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Compute the mole of CO2(g) evolved in Part II, Tube #1 through # 5 assuming that this gas could be collected at 23°C and 755 mm Hg. Tube 1

Compute the mole of CO2(g) evolved in Part II, Tube #1 through # 5 assuming that this gas could be collected at 23°C and 755 mm Hg. Tube 1

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter7: Statistical Data Treatment And Evaluation
Section: Chapter Questions
Problem 7.22QAP
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Post Laboratory Questions 1. Include the calculations made prior to making up the potassium iodide and calcium chloride solutions used in this experiment. a. Potassium iodide b. Calcium chloride 2. Write the net ionic equation that occurs in Part I. 3. Write the net ionic equation that occurs in Part II. 4. Compute the mole of CO2(g) evolved in Part II, Tube #1 through # 5 assuming that this gas could be collected at 23°C and 755 mm Hg. Tube 1 Tube 2 Tube 3 Tube 4 Tube 5
Transcribed Image Text:Post Laboratory Questions 1. Include the calculations made prior to making up the potassium iodide and calcium chloride solutions used in this experiment. a. Potassium iodide b. Calcium chloride 2. Write the net ionic equation that occurs in Part I. 3. Write the net ionic equation that occurs in Part II. 4. Compute the mole of CO2(g) evolved in Part II, Tube #1 through # 5 assuming that this gas could be collected at 23°C and 755 mm Hg. Tube 1 Tube 2 Tube 3 Tube 4 Tube 5
Flasks, 100.0 mL kers ansfer pipets ar pipets n of KI with Pb(NO3)2 irs. structor has approved your plan (pre- prepare 100.0 ml of the 0.100 M KI ording to the plan. When weighing ical, be sure to use the scoopula emove the chemical from the reagent ot use your scoopula. Any excess uld be discarded: do NOT return to Ottle. 20 ml of 0.100 M Pb(NO3)2 in a 30 eplenish the solution as needed. ut 20 mL of your Kl solution into beaker. n test tubes and label them 1 ange them in the test tube rack. solution and KI solution according table using Mohr pipets. Pb(NO3)2 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL KI 5.00 mL 4.00 mL 3.00 mL 2.00 mL 1.00 mL not to contaminate your pipet. If aminated with precipitate, rinse it from clogging. be with a piece of Parafilm, and hold it straight. After 5 e the height of precipitate reach mixture. precipitate vs. the amount of (0,0) and (6,0) indicating that s when only one solution is mount of precipitate should more Pb(NO3)2 solution to a decrease when excess added. Draw a straight line um portion of the data and -42- 9. Discard the solution into the waste container in the hood. Make sure to wash out all the precipitate into the container as well. Part II: Reaction with Cat2 and CO² 1. 2. solution that would produce the most precipitate from the intersection of the two lines in Step 7. 3. Work in pairs. After your instructor has approved your plan, make 100.0 mL of a solution that is 0.100 M in Ca²+ ion. Rinse the pipets and beakers from Part I two or three times with water, then with the solution that you plan to pipet in Part II. 4. Obtain 5 clean test tubes and arrange them on the test tube rack as you did in Part I. 5. Obtain about 20 mL of 0.10 M sodium carbonate solution in 30 mL beaker and about 20 mL of your solution in another beaker. Replenish them as needed. 6. Add Cat2 solution and CO32 solution according to the following table using Mohr pipets. Tube # Ca+2 1 2 3 4 5 CO3-² 5.00 mL 4.00 mL 3.00 mL 2.00 mL 1.00 mL 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL 7. Centrifuge all test tubes and discard supernatant solution. Make sure to balance the centrifuge with the 6th test tube filled with equivalent amount of water. 8. Add 0.10 M HCI solution drop-by-drop to the precipitate mixing after each drop is added. Record the number of drops needed to completely dissolve the precipitate. 9. Plot the number of drops of 0.10 M HCI needed vs. the amount of Cat2 solution. Include (0,0) and (6,0) indicating that no precipitate forms when only one solution is present. Similar to the Part I step 7, draw two straight lines. 10. Predict the ratio of Ca*2 to CO32 that would produce the maximum amount of precipitate. 11. The excess CaCl2 solution and the solution left in your centrifuge tube may be flushed down the sink with running water.
Transcribed Image Text:Flasks, 100.0 mL kers ansfer pipets ar pipets n of KI with Pb(NO3)2 irs. structor has approved your plan (pre- prepare 100.0 ml of the 0.100 M KI ording to the plan. When weighing ical, be sure to use the scoopula emove the chemical from the reagent ot use your scoopula. Any excess uld be discarded: do NOT return to Ottle. 20 ml of 0.100 M Pb(NO3)2 in a 30 eplenish the solution as needed. ut 20 mL of your Kl solution into beaker. n test tubes and label them 1 ange them in the test tube rack. solution and KI solution according table using Mohr pipets. Pb(NO3)2 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL KI 5.00 mL 4.00 mL 3.00 mL 2.00 mL 1.00 mL not to contaminate your pipet. If aminated with precipitate, rinse it from clogging. be with a piece of Parafilm, and hold it straight. After 5 e the height of precipitate reach mixture. precipitate vs. the amount of (0,0) and (6,0) indicating that s when only one solution is mount of precipitate should more Pb(NO3)2 solution to a decrease when excess added. Draw a straight line um portion of the data and -42- 9. Discard the solution into the waste container in the hood. Make sure to wash out all the precipitate into the container as well. Part II: Reaction with Cat2 and CO² 1. 2. solution that would produce the most precipitate from the intersection of the two lines in Step 7. 3. Work in pairs. After your instructor has approved your plan, make 100.0 mL of a solution that is 0.100 M in Ca²+ ion. Rinse the pipets and beakers from Part I two or three times with water, then with the solution that you plan to pipet in Part II. 4. Obtain 5 clean test tubes and arrange them on the test tube rack as you did in Part I. 5. Obtain about 20 mL of 0.10 M sodium carbonate solution in 30 mL beaker and about 20 mL of your solution in another beaker. Replenish them as needed. 6. Add Cat2 solution and CO32 solution according to the following table using Mohr pipets. Tube # Ca+2 1 2 3 4 5 CO3-² 5.00 mL 4.00 mL 3.00 mL 2.00 mL 1.00 mL 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL 7. Centrifuge all test tubes and discard supernatant solution. Make sure to balance the centrifuge with the 6th test tube filled with equivalent amount of water. 8. Add 0.10 M HCI solution drop-by-drop to the precipitate mixing after each drop is added. Record the number of drops needed to completely dissolve the precipitate. 9. Plot the number of drops of 0.10 M HCI needed vs. the amount of Cat2 solution. Include (0,0) and (6,0) indicating that no precipitate forms when only one solution is present. Similar to the Part I step 7, draw two straight lines. 10. Predict the ratio of Ca*2 to CO32 that would produce the maximum amount of precipitate. 11. The excess CaCl2 solution and the solution left in your centrifuge tube may be flushed down the sink with running water.
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