Stoichiometry of a Precipitation Reaction
Experiment 3: Stoichiometry of a Precipitation Reaction
Abstract: In this experiment the objectives were to try and predict the amount of product that was produced in the precipitation reaction of calcium carbonate by using stoichiometry. Then learn how to figure out the actual yield, theoretical yield and percent yield of the experiment.
Experiment and Observation: The first step in the experiment was to weigh 1g of CaCl2 +2 H2O, then pour it into the 100mL glass beaker with 25mL of distilled water and then stir it to make the solution calcium chloride. The next step was to calculate the amount of Na2CO3 I needed for it to completely react with the CaCl2 +2H2O using stoichiometry.
1.0g CaCl2+2H2O= 1mol CaCl2+2H2O =0.006802mol CaCl2+ 2H2O 147.0156g CaCl2+2H2O
g of Na2CO3 = 105.98844g Na2CO3 0.006802 mol CaCl2+2H2O = 0.7209g Na2CO3 1 mol Na2CO3 X
So I needed 0.72g of Na2CO3 to completely react with 1.0g CaCl2+ 2H2O. Since the scale I used only measures to 1 decimal point I used 0.7g instead of 0.72g of Na2CO3.
After figuring out how many g of Na2CO3 I needed the next step was to weigh out the 0.7g Na2CO3 and pour into a paper cup along with 25mL of distilled water and stir to form the solution sodium carbonate. After both solutions were made and in their separate containers the next step was to pour the sodium carbonate solution into the beaker of the calcium chloride solution and watch the calcium carbonate precipitate form.
After the Calcium Carbonate Precipitate was formed the next step was to make a funnel out of the filter paper by folding it in half twice then weighing the dry filter then opening on of the sections to make a filter in the shape of a funnel.
Then I placed the funnel filter inside the actual funnel and then placed that in a coffee cup. The next step was to swirl the beaker of the precipitate to evenly distribute the contents
Abstract: In this experiment the objectives were to try and predict the amount of product that was produced in the precipitation reaction of calcium carbonate by using stoichiometry. Then learn how to figure out the actual yield, theoretical yield and percent yield of the experiment.
Experiment and Observation: The first step in the experiment was to weigh 1g of CaCl2 +2 H2O, then pour it into the 100mL glass beaker with 25mL of distilled water and then stir it to make the solution calcium chloride. The next step was to calculate the amount of Na2CO3 I needed for it to completely react with the CaCl2 +2H2O using stoichiometry.
1.0g CaCl2+2H2O= 1mol CaCl2+2H2O =0.006802mol CaCl2+ 2H2O 147.0156g CaCl2+2H2O
g of Na2CO3 = 105.98844g Na2CO3 0.006802 mol CaCl2+2H2O = 0.7209g Na2CO3 1 mol Na2CO3 X
So I needed 0.72g of Na2CO3 to completely react with 1.0g CaCl2+ 2H2O. Since the scale I used only measures to 1 decimal point I used 0.7g instead of 0.72g of Na2CO3.
After figuring out how many g of Na2CO3 I needed the next step was to weigh out the 0.7g Na2CO3 and pour into a paper cup along with 25mL of distilled water and stir to form the solution sodium carbonate. After both solutions were made and in their separate containers the next step was to pour the sodium carbonate solution into the beaker of the calcium chloride solution and watch the calcium carbonate precipitate form.
After the Calcium Carbonate Precipitate was formed the next step was to make a funnel out of the filter paper by folding it in half twice then weighing the dry filter then opening on of the sections to make a filter in the shape of a funnel.
Then I placed the funnel filter inside the actual funnel and then placed that in a coffee cup. The next step was to swirl the beaker of the precipitate to evenly distribute the contents