Ib Chemistry Hygroscopic Bead Lab Report

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Design an experiment to investigate the stoichiometric mole ratio of a chemical reaction. Present your data in terms of the mass of one reactant compared to the mass of one product.

Purpose:
The experiment will be designed to find out the stoichiometric mole ratio of Barium Chloride and Silver Nitrate yielding a precipitate of Silver Chloride in a Barium Nitrate solution. (BaCl2 + 2AgNO3 -> Ba(NO3)2 + 2AgCl)

Research Question:
How will the amount of Barium Chloride and Silver Nitrate affect how much Silver Chloride is produced?

Hypothesis:
If there is one mole of BaCl2 in the reaction, then two moles of AgCl will be produced.

Variables:
Independent: Amount of the compound, BaCl2, in grams.
Dependent: Amount product produced, AgCl, in grams.

Materials:
* 4 -grams of Barium Chloride (BaCl2)
* 8 -grams of Silver Nitrate (AgNO3)
* Analytical Balance
* 2- Volumetric Flasks; one 50 mL flask, and one 100 mL flask * 2- Scoopulas
* 10- Weigh Boats
* 5- Filter paper
* 5- 250 mL beakers
* 2- 25 mL pipets
* Distilled water
* 2- 100 mL Erlenmeyer flasks
* 2- glass funnels

Procedure:
1. To the best of your ability, weigh out 3.75 grams of BaCl2 and 6.125 grams of AgNO3 on separate weigh boats 2. Pour the BaCl2 into the 50 mL volumetric flask from the weigh boat 3. Then add 14 mL of water to the flask to make the 0.5M solution of BaCl2 4. When pouring in the water, make sure the meniscus is right on the line 5. Next pour the AgNO3 into the 100 mL volumetric flask from the weigh boat 6. Then add the remaining 28 mL of water to make the 0.5M solution of AgNO3 7. Swirl the solutions to make sure the salts are fully dissipated, also making sure no liquid spills 8. Make sure to label a beaker to a specific mass, beaker #1 should be the .25 grams of Barium Chloride and so on 9. Use one pipet to pick up 25 mL of the Barium Chloride solution and the other to pick up 25 mL of Silver Nitrate solution 10. Release the proper amount of Barium Chloride into beaker #1 11. Do the same for beakers #2-5

12. Then release the proper amount of Silver Nitrate into each beaker like with the Barium Chloride 13. Add some water to make sure solutions mix better
14. Swirl each beaker just a bit to make sure all of the solutions have reacted 15. Weigh each filter paper and then fold filter paper into fours and put into funnel to capture the produced solid 16. Put the funnel into the top of an Erlenmeyer flask

17. Pour one beaker at a time through the top of the flask so that the filter paper catches the solid while any liquid goes through into the Erlenmeyer flask 18. Once all solid from one beaker is onto filter paper, weigh the filter paper with the solid and record the weight 19. Repeat steps 17 and 18 for each beaker

BaCl2 + 2AgNO3 -> Ba(NO3)2 + 2AgCl

.5g BaCl2 × 1 mol207g BaCl × 2 mol AgNO31 mol BaCl2 × 170g AgNO31 mol| 0.821g AgNO3| .5g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 143g AgCl1 mol| 0.691g AgCl| .5g BaCl2 × 1 mol207g BaCl × L.5 mol × 1000 mLL| 4.83mL BaCl2|

1g BaCl2 × 1 mol207g BaCl × 2 mol AgNO31 mol BaCl2 × 170g AgNO31 mol| 1.64g AgNO3| 1g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 143g AgCl1 mol| 1.38g AgCl| 1g BaCl2 × 1 mol207g BaCl × L.5 mol × 1000 mLL| 9.66mL BaCl2|

1.25g BaCl2 × 1 mol207g BaCl × 2 mol AgNO31 mol BaCl2 × 170g AgNO31 mol| 2.05g AgNO3| 1.25g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 143g AgCl1 mol| 1.73g AgCl| 1.25g BaCl2 × 1 mol207g BaCl × L.5 mol × 1000 mLL| 12.08mL BaCl2|

.25g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 170g AgNO31 mol| .411g AgNO3| .25g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 143g AgCl1 mol| .345g AgCl| .25g BaCl2 × 1 mol207g BaCl × L.5 mol × 1000 mLL| 2.42 mL BaCl2|

.75g BaCl2 × 1 mol207g BaCl × 2 mol AgCl1 mol BaCl2 × 170g AgNO31 mol| 1.23g AgNO3| .75g BaCl2 × 1 mol207g BaCl × 2...
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