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Write balanced equations describing each of the reactions in Steps1 through 5. A solution may contain any of the three group 1 cations. A white precipitateis formed upon the addition of HCI. This precipitate is partially soluble in hot waterand any residue dissolve upon the addition of NH,OH. Which group 1 ions are present? Which are absent? Which are in doubt? How would you remove all doubt?

Write balanced equations describing each of the reactions in Steps1 through 5. A solution may contain any of the three group 1 cations. A white precipitateis formed upon the addition of HCI. This precipitate is partially soluble in hot waterand any residue dissolve upon the addition of NH,OH. Which group 1 ions are present? Which are absent? Which are in doubt? How would you remove all doubt?

Chemistry
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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Could someone please give ideas on how to answer these 2 questions?

The questions are located on the first of the attached images. Thanks!

The Group 1 cations , Pb2+, Ag+, and Hg22+, form insoluble chlorides.

I think perhaps for q 1, what happens in each chemical individual equation when HCl is added to each cation

Flow Chart forthe Determination of GroupI Cations Ast, PB", Hg z +6 M Hcl I centrifuge HgClz Solid Agel, PbCI, 12, , HgCI, Liguid (Discard) Add HO, centrifuge white precipitete, Agel, PbCl < >Liquid, Pbt 1 6M Acetic acid, 1 M k, Croy 2. 16M NHyoH, contrifuge Tellow precipitate, Pb Cro y Black precipitate, HyE Liguid, Ag" 6 M HINO3 white precipitate, H9CI
Transcribed Image Text:Flow Chart forthe Determination of GroupI Cations Ast, PB", Hg z +6 M Hcl I centrifuge HgClz Solid Agel, PbCI, 12, , HgCI, Liguid (Discard) Add HO, centrifuge white precipitete, Agel, PbCl < >Liquid, Pbt 1 6M Acetic acid, 1 M k, Croy 2. 16M NHyoH, contrifuge Tellow precipitate, Pb Cro y Black precipitate, HyE Liguid, Ag" 6 M HINO3 white precipitate, H9CI
Please answerthe following two questions atthe end regarding reaction balanced equations and group 1 ions based on the 5-step procedure described below: Step 1: Preparation of a standard - In a test tube, add 2 drops of 6 M HCl to 1 ml of a standardsolution which contains Ag", Pb*, Hg.*. A precipitate of the respective chlorides will form. Centrifuge the solution and add 1 more drop of 6 M HCl to ensure complete precipitation. Centrifuge again, decant and discard the liquid and save the solid. Step 2: Separation and Identification of Pb*- Wash the precipitate with 2 ml of deionized water (DI water), stir, centrifuge, and discard the liquid. Add mlof DI waterto the testtube with the solidand immerse the testtubeina beaker half-filled with boiling water. Stirthe solution and continueheating for several minutes. Centrifuge while hot and decant the liquid into a second testtube. Save both the liquid and the solid. The liquid contains the Pb*cations since PbCl, is solublein hot water. Add one drop of 6 M aceticacid and a few drops of 1 M K¿Cro, to the liquid. A yellow precipitate of PbCro, will form, indicating the presence of Pb*inthe solution. Step 3: Separation and Identification of Hg.*- Add 10 drops of 6 M NH,OH to the precipitate and stir thoroughly. Centrifuge the mixture and pourthe liquid into a second test tube. The ammonia will forma soluble complex with silver but will reduce the mercurous ion tomercury metal. Therefore, the formation of a grey precipitate of mercury metal willestablish the presence of mercury. After centrifuging, save the liquidand discard the mercury into an appropriate container. Step 4: Identification of Ag*- Add 6 M HNO, to the liquid until a drop of solution will turn blue litmus paperred. At this acidiccondition, insoluble AgCl will again form and the presence of precipitate will indicate the presence of Ag". Step 5: Analysis of an unknown-Obtaina solution of unknown and repeat sections B through D in order to detemine which ions are present. Questions: 1. Write balanced equations describing each of the reactions in Steps 1 through 5. 2. A solution may contain any of the three group 1 cations. A white precipitateis formed upon the addition of HCI. This precipitate is partiallysoluble in hot waterandany residue dissolve upon the addition of NH,OH. Which group 1ions are present? Which are absent? Which are in doubt? How would youremove all doubt?
Transcribed Image Text:Please answerthe following two questions atthe end regarding reaction balanced equations and group 1 ions based on the 5-step procedure described below: Step 1: Preparation of a standard - In a test tube, add 2 drops of 6 M HCl to 1 ml of a standardsolution which contains Ag", Pb*, Hg.*. A precipitate of the respective chlorides will form. Centrifuge the solution and add 1 more drop of 6 M HCl to ensure complete precipitation. Centrifuge again, decant and discard the liquid and save the solid. Step 2: Separation and Identification of Pb*- Wash the precipitate with 2 ml of deionized water (DI water), stir, centrifuge, and discard the liquid. Add mlof DI waterto the testtube with the solidand immerse the testtubeina beaker half-filled with boiling water. Stirthe solution and continueheating for several minutes. Centrifuge while hot and decant the liquid into a second testtube. Save both the liquid and the solid. The liquid contains the Pb*cations since PbCl, is solublein hot water. Add one drop of 6 M aceticacid and a few drops of 1 M K¿Cro, to the liquid. A yellow precipitate of PbCro, will form, indicating the presence of Pb*inthe solution. Step 3: Separation and Identification of Hg.*- Add 10 drops of 6 M NH,OH to the precipitate and stir thoroughly. Centrifuge the mixture and pourthe liquid into a second test tube. The ammonia will forma soluble complex with silver but will reduce the mercurous ion tomercury metal. Therefore, the formation of a grey precipitate of mercury metal willestablish the presence of mercury. After centrifuging, save the liquidand discard the mercury into an appropriate container. Step 4: Identification of Ag*- Add 6 M HNO, to the liquid until a drop of solution will turn blue litmus paperred. At this acidiccondition, insoluble AgCl will again form and the presence of precipitate will indicate the presence of Ag". Step 5: Analysis of an unknown-Obtaina solution of unknown and repeat sections B through D in order to detemine which ions are present. Questions: 1. Write balanced equations describing each of the reactions in Steps 1 through 5. 2. A solution may contain any of the three group 1 cations. A white precipitateis formed upon the addition of HCI. This precipitate is partiallysoluble in hot waterandany residue dissolve upon the addition of NH,OH. Which group 1ions are present? Which are absent? Which are in doubt? How would youremove all doubt?
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