LABORATORY REPORT
SKU1033
SESSION 2023/2024
EXPERIMENT
DILUTION OF CONCENTRATED ACID SOLUTION
TITLE
1) MOHAMAD HASPIRULLAH BIN R.HAPESIDON
STUDENT’S NAME &
(E20221030576)
MATRIC NO.
2)MUHAMMAD IMRAN HAIKAL BIN OTHMAN
LECTURE GROUP A
LECTURER NAME ChM. Dr. Mohamad Idris Saidin
CHECKLIST Marks
Grammar/spelling 10
Format 10
Introduction 10
Materials & 10
Apparatus
Methods 10
Results 10
Discussion & 10
conclusion
References 10
Conceptual 20
understanding
TOTAL MARKS 100
EXPERIMENT 3
DILUTION OF CONCENTRATED ACID SOLUTION
OBJECTIVES
Upon completion of this experiment, students should be able to prepare a series of acid solution at
different concentration.
INTRODUCTION
Dilution is the process of decreasing the strength of an acid or base. We know that acids and bases
produce H3O+ and OH- ions in water. When they are diluted (by having more amount of water), the
concentration of H3O+ or OH- ions per unit volume decreases. This results in decrease of the strength
of the acid. pH value can be measured by using various methods, such as universal indicator and pH
meter. pH value depends on the concentration of H3O+ in the solution.
Figure 3.1: pH meter
CHEMICALS AND APPARATUS
Chemicals
Hydrochloric acid (37 %w/w)
Apparatus
Pipette
Volumetric flask (50 mL, 500mL)
Dropper
Glass rod Filter
funnel pH meter
3.4 PROCEDURE
Part A: Preparation of stock solution: 0.5 M Hydrochloric acid from HCl (37 %w/w)
1. Molarity of hydrochloric acid (37 %w/w) is determined by completing Part A table in Data Sheet.
2. 0.5 M hydrochloric acid is prepared in 500 mL volumetric flask from hydrochloric acid
(37%w/w).
Part B: Dilution of 0.5 M Hydrochloric acid, HCl
1. solution of 0.1 M, 0.01 M, 0.001 M and 0.0001 M is prepared in 50 mL volumetric flask using
dilution technique.
2. pH value are observed and recorded using pH meter.
DISCUSSION BASED ON THE FOLLOWING QUESTIONS
Part A: Preparation of stock solution: 0.5 M Hydrochloric acid from HCl (37 %w/w)
Pour hydrochloric acid solution (37% w/w) in a beaker.next,transfer 20.49 ml hydrochloric
acid (37% w/w) solution into 500 ml volumetric flask.then add distilled water into the volumetric flask
and then use dropper to fill until it reaches meniscus level.
Part B: Dilution of 0.5 M Hydrochloric acid
HCL with solution 0.1M has the highest concentration thus having the lowest ph scale at
1.11.next ,HCL solution that has the lowest concentration,0.0001M has the highest ph value at
3.96.both hcl solution with 0.01M and 0.001M concentration has ph value at 2.09 and 3.13
accordingly.we can say the higher concentration is,the lower ph value of acid solution which is more
acidic.
Dilution is the process in which water or any other solvent is added to the solution to decrease
the concentration, in this case,ion hidroxide,OH-.Basic solution has more hydroxide ion than
hydrogen ion. Addition of water to an acidic or basic solution causes change of pH. This results in
the increase of pH of alkali towards 7. This makes the solution more alkaline. That means the pH
increase on diluting an alkaline solution
REFERENCES
1. How to Dilute Copper Sulfate. (2017, April). Retrieved from
https://sciencing.com/dilute-copper-sulfate-8089464.html
2. Safe Handling of Hydrochloric Acid. (2006, November). Retrieved from
http://www.jsia.gr.jp/data/handling_02e.pdf
3. Preparing and diluting solutions (2012). Retrieved from
http://lrrpublic.cli.det.nsw.edu.au/lrrsecure/sites/lrrview/13897/13897_pop16.html
3.7 DATA SHEET
Part A: Preparation of stock solution: Hydrochloric acid, HCl (37% w/w)
Mass (g) of HCl in 100 g 37
Density of HCl (g/mL) 1.2
3783.33
Mass (g) of HCl in 1 mL
Molar mass of HCl (g/mol) 36.46
Molarity of hydrochloric acid (37 %w/w)
12.178
(M)
Mass of HCl needed (g) 6.089
Part B: Dilution of 0.5 M hydrochloric acid
The concentration of HCl before
dilution (mol/L) 0.5
The volume of the volumetric flask
(mL) for dilution 50
Volume needed to prepare 0.1 M
HCl (mL) 10
Volume needed to prepare 0.01 M
HCl (mL) 5
pH value of HCl solution for four (4) different concentrations
The concentration of HCl (M)
pH value 0.1 0.01 0.001 0.0001
1.11 2.09 3.13 3.96
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DATE LECTURER’S SIGNATURE/STAMP
