I need help with one of my pre-lab questions which I want to understand. Its question number 2, the one that highlighted. I don't want to make it over-complicated, I want something that I can understand. Qualitative Analysis of the Group I CationsStudent name:Team members:Date:Course:Section:Instructor:Prelaboratory Questions1. The separation of lead chloride from the chlorides of silver andmercury(I) is based on the differing solubilities of these substances incold and hot water. Use a handbook of chemical data to find the specificsolubilities (in g/100 g H₂O) in both cold and hot water for AgCl, PbCl₂and HgCl₂.Cold waterReferenceHot waterSilver chlorideLead(II) chlorideMercury(1) chloride2. Because a qualitative analysis may often consist of a rather long seriesof manipulations, precipitations, centrifugations, and separations, flowcharts are often prepared to summarize graphically the steps to beundertaken. For this analysis of Group I, prepare a simple flow chartshowing what ions are present at each point in the procedure, whatreagents are to be added, and the result to be expected at each point. 15. Qualitative Analysis of the Group I CationsObjectiveA sample containing only the Group I cations will be analyzed for the presenceof silver(1), mercury(I), and lead(II) ions.IntroductionThe Group I cations are those species that form chloride precipitates that areinsoluble in acid. The group includes Ag', Pb, and Hg₂+ (mercurous ion).These cations are precipitated from any other cations that might be present ina sample by addition of 6 M hydrochloric acid. Addition of HCl forms a mix-ture of AgCl, PbCl₂, and Hg₂Cl₂ solids.Ag (aq) + Cl (aq) → AgCl(s)Pb²(aq) + 2Cl(aq) →→→ PbCl₂(s)Hg³(aq) + 2Cl (aq) → Hg, Cl₂(s)At this point, the sample is centrifuged and the precipitate of the Group I chlo-rides isolated (in a real analysis, the centrifugate from above the precipitate issaved for further analysis of the other group cations).Lead ion is then separated from silver and mercury by taking advantage of thefact that PbCl, is much more soluble in hot water than in cold water (thesolubilities of AgCl and Hg, Cl, do not vary much with temperature). Distilledwater is added to the Group I mixed precipitate and the mixture is heated todissolve PbCl₂,. The mixture is then centrifuged quickly while still hot, and thecentrifugate containing lead ion is removed from the remaining silver/mercuryprecipitate. The presence of lead ion is then confirmed by addition of chromateion, CrO², which forms a characteristic yellow precipitate with lead ion,PbCrO₁.The precipitate containing silver and mercurous ions is then treated withaqueous ammonia. Silver ion is complexed by ammonia; the precipitate of AgClwill dissolve and is removed after centrifugation. A black/gray residue in thecentrifuge tube confirms the presence of mercury.The centrifugate containing complexed silver ion is then treated with acid,which reacts with ammonia allowing the reprecipitation of silver chloride.Alternatively, potassium iodide can be added, which also precipitates the silver(as a creamy yellow-white solid).In this experiment (and those on the qualitative analysis of Groups II-V)a known sample for only the particular group under study, as well as anunknown sample (containing one or more cations from the specific group) willbe analyzed. In real practice, a sample would not be restricted to the membersof only one analysis group, but rather would be a general mixture of allpossible cations.

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To draw a properly labelled flow chart for the qualitative analysis of Group I cations.