Hello !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 Determinationof GroupI CationsAst, PB", Hg z+6 M HclI centrifugeHgClzSolid Agel, PbCI,12,, HgCI,Liguid (Discard)Add HO, centrifugewhite precipitete, Agel, PbCl Liquid, Pbt1 6M Acetic acid, 1 M k, Croy2.16M NHyoH, contrifugeTellow precipitate, Pb Cro yBlack precipitate, HyE Liguid, Ag"6 M HINO3white precipitate, H9CI Please answerthe following two questions atthe end regarding reaction balanced equations and group1 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 standardsolutionwhich contains Ag", Pb*, Hg.*. A precipitate of the respective chlorides will form. Centrifuge thesolution and add 1 more drop of 6 M HCl to ensure complete precipitation. Centrifuge again, decant anddiscard the liquid and save the solid.Step 2: Separation and Identification of Pb*- Wash the precipitate with 2 ml of deionized water (DIwater), stir, centrifuge, and discard the liquid. Add mlof DI waterto the testtube with the solidandimmerse the testtubeina beaker half-filled with boiling water. Stirthe solution and continueheatingfor several minutes. Centrifuge while hot and decant the liquid into a second testtube. Save both theliquid and the solid. The liquid contains the Pb*cations since PbCl, is solublein hot water. Add one dropof 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 stirthoroughly. Centrifuge the mixture and pourthe liquid into a second test tube. The ammonia will formasoluble complex with silver but will reduce the mercurous ion tomercury metal. Therefore, theformation of a grey precipitate of mercury metal willestablish the presence of mercury. Aftercentrifuging, 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 litmuspaperred. At this acidiccondition, insoluble AgCl will again form and the presence of precipitate willindicate the presence of Ag".Step 5: Analysis of an unknown-Obtaina solution of unknown and repeat sections B through D in orderto 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 theaddition of HCI. This precipitate is partiallysoluble in hot waterandany residue dissolve uponthe addition of NH,OH. Which group 1ions are present? Which are absent? Which are in doubt?How would youremove all doubt?

Question

Hello !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 Determinationof GroupI CationsAst, PB&#34;, Hg z+6 M HclI centrifugeHgClzSolid Agel, PbCI,12,, HgCI,Liguid (Discard)Add HO, centrifugewhite precipitete, Agel, PbCl <>Liquid, Pbt1 6M Acetic acid, 1 M k, Croy2.16M NHyoH, contrifugeTellow precipitate, Pb Cro yBlack precipitate, HyE Liguid, Ag&#34;6 M HINO3white precipitate, H9CI Please answerthe following two questions atthe end regarding reaction balanced equations and group1 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 standardsolutionwhich contains Ag&#34;, Pb*, Hg.*. A precipitate of the respective chlorides will form. Centrifuge thesolution and add 1 more drop of 6 M HCl to ensure complete precipitation. Centrifuge again, decant anddiscard the liquid and save the solid.Step 2: Separation and Identification of Pb*- Wash the precipitate with 2 ml of deionized water (DIwater), stir, centrifuge, and discard the liquid. Add mlof DI waterto the testtube with the solidandimmerse the testtubeina beaker half-filled with boiling water. Stirthe solution and continueheatingfor several minutes. Centrifuge while hot and decant the liquid into a second testtube. Save both theliquid and the solid. The liquid contains the Pb*cations since PbCl, is solublein hot water. Add one dropof 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 stirthoroughly. Centrifuge the mixture and pourthe liquid into a second test tube. The ammonia will formasoluble complex with silver but will reduce the mercurous ion tomercury metal. Therefore, theformation of a grey precipitate of mercury metal willestablish the presence of mercury. Aftercentrifuging, 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 litmuspaperred. At this acidiccondition, insoluble AgCl will again form and the presence of precipitate willindicate the presence of Ag&#34;.Step 5: Analysis of an unknown-Obtaina solution of unknown and repeat sections B through D in orderto 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 theaddition of HCI. This precipitate is partiallysoluble in hot waterandany residue dissolve uponthe addition of NH,OH. Which group 1ions are present? Which are absent? Which are in doubt?How would youremove all doubt?

Accepted Answer

Cationic analysis refers to analysis of a salt or a mixture for cations present in them. Group I of…