![]() Rinse the beaker with distilled water and thoroughly dry with paper towel. Wash the now empty 100 mL glass beaker (that contained the Na2CO3 solution) with soap and water.Use the information and examples provided in the Exploration to determine the maximum (theoretical) amount of CaCO3, in grams, that can be produced from the precipitation reaction.Swirl the beaker to fully mix the two solutions and the precipitate of calcium carbonate will form instantly. Rinse the beaker containing Na2CO3 with 2-3 mL of distilled water and transfer the rinse to the beaker containing the CaCl2 Pour the Na2CO3 solution from the 100 mL glass beaker into the beaker containing the CaCl2.Use the stir rod to stir the Na2CO3 and break apart any clumps until it is fully dissolved into the water.Use the metal spatula to measure the calculated amount of Na2CO3, and carefully add it to the 25 mL of distilled water in the second 100 mL glass beaker. Submerge the weigh boat into the beaker to transfer all of the Na2CO3 if any residue remains on the weigh boat.Turn on the digital scale, place the plastic weigh boat on the scale and tare the scale so that it reads 0.00 g.From that calculation, determine how many grams of Na2CO3 are necessary to reach stoichiometric quantities. Use the information and examples provided in the Exploration and the values recorded in Data Table 1 from Step 8 to determine how many moles of Na2CO3 are necessary to reach stoichiometric quantities.2H2O and then calculate how many moles of pure CaCl2 are present in the 1.50 g of CaCl2.Use the information and examples provided in the Exploration to calculate how many moles of CaCl2.Rinse the weigh boat and metal spatula with distilled water and fully dry both with paper towels. ![]()
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