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Because a qualitative analysis may often consist of a rather long series of manipulations, precipitations, centrifugations, and separations, flow charts are often prepared to summarize graphically the steps to be undertaken. For this analysis of Group I, prepare a simple flow chart showing what ions are present at each point in the procedure, what reagents are to be added, and the result to be expected at each point.

Because a qualitative analysis may often consist of a rather long series of manipulations, precipitations, centrifugations, and separations, flow charts are often prepared to summarize graphically the steps to be undertaken. For this analysis of Group I, prepare a simple flow chart showing what ions are present at each point in the procedure, what reagents are to be added, and the result to be expected at each point.

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
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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 Cations** **Prelaboratory Questions** 1. **The separation of lead chloride from the chlorides of silver and mercury(I) is based on the differing solubilities of these substances in cold and hot water.** Use a handbook of chemical data to find the specific solubilities (in g/100 g H2O) in both cold and hot water for AgCl, PbCl2, and Hg2Cl2. | | Cold water | Hot water | Reference | |----------------------------|------------|-----------|-----------| | Silver chloride | | | | | Lead(II) chloride | | | | | Mercury(I) chloride | | | | --- 2. **Because a qualitative analysis may often consist of a rather long series of manipulations, precipitations, centrifugations, and separations, flow charts are often prepared to summarize graphically the steps to be undertaken.** For this analysis of Group I, prepare a simple *flow chart* showing what ions are present at each point in the procedure, what reagents are to be added, and the result to be expected at each point.
Transcribed Image Text:**Qualitative Analysis of the Group I Cations** **Prelaboratory Questions** 1. **The separation of lead chloride from the chlorides of silver and mercury(I) is based on the differing solubilities of these substances in cold and hot water.** Use a handbook of chemical data to find the specific solubilities (in g/100 g H2O) in both cold and hot water for AgCl, PbCl2, and Hg2Cl2. | | Cold water | Hot water | Reference | |----------------------------|------------|-----------|-----------| | Silver chloride | | | | | Lead(II) chloride | | | | | Mercury(I) chloride | | | | --- 2. **Because a qualitative analysis may often consist of a rather long series of manipulations, precipitations, centrifugations, and separations, flow charts are often prepared to summarize graphically the steps to be undertaken.** For this analysis of Group I, prepare a simple *flow chart* showing what ions are present at each point in the procedure, what reagents are to be added, and the result to be expected at each point.
**15. Qualitative Analysis of the Group I Cations** **Objective** A sample containing only the Group I cations will be analyzed for the presence of silver(I), mercury(I), and lead(II) ions. **Introduction** The Group I cations form chloride precipitates that are insoluble in acid. This group includes Ag⁺, Pb²⁺, and Hg₂²⁺ (mercurous ion). They are precipitated by adding 6 M hydrochloric acid, forming a mixture of AgCl, PbCl₂, and Hg₂Cl₂ solids: - Ag⁺(aq) + Cl⁻(aq) → AgCl(s) - Pb²⁺(aq) + 2Cl⁻(aq) → PbCl₂(s) - Hg₂²⁺(aq) + 2Cl⁻(aq) → Hg₂Cl₂(s) The sample is centrifuged, and the precipitate of the Group I chlorides is isolated. The supernatant is saved for further analysis of other group cations. Lead ion is separated from silver and mercury because PbCl₂ is more soluble in hot water than in cold. Hot distilled water dissolves PbCl₂. The mixture is centrifuged hot, and the supernatant containing lead ions is removed. The presence of lead is confirmed by adding chromate ion, CrO₄²⁻, forming lead chromate, PbCrO₄(s). The remaining silver/mercury precipitate is treated with aqueous ammonia. Silver ion forms Ag(NH₃)₂⁺, which dissolves; after centrifugation, only mercury remains as a black/gray residue, confirming mercury presence. The mixture containing complexed silver ion is treated with acid, re-precipitating silver chloride. Alternatively, potassium iodide can be added to precipitate silver iodide (creamy yellow-white solid). In practice, known and unknown samples will be analyzed, potentially containing mixtures from different analysis groups.
Transcribed Image Text:**15. Qualitative Analysis of the Group I Cations** **Objective** A sample containing only the Group I cations will be analyzed for the presence of silver(I), mercury(I), and lead(II) ions. **Introduction** The Group I cations form chloride precipitates that are insoluble in acid. This group includes Ag⁺, Pb²⁺, and Hg₂²⁺ (mercurous ion). They are precipitated by adding 6 M hydrochloric acid, forming a mixture of AgCl, PbCl₂, and Hg₂Cl₂ solids: - Ag⁺(aq) + Cl⁻(aq) → AgCl(s) - Pb²⁺(aq) + 2Cl⁻(aq) → PbCl₂(s) - Hg₂²⁺(aq) + 2Cl⁻(aq) → Hg₂Cl₂(s) The sample is centrifuged, and the precipitate of the Group I chlorides is isolated. The supernatant is saved for further analysis of other group cations. Lead ion is separated from silver and mercury because PbCl₂ is more soluble in hot water than in cold. Hot distilled water dissolves PbCl₂. The mixture is centrifuged hot, and the supernatant containing lead ions is removed. The presence of lead is confirmed by adding chromate ion, CrO₄²⁻, forming lead chromate, PbCrO₄(s). The remaining silver/mercury precipitate is treated with aqueous ammonia. Silver ion forms Ag(NH₃)₂⁺, which dissolves; after centrifugation, only mercury remains as a black/gray residue, confirming mercury presence. The mixture containing complexed silver ion is treated with acid, re-precipitating silver chloride. Alternatively, potassium iodide can be added to precipitate silver iodide (creamy yellow-white solid). In practice, known and unknown samples will be analyzed, potentially containing mixtures from different analysis groups.
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