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Calcium Lab

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Jennifer Liu Block 2-1 Monday, December 13, 2010 Evelyn Korompai The Preparation of Calcium Carbonate from Calcium Carbonate It was found that when 2 g of calcium carbonate is reacted with hydrochloric acid, and then the aqueous product of that reacts with sodium carbonate, the same amount of calcium carbonate (2 g) should be produced. In other words, two chemical reactions, the first reaction containing calcium carbonate as the reactant, were conducted to produce a product of calcium carbonate in an aqueous solution. \ Purpose To use 2 g of calcium carbonate and, by using two reactions, produce a product of calcium carbonate and after the reaction, calculate the percent yield. Procedure Day 1: 1) Gather all equipment. 2) Weigh out approximately 2 g of calcium carbonate into a 250 mL beaker. Record the weight in the data table. 3) Weigh a piece of filter paper and record in in your table. ...read more.


fluid Table 3: Quantitative Observations after Reaction #1 Mass Na2CO3 2.01g Mass beaker and reaction 1 product 149.93g Table 4: Observations of Reaction #2 Quantitative Qualitative 0:01 seconds-0:20 seconds During the reaction, -The Na2CO3 rests in lump 1:00 minute After stirring, -Solution is more white in colour, yet still fluid Filtering, -Clear, solution, fluid coming out of filter -Solid/powder material rests on side of paper After filtering, -The powder on the filter paper is white and thick Table 5: Observations of the Product of Reaction #2 Quantitative Qualitative Mass of powder and paper: 3.26g -Chalky, soft, brittle -White powder Questions 1) What safety precautions were required for this experiment? Explain your reasoning. Although this experiment was not very dangerous, there were still some safety requirements. First of all, we put safety goggles to protect our face not necessarily from explosions, but to ensure our complete safety at all times, in case a substance, say, the product of hydrochloric acid and calcium carbonate were to go in our eyes. 2) ...read more.


While we filtered, there is a possibility that the filter paper could have ripped a little and this would have caused some of the solid to be filtered. As a result, the mass of calcium carbonate may be a little bit off. Other errors include the fact that not all reactants may have reacted due to some unknown random error and that not all reactants retrieved from the containers are 100% pure. Conclusion In this experiment, we learned how to calculate the percent yield by using the formulas of the reactions to first calculate the expected amount of product. When we reacted 2g of calcium carbonate, our result was 1.84 g. The expected yield was 2 g, and so we were both very close to the expected yield, as our percent yield for CaCO3 is 91%. In this experiment, we learned that it is not easy to get a high percent yield, and that exact measurements are crucial when conducting an experiment. To decrease the possibility of errors to the best of our ability, we must have the most exact measurements as possible. ...read more.

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