Stoichiometry of a Precipitation Reaction

Data T sufficients Step 3 usher the advisement of the needed amount of Na2CO3 Convert 1. 0g of CaCl2-. 2 piddle to gram molecules of CaCl2-. 2H2O 1. 0g x 1 mole CaCl2-. 2H2O 147. 0 g CaCl2-. 2H2O = 0. 00680 moles CaCl2-. 2H2O The mole ratio is 11 accordingly if we have 0. 00680 moles of CaCl2-. 2H2O we will as strong need 0. 00680 moles of Na-2CO3 Convert moles of Na-2CO3 to grams of Na2CO3 = 0. 00680 moles Na-2CO3 x 105. 99g Na-2CO3 1 mole Na-2CO3 = 0. 72g This means that we need 0. 72g of Na-2CO3 to fully react with 1g of CaCl2-. H2O Step 4 Mass of weighing strike_0. 7___g Mass of weighing dish and Na2CO3__1. 4__g Net mass of the Na2CO3 __0. 7__g Step 6 Mass of filter study __0. 7__g Step 10 Mass of filter paper and dry atomic number 20 carbonate__1. 2__g Net mass of the dry atomic number 20 carbonate_0. 5___g (This is the actual yield) Step 11 Show the calculation of the theoretical yield of calcium carbonate. The mole confine between CaCl2-. 2H2O and CaCO3 is 11 that means that if we have 0. 00680 moles of CaCl2-. 2H2O we will approach 0. 00680 moles CaCO3Convert the moles of CaCO3 to grams of CaCO3 = 0. 00680 moles CaCO3 x hundred g CaCO3 1 mole CaCO3 = 0. 68g CaCO3 Show the calculation of the percent yield. = Actual yield/Theoretical yield x 100 = 0. 5/0. 68 x 100 = 73. 5% Conclusion The target of the experiment is to predict the amount of product produced in a precipitation reaction using stoichiometry. Secondly, the experiment accurately measures the reactants and products of a reaction. Also, the experiment is to shape actual yield vs. theoretical yield and to calculate the percent yield.For example in this experiment, we were able to predict that we need 0. 72g of Na-2CO3 to fully react with 1g of CaCl2-. 2H2O. another(prenominal) example is that, we calculate the amount of theoretical yield of Calcium change to be 0. 68g and the percentage yield to be 73. 5%. The scientific principles regard here was that when two or more soluble substances in signalise solutions are mixed together to form an insoluble commingle they settles of a combined solution as a solid. The solid insoluble compound is called a precipitate.For example in this experiment, we combined sodium carbonate and calcium chloride dehydrates to produce a precipitate of calcium carbonate. The formula mathematically is Na2CO3(aq) + CaCl2. 2H2 = CaCO3(s) + 2NaCl(aq) + 2H2O. Sources of erroneousness and ways to minimize them There may still be whatever solid particles in the beaker thereby we will not be able to get the correct mass (quantity) of the Calcium Carbonate. To minimize the error we should drug abuse an instrument that buttocks be able to scoop out the constitutional solid from the beaker.Also if the water in the Calcium Carbonate is not flop dried, the net mass of the Calcium Carbonate can be highly high. To solve this we must make sure the Calcium Carbonate is well dried. Error of approximation the molar mass if not well nigh(a)d, can lead to an error in the calculation. To minimize this error the instruction should demo how many decimal point or how significant figure to approximate to. I am highly impressed with the experiment.