Lab Report: Standardization of a strong acid (HCL) with weak base (Na2CO3)
Submitted to:
Dr. Md. Nazmul Abedin Khan
Assistant Professor
Department of Mathematical and Physical Sciences
Submitted by
Group Number: 2
Group member: Hrikesh,
Juboraj,
Antor
Name: Atik Sharear Ananto
Student ID: 2022-1-60-186
Date: 26-06-2022
Section: 04
1
Table of Contents
Introduction....................................................................................................... 2
Solution ............................................................................................................. 3
Error Analysis..................................................................................................... 4
Contribution ...................................................................................................... 4
Conclusion ......................................................................................................... 4
2
Introduction
To complete simple titration between an acid and a base, we need to follow some
necessary steps. In this case we take HCL as the acid and Na2CO3 as the base.
•
First, we asked the permission of our faculty teacher to work in the lab.
Through his observation, we completed our lab work. We Also
maintained proper lab regulations throughout the whole session.
•
We washed the burette with water and carefully check the burette
gauge to avoid any unwanted leaking. Also, we took 0.1 M of HCL for
the titration. With the help of the pipette, we took 10ml of standard
sodium carbonate solution into a 250 ml conical flask. Also, we took
some methyl orange as the indicator.
•
In the conical flask we took 10 ml of Na2CO3. where we added two
drops of methyl orange.
•
We selected top to bottom as our scale. We filled the burette with HCL
and noted down top point. Then we put the conical flask under the
burette. Then we carefully added drop by drop HCL into the conical
flask. Until its color changes to yellowish to red. The conical flask was
shaken continuously.
•
If the solution shows, it’s color red then it means our titration is
complete. We did exact same tasks three times and every time we
noted down top and bottom scale of HCL. And pointed out
approximately when the solution turned red and averaged it out.
•
After completing all the steps, with the permission of our course
Instructor, we carefully put down all the chemical equipment. And
submitted the calculation.
3
Solution
Sodium carbonate is the salt of a weak acid, carbonic acid. Its reaction with HCL is a
two-step process and may be represented as,
Titration:
Na2CO3 + HCl → NaHCO3 + NaCl
NaHCO3 + HCL → NaCl +H2O+CO2
Na2CO3 + 2HCL → 2NaCl + H2O+CO2
From the experiment, we noted,
Observation No
Initial Burette
Reading (mL)
Final Burette
Reading (mL)
Difference (mL)
Average (mL)
1
12.1
22.0
9.9
9.86
2
22.6
32.4
9.8
3
32.6
42.5
9.9
There are some formulas we used to calculate the error percentage.
Ma+Va = 2 x Mb (M of Na2CO3) x Vb (V of Na2CO3)
Here,
Ma= ?
Va = 9.86 mL
Mb= 0.05
Vb = 10 mL
so, Ma=
2∗10∗0.05
9.86
= 0.1014
4
Error Analysis
From the experiment, Ma = 0.1014 , In theory we know Ma = 0.1
We know
Error= |
Theoretical−Experimental
𝐸𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙
|x 100%
So,
Error = |
0.1−0.1014
0.1
| x 100%
Error= 1.4
Contribution
I carefully noted down every step, including measuring volume of acids and
base, important data about the experiment. Calculating experimental data by
using known formulas and executing it.
Learning’s
• The characteristics of titration
• At first when the solution was base, it got to be pH above 7. It was
yellowish in color.
• Flask was shaken carefully when every time HCL were added to the
solution. Slowly it was changing its color yellowish to red
• At exact point where the solution turned into red stopped adding HCL. It
means titration is complete and pH might be near 7. So pH color is
different for different atoms.
• Practical usage of some known chemical formulas .
Conclusion
All the laboratory regulations were maintained properly. This practical
experiment will widen our knowledge in our future experiments. Also, we
learned a lot through this experiment.
-End of lab report-