CATAMPONGAN, ROY JR. P.
MRS. CORAZON SACDALAN
BSES-2B
May 22,2022
Experiment No. 7
Determination of Carbonate Content on Soda Ash
Introduction
In this experiment, students will perform an experiment to determine the carbonate
content on soda ash. By performing this experiment, they will have knowledge how
determination is done, and different processes involve in this experimentation.
Objectives
At the end of this activity, the students should be able to:
 Calculate the molarity of HCl solution
 Quantify the percentage of Na2CO3 present in the sample
Materials and Apparatus
Erlenmeyer flask, beaker, buret, buret clamp and stand, volumetric flask, wash bottle, stirring
rod, 12 M HCl, sodium carbonate, methyl orange indicator
Procedure
A. Preparation and standardization of 0.10 M HCl
1.A 8.5 mL of concentrated HCl was transferred using a pipet and was diluted to a 1- L with
carbonate free distilled water.
2.Approximately 2 g of primary standard grade sodium carbonate was dried at 1100 C for 2 hours
and cooled in a desiccator.
3. Three sample with approximately 0.2 to 0.25 g of dried sodium carbonate was weighed and
transferred to three Erlenmeyer flasks.
4.Each sample was dissolved in 25 mL distilled water and 2 drops of methyl orange indicator
were added.
5. Each sample was titrated with 0.1 M HCl solution until the indicator has changed gradually
from its initial yellow color to a definite red color. The titration was stopped, and the solution
was gently boiled for 2 minutes. The flask was covered with an inverted beaker and was cooled
to room temperature. The yellow color should return. The titration was continued until a sharp
yellow to red color is achieved.
6. Finally, the molarity of the HCl solution was calculated.
B. Titration of a Soda Ash Sample
1. Three samples with approximately 0.35 to 0.45 g was weighed and then transferred into three
clean erlenmeyer flask.
2. About 50 mL of distilled water was added to each flask and was swirled gently to dissolve the
salt.
3. 4 drops of methyl orange indicator was added and was titrated with the HCl solution to an
intermediate red color.
4. The solution was boiled for 2-3 minutes, and solution was cooled to room temperature.
5. The flask’s walls were washed with distilled water from a wash bottle, and then titration was
continued until the appearance of red color.
6. The final volume of HCl was recorded and data were tabulated.
7. The percentage of Na2CO3 in the sample was calculated and reported.
Data and Results
Questions:
1. Why is the solution boiled obtaining the intermediate red color?
 It is essential to bring to solution to boil for 5 minutes because it will liberate the CO2
present in the solution. The CO2 was formed due to the combination of Na2CO3 and
HCl. If the solution wasn’t boiled, it may interfere with the result. By heating the
mixture to the boiling point, we can get rid of the CO2 present in the solution which will
result in a more accurate data.
2. What are the possible sources of error in this experiment and how can these errors be
minimized?

There are a lot of possible sources of error while performing the experiment. First, not
cleaning and rinsing the burette prior to the experiment. By not cleaning it, the whole
titration process will be compromised which would affect the result of the experiment.
Then, putting too much drop to HCl to Na2CO3 solution. With this, the color will be
darker instead of having an orange color and will affect the endpoint and concentration of
the solution.
Discussion
There can be a lot of sources of errors for this experiment. First is the over titration of the
solution which may lead to a darker color of the solution which will later affect the concentration
of solution. Another source of error is not rinsing and cleaning the burette before conducting the
titration. Burette must be cleaned since we are not aware what kind of solution was placed on it
by its previous user. Not cleaning it may contaminate the solution and may lead to inaccurate
results.
Conclusion
Based on the data gathered upon conducting the experiment, the average molarity of
hydrochloric acid is 0.1035. Meanwhile, the percentage of Na2CO3 present in the sample has an
average of 39.97%. Also, upon computation, it is found that there is an average of 0.1428 g of
Na2CO3 present in the sample.
Application
Real life application of titration related to environmental science includes wastewater analysis. In
wastewater analysis, the level of contamination is determined, the harmful chemicals present in
the water is identified, and ways how to get rid of it are formulated. Then, determining the
mineral content of drinking water. By doing a gravimetric analysis, the components present in
the water can be monitor and evaluate whether there is a component that would put our health at
risk.
References
https://www.bing.com/ck/a?!&&p=13c39babecb421ea2f014a64dc8d6eacddcd4b5122649d552e0
87f56463fe230JmltdHM9MTY1MzIwMjc2OSZpZ3VpZD02MTYwY2ZmMC00OWEyLTQ0M
DEtOGE5Yy0wZDIzNGIxZDJlYTUmaW5zaWQ9NTE2MA&ptn=3&fclid=b93efbe5-d99c-
11ec-ab5be2bfb5a0e937&u=a1aHR0cHM6Ly9hbGx1c2Vzb2YuY29tL2NoZW1pY2FsLzE1LXVzZXMtb
2YtdGl0cmF0aW9uLw&ntb=1
Gravimetric Analysis - Definition, Types and Steps (vedantu.com)