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12. Assuming your reaction occurred with a 100% yield of product being produced, name all of the substances that would be dissolved in the filtrate at the end of the reaction. Based on the amounts of reactants you added to the reaction vessel, calculate how many moles of those substances should be present?

12. Assuming your reaction occurred with a 100% yield of product being produced, name all of the substances that would be dissolved in the filtrate at the end of the reaction. Based on the amounts of reactants you added to the reaction vessel, calculate how many moles of those substances should be present?

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 94AP
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I only need the answers for the highlighted portions please :)

This was a lab I performed in my chemistry, it was using vaccum filtration to collect solids from a Barium Chloride solution (BaCl2*2H2O). I took 0.780g of Barium Chloride. I added 25ml of water it at first, then transferred it to a 50ml flask and filled it to 50ml and completely mixed the solution. Then I took 38ml of 0.0538 M Na3PO4 and mixed it with the 50ml BaCl2 solution into a 250ml beaker. After mixing those, I filtered it out and collected the solids. 

(The second image I attached has my calculations, I don't know if they're needed for these questions.)

12. Assuming your reaction occurred with a 100% yield of product being produced, name all of the substances that would be dissolved in the filtrate at the end of the reaction. Based on the amounts of reactants you added to the reaction vessel, calculate how many moles of those substances should be present? 13. A chemistry student offers a possible improvement to this lab. Since one goal of this lab is to determine the mass of the precipitate produced, wouldn't it be possible to measure the mass of an empty beaker, mix the solutions, and boil off the water until it is entirely evaporated, leaving only solid behind? Then the beaker with the precipitate could be weighed, and the difference between this mass and that of the empty beaker would be the mass of the precipitate. This would eliminate the need for the filtration step. Explain why this is a poor suggestion. Remember to check your reasoning on this question and all other questions with your instructor. 2 14. In your experiment, you very carefully made a solution of barium chloride, using a volumetric flask. The solution made for you of sodium phosphate was made similarly. Then you measured out a particular volume of each solution with graduated cylinders, carefully noting the volumes used. However, when you combined these volumes in a beaker, you were asked to rinse those graduated cylinders with water and pour that water into the same beaker where your reaction took place, without noting the volumes of water added. Why was it important to use specific volumes for some parts of the procedure but not important to note the volume of water added for others?
Transcribed Image Text:12. Assuming your reaction occurred with a 100% yield of product being produced, name all of the substances that would be dissolved in the filtrate at the end of the reaction. Based on the amounts of reactants you added to the reaction vessel, calculate how many moles of those substances should be present? 13. A chemistry student offers a possible improvement to this lab. Since one goal of this lab is to determine the mass of the precipitate produced, wouldn't it be possible to measure the mass of an empty beaker, mix the solutions, and boil off the water until it is entirely evaporated, leaving only solid behind? Then the beaker with the precipitate could be weighed, and the difference between this mass and that of the empty beaker would be the mass of the precipitate. This would eliminate the need for the filtration step. Explain why this is a poor suggestion. Remember to check your reasoning on this question and all other questions with your instructor. 2 14. In your experiment, you very carefully made a solution of barium chloride, using a volumetric flask. The solution made for you of sodium phosphate was made similarly. Then you measured out a particular volume of each solution with graduated cylinders, carefully noting the volumes used. However, when you combined these volumes in a beaker, you were asked to rinse those graduated cylinders with water and pour that water into the same beaker where your reaction took place, without noting the volumes of water added. Why was it important to use specific volumes for some parts of the procedure but not important to note the volume of water added for others?
2) a. Molar Mass w/H20= 244.25g/mol. W/H2O= 208.23g/mol b. ((0.780g Bacl2)/ (208.23g/mol*50ml))*1000ml/L=0.0749 M 3) 0.0749 mol/L * 0.050L= 0.00375 mol 4) 0.0538M * 38ml * 1L/1000ml= 0.0020 mol 5) N (required Bacl2*H2O)= 3/2*0.0020 mol= 0.0030 mol 6) N(Ba3(PO4)2)=0.0020mol/2= 0.0010 mol 7) To react completely with 0.0020 mol of Sodium Phosphate, we'll need 0.0030 mol. Therefore, Sodium Phosphate is the limiting reagent. 8) Theoretical Yield= 0.00375 mol/244.25g= 1.54 g 9) Filter paper with precipitate= 8.73g Weight of dry filter paper=7.31g Actual Yield= 8.73-7.31= 1.42g To find percent yield: (1.42/1.54)*100%= 0.92%
Transcribed Image Text:2) a. Molar Mass w/H20= 244.25g/mol. W/H2O= 208.23g/mol b. ((0.780g Bacl2)/ (208.23g/mol*50ml))*1000ml/L=0.0749 M 3) 0.0749 mol/L * 0.050L= 0.00375 mol 4) 0.0538M * 38ml * 1L/1000ml= 0.0020 mol 5) N (required Bacl2*H2O)= 3/2*0.0020 mol= 0.0030 mol 6) N(Ba3(PO4)2)=0.0020mol/2= 0.0010 mol 7) To react completely with 0.0020 mol of Sodium Phosphate, we'll need 0.0030 mol. Therefore, Sodium Phosphate is the limiting reagent. 8) Theoretical Yield= 0.00375 mol/244.25g= 1.54 g 9) Filter paper with precipitate= 8.73g Weight of dry filter paper=7.31g Actual Yield= 8.73-7.31= 1.42g To find percent yield: (1.42/1.54)*100%= 0.92%
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