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?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.)

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?

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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