Abstract
This experiment aims to determine the correlation between the concentration of a catalyst, specifically magnesium sulfate on the yield of a reaction (between Calcium Chloride and Sodium Carbonate). It highlighted how something that lowered the activation energy may impact the yield. This prompted an experiment to be conducted to assess if there was a correlation on an experimental stage. The experiment showed that there was not a clear connection between the yield and the concentration of the catalyst, but it was evident that some concentrations may have been more ideal to the situations, ultimately increasing the yield. The significance derives from the importance of using these catalysts not only to speed up reactions, but potentially increase yield. Using this knowledge, specific experiments can be done over others to produce certain products more effectively and efficiently.
Exploration
1.1 Introduction
Heartburn is a casual sensation that many of us experience occasionally, although the efficacy of these tablets have been a pressing question, particularly those containing Calcium carbonate. These tablets have been an ideal remedy for neutralizing excess stomach acid and alleviating heartburn. Diving into the scientific intricacies of these tablets and the concept behind catalysts, may provide insight on improving these types of remedies. Conducting an experiment will help explore factors that might influence their effectiveness, such as variations caused by the usage of a catalyst. This endeavor not only aligns with a personal quest for a deeper understanding of physical health but also discovers practical insights to optimize the use of antacid tablets for more efficient relief. By connecting scientific principles to everyday experiences, better well-being and more information on the efficiency of the process of creating these tablets can be achieved. In order for a chemical reaction to take place, it requires a minimum amount of energy called the “activation energy”. Substances that are able to lower the activation energy of a reaction without being consumed in the reaction are called “catalysts”.
Catalysts are commonly used to accelerate the reaction or decrease the
temperature/energy required to commence a reaction (Department of Energy, 2021). It accomplishes this task by providing an alternative pathway for the reaction to occur (Priya, 2017).They are still capable of increasing the yield of the required products in a chemical reaction and minimizing that of undesirable by-products. With this, it is able to direct the reaction to yield a particular product. This characteristic of catalysts is called “selectivity” and catalysts that have this trait are called “selective catalysts” (Department of Energy, 2021). It is important to note that catalysts are very selective substances by nature and require very specific conditions.
Selectivity in catalysts can be influenced by a variety of properties of the catalysts as well as the reactants in the reaction. The surface structure, adsorbate-induced restructuring, adsorbate mobility, reaction intermediates, surface composition, charge transport, and oxidation states are all factors that can influence the selectivity of the chosen catalyst (Park, 2008). This results in the same reactants causing various different products due to the catalyst being used.
Additionally, there is a difference in selectivity between homogeneous catalysts and heterogeneous catalysts. Heterogeneous catalysts prove to be easier to separate from the products, but provide limited selectivity (Priya, 2017). On the other hand, homogenous catalysts are significantly more difficult to separate while being more selective in its reactants. This also indicates that homogeneous catalysts will mix well with the reactants in comparison to heterogeneous catalysts. Therefore, the reactant molecules will interact more with the catalyst molecules, creating more active sites for the reaction (Priya, 2017). Although, both catalysts have their appropriate properties and reactions where each catalyst is used/preferred.
1.2 Background Information
Calcium carbonate (CaCO₃) is an inorganic salt that is commonly used as a primary substance in antacid tablets to treat heartburn and indigestion.¹ These tablets function by neutralizing the stomach acid or reducing the amount of it in the body. Calcium carbonate accomplishes this by reacting with hydrochloric acid (stomach acid) to yield calcium chloride, carbon dioxide and water (CaCO₃ (aq) + HCl (aq) → CaCl₂ (aq) + CO₂ (g) + H₂O (l)), neutralizing the stomach acid.² This reaction is called a “neutralization” reaction as it neutralizes both the base and the acid, producing salt and water. In this reaction, the calcium carbonate functions as a base and the hydrochloric acid functions as the acid. Antacid tablets are created through the combination of calcium carbonate with citric acid and any type of lubricant.³ Calcium carbonate is typically used due to the fact that it provides symptomatic relief of heartburn and indigestion. Additionally, calcium carbonate also has the highest percentage of elemental calcium with around 40%, being the best calcium supplement as well.⁴ This allows it to be much more effective and efficient in solving the problems with minimal side effects.The percentage mass of calcium carbonate in these tablets is approximately 30%, playing a large role in the functionality as well.⁵ This raises the question, how does changing the concentration of the magnesium sulfate catalyst (5%, 10%, 15%, 20% and 25%) in the reaction between sodium carbonate and calcium chloride affect the calcium carbonate yield?
1.3 Hypothesis
If the concentration of magnesium sulfate catalyst increases in the reaction, then the yield of calcium carbonate will also increase. Catalysts exhibit selectivity, enhancing the yield of desired products. Since calcium carbonate is a suitable product for the magnesium sulfate catalyst, the yield will increase with the catalyst's concentration. Thus, more catalyst generally leads to a higher yield of the desired product.
1.4 Variables
Table 2. Variables in the investigation of determining the impact of the concentration of magnesium sulfate catalyst on the calcium carbonate yield in the reaction between calcium chloride and sodium carbonate.
1.5 Materials & Equipment
Materials:
1.30 g ± 0.1g of 0.1 M Sodium Carbonate (Na₂CO₃)
1.55 g ± 0.1g of 0.1 M Calcium Chloride (CaCl₂)
0.15 g, 0.28 g, 0.43 g, 0.57 g, 0.71 g ± 0.1g Magnesium Sulfate Catalyst (MgSO₄)
Deionized Water
Table 3. Equipment used in the experiment with uncertainties.
1.6 Methodology
Firstly, organize and prepare all of the equipment. All equipment listed above must be rinsed thoroughly with distilled water. Then, measure the weight of the filter paper to determine the yield of calcium carbonate at the end of the experiment. After this point, begin to prepare the solutions required. In this experiment, the concentration of all of the solutions will be 0.1M; calcium chloride, sodium carbonate and magnesium sulfate. For the 0.1M Calcium Chloride solution, measure out 1.55g of calcium chloride using the electronic balance. Then, using a 100 cm³ graduated cylinder, measure 100mL of deionized water. Mix the measured amount of calcium chloride with 100mL of deionized water to create a 0.1 M solution of calcium chloride. Let this solution rest and now prepare the 0.1M sodium carbonate solution. Measure out 1.3g of sodium Carbonate using the electronic balance, then using a 100 cm³ graduated cylinder, measure 100mL of deionized water. Then, mix the measured amount of sodium carbonate with 100mL of deionized water to create a 0.1 M solution of sodium carbonate. Moving onto the magnesium sulfate solution, measure out 0.1g, 0.25g, 0.5g, 0.75g and 1g of magnesium sulfate using the electronic balance, according to the required concentration of the catalyst. Then, using a 100 cm³ graduated cylinder, measure 10mL, 25mL, 50mL, 75mL and 100mL of deionized water, according to the corresponding mass of magnesium sulfate. Mix the measured amount of magnesium sulfate with the appropriate amount of deionized water to create a 0.1 M solution of magnesium sulfate.
Next, the materials and equipment that will be used. Starting off with the materials, each trial requires 1.3g of Sodium Carbonate tablets, 1.55g of Calcium Chloride tablets and either 0.15g, 0.28g, 0.43g, 0.57g or 0.71g of Magnesium Sulfate chips, dependent on the concentration required. Next, use deionized water to create these solutions into a 0.1M concentration. The equipment that will be used will be 250cm³ Erlenmeyer Flask, 100cm³ graduate cylinder, stirring rod, electronic scale, filter paper and scoopula.
Now, move onto conducting the experiment itself. The first part is reacting calcium Chloride, Sodium Carbonate & Magnesium sulfate. Using a 600 cm³ beaker, mix the prepared calcium chloride solution with the prepared sodium carbonate solution. Add the prepared catalyst solution of magnesium sulfate into the 600 cm³ beaker with the reactants. Stir the solution thoroughly. Moving onto the second part of the experiment of filtering out the calcium carbonate. Place a filter paper in the form of a cone shape inside of the funnel.Then, place this funnel on top of the 250 cm³ Erlenmeyer flask. Slowly pour the prepared solution of calcium chloride, sodium carbonate and magnesium sulfate into the funnel. Wait 24 hours for the filter paper to dry. Finally, mass the filter paper with the calcium carbonate to determine the total yield of calcium carbonate.
1.7 Mathematical Formulas
Table 1. Mathematical Formulas. These formulas help in determining the accuracy and precision of my experiment. They analyze aspects of deviation from the expected results and percentage error which will help in identifying how the results align to theoretical values. Finally, the concentration formula is fundamental in ensuring the right concentration of solutions and catalysts are used, regulating the external variables that may have an impact.
1.8 Safety & Risk Assessment
Sodium carbonate (Na₂CO₃)⁶ and Calcium chloride (CaCl₂)⁷ can cause serious eye irritation, therefore it is important to wash thoroughly after handling. Additionally, protective gloves, clothing, eye protection and face protection must be worn throughout the experiment. If any of these chemicals come in contact with your eyes, rinse cautiously with water for several minutes. If the eye irritation persists, seek medical advice/attention immediately.
There are no evident hazard statements or classifications for the Magnesium sulfate (MgSO₄) that is being used as the catalyst.⁸ Calcium carbonate powder⁹ can lead to skin irritation, eye irritation and irritation to the respiratory tract. Although, the concentration produced in this experiment is 0.1M where there are no evident hazard statements or classifications. In conclusion, take precaution when using calcium carbonate powder to make your solution, especially in steps such as measuring the correct mass.
1.9 Environmental Care & Disposal
Small quantities of the chemicals were used to minimize the cost of the experiment, the damage to the environment as well as the excess waste. This limited the water usage in the experiment by decreasing the concentration of the reactants that were used. Additionally, the chemicals were precisely calculated to limit the waste of the excess reactant, calcium chloride (CaCl2).
The calcium carbonate powder that was produced was disposed into sealed containers, due to the possibility of inhalation.¹⁰ The excess calcium chloride was simply washed down the drain as it is not harmful to the environment.¹¹
Results
2.1 Qualitative Data
Table 4. Qualitative observations before, during and after the reaction.
Sample Calculations - These calculations indicate the expected yield of this experiment, in accordance to a perfect scenario and theoretical chemistry concepts. The standard deviation also provides insight into how precise the data is and the ability for the experiment to be replicated with limited error.
This standard deviation value indicates that there is very minimal deviation between the 5 trials that were conducted with 10% concentration of magnesium sulfate. Therefore, the results that were obtained are fairly accurate and consistent.
2.2 Processed Data
Table 6. Processed Quantitative Data → Effect of Concentration of Magnesium Sulfate Catalyst on the yield of Calcium Carbonate
Concentration of Magnesium Sulfate (%, ± 1%) | Volume of Water (mL,± 5 mL ) | Average Yield of Calcium Carbonate (g, ± 0.1g) | Standard Deviation | Percentage Decrease (%) |
5% | 210 mL | 0.98 g | 0.0141 | 20.3 |
10% | 225 mL | 1.03 g | 0.0259 | 16.1 |
15% | 250 mL | 0.98 g | 0.0251 | 20.7 |
20% | 275 mL | 0.83 g | 0.0327 | 32.4 |
25% | 300 mL | 0.69 g | 0.0332 | 43.9 |
Discussion
From this experiment, it can be concluded that there is a slight correlation with the usage of catalysts and the yield of the reaction. Although, the experimental yield (1.13g) is lower than the theoretical yield (1.25g), which highlights how the addition of a catalyst never increased the yield of the reaction from its theoretical yield. This may be due to a variety of reasons including that of the addition of the catalyst. Looking specifically at the concentrations 15% - 25%, it is evident that there is an overall decline in the effectiveness. This trend is indicated through the red line found on the graph (Figure 2). But, there remains one concentration where the yield of calcium carbonate peaked, being 10%. This indicates that when the mass of the catalyst is 1/10 of the entire reaction, the greatest amount of yield can be obtained.
It is also evident that as the concentration of magnesium sulfate exceeds 15%, there is a very steep decline in the yield, leading to an approximate 38% decrease from the theoretical yield. This indicates that an excess of catalyst may also have a major impact on the reaction’s yield.
According to BYJU’s, an appropriate concentration of catalysts in a reaction range from 0.1% to 7%, aligning somewhat with the results of this experiment. This indicates that although catalysts themselves may not have a large impact of increasing the yield of the reaction. Different concentrations of the catalysts may lead to various changes in the yield. An excessive amount of catalyst leads to a significant decrease in the yield.
It can be noticed that the addition of catalysts led to a major decrease in the yield of the reaction in comparison to the theoretical yield. This decrease can be explained through the various systematic, random and human errors that occurred during this experiment. These errors will be further discussed in the weaknesses of the experiment.
As for the personal engagement, the possibility of using catalysts to further increase the yield of calcium carbonate found in antacid tablets was answered. It is clear that the catalyst may not have a direct correlation with the yield, but in the process of increasing the rate of reaction, an ideal amount of 10% of magnesium sulfate catalyst must be used to ensure ideal results.
3.1 Strengths of the Experiment
A strength of the experiment is its precision as the overall uncertainty values lie relatively low, having minimal impact on the results. This is due to the low amount of reactants used in the reaction, ensuring a low range of error and deviation from the original required amounts. This is also indicated through the low standard deviation numbers in the processed data table (Table 6). Additionally, the simplicity of the experiment allows it to be easily replicated and done again as well as rapid results. Moreover, the reactants and catalyst used in the experiment are all safe chemicals allowing there to be limited environmental and safety hazards. Although, safety precautions were still taken to ensure a safe procedure.
3.2 Weaknesses & Improvements of the Experiment
There were several types of errors encountered during the experiment, which affected the accuracy and consistency of the results.
A random error occurred due to the change in room temperature from morning to afternoon. As the temperature increased, the kinetic energy of the particles also increased, potentially leading to a higher rate of reaction and a greater yield. To mitigate this, a thermometer should be used to monitor the temperature, and the experiment should be conducted in an environment with a constant temperature and minimal disturbances to limit temperature-induced deviations.
Systematic errors were also observed, with the first being minimal stirring or mixing of solutions. In some trials, the time spent stirring was reduced due to time constraints, which may have led to incomplete reactions, resulting in the solution not being fully dissolved and preventing proper precipitation. To avoid this error, equivalent amounts of time should be spent stirring in each trial to ensure the solution is completely dissolved and the precipitate is fully formed, leading to accurate yield readings.
Another systematic error occurred due to the varying drying times for the filter paper. In some trials, the drying time was extended, particularly over weekends, which allowed the precipitate to dry longer. This caused the precipitate to become lighter, as some of the water evaporated, affecting the mass measurements. To correct this, equal drying times should be ensured for all trials, with no experiment conducted past the 24-hour mark to avoid inconsistencies in drying duration and ensure fair comparisons.
3.3 Extensions of the Investigation
This investigation can be enhanced by incorporating various different factors such as temperature and pH to optimize the selectivity of the catalyst to maximize yield. It would provide results more realistic to lab conditions, connecting more with the personal engagement. Furthermore, the ideal temperature and pH for the experiment to occur may be different, justifying the discrepancy between the theoretical and actual yield of calcium carbonate. Therefore, including these factors into the experiment will lead to more accurate results in relevance to personal engagement.
Comparing a variety of catalysts applicable to this reaction would also lead to there being a greater range of results. This would provide a more detailed answer to the question of “How concentrations of different catalysts affect its selectivity, ultimately leading to a change in yield?” The variety of catalysts allows there to be a connection between the concentration of the catalyst with the type of catalyst. The usage of a metal catalyst or carbon catalyst may result in a lack of selectivity which will alter the ideal concentration to maximize yield.
3.4 Conclusion
This paper investigated the different concentrations of magnesium sulfate catalyst (5%, 10%, 15%, 20% and 25%) and its effects on the yield of calcium carbonate. It was hypothesized that as the concentration of the catalyst increased, the yield of the precipitate would also increase. The results of the experiment indicated that the concentration of the catalyst in correlation with the yield of the precipitate had an overall strong negative correlation. It indicated that as the concentration increased, the yield of the calcium carbonate started to decline. Although, there was one concentration where the yield was maximized; being 10%. This indicated that the optimal concentration to maximize yield was 10%, but the overall experiment had a trend of declining as the concentration increased. The percentage error was approximately 32% indicating that there is a large range between the different concentrations. This large error is as a result of the random and systematic errors in the experiment. Factors such as the temperature change, stirring rate and time left for filter paper to dry all have an impact on the calcium carbonate yield. These factors can be improved by conducting the procedure in a closed environment as well as keeping standard times and rates throughout the experiment. To further enhance this investigation, more factors such as temperature and pH can be measured to receive more specific/detailed results. Overall, the procedure indicated the ideal concentration of the magnesium sulfate catalyst to be 10% for it to produce the greatest yield and indicated that there is minimal correlation between catalysts and the yield of products. This can be transferred to the real world where scientists or lab technicians can produce certain products through some reactions in comparison to others. For example, if the reaction between calcium chloride and sodium carbonate with the magnesium sulfate catalyst can increase the yield, it can be prioritized over the reaction between calcium and carbonate. Expanding it to a much larger scale where kilograms of reactants are reacted together, the yield can be significantly increased. Although, it is key to consider that this experiment was done in an open system where many factors were limited, but others can implicitly have taken a toll. Finally, the extremely small amounts of reactants should also be carefully analyzed as upscaling the experiment may produce different results.
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¹ Incorporation, E. (2023, June 12). Tums Chewable Tablets (Calcium Carbonate): Uses & Side Effects. Cleveland Clinic. Retrieved December 28, 2023, from https://my.clevelandclinic.org/health/drugs/20402-calcium-carbonate-chewable-tablets
² Cleveland Clinic “Tums Chewable Tablets (Calcium Carbonate): Uses & Side Effects”
³ Alexander, T. A., & Peterson, D. L. (1987, March 17). US4650669A - Method to make effervescent calcium tablets and calcium tablets produced thereby. Google Patents. Retrieved January 8, 2024, from https://patents.google.com/patent/US4650669A/en
⁴ Mayo Clinic. (2022, November 1). Calcium and calcium supplements: Achieving the right balance. Mayo Clinic. Retrieved January 9, 2024, from https://www.mayoclinic.org/healthy-lifestyle/nutrition-and-healthy-eating/in-depth/calcium-supplements/art-20047097
⁵ Alexander, T. A., & Peterson, D. L. “Method to make effervescent calcium tablets and calcium tablets produced thereby”
⁶ Chemical Safety. (2023, March 17). Chemical info for Sodium carbonate. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=32188544&name=Calcium%20chloride
⁷ Chemical Safety. (2023, September 11). Chemical info for Calcium chloride. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=32188544&name=Calcium%20chloride
⁸ Chemical Safety. (2023, November 19). Chemical info for Magnesium sulfate. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=34074013&name=Magnesium%20sulfate
⁹ Department of Human Services ENVIRONMENTAL TOXICOLOGY SECTION. (1998, October 18). Oregon Department of Human Services HEALTH EFFECTS INFORMATION. Oregon Department of Human Services HEALTH EFFECTS INFORMATION. Retrieved February 5, 2024, from https://www.oregon.gov/oha/PH/HEALTHYENVIRONMENTS/DRINKINGWATER/MONITORING/Documents/health/caco3.pdf
¹⁰ New Jersey Department of Health. (2015, July 21). Hazardous Substance Fact Sheet. Hazardous Substance Fact Sheet. Retrieved February 5, 2024, from https://nj.gov/health/eoh/rtkweb/documents/fs/4001.pdf
¹¹ Davies, M. (2022, August 10). How To Dispose Of Calcium Chloride. Ethical Shift. Retrieved February 5, 2024, from https://www.ethicalshift.com/recycle/disposing/chemicals/how-to-dispose-of-calcium-chloride/
Works Cited
Alexander, T. A., & Peterson, D. L. (1987, March 17). US4650669A - Method to make effervescent calcium tablets and calcium tablets produced thereby. Google Patents. Retrieved January 8, 2024, from https://patents.google.com/patent/US4650669A/en
BYJU. (2017). Catalyst - Activity & Selectivity of Catalyst, Types & Examples of Catalyst. BYJU'S. Retrieved December 23, 2023, from https://byjus.com/chemistry/activity-selectivity-of-catalyst/#Selectivity-of-Catalyst
Chemical Safety. (2023, March 17). Chemical info for Sodium carbonate. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=32141786&name=Sodium%20carbonate
Chemical Safety. (2023, September 11). Chemical info for Calcium chloride. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=32188544&name=Calcium%20chloride
Chemical Safety. (2023, November 19). Chemical info for Magnesium sulfate. Safety Data Sheets (SDS). Retrieved February 5, 2024, from https://chemicalsafety.com/sds1/sdsviewer.php?id=34074013&name=Magnesium%20sulfate
Davies, M. (2022, August 10). How To Dispose Of Calcium Chloride. Ethical Shift. Retrieved February 5, 2024, from https://www.ethicalshift.com/recycle/disposing/chemicals/how-to-dispose-of-calcium-chloride/
Department of Human Services ENVIRONMENTAL TOXICOLOGY SECTION. (1998, October 18). Oregon Department of Human Services HEALTH EFFECTS INFORMATION. Oregon Department of Human Services HEALTH EFFECTS INFORMATION. Retrieved February 5, 2024, from https://www.oregon.gov/oha/PH/HEALTHYENVIRONMENTS/DRINKINGWATER/MONITORING/Documents/health/caco3.pdf
Incorporation, E. (2023, June 12). Tums Chewable Tablets (Calcium Carbonate): Uses & Side Effects. Cleveland Clinic. Retrieved December 28, 2023, from https://my.clevelandclinic.org/health/drugs/20402-calcium-carbonate-chewable-tablets
Mayo Clinic. (2022, November 1). Calcium and calcium supplements: Achieving the right balance. Mayo Clinic. Retrieved January 9, 2024, from https://www.mayoclinic.org/healthy-lifestyle/nutrition-and-healthy-eating/in-depth/calcium-supplements/art-20047097
New Jersey Department of Health. (2015, July 21). Hazardous Substance Fact Sheet. Hazardous Substance Fact Sheet. Retrieved February 5, 2024, from https://nj.gov/health/eoh/rtkweb/documents/fs/4001.pdf
Park, J. Y. (2008). Molecular factors of catalytic selectivity. PubMed. Retrieved December 23, 2023, from https://pubmed.ncbi.nlm.nih.gov/19006127/
Priya, S. (2017, February 8). Catalyst | PPT. SlideShare. Retrieved December 23, 2023, from https://www.slideshare.net/shanmugapriya138/catalyst-71899593
Science, O. (2021). DOE Explains...Catalysts. Department of Energy. Retrieved December 23, 2023, from https://www.energy.gov/science/doe-explainscatalysts
Appendices
Appendix A: Raw Quantitative Data → Effect of Concentration of Magnesium Sulfate Catalyst on the yield of Calcium Carbonate
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