Julia Wu
Purpose: The purpose of this lab was to design atomic number 20 Chloride and Magnesium Sulfate to produce 2.00 grams of precipitate.
Materials: calcium chloride, magnesium sulfate, two beakers, two flasks, dis tail end, and reach paper.
Procedure:
Write the balance equation for Calcium Chloride and Magnesium Sulfate.
Calculate how much of for from each one one reactant is needed to produce 2.00 grams of precipitate.
one time you have calculated the derive of each reactant, proceed to the lab table and retrieve the pastime equipment: two have cylinders, two beakers, two flasks, funnel, and filter paper.
seclude the mass of the filter paper.
Pour the right amount of each reactant, into the two beakers.
From each beaker pour the each reactant into a graduated cylinder. Make sure the amount you pour, is the amount you calculated for each reactant.
Next, pour each reactant into the flask.
Wait for the double replacement chemical reaction to happen. Stir if necessary.
Once the reaction has taken place, place the funnel in the routine flask.
Fold the filter paper and put down it into the funnel.
Little by little, pour the flask that the reaction took place in, into the second flask. Once you have poured all of the liquid into the second flask, wait 24 hours four the filter paper to dry.
Once the paper is dry, carefully take it out of the funnel fashioning sure not to spill the precipitate, than take the mass of the filter paper.
Data:
Reactant | Volume (mL) | Final Mass of Product |
Calcium Chloride | 19.6 mL | 1.29 g |
Magnesium Sulfate | 29.4 mL |
chemical Equation:
CaCl2 (aq) + MgSO4 (aq) CaSO4 (s) + MgCl2 (aq)
Calculations:
2.00g CaSO4 1 bulwark of CaSO4 1 mol CaCl2
= 0.0147 mol CaCl2
136.15g CaSO41 mol CaSO4
Molarity of CaCl2 = 0.75M
0.0147 mol x = 0.0147
0.75 M= x liters 0.75x = 0.0147 0.75 x =0.020 L = 20 mL CaCl2
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