GMontenaro M5 Lab 1 Dehydration of a Hydrate 2022

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SUNY Empire State College *

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1205

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Chemistry

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Apr 3, 2024

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5

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Dehydration of an Inorganic Salt Hydrate Grace Montenaro 3/16/2024 Purpose This experiment will use heat to accurately calculate the ratio of water to inorganic salt within a salt hydrate. Helping to understand how heating helps to determine the water content in a hydrate, to calculate the molar ratio of water to inorganic salt in Epsom salt and find the method for balancing the chemical equation governing the decomposition of a hydrate. Procedure A heat resistance work area will be prepared by thoroughly cleaning a glass stove oven top. The materials will be collected and measured to the correct amounts and recorded in data table 1. Three aluminum dishes will be labeled and weighed to find the mass. Epsom salt will then be added to each the new mass will be measured and recorded. The Sterno lighter will then be lit and placed under a wire stand. The 3 dishes will then be placed on top the stand for ten minutes each. Once these dishes are cooled the mass will be measured again and recorded in data table 1. These measurements will be used to calculate the mass of water in each sample, the mass of magnesium sulfate, the moles of water, and the molar ratio of water to magnesium sulfate in each sample.
1 Experimental Data Table 1 Include correct units Sample 1 2 3 Calculations for sample 1 Mass of aluminum dish 1.28g 1.26g 1.26g Mass of Al dish with Epsom salt, 2.03g 2.07g 2.06g Epsom salt, original (hydrated) mass .75g .81g .80g 2.03g-1.28g=.75g Epsom salt, after heating (dehydrated) mass .37g 38g .38g 2.03g-1.66g=.37g Mass of water lost .38g .43g .42g .75g-.37g=.38g Moles of magnesium sulfate 0.003 1 Moles 0.003 2 Moles 0.003 2 Moles Molecular mass = 120.37 g/mol .37g /120.37g/mol = 0.0031 Moles Moles of water 0.021 1 Moles 0.023 9 Moles 0.023 3 Moles Molecular mass = 18.02 g/mol .38g/18.02g/mol = 0.0211 Moles Ratio of moles water: moles of magnesium sulfate 7:1 7:1 7:1 0.0211mol/ 0.0031mol =6.81 - > 7 Average Ratio 7:1 6.81+7.74+7.28=2 © 2016 Carolina Biological Supply Company
2 1.56 21.56/3=7.19 Lab Questions 1) Since magnesium sulfate is heptahydrate, Calculate the actual mass percent of water. Show all calculations. 51.17% 2) Calculate the mass percentage of water in the hydrate using your data. Show the calculations. Mass water/mass salt x 100% = Trial 1: .38/.75x100%=50.67% Trial 1: .43/.81x100%=53.07% Trial 1: .42/.80x100%=52.50% Average: 50.67+53.07+52.50=156.24/3=52.08% 3) What is the % error you obtained on the mass percentage of water? © 2016 Carolina Biological Supply Company
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3 1.78% 4) Which experimental steps can a student perform to be sure that all the water has been removed from the hydrate? The student can ensure complete removal of water from the hydrate by repeating the experiment until consistent results are obtained. 5) Identify any potential sources of error in your experiment. (Reminder: Human error is not a source of error). Measurement of the products may lead to errors if the scale is not properly calibrated. © 2016 Carolina Biological Supply Company
4 Experimental Conclusions The experiment aimed to utilize heat to accurately determine the ratio of water to inorganic salt within a salt hydrate, showing how heating elements in establishing the water content in a hydrate, calculating the molar ratio of water to inorganic salt in Epsom salt, and understanding the method for balancing the chemical equation for the decomposition of a hydrate. The data revealed a consistent ratio of moles of water to moles of magnesium sulfate, averaging at approximately 7:1. The calculated actual mass percent of water in magnesium sulfate heptahydrate was found to be approximately 51.17%, with a calculated mass percentage of water in the hydrate from experimental data averaging around 52.08%. The percentage error obtained for the mass percentage of water was 1.78%. Personal Reflection Engaging in this experiment provided a hands-on opportunity to explore the principles of chemical reactions in a practical setting. By conducting this experiment, I gained a deeper understanding of how heating facilitates the removal of water from hydrates, enabling the calculation of molar ratios and percentages to come easier to me. Throughout the experiment, I found myself immersed in the process of data collection and analysis, meticulously recording measurements, and performing calculations, to form meaningful conclusions. One aspect that stood out to me was the calculation of the actual mass percent of water in magnesium sulfate heptahydrate, which required careful consideration of molecular masses. This exercise showed the importance of attention to detail and accuracy in scientific experimentation. The lab questions also prompted critical thinking and reflection on the experimental outcomes. Calculating and identifying the percent error provided more of an understanding into the precision of the experimental procedure and potential areas for improvement. I believe this experiment reinforced the significance of methodical approach and attention to detail in scientific inquiry, laying a solid foundation for future laboratory work and exploration in chemistry. © 2016 Carolina Biological Supply Company