Stoichiometry of a Precipitation Reaction
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Abstract
The purpose of this experiment is to calculate the actual yield of Calcium carbonate from the reaction of Calcium Chloride with Sodium carbonate. We have to then compare the actual results with the theoretical value of Calcium carbonate and find out the error. When we mix 1.0 grams of Calcium Chloride and 0.80 g of sodium carbonate, it produces around 0.60 g calcium carbonate in the actual experiment. The theoretical yield of 0.68 grams of calcium carbonate and the experimental values is near to this figure. We are to compare the theoretical values with the actual values obtained and analyze the reasons for the error.
Experiment
In this experiment, 1.0 grams of Calcium chloride are mixed with 25 ml distilled water to obtain a Calcium chloride solution. By using Stoichiometry we can calculate the amount of sodium carbonate required for this reaction. One mole of calcium chloride reacts with one mole of sodium carbonate to produce one mole of calcium carbonate.
After that, we take 0.80 g sodium carbonate and mix with 25 ml of distilled water to make a solution of sodium carbonate. The two solutions are mixed together in the 100 ml beaker, forming a milky white precipitate. The solution is
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This means that 12% is the error percentage. The sources of this error is that when the precipitate is transferred to the filter, it sticks to the sides of the beaker/filter paper. The theoretical yield is 0.68 grams of Calcium carbonate and due to the loss of precipitate in the filter paper, and while handling the exact quantity of precipitate could not be recovered, which lead to the error Also, there may be some errors in measurement since it is not possible to measure up to two decimal places accurately. Also, while keeping the funnel at an angle some of the solution spills over to the sides causing some losses of the product. (Bhatt,