesson
(Chooses students randomly to answer the following.)
To summarize what we have learned today, may I call on Ms.
Krizette to kindly complete the Metacognition of Knowing What
phrases.
(Random students giving responses/answers.)
I know that, I know something about the concentrations of solution.
Before, I know that concentration of solution is the measurement of
mixtures to form a solution.
Now, I learned that concentration of solution has six ways to be
expressed.
Likewise, I know that these ways are percent by mass, mole fraction,
molarity, molality, percent by volume, and parts per million.
Finally, I know that the ways to express concentration of solution
has/requires different SI units.
Now, you know that I have learned a lot about the concentration of
solution.
I. Evaluating Learning
That’s all for today. Thank you for your cooperation.
Now, for me to assess what you have learned in this topic. May I
asked everyone to kindly bring out a clean sheet of paper and
answer the given problems.
Answer the following problems. Write your full solution on your
answer sheet and box the final answer.
1. Hydrogen peroxide, H2O2, is used by some water treatment
systems to remove the disagreeable odor of sulfides in drinking
water. An aqueous solution of H2O2 prepared in the laboratory was
found to have a concentration of H2O2 of 20.0% by mass. What is
the mole fraction?
2. What is the molality of a solution containing 0.75 moles of
sodium hydroxide in 500 mL of water at 25℃? The density of water
at 25℃ is 1 g/mL. (Hint: d=m/v)
J. Additional activities for
application or remediation
3. A sample of 0.938 g of sodium hydroxide (NaOH) is dissolved in
60.9 g of water. What is the percent by mass of NaOH in the
solution?
CONCEPTUAL ANALYSIS
Directions: Base on what you have learned from this lesson and
from other previous lessons. Analyze the given statement and
scientifically discuss your claim.
“A solution is prepared at 200C and its concentration is expressed in
two different units; Molarity and Molality. The solution is then
heated to 880C. Which of the concentration units will change?”
V. REMARKS
VI. REFLECTION
A. No. of learners who
earned 80% in the
evaluation
B. No. of learners who
require additional activities
for remediation who scored
below 80%
C. Did the remedial lesson
work? No. of learners who
caught up with the lesson
D. No. of learners who
continue to require
remediation
E. Which of my teaching
strategies worked well? Why
did these work?
F. What difficulties did I
encounter which my
principal or supervisor can
help me solve?
G. What innovation or
localized materials did I
use/discover which I wish to
share with other teachers?
Prepared by:
FREESIA MAE P. ESPIRITU
Student Teacher
Checked by:
Approved by:
MYLINE E. PASION
Teacher III
Cooperating Teacher
DANIEL D. TABILI
School Principal II