Chemistry Pre-Lab

CHEMISTRY 1
DK014

DK014
Pre-Lab Module

EXPERIMENT 1
DETERMINATION OF THE DENSITY OF WATER

Course Learning Outcome:

Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:

At the end of this lesson, students should be able to :
1. chose the correct apparatus to determine the density of water
2. calculate the density of water
3. compare the accuracy of the density of water using different apparatus

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. Define density.

2. Give one example of the unit of density.

3. What is the density of water at 25oC.

Procedure
1. List down the apparatus in laboratory that possible to be used to measure volume of

water.

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2. Suggest the procedure to determine the density of water by using different apparatus to
measure a volume of water in laboratory

Experiment 1 : Data Analysis

1. A group of students carried out an experiment how to determine the density of 10 mL
water using different apparatus and the data is shown in the table below. Calculate the
density of water.

Data Burette Pipette Measuring
cylinder
Mass of empty beaker / g 21.4125 21.3455 21.3831
Mass of beaker + water / g 31.2535 31.3377
Mass of water transferred / g 31.0141
Density of water / g mL-1

2. Compare the accuracy of apparatus to measure the volume by using the density of
water value.

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EXPERIMENT 2
STANDARD SOLUTION AND DETERMINING
OF THE CONCENTRATION OF ACID SOLUTION.

Course Learning Outcome:

Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. define molarity and standard solution
2. state the use of standard solution
3. describe the preparation of a standard solution of sodium carbonate, Na2CO3.
4. calculate the concentration of HCl solution in an acid-base titration

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. Define molarity.

2. What is a standard solution and give the use of a standard solution

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Procedure
1. What is the possible error that might be occur during preparation of a standard solution
by using volumetric flask and State the precaution step to avoid the error mentioned .

2. What is the decimal places for burette reading. If the burette is fully filled, what is the
initial reading?

3. State three precautions that must be taken during titration to ensure the accuracy of
the results.

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Experiment 2 : Data Analysis

1. The data for a titration of HCl solution with KOH solution are as follows:

Volume of HCl used 25.0mL
Initial burette reading 0.50mL
Final burette reading
Concentration of KOH 25.60mL
1.0M

a. State the titrant and analyte respectively

b. Calculate the volume of KOH dispensed.

c. Calculate the number of mole of KOH

d. Write the balance equation for the neutralisation reaction.
e. Write the stoichiometric relation between KOH and HCl.
f. Calculate the molarity of HCl solution.

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EXPERIMENT 3
QUANTITATIVE ANALYSIS OF BAKING SODA

Course Learning Outcome:
Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. determine mass of a solution by using volume data and density.
2. calculate the percentage by mass of NaHCO3 in baking soda

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. Define percentage by mass.

2. What is the use of density in the calculation of percentage by mass?

Procedure
1. What is the standard solution used in this experiment?

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2. What is the indicator used in this experiment? State the colour change when the
endpoint during the titration.

3. Why the gross reading is needed when doing the titration?

4. State two precautions that must be taken during titration to ensure the accuracy of
the results.

Experiment 3 : Data Analysis
1. A 100 mL aqueous solution of NaOH with density of 1.515 gmL-1 at 20° C was
prepared by adding 3.8 g solid NaOH.
i. Calculate the mass of NaOH solution.

ii. Calculate the percentage by mass of NaOH solution

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EXPERIMENT 4
MOLECULAR GEOMETRY

Course Learning Outcome:
Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. draw the Lewis structure of a molecules and polyatomic ions
2. apply VSEPR theory to determine the molecular shape.
3. draw the basic molecular geometry of the molecules and polyatomic ions

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction
1. Write the steps how to draw a Lewis structure

2. What is the abbreviation of VSEPR stand for?
3. List down the general formula of the 5 basic shape.

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Procedure
1. Draw the Lewis structure of the following molecules.

MOLECULE LEWIS STRUCTURE

BeCl2

AlCl3

CCl4

PCl5

Experiment 4 : Data Analysis

1. Draw the basic shape and its bond angle for the following molecules.

MOLECULE MOLECULAR BOND ANGLE GENERAL
GEOMETRY FORMULA

BeCl2

AlCl3

CCl4

PCl5

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CHEMISTRY 2
DK024

DK024
Pre-Lab Module

EXPERIMENT 1
QUALITATIVE ANALYSIS OF ORGANIC CHEMISTRY

Course Learning Outcome:

Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:

At the end of this lesson, students should be able to :
1. identify the organic compound.
2. explain how to determine carbon, hydrogen, nitrogen and sulphur in organic
compound.
3. compare the quantity of sulphur in albumin and egg yolk

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. Define organic compound.

2. State 2 basic elements that present in an organic compound

3. Name the elements that are going to be determine during the experiment.

Procedure
(A) Determination of carbon and hydrogen in sugar

1. What is the function of using potassium chlorate in the combustion of sugar.

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(B) Determination of nitrogen in urea and albumin
1. Predict the smell of the gas emitted when urea is being heated until its melts.

2. Predict the observation when cooper sulphate is being added to the mixture of
albumin and sodium hydroxide.

(C ) Determination of sulphur in albumin and egg yolk

1. Why sodium hydroxide is added to the albumin and egg yolk before addition of the
lead acetate solution.

Experiment 1 : Data Analysis

(A) Determination of carbon and hydrogen in sugar
1. What would you observe at the mouth of the test tube and what will happened to the

lime water after the combustion of sugar.

2. Write the deduction of the observation in (1).

(B) Determination of nitrogen in urea and albumin
1. What is the gas emitted when urea is being heated and how to identify the gas.

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2. Write the deduction of the observation in (1).

(C ) Determination of sulphur in albumin and egg yolk
1. Predict is the observation after lead acetate was added to the egg yolk and albumin.

2. Predict and explain whether albumin or egg yolk contain more sulphur.

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EXPERIMENT 2
SATURATED AND UNSATURATED HYDROCARBON.

Course Learning Outcome:
Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. study the physical and chemical properties of alkane and alkene
2. distinguish between saturated and unsaturated hydrocarbon

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. What is hydrocarbon?

2. What is the type of reaction in alkane and alkene?

3. Name a test to differentiate between alkane and alkene. Explain the observation.

Procedure
1. Compare the colour intensity and soot given off for cyclohexane and cyclohexene.

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2. Predict the observation when cyclohexane and cyclohexane are added to the distilled
water.

3. State one precaution that must be taken during the reactions of cycloalkane and
cycloalkene with bromine in dichloromethane

4. Predict the observation when an alkane and an alkene is added to alkaline potassium
permanganate .

Experiment 2 : Data Analysis
1. Deduce the predicted observation of the soot given off from the combustion of
cyclohexane and cyclohexene

2. Deduce the predicted observation of the solubility of cyclohexane and cyclohexene in
water.

3. Write the chemical equation for the reaction of cyclohexane and cyclohexane with :
a) bromine in dichloromethane
b) alkaline potassium permanganate

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Pre-Lab Module

EXPERIMENT 3
REACTIONS OF ALCOHOLS

Course Learning Outcome:
Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. classify alcohols
2. study the chemical properties of alcohols

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction:
1. What is the functional group of alcohol?

2. Classify the alcohols below as primary, secondary or tertiary alcohol.

Alcohol Class of alcohol

(CH3)3CCH2CH(OH)CH 3

CH3CHCH2 CH2OH
CH3

(CH3)2C(OH)CH2CH3

Procedure
1. What is a Lucas reagent?

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2. State the observation of the Lucas test for the class of alcohol below.

Class of Observation

alcohol

Primary

Secondary

Tertiary

3. Predict the observation for the oxidation using acidified potassium permanganate
for the alcohol below.

Alcohol Observation

(CH3)3CCH2CH(OH)CH 3

CH3CHCH2 CH2OH
CH3

(CH3)2C(OH)CH2CH3

4. Describe the smell of the product formed from the esterification.

Experiment 3 : Data Analysis

1. Write the chemical equation for Lucas test for the alcohols below

Alcohol Equation

(CH3)3CCH2CH(OH)CH 3

CH3CHCH2 CH2OH
CH3

(CH3)2C(OH)CH2CH3

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2. Write the chemical equation for oxidation of the alcohols below

Alcohol Equation

(CH3)3CCH2CH(OH)CH 3

CH3CHCH2 CH2OH
CH3

(CH3)2C(OH)CH2CH3

3. Write the equations for the esterification process between ethanoic acid and 2-
propanol with sulphuric acid as catalyst.

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EXPERIMENT 4
ALDEHYDE AND KETONE

Course Learning Outcome:
Solve chemistry related problems by applying basic concepts and principles in physical and
organic chemistry. (C3, PLO4, CTPS3, MQF LOD6)

Learning Outcomes:
At the end of this lesson, students should be able to :

1. identify the carbonyl compound
2. differentiate between aldehyde and ketone

Student Learning Time:

Face-to-face Non face-to-face
1 hour 1 hour

Direction: Read over the lab manual and then answer the following question.

Introduction
1. What is the functional group of aldehyde and ketone.

2. Give a test that can be used to identify carbonyl compound.

3. Give a test that can be use to differentiate between aldehyde and ketone.

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Procedure
1. Name and write the structural formula of the reagent used for the Brady’s test.

2. Discribe the step to produce Tollen’s reagent in this experiment.

Experiment 4 : Data Analysis

1. Write the observation and write the chemical equation for Brady’s test for the carbonyl
compound below.

Carbonyl Equation

CH3 O
CH3 C CH

CH3

O

CH3CHCH2 C CH3
CH3

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2. Write the observation and write the chemical equation for Tollen’s test for the carbonyl
compound below.

Carbonyl Equation

CH3 O
CH3 C CH

CH3

O

CH3CHCH2 C CH3
CH3